Nomenclature

Cations

Alkalai = +1

Alkaline Earth = +2

Transition/Post Transition Metals

(ion charge)

Anions 

End in ide

Periodic Table and Ion Formation

Binary Ionic Formation

• Figure out charge

• Figure out number that makes charges equal

• Put how that number small

When writing names…

If it is a transition metal make sure to put roman numerals

Roman Numerals

When writing formulas with polyatomic ions….

If the there is a charge - outside the ()

If there is no charge - no ()

Determining the oxidation number for transition/post transition metals: Steps

1. Put polyatomic Ions in ()

2. Write in charges for the anion

3. Multiply the anion charge by the subscript 

4. Divide by the subscript for the cation

Determining the oxidation number for transition/post transition metals: Physical description

Naming Binary Molecular Compounds: 1

mono (Expect the first element, then it does not change)

Naming Binary Molecular Compounds: 2

di

Naming Binary Molecular Compounds: 3

tri

Naming Binary Molecular Compounds: 4

tetra

Naming Binary Molecular Compounds: 5

penta

Naming Binary Molecular Compounds: 6

hexa

Naming Binary Molecular Compounds: 7

hepta

Naming Binary Molecular Compounds: 8

octa

Naming Binary Molecular Compounds: 9

nona

Naming Binary Molecular Compounds: 10

deca

Ionic formula

metal and nonmetal or Ammonium and non-metal

Canceling Out

Molecular formula

2 Non-metal, only sharing electrons

Prefixes

Naming acids:  Acids without oxygen

Hydro____ic acid

Naming acids: oxyacids stemming from ate ions

____ ic acid

Naming acid: oxyacids stemming from ite ions

____ous acid

If it begins with a metal

IONIC, uses charges, no prefixes

If it begins with a non-metal other than H

Molecular, use prefixes, no charges

If it begins with H 

Use acid naming system 

Rules for naming molecular compounds

1. First element: decide element nam

2. Second element: start with ide name 

3. Use prefixes to show how many atoms each type there are

4. Don’t use mono on the first element

5. If you have “ao” or “oo” turn it into o

Acid

A compound in which 1 or more H ions are bonded to a negative ion. Name of acid is based on the name of the negative ion

NH⁺₄

Ammonium

NO^-₂

Nitrite

Nitrite

NO^-₂

Ammonium

NH⁺₄

NO^-₃

Nitrate

Nitrate

NO^-₃

OH^-

hydroxide

hydroxide

OH^-

SCN^-

thiocyanate

thiocyanate

SCN^-

cyanide

CN^-

CN^-

cyanide

permanganate

MnO^-₄

MnO^-₄

permanganate

hydrogen carbonate (bicarbonate)

HCO₃^-

HCO₃^-

hydrogen carbonate (bicarbonate)

hypochlorite

CIO^-

CIO^-

hypochlorite

CIO^-₂

chlorite

chlorite

CIO^-₂

CIO^-₃

chlorate

chlorate

CIO^-₃

CIO^-₄

perchlorate

perchlorate

CIO^-₄

C₂H₃O₂^-

acetate

acetate

C₂H₃O₂^-

CO₃^2-

Carbonate

Carbonate

CO₃^2-

sulfite

SO₃^2-

SO₃^2-

sulfite

SO₄^2-

sulfate

sulfate

SO₄^2-

O₂^2-

peroxide

peroxide

O₂^2-

CrO₄^2-

chromate

chromate

CrO₄^2-

Cr₂O₇^2-

dichromate

dichromate

Cr₂O₇^2-

PO₄^3-

phosphate

phosphate

PO₄^3-

PO₃^3-

phosphite

phosphite

PO₃^3-

Aluminum ion

Al⁺³

Sliver ion

Ag⁺¹

Zinc Ion

Zn⁺²

Cadmium ion

Cd⁺²

Formula unit vs formula

Unit - Ionic compound only

Formula - Ionic or covalent

Draw with dot diagram

Dot diagram is dots in valence electrons (s + p)

Type 1 vs Type 2 metal

Type 1 - One charge

Type 2 - More than one charge (transition metals)

Diatomic elements

Hydrogen, Nitrogen, Fluoride, Oxygen, Iodide, Chlorine, bromine

Sulfur root and Phosphours 

SulfurEND 

PhosphEND - not acid

PhosphorEND - acid

Ionic Bond

Electrostatic attraction between oppositely charged ions in a chemical compound

Lewis Diagram for Ionic Compound: Steps

• Identify elements

• Identify valence electrons

• Draw valence electrons around each element

• Show metal transferring electrons until it has 0

• Show nonmetal with 8 electrons

• Write with ion charged

• Enclose anions with Brackets

Lewis Diagrams for Ionic Compound

What does ionic bonds look like IRL

Crystal Lattice Structure

Crystal Lattice Structure

Covalent Bonds

Attraction between 2 nuclei for a shared pair of electrons; there electronegativity differences between the atoms

Nonpolar covalent Bond

• Very similar electronegativity

• Electrons are shared equally

Nonpolar covalent bond/pure covalent; Electronegativity difference

< 0.4

Polar covalnt bond

• Small differences in electronegativity

• Electrons are more likely to be found near the more electronegative element

Polar covalent bond: Electronegativity difference

between 0.4 and 1.8

Ionic bond

• Electrons are fully with more electronegative element

Ionic bond: electronegativity difference

>1.8

Electronegativity differences: Periodic table

Steps to Nonpolar and Covalent Bonds

• Subtract 2 elements

• Figure out bonds

• If there is an cation and anion: positive goes to negative arrow

Nonpolarand Polar Covalent bonds: Picture

Octet rule

Elements bond in order to have 8 electrons in their router shell: NONMETAL ONLY

1 bond line

2 electrons

Exceptions for Octet Rule

H forms 1 bond only and B can form 3 bonds (or 4)

Diatomic Elements: Octet Rule