Term
| the one distinguishing characteristic of all organic compounds |
|
Definition
| they all contain the element carbon |
|
|
Term
|
Definition
| the study of carbon compounds |
|
|
Term
| Why is C special? Why do most presently known chemical compounds contain C? |
|
Definition
| because of its structure and its consequent position on the periodic table |
|
|
Term
| why C is able to form so many compounds |
|
Definition
because of its ability to bond
-can share 4 ve's and form 4 strong covalent bonds
-C atoms can bond to each other, forming long chains and rings |
|
|
Term
| some elements commonly found in organic compounds |
|
Definition
|
|
Term
| the color used to represent H |
|
Definition
|
|
Term
| the color used to represent C |
|
Definition
|
|
Term
| the color used to represent N |
|
Definition
|
|
Term
| the color used to represent O |
|
Definition
|
|
Term
| the color used to represent F |
|
Definition
| some kind of pale turquoise color |
|
|
Term
| the color used to represent P |
|
Definition
|
|
Term
| the color used to represent S |
|
Definition
|
|
Term
| the color used to represent Cl |
|
Definition
|
|
Term
| the color used to represent Br |
|
Definition
|
|
Term
| the color used to represent I |
|
Definition
|
|
Term
| the general composition of an atom |
|
Definition
-small, dense nucleus with protons and neutrons
-electrons circling it at a relatively large distance |
|
|
Term
| the electron density in an atom |
|
Definition
| denser closer to the nucleus than towards the outer edge |
|
|
Term
|
Definition
| atoms with the same atomic number but different mass numbers |
|
|
Term
| the behavior of a specific electron in an atom can be described by... |
|
Definition
|
|
Term
| the solution to a wave equation |
|
Definition
|
|
Term
|
Definition
| the solution to a wave equation |
|
|
Term
|
Definition
this is the Greek letter psi
this denotes the orbital, which is the solution to a wave function |
|
|
Term
| how an orbital describes the volume of space around a nucleus that an electron is most likely to occupy |
|
Definition
| by plotting the square of the wave function, Ψ2, in 3D space |
|
|
Term
|
Definition
|
|
Term
| the orbitals we're primarily concerned with in OCHEM and biochem |
|
Definition
| s and p because they're the most common |
|
|
Term
| the shape of an s orbital |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
4 of the 5 are shaped like a 4-leaf clover
the other one is shaped like a dumbbell inside a donut |
|
|
Term
| the atoms in an orbital are organized into... |
|
Definition
| different electron shells |
|
|
Term
|
Definition
| a group of an atom's electrons with the same principal quantumn number |
|
|
Term
| each orbital in a shell can be occupied by how many electrons? |
|
Definition
|
|
Term
| composition of the first energy level in an atom |
|
Definition
| a 1s orbital, thus just 2 electrons |
|
|
Term
| composition of the second energy level in an atom |
|
Definition
| a 2s orbital and 3 2p orbitals, thus 8 electrons |
|
|
Term
| composition of the third energy level in an atom |
|
Definition
| a 3s orbital, 3 3p orbitals, and 5 3d orbitals, thus 18 electrons |
|
|
Term
|
Definition
|
|
Term
| how the p orbitals are arranged |
|
Definition
| along mutually perpendiculat directions,
denoted px, py, and pz
[image] |
|
|
Term
| the lobes of an orbital are separated by... |
|
Definition
| an area of zero electron density called a node |
|
|
Term
|
Definition
| an area of zero electron density between the nodes of an orbital |
|
|
Term
| how the lobes of the orbital are denoted in the wave function |
|
Definition
| with the algebraic signs + and - |
|
|
Term
| ground-state electron configuration |
|
Definition
| the orbitals occupied by an atom's electrons at its lowest energy arrangement (its ground state) |
|
|
Term
| the 3 rules for listing the orbitals occupied by an atom's electrons (WRITE THIS DOWN!) |
|
Definition
1: Aufbau principle; the lowest energy orbitals fill up first, according to the order 1s --> 2s --> 2p --> 3s --> 3p --> 4s --> 4d. Note that the 4s orbital lies between the 3p and 3d orbitals.
2: Pauli exclusion principle; electrons act in some ways as if they were spinning around an axis, somewhat like how the Earth spins. This spin can have different orientations, denoted as up (/|\) and down (\|/). Only 2 electrons can occupy an orbital, and they must be of opposite spin.
3: Hund's rule; if 2 or more orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half full. |
|
|
Term
|
Definition
| The lowest energy orbitals fill up first, according to the order 1s --> 2s --> 2p --> 3s --> 3p --> 4s --> 4d |
|
|
Term
| Pauli exclusion principle |
|
Definition
| Only 2 electrons can occupy an orbital, and they must be of opposite spin |
|
|
Term
|
Definition
| If 2 or more orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half full |
|
|
Term
| the orbitals that fill up first |
|
Definition
| the lowest energy orbitals |
|
|
Term
| how many electrons can occupy an orbital? |
|
Definition
|
|
Term
| how must the electrons in an orbital spin? |
|
Definition
| they must be of opposite spin |
|
|
Term
| what electrons do when 2 or more orbitals of equal energy are available |
|
Definition
| one electron occupies each with spins parallel until all orbitals are half full |
|
|
Term
| how to predict ground state electron configuration: |
|
Definition
|
|
Term
| the valency of carbon in organic compounds |
|
Definition
| tetravalent; always forms 4 bonds when it joins other elements to form stable compounds |
|
|
Term
|
Definition
| always forms 4 bonds when it joins other elements to form stable compounds |
|
|
Term
| the spatial orientation of a carbon atom's bonds |
|
Definition
| a regular tetrahedron (basically a trigonal pyramid) |
|
|
Term
| how bonds coming out of the page toward the viewer |
|
Definition
[image]
heavy, wedge-shaped line |
|
|
Term
| how bonds on the same plane as the page are represented |
|
Definition
|
|
Term
| how bonds receding back behind the page away from the viewer are represented |
|
Definition
|
|
Term
| why do atoms bond together? |
|
Definition
| because the the compound that results is more stable and lower in energy than the separate atoms |
|
|
Term
| flow of energy when a bond is formed |
|
Definition
| energy, usually as heat, always flows out of a chemical system when a bond is formed |
|
|
Term
| flow of energy when a bond is broken |
|
Definition
| energy must be put into a chemical system to break a bond |
|
|
Term
| why do atoms want an octet? |
|
Definition
| to obtain noble gas configuration |
|
|
Term
|
Definition
| electrostatic attraction between an anion and a cation |
|
|
Term
|
Definition
| sharing of electrons between atoms |
|
|
Term
|
Definition
| neutral collection of atoms held together by covalent bonds |
|
|
Term
|
Definition
|
|
Term
| a stable molecule results when... |
|
Definition
| a noble gas configuration is achieved for all the atoms |
|
|
Term
| Kekulé structures aka line-dot structures |
|
Definition
| kinda like Lewis structures, but the bonds are represented with lines instead of electron pairs |
|
|
Term
|
Definition
