1. Bonding
Year 11 Chemistry

2. Intramolecular Bonding
Ionic Bonding Definition, chemical formula and nomenclature 1
Covalent Bonding Definition, chemical formula and nomenclature 2
Metallic Bonding Definition and properties 3
Comparing Bonds Bonding and structure characteristics 4
Comparing Bonds Melting and Boiling points 5
Comparing Bonds Conductivity and Density 6

3. Ions
A chemical species (ie. Element, compound or molecule) with a charge
Can form positive or negative ions
+ive ions = Cations ( the t looks like a + … Ca+ions )
–ive ions = Anions (-ives always have to be different)

4. Ion Formation A chemical species either loses or gains electrons
to attain Noble Gas Configuration or;
as a result of energy input that breaks down bonds
Example: Self-ionisation of water – enough energy to pass over the activation energy barrier (energy required to make and break bonds)
H3O+1 and OH-1
Come together to form
2H2O

5. C Ion formation- CARBON
If carbon loses an electron will it be positively or negatively charged? C

6. Formation of an ion- CARBON
If carbon loses an electron will it be positively or negatively charged? C

7. Formation of an ion- CARBON
If carbon loses an electron will it be positively or negatively charged? C

8. Formation of an ion- CARBON
If carbon loses an electron will it be positively or negatively charged? C

9. Formation of an ion- CARBON
If carbon loses an electron will it be positively or negatively charged?
What will the charge be for carbon if it loses four electrons?
[C] +4
What about if it gains four electrons?

10. This atom has lost an electron
This atom has lost an electron. Now it has one more proton than electron. One more proton means one more positive charge. This makes the total charge of the atom POSITIVE.
This atom has gained an electron. Now it has one less proton than electron.
One less proton means one less positive charge.
This makes the total charge of the atom NEGATIVE.

14. Bonding Quiz What electron interaction occurs in ionic bonding?
What electron interaction occurs in covalent bonding?
Will an ionic or covalent bond occur between Lithium and Nitrogen?
If an atom loses electrons will it be positive or negative?
When atoms share two pairs of electrons it is known as a(n) __________ bond

15. ELECTRON SHELLS WANT TO BE FULL
From Previous Lessons
ELECTRON SHELLS WANT TO BE FULL
The formation of ions occurs when atoms gain or lose electrons
Electrons can be transferred (gained or lost) to attain Noble gas configuration through ionic bonding
Electrons can be shared to attain Nobel gas configuration through covalent bonding

16. metal + non-metal = ionic bond
Ionic Bonding
The transfer of elections that result in the formation of positive and negative ions, which cause an attraction between opposite charges
metal + non-metal = ionic bond

17. Ionic Bonds
Formed between metals and non-metals with different electronegativity's
The force of attraction is the opposing charges of the ions (opposites attract)
[METALS ]+ [NON-METALS ]-

18. Ionic Bond example Cl Na
Metal Non-metal

19. Cl Na
Metal Non-metal

20. Cl Na
Metal Non-metal

21. Cl Na
Metal Non-metal

22. Electrostatic attraction exists ‘bonding’
the two together Cl Na
Positive metal ion negative non-metal
ion

23. Ionic Bonding and Transition Metals
As we know, transition metals are so called transition metals because they have the unique characteristic of being able to transition between charges
The charge of a transition metal is always given in one of two formats
By the name of the compound it forms
By its given charge

24. Ionic Bonding and Transition Metals
Name given: the charge is indicated by the roman numeral appearing after the metal name
Metals are ALWAYS positively charged ions
Example: Lead(II) oxide
Numeral is 2,
Metal means +
∴ The charge for lead in this compound in 2+

25. Ionic Bonding and Transition Metals
Charge given:
Iron 3+ and oxygen
Fe O2-
Fe2O3
Compound name given:
Iron(III) oxide
Fe3+ and O2-

26. Properties of Ionic Bonds
Solid at room temperature High melting points Non-conductors of electricity in solid form Good conductors in liquid form or dissolved in water (aqueous)

27. Naming Ionic Compounds
Metal always named first (no changes to spelling)
Non-metal named second, with an –ide suffix
When the metal is a transition metal, the charge is shown by roman numerals in parenthesis
Example: Fe3+ and O2-  Fe2O3
Fe – Iron (transition metal, charge of 3) O – Oxygen (non-metal ∴ Oxide
Iron(III) oxide

28. Name  Chemical Formula
Working back from the name
Example: Iron(II) chloride
1. Roman numeral give transition metal charge
 Fe2+
2. Chloride is chlorine, from periodic table it is 1-
 Cl-1
3. Fe+2 + Cl-1
Fe1Cl2  FeCl2
4. Iron(II) chloride  FeCl2

29. Chemical Formula  Name
Working back from the chemical formula
Example: **FeO2**
1. Reverse the crisscross to get the charges
 Fe2+ O1-
2. Multiply out the superscripts until the non-metal has the correct charge (-1 needs to be ∴ [x 2])
 Fe+2 x 2 and O-1 x 2  Fe+4 and O-2
4. FeO2  Fe+4 and O-2  Iron(IV) oxide
Does oxygen have a 1- charge?

32. Non-metal + non-metal = covalent bond
Covalent Bonding
The sharing of elections that result in the movement of electrons around two atoms
Between atoms of similar electronegativities
Between non-metals and non-metals
Non-metal + non-metal = covalent bond

33. Covalent Bonding
Equal sharing of electrons when forming the bond

34. Cl Cl

35. Cl Cl Cl

36. Cl Cl

37. Cl Cl

38. Cl Cl

39. Cl Cl

40. Naming Covalent Compounds
Highest electronegativity non-metal is listed last
Lower electronegativity non-metal is listed first
The second element is an anion ∴ -ide suffix
Prefixes are used to denote how many of each atom are present in the compound

43. Glossary
Any words to add?