Chemistry

According to Planck's quantum theory, energy is emitted or absorbed

In photoelectric effect, the number of photoelectrons emitted is proportional to

The mode of excitation of molecule in IR spectroscopy is

Beer-Lambert's law relates absorbance (A) with

For an ideal gas, the compressibility factor (Z) is

As one moves along a given row in the periodic table ionization energy

Waterline corrosion in steel tank is an example of

Which of the following dissolved salts in water will cause the most hardness in water sample?

Optically active stereoisomers that are not the mirror images are called

In a Diels-Alder reaction, a conjugated diene reacts with

(i) State Heisenberg's uncertainty principle. What is uncertainty in the position of a particle, if the uncertainty in momentum is $ 10^{-11} kg m/s $?
(ii) Explain why classical Newtonian and Maxwell's wave mechanics theory failed to describe the behavior of microscopic (atomic and subatomic) particles.

(i) Explain the dual nature of matter and radiation. Describe de Broglie's hypothesis and briefly discuss its experimental verification.
(ii) Explain the principles of combination of atomic orbitals to form molecular orbitals.

Draw the molecular orbital energy level diagrams for (i) $ N_2 $ and (ii) $ O_{2} $ molecules. Write their molecular orbital electronic configurations, calculate their bond orders, and explain their magnetic properties.

(i) What are the salient features of crystal field theory? Also explain the crystal field splitting in octahedral complexes with energy level diagram.
(ii) Differentiate between the coordination number and oxidation number of a metal ion. Further, calculate the coordination number and oxidation number of Fe in $ K_{4}[Fe(CN)_{6}] $ and Ni in $ Ni(CO)_4 $.

(i) State the principle of vibrational spectroscopy and derive the selection rule for vibrational transitions in diatomic molecules.
(ii) Explain the mechanism of fluorescence and give its important applications.

Write informative notes on any two of the following:

(i) Derive the Van der Waals' equation of state for n moles of gas. Explain the significance of Van der Waals' constants.
(ii) Describe the deviations of real gases from ideal behaviour and discuss their causes.

(i) Explain ionic, dipolar, and van der Waals interactions with suitable examples.
(ii) Differentiate among ionization energy, electron affinity, and electronegativity, highlighting their definitions and periodic trends.

(i) What is electronic configuration? Also give the electronic configuration of Cu, $ Al^{3+} $ and $ Cl^- $.
(ii) Explain the variation of s, p, d, and f orbital energies across the periodic table.

What do you understand by hybridization? Giving suitable examples explain $ sp^{3} $, $ sp^{3}d $ and $ sp^3d^2 $ hybridization.

(i) Predict at what temperature would the following reaction be spontaneous, given that $ \Delta H=9.080~kJ/mol $ and $ \Delta S=0.0357~kJ/(K \cdot mol) $.
$ 4NH_{3} + 5O_{2} \rightarrow 4NO + 6H_{2}O $
(ii) What is the Ellingham diagram and discuss its importance in metallurgical processes.

(i) Derive Nernst equation and write its applications.
(ii) A sample of water on analysis has been found to contain the following in ppm: $ Ca(HCO_{3})_{2}=4.86 $; $ Mg(HCO_{3})_{2}=5.84 $; $ CaSO_{4}=6.80 $; $ MgSO_{4}=8.40 $. Calculate the temporary and permanent hardness of the water.

(i) What is principle of EDTA titration? How is the permanent hardness of water is determined using EDTA method?
(ii) What are the ion-exchange resins? How will you purify water by using the resins? What are the advantages of this method over other methods.

(i) What are the stereoisomers? How are they classified.
(ii) Explain the term chirality. Discuss the optical isomerism of chiral organic compounds using the example of tartaric acid.

(i) Draw and describe the conformations of cyclohexane. Discuss the relative stability of conformers.
(ii) What are the different types of reactive intermediates involved in organic reactions?

(i) Discuss elimination and substitution reactions with examples.
(ii) Give a brief note on the synthesis of aspirin.

According to Heisenberg's Uncertainty Principle, which of the following pairs cannot be simultaneously determined with high precision?

