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MCAT chem > atomic trends and bonding/ IMF > Flashcards

atomic trends and bonding/ IMF Flashcards

1
Q

what is all matter composed of?

A

atoms

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2
Q

what is a molecule?

A

when two or more atoms are combined

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3
Q

what is a compound

A

when two or more molecules are combined

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4
Q

proton charge and weight

A

at center of atom, weigh 1 amu and have 1+ charge
1.6E-19 eV

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5
Q

electron weight and charge

A

in electron clouds, -1 or -1.6E-19

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6
Q

neutron weight

A

1 amu (same as proton_

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7
Q

atomic number (z)

A

identifies element, number of protons

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8
Q

mass number

A

P + N

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9
Q

isotopes

A

same atomic number but differnt number of neutrons

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10
Q

atomic mass

A

N+P

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11
Q

automic weight

A

average of all isotopic automic masses

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12
Q

polyatomic ions

A

contain multiple atoms with different ionic forms

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13
Q

oxyanions

A

polyatomics that contain oxygen and have suffix ite or ate

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14
Q

bohr model

A

outdated but explains how electrons exsist in clouds outside the nucleus in shells

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15
Q

ground state

A

lowest energy level of an electron n=1,2,3… and can jump to higher energy levels

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16
Q

photons

A

discrete amounts of energy that are emitted as electrons jump to excited states

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17
Q

energy of electromagnetic ratiation equation

A

E= hf where h is planks constant and f is the frequency of light (which is the speed of light divided by wave length)
E= h*c/ wavelength

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18
Q

rydberg formula
used to determine the energy held by an electron in a certain energy level

A

change in Energy = R (1/nf^2 - 1/ni^2)
r is constant

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19
Q

Heisenberg principle of uncertainty

A

cannot know the momentum and exact position of an electron at the same time

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20
Q

principle quantum number

A

electrons exist in orbitals
denoted as “n” and can be 1 or greater, higher n = higher energy and farther from the nucleus
- associated with rows of the periodic table

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21
Q

orbital

A

area of space that electrons are likely to be in, can only hold two electrons at a time

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22
Q

pauli exclusion principle

A

no two electrons in an atom can have the exact same values for all 4 quantum numbers

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23
Q

azimuthal/angular momentum quantum number

A

describes the subshell
s,p,d,f

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24
Q

magnetic quantum number

A

describes the spacial orientation of the orbital within its subshell ranging from + and - L. L=0 for s, L=1 for p, L=2 for d L= 3

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25
Q

spin quantum number

A

describes the spin orientation of the electron either +1/2 or -1/2. all electrons are paired with opposite spin

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26
Q

electron configuration

A

configuration of electrons in subshells , follow aufbau principle and lower energy levels fill first

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27
Q

hunds rule

A

electrons prefer to be in orbitals by themselves and will fill each orbital with 1 electron before sharing

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28
Q

where is the s block

A

the first 2 groups

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29
Q

where is the p block

A

groups 13-18

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30
Q

where is the d block

A

transition metals

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31
Q

where is the f block

A

lanthanide and actinide series at the bottom of the periodic table

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32
Q

valence electrons

A

outermost electrons that are involved in chemical bonds

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33
Q

which is a lower energy? 3d or 4s

A

4s so it fills before 3d (according to aufbau principle)

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34
Q

true or false: half filled and full filled orbitals are more stable than ones with 3/4/ or 9 electrons

A

true! the p and d will steal from s orbital

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35
Q

alkali metals

A

group 1: high conductivity, luster, duct-ability (drawn into thin wire) , malleability, reactivity, reactive

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36
Q

alkaline earth metal

A

group 2: harder and less reactive than alkali metals, good conductors

37
Q

transition metals

A

groups 3-12. luster, hard, conduct electricity

38
Q

nonmetals

A

not shiny, poor electricity conductors

39
Q

chalcogens

A

group 16, feature O and S

40
Q

halogens

A

group 17, highly reactive

41
Q

noble gases

A

group 18, very stable. inert gases. low boiling points

42
Q

effective nuclear charge

A

the attraction between the positively charged center of an atom and the electrons surrounding it. decreases down a group and increases to the right. increases with increased number of protons

43
Q

atomic radius trend

A

increases down a group and to the left

44
Q

ionic radius

A

cations are smaller than anions

45
Q

ionization energy

A

the amount of energy required for an atom to give up an electron. increases across a period and up a group

46
Q

electron affinity

A

the amount of energy released when an electron is added to an atom. increases up a group and to the right.

47
Q

electronegativity

A

tendency of an atom to attract electrons, directly in correlation with effective nuclear charge

48
Q

how many molecules are in one mole?

A

6.02E23 molecules

49
Q

octet rule

A

each atom will act in a way that allows it to obtain 8 electrons in its valence shell for stability.

50
Q

is bond formation typically endothermic or exothermic?

