1. Alkali Metals – Group 1

2. Demonstration

3. Group 1
1 electron in outer shell
Similar reactivity

4. Alkali Metals Are soft grey metals at room temperature
Have one electron in the outer shell so all react in a similar way
Get more reactive down the group
Use page to write down word and symbol equations for the reactions of sodium with:
Oxygen
Chlorine
Water
C2.19c Worksheet
Answer questions 1-5 page 26+27
Worksheet is suitable for foundation

5. Halogens – Group 7

9. Demonstration
Fluorine:

10. The halogens all have _________ electrons in their outer shell.
The halogens are non-metals and consist of molecules made of pairs of atoms (e.g. Br2).
The formula for chlorine is:
The formula for iodine is:
In Group 7, the further down the group an element is the higher its m_______________ n______________, m___________ point and b_____________ point.
In Group 7, the reactivity of the elements ______________ going from fluorine to iodine
Copy the equation to show the reaction between fluorine and hydrogen on page 28
Describe the difference in that reaction compared to the reaction of iodine with hydrogen
Answer Q2a, 2b
Write a word and balanced symbol equation to show the reaction between iron and bromine to make iron bromide (formula is at the bottom of pg. 28)
Start reading through page 29

11. Complete the fill in the gap provided and stick in Copy the equation to show the reaction between fluorine and hydrogen on page 28 Describe the difference in that reaction compared to the reaction of iodine with hydrogen Answer Q2a, 2b Write a word and balanced symbol equation to show the reaction between iron and bromine to make iron bromide (formula is at the bottom of pg. 28) Start reading through page 29

12. Halogen reactions

13. Displacement reactions
Cl2(aq) + 2KBr(aq)  2KCl(aq) + Br2(aq) Reaction takes place as chlorine is more reactive than bromine so displaces it I2(aq) + 2KBr(aq)  no reaction as iodine is less reactive than bromine so cannot displace it Continue with questions on page 29. Skip 3b.

14. Answer all questions on page 29. Skip 3b.
Halogens boiling point worksheet – will need graph paper

15. Explaining Reactivity
Trends – lithium vs. sodium
Fluorine vs. chlorine
For the group 1 metals – the bigger the atom the easier it is to lose an electron so becomes more reactive
For the halogens – the bigger the atom the harder it is to gain an electron so becomes less reactive

16. Copy diagram from the board
State one similarity between lithium and sodium’s electrons
State one difference between lithium and sodium’s electrons
State one similarity between fluorine and chlorine’s electrons
State one difference between fluorine and chlorine’s electrons
Read the “Key Points” box page 31 and use it to help you write down three factors which affect the electrostatic attraction between the nucleus and the electrons
Answer all questions on page 31 – pay careful attention to the number of marks. Use the “key points” box and your notes to help you.
Finish all questions on page 29
Look back at page and read the section on Noble Gases

17. Noble Gases – Group 0

18. Helium periodic table of videos: https://www. youtube. com/watch

20. Write full sentence answers. Use page 25 to help
Write full sentence answers. Use page 25 to help. How is the outer shell of a Noble gas different to the outer shell of every other element? Use your glossary to define inert Explain why the Noble gases are inert How does the boiling point of the gases change from helium to radon? State what temperature you would need to cool helium down to in order to turn it into a liquid Do the same for Radon Q4 on page 25 Start Q2 and Q3 on page 34

21. Transition metals (T)

22. High melting points (except mercury) Coloured compounds Stronger and harder than alkali metals

24. Copper: https://www.youtube.com/watch?v=kop1sWzTK-I

26. Also very useful as catalysts

27. Questions 1 and 2 page 33
Question 4 page 34