Unit 5 Bonding and Nomenclature

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lithium nitrate
lead (II) sulfide
Outline
barium sulfide
lithium nitride
Chemistry
lithium nitrite
sulfur dioxide
Unit 5 Bonding and Inorganic Nomenclature
NO2
NaClO3
Fe(ClO3)2
N2O4
Fe(ClO3)3
N2O5
PowerPoint Presentation by Mr. John Bergmann
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Chemical Bonding
Ionic Bonds atoms give up or gain e and
are attracted to each other by coulombic
attraction
Na
Na1
Cl
Cl1
NaCl
ionic compounds salts
KNO3
where NO31 is a polyatomic ion
a charged group of atoms that stay together
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Properties of Salts
1. very hard
each ion is bonded to several oppositely -charged
ions
2. high melting points
many bonds must be broken
with sufficient force, like atoms are brought
next to each other and repel
3. brittle
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Covalent Bonds
atoms share e to get a full valence shell
C
1s2 2s2 2p2
(4 v.e)
1s2 2s2 2p5
(7 v.e)
F
both need 8 v.e for a full outer shell (octet
rule)
Lewis structure
a model of a covalent molecule that shows all of
the valence e
1. Two shared e make a single covalent
bond, four make a double bond, etc.
2. unshared pairs pairs of unbonded valence e
3. Each atom needs a full outer shell, i.e., 8
e.
Exception H needs 2 e
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carbon tetrafluoride (CF4)
methane (CH4)
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nitrogen triiodide (NI3)
carbon dioxide (CO2)
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covalent compounds molecular compounds
-- have lower melting points than do ionic
compounds
(consist of two nonmetal elements)
butter
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Metallic Bonds
In metals, valence shells of atoms overlap, so
v.e are free to travel between atoms through
material.
In insulators (like wood), the v.e are
attached to particular atoms.
Not so in metals.
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Properties of Metals
All due to free-moving v.e.
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• Other Types of Bonds

dipole-dipole forces
hydrogen bonds
London dispersion forces
ion-dipole forces
These are much weaker than ionic, covalent, or
metallic bonds, but very important in determining
states of matter, boiling and melting points, and
molecular shape (among other things).
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Writing Formulas of Ionic Compounds
chemical formula
shows types of atoms and how many of each
To write an ionic compounds formula, we need
1. the two types of ions
(i.e., pink and blue)
2. the charge on each ion
NaF
Na1 and F1
BaO
Ba2 and O2
Na1 and O2
Na2O
BaF2
Ba2 and F1
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charge on cation / anion becomes
subscript of anion / cation
criss-cross rule
Warning
Reduce to lowest terms.
Al3 and O2
Ba2 and S2
In3 and Br1
Al O
Ba S
In Br
InBr3
Al2O3
BaS
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• Writing Formulas w/Polyatomic Ions

Parentheses are required only when you need
more than one bunch of a particular polyatomic
ion.
Ba2 and SO42
BaSO4
Mg2 and NO21
Mg(NO2)2
NH41 and ClO31
NH4ClO3
Sn4 and SO42
Sn(SO4)2
Fe3 and Cr2O72
Fe2(Cr2O7)3
NH41 and N3
(NH4)3N
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Inorganic Nomenclature
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• Ionic Compounds (cation/anion combos)

Single-Charge Cations with Elemental Anions
The single-charge cations are
groups 1, 2, 13, and Ag1, Cd2, and Zn2
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A. To name, given the formula
1. Use name of cation.
2. Use name of anion (it has the ending ide).
sodium fluoride
NaF
BaO
barium oxide
sodium oxide
Na2O
barium fluoride
BaF2
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1. Write symbols for the two types of ions.
2. Balance charges to write formula.
Ag1
S2
Ag2S
silver sulfide
zinc phosphide
Zn2
P3
Zn3P2
I1
Ca2
CaI2
calcium iodide
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Multiple-Charge Cations with Elemental Anions
The multiple-charge cations are
Pb, Sn, and the transition elements (but of
course! not Ag, Cd, or Zn)
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A. To name, given the formula

• Figure out charge on
• cation.

