1. Atoms and Bonding
Honours

2. Revision A= Nucleus B = Protons C = Neutrons D = Electrons E =
First Shell
F =
Second Shell

3. Mass Number 12 C 6
Atomic Number

4. Drawing Atoms How many protons? Atomic Number The small number
How many electrons? Same as protons.
How many neutrons? Subtract small from large
Mass Number – Atomic Number tells us how many neutrons.

5. Drawing Atoms 1. Write down how many protons, electrons, neutrons.
2. Give out the electrons.
3. Draw the nucleus (put in protons & neutrons)
4. Draw in electrons – ones then double up
5.Check – number of dots = small number

6. Electrons Max of 2 in first shell Max of 8 in all the rest.
So “give out” the electrons like this
6 electrons = 2,4
11 electrons = 2,8,1

7. Now
Draw an atom of sodium Na23 11
Draw an atom of Chlorine Cl35 17

8. Sodium and Chlorine

9. Plus and Minus attract each other
Extra electron brings extra minus charge
Both ions have FULL outside shell– they are STABLE

10. Ionic Bonds formed

12. Magnesium & Oxygen

13. Mg and O Mg + 0  MgO Burn Mg in oxygen gas White light
White powder formed is
MgO
MgO turns litmus blue --- base

14. Ionic Bond Is the force of attraction Between oppositely charged ions
E.g. Na+ Cl- bond to form NaCl

15. Ionic Compounds Solids at room temp.
High melting points and boiling points
Soluble in water
Conduct electricity when molten or dissolved (as the ions can move and carry charge)
Fast reactions
Formed between left and right of PTE

16. RESULT
Bulb lights
Conclusion
Liquid conducts elec.
(or opposite)

17. Covalent Bond Atoms SHARE at least one pair of electrons Become STABLE
as they have FULL outside shell

18. Hydrogen (H2) Zinc + HCl Little 2 shows they are a molecule
Burns with a pop

19. Water

22. Adds to greenhouse effect
Methane CH4
In natural Gas
Adds to greenhouse effect

24. Oxygen O2
Double Bond – 2 pairs shared electrons

25. Oxygen Carried by red blood cells (haemoglobin) Used in respiration
To release energy from food (all cells)
MADE by plants in photosynthesis
MADE in lab – hyd.per and manganese dioxide
Taken in by animals and out by plants
Neutral gas
Supports combustion

26. Covalent Compounds Liquids or gases
Low melting points and boiling points
Insoluble in water
Do NOT Conduct electricity when molten or dissolved (as the ions can move and carry charge)
Slow reactions

27. Compare Ionic Solids Soluble in water Conduct High M.pt & B.pt
Fast to react
Covalent Liquids/Gas Insoluble in water Don’t conduct Low M.pt & B.pt Slow to react

28. PERIODIC TABLE Group One (Li, Na, K) Alkali Metals
One electron in outer shell – valency =one
Form positive ions – give electron away
Highly reactive – water
Stored under oil

29. Alkali Metals Same structure =same properties React with water
sodium + water  sodium hydroxide + hydrogen gas
xxxxxx + water  ……. Hydroxide + hydrogen gas
React with air
Tarnish
Form sodium oxide ( or lithium oxide etc)

30. Group Two Alkaline Earth Metals Two electrons in outer shell
Valency of 2

31. Group 7 Group 8 Halogens Noble Gases Seven electrons in outer shell
Valency = one
Cl2 and F ions in water treatment
Noble Gases
Eight electrons in outer shell
Valency = zero
STABLE
Unreactive
(role model for all the others – they want to be like nearest Noble gas)