REVIEW of IONS

OBJECTIVE: When atoms give away electrons

IONS

ION

What is it?An atom that

LOST/GAINEDelectron(s)

IONS

Goal is to get to the NEAREST Noble Gas

RULES

1. If you go LEFT, you become POSITIVE.

2. If you go RIGHT, you become NEGATIVE

IONS

Ions that LOSE electrons have a

POSTIVE charge

called

cations

pronounced “cat – ions”

IONS

All metals become

CATIONS

IONS

USE HALF SHEET FOR TRANSITION METALS

IONS

Ions that GAINS electrons have a NEGATIVE

charge

called

anions

pronounced “an – ions”

IONS

Ex: CN-

NH4+

CO32-

Because these ions are made from two or more atoms, they are called

polyatomic ions

Some ions are made from two or more atoms

IONS

-ite has less oxygenthan –ate

Memorize? Kind of

IONSSummary & Review1. What is an ion?

2. What are the two types of ions?

3. Which ions gains electrons: cations or anions?

4. Predict the charge of each atom if it were to become an ion:

Ca, Cl, Cu, F, Fe, Li, Na, N, O

Ionic Compounds

OBJECTIVE: Joining Cations + Anions to make compounds

Ionic Compounds

Na+ + Cl- NaCl cation anion ionic compound

forumula

NaCl joined byIONIC BOND

IONIC BOND = giving away/gaining electrons

Ionic Compounds

Li+ + Cl-

K+ + Cl-

Ca2+ + Cl-

Li+ + O2-

Ca2+ + O2-

LiCl

KCl

CaCl2

Li2O

CaOCharges must cancel and = 0

Ionic Compounds

Cu+ + CH3COO-

NH4+ + Cr2O7

-

Mg2+ + OH-

CuCH3COO

NH4Cr2O7

Mg(OH)2

Parenthesis for POLYATOMIC

Ionic CompoundsWrite formula for ionic compounds

1. Al3+ + O2- 2. Fe2+ + Cl-

3. Na+ + HCO3-

4. Na+ + NO2-

5. Ca2+ + PO43-

6. H+ + SO42-

7. Mg2+ + OH- 8. Fe3+ + Cl-

9. NH4+ + PO4

3-

1. Naming Ionic Compounds

Write from 1 to 5 in Roman Numerals

III

1. Naming Ionic Compounds

OBJECTIVE: Learn how to name compounds like NaHCO3

1. Naming Ionic Compounds

First Name + Last Name = Full Name

only TRANSITION METALS

have roman numerals

Cations with Roman Numerals in BOLD

1. Naming Ionic Compounds

1.Start with CATION, always

2.Name the anion using the suffix “IDE”. If anion is polyatomic…

1. Naming Ionic Compounds

“uncross”numbers to figure our

roman numeral forcation

FeCl3 Cr2O3

Cu2O Mn3N2

Mn(NO2)3

Mn(NO3)3

Mn(NO3)2

If no numbers then

1. Figure out charge of anion

FeO CrOMnO CoN

CrPO4 ZnCrO7

CuSO4 CuNO3

1. Naming Ionic Compounds

1.Start with CATION, always2.If cation is Transition Metal check

table for roman numerals3.Name the anion using the suffix

“IDE”. If anion is polyatomic…4.That’s it!

1. Naming Ionic Compounds

Writing formulas from names of ionic compounds

1.Write anion and charge.

2. Write cation and charge. 3. Cross charges and write formula.

-ATE -ITEhalf sheet

Naming Ionic Compounds

1. Sodium Chloride2. Lithium Fluoride3. Iron(II) Chloride4. Sodium Nitrate5. Magnesium

Hydroxide6. Sodium Acetate7. Ammonium Chloride8. Hydrogen Peroxide9. Sodium Carbonate10.Ammonium Phosphate

1. Naming Ionic CompoundsSUMMARY & REVIEW

Formula to Name1. Start with cation

2. When to use roman numerals?3. Then add…to anion

4. What about polyatomic ions?

Name to Formula5. Start with anion – LAST NAME

6. What if anion ends in ATE or ITE?7. Write symbol for cation – FIRST NAME

8. Roman numerals?

4. Lewis Dot Structures

7. Lewis Structures

1.Write elements 2. Count total number of valence

e3. LEAST electronegative is in

the center (usually CARBON)4.Draw bond5.Then draw dots until you run

out6.Make double/triple bonds if

necessary

7. Lewis Dot Structures

Exceptions to the Octet Rule

1. Less than 82. More than 8

3. Polyatomic Ions

7. Lewis Dot Structures

Exceptions to the Octet Rule

1. Less than 8

Group 1 &Beryllium and Boron

BeCl2 BCl3

4. Lewis Dot Structures

Exceptions to the Octet Rule

2. More than 8 Phosphorus ,Sulfur and

XenonPCl5 SF6 XeF4

4. Lewis Dot Structures

Exceptions to the Octet Rule

3. Polyatomic IonsCations AnionsSUBTRACT electrons

ADD electrons

add brackets [ ]