Units 9 And 10 Flashcards
(113 cards)
1
Q
2 electrons = electron pair geometry of
A
Linear
2
Q
3 electrons = electron pair geometry of
A
Trigonal planar
3
Q
4 electrons = electron pair geometry of
A
Tetrahedral
4
Q
5 electrons = electron pair geometry of
A
Trigonal bipyramidal
5
Q
6 electrons = electron pair geometry of
A
Octahedral
6
Q
Linear
A
2 electrons = electron pair geometry of
7
Q
Trigonal planar
A
3 electrons = electron pair geometry of
8
Q
Tetrahedral
A
4 electrons = electron pair geometry of
9
Q
Trigonal bipyramidal
A
5 electrons = electron pair geometry of
10
Q
Octahedral
A
6 electrons = electron pair geometry of
11
Q
Linear with no lone pairs molecular geometry
A
Linear
12
Q
Trigonal planar with no lone pairs
A
Trigonal planar
13
Q
Trigonal planar with 1 lone pairs
A
Bent
14
Q
Tetrahedral with no lone pairs
A
Tetrahedral
15
Q
Tetrahedral with one lone pair
A
Trigonal pyramidal
16
Q
Tetrahedral with 2 lone pairs
A
Bent
17
Q
Trigonal bipyramidal with 1 lone pair
A
See-saw
18
Q
Trigonal bipyrmidal with 2 lone pairs
A
T shaped
19
Q
Trigonal bipyramidal with 3 lone pairs
A
Linear
20
Q
Octahedral with no lone pairs
A
Octahedral
21
Q
Octahedral with 1 lone pair
A
Square pyramidal
22
Q
Octahedral with 2 lone pairs
A
Square planar
23
Q
Octahedral with 3 lone pairs
A
T shaped
24
Q
Octahedral with 4 lone pairs
A
Iinear
25
Transfer one or more electrons from one to another to form ions
Ionic
26
Electrons are shared between atoms
Covalent
27
Energy change occurring when separated ions are packed together to form a crystalline solid
Lattice energy
28
Based on Coulomb's law, which of the following is predicted to have a larger lattice energy?
LiF
29
Does MgO have a larger Latrice than NaCl?
Yes
30
Molecule formed by covalent bonds
Covalent compound
31
A 2D representation of bonding and non bonding electrons a molecule or polyatomic ion
Lewis structure
32
An electron pair found in the space between atoms
Bonding pair
33
An electron pair localized on a given atom
Lone pair
34
Valence electrons equal
Group Number
35
A condition occurring when a Lewis structure can be drawn for a particular ion
Resonance
36
Has fewer than 8 electrons
BF3
37
Has more than 8 electrons
SF6
38
Formal charge
Group # - (# lp + 1/2 bonding)
39
The best Lewis structure is the
One that minimizes formal charge
40
The octet rule usually occurs with
Boron and elements of higher periods (3 and up)
41
Linear geometry angle
180
42
Example of linear geometry
BeF2
43
Example of trigonal planar
BF3
44
Trigonal planar angle
120
45
Tetrahedral example
CF4
46
Tetrahedral angle
109.5
47
Trigonal bipyramidal example
PF5
48
Trigonal bipyramidal angle
120 and 90
49
Octahedral example
SF6
50
Octahedral angle
90
51
H2O is
Bent
52
Repulsive forces decrease in the following order
Lp vs lp greater then lp vs bonding greater than bonding vs bonding
53
Electrons are not shared equally, one atom attracts them more strongly than the other
Polar covalent bond
54
Electrons shared equally
No polar covalent bond
55
Example for ionic bond
NaCl
56
Example for covalent bond
HCl
57
Example for no polar covalent bond
Cl2
58
Ionic character of bond decreases from (blank) to (blank)
Ionic to nonpolar
59
The tendency of an atom in a molecule to attract density to itself
Electronegativity
60
Who came up with electronegativity
Linus Pauling
61
The greater the electronegativity difference between 2 atoms in a bond, the (blank) the polarity
Greater
62
Which element has the highest electronegativity
F 4.0
63
Covalent usually has a electronegativity difference of
0-0.3
64
Polar covalent usually has a electronegativity difference of
0.4-2.0
65
Ionic usually has a electronegativity difference of
2.1-4
66
of bonds between atoms
Bond order
67
Distance between the nuclei of two bonded atoms
Bond length
68
1 pair of electrons shared = bond order of
Single: 1
69
2 pair of electrons shared = bond order of
Double: 2
70
3 pairs of electrons shared = bond order of
Triple: 3
71
Energy required to break a chemical bond
Bond energy
72
Bond enthalpies are always
Positive
73
Energy of reaction equation
Sum of bond energy of bonds broken - sum of bond energy of bonds formed
74
Based on their Lewis structure which molecule has the longest carbon oxygen bond? Carbon dioxide and carbon monoxide
Carbon dioxide
75
Order bond number from shorter to longest bond
Triple, double, single
76
Bond length (blank) as the # of shared electrons increases
Shortens
77
Single bond has the (blank) bond length
Longest
78
Double bond has the (blank) bond length
Middle
79
Triple bond has the (blank) bond length
Shortest
80
Single bond has the (blank) bond energy
Lowest
81
Double bond has the (blank) bond energy
Middle
82
Triple bond has the (blank) bond energy
Highest
83
Bonds formed from the overlap of atomic orbitals
Valence bond theory
84
3 factors affect the overall energy of molecule
- Electron nuclei attraction
- nuclei nuclei repulsion
- electron electron repulsion
85
When 2 orbitals share a common region of space
Overlap
86
Covalent bond formed by overlapping end to end
Sigma bond
87
In a sigma bond, electron density is concentrated between the (blank) of the bonded atoms
Nuclei
88
Triple bonds are (blank) than single bonds
Shorter and stronger
89
Mixing or atomic orbitals to form special (hybrid) orbitals for bonding
Hybridization
90
Form new set of orbitals and give max overlap in correct geometry
Orbital hybridization
91
2 effective electron pairs
| Hybridization =
Sp
92
3 effective electron pairs
| Hybridization =
Sp2
93
4 effective electron pairs
| Hybridization =
Sp3
94
5 effective electron pairs
| Hybridization =
Sp3d
95
6 effective electron pairs
| Hybridization =
Sp3d2
96
Sp3 hybridization =
1s orbital and 3 p orbitals
97
Double bond in ethylene consists of (blank) sigma bond and (blank) pi bond
1, 2
98
Determining bond order from molecular theory- hydrogen2 =
1
99
Determining bond order from molecular theory- helium2 =
0
100
Greater the (blank), the stronger and more stable the molecule
Bond order
101
Sp3 consists of
One S, 3 p
102
Sp2 consists of
One s, 2 p
103
Sp consists of
One S, one p
104
How many remaining unhybrid orbitals does sp3 have?
None
105
How many remaining unhybrid orbitals does sp2 have?
One p
106
How many remaining unhybrid orbitals does sp have?
Two p
107
Atomic orbitals to help explain bonding within molecules
Molecular orbital (MO) theory
108
Constructive interference means
Increased amplitude between nuclei
109
Destructive interference means
Node forms between the nuclei
110
S atomic orbitals can form
Sigma molecular orbitals
111
Three principles of molecular theory
1) # of MOs = # of atomic orbitals used
2) bonding MO is lower in energy than the atomic orbitals, the antibonding MO is higher
3) electrons assigned to MOs of successively higher energy
112
Bond order equation determined by MO
bonding e - # antibonding e divided by 2
113
How many electrons should be added to the MO diagram of the He2 molecule
4
