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Chemistry > Chapter 7 (new) > Flashcards

Chapter 7 (new) Flashcards

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1
Q

Bonding orbital

A

Orbitals that serve to hold atoms together by increasing electron density.

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2
Q

Strength of Intermolecular forces relative to the kinetic energy.

A

What determines the state of matter (solid, liquid, gas) of a sample?

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3
Q

No, because it contains a sigma and pi bond.

A

Is a double bond twice as strong as a single bond?

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4
Q
A

Hybridization of the central atom with trigonal bipyramidal electron geometry.

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5
Q

sp

A

Hybridization of the central atom with linear electron geometry.

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6
Q

A sigma bond and 2 pi bonds

A

In Valence bond theory, a Lewis triple bond would be…

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7
Q
A

The angle(s) of separation for five Electron domains/groups

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8
Q

Sigma bond

A

Overlap of electron cloud density along the internuclear axis.

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9
Q

Boiling point, Melting point, Viscosity, and Surface tension

A

What increases as the strength of intermolecular forces increase?

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10
Q

Polarizability

A

Elongation of a molecule affects…

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11
Q
A

Electron pair geometry and Molecular shape for this molecule:

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12
Q

size/mass (more electrons)

A

LDF and Polarizability increase with …

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13
Q

“Central”

A

In VSEPR theory, the shape is assigned around each ___ atom.

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14
Q

London Dispersion Forces

A

A short-lived attractive force due to the constant motion of electrons within a molecule.

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15
Q
A

Electron pair geometry and Molecular shape for this molecule:

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16
Q

Hybridization

A

Mathematical combination of atomic orbitals that result in the formation of new orbitals.

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17
Q

Number of bonds / number of positions

A

How to predict partial bond order based on resonance structures.

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18
Q
A

Electron pair geometry and Molecular shape for this molecule:

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19
Q

Molecular orbital theory, MO

A

Model in which molecular orbitals belong to the molecule, not to individual atoms.

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20
Q

O, N, or F

A

Hydrogen bonding can occur when H is bonded to which atoms?

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21
Q
A

Hybridization of the central atom with tetrahedral electron geometry.

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22
Q

pi bond

A

What type of bond is broken with rotation?

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23
Q
A

Electron pair geometry and Molecular shape for this molecule:

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24
Q

No, it’s the protons that pull. Dipoles point towards the more electronegative atom in a bond.

A

Do lone pairs affect or “pull” when analyzing the polarity of a molecule?

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25
Q
A

Electron pair geometry and molecular shape of this molecule:

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26
Q

Hydrogen bonding

A

A special type of dipole-dipole attractive force between hydrogen atom bonded to an O, N, or F and a nearby lone pair.

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27
Q

Intramolecular Forces

A

Forces within a compound/molecule (ionic bonds, covalent bonds)

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28
Q

Ion-Induced dipole

A

London Dispersion Forces are also known as…

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29
Q

Valence bond theory, VB

A

Bonding theory that uses quantum mechanics to explain chemical bonding.

30
Q

the total atomic orbitals hybridized.

A

In valence bond theory, the number of hybrid orbitals equals…

31
Q
A

The angle of separation for four Electron domains/groups

32
Q
A

Electron pair geometry and Molecular shape for this molecule:

33
Q
A

Electron pair geometry and Molecular shape for this molecule:

34
Q

no

A

Do resonance structures affect VSEPR molecule construction?

35
Q
A

Hybridization of the central atom with octahedral electron geometry.

36
Q

Intermolecular Forces

A

Attractive forces between molecules.

37
Q

Electron domains/groups

A

The bonded atoms and lone pairs around a central atom are known as

38
Q

Node

A

Region of zero electron probability

39
Q

A sigma bond

A

In Valence bond theory, a Lewis single bond would be…

40
Q

Stronger

A

Hydrogen bonds are ___ than an average dipole-dipole interaction?

41
Q
A

The angle(s) of separation for six Electron domains/groups

42
Q
A

Electron pair geometry and molecular shape of this molecule:

43
Q

Vapor pressure

A

What decreases as the strength of intermolecular forces increase?

44
Q
A

Electron pair geometry and Molecular shape for this molecule:

45
Q

Hydrogen bond donor

A

In a hydrogen bond, the molecule that possesses the H is known as the…

46
Q

Valence Shell Electron Pair Repulsion (VSEPR) Theory

A

Electron domains/groups will repel each other to maximize the spatial distances.

47
Q

Lowest

A

The hybridization used is the one that yields the ___ energy.

48
Q
A

The angle(s) of separation for two Electron domains/groups

49
Q

Polarizability

A

The ease in which an electron cloud is distorted by an external charge.

50
Q
A

Electron pair geometry and Molecular shape for this molecule:

51
Q

Lone Pairs

A

Included in electron geometry but not molecule geometry.

52
Q

Pi Bond

A

Overlap of electron cloud density in front of/behind or above/below the internuclear axis.

53
Q
A

Electron pair geometry and Molecular shape for this molecule:

54
Q
A

Electron pair geometry and Molecular shape for this molecule:

55
Q
A

Electron pair geometry and Molecular shape for this molecule:

56
Q

Hydrogen bond acceptor

A

In a hydrogen bond, the molecule that possesses the lone pair is known as the…

57
Q

Molecular orbital theory, MO

A

Model that uses quantum mechanics to describe the electronic structure of molecules.

58
Q

Antibonding orbital

A

Orbitals that destabilize molecules by decreasing electron density

59
Q
A

Electron pair geometry and Molecular shape for this molecule:

60
Q
A

Hybridization of the central atom with trigonal planar electron geometry.

61
Q

Antibond

A

In MO theory, an * represents what?

62
Q

London Dispersion Forces

A

Type of intermolecular force that can apply to all atoms and molecules.

63
Q

London Dispersion Forces

A

Only intermolecular force present in symmetric, nonpolar molecules.

64
Q

Bond order

A
65
Q

More favorable

A

In MO theory, lower energy is…

66
Q

Lone pairs

A

Repel more than bonded atoms in a molecule.

67
Q
A

Electron pair geometry and Molecular shape for this molecule:

68
Q

A sigma bond and a pi bond

A

In Valence bond theory, a Lewis double bond would be…

69
Q

Dipole-dipole

A

Attractive forces between positive and negative ends of polar molecules.

70
Q
A

The angle of separation for three Electron domains/groups

Chemistry (13 decks)

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