Term
| Flash Cards for the Fall Honors Chemistry Exam[image] ~By THIS GUY! |
|
Definition
| (I actually typed these! crazy huh?) good luck everyone! tell me if anything is wrong with one of the cards! |
|
|
Term
| An example of an extensive property of matter is? |
|
Definition
|
|
Term
| Which of the following are considered physical properties of a substance? |
|
Definition
All of the above
(Color and odor, melting and boiling points, malleability and hardness) |
|
|
Term
| Which state of matter has a definite volume and takes the shape of its container? |
|
Definition
|
|
Term
| Which of the following is a physical change? |
|
Definition
|
|
Term
| Which of the following is true about homogeneous mixtures? |
|
Definition
| They are known as solutions. |
|
|
Term
| Which of the following is a heterogeneous mixture? |
|
Definition
|
|
Term
| Separating a solid from a liquid is called |
|
Definition
|
|
Term
| An example of a homogeneous mixture is? |
|
Definition
|
|
Term
| Which of the following is true about compounds? |
|
Definition
|
|
Term
| A substance that can be separated into two or more substances only by chemical change is a? |
|
Definition
|
|
Term
| What distinguishes a substance from a mixture? |
|
Definition
| Mixtures can be separated physically, while compounds cannot. |
|
|
Term
| The first figure in a proper chemical symbol always is? |
|
Definition
|
|
Term
| Which of the following represents a compound? |
|
Definition
|
|
Term
| What do chemical symbols and formulas represent respectively? |
|
Definition
|
|
Term
| What must be a change in a chemical reaction? |
|
Definition
| There must be a change in chemical properties. |
|
|
Term
| Which of the following is true for all chemical reactions? |
|
Definition
| the total mass of the reactants equals the total mass of the products. |
|
|
Term
| A chemical change occurs when a piece of wood...? |
|
Definition
|
|
Term
| When an iron nail is grounded into powder, it's mass...? |
|
Definition
|
|
Term
| How many grams of liquid water produces when sixty grams of ice melt? |
|
Definition
|
|
Term
| What is the result of adding 2.5 x 10 and 3.5 x 10? |
|
Definition
| 2.9 x 10(3) to the third power... |
|
|
Term
| How many significant figures are in the measurement 811.40 grams? |
|
Definition
|
|
Term
| How many significant figures are in the measurement 40500 mgs? |
|
Definition
|
|
Term
| Express the sum of 1111km and 222km using the correct number of significant digits? |
|
Definition
|
|
Term
| What is the measurement of 1042 L rounded off to 2 significant digits? |
|
Definition
|
|
Term
| The chief advantage of the metric system over other systems of measurement is that it...? |
|
Definition
|
|
Term
| What is the SI Unit of mass? |
|
Definition
|
|
Term
| Which of the following mass units is the largest? |
|
Definition
|
|
Term
| If the temperature changes by 100 K, by how much would it change in degrees Celsius? |
|
Definition
|
|
Term
| The quantity of 44 liters expressed in cubic meters is? |
|
Definition
|
|
Term
| Density is found by dividing? |
|
Definition
|
|
Term
| What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL? |
|
Definition
|
|
Term
| If the temperature of a piece of steel decreases, what happens to its density? |
|
Definition
|
|
Term
| As the density of a substance increases, the volume of a given mass of that substance...? |
|
Definition
|
|
Term
| As the density of a substance increases, the volume of a given mass of that substance...? |
|
Definition
|
|
Term
| The expression of 8504 km in scientific notation is |
|
Definition
|
|
Term
| The closeness of a measurement to its true value is a measure of its |
|
Definition
|
|
Term
| Which of the following measurements contains two significant figures? **-(A) 0.00400 L -(B) 0.00440 L -(C) 0.00404 L -(D) 0.00044 L |
|
Definition
|
|
Term
| Express the product of 2.2 mm and 4.00 mm using the correct number of significant digits. |
|
Definition
|
|
Term
| When multiplying and dividing measured quantities, the number of significant figures in the result should be equal to the number of significant figures in |
|
Definition
| the lease percise measurement |
|
|
Term
| Which of the folloiwing columes is the smallest? -(A) one deciliter -(B) one liter -(C) one milliliter -(D) one microliter |
|
Definition
|
|
Term
Which temperature scale has no negative temperatures?
