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MCAT Chemistry > Atoms, Molecules, and Quantum Mechanics > Flashcards

Atoms, Molecules, and Quantum Mechanics Flashcards

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1
Q

atoms

A

nucleus surrounded by 1+ electrons

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2
Q

nucleus contains

A

protons and neutrons

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3
Q

charge and mass of atomic particles

A

proton: 1+ charge, ~ 1 amu
neutron: neutral charge, ~ 1 amu
electron: 1- charge, 5.5 x 10^-4 amu

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4
Q

elements

A

building blocks of compounds, can’t be broken down further

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5
Q

atomic notation

A

^A _Z X
A = mass number (protons + neutrons)
Z = atomic number, number of protons, defines the element

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6
Q

isotopes

A

same element with different number of neutrons, named by mass number

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7
Q

atomic weight/molar mass (MM or M)

A

in atomic mass units (amu) or u

one atom of 12C has atomic weight of 12 amu

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8
Q

mass from periodic table…

A

amu or g/mol

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9
Q

mole

A

6.022 x 10^23 of something = Avogadro’s #

moles = grams/molecular weight

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10
Q

6.022 X 10^23 amu =

A

1 gram

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11
Q

periodic table rows and columns

A

horizontal row = period

vertical column = group/family

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12
Q

metals ___ electrons

A

lose electrons –> positive ions or oxidation states

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13
Q

metal characteristics

A

lustrous, ductile (easily stretched), malleable (hammered into think strips), thermally and electrically conductive
all exist as solids at room temp except mercury

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14
Q

1st and 2nd group metals

A

1st group = alkali metals (most reactive)

2nd group = alkaline earth metals

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15
Q

nonmetals form…

A 
negative ions (gain electrons) 
generally lower melting points
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16
Q

last 2 groups of nonmetals

A

2nd to last = halogens

last group = noble gases (inert gases)

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17
Q

transition metal position in periodic table

A

the 10 shorter groups in middle

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18
Q

elements in the same family/group…

A

make same number of bonds, exist as similarly charged ions (except hydrogen)

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19
Q

cations

A

+ , metals

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20
Q

anions

A
  • , nonmetals
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21
Q

transition metals loss of e’s from…

A

s first, then d

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22
Q

electron shielding

A

first electrons shield some of nuclear charge from others –> Zeff

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23
Q

Zeff

A

effective nuclear charge, amount of charge felpt by electron after shielding

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24
Q

atomic radius periodic trend

A

increase from L bottom
atoms get smaller when add electrons
bigger as add new shell / move down a period

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25
Q

Zeff periodic trend

A

increases L –> R

each new electron closer and held more tightly to nucleus

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26
Q

ionization energy periodic trend

A

increases L –> R and bottom –> top

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27
Q

ionization energy

A

energy needed to detach e- from nucleus

second ionization energy - energy to remove 2nd e –> 2+ cation, always much greater than the first

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28
Q

electronegativity

A

tendency of an atom to attract the shared e’s
large electronegativity difference = ionic bonds
moderate difference = polar covalent
minor difference = nonpolar covalent

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29
Q

electronegativity periodic trend

A

increases L –> R and bottom –> top

undefined for noble gases (don’t make bonds)

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30
Q

electron affinity

A

willingness of atom to accept additional e, energy released when e is added

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31
Q

electron affinity periodic trend

A

increase L–R and bottom –> top
get more exothermic
noble gases of endothermic (don’t follow trend)

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32
Q

metallic character periodic trend

A

increase L bottom

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33
Q

SI units: mass, length, time

A

kg, m, s

34
Q

SI units: electric current, temp, luminous intensity

A

electric current: ampere, A
temp: K
luminous intensity: candela, cd

35
Q

newton units

A

kg*m/s^2

36
Q

prefixes: mega, kilo

A 
mega = M 10^6
kilo = k 10^3
37
Q

prefixes: deci, centi, milli

A 
deci = d 10^-1
centi = c 10^-2
milli = , 10^-3
38
Q

prefixes: micro, nano, pico, femto

A 
micro = mu 10^-6
nano = n 10^-9
pico = p 10^-12
femto = f 10^-15
39
Q

covalent bond

A

2 electrons shared by 2 nuclei

40
Q

bond length

A

point where the energy level is the lowest

2 atoms will only form bond if they can lower their overall energy level by doing so, nature seeks lowest energy state