According to Crystal Field Theory, the splitting of d-orbitals in an octahedral field leads to:

Which of the following complexes will show geometrical isomerism?

In IR spectroscopy, a vibration is IR active only if:

Which of the following is not a van der Waals force?

The spontaneity of a chemical process is indicated by:

Temporary hardness of water is mainly due to:

Which of the following elements has the highest electronegativity?

Enantiomers differ in:

Diels-Alder reaction involves

State and explain Heisenberg's Uncertainty Principle. Discuss its significance in determining position and momentum of an electron.

Explain the photoelectric effect and de Broglie hypothesis.

Explain the formation of molecular orbitals using the linear combination of atomic orbitals (LCAO) approach. Differentiate between bonding and antibonding orbitals.

Discuss the crystal field splitting of d-orbital in Tetrahedral complexes.

Explain the principles of vibrational and rotational spectroscopy. What are the selection rules for rotational transitions in diatomic molecules?

Derive van der Waal's equation for real gases.

Discuss the deviation of real gases from ideal behavior. Under what conditions is the deviation more significant?

Discuss the basic principle of Nuclear Magnetic Resonance (NMR) spectroscopy. How is it useful for structural elucidation of organic compounds?

Explain the Nernst equation and its applications in calculating EMF of electrochemical cells.

What do you mean by Hardness of water. Discuss the EDTA method for estimation of hardness of water.

Explain the HSAB (Hard and Soft Acids and Bases) principle with suitable examples.

Define ionization energy & electron affinity, How do these vary in the periodic table as the atomic number increases.

Discuss the relationship between hybridization and molecular geometry. Provide examples of common geometries like tetrahedral, linear, and trigonal planar.

Define stereoisomerism. Differentiate between structural isomers, enantiomers, and diastereomers with examples.

Describe the mechanism of epoxide ring opening reactions under acidic and basic conditions.

Outline the synthesis of aspirin from salicylic acid. Include the reagents, reaction mechanism, and significance of the reaction.

According to Heisenberg's Uncertainty Principle, which of the following pairs cannot be simultaneously determined with high precision?

According to Crystal Field Theory, the splitting of d-orbitals in an octahedral field leads to:

Which of the following complexes will show geometrical isomerism?

In IR spectroscopy, a vibration is IR active only if:

Which of the following is not a van der Waals force?

The spontaneity of a chemical process is indicated by:

Temporary hardness of water is mainly due to:

Which of the following elements has the highest electronegativity?

Enantiomers differ in:

Diels-Alder reaction involves

State and explain Heisenberg's Uncertainty Principle. Discuss its significance in determining position and momentum of an electron.

Explain the photoelectric effect and de Broglie hypothesis.

Explain the formation of molecular orbitals using the linear combination of atomic orbitals (LCAO) approach. Differentiate between bonding and antibonding orbitals.

Discuss the crystal field splitting of d-orbital in Tetrahedral complexes.

Explain the principles of vibrational and rotational spectroscopy. What are the selection rules for rotational transitions in diatomic molecules?

Derive van der Waal's equation for real gases.

Discuss the deviation of real gases from ideal behavior. Under what conditions is the deviation more significant?

Discuss the basic principle of Nuclear Magnetic Resonance (NMR) spectroscopy. How is it useful for structural elucidation of organic compounds?

Explain the Nernst equation and its applications in calculating EMF of electrochemical cells.

What do you mean by Hardness of water. Discuss the EDTA method for estimation of hardness of water.

Explain the HSAB (Hard and Soft Acids and Bases) principle with suitable examples.

Define ionization energy & electron affinity, How do these vary in the periodic table as the atomic number increases.

Discuss the relationship between hybridization and molecular geometry. Provide examples of common geometries like tetrahedral, linear, and trigonal planar.

Define stereoisomerism. Differentiate between structural isomers, enantiomers, and diastereomers with examples.

Describe the mechanism of epoxide ring opening reactions under acidic and basic conditions.

Outline the synthesis of aspirin from salicylic acid. Include the reagents, reaction mechanism, and significance of the reaction.

According to Heisenberg's Uncertainty Principle, which of the following pairs cannot be simultaneously determined with high precision?