valence electrons that are not used for bonding
aka nonbonding erlectrons |
|
|
Term
| 2 models that have been developed to describe covalent bonding |
|
Definition
-valence bond theory
-molecular orbital theory |
|
|
Term
|
Definition
| According to this theory, a covalent bond forms when 2 atoms approach each other closely and a singly occupied orbital on one atom overlaps a singly occupied orbital on the other atom. The electrons are now paired in the overlapping orbitals and are attracted to the nuclei of both atoms, thus bonding the atoms together. |
|
|
Term
|
Definition
covalent bond formed by head on overlap of atomic orbitals
this is basically what happens in a single bond |
|
|
Term
| why molecules are more stable than the free atoms |
|
Definition
| because the product molecule has less energy than the starting free atoms |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| the distance between 2 nuclei that leads to maximum stability; this is at the minimum energy point between the 2 nuclei |
|
|
Term
|
Definition
| see if you can find it in the video |
|
|
Term
|
Definition
| hybrid of an s orbital and three p orbitals |
|
|
Term
| depiction of unhybridized s and p orbitals |
|
Definition
|
|
Term
| depiction of sp3 hybrid orbitals |
|
Definition
|
|
Term
| why there's directionality in a tetrahedral molecule |
|
Definition
| because the sp3 hybrid orbitals have 2 lobes and are unsymmetrical about the nucleus, giving them directionality and allowing them to form strong covalent bonds when they overlap with orbitals from other atoms |
|
|
Term
| why sp3 hybrid orbitals form stronger bonds than unhybridized s and p orbitals |
|
Definition
| because one of the 2 lobes is larger and can therefore overlap more effectively with an orbital from another atom to form a bond |
|
|
Term
| why sp3 hybrid orbitals are asymmetrical |
|
Definition
| because the 2 lobes of the p orbital have different algebraic signs (+ and -). Thus, when a p orbital hybridizes with an s orbital, the positive p lobe adds to the s orbital but the negative p lobe subtracts from the s orbital, making the orbital strongly oriented in one direction |
|
|
Term
| the bond length between C and H |
|
Definition
|
|
Term
| the bond angle in a tetrahedral molecule |
|
Definition
|
|
Term
| chemical formula for methane |
|
Definition
|
|
Term
| chemical formula for ethane |
|
Definition
|
|
Term
| the simplest molecule with a C-C bond |
|
Definition
|
|
Term
| the overlap between the C atoms in an ethane molecule |
|
Definition
|
|
Term
| the hybrid orbital that comes from each C atom in an ethane molecule |
|
Definition
|
|
Term
| length of the C-C single bond |
|
Definition
|
|
Term
| the bond angles when an atom has 4 electron domains |
|
Definition
|
|
Term
|
Definition
| this occurs when an s orbital hybridizes with the px and py orbitals, but not the pz orbital; it remains unchanged |
|
|
Term
| the orientation of sp2 hybrid orbitals |
|
Definition
| trigonal planar with the 3 lobes 120° apart from each other and the unchanged p orbital perpendicular to the sp2 plane |
|
|
Term
|
Definition
| covalent bond between 2 p orbitals |
|
|
Term
| the regions occupied by the sigma (σ) bond |
|
Definition
| the region centered between nuclei |
|
|
Term
| the regions occupied by the sigma (π) bond |
|
Definition
| the regions above and below a line drawn between the nuclei |
|
|
Term
| length of the C-H single bond |
|
Definition
|
|
Term
| length of the C=C double bond |
|
Definition
|
|
Term
| why a double bond is less than twice as strong as a single bond |
|
Definition
| because the sideways overlap in the pi (π) part is not as much as the head on overlap in thew (σ) sigma part |
|
|
Term
|
Definition
| this happens when an s orbital hybridizes with the px orbital, but not the py and pz orbitals; they remain unchanged |
|
|
Term
|
Definition
| sp-sp bond between the sp orbitals and py-py pi bond between the py orbitals and pz-pz pi bond between the pz orbitals |
|
|
Term
| length of then C-C triple bond |
|
Definition
|
|
Term
|
Definition
| often 109 pm, but sometimes 106 pm |
|
|
Term
| electron domain alignment associated with sp hybrid orbitals |
|
Definition
|
|
Term
| electron domain alignment associated with sp2 hybrid orbitals |
|
Definition
|
|
Term
| electron domain alignment associated with sp3 hybrid orbitals |
|
Definition
|
|
Term
| bond angle associated with sp hybrid orbitals |
|
Definition
|
|
Term
| bond angle associated with sp2 hybrid orbitals |
|
Definition
|
|
Term
| bond angle associated with sp3 hybrid orbitals |
|
Definition
|
|
Term
| why P can form 5 covalent bonds |
|
Definition
| due to its position on the Periodic Table, it can expand its outer shell octet and form more than the typical number of covalent bonds |
|
|
Term
| why S can form 4 covalent bonds |
|
Definition
| due to its position on the Periodic Table, it can expand its outer shell octet and form more than the typical number of covalent bonds |
|
|
Term
|
Definition
| com[pounds that contain a P atom bonded to 4 O, with one of the O bonded to a C |
|
|
Term
|
Definition
| compound with a S atom bonded to one H and one C |
|
|
Term
|
Definition
| compound that has a S atom bonded to 2 C |
|
|
Term
| molecular orbital (MO) theory |
|
Definition
| describes covalent bond formation as arising from a mathematical combination of atomic orbitals (wave functions) on different atoms to form molecular orbitals, so called because they belong to the entire molecule rather than to an individual atom |
|
|
Term
| the 2 ways for a molecular orbital to occur |
|
Definition
-the additive way
-the subtractive way |
|
|
Term
| the additive way for molecular orbitals to occur |
|
Definition
| this combination leads to a molecular orbital that is lower in energy and is roughly egg-shaped |
|
|
Term
| the subtractive way for molecular orbitals to occur |
|
Definition
| this combo leads to a molecular orbital that's higher in energy and has a node between nuclei |
|
|
Term
| bonding molecular orbital (MO) |
|
Definition
| molecular orbital that's lower in energy than the atomic orbitals from which it is formed |
|
|
Term
| antibonding molecular orbital (MO) |
|
Definition
molecular orbital that's higher in energy than the atomic orbitals from which it is formed
can't contribute to bonding because the electrons it contains can't occupy the central region |
|
|
Term
|
Definition
| shorthand method for writing structures in which C-H and C-C single bonds aren't shown, but instead understood
example: propane being written as CH3CH2CH3 |
|
|
Term
|
Definition
| shorthand way of writing structures in which C atoms are assumed to be at each intersection of 2 lines (bonds) and at the end of each line |
|
|
Term
| rules for drawing skeletal structures (WRITE THIS DOWN!) |
|
Definition
1: C atoms aren't usually shown. Instead, a C atom is assumed to be at each intersection of 2 lines (bonds) and at the end of each line. Occasionally, a C atom might be indicated for emphasis or clarity.
2: H atoms bonded to C aren't shown. Because C always has a valence of 4, we mentally supply the correct number of H atoms for each C.
