Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 1b > Chapter 10: Sections 1-4 > Flashcards

Chapter 10: Sections 1-4 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Taste and caloric value are __________ properties of food.

A

Independent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

The caloric value of a food depends on the amount of __________ released when the food is metabolized.

A

Energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

The caloric value of a food depends on the amount of energy released when the food is __________.

A

Metabolized

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

The taste of a food is __________ of its metabolism.

A

Independent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

The sensation of taste originates in the tongue, where specialized cels called taste cells act as highly sensitive and specific __________ __________.

A

Molecular detectors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

These cells can discern sugar molecules from the thousands of different types of molecules present in a mouthful of food.

A

Taste cells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

The main factors for the discrimination of sugar molecules from other molecules present in a mouthful of food are the molecule’s __________ and __________ __________.

A

Shape, charge distribution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

The surface of a taste cell contains specialized protein molecules called:

A

Taste receptors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

A molecule that we can taste.

A

Tastant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

A particular tastant fits snugly into a special pocket on the taste receptor protein called the:

A

Active site

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

These all depend on shape-specific interactions between molecules and proteins.

A

Immune response, the sense of smell, and many types of drug action

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

The valence bond theory and the molecular orbital theory are _____ complex and _____ powerful than Lewis theory.

A

More, more

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Allows prediction of the shapes of molecules based on the idea that electrons- either as lone pairs or as bonding pairs- repel one another.

A

Valence shell electron pair repulsion theory (VSEPR theory)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

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

A

Electron groups

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

The VSEPR theory is based on the idea that electron groups repel one another through __________ forces.

A

Coulombic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

According to VSEPR theory, the repulsion a between electron groups on __________ __________ of a molecule determine the geometry of the molecule.

A

Interior atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

According to VSEPR theory, the repulsion a between electron groups on interior atoms of a molecule determine the __________ of the molecule.

A

Geometry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

The preferred geometry of a molecule is the one in which the electron groups have the __________ separation possible.

A

Maximum

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

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

A

Minimum

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

The interior atom is also referred to as the:

A

Central atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

For molecules having just one interior atom, molecular geometry depends on these two things:

A

1) The number of electron groups around the central atom

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Two electron groups = __________ geometry.

A

Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

The molecular geometry of three atoms with a 180 degree bond angle due to the repulsion of two electron groups.

A

Linear geometry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

The basic idea of VSEPR theory is that repulsions between electron groups determine __________ __________.

A

Molecular geometry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Molecules that form only 2 single bonds, with no lone pairs, are rare because they do not:

A

Follow the octet rule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Three electron groups = __________ __________ geometry.

A

Trigonal planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

The molecular geometry of four atoms with 120 degree bond angles in a plane.

A

Trigonal planar geometry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Different types of electron groups exert slightly different __________. Resulting bond angles reflect these differences.

A

Repulsions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

In determine electron geometry, we consider only the electron groups on the __________ atom, rather than electron groups on the __________ atoms.

A

Central, terminal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

The VSEPR geometries of molecules with two if three electrons around the central atom are _____-dimensional.

A

Two

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Balloon models do not represent atoms; they represent __________ __________.

A

Electron groups

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

A geometrical shape with four identical faces, each an equilateral triangle.

A

Tetrahedron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

The molecular geometry of five atoms with 109.5 bond angles.

A

Tetrahedral geometry

34
Q

__________ is an example of a molecule with four electron groups around the central atom.

A

Methane

35
Q

Five electron groups = __________ __________ geometry.

A

Trigonal bipyramidal

36
Q

The molecular geometry of six atoms with 120 degree bond angles between the three equatorial electron groups and 90 degree bind angles between the two axial electron groups and the trigonal plane.

A

Trigonal bipyramidal

37
Q

The angles in the trigonal bipyramidal structure are NOT:

A

All the same

38
Q

The three bonds in the trigonal plane.

A

Equatorial positions

39
Q

The angles between the equatorial positions are:

A

120 degrees

40
Q

The two bonds on either side of the trigonal plane.

A

Axial positions

41
Q

The angle between the axial positions and the trigonal plane is:

A

90 degrees

42
Q

The molecular geometry of seven atoms with 90 degree bond angles.

A

Octahedral geometry (octahedral arrangement)

43
Q

The octahedral geometry, there are _____ equatorial groups and _____ axial groups.

