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Chemistry 1 > Chapter 10 Chemical Bonding I: The Lewis Model > Flashcards

Chapter 10 Chemical Bonding I: The Lewis Model Flashcards

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1
Q

what does the lewis model emphasize?

A

valence electrons

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2
Q

Using Lewis model, we can draw chemical structures, called what?

A

Lewis structures
or
Electron dot structure

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3
Q

what does the Lewis structure allow us to predict?

A

molecular stability
shape
size
polarity

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4
Q

Chemical bonds form because they what between the charged particles that compose atoms.

A

lower the potential energy

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5
Q

when does a chemical bond form?

A

when the potential energy of the bonded atoms is less than the potential energy of the separate atoms.

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6
Q

When a metal atom loses electrons it becomes a WHAT?

A

Cation

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7
Q

When a nonmetal atom gains electrons it becomes an what

A

anion

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8
Q

what have high electron affinities?

A

nonmetals

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9
Q

what makes it advantageous to add electrons to atoms

A

high electron affinities

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10
Q

The oppositely charged ions are then attracted to each other, resulting in an

A

ionic bond

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11
Q

have a high ionization energy

A

nonmetals

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12
Q

when is the potential energy lowest?

A

when the electrons are between the nuclei

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13
Q

The simplest theory of metallic bonding

A

metal atoms releasing their valence electrons to be shared as a pool by all

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14
Q

where does metallic bonding result from?

A

attraction of the cations for the delocalized electrons.

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15
Q

involves the transfer or sharing of valence electrons between two or more atoms.

A

chemical bonding

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16
Q

are most important in bonding.

A

valence electrons

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17
Q

indicates the number of valence electrons for main group elements.

A

column number on the periodic table

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18
Q

how many electrons do transition elements have?

A

2

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19
Q

how to represent valence electrons of main group electrons in the lewis structure?

A

dots surrounding the symbol for the element.

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20
Q

We use the what to represent nucleus and inner electrons.

A

symbol of the element

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21
Q

When atoms bond, they tend to gain, lose, or share electrons to result in eight valence electrons

A

Octet Rule `

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22
Q

exceptions to octet rule

A

H
Li
Be
B

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23
Q

having two valence electrons

A

a duet

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24
Q

is the arrangement of cations and anions in a crystalline structure

A

crystal lattice

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25
Q

long-range repeating order of the ions).

A

crystalline

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26
Q

what is a crystal lattice held by?

A

the electrostatic
attraction of the cations for all the surrounding anions.

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27
Q

The extra stability that accompanies the formation of the
crystal lattice is measured as the what?

A

lattice energy

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28
Q

the energy released when the
solid crystal forms from separate ions in the gas state.

A

lattice energy

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29
Q

what does lattice energy depend directly on

A

size of charges

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30
Q

what does lattice energy depend indirectly on

A

distance between ions

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31
Q

is a hypothetical series of reactions that represents the formation of an ionic compound from its constituent elements.

A

Born-Haber Cycle

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32
Q

The force of attraction between oppositely charged particles is directly proportional to what?

A

the product of the charges

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33
Q

Larger charge the what the attraction

A

stronger

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34
Q

the strong the attraction the what the Lattice energy

A

more

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35
Q

all ionic compounds are what at room temp?

A

SOLID

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36
Q

what kind of attraction is nondirectional

A

electrostatic attraction

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37
Q

predicts ionic compounds should have high melting points and boiling points because breaking down the crystal should require a lot of energy.

A

Lewis theory

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38
Q

the stronger the attraction, the what the melting point?

A

the higher

39
Q

is measured by rubbing two materials together and seeing which “streaks” or cuts the other.

A

hardness

40
Q

The harder material is the one that what?

A

cuts or doesn’t streak

41
Q

To conduct electricity, a material must have what?

A

charged particles that are able to flow through the material.

42
Q

Lewis theory predicts that ionic solids should not conduct what?

A

electricity

43
Q

what should conduct electricity

A

liquid ionic compound
and
ionic compound dissolved in water

44
Q

The sharing of valence electrons is called

A

covalent bonding

45
Q

Electrons that are shared by atoms are called

A

bonding pairs

46
Q

Electrons that are not shared by atoms but belong to a particular atom are called

A

lone pairs

or nonbonding pairs

47
Q

When two atoms share one pair of electrons, it
is called a

A

single covalent bond

48
Q

When two atoms share two pairs of electrons the result is called a

A

double covalent bond

49
Q

When two atoms share three pairs of electrons the result is called a

A

triple covalent bond.