3: Atoms other than C and H are shown. |
|
|
Term
| what the end of the line in a skeletal structure represents |
|
Definition
|
|
Term
| what a 2-way intersection in a skeletal structure represents |
|
Definition
|
|
Term
| what a 3-way intersection in a skeletal structure represents |
|
Definition
|
|
Term
| what a 4-way intersection in a skeletal structure represents |
|
Definition
|
|
Term
| bonds that have a circular cross-section and are formed by head-on interaction |
|
Definition
|
|
Term
| bonds formed by sideways interaction of p orbitals |
|
Definition
|
|
Term
| shape of a hexagonal benzene molecule |
|
Definition
|
|
Term
| hybridization of C+ ion when it forms 3 single bonds |
|
Definition
|
|
Term
| geometry of C+ ion when it forms 3 single bonds |
|
Definition
|
|
Term
| electronic relationship refers to... |
|
Definition
|
|
Term
| singlet (spin-paired) orbital |
|
Definition
| has pair of electrons, opposite spin |
|
|
Term
| triplet (spin-unpaired) orbital |
|
Definition
|
|
Term
| how the chemical symbols in an organic compound's molecular formula are ordered |
|
Definition
| first C, then H, then alphabetical from there |
|
|
Term
| why the 4 bonds of C can be arranged in a variety of ways |
|
Definition
| because of differences in hybridization |
|
|
Term
| bond angle of tetrahedral bonds |
|
Definition
|
|
Term
| hybridization of tetrahedral |
|
Definition
|
|
Term
| hybridization of trigonal planar |
|
Definition
|
|
Term
| bond angle of trigonal planar |
|
Definition
|
|
Term
| where the p orbital is in trigonal planar |
|
Definition
| perpendicular to the sp2 orbitals on the trigonal planar |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| some other elements that are often found in organic compounds |
|
Definition
|
|
Term
|
Definition
| small collection of atoms that gives a molecule specific properties |
|
|
Term
| volume of an atom has to do with... |
|
Definition
|
|
Term
| the most common C isotope |
|
Definition
C-12
99% of the C in mature |
|
|
Term
| distance between energy layers vs. distance from nucleus |
|
Definition
| the further you get from the nucleus, the closer and closer those energy layers get |
|
|
Term
| s orbitals always cone ______ at a time |
|
Definition
|
|
Term
| p orbitals always cone ______ at a time |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| point of zero electron density between the nodes of an orbital |
|
|
Term
| the difference between the p orbitals |
|
Definition
| the orientation; they're the same except for the axis |
|
|
Term
|
Definition
| exactly the same in energy |
|
|
Term
| d orbitals always cone ______ at a time |
|
Definition
|
|
Term
| f orbitals always cone ______ at a time |
|
Definition
|
|
Term
| why the 1st energy level can have only 2 electrons |
|
Definition
| because it has only 1 s orbital |
|
|
Term
| stability of orbital vs. distance from nucleus |
|
Definition
| the further from the nucleus, the less stable the orbital |
|
|
Term
| where the node is in a p orbital |
|
Definition
|
|
Term
| the most common elements we will deal with in OCHEM |
|
Definition
|
|
Term
|
Definition
| an atom's affinity for electrons |
|
|
Term
| general trend for electronegativity |
|
Definition
|
|
Term
| what causes polarity in bonds? |
|
Definition
|
|
Term
| some elements that have the same electronegativities as C |
|
Definition
|
|
Term
| why the C-O bond is more polar than the C-Cl bond |
|
Definition
| because O is 2 elements to the right of C and Cl is just 1 element to the right of S |
|
|
Term
| # of nodes vs. energy of orbital |
|
Definition
| the more nodes, the higher the energy |
|
|
Term
| the difference between a 1st energy orbital (such as 1s) and a 2nd energy orbital (such as 2s) |
|
Definition
|
|
Term
| the type of node in an s orbital |
|
Definition
|
|
Term
| why the valence electrons are so special |
|
Definition
| because the define the chemistry and size of the element |
|
|
Term
| trend in size of atoms as you go down the columns of the PTable |
|
Definition
| size increases, but by increasingly smaller increments |
|
|
Term
| trend in size of atom as you go right along the rows of the PTable |
|
Definition
| size of the atom decreases |
|
|
Term
| electronegativity vs. size of atom in the same row |
|
Definition
|
|
Term
| the 2 main types of bonds |
|
Definition
|
|
Term
|
Definition
| bond created by attraction of electric charge |
|
|
Term
| the elements that typically yield anions |
|
Definition
|
|
Term
| the elements that tend to form anions are the ones that are more... |
|
Definition
|
|
Term
|
Definition
| sharing of electron density between 2 separate nuclei |
|
|
Term
|
Definition
| covalent bonds with unequal sharing of electrons |
|
|
Term
| is bond formation endothermic or exothermic? |
|
Definition
|
|
Term
| which is more stable? molecule or individual atoms? |
|
Definition
|
|
Term
| is bond breaking endothermic or exothermic? |
|
Definition
|
|
Term
|
Definition
| the energy input needed to break bonds apart |
|
|
Term
|
Definition
[image]
the bond length is nominal bond length |
|
|
Term
|
Definition
|
|
Term
| what happens to the energy of the bond as the nuclei get further apart? |
|
Definition
|
|
Term
| how wavelength is related to energy |
|
Definition
ΔE = hv
ΔE = change in energy
h = Planck's constant
v = wavelength (nm) |
|
|
Term
|
Definition
|
|
Term
| bond length vs. bond strength |
|
Definition
|
|
Term
|
Definition
| 1 / 1 billionth
1 x 10-9 meter |
|
|
Term
|
Definition
| 1 / trillionth
1 x 10-12 meter |
|
|
Term
| frequency of vibration of bonds vs. length of bond |
|
Definition
|
|
Term
| why the length and strength of bonds between atoms is important for chemistry |
|
Definition
| because it helps predict reactivity |
|
|
Term
| length of bond between atoms vs. reactivity |
|
Definition
|
|
Term
| how size of atom affects reactivity |
|
Definition
| affects internuclear distance, thus affecting bond length and frequency |
|
|
Term
| is the covalent bond between 2 atoms static? |
|
Definition
|
|
Term
| how a covalent bond between 2 atoms vibrates |
|
Definition
| at a specific frequency characteristic to that bond |
|
|
Term
| depiction of where this equation, ΔE = hv, fits into internuclear bonds |
|
Definition
|
|
Term
| Heisenberg's uncertainty principle |
|
Definition
| you can know either the location or energy of the electron, but not both |
|
|
Term
| the amount of time an electron spends in its specific orbital |
|
Definition
|
|
Term
|
Definition
|
|
Term
| depiction of how to draw a p ordital |
|
Definition
[image]
one lobe is shaded to indicate that one of the numbers is positive
the horizontal line is a plane where the node is |
|
|
Term
| the 2 key types of orbitals you gotta pick up on in molecular orbital theory |
|
Definition
|
|
Term
|
Definition
| as you increase the energy, you increase the # of nodes |
|
|
Term
| depiction of how s orbitals interact in covalent bonding |
|
Definition
[image]
the one on top shows antibonding orbitals as a result of destructive interference at high energy and the one on bottom shows bonding molecular orbitals as a result of constructive interference at low energy
the arrows at the bottom represent the opposite spins of paired electrons |
|
|
Term
| what a theory is used for |
|
Definition
| it's used to make predictions |
|
|
Term
| example of how to characterize a bond (ON TEST!) |
|
Definition
[image]
this shows the orbitals involved in forming the bond |
|
|
Term
| depiction of how electron configuration contributes to covalent bonds when bonding atoms are tetrahedral |
|
Definition
|
|
Term
| how to characterize double bonds when the bonding atoms are trigonal planar |
|
Definition
|
|
Term
| why the bond angles that are assumed are often approximations |
|
Definition
| because of the molecule not being entirely symmetrical |
|
|
Term
| the orbitals that are relevant in VSEPR theory |
|
Definition
|
|
Term
| the type of orbitals used by sigma bonds |
|
Definition
|
|
Term
| how to characterize triple bonds when the bonding molecule is linear |
|
Definition
[image]
remember, a triple bond contains 1 sigma bond and 2 pi bonds |
|
|
Term
| what a triple bond contains |
|
Definition
| 1 sigma bond and 2 pi bonds |
|
|
Term
| depiction of unhybridized s and p orbital overlapping |
|
Definition
[image]
the shaded area of the p orbital is positive
everything unshaded is negative |
|
|
Term
| depiction of sp hybrid orbital |
|
Definition
[image]
the shaded area is positive |
|
|
Term
| the effect of hybridization on the sp orbital |
|
Definition
destructive interference causes the positive lobe to decrease in amplitude and the negative lobe to increase in amplitude
[image] |
|
|
Term
| the orbitals that define shape of an atom |
|
Definition
|
|
Term
|
Definition
| the electrons that are in the hybridized orbitals |
|
|
Term
| what causes π (pi) bonds? |
|
Definition
|
|
Term
| the symmetry a sigma bonding orbital has |
|
Definition
| cylindrically symmetrical (cross section along any point in the bond is circular) |
|
|
Term