According to Crystal Field Theory, the splitting of d-orbitals in an octahedral field leads to:

Which of the following complexes will show geometrical isomerism?

In IR spectroscopy, a vibration is IR active only if:

Which of the following is not a van der Waals force?

The spontaneity of a chemical process is indicated by:

Temporary hardness of water is mainly due to:

Which of the following elements has the highest electronegativity?

Enantiomers differ in:

Diels-Alder reaction involves

State and explain Heisenberg's Uncertainty Principle. Discuss its significance in determining position and momentum of an electron.

Explain the photoelectric effect and de Broglie hypothesis.

Explain the formation of molecular orbitals using the linear combination of atomic orbitals (LCAO) approach. Differentiate between bonding and antibonding orbitals.

Discuss the crystal field splitting of d-orbital in Tetrahedral complexes.

Explain the principles of vibrational and rotational spectroscopy. What are the selection rules for rotational transitions in diatomic molecules?

Derive van der Waal's equation for real gases.

Discuss the deviation of real gases from ideal behavior. Under what conditions is the deviation more significant?

Discuss the basic principle of Nuclear Magnetic Resonance (NMR) spectroscopy. How is it useful for structural elucidation of organic compounds?

Explain the Nernst equation and its applications in calculating EMF of electrochemical cells.

What do you mean by Hardness of water. Discuss the EDTA method for estimation of hardness of water.

Explain the HSAB (Hard and Soft Acids and Bases) principle with suitable examples.

Define ionization energy & electron affinity, How do these vary in the periodic table as the atomic number increases.

Discuss the relationship between hybridization and molecular geometry. Provide examples of common geometries like tetrahedral, linear, and trigonal planar.

Define stereoisomerism. Differentiate between structural isomers, enantiomers, and diastereomers with examples.

Describe the mechanism of epoxide ring opening reactions under acidic and basic conditions.

Outline the synthesis of aspirin from salicylic acid. Include the reagents, reaction mechanism, and significance of the reaction.

According to Heisenberg's Uncertainty Principle, which of the following pairs cannot be simultaneously determined with high precision?

According to Crystal Field Theory, the splitting of d-orbitals in an octahedral field leads to:

Which of the following complexes will show geometrical isomerism?

In IR spectroscopy, a vibration is IR active only if:

Which of the following is not a van der Waals force?

The spontaneity of a chemical process is indicated by:

Temporary hardness of water is mainly due to:

Which of the following elements has the highest electronegativity?

Enantiomers differ in:

Diels-Alder reaction involves

State and explain Heisenberg's Uncertainty Principle. Discuss its significance in determining position and momentum of an electron.

Explain the photoelectric effect and de Broglie hypothesis.

Explain the formation of molecular orbitals using the linear combination of atomic orbitals (LCAO) approach. Differentiate between bonding and antibonding orbitals.

Discuss the crystal field splitting of d-orbital in Tetrahedral complexes.

Explain the principles of vibrational and rotational spectroscopy. What are the selection rules for rotational transitions in diatomic molecules?

Derive van der Waal's equation for real gases.

Discuss the deviation of real gases from ideal behavior. Under what conditions is the deviation more significant?

Discuss the basic principle of Nuclear Magnetic Resonance (NMR) spectroscopy. How is it useful for structural elucidation of organic compounds?

Explain the Nernst equation and its applications in calculating EMF of electrochemical cells.

What do you mean by Hardness of water. Discuss the EDTA method for estimation of hardness of water.

Explain the HSAB (Hard and Soft Acids and Bases) principle with suitable examples.

Define ionization energy & electron affinity, How do these vary in the periodic table as the atomic number increases.

Discuss the relationship between hybridization and molecular geometry. Provide examples of common geometries like tetrahedral, linear, and trigonal planar.

Define stereoisomerism. Differentiate between structural isomers, enantiomers, and diastereomers with examples.

Describe the mechanism of epoxide ring opening reactions under acidic and basic conditions.

Outline the synthesis of aspirin from salicylic acid. Include the reagents, reaction mechanism, and significance of the reaction.

According to Heisenberg's Uncertainty Principle, which of the following pairs cannot be simultaneously determined with high precision?