A

4, 2

44
Q

The geometrical arrangement of electron groups.

A

Electron geometry

45
Q

The geometrical arrangement of atoms.

A

Molecular geometry

46
Q

When dealing with lone pairs, notice that the electron geometry and the molecular geometry are different; the electron geometry is __________ to the molecular geometry.

A

Relevant

47
Q

Lone pair electrons generally exert slightly __________ repulsions than bonding electrons.

A

Greater

48
Q

A lone electron pair is more spread out in space than a bonding electron pair because a lone pair is attracted to _____ nucleus while a bonding pair is attracted to _____.

A

1, 2

49
Q

The lone pair occupies more of the __________ __________ around a nucleus.

A

Angular space

50
Q

The lone pair occupies more of the angular space around a nucleus, exerting a __________ repulsive force on neighboring electrons.

A

Greater

51
Q

A non-bonding electron pair occupies _____ space than a bonding pair.

A

More

52
Q

As shown in a water molecule, it’s electron geometry is tetrahedral but its molecular geometry is __________.

A

Bent

53
Q

The bond angle in H2O is even small than in NH3 because H2O has 2 __________ __________ on the central oxygen atom.

A

Lone pairs

54
Q

The more lone pairs, the __________ the bond angles.

A

Smaller

55
Q

The electron group (lone pair-lone pair) is:

A

Most repulsive

56
Q

The electron group (bonding pair-bonding pair) is:

A

Least repulsive

57
Q

The seesaw molecular geometry is sometimes called an:

A

Irregular tetrahedron

58
Q

When a lone pair could occupy either an equatorial position or an axial position, the lone pair should occupy the position that __________ its interaction with the bonding pairs.

A

Minimizes

59
Q

When a lone pair could occupy either an equatorial position or an axial position, the lone pair should occupy the position that minimizes its interaction with the bonding pairs. Therefore, it would occupy an:

A

Equatorial position

60
Q

In seesaw molecular geometry, the lone pair never occupies the __________ position.

A

Axial

61
Q

When two of the five electron groups around the central atom are lone pairs, the lone pairs occupy how many if the equatorial positions?

A

Two of the three

62
Q

When 3/5 of the electron groups around the central atom are lone pairs, the lone pair occupies all three of the equatorial positions and the resulting molecular geometry is __________.

A

Linear

62
Q

The molecular geometry of a molecular with octahedral electron geometry and one lone pair.

A

Square pyramidal

63
Q

In molecular geometry diagrams, what is not shown?

A

Lone pairs

64
Q

The molecular geometry of a molecule with octahedral electron geometry and two lone pairs.

A

Square planar

65
Q

When 2/6 electron groups around the central atom are lone pairs, the lone pairs occupy positions:

A

Across from each other

66
Q

When 2/6 electron groups around the central atom are lone pairs, the lone pairs occupy positions across for each other to minimize:

A

Lone pair-lone pair repulsions

67
Q

The geometry of a molecule is determined by:

A

The # of electron groups on the central atom

68
Q

The number of electron groups can be determined from:

A

The Lewis structure of the molecule

69
Q

Each of the following counts as a single electron group:

A

A lone pair, a single bond, a double one, and triple bond, or a single electron

70
Q

Double and triple bonds occupy _____ space than single bonds.

A

More

71
Q

Which statement is always true according to VSEPR theory?

A

The shape of a molecule is determined by repulsions among all electrons groups on the central atom (or interior groups, if there is more than one).

72
Q

What is the 1st step in predicting molecular geometries?

A

Draw a Lewis structure for the molecule

73
Q

What is the 2nd step in predicting molecular geometries?

A

Determine the # of electron groups around the central atom

74
Q

What is the 3rd step in predicting molecular geometries?

A

Determine the # of bonding pairs and lone pairs

75
Q

What is the 4th step in predicting molecular geometries?

A

Use table 10.1 to determine the electron geometry and molecular geometry

76
Q

Use this to represent a bond in plane of paper.

A

Straight line

77
Q

Use this to represent a bond going into the paper.

A

Hatched wedge

78
Q

Use this to represent a bond coming out of the paper.

A

Solid wedge

79
Q

Larger molecules may have two or more __________ atoms.

A

Interior

Chemistry 1b (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions