How does the group and period no. of an element relate to its electron configuration?
Group No. - Relates to the number of outer electrons an element has
Period No. - Relates to the total number of electrons shells an element has
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1) What group are alkali metals in?
2) What properties do they have?
3) Why are they called alkali metals?
1) Group 1
2) Soft, relatively low melting point
3) When reacting with water, they form alkaline solutions
2 of 15
General equation of alkali metal + water
alkali metal + water ---> metal hydroxide + hydrogen
3 of 15
How are alkali metals stored?
They are kept in water to prevent oxidation
4 of 15
1) What happens to their reactivity when going down group 1?
2) Why?
1) The reactivity increases
2) There are more electron shells to shield the positive nucleus and the outer electron. There is a weaker electrostatic attraction so it's easier to remove the outer electron to form a cation
5 of 15
1) What group are halogens in?
2) What is the trend going down group 7?
1) Group 7
2) F(g),Cl(g), Br(l), I(s), melting and boiling point increases. Colour gets darker. Lower reactivity
6 of 15
Explain the reason for the trends
The molecules get bigger so there are more intermolecular forces of attraction so more energy is needed to break them apart.
Lower reactivity is due to the atomic radius increasing. There is a weaker electrostatic force of attraction between the outer she
7 of 15
What colour is each halogen as an unreacted element and then when in solution?
Fluorine: Yellow gas
Chlorine: Yellow-green gas | Water: Pale green
Bromine: Red-brown liquid | Water: Orange
Iodine: Dark Purple | Water: Dark brown
8 of 15
What is the chemical test for chlorine?
Damp blue litmus paper turns red then bleaches white
9 of 15
What experiment do you use to prove the halogens' reactivity?
Displacement reactions of the halogen and a halide salt e.g. potassium chloride, potassium bromide and potassium iodide.
10 of 15
What does hydrogen + halide form?
hydrogen + halogen ---> hydrogen halide
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What forms when dissolving a hydrogen halide in water?
An acidic solution, the hydrogen ions dissociate to make the solution acidic
12 of 15
1) What group are the noble gases in?
2) What properties do they have?
3) Why?
1) Group 0 OR Group 8
2) They are inert so they are monatomic
3) They have full outer electron shells and so are stable
13 of 15
1) What is the trend going down group 8?
2) Explain the reason for the trend?
1) They get more dense and have higher melting and boiling points?
2) The atoms get bigger so there is more surface area for more atomic forces. More energy is required to break them
14 of 15
Name some uses of each noble gas
He: Silicon chips, Preserving artifacts, balloons
Ne: Fluorescent lights, neon lasers
Ar: Electric light bulbs, argon rock dating, welding
15 of 15
Other cards in this set
Card 2
Front
1) What group are alkali metals in?
2) What properties do they have?
3) Why are they called alkali metals?
Back
1) Group 1
2) Soft, relatively low melting point
3) When reacting with water, they form alkaline solutions
Card 3
Front
General equation of alkali metal + water
Back
Card 4
Front
How are alkali metals stored?
Back
Card 5
Front
1) What happens to their reactivity when going down group 1?
2) Why?
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