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CHEM 1120 > Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecualr Orbital Theory > Flashcards

Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecualr Orbital Theory Flashcards

1
Q

Define electron groups

A

A general term for lone pairs, single bonds, multiple bonds, or lone electrons in a molecule

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2
Q

According to VESPR theory what do the repulsions between electron groups on interior atoms of a molecule determine?

A

The geometry of the molecule

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3
Q

The preferred geometry of a molecule is the one which electron groups have the _____ separation (and therefore _____ energy) possible

A

Maximum

Minimum

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4
Q

For molecules that have just one interior atom (the central atom), what two things does the the molecular geometry depend on?

A
  1. The number of electron groups around the central atom

2. How many of those electron groups are bonding groups and how many are lone pairs

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5
Q

What is the electron geometry for two electron groups?

A

Linear geometry

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6
Q

What are the angles between the two electron group in linear geometry

A

180°

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7
Q

Is a double bond still one electron group?

A

Yes

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8
Q

Linear geometry can be observed in all molecules that have….

A

Two electron groups and no lone pairs

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9
Q

What electron geometry forms with 3 electron groups?

A

Trigonal planar

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10
Q

What angle for trigonometry planar geometry maximizes the electron groups separation?

A

120°

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11
Q

Electron geometry, the geometry predicted by VESPR theory, is ______

A

Idealized

This means that it is close but not the same as the geometry found experimentally

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12
Q

What is the electron geometry for four electron groups?

A

Tetrahedral geometry

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13
Q

What are the ideal angles of tetrahedral geometry?

A

109.5°

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14
Q

What is the geometry for five electron groups?

A

Trigonal bipyramidal geometry

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15
Q

What are the angles like for trigonal bipyramidal geometry?

A

The angles between the equatorial positions (the three bonds in the trigonal plane) are 120°, while the angle between the axial positions (the two bonds on either side of the trigonal plane) and the trigonal plane is 90°

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16
Q

What is the electron geometry for 6 electron groups?

A

Octahedral geometry

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17
Q

Define valance shell electron pair repulsion theory (VSEPR theory)

A

A theory that allows prediction of the shapes of molecules based on the idea that electrons—either as lone pairs or bonding pairs—repel one another

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18
Q

What are the angles for octahedral geometry?

A

All angles are 90°

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19
Q

Define electron geometry

A

The geometrical arrangement of electron groups in a molecule

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20
Q

Define molecular geometry

A

The geometrical arrangement of atoms in a molecule

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21
Q

Lone pairs take up ____ than bonding pairs

A

More

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22
Q

What is the molecular geometry of a molecule with 4 electron groups, with one of them being a lone pair?

A

Trigonal pyramidal

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23
Q

What is the molecular geometry of a molecule with 4 electron groups, with two of them being a lone pairs?

A

Bent

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24
Q

Lone pair–lone pair repulsion is _____ than lone pair–bonding pair repulsion which is _____ than bonding pair–bonding pair repulsion

A

Greater

Greater

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25
Lone pairs ____ occupy axial positions
Never
26
What is the molecular geometry of a molecule with 5 electron groups, with one of them being a lone pair?
Seesaw
27
What is the molecular geometry of a molecule with 5 electron groups, with two of them being a lone pairs?
T-shaped
28
What is the molecular geometry of a molecule with 5 electron groups, with three of them being a lone pairs?
Linear
29
What is the molecular geometry of a molecule with 6 electron groups, with one of them being a lone pair?
Square pyramidal
30
What is the molecular geometry of a molecule with 6 electron groups, with two of them being a lone pairs?
Square planar
31
How can you determine the number of electron groups
From the Lewis structure
32
A straight line is....? A hashed wedge is...? A solid wedge is...?
Bond in the plane of the paper Bond going into the page Bing coming out of the page
33
If a diatomic molecule has a polar bond, is the whole molecule polar?
Yes
34
If the bond in a diatomic molecule is nonpolar, the molecule as a whole will be ______
Nonpolar
35
If the molecular geometry is such that the dipole moments of idividual polar bonds sum together to a net dipole moment the the molecule will be ____
Polar
36
It the molecular geometry is such that the dipole moments of the individual polar bonds cancel each other (that is, sum to zero), then the molecule will be _____
Nonpolar
37
Wether or not a polyatomic molecule will be polar or nonpolar (if it contains polar bonds) depends completely upon...?
The molecular geometry of the molecule
38
Polar molecules mix ___ with other polar molecules but mix ____ with nonpolar molecules
Well | Badly
39
Define valance bond theory
An advanced model of chemical bonding in which electrons reside in quantum-mechanical orbitals localized on individual atoms that are a hybridized blend of standard atomic orbitals; chemical bonds result from an overlap of these orbitals
40
The energy of interaction is usually _____ (or _____) when the interacting atomic orbitals contain a total of two electrons that can spin pair
Negative | Stabilizing
41
In valance bonding theory, what do the atoms in a molecule reside in?
Quantum-mechanical atomic orbitals | Such as s,p,d,f and hybrid combinations of these
42
In valence bond theory, Which two ways can a covalent bond occur?
When two half-filled orbitals with spin pairing of the two valence electrons Or less commonly, the overlap of a completely filled orbital with an empty orbital
43
In valance bond theory, what determines the shape of the molecule?
The geometry of the overlapping orbitals
44
Define hybridization
A mathematical procedure in which standard atomic orbitals are combined to form new, hybrid orbitals
45
Define hybrid atomic orbitals (hybrid orbitals)
Orbitals formed from the combination of standard atomic orbitals that correspond more closely to the actual distribution of electrons in chemically bonded atom
46
Are hybrid orbitals still located on individual atoms? What is the difference between orbitals and hybrid orbitals
Yes | Hybrid orbitals are different shapes and energies than standard atomic orbitals
47
Hybrid orbitals _____ the energy of the molecule by _____ the orbital overlap in a bond
Minimize | Maximizing
48
What does the standard number of atomic orbitals added together always equal?
The number of hybrid orbitals formed | ie total number of orbitals is conserved
49
What does the particular combination of standard atomic orbitals added together determine?
The shape and energy of the hybrid orbitals formed
50
Tendency to hybridize _____ with the number of bonds formed
Increases
51
What does the hybridization of one s orbital and three p orbitals result in?
Four sp3 hybrid
52
What does the hybridization if one s and two p orbitals result in?
Three sp2 hybrids and one leftover UN hybridized p orbitals
53
What does the hybridization of one s and one p orbital result in?
Two sp orbitals and two left over unhybridized p orbitals
54
Define Pi bond
The bond that forms between two p orbitals that overlap side to side
55
Which bond is stronger sigma or Pi?
Sigma
56
Why do Pi bonds make rotation impossible?
you have to break the bond to rotate
57
define sigma bond
The resulting bond that forms between a combination of any two s,p or hybridized orbitals that overlap end to end
58
in general sigma bonds are ____ than pi bonds
stronger
59
what is the hybridization of linear geometry?
sp ( + 2 unhbridized p)
60
what is the hybridization of trigonal planar?
sp2 ( + 1 unhbridized p)
61
what is the hybridization of tetrehedral?
sp3

CHEM 1120 (22 decks)

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