A

it is stable and releases energy so it is exothermic

51
Q

incomplete octet

A

special case for hydrogen where it is a filled valence shell with a single bond H-H
others: Boron - 6
he- 2 li-2 be - 4

52
Q

expanded octet

A

atom has more than 8 valence electrons. in case of PF5 there are 10

53
Q

what is unique about octets in the third period?

A

they readily form expanded octets

54
Q

intramolecular forces (definition and types)

A

forces that work inside a molecule to keep it together
ionic and covalent bonds

55
Q

ionic bonds

A

form between a metal and a nonmetal, the two species have a large difference in ELECTRONEGATIVITY. form cations and anions

56
Q

pauling scale

A

assigns electronegativity values.
fluorine is the most eneg @ 4.0 and the alkali metals have an eneg of around 1.0
** ionic bonds form when the difference in electronegativity between two atoms is 1.7 or greater

57
Q

covalent bonding

A

sharing of electrons among nonmetals
- can be equal or unequal sharing
- the difference in electronegativity between the two atoms is small

58
Q

nonpolar covalent bonds

A

when electronegativity between atoms sharing electrons are similar or the same and they share electrons equally
- <.5

59
Q

polar covalent bonds

A

occur when difference in electronegativity is between .5 and 1.7 and electrons are shared unequally, with the more electronegative atom recieving more electrons and causing dipole moments

60
Q

dipole moments

A

unequally sharing of electrons causes partial positive charges on less electronegative atoms pointing toward the more electronegative atom with a partial negative

61
Q

coordinate covalent bond

A

when shared electrons are derived from a lone pair of one atom

62
Q

bond order

A

number of bonds between two atoms
single, double, triple

63
Q

sigma bond

A

forms due to end to end overlap of two atomic orbitals
a single bond forms 1 sigma bond

64
Q

pi bond

A

forms when atomic orbitals point above and below the atoms making them parallel.
a double bond contains a pi and a sigma

65
Q

bond length

A

inversely related to bond order. single bonds are the longest and triple bonds are the shortest

66
Q

bond energy

A

energy required to break a covalent bond. the higher the bond energy, the stronger the bond
- increases with bond order

67
Q

metallic bonding

A

an intramolecular force less common than ionic and covalent. occurs when metal atoms are joined together and electrons become delocalized in a sea of electrons that freely move through a solid and allows for electrical conduction and heat

68
Q

intermolecular forces

A

attractive forces between molecules that are notably WEAKER than intramolecular forces and can be broken with heat . bonds driven by charge
types: london, dipole, hydrogen, ion-dipole
- stronger polarity = stronger intermolecular forces
- determine behavior and melt/boiling points

69
Q

london-dispersion forces

A

weakest intermolecular force caused by random dipole moments, fluctuations in polar and nonpolar bonds
- larger compounds are more likely to experience london dispersion forces

70
Q

dipole-dipole interactions

A

intermolecular force that is stronger than london dispersion. dipoles are stable (polar bonds only)

71
Q

hydrogen bonding

A

between a hydrogen bound to F, O, N and a lone pair on another F, O, or N

72
Q

ion-diple forces

A

strongest intermolecular force. ions are most polar and occur when two molecules have charge
ex: peptide hormone signalling with a basic aminoacid

73
Q

lewis structure

A

establish relationships between atoms and their valence electrons
- valence electrons = group number (except transition metals)
- atom with lowest electronegativity goes in the middle

74
Q

resonance structures

A

compounds with lone pairs that can move bonds to different positions
- can only shift lone pairs and double bonds, never single bonds
- delocalization of electrons increases stability of structure

75
Q

formal charge

A

disparity between the number of valence electrons an atom has and the electrons it actually has.
formal charge = VE - bonds - lone pair electrons

76
Q

orbital hybridization

A

mixing atomic orbitals to form hybrid orbitals

77
Q

what does a triple bond consist of

A

2 pi and 1 sigma bond

78
Q

two regions of hybridization (triple bond) yields what?

A

sp

79
Q

three regions of hybridization (double bond) yields what?

A

sp2

80
Q

4 regions of hybridization (single bond) yields what?

A

sp3

81
Q

VSPER theory

A

uses lewis structures to determine shapes of molecules due to electron repulsion
- use number of lone pairs and bonded atoms to predict bond angle and shape

82
Q

electronic geometry

A

takes into account lone pairs and bonded atoms to predict shape

83
Q

molecular geometry

A

only takes into account boned atoms when predicting shape

84
Q

tetrahedral molecular shape

A

4 electron rich regions and 4 bonded atoms
- CH4
- bond angle is 109.5

85
Q

trigonal pyrimidal molecular shape

A

4 regions of electron rich. 3 bonded atoms and 1 lone pair
- bond angle is 107
nh3

86
Q

bent molecular shape

A

2 bonds and 2 lone pairs, bond angle is 104
ex: h2o

87
Q

linear molecular shape

A

2 bonds no lone pairs, bond angle is 180

88
Q

trigonal planar molecular shape

A

3 bonds no lone pairs, bond angle 120
ex bf3

MCAT chem (11 decks)

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