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Chem > Ch 6 Section 5 > Flashcards

Ch 6 Section 5 Flashcards

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1
Q

Molecular geometry is the

A

3-dimensional arrangement of a molecule’s atoms in space

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2
Q

The polarity of each bond along with the geometry of the molecule determines

A

Molecular polarity

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3
Q

Molecular polarity is the

A

Uneven distribution of molecular charge

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4
Q

Molecular polarity strongly influenced the forces that act

A

Between molecules in liquids and solids

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5
Q

A chemical formula reveals little information about

A

A molecules geometry

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6
Q

After performing many tests designed to reveal the shapes of various molecules chemists developed two different

A

Equally successful theories to explain certain aspects of their findings

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7
Q

One theory accounts for

A

Molecular bond angles

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8
Q

The other theory is used to describe the orbitals that

A

Contain the valence electrons of a molecules atoms

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9
Q

Diatomic molecules like h2 and HCl must be

A

Linear because they consist of only two atoms

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10
Q

To predict the geometries of more complicated molecules one must consider the

A

Locations of all electron pairs surrounding the bonded atoms

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11
Q

The abbreviation VSEPR stands for

A

valence-shell, electron-pair repulsion

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12
Q

The abbreviation for VSEPR refers to the repulsion between

A

Pairs of valence electrons of the atoms in a molecule

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13
Q

VSEPR theory states that repulsion between the sets of valence level electrons surrounding an atom causes these sets to be

A

Oriented as far apart as possible

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14
Q

According to the VSEPR theory the shared pairs in BeF2 will be as far

A

Away from each other as possible

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15
Q

The distance between electron pairs is maximized if the bonds to fluorine are on

A

Opposite sides of the beryllium afl , 180 degrees apart. Thus the molecule is linear

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16
Q

If we represent the central atom in s molecule by the letter A and we represent the atoms bonded to the central atom by the letter B then according to VSEPR theory BeF2 is an example of an

A

AB2 molecule which is linear

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17
Q

In an AB3 molecule the three A-B bonds stay farthest apart by pointing to the corners of an

A

Equilateral triangle giving 120 degree angles between the bonds

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18
Q

The central atoms in AB4 molecules follow the octet rule by sharing

A

Four electron pairs with B atoms

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19
Q

In AB4 molecules the distance between electron pairs is maximized if each A-B bond points to

A

One of four corners of a tetrahedron

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20
Q

Ammonia (NH3) and water (H2O) are examples of molecules in which the central atom has both

A

Shared and unshared electron pairs

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21
Q

VSEPR theory postulates that the line pair of electrons occupies space around the (ammonia atom)

A

Nitrogen atom just as the bonding pairs do

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22
Q

Thus in ammonia the electron pairs maximize their separation by assuming the

A

Four corners of a tetrahedron

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23
Q

Lone pairs do occupy space but our description of the observed space of s molecules refers to the

A

Positions of atoms only

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24
Q

The general VSEPR formula for molecules such as ammonia is

A

AB3E where E represents the unshared electron pair

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25
Q

The VSEPR formula for water is

A

AB2E2

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26
Q

For H2O VSEPR theory states that the lone pairs occupy space around the central atom but that the actual shape of the molecule is determined by the position of the

A

Atoms only, resulting in a bent molecule

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27
Q

The bond angles in ammonia and water are smaller because the unshared electron pairs

A

Repeal electrons more strongly than do bonding electron pairs

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28
Q

In VSEPR theory double and triple bonds are treated in the same way as

A

Single bonds

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29
Q

In VSEPR theory poly atomic ions are treated similarly to

A

Molecules

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30
Q

Lewis structures and VSEPR theory and molecular geometry can be used together to predict the… Of poly atomic ions as well as… With

A

Shapes; molecules with double or triple bonds

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31
Q

VSEPR troth does not reveal the relaid shop between a molecules

A

Geometry and the orbitals occupied by its bonding electrons

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32
Q

To explain the orbitals of an atom become rearranged when the atom forms covalent bonds, a different

A

Model, hybridization is used

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33
Q

Hybridization is the mixing of two or more atomic orbitals of similar energies on the same atom to

A

Produce new hybrid atomic orbitals of equal energies

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34
Q

The sp3 orbitals all have the same

A

Energy which is greater than that of the 2s orbitals but less than that of the 2p orbitals

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35
Q

Hybrid orbitals are orbitals of

A

Equal energy produced by the combination of two or more orbitals on the same atom

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36
Q

The number of hybrid orbitals produced equals the number of

A

Orbitals that have combined

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37
Q

Hybridization also explains the

A

Bonding and geometry of many molecules formed by group 15 and 16 elements

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38
Q

The linear geometry of molecules such as beryllium fluoride is made possible by hybridization involving the

A

S orbital and one available empty p orbital To yield sp hybrid orbitals

39
Q

The trogonal-planar geometry of molecules such as boron fluoride is made possible by hybridization involving the

A

S orbital one singly occupied p orbital and one empty p orbital to yield sp2 hybrid orbitals

40
Q

Atomic orbitals: s, p
Type of hybridization:sp
Number of hybrid orbitals: 2
Geometry:

A

180 degrees; linear

41
Q

Atomic orbitals:s,p,p
Type of hybridization: sp2
Number of hybrid orbitals: 3
Geometry:

A

120 degrees: trigonal planar

42
Q

The properties of molecules depend not only on the bonding of atoms but also on

A

Molecular geometry

43
Q

Atomic orbitals:s,p,p,p
Type of hybridization: sp3
Number of hybrid orbitals: 4
Geometry:

