1. Starter Activity 04/05/2019 1) Atom 2) Element 3) Compound 4) Mixture
Match up the key words with their definitions and examples:
1) Atom
a) Made up of only one type of atom
V) Calcium Carbonate
2) Element
b) 2+ atoms joined together
W) Oxygen
3) Compound
c) Made up of 2+ different atoms joined together
X) Iron
4) Mixture
d) Smallest particle of an element
Y) Sea water
5) Molecule
e) Many atoms/compounds not joined
Z)________
Then draw particle diagrams to represent elements, mixtures and compounds.

2. Use Booklets in pack complete HWK 1
BIOLOGY HWK
Use Booklets in pack complete HWK 1
Take them home with you and bring back when HWK is due Tuesday 18th Nov…..attempt all questions.
Also see last page of booklet has progression plan so you know what’s being covered next lesson.

3. Learning Outcomes
04/05/2019
A*-B: Explain the rules related to ionic bonding and why ions form.
A/B: Understand how different atoms can join together to make new chemical compounds with new and different properties.
B/C: Describe how all substances are made up of atoms.
B/C: Describe how positive and negative ions form.
Key vocabulary: Atoms, compounds, elements, periodic table, chemical bond.

4. 04/05/2019
Particle diagrams
Examples of elements: only 1 type of atom! (On the right is an element that is a molecule, like O2)
Examples of compounds: Two or more different atoms chemically bonded together.
Examples of mixtures: different elements or compounds mixed together – not bonded!

5. Quiz: Traffic lights time!
04/05/2019
Quiz: Traffic lights time!
You’ll be shown a series of particle diagrams.
You need to hold up the colour card (red, orange or green) that represents your answer.
Think quick: only 5 seconds per diagram!
Element
Compound
Mixture

6. Question 1: Is this an element, a compound or a mixture?

7. Question 2: Is this an element, a compound or a mixture?

8. Question 3: Is this an element, a compound or a mixture?
mixture of compounds

9. Question 4: Is this an element, a compound or a mixture?
mixture of elements

10. Question 5: Is this an element, a compound or a mixture?

11. Question 6: Is this an element, a compound or a mixture?
mixture of an element and a compound

12. Question 7: Is this an element, a compound or a mixture?
mixture of elements

13. Question 8: Is this an element, a compound or a mixture?

14. Particle diagrams: In reactions!
04/05/2019
Particle diagrams: In reactions!
On your mini-whiteboards:
Draw particle diagrams to represent iron and sulfur.
Use these diagrams to show how iron sulphide, a compound, is formed (you’ll need a 3rd diagram). Fe S
FeS

15. Review: Complete the grid on a mini-whiteboard
04/05/2019
Review: Complete the grid on a mini-whiteboard
Formula
Element or compound?
How many of each element is in the molecule or compound?
MgO O2 KI
CaSO4 S8
Compound
1x Mg, 1x O
Element (Molecule)
2x O
Compound
1x K, 1x I
Compound
1x Ca, 1x S, 4x O
Element (Molecule)
8x S
Don’t forget that element symbols are either a capital letter by itself (C, S, N, O…) or is 2 letters: a capital and a lower-case letter (Mg, Cu, Fe, Zn, Cl…)

16. 04/05/2019
The atom: Helium
The mass number (sometimes called atomic mass) tells us the combined number of protons and neutrons in the nucleus of an atom.
The atomic number (sometimes called proton number) tells us the number of protons in the nucleus of an atom.
…For a neutral atom it also tells us how many electrons the atom has in electron shells in total.

17. Protons, neutrons and electrons are examples of subatomic particles.
The atom: Helium
04/05/2019
Nucleus
Neutron
(No charge)
Electron
(Negative charge)
Protons, neutrons and electrons are examples of subatomic particles.
Proton
(Positive charge)
Electron Shell

18. Charges of subatomic particles
04/05/2019
Play the YouTube clip as a recap of the revision so far.
Particle
Charge
Relative mass
Proton +1 1
Neutron
Electron -1
1/2000
For an uncharged atom: the number of protons and electrons is equal!
E.g. Carbon atom
Uncharged = 0 charge.
6 Protons = 6x+1 = +6
6 electrons = 6x-1 = -6
The +6 charge from the protons and -6 charge from electrons cancel each other out (as there’s the same number of each)!

