LT2 Flashcards
(119 cards)
1
Q
what is the principal quantum number?
A
the usual energy level assigned in the Bohr model (n)
2
Q
what is the quantum # also knows as?
A
the principal energy level or shell
3
Q
on the periodic table, where can one find the principal quantum #?
A
the period
4
Q
the sublevels or subshells of the principal energy level
A
angular momentum quantum number (l)
5
Q
what does (l) correspond to?
A
the shape of the region of the most probable location of the electron (orbital)
6
Q
how do you determine (l)?
A
n-1, n-2, … 0
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
8
Q
also known as the orbital number
A
magnetic quantum number (ml)
9
Q
what does the magnetic quantum number indicate?
A
the orientation of the orbital around the nucleus
10
Q
how do you determine the (ml)?
A
-(l) to +(l)
11
Q
the direction of the spin of an electron
A
spin quantum number (ms)
12
Q
what does a spin up (ms) indicate?
A
+1/2
13
Q
what does a spin down (ms) indicate?
A
-1/2
14
Q
what do the 4 quantum numbers indicate?
A
the “address” an electron in an atom
15
Q
principle that electrons must occupy the lowest energy orbital available first
A
aufbau principle
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
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
18
Q
electron config. of Chronium (Cr)
A
[Ar]3d^5 4s^1
19
Q
electron config. of Copper (Cu)
A
[Ar]3d^10 4s^1
20
Q
electron config. of Molybdenum (Mo)
A
[Kr] 4d^5 5s^1
21
Q
electron config. of Palladium (Pd)
A
[Kr]4d^10 5s^0
22
Q
electron config. of Silver (Ag)
A
[Kr]4d^10 5s^1
23
Q
electron config. of Gold (Ag)
A
[Xe]4f^14 5d^10 6s^1
24
Q
what is periodicity?
A
the elements form a repeating pattern of chemical properties and reactivity
25
what are periodic trends?
trends or patterns that are consequences of electron distribution; arise due to valence electrons
26
trend in atomic size
increases down a group, increases right to left
27
what are atomic size trends due to?
the energy level differences and the effective nuclear charge (Zeff)
28
what is the Zeff?
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
29
a cation ionic size is _ than the original atomic size
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)
30
an anion ionic size is _ than the original atomic size
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)
31
the energy required for the complete removal of an electron
ionization energy
32
why is ionization energy also known as cation formation?
bc the removal of an electron from a neautral-charged atom results in a positively-charged ion
33
atoms with low IE1 tend to form _ during reactions
cations
34
atoms with high IE1 tend to form _ during chemical reactions
anions
35
as size _, it takes more energy to remove an electron
decreases
36
periodic trend that refers to the energy required to add an electron
electron affinity
37
the relative ability of a bonded atom to attract shared electrons
electronegativity
38
the most electronegative atom
fluorine
39
periodic trend of electronegativity
increases up a group, L-R
40
electron affinity pertains to _ formation
anion
41
the relative tendency to lose electrons = form cations
metallic behavior
42
what is the trend of metallic behavior?
increases down a group, R-L
43
elements at the _ of the metalloid staricase tend to form cations
left
44
elements at the _ of the metalloid staircase tend to form anions
right
45
what are primary bonds?
bonds that are strong
46
what are the 3 types of primary bonds?
ionic, covalent, and metallic
47
which primary bond refers to the transfer of electrons from one to another form a new compound?
ionic
48
which kinds of elements interact in ionic bonding?
non-metal and metal
49
in ionic bonding, which ion gives and which one takes
cation gives, anion takes
50
primary bonding that refers to the sharing of electrons between atoms to form a new compound
covalent bonding
51
which kinds of elements interact during covalent bonding?
non-metals
52
the 3 properties of covalent bonds
bond order, energy/strength, length
53
property of covalent bonds that refer to the number of electron pairs shared by two bonded atoms
```
bond order
(single, double, triple)
```
54
property of covalent bonds that refer to the energy required to overcome the mutual attraction between the bonded nuclei and the shared electrons
bond energy/strength
55
endothermic process of bond energy/strength
bond breakage (requires heat input)
56
exothermic process of bond energy/strength
bond formation (releases heat)
57
property of covalent bonding that refers to the distance between nuclei of two bonded atoms
bond length
58
what is the relationship between bond order, strength, and length?
high bond order = higher bond strength = lower distance (and vice versa)
59
primary bond that refers to the attraction between metal ions and their delocalized VEs
metallic bonding
60
true or false, VEs fo not belong to any one atom
true
61
vacant _ and _ orbitals of the metals atoms' outer energy levels overlap
p ; d
62
term that refers to delocalized valence electrons
electron sea model
63
who observed the octet rule?
