Homework: Re-write in
paragraph form – notes pages 1
and 3. Add additional
information learned in practice.
Objective: To interpret (correctly write) formulas and
names for compounds – using IUPAC convention
Warm-up: review names & formulas
Review: Binary Ionic Compounds
More Complex Ionic Compounds
With Polyatomic Ions
With Transition Metals
Covalent Compounds
Formula
MgCl₂
SO₂
PCl₃
AlBr₃
K₃N
BrO₃
H₂O
Type of Bond and
Compound
Name
Inorganic
Compounds
Covalent
(molecul
es)
Ioni
c
M&
NM
With
Roman
numeral
3 or
more
elements
NM &
NM
Diatomic
Molecules
Acids
Metals lose valence electrons
Non-metals gain valence electrons

Ionic bonding occurs when a metal loses 1 or more
electrons to a non-metal in an effort to attain a
stable octet of valence electrons.

Use Electron Dot Diagrams (Lewis diagrams) to
show the ionic bonds for one formula unit.
Na
Cl = Na⁺¹Cl⁻¹
Cl Ca Cl
= Ca Cl
Include polyatomic ions
Barite = BaSO₄
Used to make paper & glass
Source of barium used
For x-rays of the digestive
system
Gypsum = CaSO₄· 2H₂O
Used for plaster for
walls, ceilings, sculptures
Calcite = CaCO₃
Used in paint,
Antacids, calcium
Supplement for food
Calcium sulfate
in casts
Acetate uses
Barium sulfate
to absorb x-rays
Sodium
acetate
In Heat packs
Sodium hydrogen carbonate
(old name: sodium bicarbonate)
Medical: used in emergency
situations to correct pH of blood
Baking soda: to make cakes rise
Bleach
Dentistry:
Clean and disinfect
Root canals
Rocket fuels:
Source of oxygen
Examine the names & formulas:
What is the pattern? Do they end in “–ide?”
Ions with -1 charge
perbromate
BrO4-1
bromate
BrO3-1
bromite
BrO2-1
hypobromite
BrO-1
perchlorate
ClO4-1
chlorate
ClO3-1
chlorite
ClO2-1
hypochlorite
ClO-1
periodate
IO4-1
iodate
IO3-1
iodite
IO2-1
hypoiodite
IO-1
nitrate
NO3-1
nitrite
NO2-1
hydroxide
OH-1
cyanide
CN-1
thiocyanate
SCN-1
acetate
C2H3O2-1
Permanganate MnO4-1
bicarbonate
HCO3-1
Ions with a -2 Charge
carbonate
CO3-2
phthalate
C8H4O4-2
sulfate
SO4-2
sulfite
chromate
dichromate
oxalate
peroxide
SO3-2
CrO4-2
Cr2O7-2
C2O4-2
O2-2
Ions with a -3 Charge
phosphate
PO4-3
phosphite
PO3-3
arsenate
AsO4-3
Ions with +1 charge
ammonium ion NH4+1
NAME
Nitrate
Acetate
Carbonate
Sulfate
Phosphate
Hydroxide
Ammonium
FORMULA
CHARGE
Sodium + nitrate
Formula

Name:
Calcium + nitrate
Cl¹⁻
Na¹⁺
NH₄¹⁺
Zn²⁺
Co³⁺
CO₃² OH
⁻
SO₄²⁻ PO₄³⁻ NO₃¹
⁻






The transition metals are elements in Groups
_____ to _______.
+ post transition metals: under the staircase.
Transition metals can have more than one charge.
Use Roman numerals after the name.
Roman numbers:
I=
II =
III =
IV =
V=

Examples
Iron II oxide
Iron III oxide
Write the formulas for:
Copper I oxide
Cobalt III chloride
Nickel II sulfide
Sulfide
Mercury II
Iron III
Iron II
Sulfate
Oxide
Carbonate






Many transition and post transition metals have
multiple oxidation numbers (charges)
Ni: oxidation numbers of _____ & _____
Fe:
Find other examples:
Write formulas
Write names
Inorganic
Compounds
Covalent
(molecules)
Ionic
M&
NM
With
Roman
numeral
3 or
more
elements
NM &
NM
Diatomic
Molecules
Acids
Molecules
Names & Formulas for Inorganic Covalent Compounds
-Stable
-Most
atoms are bonded in compounds
-Separated
with chemical reactions
-Usually need high heat or electricity

First-element name
2nd – end in “ide”

Use prefixes

-Always with 2nd
element
-With 1st element
except mono-
Prefix
monoditritetrapentahexaheptaoctanonadeca-
Element with lowest EN goes first
On the Periodic Table – across /down
Number
1
2
3
4
5
6
7
8
9
10

Complete the table in your notes.
Write the names

Write the formula


Acids are molecules that are in aqueous solution
(_________ in __________) and produce hydrogen
ions (H¹⁺)
Typically start with H

Almost act as an ionic compound

Electronegativity Difference:



Hydro + Halogen (ic) + Acid
HBr
Hydrobromic acid

Contains oxygen (in a polyatomic ion)
◦ Note the endings of the anion & the acid name




H + nitrate = Nitric Acid
H + sulfate =
H + phosphate =
H + acetate =

Heck
No
Halogens

Named with the element name
Molecular name and formula: common name
 Dihydrogen monoxide =
 Carbon tetrahydride =
 Nitrogen trihydride =
Common elements found in the Earth's rocks.
Element
Oxygen
Silicon
Aluminum
Iron
Calcium
Sodium
Potassium
Magnesium
Chemical Percent Weight in
Symbol
Earth's Crust
O
46.60
Si
27.72
Al
8.13
Fe
5.00
Ca
3.63
Na
2.83
K
2.59
Mg
2.09
Important Minerals found in Rocks
Group
Sulfides
Halides
Oxides
Carbonates
(Nitrates and
Borates)
Sulfates
Phosphates
Silicates
Typical Minerals
Chemistry
Cinnabar
Galena
Pyrite
Fluorite
Halite
Corundum
Cuprite
Hematite
Calcite
HgS
PbS
FeS2
CaF2
NaCl
Al2O3
Cu2O
Fe2O3
CaCO3
Dolomite
CaMg(CO3)2
Malachite
Cu2(CO3)(OH)2
Anhydrite
CaSO4
Gypsum
CaSO4 -2(H2O)
Apatite
Ca5(F,Cl,OH)(PO4 )
Quartz
SiO₂
(metalloid & oxygen)
Compound Name