19. Formation of ions Li+ + + + - - - = 0 + + +- - = 1+ 04/05/2019
Atoms of elements as you find them on the periodic table are neutral: Equal numbers of protons and electrons!
Sometimes, electrons can be lost or gained!
Li+
Lithium Atom
Lithium Ion
Metals, such as the lithium atom on the left, will lose electrons – they become positive ions (know as cations)
= 0
= 1+
3x p and 3x e- cancel
More p than e-

20. 04/05/2019
Formation of ions
Atoms of elements as you find them on the periodic table are neutral: Equal numbers of protons and electrons!
Sometimes, electrons can be lost or gained! F-
Fluorine Atom
Fluoride Ion
Non-Metals will gain electrons – they become negative ions (know as anions)
9x Protons = +9
9x Protons = +9
9x electrons = -9
10x electrons = -10
Cancel out: 0 charge
=9 – 10 = 1- charge

21. A reminder… Metals – Left of line Non-Metals – right of line
04/05/2019
Metals – Left of line
Non-Metals – right of line

22. Be O N Br Cs S Ar Identifying ions 04/05/2019
For the elements listed below:
State whether it is a metal or non-metal.
State whether it will gain or lose electrons.
Write the formula of its ion.
Example: Ba (Barium)
It is on the left: Metal element.
Metals lose electrons.
Group 2: Loses 2 electrons = Ba2+
Be O N Br Cs S Ar
Hint:
Metals in groups 1 and 2 (that’s the first and second columns) lose electrons equal to their group number. E.G. Sodium, Na, is in group 1. Loses 1 electron  Na+
Non-metals in groups 5, 6 and 7 gain electrons to get up to 8. E.G. Fluorine, F, is in group 7. It gains 1 electron  F-

23. Electron shells up to period 5
04/05/2019
Electron shells
In a previous lesson, you learned that electrons orbit the nucleus of an atom.
Now you’ll find out how they’re arranged around that nucleus!
Electron shells up to period 5
The black circle = the nucleus.
Each ring around the nucleus is an electron shell.
Elements have electron shells equal to their period number.
Outer electrons = group number.
Level 1: Holds up to 2 electrons.
Levels 2 and 3: Both hold up to 8.
Level 4: hold remaining electrons.
(You only need to know first 20 elements)

24. Examples of electronic structure
04/05/2019
Now you work out Phosphorus and Calcium.
Each ring around the nucleus is an electron shell.
Elements have electron shells equal to their period number.
Outer electrons = group number.
Element=Carbon: Period 2, Group 4; Electronic Config. = 2,4
Element=Phosphorus: Period 3, Group 5; Electronic Config. = 2,8,5
Element=Calcium: Period 4, Group 2; Electronic Config. = 2,8,8,2

25. Draw ions of: Sodium, beryllium and aluminium.
Drawing ions: Metals
04/05/2019
This applies for metals in groups 1, 2 and 3.
Formation of the metal cation requires the removal of the electrons in the outer shell.
For every electron lost, a positive charge forms: Li+ Mg2+
You will end up losing a shell resulting in a full outer shell of electrons (either 2 or 8, depending on which shell).
Draw ions of: Sodium, beryllium and aluminium.

26. Drawing ions: Non-Metals
04/05/2019
This applies for non-metals in groups 5, 6 and 7.
Formation of the non-metal anion requires the addition of electrons to the outer shell.
For every electron gained, a negative charge forms: F- S2-
You will end up with a full outer shell of electrons (either 2 or 8, depending on which shell).
Draw ions of: Nitrogen, oxygen and chlorine.

27. Why form ions? Noble Gas configuration
04/05/2019
Chemical reactions are based on forming the most stable chemical structure.
Atoms form ions as this results in them becoming more stable.
The Noble gases below have full outer-shells (valence shells) of electrons – this is a very stable configuration.