| if a bond is cylindrically symmetrical, it's a ______ bond |
|
Definition
|
|
Term
| if a bond is not cylindrically symmetrical, it's a ______ bond |
|
Definition
|
|
Term
|
Definition
| the electrons in the unhybridized π (pi) bonds |
|
|
Term
| which electrons are more energetic? those in the sigma system or those in the pi system? |
|
Definition
|
|
Term
| why are the electrons in the pi system more energetic than those in the sigma system? |
|
Definition
|
|
Term
| which electrons are most likely to be reactive in a chemical reaction? |
|
Definition
| the more energetic ones; those in the pi system |
|
|
Term
| can electrons that influence shape of an atom be part of the pi system? |
|
Definition
| no, they're part of the sigma system |
|
|
Term
| principal quantum number (n) |
|
Definition
| this defines the energy level of an electron |
|
|
Term
| angular momentum quantum number (l) |
|
Definition
| this defines the shape of the orbital |
|
|
Term
|
Definition
| set of electrons that have the same n and l values |
|
|
Term
| how a subshell is designated |
|
Definition
| by a letter and a number, such as s1, s2, and p2 |
|
|
Term
| magnetic quantum number (ml) |
|
Definition
describes the orientation of the orbital in space
can have values of l to -l, including 0 |
|
|
Term
| value of l for the s orbital |
|
Definition
|
|
Term
| value of l for the p orbital |
|
Definition
|
|
Term
| subshell designation for the s orbital |
|
Definition
ns
n = principal quantum number |
|
|
Term
| subshell designation for the p orbital |
|
Definition
np
n = principal quantum number |
|
|
Term
| possible values of ml for the s orbital |
|
Definition
|
|
Term
| possible values of ml for the p orbital |
|
Definition
|
|
Term
| the elements with their valence electrons in the s orbital |
|
Definition
| He and the Group 1A and 2 A elements |
|
|
Term
| the elements with their valence electrons in the p orbital |
|
Definition
|
|
Term
| the elements with their valence electrons in the d orbital |
|
Definition
|
|
Term
| the elements with their valence electrons in the f orbital |
|
Definition
|
|
Term
|
Definition
| bonds between atoms such that the electrons are more strongly attracted by one atom than the other such that the electron distribution between atoms is not symmetrical |
|
|
Term
δ
indicate what this is used for |
|
Definition
lower case Greek letter delta
used to indicate partial charge |
|
|
Term
|
Definition
| partial positive charge, used for electron poor atom |
|
|
Term
|
Definition
| partial negative, used for electron rich atom |
|
|
Term
| bond polarity is due to... |
|
Definition
| differences in enegativity (EN) |
|
|
Term
|
Definition
| an atom's ability to attract electrons |
|
|
Term
| periodic trend in electronegativity |
|
Definition
| increases as you go northeast |
|
|
Term
| electronegativity difference in covalent bonds |
|
Definition
|
|
Term
| electronegativity difference in polar covalent bonds |
|
Definition
|
|
Term
| electronegativity difference in ionic bonds |
|
Definition
|
|
Term
| depiction of how arrows are used to indicate electron distribution |
|
Definition
[image]
This is a crossed arrow, with the arrow pointing to the negative end and the other end being crossed to indicate positive end. Electrons are displaced in the direction of the arrow. |
|
|
Term
|
Definition
| the shifting of electrons in a δ bond in response to the electronegativity of nearby atoms |
|
|
Term
| partial charge on atom or bong? |
|
Definition
|
|
Term
| molecular polarity results from... |
|
Definition
| the vector summation of all individual bond polarities and lone-pair contributions in the molecule |
|
|
Term
| net molecular polarity is measured by... |
|
Definition
|
|
Term
|
Definition
| the magnitude of the charge Q at either end of the molecular dipole times the distance r between the charges |
|
|
Term
| how to calculate dipole moment |
|
Definition
μ = Q X r
μ = dipole moment (C • m)
Q = magnitude of charge (C)
r = distance between charges (m) |
|
|
Term
| how dipole moments are expressed in SI |
|
Definition
|
|
Term
1 D = ______ coulomb meters (C • m)
D = debye |
|
Definition
| 3.336 X 10-30 coulomb meters (C • m) |
|
|
Term
| some elements with substantially different enegativities from C |
|
Definition
|
|
Term
| effect of lone pairs on dipole moment |
|
Definition
| lone pairs can alter the direction of the dipole moment |
|
|
Term
|
Definition
| the charge on a particular atom in a molecule if that atom was by itself |
|
|
Term
| what formal charges are used for |
|
Definition
|
|
Term
| why it's helpful to identify and calculate formal charges correctly |
|
Definition
| because they can give clues about chemical reactivity |
|
|
Term
|
Definition
| individual structural forms of a resonance hybrid |
|
|
Term
| the only difference between resonance forms |
|
Definition
| the placement of the π and nonbonding valence electrons |
|
|
Term
|
Definition
| molecule that can't be represented adequately using a single line structure and must instead be considered as an average of 2 or more resonance forms |
|
|
Term
| rules for resonance forms |
|
Definition
1: Individual resonance forms are imaginary, not real.
2: resonance forms differ only in the placement of their π or nonbonding electrons
3: different resonance forms of a substance don't have to be equivalent
4: resonance forms obey normal rules of valency
5: the resonance hybrid is more stable than any individual resonance form |
|
|
Term
| the real structure of resonance forms |
|
Definition
| a composite, or resonance hybrid |
|
|
Term
| how the movement of electrons is represented on drawings |
|
Definition
|
|
Term
| # of resonance forms vs. stability of substance and why |
|
Definition
| the more resonance forms, the more stable the substance because its electrons are spread out over a larger part of the molecule and are closer to more nuclei |
|
|
Term
| a useful technique for drawing resonance forms |
|
Definition
| in general, any 3 atom grouping with a p orbital on each atom has 2 resonance forms |
|
|
Term
|
Definition
| atom that contains a single unpaired electron |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| conjugate base (Brønstead-Lowry) |
|
Definition
| the ion that results when an acid loses a proton |
|
|
Term
| conjugate acid (Brønstead-Lowry) |
|
Definition
| the ion that results when a base gains a proton |
|
|
Term
| how acids and bases interact in the general sense |
|
Definition
| acid + base <--> conjugate base + conjugate acid |
|
|
Term
| how water can act as an acid or a base |
|
Definition
| by accepting (base) or donating (acid) a proton |
|
|
Term
|
Definition
| measures the exact strength of a given acid in water |
|
|
Term
| how to calculate acidity constant (Ka) |
|
Definition
| Ka = ([H3O+][CB])/([acid])
Ka = acidity constant
CB = conjugate base |
|
|
Term
|
Definition
| negative common logarithm of the Ka |
|
|
Term
|
Definition
|
|
Term
| size of pKa vs. size of Ka |
|
Definition
|
|
Term
| size of pKa for stronger acid |
|
Definition
|
|
Term
| size of Ka for stronger acid |
|
Definition
|
|
Term
| size of pKa for weaker acid |
|
Definition
|
|
Term
| size of Ka for weaker acid |
|
Definition
|
|
Term
| some acids in order of size of pKa (highest to lowest)
refer to video to complete the list |
|
Definition
| -R (group of C's and H's)
-ammonia (NH3) and R2NH2NH3
-water and ROH
-Hydronium (H3O+)
-[image]
-HCl, HBr, H2SO4 |
|
|
Term
| acid strength vs. strength of conjugate base |
|
Definition
|
|
Term
| the direction the proton goes in an acid-base reaction goes |
|
Definition
| from the stronger acid to the stronger base |
|
|
Term
| where the strong acids and bases and weak acids and bases must be in an acid-base reaction |
|
Definition
| starting acids and bases should be stronger and ending acids and bases should be weaker |
|
|
Term
| how to convert pKa into Ka |
|
Definition
| Ka = 10-pKa
write it in scientific notation |
|
|
Term
| organic acids are characterized by... |
|
Definition
| the presence of a positively polarized H atom |
|
|
Term
| the 2 main kinds of organic acids |
|
Definition
-those that contain a H atom bonded to an electronegative O atom (O-H)
-those that contain a H atom bonded to a C atom next to C=O bond (O=C-C-H) |
|
|
Term
| some ways anions can be stabilized |
|
Definition
-having a negative charge on a highly electronegative atom
-resonance |
|
|
Term
| why organic acids with O-H bonds are acidic |
|
Definition
| because the conjugate base is stabilized by having its negative charge on a strongly electronegative atom |
|
|
Term
| why organic acids with C=O bonds are acidic |
|
Definition
| because the conjugate base is stabilized by resonance |
|
|
Term
|
Definition
| organic acids that contain the -CO2H grouping |
|
|
Term
| organic bases are characterized by... |
|
Definition
| the presence of an atom with a lone pair of electrons that can bond to H+ |
|
|
Term
|
Definition
|
|
Term
|
Definition
donates an electron pair
has pair of nonbonding electrons that it can use to bond to a Lewis acid |
|
|
Term
| what happens to the electron pair in the interaction of Lewis acids and bases? |
|
Definition
| it is shared in a covalent bond |
|
|
Term
| why metal cations can be Lewis acids |
|
Definition
| because they accept a pair of electrons when they bond to a base |
|
|
Term
| why some metal compounds can be Lewis acids |
|
Definition
| because they have unfilled valence orbitals and can accept electron pairs from Lewis bases |
|
|
Term
| why most O and N containing organic compounds act like Lewis bases |
|
Definition
| because they have lone pairs of electrons |
|
|
Term
| if an acid-base rxn forms a complex, can it go back and forth? |
|
Definition
|
|
Term
| other than bonds within molecules, this is also important in chemical reactions |
|
Definition
|
|
Term
|
Definition
interactions between molecules
aka intermolecular forces and van der Waals forces |
|
|
Term
| types of noncovalent interactions between molecules |
|
Definition
-dipole-dipole forces
-(London) dispersion forces
-H bonds |
|
|
Term
|
Definition
they occur between polar molecules as a result of electrostatic interactions among dipoles
-can be attractive or repulsive depending on orientation of the molecules
-attractive predominates because it's lower in energy |
|
|
Term
| dipole-dipole forces can be attractive or repulsive depending on... |
|
Definition
| orientation of the molecules |
|
|
Term
| attractive dipole-dipole forces predominate because... |
|
Definition
|
|
Term
| depiction of attractive and repulsive dipole-dipole forces |
|
Definition
|
|
Term
| (London) dispersion forces |
|
Definition
| occur between all neighboring molecules and arise because the electron distribution within molecules is consistently changing |
|
|
Term
| what causes dispersion forces in nonpolar molecules? |
|
Definition
| dipole moments that are caused by consistently changing electron distribution |
|
|
Term
|
Definition
| attractive interaction between a H bonded to an O or N atom and an unshared electron pair on another N or O atom |
|
|
Term
| depiction of (London) dispersion forces |
|
Definition
|
|
Term
|
Definition
|
|
Term
| what causes water to be liquid at standard temperatures? |
|
Definition
|
|
Term
| what makes a sugar molecule hydrophilic? |
|
Definition
| the -OH groups in its structure that enable it to form H bonds |
|
|
Term
| what makes vegatable oil hydrophobic? |
|
Definition
| has no groups that have H bonds, so it's limited to (London) dispersion forces |
|
|
Term
|
Definition
|
|
Term
| magnitude of charge in ionic bonds |
|
Definition
|
|
Term
| what the pKa of an acid must be to react almost completely with water |
|
Definition
| at least 3 units lower than that of water
the pKa of water is 15.74; therefore, the pKa must be 12.74 or less |
|
|
Term
|
Definition
|
|
Term
| how to calculate pH using molarity (M) and pKa |
|
Definition
| 1: find Ka
2: plug M and Ka into the Ka formula
3: solve for neumerator
4: plug what you get into the pH equation |
|
|
Term
| what does an acid need to have if it wants to significantly react with the salt of another acid? |
|
Definition
|
|
Term
| why reactions of the same chemical can yield different results |
|
Definition
| change in distribution of electrons caused by resonance |
|
|
Term
| one reason two acids that contain an OH group can have differing acidity |
|
Definition
| because one is better able to be stabilized by resonance, i.e., more resonance structures |
|
|
Term
| can resonance contribute to whether or not a molecule or ion has a dipole moment? |
|
Definition
if uniform, then no
if not uniform, then it could |
|
|
Term
| why an O atom with 2 single bonds can have a dipole moment |
|
Definition
| because of the lone pair electrons, which contribute its tetrahedral shape |
|
|
Term
| in which direction are acid-base reactions favored? |
|
Definition
| the direction in which the pKa pf the acid increases |
|
|
Term
| why CH3CH2CH2OH has a higher boiling point than CH4 |
|
Definition
|
|
Term
| when a molecule has H bonding and dipole moments, which contributes greater to interactions with other molecules? |
|
Definition
|
|
Term
| how more electronegative elements can increase the acidity of organic acids that contain an O-H bond |
|
Definition
| pulling electrons, the effect going down the chain, ultimately weakening the O-H bond |
|
|
Term
| example of how to draw a 3D representation of a tetrahedral molecule |
|
Definition
[image]
especially note that the wedge and dotted line have to track together; one is essentially hiding behind the other |
|
|
Term
| example depiction of bond polarity and dipole moment |
|
Definition
|
|
Term
how the length of the nonpolar zig-zag line on these 2 molecules affects the dipole moment
[image] |
|
Definition
| the longer the nonpolar zig-zag line, the lower the net dipole moment |
|
|
Term
| does the sigma system change when drawing resonance structures? |
|
Definition
|
|
Term
| the difference between resonance forms |
|
Definition
| where you put the pi electrons |
|
|
Term
| when drawing resonance forms, never mess with... |
|
Definition
|
|
Term
| one thing that can make one resonance form more prominent than the other |
|
Definition
| electronegativity of a certain atom |
|
|
Term
| the absence of this system makes a molecule or ion unable to have resonance |
|
Definition
|
|
Term
| the most important thing to look for when determining which resonance form is better than the other |
|
Definition
| whether or not atoms obey the octet rule; this supersedes electronegativity |
|
|
Term
| what it means when one resonance form is better than the other |
|
Definition
| the actual thing looks more like one than the other |
|
|
Term
| rules for assessing which resonance structures are the best representations |
|
Definition
1: the most important resonance contributors have the greatest numbers of filled octets
2: the structure with fewer formal charges is the better representation
3: electronegativity of specific elements |
|
|
Term
| when all resonance structures for a particular molecule or ion are equally good representations of it, they are... |
|
Definition
|
|
Term
|
Definition
| measures involvement of s orbital as part of the hybrid |
|
|
Term
| s-character of an sp3 hybridized atom |
|
Definition
|
|
Term
| s-character of an sp2 hybridized atom |
|
Definition
|
|
Term
| s-character of an sp hybridized atom |
|
Definition
|
|
Term
| importance of s-character |
|
Definition
| the higher an atom's s-character, the higher its electronegativity |
|
|
Term
| length of C-C bond vs. strength of bond |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| completely dissociates in water |
|
|
Term
| why ionic compounds (salts) will dissolve in water |
|
Definition
| because water supports the presence of ions |
|
|
Term
| why salts won't dissolve in nonpolar solvents |
|
Definition
| because the nonpolar solvent has no "handle" to grab onto ions |
|
|
Term
|
Definition
|
|
Term
| this is constant once e'librium is established |
|
Definition
| c'trations of products and reactants |
|
|
Term
|
Definition
| no, because you can't have negative c'trations |
|
|
Term
| relationship between ΔG and Keq |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| why is a proton more likely to dissociate from O than from C? |
|
Definition
| because O is more e'negative |
|
|
Term
|
Definition
|
|
Term
| what R is used to represent |
|
Definition
| collection of H's and C's |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| Keq = ([CA][CB]) / ([A][B]) |
|
|
Term
| once e'librium is established, the side containing which base will be favored? |
|
Definition
the side containing the more stable base
a base that undergoes resonance could be the more stable base |
|
|
Term
| pKa of this molecule
[image] |
|
Definition
|
|
Term
| when you go down a column on the PTable, e'negativity gives way to... |
|
Definition
|
|
Term
|
Definition
| the ability to obtain an induced polarity |
|
|
Term
| PTable trend in polarizeability |
|
Definition
| the further down you go down the column, the more polarizeable |
|
|
Term
| how polarizeability affects strength of acid |
|
Definition
| the more polarizeable the element from which an anion is derived, the stronger the acid |
|
|
Term
| why acids containing more polarizeable elements tend to be more acidic |
|
Definition
| because the anion derived from a more polarizeable element tends to be more stable than that derived from a less polarizeable anion |
|
|
Term
| polarizeability of an element vs. the stabylity of its anion |
|
Definition
|
|
Term
| depiction of an endothermic reaction for an endothermic reaction |
|
Definition
|
|
Term
| the 2 commandments of resonance |
|
Definition
1: don't break any single bonds
2: don't exceed an octet for 2nd row elements |
|
|
Term
| questions to ask once resonance is established |
|
Definition
1: can we convert any lone pairs into pi bonds without violating the two commandments?
2: can we convert any pi bonds into lone pairs without violating the 2 commandments?
