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MCAT > Gen Chemistry 1 (complete) > Flashcards

Gen Chemistry 1 (complete) Flashcards

1
Q

A student introduces a particle of unknown identity between two oppositely-charged electrodes and notes that it accelerates toward one of the two electrodes. The particle could be any of the following, EXCEPT a(n):
A) anion B) cation C) neutron D) proton
explain the answer

A

C neutron
in order for acceleration to happen there needs to be a charge, so the only one that would not have a charge would be a neutron

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2
Q

catalyst is?

A

any substance that increases reaction rate by decreasing activation energy

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3
Q

covalent bonds are formed between _____

A

nonmetals; they share electrons

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4
Q

explain what happens to energy when a bond is formed and broken

A

energy is required when you need to break a bond
energy is released when you need to form a bond

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5
Q

how do reactions caused by collisions work

A

reactants must collide with enough energy to overcome the activiation energy
reactants must be in the correct spatial orientation

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6
Q

in an anion, what is more; a proton or electron?

A

electron

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7
Q

ionic bonds are formed between ______

A

a metal and nonmetal

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8
Q

Keq=

A

([products]^x)/([reactants]^y)

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9
Q

Metals are (Larger/smaller) atoms with (loosely/tightly) held electrons
Nonmetals are (Larger/smaller) atoms with (loosely/tightly) held electrons

A

metals are larger atoms with loosely held electrons
nonmetals are smaller atoms with tightly held electrons

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10
Q

Metals form _____. Non metals form ______

A

cation; anion

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11
Q

Neutron + positron=

A

proton

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12
Q

Proton + Electron =

A

neutron

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13
Q

reaction quotient

A

Q>K, the reaction is left/reactants
Q<K, the reaction is right/products

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14
Q

types of decay
alpha decay
beta decay
electron capture
positron emission
gamma emission

A

alpha: loss of one He nucleus (z-2)
beta: neutron is changed into proton (z+1)
electron: proton is changed into neutron (z-1)
positron: proton is changed into neutron (SEPARATE FROM BETA DECAY) (neutron + positron)
gamma: the rays are emitted as a byproduct of the types of decay

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15
Q

what do collisions cause

A

reactions

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16
Q

what is an atom with fewer electrons that protons

A

cation

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17
Q

what is an isotope and do they have odd or even numbers?

A

multiple versions of the same atom, but they have a different amount of neutrons; they do not all have odd numbers, but many do

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18
Q

do isotopes have the same number of protons and neutrons

A

same number of protons but different number of neutrons

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19
Q

what is kinetics

A

study of reaction rate; aka how quickly the reaction proceeds

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20
Q

what is Le Chatelier’s Principle?

A

systems already at equilibrium, that experience change, will shift to the left or to the right to reduce the effects of that change and re-establish equilibrium

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21
Q

when it comes to heat of combustion, how does energy play a role in it?

A

the higher the energy (meaning it is less stable), the higher the heat of combustion

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22
Q

when it comes to size, is a cation bigger or smaller than the neutral counterpart? how about an anion?

A

Cations are smaller than their neutral counterpart and anions are larger than their neutral counterpart.

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23
Q

on the periodic table, how does electronegativity work? how about size

A

everything goes to F for electronegativity (the more right and up you, the higher the electronegativity)
the opposite for size (the more right and up you, the smaller the size)

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24
Q

what is the equation for the maximum number of electron in terms of n
how about the equation for maximum number of electrons in subshell

A

n=2n^2
4/+2

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25
Q

what is the work function

A

KE= E- ⌀
KE= kinetic energy of the electron
E= energy put into system (energy of photon)
⌀= energy required to release an electron from a metal surface (energy needed to eject a valence e-)

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26
Q

what is kinetic energy in terms of chemistry

A

excess energy of the system

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27
Q

bonding orbitals vs anti-bonding orbitals (in terms of energy and electron attractive or repulsion)

A

bonding: lower energy; electrons are in-phase and attractive
anti-bonding: higher energy; electrons are out of phase and repulsive

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28
Q

which are stronger: covalent or ionic?

A

covalent

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29
Q

what are electrolytes

A

ions that dissolve in solution that allow the solution to conduct electricity

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30
Q

what are considered good candidates for electrolytes?

A

strong acids/bases and compounds with a high ionic character make good electrolytes

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31
Q

ionic character

A

a measure of of the polarity between 2 atoms bonded together

32
Q

what is condosity

A

concentration of a sodium chloride solution that would conduct electricity exactly as well as the solution in question

33
Q

what is bond energy

A

average energy needed to break all the chemical bonds between two types of atoms in a molecule

34
Q

what is the difference between bond energy and bond dissociation energy

A

bond energy is energy contained within the bonds while the other is energy required to break bonds

35
Q

what is the equation of percent mass

A

(mass of target element/total molecular mass)x100

36
Q

molecular formula vs empirical formula

A

molecular: formula showing the atoms of a molecule. ex. C2H4O2
empirical: formula showing the most simplified form of a molecule. ex. C2H4O2—> CH2O

37
Q

formula of hydroxide

A

-OH

38
Q

formula of nitrate

A

NO3-

39
Q

formula of nitrite

A

NO2-

40
Q

formula of chlorate

A

ClO3-

41
Q

formula of chlorite

A

ClO2-

42
Q

formula of hypochlorite

A

ClO-

43
Q

formula of perchlorate

A

ClO4-

44
Q

formula of carbonate

A

CO3-

45
Q

formula of bicarbonate

A

HCO3-

46
Q

formula of ammonium

A

NH4+

47
Q

formula of sulfate

A

SO2 2-

48
Q

formula of phosphate

A

PO4 3-

49
Q

formula of manganite

A

MnO(OH)

50
Q

formula of permanganate

A

KMnO4-

51
Q

formula of cyanide

A

CN-

52
Q

single displacement formula

A

AB+C <=> A+BC

53
Q

double displacement formula

A

AB+CD<=>AC+BD

54
Q

combination formula

A

A+B <=> AB

55
Q

decomposition formula

A

AB<=>A+B

56
Q

how do you find the limiting reagent

A

convert everything to moles. make sure the equation is balanced, then the reagent with the smallest molar amount is the limiting reagent

57
Q

what is the theoretical yield

A

amount of product that would be created under ideal conditions

58
Q

what is the actual yield

A

amount of product actually create. it can be less than theoretical yield due to inefficiencies

59
Q

what is the percent yield formula

A

(actual over theoretical)x100

60
Q

according to Le Chatelier’s, how do you increase the yield

A

start with more reactants
remove products as they are formed

61
Q

what is the law of mass action

A

Keq= [products]^x/[reactants]^y

62
Q

if Keq > 1, the reaction is (spontaneous/non-spontaneous), which means…

A

it is spontaneous, which means that at equilibrium there will be more products than reactants

63
Q

if Keq < 1, the reaction is (spontaneous/non-spontaneous), which means…

A

it is non-spontaneous, which means that equilibrium there will be more reactants than products

64
Q

true or false: Keq can only be calculated at equilibrium

A

true

65
Q

what is Q

A

any point or ratio where the products and reactants are not at equilibrium

66
Q

Q > K means…
think in terms of if the reaction goes right or left

A

more products than at equilibrium so reaction will go to the left

67
Q

Q < K means…
think in terms of if the reaction goes right or left

A

more reactants than at equilibrium so reaction will go the right

68
Q

what is the difference between kinetics and thermodynamics
in terms of speed and stability

A

kinetics: speed at which a reaction occurs; does NOT take into account how stable the product is
thermodynamics: stability of reactants and products; does NOT take into account the speed of the reaction

69
Q

what are two things that need to happen in order for a reaction to occur

A
  1. collide with enough energy to overcome the energy of activation
  2. be in the right spatial orientation
70
Q

when it comes to rate order graphs, what happens in the 0th order

A

negative slope; [A] vs time is linear

71
Q

when it comes to rate order graphs, what happens in the 1st order

A

negative slope; ln[A] vs time is linear

72
Q

when it comes to rate order graphs, what happens in the 2nd order

A

positive slope; 1/[A] vs time is linear

73
Q

when writing a rate law, what determines the rate

A

the slow step because when there is a slow step, the speed of the fast step is negligible

74
Q

fast reactions have (large/small) rate constants
slow reactions have (large/small) rate constants

A

fast: large
slow: small

75
Q

what are the units of the 0th order reaction

A

mol/(LxS)

76
Q

what are the units of the 1st order reaction

A

1/s or s^-1

77
Q

what are the units of 2nd order reaction

A

L/(mol x s)

MCAT (13 decks)

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