Is p-Block Elements – Group 14 (Carbon Family) part of the EAPCET Chemistry syllabus?

Yes. p-Block Elements – Group 14 (Carbon Family) is taught in Intermediate first year Chemistry, and the EAPCET Engineering syllabus is based on the Intermediate first- and second-year syllabus. Check the official notification each year for any changes.

How many Chemistry questions are there in EAPCET?

40 of the 160 questions in the Engineering paper are Chemistry, spread across 24 chapters.

What mistakes do students make in p-Block Elements – Group 14 (Carbon Family)?

Writing SiO₂ as a linear molecule like CO₂ — silicon does not form pπ–pπ double bonds, so SiO₂ is a three-dimensional network of SiO₄ tetrahedra. Saying graphite conducts electricity equally in all directions — it conducts mainly along the layers through delocalised π electrons. Treating SnCl₂ as an oxidising agent — Sn²⁺ is a reducing agent because Sn⁴⁺ is more stable for tin; it is lead where +2 is more stable. Expecting CCl₄ to hydrolyse like SiCl₄ — carbon has no vacant d orbitals to accept a lone pair from water.

EAPCET Chemistry · Intermediate first year

p-Block Elements – Group 14 (Carbon Family)

This chapter covers the carbon family: trends, catenation, allotropes of carbon, oxides, and silicon compounds such as silicones and silicates.

Subject: Chemistry
Taught in: Intermediate first year
Chemistry in the paper: 40 of 160 questions

Key formulas and results

Configuration ns²np²; carbon shows the greatest catenation
Diamond is sp³ bonded; graphite is sp² bonded and conducts electricity
Lead’s +2 state is more stable than +4 (inert pair effect)
CO is a neutral oxide; CO₂ is acidic
SiO₂ is a three-dimensional network solid

What this chapter covers

General trends in group 14
Catenation
Allotropes of carbon
Oxides of carbon
Silicones, silicates and zeolites

How it is usually asked

Allotropes and their properties
Stability of oxidation states
Silicones and silicates
Properties of CO and CO₂

Understanding p-Block Elements – Group 14 (Carbon Family)

Group 14 elements (C, Si, Ge, Sn, Pb) have four valence electrons, ns²np², and show +4 and +2 oxidation states. Down the group the +2 state becomes more stable because of the inert pair effect: Sn²⁺ is a reducing agent (it is easily oxidised to Sn⁴⁺), while Pb⁴⁺ compounds such as PbO₂ are strong oxidising agents. Carbon shows catenation far more than any other element because C–C bonds are short and strong, which is why there are millions of carbon compounds.

Carbon differs from silicon in two ways that explain many questions. Carbon forms strong pπ–pπ multiple bonds, so CO₂ is a discrete linear molecule, while silicon cannot, so SiO₂ is a network solid. Silicon has vacant 3d orbitals, so it can expand its covalency: SiCl₄ hydrolyses in water and [SiF₆]²⁻ exists, but CCl₄ does not hydrolyse and [CF₆]²⁻ is not possible.

Diamond is a three-dimensional network of sp³ carbon atoms, hard and non-conducting; graphite has layers of sp² carbon with delocalised electrons, so it conducts along the layers and is slippery. Fullerene C₆₀ is a sp² cage of 12 five-membered and 20 six-membered rings. CO is neutral and toxic because it binds haemoglobin strongly; CO₂ is acidic. Silicones, made by hydrolysing alkylchlorosilanes, are water-repellent polymers with an –Si–O–Si– backbone.

Worked example

EAPCET-style question

Which of the following oxides is the strongest oxidising agent?

(1) $\ce{CO2}$
(2) $\ce{GeO2}$
(3) $\ce{SnO2}$
(4) $\ce{PbO2}$

Solution

All four oxides contain the element in the +4 state.
Down group 14 the inert pair effect makes the +2 state increasingly more stable than +4.
For lead, Pb(+4) readily gains two electrons to become the more stable Pb(+2).
An element in an unstable higher state that readily goes down to a stable lower state is a strong oxidising agent.
So PbO₂ is the strongest oxidising agent; CO₂ is the weakest, since +4 is carbon’s most stable state.

Answer: $\ce{PbO2}$

Common mistakes to avoid

Writing SiO₂ as a linear molecule like CO₂ — silicon does not form pπ–pπ double bonds, so SiO₂ is a three-dimensional network of SiO₄ tetrahedra.
Saying graphite conducts electricity equally in all directions — it conducts mainly along the layers through delocalised π electrons.
Treating SnCl₂ as an oxidising agent — Sn²⁺ is a reducing agent because Sn⁴⁺ is more stable for tin; it is lead where +2 is more stable.
Expecting CCl₄ to hydrolyse like SiCl₄ — carbon has no vacant d orbitals to accept a lone pair from water.

How to prepare it

Compare carbon and silicon side by side — many questions ask why they behave differently.

Once the formulas feel familiar, test them the way the exam does: practise p-Block Elements – Group 14 (Carbon Family) questions chapter-wise, then attempt a full previous year paper to see whether it holds up under a 3-hour timer.

Related Chemistry chapters

See every chapter in the EAPCET Chemistry syllabus.

Practise p-Block Elements – Group 14 (Carbon Family) chapter-wise

Chapter-wise quizzes show exactly which topics in this chapter you still get wrong — before a full paper does.

Frequently asked questions

Is p-Block Elements – Group 14 (Carbon Family) part of the EAPCET Chemistry syllabus?: Yes. p-Block Elements – Group 14 (Carbon Family) is taught in Intermediate first year Chemistry, and the EAPCET Engineering syllabus is based on the Intermediate first- and second-year syllabus. Check the official notification each year for any changes.
How should I prepare p-Block Elements – Group 14 (Carbon Family) for EAPCET?: Compare carbon and silicon side by side — many questions ask why they behave differently.
How many Chemistry questions are there in EAPCET?: 40 of the 160 questions in the Engineering paper are Chemistry, spread across 24 chapters.
What mistakes do students make in p-Block Elements – Group 14 (Carbon Family)?: Writing SiO₂ as a linear molecule like CO₂ — silicon does not form pπ–pπ double bonds, so SiO₂ is a three-dimensional network of SiO₄ tetrahedra. Saying graphite conducts electricity equally in all directions — it conducts mainly along the layers through delocalised π electrons. Treating SnCl₂ as an oxidising agent — Sn²⁺ is a reducing agent because Sn⁴⁺ is more stable for tin; it is lead where +2 is more stable. Expecting CCl₄ to hydrolyse like SiCl₄ — carbon has no vacant d orbitals to accept a lone pair from water.