Alkali metals, halogens and noble gases: their properties, the trends down each group and why they happen, displacement reactions, and how transition metals compare with Group 1.
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1.What are the Group 1 elements called?
The alkali metals.
2.How many outer electrons does a Group 1 atom have?
One.
3.What ion does a Group 1 element form?
A positive ion with a charge of 1+, formed by losing its single outer electron.
4.Give three physical properties of the alkali metals.
They are soft, have low densities compared with other metals, and have low melting points that decrease down the group.
5.What happens to reactivity going down Group 1?
It increases.
6.Explain why reactivity increases down Group 1.
The outer electron is in a shell further from the nucleus and is shielded by more inner shells, so it is held less strongly and is lost more easily.
7.What is produced when an alkali metal reacts with water?
A metal hydroxide and hydrogen gas.
8.Describe what you see when sodium is added to water.
It melts into a ball, fizzes and moves rapidly across the surface as hydrogen is released, and it eventually disappears.
9.Why is the resulting solution alkaline?
A metal hydroxide is formed, which dissolves to give a solution with a pH above 7.
10.What is produced when an alkali metal reacts with chlorine?
A white metal chloride, which is a salt that dissolves to give a colourless solution.
11.What are the Group 7 elements called?
The halogens.
12.How many outer electrons does a halogen atom have?
Seven.
13.What ion does a halogen form?
A negative ion with a charge of 1-, formed by gaining one electron.
14.What kind of molecules do halogens form?
Molecules made of pairs of atoms, such as Cl2 and Br2.
15.Describe the appearance of chlorine, bromine and iodine at room temperature.
Chlorine is a pale green gas, bromine is a red-brown liquid, and iodine is a grey solid that forms a purple vapour.
16.What happens to melting and boiling points down Group 7?
They increase, because the molecules get larger and the forces between them are stronger.
17.What happens to reactivity going down Group 7?
It decreases.
18.Explain why reactivity decreases down Group 7.
The outer shell is further from the nucleus and more shielded, so an incoming electron is attracted less strongly and is harder to gain.
19.What is a displacement reaction in Group 7?
A more reactive halogen displaces a less reactive halogen from a solution of one of its salts.
20.Will chlorine displace bromine from potassium bromide?
Yes. Chlorine is more reactive than bromine, so it takes its place and the solution turns orange as bromine is released.
21.Will iodine displace chlorine from potassium chloride?
No. Iodine is less reactive than chlorine, so no reaction happens.
22.What are the Group 0 elements called?
The noble gases.
23.Why are the noble gases unreactive?
They have a full outer shell of electrons, so they do not need to gain, lose or share any.
24.How many outer electrons does helium have compared with the other noble gases?
Helium has two, which fills its only shell. The others have eight.
25.What happens to boiling point going down Group 0?
It increases, because the atoms get larger and the forces between them get stronger.
26.Where are the transition metals found?
In the block between Group 2 and Group 3.
27.Give three ways transition metals differ from Group 1 metals.
They are harder, stronger and denser, they have higher melting points, and they are much less reactive.
28.Give three chemical properties typical of transition metals.
They can form ions with different charges, their compounds are often coloured, and they are useful as catalysts.
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