A

109.5 degrees; tetrahedral

44
Q

Atoms bonded to central atom: 2
Lone pairs of electrons: 0
Type of molecule: AB2
Molecular shape:

A

Linear

45
Q

Atoms bonded to central atom: 3
Lone pairs of electrons: 0
Type of molecule: AB3
Molecular shape:

A

Trigonal-planar

46
Q

Atoms bonded to central atom: 2
Lone pairs of electrons: 1
Type of molecule: AB2E
Molecular shape:

A

Bent or angular

47
Q

Atoms bonded to central atom: 4
Lone pairs of electrons: 0
Type of molecule: AB4
Molecular shape:

A

Tetrahedral

48
Q

Atoms bonded to central atom: 3
Lone pairs of electrons: 1
Type of molecule: AB3E
Molecular shape:

A

Trigonal-pyramidal

49
Q

Atoms bonded to central atom: 2
Lone pairs of electrons: 2
Type of molecule: AB2E2
Molecular shape:

A

Bent or angular

50
Q

Atoms bonded to central atom: 5
Lone pairs of electrons: 0
Type of molecule: AB5
Molecular shape:

A

Trigonal-bipyramidal

51
Q

Atoms bonded to central atom: 6
Lone pairs of electrons: 0
Type of molecule: AB6
Molecular shape:

A

Octahedral

52
Q

As a liquid is heated the kinetic energy of its particles

A

Increases

53
Q

At the boiling point the needy is sufficient to overcome the force of

A

Attraction between the liquids particles

54
Q

The particles pull away from each other and enter the

A

Gas phase

55
Q

Boiling point therefore is a good measure of the force of

A

Attraction between particles of a liquid

56
Q

The higher the boiling point the stronger the

A

Forces between particles

57
Q

The forces of attraction between molecules are known as

A

Intermolecular forces

58
Q

Intermolecular forces. Art in strength but are generally weaker than bonds that join

A

Atoms in molecules, ions in ionic compounds, or metal atoms in solid metals

59
Q

The values for ionic compounds and metals are much higher than those for

A

Molecular substances

60
Q

The strongest intermolecular forces exist between

A

Polar molecules

61
Q

Polar molecules act as tiny dipoles because of their

A

Uneven charge distribution

62
Q

A dipole is created by equal but opposite charges that are

A

Separated by a short distance

63
Q

The direction of a dipole is from the dipoles

A

Positive pole to its negative pole

64
Q

A dipole is represented by an arrow with a head pointing toward the

A

Negative pole and a crossed tail situated at the positive pole

65
Q

The negative region in one polar molecule attracts the

A

Positive region in adjacent molecules

66
Q

The forces of attraction between polar molecules are known as

A

Dipole-dipole forces

67
Q

The forces of attraction between polar molecules are known as

A

Dipole-dipole forces

68
Q

Dipole-dipole forces are short range forces, acting only between

A

Nearby molecules

69
Q

The polarity of diatonic molecules such as ICl is determined by just

A

One bond

70
Q

For molecules containing more than two atoms molecular polarity depends on both the

A

Polarity and the orientation of each bond

71
Q

Because the molecule is bent the polarities of these two bonds combine to make the molecule

A

Highly polar

72
Q

In some molecules individual bond dipoles

A

Cancel one another causing the molecular polarity to be zero

73
Q

A polar molecule can induce a dipole in an Nonpolar molecule by

A

Temporarily attracting its electrons

74
Q

The result is a short range intermolecular force that is somewhat

A

Weaker than the dipole-dipole force

75
Q

Some hydrogen containing compounds have unusually high

A

Boiling points

76
Q

These high boiling points is explained by the presence of a particularly strong type of

A

Dipole-dipole force

77
Q

In compounds containing H-F, H-O, or H-N bonds, the large electronegativity differences between hydrogen atoms and fluorine, oxygen, or nitrogen atoms make the bonds connecting them

A

Highly polar

78
Q

The high polarity gives the hydrogen atom a positive charge that is almost half as large as that of a

A

Proton

79
Q

The small size of the hydrogen atom allows the atom to come very close to an

A

Unshared pair of electrons on an adjacent molecule

80
Q

The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an electronegative atom in a nearby molecule is known as

A

Hydrogen bonding

81
Q

Hydrogen bonds are usually represented by dotted lines connecting the hydrogen bonded hydrogen to the unshared electron pair of the

A

Electronegative atom to which it is attracted

82
Q

Even noble gas atoms and molecules that are Nonpolar experience a

A

Weak intermolecular attraction

83
Q

In any atom or molecule the electrons are in

A

Continuous motion

84
Q

Thus at any instant the electron distribution may be slightly

A

Uneven

85
Q

The momentary uneven charge creates a positive pole in one part of the atom or molecule and a

A

Negative pole in another

86
Q

This temporary dipole can then induce a dipole in an

A

Adjacent atom or molecule

87
Q

The two are held together for an instant by the weak attraction. Between the

A

Temporary dipoles

88
Q

The intermolecular attract drinks resulting from the constant motion of electrons and the creation of instantaneous dipoles are called

A

London dispersion forces

89
Q

London dispersion forces are named after

A

Fritz London who first proposed their existence in 1930

90
Q

London forces act between all

A

Atoms and molecules

91
Q

London forces are the only intermolecular forces acting among

A

Noble gas atoms and Nonpolar molecules

92
Q

Because London forces are dependent on he motion of electrons their strength increases with the number of

A

Electrons in the interacting atoms or molecules

93
Q

London forces increase with increasing

A

Atomic or molar mass

Chem (54 decks)

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