2. Write name of cation.
3. Write Roman numerals in ( ) to show
cations charge.
Stock System of nomenclature
4. Write name of anion.
iron oxide
FeO
Fe?
O2
iron (II) oxide
Fe2
Fe2O3
iron oxide
Fe?
O2
iron (III) oxide
Fe?
O2
O2
Fe3
Fe3
CuBr
copper bromide
Cu?
Br1
copper (I) bromide
Cu1
CuBr2
copper bromide
Cu2
Br1
copper (II) bromide
Br1
Cu?
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B. To find the formula, given the name
1. Write symbols for the two types of ions.
2. Balance charges to write formula.
cobalt (III) chloride
Co3
Cl1
CoCl3
Sn4
O2
SnO2
tin (IV) oxide
tin (II) oxide
O2
Sn2
SnO
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Compounds Containing Polyatomic Ions
Insert name of ion where it should go in the
compounds name.
Write formulas
iron (III) nitrite
Fe3
NO31
Fe(NO3)3
iron (III) nitrite
ammonium phosphide
ammonium phosphide
NH41
P3
(NH4)3P
ammonium chlorate
ammonium chlorate
NH41
ClO31
NH4ClO3
zinc phosphate
zinc phosphate
Zn2
PO43
Zn3(PO4)2
lead (II) permanganate
lead (II) permanganate
Pb2
MnO41
Pb(MnO4)2
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Write names
(NH4)2S2O3
(NH4)2S2O3
ammonium thiosulfate
AgBrO3
AgBrO3
silver bromate
(NH4)3N
(NH4)3N
ammonium nitride
CrO42
U?
uranium (VI) chromate
U6
U(CrO4)3
U(CrO4)3
CrO42
CrO42
Cr2(SO3)3
Cr2(SO3)3
Cr?
Cr3
SO32
chromium (III) sulfite
Cr?
Cr3
SO32
SO32
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Covalent Compounds
-- contain two types of
nonmetals
nonmetals
Key
FORGET CHARGES!
Use Greek prefixes to indicate how many atoms of
each element, but dont use mono on first
element.
hexa
mono
di
hepta
tri
octa
tetra
nona
penta
dec
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EXAMPLES
CO2
carbon dioxide
carbon monoxide
CO
dinitrogen trioxide
N2O3
dinitrogen pentoxide
N2O5
CCl4
carbon tetrachloride
nitrogen triiodide
NI3
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Dihydrogen Monoxide A Tale of Danger and
Irresponsibility
-- major component of acid rain
-- found in all cancer cells
-- inhalation can be deadly
-- excessive ingestion results in acute physical
symptoms
e.g., frequent urination, bloated
sensation, profuse sweating
-- often an industrial byproduct of chemical
reactions dumped wholesale into rivers and lakes
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Traditional System of Nomenclature
used historically (and still some today) to
name compounds w/multiple-charge cations
1. Use Latin root of cation.
To use
2. Use -ic ending for higher charge
-ous ending for lower charge.
3. Then say name of anion, as usual.
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Element Latin root -ic -ous gold,
Au aur- Au3 Au1 lead, Pb plumb- Pb4 Pb2
tin, Sn stann- Sn4 Sn2 copper,
Cu cupr- Cu2 Cu1 iron, Fe ferr- Fe3 Fe2
Write formulas
Write names
P3
P3
cuprous sulfide
Pb3P4
cuprous sulfide
Pb3P4
Pb?
Pb4
Pb?
Pb?
Pb4
Pb4
P3
P3
plumbic phosphide
Cu1
S2
Cu2S
auric nitrite
Pb3P2
auric nitrite
Pb3P2
Pb?
Pb2
Pb?
Pb?
P3
P3
Pb2
Pb2
plumbous phosphide
Au3
NO21
Au(NO2)3
OH1
ferrous fluoride
Sn(OH)4
ferrous fluoride
Sn(OH)4
OH1
OH1
Sn4
Sn?
OH1
stannic hydroxide
Fe2
F1
FeF2
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Empirical Formula and Molecular Formula
Compound Molecular Formula Empirical Formula
glucose C6H12O6
propane C3H8
butane C4H10
naphthalene C10H8
sucrose C12H22O11
octane C8H18
CH2O
C3H8
C2H5
C5H4
C12H22O11
C4H9
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0
0
30
0
0
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KEYS - Nomenclature
Objectives
Worksheet - binary cmpds single charge cation
Worksheet - binary compounds
Worksheet - ions in chemical formulas
Worksheet - ions in chemical compounds
Worksheet - ionic cmpds polyatomic ions w
multiple-charge cation
Worksheet - ionic formulas (binary, polyatomic,
transition)
Worksheet - empirical and molecular
Worksheet ionic cmpds traditional system of
nomenclature
Worksheet - vocab (bonding)
Worksheet - covalent binary cmpds non-metal -
non-metal
Worksheet - ionic cmpds polyatomic ions
Activity bonding PP
Worksheet - ionic binary cmpds multiple charge
cation
Activity - molecular models
Worksheet - errors in chemical formulas and
nomenclature
activity - mole pattern
Worksheet - oxidation numbers and ionic cmpds
Textbook - questions
Worksheet - names and formulas of cmpds
Outline (general)
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Resources - Nomenclature
Objectives
Worksheet - binary cmpds single charge cation
Worksheet - binary compounds
Worksheet - ions in chemical formulas
Worksheet - ions in chemical compounds
Worksheet - ionic cmpds polyatomic ions w
multiple-charge cation
Worksheet - ionic formulas (binary, polyatomic,
transition)
Worksheet - empirical and molecular
Worksheet - traditional system of nomenclature
Worksheet - vocab (bonding)
Worksheet - covalent binary cmpds non-metal -
non-metal
Worksheet - ionic cmpds polyatomic ions
Activity - bonding pieces
Worksheet - ionic binary cmpds multiple charge
cation
Activity - molecular models
Worksheet - errors in chemical formulas and
nomenclature
Activity - mole pattern
Worksheet - oxidation numbers and ionic cmpds
Textbook - questions
Worksheet - names and formulas of cmpds
Outline (general)