Chemical Bond

Chemical bond force of attraction between atoms in a compound

Chemical Formula shows the elements that make up a compound & its subscript tells how many of each element

Types of Compounds Ionic compounds

metal + nonmetal

Covalent Compounds nonmetal + nonmetal

Rules for naming Ionic

Compounds

Ionic compounds are formed when a metal and nonmetal bond

Ionic Compounds Cont.

1. The first element says its name

2. The second element starts to say its name, but changes its ending to ide

Examples of Ionic Compounds Sodium + Chlorine =

Sodium ChlorideFormula: Na1Cl1

Potassium + Fluorine = Potassium Fluoride

Formula: K1F1

Rules for Subscripts in Formulas

To determine subscripts, use the element’s oxidation number

Oxidation Numbers

Group 1 alkali metals is +1 Group 2 alkali earth metals is +2 Group 13 boron group is +3 Group 14 carbon group is +4 or -4 Group 15 nitrogen group is -3 Group 16 oxygen group is -2 Group 17 halogen group is -1

Oxidation cont. The oxidation numbers cross

over to the opposite element and become subscripts

Example: (+2) (-1) Beryllium + Bromine =

Beryllium BromideFormula: Be1Br2

More examples of naming +3 -2 Aluminum + Oxygen =

Aluminum Oxide Formula: Al2O3

Common nonmetals name Oxygen → oxide Sulfur → sulfide Fluorine → fluoride Chlorine →chloride Carbon → carbide Nitrogen → nitride Hydrogen → hydride Bromine → bromide

Rules for Covalent Compounds

Covalent Compounds form when a nonmetal and nonmetal bond

Covalent Compounds cont. The first element says its

name plus has a prefix which tells the subscript

The second element has a prefix, then starts to say its name, but changes its ending to ide

Examples of Covalent Compounds

diBoron + diPhosphorous = B2P2

(mono)Carbon Tetrahydride = C1H4

Prefix names 1 mono 2 di 3 tri 4 tetra 5 penta

6 hexa 7 hepta 8 octa 9 nona 10 deca

Polyatomic ions

If a compound has more than 2 elements, then it has a polyatomic ion.

Polyatomic ions have special names and charges

See page 173

Some Polyatomic Ions (p173)

Ammonia NH4 Acetate C2H3O2

Hydroxide OH Peroxide O2

Nitrate NO3 Permanganate MnO4 Sulfate SO4 Hydrogen sulfate HSO4

Carbonate CO3 Hydrogen carbonate HCO3

Phosphate PO4 Hydrogen Phosphate HPO4

Chromate CrO4 Dichromate Cr2O7

Silicate SiO3 Hypochlorite OCl

Properties of Acids Taste sour Contain Hydrogen (H) React w/ metals to

produce Hydrogen Litmus from blue to

red

Name of Acid Formula Where Found

Acetic acid HC2H3O2 Vinegar

Boric acid H3BO3 Eyewash

Carbonic acid H2CO3 Rain water, soft drinks

Hydrochloric acid HCl Gastric juice

Citric acid H3C6H5O7 Citrus fruit

Sulfuric acid H2SO4 Batteries, acid rain

Properties of Bases Taste bitter Contain OH polyatomic Feels slippery Litmus from red to blue

Name of Base Formula Where Found

Aluminum hydroxide

Al(OH)3 Deodorants, antacids

Magnesium hydroxide

Mg(OH)2 Laxatives, antacids

Potassium hydroxide

KOH Soap, glass

Sodium hydroxide

NaOH Drain cleaner, soap making

Calcium hydroxide

Ca(OH)2 mortar