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

Atoms, Molecules, and Quantum Mechanics Flashcards

(80 cards)

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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
Zeff periodic trend
increases L --> R | each new electron closer and held more tightly to nucleus
26
ionization energy periodic trend
increases L --> R and bottom --> top
27
ionization energy
energy needed to detach e- from nucleus | second ionization energy - energy to remove 2nd e --> 2+ cation, always much greater than the first
28
electronegativity
tendency of an atom to attract the shared e's large electronegativity difference = ionic bonds moderate difference = polar covalent minor difference = nonpolar covalent
29
electronegativity periodic trend
increases L --> R and bottom --> top | undefined for noble gases (don't make bonds)
30
electron affinity
willingness of atom to accept additional e, energy released when e is added
31
electron affinity periodic trend
increase L--R and bottom --> top get more exothermic noble gases of endothermic (don't follow trend)
32
metallic character periodic trend
increase L bottom
33
SI units: mass, length, time
kg, m, s
34
SI units: electric current, temp, luminous intensity
electric current: ampere, A temp: K luminous intensity: candela, cd
35
newton units
kg*m/s^2
36
prefixes: mega, kilo
``` mega = M 10^6 kilo = k 10^3 ```
37
prefixes: deci, centi, milli
``` deci = d 10^-1 centi = c 10^-2 milli = , 10^-3 ```
38
prefixes: micro, nano, pico, femto
``` micro = mu 10^-6 nano = n 10^-9 pico = p 10^-12 femto = f 10^-15 ```
39
covalent bond
2 electrons shared by 2 nuclei
40
bond length
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
energy needed to ___ bond
break bonds (no energy released from breaking bond)
42
bond dissociation energy / bond energy
energy to achieve complete separation | between energy at bond length and zero
43
empirical formula
whole # ratio of relative number of atoms | ex: CH2O
44
molecular formula
exact # of elements | ex: C6H12O6
45
percent composition by mass
ex: of carbon in glucose | (mol. weight of carbon * ratio)/mol. weight of glucose
46
empirical formula from mass composition
assume 100 g sample ex: 6% H 94% O 6g/ 1g/mol = 6 moles 94g/16g/mol = 5.9 moles
47
naming copper(I) and (II)
``` (I) = cuprous (II) = cupric ```
48
naming NO2- vs NO3-
hypo-ite NO2- = nitrite NO3- = nitrate per-ate
49
"runs to completion"
move to right until supply of at least 1 reactant is depleted most reach equilibrium first and don't run to completion
50
find limiting reagent
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
theoretical yield
amount of product when reaction runs to completion (calculated)
52
percent yield
actual/theoretical x 100
53
combination reaction
A +B --> C
54
decomposition reaction
C --> A + B
55
single displacement reaction
A + BC --> B + AC
56
double displacement reaction
AB + CD --> AD + CB
57
"delta" triangle above/below reaction arrow
heat is added
58
"naught" circle symbol
standard state conditions
59
quantum mechanics
elementary particles can only gain/lose energy and other quantities in discrete units
60
quantum numbers
set of 4 numbers, the ID # of the electron
61
Pauli exclusion principle
no 2 e's in the same atom can have the same 4 quantum #s
62
principle quantum number
n, shell level for electron, energy level
63
azimuthal quantum number
``` l, subshell shape l = 0 s = 1 p = 2 d = 3 f ```
64
magnetic quantum number
ml, precise orbital of given subshell | from -l --> +l
65
electron spin quantum number
ms, distinguish the 2 e's that may occupy same orbital +1/2 or -1/2
66
number of total orbital in a shell
n^2 | 1,4,9,16... with 2 e's in each orbital
67
Heisenberg Uncertainty Principle
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
Aufbau principle
each new e- added to lowest energy level available
69
shell level of most recently added e- corresponds to...
period number - transition metals: one behind the period - lanthanides and actinides (2 period under table): 2 behind period
70
subshell
orbital shape, 90% chance of finding the e- in shape
71
s subshell shapes
circles, 1s smallest, get bigger as numbers increase
72
p subshell shape
flower petal around axis | ex: 2px, 2py, 2pz
73
valance electrons
outermost shell, contribute most to chemical properties
74
electron configuration
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
abbreviated electron configuration
use next smallest noble gas | ex: [Ar] 4s2 3d10 4p5
76
ground state
e- all in lowest energy level
77
configurations for ions/atoms w/ excited e-s
+ charge, take away 1 - charge, add 1 total number of e- in configuration = total # in atom
78
Hund's rule
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
Plank's Quantum Theory
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
photoelectric effect
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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