50
Q

Lewis theory of covalent bonding implies that the attractions between atoms are

A

directional

51
Q

Lewis theory predicts covalently bonded compounds will be found as what?

A

individual molecules

52
Q

Lewis theory predicts that the melting and boiling points of molecular compounds should be

A

low

53
Q

what bonds are strong and what attraction is weak

A

covalent
attractions

54
Q

Lewis theory predicts that the hardness and brittleness of molecular compounds should vary depending on the

A

strength of intermolecular attractive forces.

55
Q

most of the molecular solids are what?

A

soft and waxy

56
Q

should the molecular solids conduct electricity?

A

no

57
Q

should the molecular liquids conduct electricity?

A

no

58
Q

what conducts electricity when dissolved in water?

A

Molecular acids

59
Q

Lewis theory predicts that the more electrons two atoms share, the what the bond should be.

A

stronger and shorter

60
Q

is measured by how much energy must be added to break the bond.

A

bond strength

61
Q

is determined by measuring the distance between the nuclei of bonded atoms

A

bond length

62
Q

Covalent bonding between different types of atoms results in

A

unequal sharing of electrons.

63
Q

unequal sharing of electrons.

A

polar covalent bond
bond polarity

64
Q

The end with the larger electron density gets a what?

A

a partial negative

65
Q

The end that is electron deficient gets a

A

a partical positive charge

66
Q

The charged ends of the molecule represent a

A

dipole

67
Q

is a measure of bond polarity.

A

dipole moment

68
Q

is a material with a + and − end.

A

dipole

69
Q

Generally, the more electrons two atoms share and the larger the atoms, the what the dipole moment.

A

larger

70
Q

The ability of an atom to attract bonding electrons to itself is called

A

electronegativity

71
Q

is the most electronegative element.

A

fluorine

72
Q

is the least electronegative element.

A

francium

73
Q

are not assigned values.

A

noble gas atoms

74
Q

The larger the difference in electronegativity, the what the bond.

A

more polar

75
Q

If the difference in electronegativity between bonded atoms is what the bond is pure covalent.

A

0

76
Q

If the difference in electronegativity between bonded atoms is what the bond is nonpolar covalent

A

0.1 to 0.4

77
Q

If the difference in electronegativity between bonded atoms is what the bond is polar covalent

A

0.5 to 1.9

78
Q

If the difference in electronegativity between bonded atoms is what the bond is ionic

A

larger than or equal to 2.0

79
Q

is the percentage of a bond’s measured dipole moment compared to what it would be if the electrons were completely transferred.

A

percent ionic character

80
Q

The percent ionic character indicates the degree to which the electron is what?

A

transferred

81
Q

Elements with empty d orbitals can have more than eight electrons.

A

expanded octets

82
Q

Delocalization of charge helps to what?

A

stabilize the molecule

83
Q

When there is more than one Lewis structure for a molecule that differ only in the position of the electrons, they are called

A

resonance structures

84
Q

The actual molecule is a combination of the resonance forms a what?

A

resonance hybrid

85
Q

is a fictitious charge assigned to each atom in a Lewis structure that helps us to distinguish among competing Lewis structures.

A

formal charge

86
Q

most stable structures have what?

A

– Fewer formal charges.
– Smaller formal charges.
– Negative formal charges on the more electronegative atom.

87
Q

Chemical reactions involve breaking bonds in reactant molecules and making new bonds to create the products.

A

bond energies

88
Q

The amount of energy it takes to break one mole of a bond in a compound is called the

A

bond energy

89
Q

each atom gets 1⁄2 bonding electrons

A

Homolytic Cleavage

90
Q

electrons are unequally divided

A

Heterolytic Cleavage

91
Q

actual bond energy depends on what?

A

the
surrounding atoms and other factors.

92
Q

The distance between the nuclei of bonded atoms is called the

A

bond length

93
Q

involves the metal atoms releasing their valence electrons to be shared by all atoms/ions in the metal.

A

The simplest theory of metallic bonding

94
Q

As temperature increases, the electrical conductivity of metals

A

decreases

Chemistry 1 (14 decks)

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