Formula Writing

Formulas show both:Quantitative – how much, how many atomsQualitative – what types of elements present

3 C6H12O6 3 – coefficient, how many glucose

(3 moles)

This tells you:Quantitative(subscripts) – 6 Carbon, 12 Hydrogen and 6 Oxygen are presentQualitative – Made up of Carbon, Hydrogen and Oxygen

Types of Formulas

1. Empirical – simplest whole number ratio1. CH2O

2. Molecular (true formula)1. C6H12O6

3. Structural

4. Hydrates

1. CuSO4 5 H2O.

Formula Writing1. Sum of all oxidation numbers of any formula must = 02. work only with the metals, non-metals and polyatomic ions (table E)

CrissCross Method

K+ Cl- Mg+2 S-2 Al+3 Cl-1 Mg +2 Br -

K Cl Mg S AlCl3 MgBr2

Formula Writing1. Sum of all oxidation numbers of any formula must = 02. work only with the metals, non-metals and polyatomic ions (table E)

CrissCross Method

K+ ClO4- Mg+2 PO4

-3 Al+3 NO2-1 Mg +2 Mn04

-

KClO4 Mg3(PO4)2 Al(NO2)3 Mg(MnO4)2

Zone 1

Zone 2

Zone 3

Binary Compounds - ide

• Grp 1,2 M – NM Trans M – NM Molecular compds (Covalent NM – NM)

“Call it like you see it” “Call it like you see it” Use Prefix on 2nd NM Roman Numerals to indicate Use on first if more than 1NMNaCl FeCl2 FeCl3 1- mono, 2- di, 3-tri, 4 tetra

Name Metal – Sodium Name Metal with ox # 5- penta, 6 hexa Name the Non Metal Iron II Chloride Iron III Chloride (Chlorine) drop end add - ide CO Carbon Monoxide Sodium Chloride CO2 Carbon Dioxide

N2O5 Dinitrogen Pentoxide

Zone 1-3Zone 2-3 Zone 3-3

Zone 1

Zone 2

Zone 4

Zone 3

Ternary Compounds Zone 1-3

Zone 2-3 Zone 3-4Zone 3-3

Transition M –PI-

nm(Roman Numerals)

Cu2SO4

Copper (I) Sulfate

CuSO4

Copper (II) sulfate

Group 1,2 M –PI-

nm

Na2SO4

Sodium Sulfate

Al2(SO4)3

Aluminum Sulfate

PI + - PI -

m nm(call it like you say it)

(NH4)2SO4

Ammonium Sulfate

NH4NO3

Ammonium Nitrate

PI+ - NMm(name it like a binary –ide)

NH4Cl

Ammonium chloride

Naming AcidsBinary vs Ternary

HCl1. Always start with “Hydro”2. Name the non-metal

1. Chlorine3. Change ending to

1. - ic acid4. Name = Hydrochloric Acid

H – polyatomic ion (end in ate or ite)H – ate H- ite

Remember, you ate it and it was icky! (ate-ic) (ite-ous)H2SO4 HNO2

Sulfuric Acid Nitrous Acid

(formula always begin with H)

Types of Equations

Synthesis ( 2 to 1)A + B AB

Decomposition(1 to 2)AB A + B

Combustion(Always produces CO2 and H2OBurn reaction – need O2

C3H8 + O2 CO2 + H2O

FermentationAlways produces Alcohol and CO2

(C2H5OH + CO2)

C6H12O6 C2H5OH + CO2

Types of Equations

Single Replacement ( element-compound element

compound) Red is the Metal A + BC AC + B ***Remember Table J Activity Series Who

is the Bully?

Ca + HCl CaCl2 + H2 (g) works.

Cu + HCl N.R. Why?

AG + MgCl2 Reaction….yes or no?

Types of Equations

Double Replacement ( compound-compound compound - compound) Red is the Metal A B + C D AD + CB

HCl + NaOH NaCl + HOH

NaCl + HOH NaOH + HCl

MgCl2 + (NH4)2SO4

A Reaction will go to completion when:

1. A gas (g) is produced

2. Water is a product

3. One of the products is insoluble (does not dissolve)

Table F solubility Guidelines

Table F Solubility Guidelines for Aqueous solutions

Try these out!

• Zn + HCl ZnCl2 + H2

• NaClO3 NaCl + O2

• P4 + Cl2 PCl3

• HCl + Mg(OH)2 MgCl2 + H(OH)

• BaO + SO3 BaSO4

• Pb + AgNO3 Ag + Pb(NO3)2

• AgNO3 + Na2CrO4 Ag2CrO4 + NaNO3

What type of reactions do we see?

Balancing Equations**An equation must show conservation of both Mass and Charge

2Ca0 + O20 2Ca+2O-2

Steps to follow:1. Write the correct formula first, if needed2. Pick a start point and let it take you to the next……3. If you see water, change the formula from H2O to H(OH)4. Always work the polyatomic ions (SO4, NO3etc.) as a

whole5. Try not to deal with any odd # coefficients.

a. if present, double their value to make it even

___ Li + ___Br2 ___ LiBr

___Al + ___Cl3 ___AlCl3 ___Al2O3 ___Al + ___O2

___HgO ___Hg + ___O2

___Ca3(PO4)2 + ___H2SO4 ___Ca(SO4) + ___ H3PO4

(Combustion Reactions: Always do in this order- C,H,O)

____C3H8 + ___O2 ___CO2 + ____H2O

PRACTICE