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Title:

1
A students work (without solutions manual) 10
problems/night.
Alanah Fitch Flanner Hall 402 508-3119 afitch_at_luc.
edu Office Hours W F 2-3 pm
2
Properties and Measurements
Property Unit Reference State Size
m size of earth Volume cm3 m Weight gram
mass of 1 cm3 water at specified Temp
(and Pressure) Temperature oC, K boiling,
freezing of water (specified Pressure) 1.6605
3873x10-24g amu (mass of 1C-12
atom)/12 quantity mole atomic mass of an
element in grams Pressure atm, mm Hg earths
atmosphere at sea level Energy, of
electrons energy of electron in a
vacuum Electronegativity F
3
Covalent bonding
Patterns in abundance suggest a. periodicity b.
preferred electronic configuration of
elements Leading to the Second Rule Everybody
wants to be Like Mike a. Ions Groups 16 and
17 gain electrons Groups 1 and 2 lose b. Other
atoms share electrons to have eight electrons
COVALENT BONDING
4
Rule 5 There are no stupid questions Rule 4
Slow me Down Rule 3 Chemists are Lazy Rule 2
Everybody wants to be a Noble Gas Rule 1
Everybody wants a partner of the opposite charge

Covalent Bonding getting to a noble gas
electron configuration by
sharing electrons
Lewis structures and the Octet Rule
Valence bond theory

Repulsion of two hydrogen atoms with their
Proton core
5
Repulsion of two hydrogen atoms with their proton
core
e
e

e
e
Repulsion is low where Electrons shield nucleus,
and where Electrons can be stabilized by
both Positive charges
Repulsion is high close where Protons see each
other
Repulsive energy

e
e
Atoms which are far apart Do not even see each
other There is no energy, repulsive Or attractive
between the two
Attractive energy
6
Repulsion of two hydrogen atoms with their proton
core
e
e

e
e
Repulsion is low where Electrons shield nucleus,
and where Electrons can be stabilized by
both Positive charges
Repulsion is high close where Protons see each
other
Repulsive energy

e
e
Atoms which are far apart Do not even see each
other There is no energy, repulsive Or attractive
between the two
Attractive energy
7
Repulsion of two hydrogen atoms with their proton
core
e
e

e
e
Repulsion is low where Electrons shield nucleus,
and where Electrons can be stabilized by
both Positive charges
Repulsion is high close where Protons see each
other
Repulsive energy

e
e
Electrons are the jelly and peanut butter
between the slices of bread (protons)
Atoms which are far apart Do not even see each
other There is no energy, repulsive Or attractive
between the two
Attractive energy
8
Repulsion of two hydrogen atoms with their proton
core
e
e

e
e
Repulsion is low where Electrons shield nucleus,
and where Electrons can be stabilized by
both Positive charges
Repulsion is high close where Protons see each
other
Repulsive energy

