Chapter 10: Sections 1-4

Question 1

Taste and caloric value are __________ properties of food.

Answer 1

Independent

Question 2

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

Answer 2

Energy

Question 3

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

Answer 3

Metabolized

Question 4

The taste of a food is __________ of its metabolism.

Answer 4

Independent

Question 5

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

Answer 5

Molecular detectors

Question 6

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

Answer 6

Taste cells

Question 7

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

Answer 7

Shape, charge distribution

Question 8

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

Answer 8

Taste receptors

Question 9

A molecule that we can taste.

Answer 9

Tastant

Question 10

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

Answer 10

Active site

Question 11

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

Answer 11

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

Question 12

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

Answer 12

More, more

Question 13

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

Answer 13

Valence shell electron pair repulsion theory (VSEPR theory)

Question 14

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

Answer 14

Electron groups

Question 15

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

Answer 15

Coulombic

Question 16

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

Answer 16

Interior atoms

Question 17

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

Answer 17

Geometry

Question 18

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

Answer 18

Maximum

Question 19

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

Answer 19

Minimum

Question 20

The interior atom is also referred to as the:

Answer 20

Central atom

Question 21

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

Answer 21

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

Question 22

Two electron groups = __________ geometry.

Answer 22

Linear

Question 23

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

Answer 23

Linear geometry

Question 24

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

Answer 24

Molecular geometry

Question 25

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

Answer 25

Follow the octet rule

Question 26

Three electron groups = __________ __________ geometry.

Answer 26

Trigonal planar

Question 27

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

Answer 27

Trigonal planar geometry

Question 28

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

Answer 28

Repulsions

Question 29

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

Answer 29

Central, terminal

Question 30

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

Answer 30

Two

Question 31

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

Answer 31

Electron groups

Question 32

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

Answer 32

Tetrahedron

Question 33

The molecular geometry of five atoms with 109.5 bond angles.

Answer 33

Tetrahedral geometry

Question 34

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

Answer 34

Methane

Question 35

Five electron groups = __________ __________ geometry.

Answer 35

Trigonal bipyramidal

Question 36

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.

Answer 36

Trigonal bipyramidal

Question 37

The angles in the trigonal bipyramidal structure are NOT:

Answer 37

All the same

Question 38

The three bonds in the trigonal plane.

Answer 38

Equatorial positions

Question 39

The angles between the equatorial positions are:

Answer 39

120 degrees

Question 40

The two bonds on either side of the trigonal plane.

Answer 40

Axial positions

Question 41

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

Answer 41

90 degrees

Question 42

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

Answer 42

Octahedral geometry (octahedral arrangement)

Question 43

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

Answer 43

4, 2

Question 44

The geometrical arrangement of electron groups.

Answer 44

Electron geometry

Question 45

The geometrical arrangement of atoms.

Answer 45

Molecular geometry

Question 46

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

Answer 46

Relevant

Question 47

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

Answer 47

Greater

Question 48

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 _____.

Answer 48

1, 2

Question 49

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

Answer 49

Angular space

Question 50

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

Answer 50

Greater

Question 51

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

Answer 51

More

Question 52

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

Answer 52

Bent

Question 53

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

Answer 53

Lone pairs

Question 54

The more lone pairs, the __________ the bond angles.

Answer 54

Smaller

Question 55

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

Answer 55

Most repulsive

Question 56

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

Answer 56

Least repulsive

Question 57

The seesaw molecular geometry is sometimes called an:

Answer 57

Irregular tetrahedron

Question 58

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.

Answer 58

Minimizes

Question 59

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:

Answer 59

Equatorial position

Question 60

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

Answer 60

Axial

Question 61

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

Answer 61

Two of the three

Question 62

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 __________.

Answer 62

Linear

Question 62

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

Answer 62

Square pyramidal

Question 63

In molecular geometry diagrams, what is not shown?

Answer 63

Lone pairs

Question 64

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

Answer 64

Square planar

Question 65

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

Answer 65

Across from each other

Question 66

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

Answer 66

Lone pair-lone pair repulsions

Question 67

The geometry of a molecule is determined by:

Answer 67

The # of electron groups on the central atom

Question 68

The number of electron groups can be determined from:

Answer 68

The Lewis structure of the molecule

Question 69

Each of the following counts as a single electron group:

Answer 69

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

Question 70

Double and triple bonds occupy _____ space than single bonds.

Answer 70

More

Question 71

Which statement is always true according to VSEPR theory?

Answer 71

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).

Question 72

What is the 1st step in predicting molecular geometries?

Answer 72

Draw a Lewis structure for the molecule

Question 73

What is the 2nd step in predicting molecular geometries?

Answer 73

Determine the # of electron groups around the central atom

Question 74

What is the 3rd step in predicting molecular geometries?

Answer 74

Determine the # of bonding pairs and lone pairs

Question 75

What is the 4th step in predicting molecular geometries?

Answer 75

Use table 10.1 to determine the electron geometry and molecular geometry

Question 76

Use this to represent a bond in plane of paper.

Answer 76

Straight line

Question 77

Use this to represent a bond going into the paper.

Answer 77

Hatched wedge

Question 78

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

Answer 78

Solid wedge

Question 79

Larger molecules may have two or more __________ atoms.

Answer 79

Interior