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TEST 3
TEST 3
84 terms
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16 plays
3.3
Flashcards
84 cards
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Practice quiz
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Questions
84
Answers
1
# of atomic orbitals in = # of hybrid orbitals out
False
True
2
For Cations, you add an electron.
False
True
3
Covalent bonds break at melting point
True
False
4
Electrons in anti-bonding orbitals make the system less stable
Valence bond theory
Molecular orbital theory (MO)
5
Where does the energy come from?
The system
The surroundings
6
Double bonds are delocalized
False
True
7
How can carbon form 4 identical bonds in diamond?
Valence bond theory
MO theory
Hybrid orbitals
High amounts of energy
8
Atomic orbitals may combine to form hybrid orbitals that are used for bonding
Valence bond theory
Molecular orbital theory (MO)
9
LDFs are strong. They require a lot of energy to break
False
True
10
Graphite conducts electricity
True
False
11
What does it mean when pi electrons (electrons in a pi bond) are delocalized?
Free to move/roam inside carbon atoms like in graphite
They move at a random rate
They’re not free to roam, they’re stuck to the atom that they’re bonded too
12
Metallic bonding only happens...
Between metals
Between non-metals
Between oppositely charged species
13
A double bond is a sigma and pi bond
True
False
14
Diamond
False
True
15
What kinds of interactions/bonds must be overcome in order to melt B, C?
LDF/Covalent
Metallic
LDF
Covalent
16
Atomic orbitals overlap to form a bond
Valence bond theory
Molecular orbital theory (MO)
17
This illustrates covalent bonding
True
False
18
Why does diamond not conduct electricity?
Electrons located inside bonds between atoms. Not free to roam, localized
3D networks of strong covalent bonds makes bonds difficult to break
The large band gap between bonding and anti bonding orbitals
19
LDFs are caused by
Fluctuating charge distributions
Attraction of electrons from one atom to nuclei from another atom
20
Why is graphite shiny?
It can emit and absorb photons
Because sheets can slide over each other
Because of the delocalized free to roam atoms around the entire framework
21
Why does graphite conduct electricity?
Because of the delocalized free to roam atoms around the entire framework
Because sheets can slide over each other
It can emit and absorb photons
22
Do these processes release or require energy?
Release
Require
23
Sigma bonds are localized
True
False
24
When you see a hybridized orbital like tetrahedral carbon sp3, what can you assume?
It has very directed strong bonds
Low MP/low decomposition temperature
High MP / decomposition temperature
Both A&B
25
Graphite...
All of the above
Has layers sliding over each other
Has strong covalent bonds between atoms
Has weak forces between layers
26
Diamond
True
False
27
Electrons in bonding orbitals stabilize the system
Valence bond theory
Molecular bonding theory (MO)
28
Boron and Carbon....
Are Allotropes
Are Metallically bonded
Are Metals
29
Graphite’s geometry, hybridization, and bond angle is...
Trigonal planar, sp2, 120
Tetrahedral, sp2, 120
Tetrahedral,sp3,<109
Trigonal planar, sp2, <109
30
A covalent bond cannot break at melting point. Only LDFs are overcome.
False
True
31
Covalent bonds are relatively weak
False
True
32
Why is diamond hard?
3D networks of strong covalent bonds makes bonds difficult to break
Electrons located in bonds between and are not free to roam
The large band gap between bonding and anti bonding orbitals
33
How many atomic orbitals (in one carbon) should come together to make 4 hybrid orbitals?
5
3
2
4
34
Graphite has a delocalized pi network over the whole sheet of atoms
True
False
35
Diamond’s geometry is tetrahedral, it has a sp3 hybridization, and a <109 bond angle
False
True
36
This illustrates LDF
False
True
37
A covalent bond...
Present between all molecular species
Is hard to predict
Both A & B
Present only when atomic orbitals interact constructively
38
When a substance melts....
Interactions between particles have to be overcome
Interactions between particles spike to promote movement
Interactions between particles stay the same
39
Why are diamond and graphite properties so different?
Because graphite displays more electronegativity
Because of how strong LDFs are
Because of the way carbon atoms bond
40
The ___ the overlap, the ___ the bond.
Greater, stronger
Greater, weaker
Lesser, stronger
41
Do these processes release or require energy?
Release
Require
42
Covalent bonds are caused by
Fluctuating charge distributions
Attraction of electrons from one atom to nuclei from another atom
43
What kinds of interactions are needed to melt He, Ne?
LDF/Covalent
Metallic
Covalent
LDF
44
A single bond is a sigma bond
True
False
45
What causes diamond’s properties?
C atoms having the same distance in between atoms causing a rigid network
None of the above
The covalent bonds inside c atoms and LDF between c atom layers
The weak force in between layers of C
46
Both double bonds and triple bonds are free to move (meaning they can be split)
False
True
47
Why must we assume a tetrahedral pattern with diamond?
There is a p orbital left over
Because carbon forms a sigma bond
Large gap between anti bonding and bonding orbitals
48
The magnitude of the MP and BP provides an estimate of...
The strength of attractive forces between particles
Networks that are formed
I dont know
The strength of a covalent bond
49
A double bond is 1 sigma and 2 pi bonds
True
False
50
In diamond, each carbon forms 4 identical bonds to 4 identical carbons
True
False
51
What causes diamond to be translucent?
Electrons located inside bonds between atoms. Not free to roam
3D networks of strong covalent bonds makes bonds difficult to break
The large band gap between bonding and anti bonding orbitals
52
The bigger the atom, the higher the MP and BP
False
True
53
Graphene is a one layer thin graphite sheet
False
True
54
For anions you subtract an electron
True
False
55
Electrons are delocalized
Molecular orbital theory (MO)
Valence bond theory
56
Graphite has a localized sigma bond framework
True
False
57
Electrons are localized in the bond
Molecular orbital theory (MO)
Valence bond theory
58
Carbon has 4 valence electrons in different types of orbitals
False
True
59
Each orbital can contain up to two electrons
Valence bond theory
Molecular orbital theory (MO)
60
Allotropes are extended networks of covalent bonds
False
True
61
The greater the overlap, the stronger the bond
Valence bond theory
Molecular orbital theory (MO)
62
Sigma bonds (H-H) are delocalized
False
True
63
What kinds of interactions/bonds must be overcome in order to melt H2, F2
Covalent
LDF
Metallic
LDF/Covalent
64
What is happening here?
Hybridization
MO theory
Valence bond theory
Polarity
65
Each bond is made up of two electrons
Valence bond
Molecular orbital theory (MO)
66
Triple bonds are delocalized
True
False
67
What causes graphite to have the “slippery” property
The tetrahedral shape of graphite causes the slippery property
The weak forces in between layers causes graphite to be slippery (LDFS)
The strong carbon bonds cause the slippery property
68
Bonds in valence bond theory are delocalized
False
True
69
Diamond and graphite are made of...
Cobalt
Calcium
Boron, carbon
Carbon
70
In this model we can assume....
Atomic orbitals overlap to form bonds
Atomic orbitals cancel each other out
Atomic orbitals are delocalized
71
Sigma bonds
All of the above
Are localized
Can exist independently
Are less reactive
72
Diamond conducts electricity
True
False
73
What is the electron configuration of Carbon?
[He] 2s2 2p5
[Ne] 3s2 3p5
[He] 2s2 2p2
[Ne] 3s2 3p4
74
What kinds of interactions/bonds must be overcome in order to melt Li, Be
Metallic
LDF
Covalent
Covalent/LDF
75
Tetra means...
3
4
2
1
76
Where does the energy go?
The surroundings
The system
77
Hybridization means to “mix up.” Atomic orbitals form bonding orbitals that combine with orbitals from another atom
True
False
78
Bonds in valence bond theory are also known as
covalent bonds
Sticks ( H——H)
LDF bonds
79
A triple bond is a sigma and two pi bonds
True
False
80
Atomic orbitals combine to form an equal number of molecular orbitals
Valence bond theory
Molecular orbital theory (MO)
81
Covalent bonding forms...
Between oppositely charged species
Between metals
Between non-metals
82
This model of bonding depicts MO theory
True
False
83
H can form bonds with...
O
F
All of the above
N
84
In carbon (diamond) all four bonds are identical
False
True
