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Manu > Chemistry Chapter 8 > Flashcards

Chemistry Chapter 8 Flashcards

1
Q

When sharing of electrons occurs, the attachment between atoms that results is called a…

A

Covalent bond

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2
Q

When such an attachment is formed, bond dissociation energy is released, and the process is..

A

exhotermic

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3
Q

When two or more atoms bond by means of electron sharing, the resulting particle is called a

A

molecule

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4
Q

If the electrons shared are centered between the two atoms, the attachment is called a

A

sigma bond

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5
Q

If the sharing involves the overlap of parallel orbitals, the attachment is called a

A

pi bond

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6
Q

How many electrons are shared in a double covalent bond?

A

four

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7
Q

Bond length is the distance between

A

the nuclei of two attached atoms

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8
Q

Which of the following relationships relating to bond length is generally correct?

A

the shorter the bond, the stronger the bond

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9
Q

Binary molecular compounds are generally composed of a metal and a nonmetal.

A

false

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10
Q

The second element in the formula of a binary compound is named using the
suffix -ite.

A

false

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11
Q

The prefix tetra- indicates three atoms.

A

false

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12
Q

The prefix hexa- indicates six atoms.

A

true

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13
Q

In naming the first element in a formula, the prefix mono- is not used.

A

true

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14
Q

For binary acids, the hydrogen part of the compound is named using the prefix
hydro-.

A

true

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15
Q

An oxyacid contains only two elements.

A

false

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16
Q

If the name of the anion of an oxyacid ends in -ate, the acid name contains the
suffix -ous.

A

false

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17
Q

CO

A

carbon monoxide

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18
Q

CO2

A

carbon dioxide

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19
Q

H2CO3

A

carbonic acid

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20
Q

NH3

A

ammonia

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21
Q

N2O4

A

Dinitrogen tetroxide

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22
Q

HNO2

A

Nitrous acid

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23
Q

HNO3

A

nitric acid

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24
Q

HBr

A

hyrdobromic acid

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25
Q

HBrO3

A

bromic acid

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26
Q

A structural formula shows the arrangement of the atoms in a molecule.

A

true

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27
Q

The central atom in a molecule is the one with the highest electron affinity.

A

false

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28
Q

In molecules, hydrogen is always a terminal atom.

A

true

29
Q

The number of bonding pairs in a molecule is equal to the number of electrons.

A

true

30
Q

To find the total number of electrons available for bonding in a positive ion, you
should add the ion charge to the total number of valence electrons of the atoms
present.

A

false

31
Q

The electrons in a coordinate covalent bond are donated by both the bonded
atoms.

A

false

32
Q

Resonance occurs when more than one valid Lewis structure can be written for a
molecule.

A

true

33
Q

Nitrate is an example of an ion that forms resonance structures.

A

true

34
Q

The carbon dioxide molecule contains two double bonds.

A

true

35
Q

All electrons in an atom are available for bonding.

A

false

36
Q

In the sulfate ion (SO42−), 32 electrons are available for bonding.

A

true

37
Q

When carbon and oxygen bond, the molecule contains ten pairs of bonding
electrons.

A

false

38
Q

Odd number of valence electrons

A

NO

39
Q

. Fewer than 8 electrons around an atom

A

SF6

40
Q

More than 8 electrons around central atom

A

O3

41
Q

More than one valid Lewis structure

A

BF3

42
Q

The VSEPR model is used mainly to

A

determine molecular shape

43
Q

The bond angle is the angle between

A

two terminal atoms and the central atom.

44
Q

The VSEPR model is based on the idea that

A

shared and unshared electron pairs repel each other as much as possible.

45
Q

The shape of a molecule whose central atom has four pairs of bonding electrons is

A

tetrahedral

46
Q

The shape of a molecule that has two covalent single bonds and no lone pairs on the central atom is6

A

linear

47
Q

The shape of a molecule that has three single covalent bonds and one lone pair on the central atom is

A

trigonal pyramidal.

48
Q

The formation of new orbitals from a combination or rearrangement of valence electrons is called

A

hybridization

49
Q

The orbitals that are produced in this way are ________________________ to one another

A

identical

50
Q

An example of an element that commonly undergoes such formation is

A

methane

51
Q

When this atom combines its three p orbitals and its one s orbital, the orbitals that result are called ____________________ orbitals.

A

sp3

52
Q

An example of a molecule that has this type of orbital is

A

carbon

53
Q

What is the meaning of the term electronegativity?

A

electronegativity is the relative ability of an element’s atom to attract electrons in a chemical bond.

54
Q

Which element has the highest electronegativity? What is the numerical value? What are the name and group number of the chemical family that has the highest overall electronegativities?

A

Fluorine (F) w/ 3.98. In the nonmetal familiy (group 17) it has the highest overall electronegatives.

55
Q

Which element has the lowest electronegativity? What is the numerical value? What are the name and group number of the chemical family that has the lowest overall electronegativities?

A

Francium (Fr) w/ 0.7. In the metal family (group 1) it has the lowest overall electronegatives.

56
Q

What general trend in electronegativity do you note going down a group? Across a period?

A

Going down a group, its numerical value decreases. Across a group, it decreases

57
Q

How are the electronegativity values used to determine the type of bond that exists
between two atoms?

A

you subtract the values.

58
Q

Ionic compounds are usually soluble in polar substances.

A

true

59
Q

In a covalent molecular compound, the attraction between molecules
tends to be strong.

A

false

60
Q

Unequal sharing of electrons between two bonded atoms always indicates

A

a polar covalent bond.

61
Q

When electronegativities of two bonded atoms differ greatly, the bond is

A

ionic

62
Q

What is the electronegativity difference that usually is the dividing line between covalent and ionic bonds?

A

1.7

63
Q

Where is the symbol “sygma” placed next to?

A

the less electronegative atom in a polar covalent bond

64
Q

A nonpolar covalent bond is one in which

A

electrons are shared equally

65
Q

Molecules containing only polar covalent bonds

A

may or may not be polar.

66
Q

What factor other than electronegativity determines whether a molecule as a whole is polar or not?

A

its geometry

67
Q

Which of the following correctly describes the compound water, H2O?

A

polar overall, with nonpolar covalent bonds

68
Q

Which of the following correctly describes the compound carbon tetrachloride, CCl4?

A

nonpolar overall, with polar covalent bonds

69
Q

A molecule of ammonia, NH3, is

A

polar because there is an electronegativity difference and the molecule is trigonal pyramidal

Manu (18 decks)

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