1. Topic 2 – Ionic Compounds and Analysis
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Starter:
What is an element?
What is a compound?
What is a mixture?
EXT: What do you think an ion is?

2. Sodium chloride (salt)
Compounds
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Sodium chloride (salt)
Methane
Compounds are formed when two or more elements are chemically combined. Some examples:
Glucose
2.1
Be able to demonstrate an understanding that atoms of different elements can combine to form compounds by the formation of new chemical bonds
How are these compounds formed? Let’s consider two ways – “ionic” and “covalent” bonding.
We are going to focus on ionic

3. Naming compounds
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Rule 1 – When two elements join and one is a halogen, oxygen or sulphur the name ends with ____ide
e.g. Magnesium + oxygen magnesium oxide
Sodium + chlorine
Magnesium + fluorine
Lithium + iodine
Chlorine + copper
Oxygen + iron
KBr
LiCl
CaO
MgS KF
2.5
Be able to demonstrate an understanding of the use of the endings –ide and –ate in the names of compounds

4. e.g. Copper + sulphur + oxygen Copper sulphate
Naming compounds
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Rule 2 – When three or more elements combine and one of them is oxygen the ending is _____ate
e.g. Copper + sulphur + oxygen Copper sulphate
Calcium + carbon + oxygen
Potassium + carbon + oxygen
Calcium + sulphur + oxygen
Magnesium + chlorine + oxygen
Calcium + oxygen + nitrogen
AgNO3
H2SO4
K2CO3

5. Introduction to Bonding
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Hi. My name’s Johnny Chlorine. I’m in Group 7, so I have 7 electrons in my outer shell Cl
I’d quite like to have a full outer shell. To do this I need to GAIN an electron. Who can help me?

6. Here comes a friend, Sophie Sodium
Ionic Bonding
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Here comes a friend, Sophie Sodium Na
Hey Johnny. I’m in Group 1 so I have one electron in my outer shell. I don’t like only having one electron there so I’m quite happy to get rid of it. Do you want it?
Okay - + Cl Na
Now we’ve both got full outer shells and we’ve both gained a charge which attracts us together. We’ve formed an IONIC bond.

7. Ions
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An ion is formed when an atom gains or loses electrons and becomes charged: + -
The electron is negatively charged
The proton is positively charged + +
If we “take away” the electron we’re left with just a positive charge:
2.2
Be able to describe how ionic bonds are formed by the transfer of electrons to produce cations and anions
2.3
Be able to describe an ion as an atom or group of atoms with a positive or negative charge
This is called an ion (in this case, a positive hydrogen ion, also called a cation).

8. Words – full, transfers, positively, negatively, metals, anion, stable
Ionic bonding
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This is where a metal bonds with a non-metal (usually). Instead of sharing the electrons one of the atoms “_____” one or more electrons to the other. For example, consider sodium and chlorine: Na Cl
Sodium has 1 electron on its outer shell and chlorine has 7, so if sodium gives its electron to chlorine they both have a ___ outer shell and are ______. Na +
A _______ charged sodium ion (cation)
A _________ charged chloride ion (______) Cl -
2.4
Be able to describe the formation of sodium ions, Na+, and chloride ions, Cl-, and hence the formation of ions in other ionic compounds from their atoms, limited to compounds of elements in groups 1, 2, 6 and 7
Group 1 _______ will always form ions with a charge of +1 when they react with group 7 elements. The group 7 element will always form a negative ion with charge -1.
Words – full, transfers, positively, negatively, metals, anion, stable

9. Naming Ionic compounds worksheet
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Naming Ionic compounds worksheet
Rule 1 – When two elements join and one is a halogen, oxygen or sulphur the name ends with ____ide
e.g. Magnesium + oxygen magnesium oxide
Rule 2 – When three or more elements combine and one of them is oxygen the ending is _____ate
e.g. Copper + sulphur + oxygen Copper sulphate

10. The Periodic Table
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Looking at their position in the Periodic Table and understanding their electron structure, we can predict the charge of different ions.
For example, group 1 elements all want to lose one electron so they will all form cations with a charge of +1
What type of ion (and its charge) will elements from groups 2, 6 and 7 form? H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg

11. Some examples of ionic bonds
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Magnesium chloride: Cl Mg 2+ Mg + Cl - Cl
MgCl2
Calcium oxide:
This is how you would draw ionic compounds O Ca + 2+ 2-
CaO

12. Balancing ions Some common ions:
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Some common ions:
Sodium – Na+
Potassium – K+
Magnesium – Mg2+
Ammonium – NH4+
Chloride – Cl-
Bromide – Br-
Oxide – O2-
Sulphate – SO42-
Determine the formula of these compounds:
Sodium chloride
Magnesium oxide
Magnesium chloride
Ammonium chloride
Sodium sulphate
Sodium oxide
Answers:
NaCl
MgO
MgCl2
NH4Cl
Na2SO4
NaO
2.6
Deduce the formulae of ionic compounds (including oxides, hydroxides, halides, nitrates, carbonates and sulfates) given the formulae of the constituent ions
EXT: Draw them!

13. Drawing ions and ionic compounds worksheet

14. Structure of ionic compounds
The ions in an ionic compound are arranged in a very regular way. This structure is known as a lattice structure. Why do you think they arrange themselves like this?

15. Giant Ionic Structures
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Cl-
Na+
When many positive and negative ions are joined they form a “giant ionic lattice” where each ion is held to the other by strong electrostatic forces of attraction (ionic bonds).
TASK:
Put together a ‘Chemistry for dummies’ guide on ions, ionic bonding and ionic compounds
2.7
Be able to describe the structure of ionic compounds as a lattice structure (HT only):
a) consisting of a regular arrangement of ions
b) held together by strong electrostatic forces (ionic bonds) between oppositely-charged ions

16. Giant Ionic Structures
25/04/2017
Cl-
Na+
When many positive and negative ions are joined they form a “giant ionic lattice” where each ion is held to the other by strong electrostatic forces of attraction (ionic bonds).
Reference to next lesson :If these ions are strongly held together what affect would this have on the substance’s:
Melting point?
Boiling point?
State (solid, liquid or gas) at room temperature?
2.7
Be able to describe the structure of ionic compounds as a lattice structure (HT only):
a) consisting of a regular arrangement of ions
b) held together by strong electrostatic forces (ionic bonds) between oppositely-charged ions