S2.1 The ionic model Questionbank

$\text{MgCl}$

$\text{MgCl}_2$

$\text{Mg}_2\text{Cl}$

$\text{Mg}_2\text{Cl}_3$

They have low melting points.

They conduct electricity in solid state.

They consist of molecules with shared electrons.

They conduct electricity when molten or in solution.

$-1$

$-2$

$+1$

$+2$

$1s^2\ 2s^2\ 2p^4$

$1s^2\ 2s^2\ 2p^6$

$1s^2\ 2s^2\ 2p^5$

$1s^2\ 2s^1\ 2p^6$

$\mathrm{SnO_2}$

$\mathrm{SO_2}$

$\mathrm{SrO}$

$\mathrm{SiO_2}$

$\mathrm{Na_2S}$

$\mathrm{Na_2O}$

$\mathrm{K_2O}$

$\mathrm{K_2S}$

Solid sodium chloride conducts electricity because its ions are free to move.

Molten magnesium oxide conducts electricity because its ions can move freely in the liquid state.

Solid calcium chloride conducts electricity because of the movement of electrons within its lattice.

Dissolved aluminum chloride in water does not conduct electricity because the ions are tightly bound.

A

B

C

D