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MCAT > general chem > Flashcards

general chem Flashcards

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MCAT flashcards
1
Q

effective nuclear charge _______ from left to right in periods

A

increases

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2
Q

as you move down elements of given group, ____ increases by one each time

A

principle quantum number

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3
Q

Zeff is _____ in groups

A

pretty consistent

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4
Q

atomic radius refers to ______, while ionic radius is dependent on ________

A

size of neutral element

how the element ionizes based on its element type and group #

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5
Q

______ is essentially the opposite that of all other periodic trends

A

atomic radius

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6
Q

while other periodic trends _________ going up and to the right, atomic radius _______ going down and to the right

A

increase
increase

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7
Q

metals ______ e- and become ______

A

lose
positive

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8
Q

non metals ______ e- and become ____

A

gain
negative

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9
Q

the nonmetals close to the metalloid line possess a ___ ionic radius than their counterparts closer to group VIIIA

A

larger

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10
Q

metals closer to the metalloid line have ______ e- to lose to achieve the electronic configuration seen in group VIIIA

A

more

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11
Q

noble gases are known as ____ because they have minimal chemical reactivity due to their filled valence shells

A

inert gases

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12
Q

the ng have _ boiling points

A

low

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13
Q

transition elements are considered to be ___ and have _ electron affinitites, ionization energies, and electronegativities

A

metals
low

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14
Q

transition metals are capable of losing what

A

different numbers of e- from s and d orbitals in their valence shells

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15
Q

_______ only need one more electron to have a noble gas-like configuration

A

halogens

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16
Q

chalcogens

A

group of non metals and mealloids
size e- in their valence electron shell
small atomic radii and large ionic radii

oxygen is most important element in this group
selenium important for microorganims
at high conc many of these elements can be toxic or damaging

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17
Q

alkaline earth metals

A

slightly higher effective nuclear charges and slighl smaller atomic radii than alkali metals

two e- in valence shell

alkali and alkaline earth metals togt called active metals

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18
Q

alkali metals

A

densities lower than other metals

one loosely bound e- in outermost shells
Zeff values low
largest atomic radii of all elemetns in respective periods
low ionization nrg
low e- affinity low electronegativity

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19
Q

pauling electronegativity scale

A

0.7 cesium

4.0 flourine

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20
Q

electronegativity ____ across period from l to r and __ in group from t to b

A

increases
decreases

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21
Q

e- affinity is what

A

energy dissipated by gaseous species when it gains and e-

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22
Q

electron affinity ____ across period from l to r and what from t to b

A

increases
decreases

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23
Q

noble gases have what electron affiniteis

A

zero

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24
Q

ionization energy is what

A

energy required to remove an e- from gaseous species

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25
Q

electron affinity is a what process

A

exothermic

26
Q

ionization energy is a what process

A

endothermic

27
Q

ionzation energy trend

A

increases from l to r

decreases t to b

28
Q

first ionization energy will be ____ than second, will be_____ than third, etc…

A

smaller
smaller

29
Q

what are the exceptions to the octet rule?

A

incomplete octet: stable with fewer than 8 electrons in their valence shell and include hydrogen 2, helium 2,lithium 2, beryllium 4, and boron 6

expanded octet: any element in period 3 and greater can hold more than 8 electrons, phosphorus 10 sulfur 12, chlorin 15, and many others

odd number of electrons: any molecule with odd number of valence electrons cannot distribute those electrons to give eight to each atom - nitric oxide 11

30
Q

ionic bonding

A

one or more electrons from an atom with a low ionization energy - typically a metal, are transferred to an atom with high electron affinity - typically nonmetal

31
Q

covalent bonding

A

electron pair is shared between two atoms - typically nonmetals that have relatively similar values of EN

32
Q

coordinate covalent

A

if both shared electrons are contributed by only one of the two atoms

generally means lone pair of one atom attacked another atom with an unhybridized p orbital to form a bond

33
Q

ionic compounds melting boiling point etc

A

high melting / boiling point

34
Q

bond length

A

avg distance between two nuclei of atoms in a bond

35
Q

bond energy

A

energy required to break a bond by separating its components into their isolated gaseous atomic states

36
Q

electronic geometry

A

spatial arragenment of all pairs of electrons around the central atom, including both the bonding and lone pairs

37
Q

molecular eometry

A

describes spatial arrangement of only the bonding pairs of electronsco

38
Q

coordination number

A

number of atoms that surround and are bonded to a central atom

39
Q

when orbitals overlap head to head, the resulting bond is a what bond

A

sigma

they allow for free roation about their axes because the electron density of the bonding orbital is a single linear acumulation between atomic nuclei

40
Q

when orbitals overlap in such a way that there are two parallel electron cloud densities, a what bond is formed?

A

pi

do not allow for free rotation because the electron densities of the orbitals are parllel and cannot be twisted in such a way that allows continous overlapping of the clouds of electron densities

41
Q

law of constant composition

A

any pure sample of given compound will contain same elements in an identical mass ratio

42
Q

types of rxns

A

combination rxn
decomposition rxn
combustion
single displacement
double displacement
neutralization

43
Q

_____ compounds make good electrolytes becaue they dissolve the most readily

A

ionic

44
Q

_____ compounds are the weakest because they do not form current-carrying ions

A

nonpolar covalent compounds

45
Q

collision theory of chemcial kinetics

A

the rate of a reaction is proportional to the number of collisions per second between the reaacting molecules

46
Q

low activation energy and high temp make the negative exponnent of arrhenius equation ____ in magnitude and thus ____ the rate constant, k

A

smaller
increases

47
Q

factors affecting rxn rate

A

reactant conntrations
temp
medium
catalysts

48
Q

the greater the conc of the reactants, the ____ the number of effective collisions per unit time

A

greater
rxn rate will increase for all but zero order rxns

49
Q

homogenous and heterogenous catalysis

A

catalyst is in same phase as reactants

caalye is in distinct phase

50
Q

what are the only things that can change the rate of a zero order reaction?

A

temperature and addition of catalyst

51
Q

isothermal processes

adiabatic processes

isobaric

isovlumetric / isochoric

A

systems temp is constant

no heat is exchaged between syste and enviornment

pressure is contstant

no change in volume

52
Q

hess’ law states what

A

enthalpy changes of reactions are additive

53
Q

boyles law

A

pressure and volume inversely related

54
Q

charles’ law

A

volume and temperature are directly proportional

55
Q

the ______ of a gas will increase with increasing partial pressu reo fthe gas

A

solubility

56
Q

chelation

A

central cation can be bonded to the same ligand in multiple places

57
Q

_______ and ______ cells house spontaneous reactions, while _____ cells contain nonspontaneous reactions

A

galvanic

concentration

electrolytic

58
Q

purpose of salt bridge

A

exchange anions and cations to balance, or dissipate newly generated charges

59
Q

energy density in batteries

A

measure of a battery’s ability to produce power as a function of its weight

60
Q

isoelectric focusing

A

separate amino acids or polypeptides basedo n their isoelectric points

61
Q
A

MCAT (6 decks)

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