14 th group elements (p-block) practice · Easy

Option C (-4 to +4) is correct because the oxidation number of carbon changes from -4 in methane ($\mathrm{CH}_4$) to +4 in carbon dioxide ($\mathrm{CO}_2$).

Option B (White turning to grey) is correct because $SnCl_2$ reduces $HgCl_2$ to $Hg_2Cl_2$ (white) and then to Hg (grey).

Option A ($CO\mathrm{ } + {\mathrm{N}_2}$) is correct because producer gas is primarily a mixture of carbon monoxide and nitrogen.

Option A is correct because the network structure of quartz ($SiO_2$) resembles the tetrahedral network arrangement found in diamond.

Option C (+2 & +4) is correct because lead exhibits both +2 and +4 oxidation states, with +2 being more stable due to the inert pair effect.

Option C is correct because CO (carbon monoxide) is a neutral oxide and does not affect litmus paper.

Option B (${\mathrm{O}_2}$) is correct because $\mathrm{Pb}{\mathrm{O}_2}$ on reaction with $\mathrm{HN}{\mathrm{O}_3}$ gives oxygen gas.

Option 14 is correct because elements in group 14 can form two chlorides with a difference of 2 in the oxidation state (e.g., SnCl2 and SnCl4).

The correct answer is B (Some of the $\mathrm{SiO}_4^{4 - }$ units are replaced by $\mathrm{AlO}_4^{5 - }$ and $\mathrm{AlO}_6^{9 - }$ ions in zeolite) because the correct replacement is $\mathrm{AlO}_4^{4-}$ not $\mathrm{AlO}_4^{5 - }$ and $\mathrm{AlO}_6^{9 - }$.

The correct answer is A (Diamond) because diamond has a giant covalent network structure with strong covalent bonds throughout the lattice, requiring a large amount of energy to break, hence the highest boiling point.

Option C is correct because carbon suboxide (C3O2) is a linear molecule, not bent, and each carbon atom is sp-hybridized.

The correct answer is D (Has carbon atoms arranged in large plates of rings of strongly bound carbon atoms with weak interplate bonds) because the layered structure of graphite, with strong covalent bonds within the layers and weak van der Waals forces between them, allows it to act as a lubricant and makes it difficult to melt.

The correct answer is B (Solids) because silicon dioxide and other silicon oxides exist as solid materials at room temperature.

Option D (All of these) is correct because hydrolysis of $Be_2C$, $Al_4C_3$, and $Mn_3C$ all produce methane ($CH_4$).

Option C is correct because in $SiO_4^{4-}$, silicon is tetrahedrally surrounded by oxygen atoms, resulting in $sp^3$ hybridization.

Option B is correct because graphite's structure consists of strongly bonded carbon layers with weak interlayer forces, making it soft and difficult to melt.

Option B (Flint glass) is correct because flint glass contains lead oxide, which increases its refractive index, making it suitable for optical lenses.

Option D (Animal charcoal) is correct because animal charcoal contains the highest percentage of impurities compared to the other forms of carbon listed.

Option A ($\mathrm{SiC}$) is correct because carborundum is the common name for silicon carbide (SiC), a very hard ceramic compound used as an abrasive.

Option C (A is true but R is false) is correct because ${Pb}^{4+}$ can be reduced easily to ${Pb}^{2+}$ due to the inert pair effect, but ${Pb}^{2+}$ is diamagnetic, not paramagnetic.

Option A (CO) is correct because the molar mass of CO (28 g/mol) is closest to the average molar mass of air (approximately 29 g/mol), making its vapor density near to air.

The correct answer is D (+2, +4) because lead exhibits +2 and +4 oxidation states due to the inert pair effect.

Option C (Si) is correct because silicon, due to its size and electronic configuration, typically exhibits a coordination number of four in its compounds.

Option C is the correct answer because zeolites are aluminosilicates that do exist naturally.

Option D (Three dimensional network silicate) is correct because quartz (SiO2) has a three-dimensional network structure where each silicon atom is bonded to four oxygen atoms, and each oxygen atom is bonded to two silicon atoms.

Option B (Fullerene) is correct because fullerenes, such as $C_{60}$, are recently discovered allotropes of carbon.

The correct answer is A ($\mathrm{S}{\mathrm{n}^{2 + }}$ is reducing while $\mathrm{P}{\mathrm{b}^{\mathrm{4 + }}}$ is oxidising) due to the inert pair effect.

Option A (Galena) is correct because Galena is the principal ore of lead, chemically known as lead sulfide (PbS).

The correct answer is A (Carbon cannot expand its octet but silicon can expand) because silicon has available d-orbitals that allow it to expand its octet and accommodate more ligands, facilitating hydrolysis, while carbon does not.

Option C (Water gas is a mixture of water vapour and hydrogen) is false because water gas is a mixture of hydrogen and carbon monoxide, not water vapor and hydrogen.