According to Crystal Field Theory, the splitting of d-orbitals in an octahedral field leads to:

Which of the following complexes will show geometrical isomerism?

In IR spectroscopy, a vibration is IR active only if:

Which of the following is not a van der Waals force?

The spontaneity of a chemical process is indicated by:

Temporary hardness of water is mainly due to:

Which of the following elements has the highest electronegativity?

Enantiomers differ in:

Diels-Alder reaction involves

State and explain Heisenberg's Uncertainty Principle. Discuss its significance in determining position and momentum of an electron.

Explain the photoelectric effect and de Broglie hypothesis.

Explain the formation of molecular orbitals using the linear combination of atomic orbitals (LCAO) approach. Differentiate between bonding and antibonding orbitals.

Discuss the crystal field splitting of d-orbital in Tetrahedral complexes.

Explain the principles of vibrational and rotational spectroscopy. What are the selection rules for rotational transitions in diatomic molecules?

Derive van der Waal's equation for real gases.

Discuss the deviation of real gases from ideal behavior. Under what conditions is the deviation more significant?

Discuss the basic principle of Nuclear Magnetic Resonance (NMR) spectroscopy. How is it useful for structural elucidation of organic compounds?

Explain the Nernst equation and its applications in calculating EMF of electrochemical cells.

What do you mean by Hardness of water. Discuss the EDTA method for estimation of hardness of water.

Explain the HSAB (Hard and Soft Acids and Bases) principle with suitable examples.

Define ionization energy & electron affinity, How do these vary in the periodic table as the atomic number increases.

Discuss the relationship between hybridization and molecular geometry. Provide examples of common geometries like tetrahedral, linear, and trigonal planar.

Define stereoisomerism. Differentiate between structural isomers, enantiomers, and diastereomers with examples.

Describe the mechanism of epoxide ring opening reactions under acidic and basic conditions.

Outline the synthesis of aspirin from salicylic acid. Include the reagents, reaction mechanism, and significance of the reaction.

How many electrons can exist with the principal quantum number's value as 4?

A ball of mass 0.5kg is moving with velocity 6.626 m/s. What's the wavelength of that ball?

As per Heisenberg's principle of uncertainty, the relation between relative momentum and relative position is ______.

Arrange the following intermediate into decreasing order of stability.

The distance between the centers of the peaks of doublet is called as?

How many peaks are expected in low-resolution NMR spectrum of vinyl chloride and ethyl cyclopropane?

Which of the following phase changes are endothermic?

The Gibbs free energy is positive when a change in enthalpy and change in entropy are positive at ______.

The type of hardness that occurs due to the presence of bicarbonate of calcium and magnesium ions hardness is ______.

Which of the following is an alkane which can exhibit optical activity?

Write short notes on:

What are Quantum numbers and what do they signify? How are these numbers related with each other?

Give reason for the following:-

Find out the bond orders of CO, $ \text{N}_2 $, $ \text{O}_2^\text{2-} $, $ \text{O}_2^\text{2+} $

Which of the following two molecules has a higher bond length (i) $ \text{O}_2 $: (ii) $ \text{O}_2^- $? Explain using Molecular orbital Theory.

Describe and compare the splitting of d- orbitals under the influence of octahedral and tetrahedral ligand fields.

Explain Crystal Field Stabilization Energy (CFSE) and pairing Energy (PE). How do the CFSE values related to the corresponding colours of d-block metal complexes?

Why is methanol a good solvent for U.V. Visible but not for IR spectroscopy?

Calculate the number of vibrational degrees of freedom in the following compounds

What is the importance of fingerprint region in IR spectra?

Discuss spin-spin relaxation in NMR spectroscopy and draw and explain the splitting pattern observed in the 1H NMR of $ \text{CHCl}_2\text{CH}_2\text{Cl} $.

The frequency of oscillation of HF is $ 4.12 \times 10^{-14} $ Hz. Calculate the vibrational energy and its force constant. $ M_{H} = 1.0078u $, $ M_{F} = 18.9984u $.

What are ion exchange Resins? Discuss their application in water softening. How are spent resins regenerated?

