What will be the basicity of H₃BO₃, which is not a protic acid?

The energy of an electron in the 3rd orbit of hydrogen atom is -E. The energy of an electron in the first orbit will be ___________

Match the list-I and list-II using the correct code given below the list.

Water gas is _____.

Plaster of Paris is obtained by heating gypsum to ______

Mathematical expression of Boyle's law is ____________.

All the naturally occurring processes proceed spontaneously in a direction which leads to _______________

For the reaction AB (g) ⇌ A(g) + B(g), at equilibrium, AB is 20% dissociated at a total pressure of P, The equilibrium constant K_P is related to the total pressure by the expression __________

At 100^o C the vapour pressure of a solution containing 6.5g a solute in 100g water is 732mm. If K_b = 0.52, the boiling point of this solution will be __________

Identify the incorrect statement with respect to hybridisation.

The IUPAC name of the compound \({ H }_{ 3 }C-\overset { \underset { | }{ { CH }_{ 3 } } }{ \underset { \overset { | }{ { CH }_{ 3 } } }{ C } } -CH=C{ \left( { CH }_{ 3 } \right) }_{ 2 }\) is _____________

Which of the following compound can show resonance ?

Statement - I : n - butane and iso - butane are isomers.
Statement - II : Because they are having same molecular formula but differs only in the structural formula.

Which one of the following is used as a metal cleaning solvent?

Ozone depletion will cause ___________.

Balance the following equations by ion electron method.
\({ Na }_{ 2 }{ S }_{ 2 }{ O }_{ 3 }+{ I }_{ 2 }\longrightarrow { Na }_{ 2 }{ S }_{ 4 }{ O }_{ 6 }+NaI\)

An atom of an element contains 35 electrons and 45 neutrons. Deduce
(i) the number of protons
(ii) the electronic configuration for the element
(iii) All the four quantum numbers for the last electron

Write balanced chemical equation for the following processes
Heating calcium in oxygen

State the following laws:
(i) Avogadro's law
(ii) Gay-Lussac's law.

For the equilibrium PCI₅(s) ⇌ PCl₃(g) + CI₂(g) at 25°C k_c = 1.8 x 10^-7 R = 8.314 Jk^-1 mol-¹ Calculate ΔG^o for the reaction.

When the numerical value of the reaction quotient (Q) is greater than the equilibrium constant (K), in which direction does the reaction proceed to reach equilibrium?

Consider the molecules NH₂^-, NH₃, NH₄⁺. Arrange them in the decreasing order of bond angles and give reason for your arrangement.

Describe optical isomerism with suitable example.

Write down the possible isomers of C₅H₁₁Br and give their IUPAC and common names.

Calculate the oxidation number of underlined atoms \(\\ { Na }_{ 2 }[\underline { F } e{ (CN) }_{ 6 }]\)

Explain briefly the time independent schrodinger wave equation?

Elements a, b, c and d have the following electronic configurations:
a: 1s², 2s², 2p⁶
b: 1s², 2s², 2p⁶, 3s², 3p¹
c: 1s², 2s², 2p⁶, 3s², 3p⁶
d: 1s², 2s², 2p¹
Which elements among these will belong to the same group of periodic table.

What are metallic hydrides? Explain about it.

Write balanced chemical equation for each of the following chemical reactions.
Lithium metal with nitrogen gas.

What is inversion temperature? How is it related to Vander Waals constants?

What are state and path functions? Give two examples

Ethylene glycol (C₂H₆O₂) can be at used as an antifreeze in the radiator of a car. Calculate the temperature when ice will begin to separate from a mixture with 20 mass percent of glycol in water used in the car radiator. K_f for water = 1.86 K Kg mol^-1 and molar mass of ethylene glycol is 62 g mol^-1.

Which of the following compounds will not exist as resonance hybrid? Give reason for your answer.
(i) CH₃ - OH
(ii) R-CONH₂
(iii) CH₃-CH = CH-CH₂NH₂

Write the steps to be followed while balancing redox equation by oxidation number method.

The quantum numbers of six electrons are given below. Arrange them in order of increasing energies.If any of these combination(s) has/have the same energy lists.
(i) n = 4, l = 2, m₁ = -2, m_s =  - \(\frac { 1 }{ 2 } \)
(ii) n = 3, l = 2, m₁ = 1, m_s = +\(\frac { 1 }{ 2 } \)
(iii) n = 3, l = 1, m₁ = 0, m_s = +\(\frac { 1 }{ 2 } \)
(iv) n = 3, l = 2, m₁ = -2, m_s = - \(\frac { 1 }{ 2 } \)
(v) n = 3, l = 1, m₁ = -1, m_s = + \(\frac { 1 }{ 2 } \)
(vi) n = 4, l = 1, m₁ = 0, m_s =  +\(\frac { 1 }{ 2 } \)

Explain about the factors that influence the ionization enthalpy.

Justify the position of hydrogen in the periodic table?

How are peroxides and superoxides formed by alkali metals?

1 mole of an ideal gas is maintained at 4.1 atm and at a certain temperature absorbs 3710J heat and expands to 2 Iitres. Calculate the entropy change in expansion process.

What type of bond is formed between K⁺ and CI ^-? Explain the bond formation.

Give IUPAC names for the following compounds
CH₃ – CH = CH – CH = CH – C ≡ C – CH₃

The simplest aromatic hydrocarbon C₆H₆ reactsⒷ on treatment with sodium hydroxide will (C₆H₅OH), Phenol, © as the product. Also Cl₂ to giveⒶ which on reaction with sodium hydroxide gives Ⓑ.Ⓑ of molecular formula C₆H₆O. @ on treatment with ammonia will give C₆H₇N as @. Identify Ⓐ, Ⓑ, ©, and explain the reactions involved.

Differentiate the following
(i) BOD and COD
(ii) Viable and non-viable particulate pollutants