Define relative atomic mass.

Calculate the average atomic mass of naturally occurring magnesium using the following data.

Isotope	Istopic atomic mass	Abundance(%)
Mg24	23.99	78.99
Mg25	24.99	10.00
Mg26	25.98	11.01

Consider the following electronic arrangements for the d⁵ configuration.
(a)

\(\upharpoonleft \downharpoonright \)

\(\upharpoonleft \downharpoonright \)

\(​​\upharpoonleft \)

(b)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(\upharpoonleft \downharpoonright \)

(c)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

which of these represents the ground state

Which ion has the stable electronic configuration? Ni²⁺ or Fe³⁺.

What are isoelectronic ions? Give examples.

The first ionisation energy (lE₁) and second ionisation energy (lE₂) of elements X, Y and Z are given below.

Element	IE1(kJ mol-1)	IE2(kJ mol-1)
X	2370	5250
Y	522	7298
Z	1680	3381

Which one of the above elements is the most reactive metal, the least reactive metal and a noble gas?

Why sodium hydroxide is much more water soluble than chloride ?

Give suitable explanation for the following facts about gases.
Gases don't settle at the bottom of a container.

Define Hess's law of constant heat summation.

Calculate ΔH_r⁰ for the reaction CO₂(g) + H₂(g) ⟶ CO(g) + H₂O (g) given that ΔH^f₀ for CO₂ (g), CO (g) and H₂O (g) are - 393.5, - 111.31 and - 242 kJ mol^-1 respectively.

Consider the following reactions,
H₂(g) + I₂(g) ⇌ 2 HI(g)
In each of the above reaction find out whether you have to increase (or) decrease the volume to increase the yield of the product.

Consider the following reactions,
CaCO₃ (s) ⇌ CaO (s) + CO₂(g)
In the above reaction find out whether you have to increase (or) decrease the volume to increase the yield of the product.

If 5.6 g of KOH is present in
(a) 500 mL and
(b) 1 litre of solution 
Calculate the molarity of each of these solutions.

Define the term ‘isotonic solution’.

Draw the lewis structure for
Phosphoric acid

Draw the MO diagram for acetylide ion C₂^2– and calculate its bond order.

Classify the following compounds based on the structure
\(\text { i) } \mathrm{CH} \equiv \mathrm{C}-\mathrm{CH}_{2}-\mathrm{C} \equiv \mathrm{CH}\)
\(\text { ii) } \mathrm{CH}_{3}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{3}\)

Give two examples for each of the following type of organic compounds.
aliphatic open chain.

Write short notes on Resonance.

How will you prepare propane from a sodium salt of fatty acid?

Write the IUPAC names for the following alkenes.

Give IUPAC names for the following compound
(CH₃)₃ C – C ≡ C – CH (CH₃)₂

Draw the structures for the following alkenes.
4 – Methyl – 2 pentene

Discuss the aromatic nucleophilic substitutions reaction of chlorobenzene.

Write the equilibrium constant (K_C) expression for the following reactions
(i) Cu²⁺(aq) + 2Ag (s) ⇌ Cu(s) + 2Ag⁺ (aq)
(ii) 4HCl(g) + O₂g ⇌ 2Cl₂(g) + 2H₂O(g)

State Henry's law.

How does the polarizing power of cations affect the covalent character imparted into the ionic bond ?

Calculate the formal charge of the atoms (numbered) in the following:

Expand the structure.

How will you control photochemical smog?