9.67ml of EDTA solution consumes exactly 10.2 mg of $ \text{CaCO}_3 $ equivalents. 100 ml of a given Hard water sample consumes 17.5 ml of above EDTA solution. 250 ml of the above hard water sample was boiled completely and boiled off sample consumed 35 ml of above EDTA solution. Calculate the temporary and permanent hardness of the above hardware sample in $ ^{\circ}C $, $ ^{\circ}F $ and as $ \text{CaCO}_3 $ equivalents.

Differentiate between terms Configuration and Conformation with suitable examples.

Discuss stereochemistry of tartaric acid.

Explain racemisation of optical isomers with suitable examples.

What do you mean by cyclization and ring opening reactions give two examples of each type of these reactions.

What are carbonium ions? Show hybridisation in the structure of carbonium ion and discuss the stability of primary, secondary and tertiary carbonium ions.

How many electrons can exist with the principal quantum number's value as 4?

A ball of mass 0.5kg is moving with velocity 6.626 m/s. What's the wavelength of that ball?

As per Heisenberg's principle of uncertainty, the relation between relative momentum and relative position is ______.

Arrange the following intermediate into decreasing order of stability.

The distance between the centers of the peaks of doublet is called as?

How many peaks are expected in low-resolution NMR spectrum of vinyl chloride and ethyl cyclopropane?

Which of the following phase changes are endothermic?

The Gibbs free energy is positive when a change in enthalpy and change in entropy are positive at ______.

The type of hardness that occurs due to the presence of bicarbonate of calcium and magnesium ions hardness is ______.

Which of the following is an alkane which can exhibit optical activity?

Write short notes on:

What are Quantum numbers and what do they signify? How are these numbers related with each other?

Give reason for the following:-

Find out the bond orders of CO, $ \text{N}_2 $, $ \text{O}_2^\text{2-} $, $ \text{O}_2^\text{2+} $

Which of the following two molecules has a higher bond length (i) $ \text{O}_2 $: (ii) $ \text{O}_2^- $? Explain using Molecular orbital Theory.

Describe and compare the splitting of d- orbitals under the influence of octahedral and tetrahedral ligand fields.

Explain Crystal Field Stabilization Energy (CFSE) and pairing Energy (PE). How do the CFSE values related to the corresponding colours of d-block metal complexes?

Why is methanol a good solvent for U.V. Visible but not for IR spectroscopy?

Calculate the number of vibrational degrees of freedom in the following compounds

What is the importance of fingerprint region in IR spectra?

Discuss spin-spin relaxation in NMR spectroscopy and draw and explain the splitting pattern observed in the 1H NMR of $ \text{CHCl}_2\text{CH}_2\text{Cl} $.

The frequency of oscillation of HF is $ 4.12 \times 10^{-14} $ Hz. Calculate the vibrational energy and its force constant. $ M_{H} = 1.0078u $, $ M_{F} = 18.9984u $.

What are ion exchange Resins? Discuss their application in water softening. How are spent resins regenerated?

9.67ml of EDTA solution consumes exactly 10.2 mg of $ \text{CaCO}_3 $ equivalents. 100 ml of a given Hard water sample consumes 17.5 ml of above EDTA solution. 250 ml of the above hard water sample was boiled completely and boiled off sample consumed 35 ml of above EDTA solution. Calculate the temporary and permanent hardness of the above hardware sample in $ ^{\circ}C $, $ ^{\circ}F $ and as $ \text{CaCO}_3 $ equivalents.

Differentiate between terms Configuration and Conformation with suitable examples.

Discuss stereochemistry of tartaric acid.

Explain racemisation of optical isomers with suitable examples.

What do you mean by cyclization and ring opening reactions give two examples of each type of these reactions.

What are carbonium ions? Show hybridisation in the structure of carbonium ion and discuss the stability of primary, secondary and tertiary carbonium ions.

State de Broglie's principle.

What is an orbital?

Arrange the covalent bonds C—F, C—Br, C—Cl and C—I in increasing order of strength.

Which of $ \text{NH}_3 $, $ \text{PH}_3 $, $ \text{AsH}_3 $ and $ \text{SbH}_3 $ possesses largest bond angle? Give reason.

