writing and naming chemical formulas

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Writing and Naming Chemical Formulas and CompoundsWriting and Naming Chemical Formulas and Compounds

I. Binary Compound – Compounds of 2 elements 1. Ionic Compounds – Metal + Non-MetalRule in Naming: Give the name of the 1st element followed by the second element ending in –ide.2. Covalent Compounds – Non-Metal + Non-metalRule in Naming: Use the Greek prefixes

1 – mono 6 - hexa 2 – di 7 - hepta3 – tri 8 - octa4 – tetra 9 - nona5 – penta 10 – deca

3. Metallic Compounds – Metals with variable oxidation numbers

Metal Classical Name

Stock System

CopperCu+1 Cuprous Copper (I)Cu+2 Cupric Copper (II)

LeadPb+2 Plumbous Lead (II)Pb+4 Plumbic Lead (IV)

MercuryHg+1 Mercurous Mercury (I)Hg+2 Mercuric Mercury (II)

PlatinumPt+2 Plantinous Platinum (II)Pt+4 Platinic Platinum (IV)

TinSn+2 Stannous Tin (II)

Sn+4 Stannic Tin (IV)

AntimonySb+3 Stibious Antimony (III)Sb+5 Stibic Antimony (V)

GoldAu+1 Aurous Gold (I)Au+3 Auric Gold (III)

Nickel Ni+2 Nickelous Nickel (II)Ni+3 Nickelic Nickel (III)

IronFe+2 Ferrous Iron (II)Fe+3 Ferric Iron (III)

4. Hydrogen + Non-metal = acid without oxygenEx.: H+1 + S-2 = Hydrosulfuric Acid

II. Ternary Compounds – compounds of 3 elements Polyatomic ions – are composed of more than 2 elements but behave like single ions. (Metals +

Polyatomic ions)

NH4+1 Ammonia

CO3-2 Carbonate

HCO3-1 BicarbonateClO-1 Hypochlorite

ClO2-1 Chlorite

ClO3-1 Chlorate

ClO4-1 Perchlorate

NO2-1 Nitrite

NO3-1 Nitrate

SO3-2 Sulfite

SO4-2 Sulfate

PO3-3 Phosphite

PO4-3 Phosphate

CrO4-2 Chromate

Cr2O7-2 Dichromate

C2O4-2 Oxalate

MnO4-1 Permanganate

Mn03-1 Manganate

Mn02-1 Manganite

OH-1 Hydroxide

BrO-1 Hypobromite

BrO2-1 Bromite

BrO3-1 Bromate

BrO4-1 Perbromate

IO-1 Hypoiodite

IO2-1 Iodite

IO3-1 Iodate

IO4-1 Periodate

1. Metal + Polyatomic Ion: Na+1 + OH-1 = NaOH or Sodium HydroxideMg+2 + NO3

-1 = Mg(NO3)2 or Magnesium Nitrate 2. Hydrogen + Polyatomic Ion: Non-metal + Polyatomic = Hydrogen + Polyatomic

H+1 + SO4-2 = H2SO4 or Sulfuric Acid

H+1 + NO2-1 = Nitrous Acid

3. Metal + Hydroxide = Base Na+1 + OH-1 = NaOH or Sodium HydroxideMg+2 + OH-1 = Mg(OH)2 or Magnesium Hydroxide

What is a Chemical Equation?What is a Chemical Equation?

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It is a shorthand way of writing chemical reactions using symbols and formulas Ex: Hydrogen + Oxygen Water

H2 + O2 H2O

Parts of a Chemical Equation1. Reactant – left side 2. Products – right side3. (+) – b/w the compound or element4. / = - separate the reactant from the product

5. (reversible arrows) – describe either the reactant or product 6. Symbols – used to describe the physical property of an element

a. (g) or - gasb. (s) or - solidc. (l) or __ - liquid

d. (aq) – aqueous or water solutione. ∆ - heat

Types of Chemical Reaction1. Combination – A + B = AB2. Decomposition – AB = A + B3. Single Replacement – A + BC = AC + B4. Double Replacement - AB + CD = AD + CB

How to Balance Chemical EquationsHow to Balance Chemical Equations

BY INSPECTION or TRIAL AND ERROR BY REDUCTION – OXIDATION (REDOX) REACTION

The Reduction – Oxidation ReactionThe Reduction – Oxidation Reaction loss and gain of electrons

Oxidation – Loss of electrons and the adition of oxygen- Attain in a more (+) oxidation number

Reduction – gain of electrons and removal of oxygen- Attain in a more (-) oxidation number

The element that is oxidized means addition of oxygen or reducing agent The element that is reduced is called the oxidizing agent

StoichiometryStoichiometry

It refers to the measurement based on a balanced chemical equation

1. Formula Mass - total mass of an element in a compound in amu2. Molecular Mass – refers to a mass of an molecule/covalents in amu3. Molar Mass – refers to the formula mass in grams

Moles = mass in grams/molecular mass

4. Percentage Composition – percent per 1005. Empirical Formula – based on % composition and molecular mass or the simplest formula6. Molecular Formula – true formula of a compound

Date: December 9, 2007Re: C:\Documents and Settings\Carlo Joseph\My Documents\Chemistry.docFile Name: Chemistry.doc