Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEMLec > LT2 > Flashcards

LT2 Flashcards

1
Q

what is the principal quantum number?

A

the usual energy level assigned in the Bohr model (n)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what is the quantum # also knows as?

A

the principal energy level or shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

on the periodic table, where can one find the principal quantum #?

A

the period

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

the sublevels or subshells of the principal energy level

A

angular momentum quantum number (l)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what does (l) correspond to?

A

the shape of the region of the most probable location of the electron (orbital)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

how do you determine (l)?

A

n-1, n-2, … 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what orbital block corresponds to which (l) and which shape?

A

S-(l)0-Spherical
P-(l)1-Dumbbell or bowtie
D-(l)2-4leaf clover
F-(l)3-Complex shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

also known as the orbital number

A

magnetic quantum number (ml)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what does the magnetic quantum number indicate?

A

the orientation of the orbital around the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

how do you determine the (ml)?

A

-(l) to +(l)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

the direction of the spin of an electron

A

spin quantum number (ms)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what does a spin up (ms) indicate?

A

+1/2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what does a spin down (ms) indicate?

A

-1/2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what do the 4 quantum numbers indicate?

A

the “address” an electron in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

principle that electrons must occupy the lowest energy orbital available first

A

aufbau principle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

principle that states that there must be a maximum of 2 electrons per orbital & each must have an opposite spin

A

pauli exclusion principle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

principle that states that electrons must occupy the orbitals in the same sublevel first before pairing up with the electrons in opposite spin

A

hund’s rule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

electron config. of Chronium (Cr)

A

[Ar]3d^5 4s^1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

electron config. of Copper (Cu)

A

[Ar]3d^10 4s^1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

electron config. of Molybdenum (Mo)

A

[Kr] 4d^5 5s^1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

electron config. of Palladium (Pd)

A

[Kr]4d^10 5s^0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

electron config. of Silver (Ag)

A

[Kr]4d^10 5s^1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

electron config. of Gold (Ag)

A

[Xe]4f^14 5d^10 6s^1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

what is periodicity?

A

the elements form a repeating pattern of chemical properties and reactivity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

what are periodic trends?

A

trends or patterns that are consequences of electron distribution; arise due to valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

trend in atomic size

A

increases down a group, increases right to left

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what are atomic size trends due to?

A

the energy level differences and the effective nuclear charge (Zeff)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

what is the Zeff?

A

the net charge experienced by a particular electron in a multielectron atom resulting from a balance of the attractive force of the nucleus and the repulsive forces of other electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

a cation ionic size is _ than the original atomic size

A

smaller (bc the atom adopts a positively-charged ion, it lost electrons and thus has less repulsion, thus less distance between the core electrons and the valence electrons, thus a smaller size)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

an anion ionic size is _ than the original atomic size

A

larger (bc the atom adopts a negatively-charged ion, it gains electrons and thus has more repulsion, thus more distance between the core electrons and the valence electrons, thus a bigger size)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

the energy required for the complete removal of an electron

A

ionization energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

why is ionization energy also known as cation formation?

A

bc the removal of an electron from a neautral-charged atom results in a positively-charged ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

atoms with low IE1 tend to form _ during reactions

A

cations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

atoms with high IE1 tend to form _ during chemical reactions

A

anions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

as size _, it takes more energy to remove an electron

A

decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

periodic trend that refers to the energy required to add an electron

A

electron affinity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

the relative ability of a bonded atom to attract shared electrons

A

electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

the most electronegative atom

A

fluorine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

periodic trend of electronegativity

A

increases up a group, L-R

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

electron affinity pertains to _ formation

A

anion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

the relative tendency to lose electrons = form cations

A

metallic behavior

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

what is the trend of metallic behavior?

A

increases down a group, R-L

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

elements at the _ of the metalloid staricase tend to form cations

A

left

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

elements at the _ of the metalloid staircase tend to form anions

A

right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

what are primary bonds?

A

bonds that are strong

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

what are the 3 types of primary bonds?

A

ionic, covalent, and metallic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

which primary bond refers to the transfer of electrons from one to another form a new compound?

A

ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

which kinds of elements interact in ionic bonding?

A

non-metal and metal

49
Q

in ionic bonding, which ion gives and which one takes

A

cation gives, anion takes

50
Q

primary bonding that refers to the sharing of electrons between atoms to form a new compound

A

covalent bonding

51
Q

which kinds of elements interact during covalent bonding?

A

non-metals

52
Q

the 3 properties of covalent bonds

A

bond order, energy/strength, length

53
Q

property of covalent bonds that refer to the number of electron pairs shared by two bonded atoms

A 
bond order
(single, double, triple)
54
Q

property of covalent bonds that refer to the energy required to overcome the mutual attraction between the bonded nuclei and the shared electrons

A

bond energy/strength

55
Q

endothermic process of bond energy/strength

A

bond breakage (requires heat input)

56
Q

exothermic process of bond energy/strength

A

bond formation (releases heat)

57
Q

property of covalent bonding that refers to the distance between nuclei of two bonded atoms

A

bond length

58
Q

what is the relationship between bond order, strength, and length?

A

high bond order = higher bond strength = lower distance (and vice versa)

59
Q

primary bond that refers to the attraction between metal ions and their delocalized VEs

A

metallic bonding

60
Q

true or false, VEs fo not belong to any one atom

A

true

61
Q

vacant _ and _ orbitals of the metals atoms’ outer energy levels overlap

A

p ; d

62
Q

term that refers to delocalized valence electrons

A

electron sea model

63
Q

who observed the octet rule?

A

Gilbert Newton Lewis

64
Q

what did Lewis observe?