-(A) Joule
-(B) Celsuius
-(C) Fahernheit
-(D) Kelvin |
|
Definition
|
|
Term
|
Definition
|
|
Term
| The smallest particle of an elements that retains the properties of that elements is a? |
|
Definition
|
|
Term
| Dalton hypothesized that atoms are indivisible and that all atoms of an elements are identical. It is now known that? |
|
Definition
|
|
Term
| Who conducted experiments to determine the quantity of charge carried by an electron? |
|
Definition
|
|
Term
| Which of the following is true concerning subatomic particles? |
|
Definition
| The neutron was discovered by Chadwick in 1932. |
|
|
Term
| All atoms are? (referring the the charge) |
|
Definition
| Neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons. |
|
|
Term
| The nucleus of an atom is? |
|
Definition
| central core and is composed of protons and neutrons |
|
|
Term
| The particles that are found in the nucleus of an atom are? |
|
Definition
|
|
Term
| The atomic number of an element is the total number of which particles in the nucleus? |
|
Definition
|
|
Term
An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are?[image]<- This guy fixed this card. |
|
Definition
76 protons and 76 electrons [image] And its his Birthday. Thanks Marlowe for pointing out the error and Happy Birthday! |
|
|
Term
| The sum of the protons and neutrons in an atom equals the? |
|
Definition
|
|
Term
| What does the number 84 in the name krypton-84 represent? |
|
Definition
|
|
Term
| All atoms of the same element have the same? |
|
Definition
|
|
Term
| All atoms of the same element have the same? |
|
Definition
|
|
Term
| Isotopes of the same element have different? |
|
Definition
|
|
Term
| The mass number of an element is equal to? |
|
Definition
| the total number of protons and neutrons in the nucleus. |
|
|
Term
| Using the periodic table, determine the number of neutrons in oxygen-16 |
|
Definition
|
|
Term
| How many protons, electrons, and neutrons does an atom with the atomic number 50 and mass number 125 contain? |
|
Definition
| 50 protons 50 electrons and 75 neutrons |
|
|
Term
| If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? |
|
Definition
2/9 E
for all of you goobers out there
2/9 means the two is over the 9
doing subscripts would take too much time
and i have little of that |
|
|
Term
| Select the correct symbol for an atom of tritium |
|
Definition
|
|
Term
| How is the number of neutrons in the nucleus of an atom calculated? |
|
Definition
| Subtract the number of protons from the mass number |
|
|
Term
| How do the isotopes hydrogen 1 and 2 differ? |
|
Definition
| H-2 has 1 neutrons and H-1 had none! |
|
|
Term
| Which of the following isotpes has the same number of neutrons as phosphorus-31? |
|
Definition
|
|
Term
| What unit is used to measure weighted average atomic mass? |
|
Definition
|
|
Term
| Which of the following equals the weighted average atomic mass unit? |
|
Definition
| the mass of helium-4 atom |
|
|
Term
| why do chemists use relative masses of atoms compared to a reference isotope rather than the actual masses of the atoms? |
|
Definition
| the actual mass of an electron is very large compared to the actual mass of a proton. |
|
|
Term
| The atomic mass of an element is the? |
|
Definition
| Total number of subatomic particles in its nucleus |
|
|
Term
| The atomic mass of the element depends on the? |
|
Definition
Mass and relative abundance of each isotope of that element.
(HOLY COW. THIS IS CARD 69 in 22 MINUTES. STILL GOING!) |
|
|
Term
| Which of the following was originally a tenet of Dalton's atomic theory. but had to be revised about a century ago? |
|
Definition
Atoms are tiny indivisible particles.
(haha the quiz that i took this question off of, i got a 2 outta 10! miserble isnt it? thank you karen for giving me the answers!) |
|
|
Term
| Why did J.J. Thomson reason that electrons must be a part of the atoms of all elements? |
|
Definition
| Charge-to-mass ratio of electrons was the same, regardless of the gas used. |
|
|
Term
| Which of the following is true about subatomic particles? |
|
Definition
| The mass of a neutron nearly equals the mass of a proton |
|
|
Term
| As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true? |
|
Definition
| Electrons are distributed around the nucleus and occupy almost all the volume of the atom. |
|
|
Term
| If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals? |
|
Definition
| one electron in each orbital. |
|
|
Term
| How many half-filled orbitals are in a bromine atom? |
|
Definition
|
|
Term
| Stable electron configurations are likely to contain...? |
|
Definition
|
|
Term
| Bohr's model could only explain the spectra of which types of atoms? |
|
Definition
| single atoms with one electron |
|
|
Term
| How many unpaired electrons are in a sulfur atom? (atomic number 16) |
|
Definition
|
|
Term
| What are qunta of light called? |
|
Definition
photons
(man i actually got a 3/10 on this quiz. must be a record. missing 3 out of 10 questions. gah i swear its like i TRIED to miss all of them. miserable! |
|
|
Term
| Which scientist developed the quantum mechanical model of the atom? |
|
Definition
|
|
Term
| How are the frequency and wavelength of light related? |
|
Definition
| They are inversely proportional to each other. |
|
|
Term
| Emission of light from an atom occurs when an element___. |
|
Definition
| Drops from a higher to a lower energy level. |
|
|
Term
| In the bohr model of the atom an electron in an orbit has a fixed ___. |
|
Definition
|
|
Term
| How does the energy of an electron change when the electron moves closer to the nucleus? |
|
Definition
|
|
Term
| The principle quantum number indicates what property of an electron? |
|
Definition
|
|
Term
| What is the shape of the 3p atomic orbital? |
|
Definition
|
|
Term
| How many energy sublevels are in the second principle energy level? |
|
Definition
|
|
Term
| What is the maximum number of S orbitals in any single enery level in an atom. |
|
Definition
|
|
Term
| What is the maximum number of electrons in the second principle energy level? |
|
Definition
|
|
Term
| When an electron moves from a low to a higher energy level, the electron ___. |
|
Definition
| absorbs a quantum of energy. |
|
|
Term
| The shape (not the size) of an electron cloud is determined by the electron ___. |
|
Definition
|
|
Term
| The letter P in the symbol 4p3 indicates the ___. |
|
Definition
|
|
