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Introduction to Chemistry > chapter 3: Bonding general concepts > Flashcards

chapter 3: Bonding general concepts Flashcards

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1
Q

what is chemical bonding?

A

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

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2
Q

what are some electrostatic interactions in bonds

A

the attraction between electron and nuclei, repulsions between electrons, repulsions between nuclei

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3
Q

what are the types of chemical bonds

A

metal to nonmetals, nonmetal to nonmetal, metal to metal

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4
Q

what is a metal to nonmetal bond called

A

ionic bond

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5
Q

what is a nonmetal to nonmetal bond

A

covalent bond

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6
Q

what is a metal to metal bond

A

metallic bond

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7
Q

what is a chemical formula

A

composition of a substance

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8
Q

what are the 3 types of chemical formulas

A

empirical formula, molecular, structural

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9
Q

what is the empirical formula

A

the lowest whole number ratio of atoms

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10
Q

what is a molecular formula

A

give the exact number of the atoms

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11
Q

what is a structural formula

A

sketch or diagram of how the atoms in a molecule are bonded together

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12
Q

what is a molecular model

A

the more accurate and complete way to specify a compound

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13
Q

what do a ball and stick model represent?

A

chemical bonds, balls are color-coded for specific elements

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14
Q

what is constructive interference?

A

waves interact to make a longer wave

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15
Q

what is destructive interference?

A

waves interact to cancel each other

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16
Q

what did the pauli exclusion state

A

no 2 electrons in the same atom can make the same energy and no orbital can have more than 2 electrons, and can’t have the same spin

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17
Q

what was hund’s rule

A

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied,

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18
Q

what is the aufbau principle

A

electrons fill from the lowest energy first

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19
Q

what is an example of a ionic bond

A

NaCl

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20
Q

what is an example of a covalent bond

A

H2O

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21
Q

what is an example of a metallic bond

A

Na+

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22
Q

what is a chemical formula

A

composition of a substance

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23
Q

what are the three types of chemical formulas

A

empirical, molecular, structural

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24
Q

what is an empirical formula

A

gives the lowest whole number ration of atoms

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25
Q

what is a molecular formula

A

molecular formula gives the exact # of atoms of each element in the compound

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26
Q

what is a structural formula

A

sketch of graph of how the atoms ina molecule are bonded together

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27
Q

what is a molecular model

A

more accurate and complete way to specify a compound

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28
Q

what is a ball and stick model

A

balls and sticks represent the chemical bonds
balls = atoms
sticks= bond

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29
Q

what is a space filling molecular model

A

atoms fill in the space between each more closely to represent an estimate of how a molecule might appear

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30
Q

how is an ionic bond formed

A

when oppsitely charged ions attract each other

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31
Q

what is another name for ionic bond

A

ionic compound

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32
Q

what is an ionic compound composed of in a sold state

A

lattice

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33
Q

what is a lattice

A

3D array of alternating cations and anions

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34
Q

does a lattice have low or high potential energy

A

low

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35
Q

what is the principle of coulomb’s law

A

ionic compounds are stable bc of the attraction between ions and unlike charges

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36
Q

what does coulomb’s law state

A

longer distance = less attraction; shorter distance = more attraction
higher charge = stronger force= larger lattice energy

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37
Q

what is coulomb’s formula

A

k (Q1Q2/r^2) = F

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38
Q

what does k represent in coulombs

A

coulomb’s constant; 2.13x10^-19 nm

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39
Q

what does r^2 represent

A

the distance

if the distance is larger than the charge then there is not a lot of force or energy

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40
Q

what are some properties of ionic compounds

A

high melting points and boiling points

solids are brittle and hard

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41
Q

why does it take a lot of energy to breakdown the crystal lattice

A

attractions between ions are strong

stronger attracton = higher melting point

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42
Q

why is the position of the ion in the crystal important

A

where the attractive forces are

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43
Q

what happens when you displace ionss

A

charges come closer together

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44
Q

what do covalently bounded atoms make

A

a molecule

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45
Q

what is another name for a covalent bond

A

molecular compound

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46
Q

what is bond length

A

equilibrium distance between the nuclei of two groups or atoms that are bonded to each other.

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47
Q

what are some properties of covalent bonds

A

○ Low melting and boiling points
○ Found in all 3 states at room temperature
○ Breaks attractions between molecules but not the bond
○ Strong covalent bonds within the molecules, weaker intermolecular between molecules

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48
Q

what is a polar covalent bond

A

Covalent bond where electrons are not shared equally

49
Q

When will a molecule have more electron density?

A

When one electronegative atom pulls harder on an atom that is lower in electronegativity ( the one with high electronegativity is denser)

50
Q

What is electronegativity?

A

Ability of atoms in a molecule to attract electrons to themselves

51
Q

What is the electronegativity trend for the periodic table

A

○ Decreases down a group

○ Increases across a period

52
Q

What is the most electronegative atom

A

fluorine

53
Q

• Who founded the method for determining electronegativity?

A

linus pauling ( won Nobel prize for chemistry and peace)

54
Q

What does a larger difference in electronegativity equal?

A

more polar bond

55
Q

how are the bond length and electronegativity related

A

○shorter bond length = high electronegativity difference (strong bond bc the further away two atoms are then it’s stronger)
○longer bond length = low electronegativity difference (weaker)

56
Q

What does electronegativity have to be to have a non-polar covalent bond?

