Term
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Definition
occupies space
solid, liquid, gas |
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Term
| What are the two types of energy |
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Definition
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Term
| What are the four forms of energy and which is most common? |
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Definition
Chemical is most common- stored in chemical bonds, concentration differences?
electrical- charged particle; ions
mechanical- directly moving object; pushing box on floor
radiant- travels in waves; light
thermal-molecular movement; heat |
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Term
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Definition
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Term
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Definition
| sum of the masses of protons and neutrons |
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Term
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Definition
changing mass numbers due to different number of neutrons
used in nuclear medicine- decay of radioactive particle; marker for activity |
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Term
| True or false, all neutral atoms are stable |
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Definition
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Term
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Definition
Positron emission tomography; nuclear medicine test' harnesses energy when positrons collide with electrons; give off gamma rays
use of isotopes
more active tissue is the more radioactive isotopes will concentrate in the tissue |
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Term
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Definition
| atoms are buildling blocks of elements: collections of same type of atoms together form elements |
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Term
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Definition
| 2 or more atoms, same/different elements. If elements are same then have molecules of that element |
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Term
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Definition
| 2 or more DIFFERENT ELEMENTS |
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Term
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Definition
| 2 or more substances combine together |
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Term
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Definition
| homoenous; contain matter and energy |
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Term
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Definition
smaller quantity: ions, proteins, carbohydrates, etc.
no enzymes needed to create/destroy solutions |
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Term
| Concentrations of solutions |
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Definition
| percent molarity osmolarity/osmolality |
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Term
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Definition
| 6.02 X 10^23= 1 mole of substance |
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Term
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Definition
| sum of atomic weights in grams= 1 mole of substance |
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Term
| Osmolarity (L)/osmolality (kg) |
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Definition
# of particles w/in a solution the same value as molarity (osmolality)
important in controlling movement of fluids b/t body comparments. differences in osmolality b/t compartments serves as energy
osmolarity changes with temperature because of volume...(layers=temperature) |
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Term
| glucose when dissolved in water doesn't dissociate so molarity of glucose is same as osmolarity; HOWEvER NaCl dissolved in water dissociates so osmolarity is doubled |
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Definition
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Term
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Definition
| not as homogenous; solute is large but dissolvable, particles scatter light, jello, cell cytosol fluid |
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Term
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Definition
| mixtures where the solute will settle out unless you repeatedly shake it sand in water, blood cells in plasma |
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Term
| True or false, if valence shell is full atom is not reactive |
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Definition
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Term
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Definition
| combinations of atoms via electron sharing, often requires energy input to cause reaction to occur |
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Term
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Definition
| electron exist in different regions around nucleus; each shell is different level of energy |
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Term
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Definition
outermost shell; electron can be reactive
form chemical bond with one another
closer to the nucleus=lower energy
if valence is not full then atom is reactive |
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Term
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Definition
one atom DONATES electron to electron shell of another atom
anion and cation |
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Term
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Definition
electron sharing b/t 2 atoms
non polar molecules- equal sharing CH4
Polar molecules- unequal sharing but not ionic H2O |
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Term
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Definition
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Term
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Definition
| unequeal sharing but not ionic H20 |
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Term
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Definition
| attraction b/t slightly charged moelcules such as water |
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Term
| Patterns of chemical reactions |
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Definition
| synthesis, decomposition, exchange, oxidation reduction, exergonic, endergonic |
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Term
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Definition
| A+B -> AB two components for complex component |
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Term
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Definition
| AB-> A + B complex component and break down into simple component |
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Term
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Definition
| AB+C--> AC + B exchange 1 component for another |
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Term
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Definition
electron donor is oxidized
electron recipient is reduced
important in energy transfer
ionic bond formation is a type of redox reaction |
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Term
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Definition
| give off energy; breakdown of glucose molecule |
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Term
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Definition
| absorb energy formation of ATP |
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Term
| reversibility of chemical reactions |
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Definition
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Term
| Effectors of chemical reactions |
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Definition
temperature
particle size (bigger particle slower reaction, easier the target)
concentration (more solute faster reaction)
catalysts |
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Term
| Higher the temperature the faster rate of reaction, True or false |
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Definition
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Term
The larger the particle the faster the reaction and the harder targert is
True or false |
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Definition
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Term
The greater ratio of solute and solvent the faster the rate of reaction
true or false |
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Definition
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Term
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Definition
| enzymes to quicken the rate of reaction w/o becoming part of the product. |
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