3: can we convert any pi bonds into pi bonds without violating the 2 commandments? |
|
|
Term
| rules for assessing the relative importance of a resonance structure |
|
Definition
1: the most important resonance forms have the greatest number of filled octets
2: the structure with fewer fortmal charges is more important
3: other things being equal, a structure with negative charge on the more electronegative element will be more important
4: resonance structures with equally good Lewis structures are described as equivalent and contribute equally to the resonance hybrid |
|
|
Term
| some factors that affect stability of conjugate bases |
|
Definition
1: atom - what atom is the charge on?
2: resonance - does resonance make one conjugate base more stable than the other?
3: induction - are any conjugate bases stabilized by inductive effects?
4: orbital - in what orbital do we find the negative charge for each conjugate base? |
|
|
Term
| an ac id's willingness to give up a proton is affected by... |
|
Definition
| stability of that bond between the H and the other atom |
|
|
Term
| trend in the ability of an element to stabilize charge |
|
Definition
| increases as you go down the column |
|
|
Term
| why HI would be more willing to give up its proton, i.e., more acidic, than HF |
|
Definition
| because I has a larger volume over which to spread the charge, tius being more stable when it gives up its proton |
|
|
Term
| why resonance is such a stabilizing force |
|
Definition
| because a delocalized negative charge is more stable than a localized negative charge |
|
|
Term
| if the conjugate base of one acid has resonance and the other one doesn't, which acid will be more acidic? |
|
Definition
|
|
Term
| induction (acid-base context) |
|
Definition
| the pulling of electron density caused by differences in electronegativity |
|
|
Term
| how orbital affects acidity of an atom |
|
Definition
| sp orbitals tend to be more stable than sp2 and sp3 or bitals because sp orbitals tend to have their electrons closer to the nucleus |
|
|
Term
| which H is more acidic: H bonded to sp3 hybridized N or H bonded to sp hybridized C? |
|
Definition
| H bonded to sp hybridized C |
|
|
Term
|
Definition
| the effect of CH groups hindering interaction with the solvent |
|
|
Term
|
Definition
| shows how the electrons move during a reaction to form the products |
|
|
Term
| how to show the mechanism of an acid-base rxn |
|
Definition
draw an arrow to indicate floe of electrons from Lewis acid to
Lewis base |
|
|
Term
|
Definition
| groups of atoms within a molecule that have a characteristic chemical behavior |
|
|
Term
| the chemistry of every organic molecule is determined by... |
|
Definition
|
|
Term
| 3 categories functional groups can be categorized into |
|
Definition
-those w/ C-C multiple bonds
-those in which C forms a single bond with an enegative atom
-those w/ C=O 2bl bond |
|
|
Term
|
Definition
|
|
Term
| alkanes are described as... |
|
Definition
|
|
Term
| why alkanes are hydrocarbons |
|
Definition
| because they contain only C and H |
|
|
Term
| why alkanes are saturated |
|
Definition
| because all bonds are single |
|
|
Term
| the general formula for alkanes |
|
Definition
|
|
Term
|
Definition
| alkane w/ all the C's in a row |
|
|
Term
|
Definition
| alkane that has a branched C chain |
|
|
Term
|
Definition
| isomers whose atoms are connected differently |
|
|
Term
| do constitutional isomers have different properties? |
|
Definition
|
|
Term
| straight-chain alkanes are named according to... |
|
Definition
| # of C's in their C chain |
|
|
Term
|
Definition
| the partial structure that results from the removal of 1 H from an alkane |
|
|
Term
| how alkyl groups are named |
|
Definition
| by replacing -ane with -yl |
|
|
Term
|
Definition
| formed by removal of an H atom from the end of a straight-chain alkane |
|
|
Term
| branched-chain alkyl groups |
|
Definition
| formed by removing an H from an internal C |
|
|
Term
| the prefixes sec- and tert- refer to... |
|
Definition
| the number of other C atom attached to the branching C atom |
|
|
Term
|
Definition
| secondary (2 C's attached to the branching C) |
|
|
Term
|
Definition
| tertiary (3 C's attached to the branching C) |
|
|
Term
| the possible degrees of alkyl substitution for C |
|
Definition
-primary
-2ndary
-tertiary
-quarternary |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| this symbol refers to the rest of the molecule |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| the system of nomenclature used in this book for naming alkanes |
|
Definition
|
|
Term
| the components of a chemical name in the IUPAC system |
|
Definition
-locant
-prefix
-parent
-suffix |
|
|
Term
|
Definition
| shows the location of substituents and functional groups |
|
|
Term
|
Definition
| indicates the type of constituent or functional group |
|
|
Term
|
Definition
| # of C's in the principal chain |
|
|
Term
|
Definition
| identifies functional group family |
|
|
Term
|
Definition
1: find the parent hydrocarbon
2: number the atoms in the parent chain
3: identify and number the substituents
4: write the name as a single word
5: name a complex substituent as if it was a compound, and set it off in parentheses |
|
|
Term
| how to find the parent hydrocarbon in an alkane |
|
Definition
1: find the longest continuous chain of C's, and use its name as the parent name
2: if 2 chains have the same number of C's, choose the one with more branch points |
|
|
Term
| how to number the atoms in the parent chain |
|
Definition
1: start numbering at the end nearer the 1st branch point
2: if branching occurs an equal distance from both ends, begin numbering at the end nearer the second branch point |
|
|
Term
| how to identify and number the substituents |
|
Definition
1: give each substituent a number that corresponds to its number on the parent chain
2: 2 substituents on the same C receive the same # |
|
|
Term
| how to write the name as a single word |
|
Definition
1: use hyphens to separate prefixes and commas to separate numbers
2: use the prefixes di-, tri-, and tetra- if necessary, but don't use them for alphabetizing |
|
|
Term
| how to name a complex substituent as if it was a compound and set it off within parentheses |
|
Definition
1: some simple branched-chain alkyl groups have common names
2: the prefix iso- is used for alphabetixing, but sec- and tert- are not |
|
|
Term
| some properties of alkanes |
|
Definition
| -alkanes are chemically inert to most laboratory reagents
-alkanes react with O2 (combustion) and Cl2 (substitution)
-the boiling and melting points of alkanes increase with increasing molecular weight
-increased branching lowers an alkane's boiling point |
|
|
Term
| reactivity of alkanes to most laboratory reagents |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| boiling and melting points of alkanes vs. molecular weight |
|
Definition
|
|
Term
| why the boiling and melting poiunts of alkanes increase with increasing molecular weight |
|
Definition
|
|
Term
| strength of dispersion forces vs. molecular weight |
|
Definition
|
|
Term
| branching vs. an alkane's boiling point |
|
Definition
| the more branching, the higher the boiling point |
|
|
Term
| some straight-chain alkanes |
|
Definition
|
|
Term
|
Definition
| the branch of chemistry concerned with the 3D aspects of molecules |
|
|
Term
|
Definition
|
|
Term
| what produces isomers of ethane at different conformation? |
|
Definition
| rotation about a single bond |
|
|
Term
| 2 ways isomers can be represented |
|
Definition
-sawhorse representations
-Newman projections |
|
|
Term
|
Definition
| views the C-C bond at an oblique angle |
|
|
Term
|
Definition
| views the C-C bond end-on-end and represents the 2 C's as a circle |
|
|
Term
|
Definition
the lowest energy conformation
occurs when all C-H bonds are as far from each other as possible (H's not lining up with each other) |
|
|
Term
|
Definition
the highest energy conformation
occurs when all the C-H bonds are as close to each other as possible (H's lining up with each other) |
|
|
Term
| the energy difference in staggered conformation is due to... |
|
Definition
| torsional strain from interactions between C-H bonding orbitals on one C and C-H bonding antibonding orbitals on an adjacent C, stabilizing the staggered conformation |
|
|
Term
|
Definition
| the extra energy in eclipsed conformation |
|
|
Term
| graph showing potential energy vs. angle of rotation |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| photograph the conformations in section 3.7 |
|
|
Term
| the lowest energy conformation of butane occurs when... |
|
Definition
| the 2 large methyl groups are as far from each other as possible |
|
|
Term
| gauche conformation of butane |
|
Definition
| when 2 methyl groups are 60 degrees apart |
|
|
Term