A

0-0.4

57
Q

What does the electronegativity difference have to be to be a polar bond

A

0.5-1.9

58
Q

What happens if the electronegativity difference is larger than or equal to 2.0

A

ionic bond

59
Q

what does ion size depend on

A 
nuclear charge
# of electrons
orbitals in which the electrons reside
60
Q

what does a higher effective nuclear charge mean

A

A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius.

61
Q

what type of ion is smaller than the parent

A

cation

62
Q

what type of ion is larger than the parent ion

A

anion

63
Q

how does ion size increase

A

go down a column bc of the increasing n value

64
Q

what is an isoelectronic series

A

ions have the same # of electrons

65
Q

In an isoelectronic series, why is it that the ion w/ the highest charge is the smallest

A

○ Bc the nucleus exerts a stronger force of attraction and the electrons are pulled closer to the nucleus

66
Q

cation with the highest postive charge has what radius

A

smallest radius

67
Q

anion with the highest negative charge has what size radius

A

largest radius

68
Q

what do more protons mean

A

greater positive charge = small radius

69
Q

what do fewer protons mean

A

greater negative charge = large radius

70
Q

what is the trend for atomic radius

A

decreases from left to right

increases down a group

71
Q

how can you determine the formulas of ionic compounds

A

charge on cation = subscript of anion

charge on anion = subscript of anion

72
Q

what is the percent ionic character

A

no bond is 100% between discrete pairs of atoms

73
Q

what do models help with

A

explain how nature operates on a microscopic level based on experiences in the macroscopic workd

74
Q

why can models be wrong

A

oversimplified

75
Q

what is a bonding model?

A

the model that explains the stability of molecules

76
Q

what is the localized electron bonding model

A

lewis structure; assumes that a molecule is composed of atoms that are bound together by sharing electrons using the orbitals

77
Q

what are lone pairs

A

electrons that are not paried

78
Q

what is the LE model composed of

A
  • description of the VE arrangement in a molecule
  • prediction of the geometry of the molecule using the vsepr model
  • description of the type of orbitals used by the atoms
79
Q

who were lewis structures named after

A

G.N lewis

80
Q

what are valence electrons

A

outer shell electrons that are involved in chemical bonding

81
Q

what are core electrons

A

inner shell electrons

82
Q

What is the octet rule?

A

○ When atoms bond they gain, lose, or share electrons to have 8 valence electrons
○ 8 valence electrons are stable

83
Q

What does more stable atom mean?

A

Lower potential energy

84
Q

What do chemical reactions involve?

A

○ Breaking bonds in reactant molecules and making new bonds to create products

85
Q

What is the strength of a bond measured by?

A

○ How much energy is required to break the bond (bond energy)

86
Q

What happens when atoms share more electrons

A

the bond is stronger

87
Q

What does a shorter bond mean

A

The bond is stronger

88
Q

Why do we use the average bond length

A

○ Actual bond length depends on other atoms; we use the avg for similar bonds from many compounds

89
Q

what are the bond length trends

A

increases down a group (the principal number increases )

bond length decreaes left to right across a period bc getting farther away from the nucleus

90
Q

What is formal charge

A

The charge it would have if all of the bonding electrons were shared equally between the bonded atoms

91
Q

• What is the formal charge formula

A

Formal charge = # of valence electrons - # of dots in the pairs- # of bonds it sees

92
Q

• What determines the best Lewis structure

A

○ One w/ the fewest charges

Puts a negative charge on the most electronegative

93
Q

What are resonance structures used for?

A

used to describe multiple structures of a molecule

94
Q

What does a resonance structure differ in

A

The position of electrons

95
Q

• What are the exceptions to the octet rule?

A

○ Ions or molecules w/ an odd number of electrons
○ Ions or molecules w/ less than an octet
○ Ions or molecules w/ more than 8 ve

96
Q

What are odd number of electrons called

A

radicals

97
Q

what is chemical nomenclature

A

system that us used to name substances w/ common names

98
Q

how do you name ionic compounds/ bonds

A

name of cation metal = base name of anion nonmetal (ide)

ex. Nacl = sodium chloride

99
Q

what is a multivalent cation

A

metal with multiple charges

100
Q

how to name a multivalent cation

A

name of cation metal ( charge of cation in roman numeral in () ) base name of anion + ide

101
Q

what does more oxygen =

A

ate

102
Q

what does less oxygen =

A

ite

103
Q

how many oxygens do central atoms on the second row have

A

3

104
Q

how many oxygens do central atoms on the third row have

A

4

105
Q

in polyatomic ions when does the charge increase

A

when you go from left to right

106
Q

what is the rule for ammonium?

A

ammonium with a non metal ends in ide

107
Q

how to name molecular compounds / covalent compounds

A

prefix + name of 1st element + prefix + base element of second element + ide
example: NI3 = nitrogen triiodide

108
Q

what is does mono mean

A

1

109
Q

what does di- mean

A

2

110
Q

what does tri- mean

A

3

111
Q

what does tetra- mean

A

4

112
Q

what does penta-mean

A

5

113
Q

what does hexa- mean

A

6

114
Q

what does hepta- mean

A

7

115
Q

what does octa mean

A

8

116
Q

what does nona mean

A

9

117
Q

what does deca mean

A

10

118
Q

what are binary acids and what is the formula

A

contain only 2 different elements and their names
hydro + base name of nonmetal ic + acid
example: HF = hydrofluoric acid

119
Q

how to name oxyacids

A

polyatomic ion ends in ate = ic and acid
example: HNo3 = nitric acid
if it ends in ite = ous
chlorite = chlorous acid

Introduction to Chemistry (12 decks)

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