Chemistry valencies Yr 11

Ammonium

NH₄⁺

Hydrogen

H⁺

Potassium

K⁺

Silver

Ag⁺

Sodium

Na⁺

Calcium

Ca²⁺

Copper (II)

Cu²⁺

Iron (II)

Fe²⁺

Lead

Pb²⁺

Magnesium

Mg²⁺

Nickel

Ni²⁺

Strontium

Sr²⁺

Zinc

Zn²⁺

Aluminium

Al³⁺

Chromium

Cr³⁺

Iron (III)

Fe³⁺

Bromide

Br⁻

Chloride

Cl⁻

Cyanide

CN⁻

Dihydrogenphosphate

H₂PO₄⁻

Ethanoate (acetate)

CH₃COO⁻

Fluoride

F⁻

Hydrogencarbonate

HCO₃⁻

Hydrogensulfate

HSO₄⁻

Hydroxide

OH⁻

Iodide

I⁻

Nitrate

NO₃⁻

Nitrite

NO₂⁻

Permanganate

MnO₄⁻

Carbonate

CO₃²⁻

Chromate

CrO₄²⁻

Dichromate

Cr₂O₇²⁻

Hydrogenphosphate

HPO₄²⁻

Oxalate

C₂O₄²⁻

Oxide

O²⁻

Sulfate

SO₄²⁻

Sulphide

S²⁻

Sulfite

SO₃²⁻

Nitride

N³⁻

Phosphate

PO₄³⁻

caesium

Cs⁺

lithium

Li⁺

rubidium

Rb⁺

barium

Ba²⁺

cobalt

Co²⁺

manganese (II)

Mn²⁺

peroxide

O₂ ²⁻

ionic compound

bonding in compounds containing elements from Groups 1 or 2 of the Periodic Table combined with Groups 16 and 17 is ionic.

covalent molecular compound

• systematic naming system

• exceptions: water, hydrogen peroxide, nitrous oxide (dinitrogen monoxide), nitric acid (nitrogen monoxide), methane, ammonia, oxide

mass spectometry

Ionisation- Beams of electrons are forced into vapourised samples of atoms to form positive ions Acceleration- one positively charged (repels the ions) grid and one negatively charged (attracts the ions) grid magnetic fields that move, hence particles move towards negatively charged grid

Deflection- ions are separated into streams and the curvature depending on their mass/charge

Detection- the relative abundance of each ion detected

chemical properties

• corrosive

• flammable

physical properties

• durability

• malleability

• density

• melting and boiling properties