e
e
Atoms which are far apart Do not even see each
other There is no energy, repulsive Or attractive
between the two
Attractive energy
9
When the two hydrogen atoms are together, the
electron configuration On hydrogen Looks like?
10
When the two hydrogen atoms are together, the
electron configuration On hydrogen Looks like?
He
11
When the two hydrogen atoms are together, the
electron configuration On Hydrogen Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
12
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
13
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
14
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
The inner shell electrons do not Show
in this diagram
15
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
Only the outer-most or valence shell
electrons Show in this Lewis Dot Structure
16
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
Only the outer-most or valence shell electrons
Show in this Lewis Dot Structure
How many valence electrons?
17
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
Only the outer-most or valence shell electrons
Show in this Lewis Dot Structure
How many valence electrons? last number in
group
18
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
Only the outer-most or valence shell electrons
Show in this Lewis Dot Structure
The shared pair of Electrons covalent bond
19
When the two hydrogen atoms are together, the
electron configuration Looks like?
He
When a hydrogen atom and a fluorine atom share
electrons, the Electron configuration on
fluorine looks like?
Only the outer-most or valence shell
electrons Show in this Lewis Dot Structure
The shared pair of Electrons covalent bond
The unshared pairs of electrons are red hots
20
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
21
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Valence electrons on oxygen?
22
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Valence electrons on oxygen?
23
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Valence electrons on oxygen?
Valence electrons on hydrogen?
24
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Valence electrons on oxygen?
Valence electrons on hydrogen?
25
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
26
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
27
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
28
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Invoking Rule 2 Chemists are Lazy the diagram
above is too tedious to write out all the time
29
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Invoking Rule 2 Chemists are Lazy the diagram
above is two tedious to write out all the time
Lewis dot structure for hydroxide
30
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Invoking Rule 2 Chemists are Lazy the diagram
above is two tedious to write out all the time
Lewis dot structure for hydroxide
The single electron pair shared between the two
bonded atoms Is called a single bond It is drawn
as a line.
31
When a hydrogen atom and an oxygen atom share
valence electrons plus an Extra electron, the
electron configuration on hydrogen and oxygen
look like?
Invoking Rule 2 Chemists are Lazy the diagram
above is two tedious to write out all the time
Lewis dot structure for hydroxide
The single electron pair shaired between the two
bonded atoms Is called a single bond It is drawn
as a line.
32
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
33
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
Valence electrons on oxygen?
34
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
Valence electrons on oxygen?
35
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
Valence electrons on oxygen?
Valence electrons on hydrogen?
36
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
Valence electrons on oxygen?
Valence electrons on hydrogen?
37
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
38
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
39
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
Two shared electron pairs
40
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
Two shared electron pairs Two single bonds
41
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
When three hydrogen atoms and a nitrogen atom
share valence electrons, the electron
configuration on hydrogen and nitrogen look like?
42
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
When three hydrogen atoms and a nitrogen atom
share valence electrons, the electron
configuration on hydrogen and nitrogen look like?
Valence shell of nitrogen?
43
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
When three hydrogen atoms and a nitrogen atom
share valence electrons, the electron
configuration on hydrogen and nitrogen look like?
Valence shell of nitrogen?
44
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
When three hydrogen atoms and a nitrogen atom
share valence electrons, the electron
configuration on hydrogen and nitrogen look like?
45
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
When three hydrogen atoms and a nitrogen atom
share valence electrons, the electron
configuration on hydrogen and nitrogen look like?
46
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
When three hydrogen atoms and a nitrogen atom
share valence electrons, the electron
configuration on hydrogen and nitrogen look like?
Three pairs of shared electrons three single
bonds
47
When two hydrogen atoms and an oxygen atom share
valence electrons, the electron configuration on
hydrogen and oxygen look like?
When three hydrogen atoms and a nitrogen atom
share valence electrons, the electron
configuration on hydrogen and nitrogen look like?
48
When four hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
49
When four hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
Valence shell of carbon?
50
When four hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
Valence shell of carbon?
51
When four hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
52
When four hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
53
When four hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
54
When four hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
Two electron pairs shared is a Double bond
55
When two hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
56
When two hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
57
When two hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
58
When two hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
59
When two hydrogen atoms and two carbon atoms
share valence electrons, the electron
configuration on hydrogen and carbon look like?
Three electron pairs shared is a Triple bond
60
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (last
number of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

61
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

62
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

63
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

64
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

65
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

H can only have one bond because it can share
only one Electron. Poor H.
66
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

Halogens have lots of electrons but really do not
like to share. Greedy halogens All they want is
one more to make up the Mike configuration
67
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

68
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

69
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

70
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

71
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
bonds
a. C, N, O, S

72
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
or triple bonds
a. C, N, O, S

73
Rules for Writing Lewis Dot Structures

Count the number of valence electrons (lat number
of group) of all atoms
a. For an anion add the appropriate extra number
of electrons
b. For a cation subtract the appropriate extra
number of electrons
Draw a molecular skeleton, joining by single
bonds to the central atom.
a. The central is usually the atom written first
in the formula (N in NH4, S in SO2, and C in
CCl4).
b. The terminal atoms are usually H, O.
c. Halogens are always terminal atoms.
Determine the number of valence electrons still
available for distribution after subtracting two
electrons for each single bond.
Determine the number of electrons required to
complete the octet
a. H gets only two electrons
b. Other exceptions to be noted below
5. Fill in the region required for the octet.
Make up deficit of electrons by creating double
or triple bonds
a. C, N, O, S

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
SO2
N2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12
Hypochlorite? Hypo smallest number of oxygens
O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12 -2(6 electrons for
O,Cl) 12 remaining 0
OCl-
Valence shell electrons?
O 6 C l 7 Negative charge 1 Total
electrons 14
Skeleton
76

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12
Hypochlorite? Hypo smallest number of oxygens
O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12 -2(6 electrons for
O,Cl) 12 remaining 0
OCl-
Valence shell electrons?
O 6 Cl 7 Negative charge 1 Total
electrons 14
Skeleton
78

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12
Hypochlorite? Hypo smallest number of oxygens
O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12 -2(6 electrons for
O,Cl) 12 remaining 0
OCl-
Valence shell electrons?
O 6 Cl 7 Negative charge 1 Total
electrons 14
Skeleton
79