| the energy difference in different conformations of molecules is due to... |
|
Definition
|
|
Term
|
Definition
| the repulsive interaction that results from forcing atoms to be closer together than their atomic radii allow |
|
|
Term
| the highest energy conformations of butane occur when... |
|
Definition
| the 2 methyl groups are eclipsed |
|
|
Term
| the most favored conformation for any straight-chain alkane |
|
Definition
| has C-C bonds in staggered arrangements and large substituents anti to each other |
|
|
Term
| the conformation adopted by most molecules |
|
Definition
| the most stable conformation |
|
|
Term
| the 5 parts to every name when naming organic molecules |
|
Definition
1: stereoisomerism
2: substituents
3: parent
4: unsaturation
5: functional group |
|
|
Term
|
Definition
| indicates whether 2bl bonds are cis/trans and indicates stereocenters (R,S) |
|
|
Term
|
Definition
| groups connected to the main chain |
|
|
Term
|
Definition
|
|
Term
|
Definition
| identifies whether there are any 2bl or triple bonds |
|
|
Term
|
Definition
| the group after which the compound is named |
|
|
Term
| why you must name an organic molecule starting with the functional group |
|
Definition
| because the position of the functional group affects which parent chain you chose |
|
|
Term
| alkene (double bond) functional group |
|
Definition
|
|
Term
|
Definition
| alkene (double bond) functional group |
|
|
Term
| alkyne (triple bond) functional group |
|
Definition
|
|
Term
|
Definition
| alkyne (triple bond) functional group |
|
|
Term
| arene (aromatic ring) functional group |
|
Definition
| 6 trigonal planar C's in a ring |
|
|
Term
| 6 trigonal planar C's in a ring |
|
Definition
| arene (aromatic ring) functional group |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| monophosphate functional group |
|
Definition
|
|
Term
|
Definition
| monophosphate functional group |
|
|
Term
| diphosphate functional group |
|
Definition
|
|
Term
|
Definition
| diphosphate functional group |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| imine (Schiff base) functional group |
|
Definition
|
|
Term
|
Definition
| imine (Schiff base) functional group |
|
|
Term
|
Definition
RN
the bond is a triple bond |
|
|
Term
RN
the bond is a triple bond |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| disulfide functional group |
|
Definition
|
|
Term
|
Definition
| disulfide functional group |
|
|
Term
| sulfoxide functional group |
|
Definition
|
|
Term
|
Definition
| sulfoxide functional group |
|
|
Term
| aldehyde functional group |
|
Definition
|
|
Term
|
Definition
| aldehyde functional group |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| carboxylic acid functional group |
|
Definition
|
|
Term
|
Definition
| carboxylic acid functional group |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| thioester functional group |
|
Definition
|
|
Term
|
Definition
| thioester functional group |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| acid chloride functional group |
|
Definition
|
|
Term
|
Definition
| acid chloride functional group |
|
|
Term
| carboxylic acid anhydride functional group |
|
Definition
|
|
Term
|
Definition
| carboxylic acid anhydride functional group |
|
|
Term
suffix associated with alkene
(double bond) functional group |
|
Definition
|
|
Term
| suffix associated with alkyne (triple bond) functional group |
|
Definition
|
|
Term
| suffix associated with arene (aromatic ring) functional group |
|
Definition
|
|
Term
| suffix associated with halide functional group |
|
Definition
|
|
Term
| suffix associated with alcohol functional group |
|
Definition
|
|
Term
| suffix associated with ether functional group |
|
Definition
|
|
Term
| suffix associated with monophosphate functional group |
|
Definition
|
|
Term
| suffix associated with diphosphate functional group |
|
Definition
|
|
Term
| suffix associated with amine functional group |
|
Definition
|
|
Term
| suffix associated with imine (Schiff base) functional group |
|
Definition
|
|
Term
| suffix associated with nitrile functional group |
|
Definition
|
|
Term
| suffix associated with thiol functional group |
|
Definition
|
|
Term
| suffix associated with sulfide functional group |
|
Definition
|
|
Term
| suffix associated with disulfide functional group |
|
Definition
|
|
Term
| suffix associated with sulfoxide functional group |
|
Definition
|
|
Term
| suffix associated with aldehyde functional group |
|
Definition
|
|
Term
| suffix associated with ketone functional group |
|
Definition
|
|
Term
| suffix associated with carboxylic acid functional group |
|
Definition
|
|
Term
| suffix associated with ester functional group |
|
Definition
|
|
Term
| suffix associated with thioester functional group |
|
Definition
|
|
Term
| suffix associated with amide functional group |
|
Definition
|
|
Term
| suffix associated with acid chloride functional group |
|
Definition
|
|
Term
| suffix associated with carboxylic acid anhydride functional group |
|
Definition
|
|
Term
| suffix to use when there's no functional group involved |
|
Definition
| put an e at the end of it |
|
|
Term
| when naming the parent chain, meth means... |
|
Definition
| 1 C atom in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, eth means... |
|
Definition
| 2 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, prop means... |
|
Definition
| 3 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, but means... |
|
Definition
| 4 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, pent means... |
|
Definition
| 5 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, hex means... |
|
Definition
| 6 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, hept means... |
|
Definition
| 7 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, oct means... |
|
Definition
| 8 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, non means... |
|
Definition
| 9 C atoms in the alkane or parent chain |
|
|
Term
| when naming an alkane or the parent chain, dec means... |
|
Definition
| 10 C atoms in the alkane or parent chain |
|
|
Term
|
Definition
| alkane or parent chain with 1 C atom |
|
|
Term
|
Definition
| alkane or parent chain with 2 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 3 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 4 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 5 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 6 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 7 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 8 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 9 C atoms |
|
|
Term
|
Definition
| alkane or parent chain with 10 C atoms |
|
|
Term
|
Definition
| methane with one H replaced by R |
|
|
Term
|
Definition
| ethane with 1 H replaced by R |
|
|
Term
|
Definition
| propane with 1 H replaced by R |
|
|
Term
|
Definition
| butane with 1 H replaced by R |
|
|
Term
|
Definition
| pentane with 1 H replaced by R |
|
|
Term
|
Definition
| hexane with 1 H replaced by R |
|
|
Term
|
Definition
| heptane with 1 H replaced by R |
|
|
Term
|
Definition
| octane with 1 H replaced by R |
|
|
Term
|
Definition
| nonane with 1 H replaced by R |
|
|
Term
|
Definition
| decane with 1 H replaced by R |
|
|
Term
| when there is a double bond, should the parent chain include the double bond? |
|
Definition
|
|
Term
| when there is no double bond, but there is a functional group attached, should the parent chain include the C next to the functional group? |
|
Definition
|
|
Term
|
Definition
[image]
attached to the end C |
|
|
Term
|
Definition
|
|
Term
|
Definition
[image]
attached to the middle C |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
[image]
here, it's connected to a Cl |
|
|
Term
|
Definition
|
|
Term
|
Definition
[image]
notice the Cl is attached to the secondary C |
|
|
Term
|
Definition
|
|
Term
|
Definition
[image]
notice the R is attached to the tertiary C |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| to represent a generalized organic group |
|
|
Term
| what characters to use to indicate whether a C is primary, 2ndary, tertiary, or quarternary |
|
Definition
|
|
Term
| is an H bonded to a primary C primary, secondary, or tertiary? |
|
Definition
|
|
Term
| is an H bonded to a secondary C primary, secondary, or tertiary? |
|
Definition
|
|
Term
| is an H bonded to a tertiary C primary, secondary, or tertiary? |
|
Definition
|
|
Term
| the template for the name of an alkane |
|
Definition
| locant-prefix-parent-suffix |
|
|
Term
| what the locant in the name of an alkane is supposed to indicate |
|
Definition
| where the substituents and functional groups are |
|
|
Term
| what the prefix in the name of an alkane is supposed to indicate |
|
Definition
| what the substituents are |
|
|
Term
| what the parent in the name of an alkane is supposed to indicate |
|
Definition
