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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

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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
Q

Lone pairs ____ occupy axial positions

A

Never

26
Q

What is the molecular geometry of a molecule with 5 electron groups, with one of them being a lone pair?

A

Seesaw

27
Q

What is the molecular geometry of a molecule with 5 electron groups, with two of them being a lone pairs?

A

T-shaped

28
Q

What is the molecular geometry of a molecule with 5 electron groups, with three of them being a lone pairs?

A

Linear

29
Q

What is the molecular geometry of a molecule with 6 electron groups, with one of them being a lone pair?

A

Square pyramidal

30
Q

What is the molecular geometry of a molecule with 6 electron groups, with two of them being a lone pairs?

A

Square planar

31
Q

How can you determine the number of electron groups

A

From the Lewis structure

32
Q

A straight line is….?
A hashed wedge is…?
A solid wedge is…?

A

Bond in the plane of the paper
Bond going into the page
Bing coming out of the page

33
Q

If a diatomic molecule has a polar bond, is the whole molecule polar?

A

Yes

34
Q

If the bond in a diatomic molecule is nonpolar, the molecule as a whole will be ______

A

Nonpolar

35
Q

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 ____

A

Polar

36
Q

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 _____

A

Nonpolar

37
Q

Wether or not a polyatomic molecule will be polar or nonpolar (if it contains polar bonds) depends completely upon…?

A

The molecular geometry of the molecule

38
Q

Polar molecules mix ___ with other polar molecules but mix ____ with nonpolar molecules

A

Well

Badly

39
Q

Define valance bond theory

A

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
Q

The energy of interaction is usually _____ (or _____) when the interacting atomic orbitals contain a total of two electrons that can spin pair

A

Negative

Stabilizing

41
Q

In valance bonding theory, what do the atoms in a molecule reside in?

A

Quantum-mechanical atomic orbitals

Such as s,p,d,f and hybrid combinations of these

42
Q

In valence bond theory, Which two ways can a covalent bond occur?

A

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
Q

In valance bond theory, what determines the shape of the molecule?

A

The geometry of the overlapping orbitals

44
Q

Define hybridization

A

A mathematical procedure in which standard atomic orbitals are combined to form new, hybrid orbitals

45
Q

Define hybrid atomic orbitals (hybrid orbitals)

A

Orbitals formed from the combination of standard atomic orbitals that correspond more closely to the actual distribution of electrons in chemically bonded atom

46
Q

Are hybrid orbitals still located on individual atoms? What is the difference between orbitals and hybrid orbitals

A

Yes

Hybrid orbitals are different shapes and energies than standard atomic orbitals

47
Q

Hybrid orbitals _____ the energy of the molecule by _____ the orbital overlap in a bond

A

Minimize

Maximizing

48
Q

What does the standard number of atomic orbitals added together always equal?

A

The number of hybrid orbitals formed

ie total number of orbitals is conserved

49
Q

What does the particular combination of standard atomic orbitals added together determine?

A

The shape and energy of the hybrid orbitals formed

50
Q

Tendency to hybridize _____ with the number of bonds formed

A

Increases

51
Q

What does the hybridization of one s orbital and three p orbitals result in?

A

Four sp3 hybrid

52
Q

What does the hybridization if one s and two p orbitals result in?

A

Three sp2 hybrids and one leftover UN hybridized p orbitals

53
Q

What does the hybridization of one s and one p orbital result in?

A

Two sp orbitals and two left over unhybridized p orbitals

54
Q

Define Pi bond

A

The bond that forms between two p orbitals that overlap side to side

55
Q

Which bond is stronger sigma or Pi?

A

Sigma

56
Q

Why do Pi bonds make rotation impossible?

A

you have to break the bond to rotate

57
Q

define sigma bond

A

The resulting bond that forms between a combination of any two s,p or hybridized orbitals that overlap end to end

58
Q

in general sigma bonds are ____ than pi bonds

A

stronger

59
Q

what is the hybridization of linear geometry?

A

sp ( + 2 unhbridized p)

60
Q

what is the hybridization of trigonal planar?

A

sp2 ( + 1 unhbridized p)

61
Q

what is the hybridization of tetrehedral?

A

sp3

CHEM 1120 (22 decks)

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