1. Reflecting on bonding
Brainstorm everything you already know about bonding.
You have one minute

2. Lesson 1
Ionic Bonding

3. Lesson 1: Ionic Bonding Objectives:
Reflect on prior knowledge of bonding
Refresh knowledge and understanding of ionic bonding

4. Homework Research and make notes on metallic bonding. Including:
Description of the nature of the metallic bond
Factors affecting the strength of metallic bonds
Explanation of the malleability of metals
Explanation of the electrical conductivity of metals
Factors affecting the conductivity of metals

5. Overview

6. Recapping ionic bonding
An ionic bond is:
The electrostatic attraction between two oppositely charged ions
sodium fluoride lithium oxide
Ionic bonds typically form between a metal and a non-metal
Ionically bonded compounds are often referred to as salts
Na+ F-
Li+
O2-

7. Formation of simple ions
Positive ions (cations)
Positive ions are formed when metals lose their outer shell electrons
Group 1: Li  Li+ + e-
Group 2: Ca  Ca2+ + 2e-
Group 3: Al  Al3+ + 3e-
Transition metals – form multiple different ions
Fe  Fe2+ + 2e-
Fe  Fe3+ + 3e-
Negative ions (anions)
Negative ions are formed when non-metals gain enough electrons to complete their outer shells
Group 5: N + 3e-  N3-
Group 6: O + 2e-  O2-
Group 7: F + e-  F-

8. Polyatomic ions
Many ions are made of multiple atoms with an overall negative charge
The negative ones are mostly acids that have lost their hydrogen(s)
You need to know about:
Sulphate, SO42-
Phosphate, PO43-
Nitrate, NO3-
Carbonate, CO32-
Hydrogen carbonate, HCO3-
Ethanoate (acetate), CH3CO2-
Hydroxide, OH-
Ammonium, NH4+

9. The formula of ionic compounds
Ionic compounds are always neutral, so the charges must balance
Example 1: calcium reacting with fluorine:
Calcium forms Ca2+, fluorine forms F-
The formula is CaF2 so two F- charges cancel the one Ca2+
Example 2: iron (II) reacting with phosphate
Iron (II) is the Fe2+ ion, phosphate is PO43-
The formula is Fe3(PO4)2
The 6+ charges from iron (2+ x 3) balance the 6- charges (3- x 2) from phosphate
Look for the lowest common multiple
Ionic compounds do not form molecules so these are always empirical formulae

10. The names of ionic compounds
The cation gives the first part of the name
Normally a metal except in the case of ammonium (NH4+)
In the case of transition metals, Roman numerals tell you the charge on the metal ion
The anion gives the second part of the name
Simple ions: ‘-ide’…e.g. chloride, fluoride, nitride etc
Complex ions: just their name: sulphate, phosphate etc
Note: the ‘-ate’ ending usually refers to polyatomic ions containing oxygen, which provides the negativity…more on this in the redox unit
Examples:
CaF2: calcium fluoride
Fe3(PO4)2: iron (II) phosphate

11. Your turn
Deduce the formulae and names of the ionic compounds formed between:
Lithium and fluorine
Magnesium and iodine
Aluminium and oxygen
Iron (II) and sulphur
Calcium and nitrogen
Sodium and sulphate ions
Chloride and ammonium ions
Iron (III) and sulphate ions
Iron (II) and nitrate ions
Potassium and carbonate ions
Work through the simulation here:

12. Key Points
Ionic bonds are the attraction between two oppositely charged ions
Ionic bonds form between metals and non metals
Metals lose their outer shell
Non-metals complete their outer shell
The number of each ion in the formula is determined by the lowest common multiple of their charges