| how many carbons in alkane |
|
|
Term
| what the suffix in the name of an alkane is supposed to indicate |
|
Definition
|
|
Term
| if 2 hydrocarbon chains of equal length have different numbers of branch points, which hydrocarbon chain is the parent? |
|
Definition
| the one with more branch points |
|
|
Term
| when numbering the C's in the hydrocarbon chain, where should you begin? |
|
Definition
| at end nearer to the first branch point |
|
|
Term
| when numbering the hydrocarbons in a molecule with branching an equal distance away from the parent chain, where should you begin? |
|
Definition
| at the end nearer to the 2nd branch point |
|
|
Term
| order to list substituents when naming an alkane |
|
Definition
|
|
Term
| how a substituent that is itself branched is included in the name of an alkane |
|
Definition
1: numbered beginning at its point of attachment to the main chain
2: it is then set off in parentheses |
|
|
Term
| why a positive charge can be an indicator of acidity |
|
Definition
| because having the positive charge, it's more like hydronium |
|
|
Term
| what arrows in acid-base reactions indicate |
|
Definition
|
|
Term
| what do you compare when comparing bases? |
|
Definition
| stability of the electrons on each base |
|
|
Term
| number of resonance forms vs. stability of an anion |
|
Definition
| the more resonance forms, the more stable |
|
|
Term
| the only intermolecular force that deals with nonpolar molecules |
|
Definition
|
|
Term
|
Definition
intermolecular forces that occur as the result of induced dipoles between molecules
induced dipoles occur as the result of an instantaneous uneven distribution of electrons |
|
|
Term
| how the size of the molecule's electron cloud affects London forces |
|
Definition
| the bigger the electron cloud, the easier it is to distort the London forces into greases |
|
|
Term
| polarizeability vs. strength of London forces |
|
Definition
|
|
Term
| what branching of molecule does to boiling point |
|
Definition
| general rule of thumb: branching tends to lower the boiling point |
|
|
Term
| how the shape of different isomers of the same compound can affect boiling point |
|
Definition
| the more spherical the molecule, the lower the boiling point due to less area of overlap between adjacent molecules and weaker London forces |
|
|
Term
|
Definition
| positive end of a bond on one molecule being attracted to the negative end of a bond on another molecule |
|
|
Term
|
Definition
a dipole-dipole force between a proton attached to an N or O and an O or N
this isn't a bond; it's an association or attraction |
|
|
Term
| in an organic molecule, a functional group is... |
|
Definition
| a group of atoms that isn't a sp3 hybridized CH group |
|
|
Term
|
Definition
| isomers that have their atoms connected in a different order |
|
|
Term
| amount of substitution arount a bond vs. amount of strain |
|
Definition
| the more substitution around a bond, the more strain |
|
|
Term
| the general formula for cycloalkanes that have 1 ring |
|
Definition
|
|
Term
|
Definition
1: find the parent
2: number the substituents |
|
|
Term
| how to find the parent in a cycloalkane |
|
Definition
-if the number of C atoms in a ring is larger than the number in the largest substituent, the compound is named as an alkyl-substituted cycloalkane
-if the number of C atoms in the ring is smaller than the number in the largest substituent, the compound is named as a cycloalkyl-substituted alkane |
|
|
Term
| alkyl-substituted cycloalkane |
|
Definition
| cycloalkane where the # of C atoms in the ring is larger than the number in the largest substituent |
|
|
Term
| cycloalkyl-substituted alkane |
|
Definition
| cycloalkane where the # of C atoms in the ring is smaller than the number in the largest substituent |
|
|
Term
| how to number the substituents in a cycloalkane |
|
Definition
1: start at a point of attachment and number the substituents so that the second substituent has the lowest possible number
2: if necessary, proceed until a point of difference is found
3: if 2 or more substituents might potentially receive the same number, number them by alphabetical priority
4: halogens are treated in the same way as alkyl groups |
|
|
Term
| size of a cycloalkane's ring vs. amount of rotational freedom |
|
Definition
|
|
Term
| cis-disubstituted cycloalkane ring |
|
Definition
| has 2 substituents on the same side of the ring |
|
|
Term
| trans-disubstituted cycloalkane ring |
|
Definition
| has 2 substituents on opposite sides of the ring |
|
|
Term
| general principles of conformation of cycloalkanes |
|
Definition
1: ring strain
2: heats of combustion of cycloalkanes
3: the nature of ring strain |
|
|
Term
| how to measure the strain in cycloalkanes |
|
Definition
| measure the total energy of a compound and compare it to a strain-free reference compound |
|
|
Term
|
Definition
| the amount of heat released when a compound is completely burned in oxygen |
|
|
Term
| amount of strain vs. heat of combustion |
|
Definition
|
|
Term
| how strain a per CJH2 unit can be calculated and plotted |
|
Definition
| as a function of ring size |
|
|
Term
| the rings that have serious strain |
|
Definition
|
|
Term
| rings tend to adopt these conformations |
|
Definition
|
|
Term
| factors that account for ring strain |
|
Definition
-angle strain occurs when bond angles are distorted from their normal values
-torsional strain is due to eclipsing of bonds
-steric strain results when atoms approach too closely |
|
|
Term
|
Definition
| occurs when bond angles are distorted from their normal values |
|
|
Term
|
Definition
| caused by eclipsing of bonds |
|
|
Term
|
Definition
| results when atoms approach too closely |
|
|
Term
| some small cycloalkane rings |
|
Definition
-cyclopropane
-cyclobutane
-cyclopentane |
|
|
Term
| why cyclopropane is more reactive than other cycloalkanes |
|
Definition
|
|
Term
| what cyclopentane does to relieve torsional strain |
|
Definition
| adopts a puckered conformation |
|
|
Term
|
Definition
| in this conformation, one C is bent out of plane and the H's are nearly staggered |
|
|
Term
| a conformation of cyclohexane |
|
Definition
|
|
Term
| where the bonds are in chair conformation cyclohexane |
|
Definition
| lower bonds in front and upper bonds in back |
|
|
Term
| the strain in chair conformation cyclohexane |
|
Definition
|
|
Term
| the strain that results when chair conformation cyclohexane converts to boat conformation cyclohexane |
|
Definition
| has little ange strain, but experiences both steric and torsional strain |
|
|
Term
| the 2 kinds of positions on a cyclohexane ring |
|
Definition
-6 axial H's
-6 equatorial H's |
|
|
Term
|
Definition
| perpendicular to the plane of the ring |
|
|
Term
|
Definition
| roughly in the same plane of the ring |
|
|
Term
| the orientation of the H's of each C in cyclohexane |
|
Definition
| each C has 1 axial H and 1 equatorial H |
|
|
Term
| orientation of the H's on the side of the ring in cyclohexane |
|
Definition
| each side of the ring has alternating axial and equatorial H's |
|
|
Term
| if all the H's in a cyclohexane ring are on the same face, they are... |
|
Definition
|
|
Term
| how different chair conformations of cyclohexanes interconvert |
|
Definition
|
|
Term
| what a ring flip does to the axial and equatorial bonds in cyclohexane |
|
Definition
| an axial bond becomes equatorial and an equatorial bond becomes axial |
|
|
Term
| the energy barrier to conversion in cyclohexane |
|
Definition
|
|
Term
|
Definition
| interactions between an axial group and a ring H 2 C's away |
|
|
Term
| what causes diaxial interactions? |
|
Definition
|
|
Term
| the interactions that occur in gauche butane |
|
Definition
| diaxial interactions caused by steric energy |
|
|
Term
| the position in which substituents on a cycloalkane are more stable |
|
Definition
|
|
Term
| the size of the strain between substituents in a cyclohexane depends on... |
|
Definition
| the size and nature of the group |
|
|
Term
| the orientation of the substituents in the chair conformations of a cis isomer |
|
Definition
| one is axial and the other is equatorial |
|
|
Term
| the orientation of the substituents in the chair conformations of a trans isomer |
|
Definition
| both are either axial or equatorial |
|
|
Term
| why axial orientation is less stable than equatorial orientation |
|
Definition
| because there's diaxial interactions in the axial orientation |
|
|
Term
| 2 ways cycloalkane rings can be fused |
|
Definition
|
|
Term
|
Definition
| have rings that are connected by bridges |
|
|
Term
| why a compound with an OH group has a higher boiling point than an otherwise identical compound with a lone O |
|
Definition
|
|
Term
| stability vs. ΔHcombustion |
|
Definition
|
|
Term
| energy of bond vs. size of atoms involved |
|
Definition
|
|