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12
Hypochlorite? Hypo smallest number of oxygens
O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12 -2(6 electrons for
O,Cl) 12 remaining 0
OCl-
Valence shell electrons?
O 6 Cl 7 Negative charge 1 Total
electrons 14
Skeleton
80

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

O 6 Cl 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12
Hypochlorite? Hypo smallest number of oxygens
O 6 C 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12 -2(6 electrons for
O,Cl) 12 remaining 0
OCl-
Valence shell electrons?
O 6 Cl 7 Negative charge 1 Total
electrons 14
Skeleton
81

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

O 6 Cl 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12
Hypochlorite? Hypo smallest number of oxygens
O 6 Cl 7 Negative charge 1 Total
electrons 14 -1Single bond -2
12 -2(6 electrons for
O,Cl) 12 remaining 0
OCl-
Valence shell electrons?
O 6 Cl 7 Negative charge 1 Total
electrons 14
Skeleton
82

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

O 6 C 4 4(H) 4 Negative charge
0 Total electrons 14 -5single bonds -10
remaining 4
Valence shell electrons?
O 6 C 4 4(H) 4 Negative charge
0 Total electrons 14
Octets
Carbon has its octet Hydrogen has its duet Oxygen
requires 4 more electrons
Skeleton
O 6 C 4 4(H) 4 Negative charge
0 Total electrons 14 -5single bonds -10
remaining 4 -octet for oxygen -4 remaining 0
Carbon is first in formula Hydrogen is always
terminal
84

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Octets
Each nitrogen requires 6 more
2N 10 Negative charge 0 Total
electrons 10 -1single bond -2 Remaining 8 Octet
completion -12 Difference -4
Valence shell electrons?
2N 10 Negative charge 0 Total electrons 10
Skeleton
We are short 4 electrons for the octet, The only
way to get extra ones is to Share four more
electrons triple Bond.
2N 10 Negative charge 0 Total
electrons 10 -1single bond -2 Remaining 8
Place the remaining 8 electrons equally On the
two equal nitrogens
94

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Draw Lewis structures of
Hypochlorite ion
Methyl alcohol, CH3OH
N2
SO2

Octets
2O 12 1S 6 Negative charge 0 Total
electrons 18 -2(single bonds) -4 Remaining
electrons 14 Octet for S -4 2(Octet for each
O) -12 Deficit? -2
Valence shell electrons?
2O 12 1S 6 Negative charge 0 Total
electrons 18
Skeleton, First atom in formula is central
We are short 2 electrons for the octet, The only
way to get extra ones is to Share two more
electrons double bond.
2O 12 1S 6 Negative charge 0 Total
electrons 18 -2(single bonds) -4 Remaining
electrons 14
Place the remaining 14 electrons to fill octets
114
We got this Lewis dot structure
No reason not to write instead
Which would lead to
Is there any reason for us to Presume one of
these is correct And not the other?
No
Grammar double-headed arrow is used to separate
resonance structures
115
We got this Lewis dot structure
No reason not to write instead
Which would lead to
Is there any reason for us to Presume one of
these is correct And not the other?
No
Grammar double-headed arrow is used to separate
resonance structures
116
We got this Lewis dot structure
No reason not to write instead
Which would lead to
Is there any reason for us to Presume one of
these is correct And not the other?
No
Grammar double-headed arrow is used to separate
resonance structures
117
We got this Lewis dot structure
No reason not to write instead
Which would lead to
Is there any reason for us to Presume one of
these is correct And not the other?
No
Grammar double-headed arrow is used to separate
resonance structures
118
We got this Lewis dot structure
No reason not to write instead
Which would lead to
Is there any reason for us to Presume one of
these is correct And not the other?
No
Grammar double-headed arrow is used to separate
resonance structures
119
We got this Lewis dot structure
No reason not to write instead
Which would lead to
Is there any reason for us to Presume one of
these is correct And not the other?
No
Grammar double-headed arrow is used to separate
resonance structures
120
Remember our Marshmallows?
No Clean Socks
NO3-
N 5 3(O) 18 Charge 1 Total 24 -single
bonds -6 Remaining 18 Octets (6x3 O 2 for
N) 20 Deficit of 1 electron pair
Charge is distributed over All three of the
resonance Forms one big fat marshmallow
121
Remember our Marshmallows?
No Clean Socks
NO3-
N 5 3(O) 18 Charge 1 Total 24 -single
bonds -6 Remaining 18 Octets (6x3 O

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