Names and Formulas

Ionic Compounds
◦ Binary Main Group M & NM
◦ Using Polyatomic ions
◦ Transition metals with variable charges

Covalent Compounds
◦ Names & Formulas
NC Essential Standards

1.2: Understand the bonding that occurs in simple
compounds in terms of bond type, strength and
properties.
◦ 1.2.1: compare the relative strength of ionic, covalent, and
metallic bonds
◦ 1.2.2: Infer the type of bond and its chemical formula formed
between atoms
◦ 1.2.3: Compare inter- and intra- particle forces.
◦ 1.2.4: Interpret the name and formula of compounds using the
IUPAC convention
◦ 1.2.5: Compare the properties of ionic, covalent, metallic, and
network compounds.
Language of chemistry:
Standardize system to represent compounds
Inorganic
Compounds
Covalent
(molecules)
Ionic
M&
NM
With
Roman
numeral
3 or
more
elements
NM &
NM
Diatomic
Molecules
Acids
Inorganic
Compounds
Covalent
(molecules
)
Ionic
Binary representative
metals
Transition &
post transition
metals
Formulas
Formulas
Names
Names
Polyatomic
ions
Binary
Diatomic
molecules
Acids
Formulas
Formulas
Formulas
Formulas
Names
Names
Names
Names
Binary Ionic Compound with
Representative Metals
Example: Chlorine and magnesium
 Rules for formula

◦ Metal (cation)1st NM (anion) 2nd
◦ Change number of each until charges = 0
◦ Subscripts tell the number of atoms/moles

Rules for names:
◦ Metal 1st – metal’s element name
◦ NM 2nd – change ending to “-ide”
◦ No prefixes
Ionic compounds with polyatomic ions

Rules for formulas
◦
◦
◦
◦

Cation 1st Anion 2nd
Use parentheses around the polyatomic ion
Change number of each ion until charges = 0
Check polyatomic ion: name, formula & charge
Rules for Names
◦ Cation 1st Anion 2nd
◦ Be careful about the ending (“-ate”, etc.)
◦ No prefixes
Using polyatomic ions:
Sodium + nitrate
Formula
Name:
Ammonium + nitride
NAME
FORMULA
Common Polyatomic Ions
Nitrate
NO₃⁻¹
CHARGE
-1
Acetate
C₂H₃O₂⁻¹
-1
Carbonate
CO₃⁻²
-2
Sulfate
SO₄⁻²
-2
Phosphate
Hydroxide
PO₄⁻³
OH ⁻¹
-3
-1
Ammonium
NH⁺¹
+1
Memorizing polyatomic ions
Nick the Camel ate a clam for supper in
Phoenix
 http://www.youtube.com/watch?v=TZgv2
1FmEzk&list=PLs9HjZz1-dAB_gUIJJOhAu1Rrvaa56J6

Criss – Cross method

Use the charges (oxidation numbers) to help
determine the number of atoms (moles)
Al⁺³(CO₃⁻²)
Check if it the smallest (simplest) ratio
Writing Formulas (criss –cross method)
selected examples from worksheet
Cl¹⁻ CO₃²⁻ OH¹⁻ SO₄²⁻ PO₄³ NO₃¹⁻
⁻
Na⁺¹
NH₄⁺¹
K⁺¹
Ca⁺²
Mg⁺²
Ionic Compounds with Transition Metals






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=
Transition metals

Examples
Iron II oxide
Iron III oxide
Write the formulas for:
Copper I oxide
Cobalt III chloride
Tin IV sulfide
Note: Check for the smallest (simplest) ratio
Writing Formulas (criss –cross method)
selected examples from worksheet
Cl¹⁻ CO₃²⁻ OH¹⁻ SO₄²⁻ PO₄³ NO₃¹⁻
⁻
Zn⁺²
Fe⁺³
Co⁺³
Fe⁺²
Formula Writing Practice – selected examples
Sulfide
Mercury II
Iron III
Iron II
Sulfate
Oxide
Carbonate
Language of chemistry:
Standardize system to represent compounds
Inorganic
Compounds
Covalent
(molecules)
Ionic
M&
NM
With
Roman
numeral
3 or
more
elements
NM &
NM
Diatomic
Molecules
Acids
Inorganic
Compounds
Covalent
(molecules
)
Ionic
Binary representative
metals
Transition &
post transition
metals
Formulas
Formulas
Names
Names
Polyatomic
ions
Binary
Diatomic
molecules
Acids
Formulas
Formulas
Formulas
Formulas
Names
Names
Names
Names
Inorganic Covalent Compounds
Names & Formulas

Binary

Diatomic

Acids
Note: Organic compounds different naming
system
Inorganic
Compounds
Covalent
(molecules)
Ionic
Binary
Main metals
Transition
metals
Polyatomic
ions
Binary
Diatomic
Acids
Inorganic covalent compounds
Earth’s atmosphere
Names of Binary Molecules


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
Practice:
Complete the table in your notes.
 Write the names


Write the formula
Acids
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:
Acids: H + Halogen
Hydro + Halogen (ic) + Acid
 HBr
 Hydrobromic acid

Oxyacids: common acids

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 =

7 Diatomic Molecules

Heck
No
Halogens

Named with the element name
Common Names for 3 Molecules
Molecular name and formula: common name
 Dihydrogen monoxide =
 Carbon tetrahydride =
 Nitrogen trihydride =
Methane: CH₄
Ammonia: NH₃
Water: H₂0