Calculate the number of protons, neutrons, and electrons of the following atoms or ions:

Determine the units of the K. and Kp for the following reactions:

(i) H₂(g) + I₂(g) ⇔ 2HI(g)

(ii) CH₄(g) + H₂O(g) ⇔ CO(g) + 3H₂(g)

(iii) PCl₅(g) ⇔ PCl₃(g) + Cl₂(g)

All transition elements are d-block elements, but not all d-block elements are transition elements - explain.

Write down the Friedel-Crafts reactions of benzene with mechanism.

Explain with the help of Le Chatelier's principle, the effect of temperature and pressure on the reaction:

N₂O₄(g) ⇔ 2NO₂(g);    ΔH= +55.3KJ/mol

Draw the shape of five d orbitals.

What is Le Chatelier's principle? Explain with the help of Le Chatelier's principle, the effect of temperature and pressure on the reaction:

2SO₂(g) + O₂(g) ⇔ 2SO₃(g)    ΔH°= -196.6 KJ

Why second ionization energy is always higher than first ionization energy of an element?

Write a short note on "Aldol condensation reaction".

A 5.0 L vessel contained 0.0185 mole of phosphorous trichloride, 0.0158 mole of phosphorous pentachloride and 0.0870 mole of chlorine at 230°C in an equilibrium mixture. Calculate the value of K_c and K_p for the reaction:

PCl₅ (g) ⇔ PCl₃(g) + Cl₂(g)

Sc is a d block element, but not a transition metal- explain why?

Write down the integrated rate equations of second order reaction. Show that, half-life of a second order reaction is depending on initial concentration of reactant.

Compare and explain the electron affinity of chlorine and fluorine.

Give suitable examples of following reactions:

(i) Markovnikov addition reaction,

(ii) Unimolecular nucleophilic substitution reaction,

(iii) Clemmensen's reduction reaction,

(iv) Williamson's ether synthesis reaction, and

(y) Sulphonation reaction of benzene.

Which of the following orbitals are possible and not possible: 2s, 2d, 3p and 3f. Mention the reason.

Write down the differences between order and molecularity of reactions.

Explain the Pauli exclusion principle.

Find the maximum wavelength of spectral lines of Balmer series in Hydrogen atom. Given that, Rydberg constant is 109679 cm^-1.

Write down the limitations of periodic table.

Briefly discuss the Rutherford's alpha particle scattering experiment.

Scandium is a d block element, but not a transition metal- explain why?

Write down the difference between sigma bond and pi bond.

Define the solution. Classify the solutions with examples based on physical state of solute and solvent.

State and explain the Phase rule. Calculate the number of phases, components and degrees of freedom for the following systems.

    i) CaCO₃ (s) ⇔ CaO (s) + CO₂ (g)

    ii) Saturated solution of NaCl

Establish the relation between K_p and K_c.

Briefly explain the electrolysis of hydrochloric acid.

State and explain Markovnikov and anti-Markovnikov rules.

State the Bohr atomic model. What are the limitations of Bohr atomic model?

Write down the electronic configuration and predict the position (group no. and period no.) in periodic table of following elements: S (16), K (19) and Zn (30).

What do you mean by hybridization of atomic orbitals? Briefly discuss the hybridization of Be, B, and C in of BeCl₂, BF₃, and CH₄, respectively.

What is the molarity of solution prepared by dissolving 25 g of NaOH in 750 mL of solution?

Define colligative properties. Why is the elevation of boiling colligative property?

What is Le Chatelier's principle? Explain with the help of Le Chatelier's principle, the effect of temperature and pressure on the following reaction:

N₂(g)+3H₂(g) ⇔ 2NH₃ (g); ∆H = -92.2 KJ

What is the fundamental difference between an electrolytic cell and an electrochemical cell.

Write short notes on:

    i) Sulphonation of Benzene

    ii) Wurtz reaction

    iii)Aldol condensation reaction

If the principal quantum number (n) of an atomic orbital is 4, what are possible values of subsidiary quantum number (l) and magnetic quantum number (m)?

Why ionization potential energy of Nitrogen is higher than that of Oxygen? Explain.

Write down the conditions for the formation of coordination bonds.

What is the percent by weight of NaCl, if 1.50 g of NaCl is dissolved in 5.80 g of water?

'The vapor pressure of a solution is directly proportional to the mole fraction of the solvent'. Justify the statement from Raoult's law of vapor pressure.

Show that, "In zero order reaction, the rate constant is equal to the rate of reaction at all concentrations".

In the following reaction, label each species as an acid or bases. Show the conjugate acid-base pairs.

(i) HCO₃^-(aq) + HF(aq) ⇔ H₂CO₃(aq) + F^-(aq)

(ii) NH₃(aq) + H₂S(aq) ⇔ NH₄⁺aq) + HS^-(aq)

Write short notes on the following topics:

i) Pauli Exclusion Principle and ii) Diagonal relationships

Write a short note on "hydrogen bond".

Define colligative properties. Mention the name of colligative properties of dilute solutions.

Write down the integrated rate equations of first order and second order reactions. Show that, "Half-life of a first order reaction is independent on initial concentration of reactant".

Calculate the pH of following aqueous solution:

(i) 0.01 M HCl, (ii) 0.02 M H₂SO₄, and (iii) 0.02 M NaOH.

Explain the Raoult's law.

Calculate the E°cell of the following:

Zn (s) / Zn²⁺ || Ag / Ag(s)

        Given that, E°_Zn/Zn²⁺ = +0.76 V and E°_Ag/Ag⁺ = -0.799 V