Question

From the list of the characteristics given below, select the five which are relevant to non-metals and their compounds.

$\left(\mathrm{i}\right)$ Ductile

$\left(\mathrm{ii}\right)$ Conducts electricity

$\left(\mathrm{iii}\right)$ Brittle

$\left(\mathrm{iv}\right)$ Acidic oxides

$\left(\mathrm{v}\right)$ Basic oxides

$\left(\mathrm{vi}\right)$ Discharged at anode

$\left(\mathrm{vii}\right)$ Discharged at cathode

$\left(\mathrm{viii}\right)$ Ionic chlorides

$\left(\mathrm{ix}\right)$ Covalent chlorides

$\left(\mathrm{x}\right)$ Reaction with dilute sulfuric acid yields hydrogen

$\left(\mathrm{xi}\right)$ $1,2$ or $3$ valence electrons

$\left(\mathrm{xii}\right)$ $5,6$ or $7$valence electrons

Answer 1

Properties of metals and non-metals

$\left(\mathrm{i}\right)$ Ductile:

• The elements which can be turned into the wire on hammering are said to be ductile and this property is known as Ductility.
• This property is found in metals
• Example: Gold$\left(\mathrm{Au}\right)$ and Silver$\left(\mathrm{Ag}\right)$

$\left(\mathrm{ii}\right)$ Conduct electricity:

• Those elements which have free electrons, can conduct electricity.
• Metals have this property.
• Example: Iron$\left(\mathrm{Fe}\right)$, Gold$\left(\mathrm{Au}\right)$, Copper$\left(\mathrm{Cu}\right)$, etc.

$\left(\mathrm{iii}\right)$ Brittle:

• Those elements which crack when subjected to stress conditions are said to be brittle and property is known as brittleness.
• Non-metals have this property of brittleness.
• Example: Graphite, an allotrope of Carbon$\left(\mathrm{C}\right)$

$\left(\mathrm{iv}\right)$ Acidic oxides:

• Oxides of elements that show acidic behavior on dissolving in water are termed acidic oxides.
• Oxides of non-metals are acidic in nature.
• Example: ${\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to {\mathrm{H}}_2{\mathrm{CO}}_3\left(\mathrm{aq}\right)$

(Carbon dioxide) (Water) (Carbonic acid)

(Non-Metal oxide) (Acidic in nature)

$\left(\mathrm{v}\right)$ Basic oxides:

• Oxides of elements that show basic behavior on dissolving in water are termed basic oxides.
• Oxides of metals are basic in nature.
• Example: $\mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to \mathrm{Ca}{\left(\mathrm{OH}\right)}_2\left(\mathrm{aq}\right)$

(Calcium oxide) (Water) (Calcium hydroxide)

(Metal oxide) (Basic in nature)

$\left(\mathrm{vi}\right)$ Discharged at anode:

• Negatively charged ions are attracted towards the anode in an electrochemical cell.
• At anode oxidation of these ions takes place by losing electrons and getting discharged.
• These discharged elements are non-metal.

$\left(\mathrm{vii}\right)$ Discharged at cathode:

• Positively charged ions are attracted towards the cathode in an electrochemical cell.
• At cathode reduction of these ions takes place by gaining electrons and getting discharged.
• These discharged elements are metal.

$\left(\mathrm{viii}\right)$ Ionic chlorides:

• In ionic chlorides, an ionic interaction is present between the Chlorine$\left(\mathrm{Cl}\right)$ atom and the other element.
• These other elements are metals.
• Example: Sodium chloride$\left(\mathrm{NaCl}\right)$

$\left(\mathrm{ix}\right)$ Covalent chlorides:

• In covalent chlorides, covalent bonding is present between the Chlorine$\left(\mathrm{Cl}\right)$ atom and the other element.
• These other elements are non-metals.
• Example: Carbon tetrachloride$\left({\mathrm{CCl}}_4\right)$

$\left(\mathrm{x}\right)$ Reaction with dilute sulfuric acid yields Hydrogen:

• Metals have a tendency to release Hydrogen $\left({\mathrm{H}}_2\right)$ when it reacts with acid.
• Example: $\mathrm{Fe}\left(\mathrm{s}\right)+{\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right)\to {\mathrm{FeSO}}_4\left(\mathrm{s}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

(Metal) (Dilute Sulfuric acid) (Ferrous sulfate) (Hydrogen gas)

$\left(\mathrm{xi}\right)$ $1,2$or $3$ valence electrons:

• Metals have 1, 2 or 3 valence electrons.
• Example: Lithium$\left(\mathrm{Li}\right)$, Beryllium$\left(\mathrm{Be}\right)$, or Aluminum$\left(\mathrm{Al}\right)$.

$\left(\mathrm{xii}\right)$ $4,5$ or $6$ valence electrons:

• Non-metals have 4, 5 or 6 valence electrons.
• Example: Carbon$\left(\mathrm{C}\right)$, Nitrogen$\left(\mathrm{N}\right)$ or Oxygen$\left(\mathrm{O}\right)$

Hence, from the above list $\left(\mathrm{iii}\right),\left(\mathrm{iv}\right),\left(\mathrm{vi}\right),\left(\mathrm{ix}\right)$ $\left(\mathrm{xii}\right)$ are relevant to non-metals and their compounds.