Gilbert Newton Lewis
64
what did Lewis observe?
when atoms bond, they lose, gain or share electrons to attain a filled outer level of eight electrons (in order to gain stability)
65
with regard to the Lewis electron-dot symbol, for a metal, the _ _ _ _ is the maximum number of electrons and atom _ to form a _
total number of dots ; loses ; cation
66
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 _ _
number of unpaired dots ; anion ; covalent bonds
67
2D structural formula consisting of electron dot symbols with lines as bonding pairs and dots as lone pairs
Lewis structures
68
what is the Lewis structure also known as?
Lewis formula
69
which atom should be placed at the center of the Lewis structure?
the one with the lowest electronegativity
70
exceptions in Lewis structure
```
max. bonds formed:
Hydrogen=1
Oxygen=2
Nitrogen=3
Carbon=4
(HONC)
```
71
rules for halogens in Lewis structure
they can only form one bond when they are the surrounding atom
72
Lewis structure rule for Fluorine
it is always a surrounding atom
73
exceptions in the octet rule (max. VEs)
```
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
what is m in AXmEn
of bonding electron group
75
what is n in AXmEn
of lone pairs surrounding the central atom
76
used to construct a 3D molecular shape
VSEPR theory
77
ideal bond angle of linear shape
180
78
ideal bond angle of trigonal planar
120
79
ideal bond angle tetrahedral
109.5
80
ideal bond angle of trigonal bipyramidal
equatorial=120 (horizontal), axial-equatorial (vertical)=90
81
ideal bond angle of octahedral
90
82
cause deviations from ideal bond angles
electron-pair repulsions
83
electron-pair repulsions from least deviant to most
bonding pair-bonding pair, lone pair-bonding pair, lone pair-lone pair
84
why do bonding pairs have the least deviation?
bc they are already localized
85
bonding pair repulsions from least deviant to most
single bond, double bond, triple bond
86
discovered electronegativity
Linus Pauling
87
the uneven distribution of electrons in a bond due to different ENs
bond polarity
88
this can help predict the type of bond formed
electronegativity difference
89
when ^EN is greater than 1.7 the ionic character is?
mostly ionic
90
when 0.4-1.7 the ionic character is?
polar covalent
91
when ^EN is less than 0.4 the ionic character is?
mostly covalent
92
when ^EN is 0 the ionic character is?
nonpolar covalent
93
how do you know when a molecule is polar?
the electrons tend towards ONE of the atoms in a bond
94
primary bonding are _ forces
intramolecular
95
secondary bonding are _ forces
intermolecular
96
why are secondary bonding weaker?
bc they typically involve smaller charges that are father apart
97
IMFA that occurs when an ion and a nearby polar molecule attract each other
ion-dipole interaction
98
IMFA that occurs between/among polar molecules; align themselves due to partial charges
dipole-dipole (ex. HCl molecules)
99
IMFA special type of dipole-dipole bonding between H and F-O-N
hydrogen bonding
100
IMFA dependent on the polarizability of the components; when an ion's charge distorts the electron cloud of a nearby nonpolar molecule
ion-induced dipole forces
101
IMFA arises when a polar molecule distorts the electron cloud of a nearby nonpolar molecule
dipole-induced dipole forces
102
IMFA instantaneous dipole caused by momentary oscilations of electron charge in atoms
london dispersion forces
103
london dispersion forces are dependent on the _ between molecules
distance
104
true or false, london dispersion forces are only present for molecules
false, LDF is present in all molecules
105
which molecule would have a higher boiling point, a short or a long one?
a long one, bc there's more surface area
106
relationship between polarizability and boiling point
directly proportional
107
intermolecular forces that bind similar molecules to one another
cohesive forces
108
intermolecular forces that bind a substance to a surface
adhesive forces
109
the ability of a liquid to rise within a narrow tube due to cohesive and adhesive forces
capillary action
110
stronger IMFA in the liquid = _ cohesive forces and _ meniscus
greater, convex (ex. Hg, remember sad face)
111
stronger IMFA between the liquid and capillary = _ adhesive forces and _ meniscus
greater, concave (ex. H2O, remember smiley face)
112
the energy required to break through the surface or disrupt a liquid drop and spread the material out as a film
surface tension
113
stronger IMFA in the liquid= _ surface tension
higher
114
the ease with which the electron cloud of a particle can be distorted
polarizability
115
true or false, smaller atoms/ions are more polarizable than larger ones
less polarizable
116
what is the trend for polarizability
increases down a group and R-L
117
polarizability trend is fashioned after what other trend?
atomic size
118
true or false, cations are less polarizable than their parent atoms because they are smaller
true
119
true or false, anions are more polarizable because they are larger
true