41
Q

energy needed to ___ bond

A

break bonds (no energy released from breaking bond)

42
Q

bond dissociation energy / bond energy

A

energy to achieve complete separation

between energy at bond length and zero

43
Q

empirical formula

A

whole # ratio of relative number of atoms

ex: CH2O

44
Q

molecular formula

A

exact # of elements

ex: C6H12O6

45
Q

percent composition by mass

A

ex: of carbon in glucose

(mol. weight of carbon * ratio)/mol. weight of glucose

46
Q

empirical formula from mass composition

A

assume 100 g sample
ex: 6% H 94% O
6g/ 1g/mol = 6 moles
94g/16g/mol = 5.9 moles

47
Q

naming copper(I) and (II)

A 
(I) = cuprous 
(II) = cupric
48
Q

naming NO2- vs NO3-

A

hypo-ite
NO2- = nitrite
NO3- = nitrate
per-ate

49
Q

“runs to completion”

A

move to right until supply of at least 1 reactant is depleted
most reach equilibrium first and don’t run to completion

50
Q

find limiting reagent

A

use mole ratios to find how much of other reactant would be needed if other is used up
one will be not enough –> limiting reagent

51
Q

theoretical yield

A

amount of product when reaction runs to completion (calculated)

52
Q

percent yield

A

actual/theoretical x 100

53
Q

combination reaction

A

A +B –> C

54
Q

decomposition reaction

A

C –> A + B

55
Q

single displacement reaction

A

A + BC –> B + AC

56
Q

double displacement reaction

A

AB + CD –> AD + CB

57
Q

“delta” triangle above/below reaction arrow

A

heat is added

58
Q

“naught” circle symbol

A

standard state conditions

59
Q

quantum mechanics

A

elementary particles can only gain/lose energy and other quantities in discrete units

60
Q

quantum numbers

A

set of 4 numbers, the ID # of the electron

61
Q

Pauli exclusion principle

A

no 2 e’s in the same atom can have the same 4 quantum #s

62
Q

principle quantum number

A

n, shell level for electron, energy level

63
Q

azimuthal quantum number

A 
l, subshell shape 
l = 0 s
= 1 p
= 2 d
= 3 f
64
Q

magnetic quantum number

A

ml, precise orbital of given subshell

from -l –> +l

65
Q

electron spin quantum number

A

ms, distinguish the 2 e’s that may occupy same orbital +1/2 or -1/2

66
Q

number of total orbital in a shell

A

n^2

1,4,9,16… with 2 e’s in each orbital

67
Q

Heisenberg Uncertainty Principle

A

uncertainty in the product of position of particle and its momentum, on order of Plank’s constant
-more known about position, less about momentum

68
Q

Aufbau principle

A

each new e- added to lowest energy level available

69
Q

shell level of most recently added e- corresponds to…

A

period number

  • transition metals: one behind the period
  • lanthanides and actinides (2 period under table): 2 behind period
70
Q

subshell

A

orbital shape, 90% chance of finding the e- in shape

71
Q

s subshell shapes

A

circles, 1s smallest, get bigger as numbers increase

72
Q

p subshell shape

A

flower petal around axis

ex: 2px, 2py, 2pz

73
Q

valance electrons

A

outermost shell, contribute most to chemical properties

74
Q

electron configuration

A

list shells and subshells w/ superscript to show # of e-s
Na: 1s2, 2s2, 2p6, 3s1
Br: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p5

75
Q

abbreviated electron configuration

A

use next smallest noble gas

ex: [Ar] 4s2 3d10 4p5

76
Q

ground state

A

e- all in lowest energy level

77
Q

configurations for ions/atoms w/ excited e-s

A

+ charge, take away 1
- charge, add 1
total number of e- in configuration = total # in atom

78
Q

Hund’s rule

A

e’s wont fill any orbital in same subshell until all orbital s in that subshell contain at least 1 electron, unpaired e’s will have parallel spins

79
Q

Plank’s Quantum Theory

A

delta E = hf
if transfer energy via electromagnetic wave, increase energy w/out changing frequency, can only change in discrete increments, radiation must be emitted or received in energy packets

80
Q

photoelectric effect

A

kinetic energy of e’s increases only when frequency is increased

  • photon released when e- falls to lower energy shell
  • electron bumped up to excited state after absorbing a photon
  • electrons ejected by one-to-one photon-electron collisions

MCAT Chemistry (7 decks)

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