Edexcel Chemistry A-level: Inorganic Chemistry Topic 4A

What is the product of the thermal decomposition of barium carbonate?

Why do Group 1 metals tend to have low melting points?

Which property decreases down Group 1 in the periodic table?

What makes the outer electrons of Group 2 metals easier to lose down the group?

Which Group 2 metal is most likely to react most vigorously with water?

What property of Group 2 metals allows them to form 2+ ions when they react?

Why do Group 1 metals produce different colors in flame tests?

Which Group 2 metal compound produces a crimson red color in flame tests?

What is the color observed when barium compounds are subjected to a flame test?

Why do halogens gain an electron to form a 1- ion?

What trend is observed in the atomic radius of Group 7 elements?

In thermal decomposition reactions, what happens to Group 2 metal compounds?

What is the product of the thermal decomposition of magnesium hydroxide?

Which of the following is a property of group 2 metals?

Which of the following group 1 metals can react with excess oxygen to form metal peroxides?

What type of reaction occurs when group 2 hydroxides react with dilute acid?

When group 2 metals react with dilute acids, what is one of the products formed?

What color precipitate is formed when group 2 metals react with chlorine gas?

Reactions of Magnesium

Magnesium is oxidised from an oxidation state of 0 to +2
Magnesium reacts slowly with liquid water, but faster with steam, producing a bright white flame and forming hydrogen and magnesium oxide, a white powder

Reactions of Group 2 Metals

Group 2 metals react with chlorine gas to form metal chlorides, which are all white precipitates
The reactions become more vigorous down the group as the elements are more reactive
Group 2 metals react with oxygen to form oxides, which can be vigorous
Strontium and barium can react with excess oxygen and heat energy to form metal peroxides
Group 2 metals react with dilute acids to produce bubbles of hydrogen gas and solutions of metal compounds
Group 2 hydroxides react with dilute acid to form a salt and water, a type of neutralisation reaction

Properties of Group 2 Elements

Group 2 metals react by losing two electrons to form 2+ ions, achieving a full outer shell
Atomic radius of Group 2 metals increases down the group due to additional electron shells
Reactivity of Group 2 metals increases down the group due to increased electron shielding and atomic radius
First ionisation energy of Group 2 metals decreases down the group due to a greater atomic radius and increased shielding

Flame Tests

The colours observed in the flame tests of Group 1 and Group 2 metal compounds are due to electron transitions
The colour produced depends on the wavelength of the light energy emitted
Not all atoms and ions produce a colour in the flame test as the energy emitted may not have a wavelength in the visible light part of the electromagnetic spectrum

Trends in Halogen Properties

Group 7 elements are highly reactive non-metals
Atomic radius of Group 7 elements increases down the group due to additional electron shells

Learn about the elements of Group 1 & 2 in Inorganic Chemistry and the Periodic Table with detailed notes from PMT Education. Understand how Group 2 elements form 2+ ions by losing two electrons. Explore the physical properties of these elements.