A

when atoms bond, they lose, gain or share electrons to attain a filled outer level of eight electrons (in order to gain stability)

65
Q

with regard to the Lewis electron-dot symbol, for a metal, the _ _ _ _ is the maximum number of electrons and atom _ to form a _

A

total number of dots ; loses ; cation

66
Q

with regard to the Lewis electron-dot symbol, for a non-metal, the _ _ _ _ equals either the number of electrons an atoms gains in becoming an _ or the number it shares in forming _ _

A

number of unpaired dots ; anion ; covalent bonds

67
Q

2D structural formula consisting of electron dot symbols with lines as bonding pairs and dots as lone pairs

A

Lewis structures

68
Q

what is the Lewis structure also known as?

A

Lewis formula

69
Q

which atom should be placed at the center of the Lewis structure?

A

the one with the lowest electronegativity

70
Q

exceptions in Lewis structure

A 
max. bonds formed:
Hydrogen=1
Oxygen=2
Nitrogen=3
Carbon=4
(HONC)
71
Q

rules for halogens in Lewis structure

A

they can only form one bond when they are the surrounding atom

72
Q

Lewis structure rule for Fluorine

A

it is always a surrounding atom

73
Q

exceptions in the octet rule (max. VEs)

A 
Helium=2 (doublet)
Beryllium=4 (quartet)
Boron=6 (sextet)
(HeBeB) and 
atoms from pd greater than or equal to 3=hypervalent compounds (extended octet)
74
Q

what is m in AXmEn

A

of bonding electron group

75
Q

what is n in AXmEn

A

of lone pairs surrounding the central atom

76
Q

used to construct a 3D molecular shape

A

VSEPR theory

77
Q

ideal bond angle of linear shape

A

180

78
Q

ideal bond angle of trigonal planar

A

120

79
Q

ideal bond angle tetrahedral

A

109.5

80
Q

ideal bond angle of trigonal bipyramidal

A

equatorial=120 (horizontal), axial-equatorial (vertical)=90

81
Q

ideal bond angle of octahedral

A

90

82
Q

cause deviations from ideal bond angles

A

electron-pair repulsions

83
Q

electron-pair repulsions from least deviant to most

A

bonding pair-bonding pair, lone pair-bonding pair, lone pair-lone pair

84
Q

why do bonding pairs have the least deviation?

A

bc they are already localized

85
Q

bonding pair repulsions from least deviant to most

A

single bond, double bond, triple bond

86
Q

discovered electronegativity

A

Linus Pauling

87
Q

the uneven distribution of electrons in a bond due to different ENs

A

bond polarity

88
Q

this can help predict the type of bond formed

A

electronegativity difference

89
Q

when ^EN is greater than 1.7 the ionic character is?

A

mostly ionic

90
Q

when 0.4-1.7 the ionic character is?

A

polar covalent

91
Q

when ^EN is less than 0.4 the ionic character is?

A

mostly covalent

92
Q

when ^EN is 0 the ionic character is?

A

nonpolar covalent

93
Q

how do you know when a molecule is polar?

A

the electrons tend towards ONE of the atoms in a bond

94
Q

primary bonding are _ forces

A

intramolecular

95
Q

secondary bonding are _ forces

A

intermolecular

96
Q

why are secondary bonding weaker?

A

bc they typically involve smaller charges that are father apart

97
Q

IMFA that occurs when an ion and a nearby polar molecule attract each other

A

ion-dipole interaction

98
Q

IMFA that occurs between/among polar molecules; align themselves due to partial charges

A

dipole-dipole (ex. HCl molecules)

99
Q

IMFA special type of dipole-dipole bonding between H and F-O-N

A

hydrogen bonding

100
Q

IMFA dependent on the polarizability of the components; when an ion’s charge distorts the electron cloud of a nearby nonpolar molecule

A

ion-induced dipole forces

101
Q

IMFA arises when a polar molecule distorts the electron cloud of a nearby nonpolar molecule

A

dipole-induced dipole forces

102
Q

IMFA instantaneous dipole caused by momentary oscilations of electron charge in atoms

A

london dispersion forces

103
Q

london dispersion forces are dependent on the _ between molecules

A

distance

104
Q

true or false, london dispersion forces are only present for molecules

A

false, LDF is present in all molecules

105
Q

which molecule would have a higher boiling point, a short or a long one?

A

a long one, bc there’s more surface area

106
Q

relationship between polarizability and boiling point

A

directly proportional

107
Q

intermolecular forces that bind similar molecules to one another

A

cohesive forces

108
Q

intermolecular forces that bind a substance to a surface

A

adhesive forces

109
Q

the ability of a liquid to rise within a narrow tube due to cohesive and adhesive forces

A

capillary action

110
Q

stronger IMFA in the liquid = _ cohesive forces and _ meniscus

A

greater, convex (ex. Hg, remember sad face)

111
Q

stronger IMFA between the liquid and capillary = _ adhesive forces and _ meniscus

A

greater, concave (ex. H2O, remember smiley face)

112
Q

the energy required to break through the surface or disrupt a liquid drop and spread the material out as a film

A

surface tension

113
Q

stronger IMFA in the liquid= _ surface tension

A

higher

114
Q

the ease with which the electron cloud of a particle can be distorted

A

polarizability

115
Q

true or false, smaller atoms/ions are more polarizable than larger ones

A

less polarizable

116
Q

what is the trend for polarizability

A

increases down a group and R-L

117
Q

polarizability trend is fashioned after what other trend?

A

atomic size

118
Q

true or false, cations are less polarizable than their parent atoms because they are smaller

A

true

119
Q

true or false, anions are more polarizable because they are larger

A

true

CHEMLec (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions