WorksheetsTopic 10 Group 2
Total questions: 10
Worksheet time: 8mins
The table shows the decomposition temperature of the carbonates of Group 2 elements.
Why is BeCO3 unstable thermally?
The electron cloud of the Be2+ ion is polarised by the CO32– ion.
The electron cloud of the CO32– ion is polarised by the Be2+ ion.
Going down Group 2, the size of the cation increases and the polarisation of the anion by the cation becomes greater.
A small cation absorbs energy more efficiently and can be excited to a higher energy level which is unstable.
Beryllium is a Group 2 element. Which of the following is the anomalous properties of beryllium?
Beryllium oxide is amphoteric
Beryllium chloride does not dissolve in water
Beryllium forms a covalent compound with fluorine
Beryllium oxide can form dimer.
Aqueous beryllium chloride has a pH less than 7 because
the charge density of the beryllium ion is high
the beryllium ion undergoes hydrolysis
beryllium chloride undergoes partial dissociation in water
beryllium chloride is a covalent compound
The solubilities of the sulphates of Group 2 metals decrease down the group because
the cation size increases from Mg2+ to Ba2+
the hydration energy of the cations becomes less exothermic from Mg2+ to Ba2+
the sulphates ion very much smaller than these cations.
The carbonates, nitrates and hydroxides of Group 2 elements decompose to their respective oxides when heated. Hence, it can be concluded that
all compounds of Group 2 elements are unstable to heat
Group 2 elements are strong reducing agents
the oxide is energetically more stable than the carbonates, nitrates and hydroxides
the metallic properties of the elements increases down the Group
Barium sulphate, BaSO4 is less soluble than magnesium sulphate, MgSO4. This is because
BaSO4 is covalent whereas MgSO4 is ionic
the lattice energy of BaSO4 is higher than that of MgSO4
the hydration energy of Ba2+ is less than than of Mg2+
the enthalpy of solution of BaSO4 is more exothermic than that of MgSO4
The metals of Group 2 react readily with oxygen to form compounds of general formula MO. When each of these oxides is added to water, which forms the most alkaline ?
MgO
CaO
SrO
BaO
Steam is passed over heated magnesium to give compound X and hydrogen.
what is not the property of Compound X ?
It has a high melting point
It is a basic oxide
It is a white solid
It is very soluble in water
Which statement about the oxides and hydroxides of the Group 2 elements Mg, Ca, Sr and Ba is correct ?
Each of the oxides reacts readily with water to form pH 12 or above
Magnesium oxide is used as a furnace lining because it has giant molecular structure and hence a high melting point
The hydroxides are produced directly by the thermal decomposition of the corresponding nitrates
The solubility of hydroxides increases from Mg to Ba
What can be seen when a piece of magnesium ribbon is placed in cold water?
A vigorous effervescence occurs
Bubbles of gas form slowly on the magnesium
The magnesium floats on the surface of the water and reacts quickly
The magnesium glows and a white solid is produced