Out of $ \text{Cr}^{2+} $ and $ \text{Cr}^{3+} $, which one is stable in aqueous solution?

$ \text{Cu}^+ $ is colourless, but $ \text{Cu}^{2+} $ is coloured. Why?

What is selection rule?

A gas expands against vacuum. What is the work done on it?

What is the condition for a reaction to be in equilibrium?

The presence of $ \text{CO}_2 $ in boiler feed water should be avoided. Why?

Write short notes on the following:

Discuss photoelectric effect (with mathematical equations) for explaining the particle nature of light.

How many photons of light having a wavelength of 4000 Å are necessary to provide 1 J of energy? $ (h = 6.626 \times 10^{-34} \, \text{J s}) $

Which of the following two molecules has a higher bond length? (i) $ \text{O}_2 $ (ii) $ \text{O}_2^+ $ (iii) $ \text{O}_2^- $ Explain using molecular orbital theory.

Draw the MO energy level diagram for NO molecule. Using this diagram, calculate and explain bond order and magnetic behaviour of (i) NO, (ii) $ \text{NO}^+ $ and (iii) $ \text{NO}^- $.

The internuclear distance of NaCl is $ 2.36 \times 10^{-10} \text{ m} $. Calculate the reduced mass and moment of inertia of NaCl. (Atomic mass of Cl = $ 35 \times 10^{-3} \text{ kg mol}^{-1} $ and Na = $ 23 \times 10^{-3} \text{ kg mol}^{-1} $).

Calculate the force constant for CO, if it absorbs at $ 2.143 \times 10^{5} \, \text{m}^{-1} $. (Atomic mass of C = $ 12 \times 10^{-3} \, \text{kg mol}^{-1} $ and O = $ 16 \times 10^{-3} \, \text{kg mol}^{-1} $)

Which type of electronic transition(s) is/are observed in UV-visible spectrum of phenol in the range 200 nm to 900 nm? Justify your answer.

How many types of $ ^{1}\text{H} $ NMR signals are expected for (i) $ \text{CH}_2\text{BrCH}_2\text{Cl} $ and (ii) $ \text{CH}_3\text{OCH}_3 $? Mention relative intensity ratio for the signal(s) observed for (i) and (ii).

At what frequency shift from TMS, would a group of nuclei with δ = 1:5 resonate in NMR spectrometers operating at 60 MHz and 400 MHz?

2 mol of $ \text{NH}_3 $ at 300 K occupy a volume of $ 5 \times 10^{-3} \, \text{m}^3 $. Calculate the pressure using van der Waals equation $ (a = 0.417 \, \text{Nm}^4 \, \text{mol}^{-2} $ and $ b = 0.037 \times 10^{-3} \, \text{m}^3 \, \text{mol}^{-1}) $. Compare the above result with the pressure calculated using ideal gas equation.

7 mol of a monatomic ideal gas are compressed reversibly and adiabatically. The initial volume is 16 dm³ and the final volume is 7 dm³. The initial temperature is 27 °C.

Given, $ C_v = 20 \cdot 91 \, \text{JK}^{-1} \, \text{mol}^{-1} $, $ \gamma = 1 \cdot 4 $.

Write a cell (in proper cell representation) whose cell reaction is $ \text{AgCl} \rightarrow \text{Ag}^+ + \text{Cl}^- $, using the following standard electrode potentials at 298 K:

$ E°_{\text{AgCl}/\text{AgCl}^-} = 0 \cdot 22 \, \text{V} $, $ E°_{\text{Ag}^+/\text{Ag}} = 0 \cdot 80 \, \text{V} $

Calculate $ E° $ of the cell. Calculate solubility product (or solubility constant) of AgCl and its solubility at 298 K.

A water sample had the following constituents per litre:

$ \text{CaCO}_3 = 65 \, \text{mg} $, $ \text{MgHCO}_3 = 80 \, \text{mg} $

$ \text{CaSO}_4 = 155 \, \text{mg} $, $ \text{MgSO}_4 = 135 \, \text{mg} $

$ \text{NaCl} = 8 \, \text{mg} $

Calculate the quantity of temporary and permanent hardness in the water sample. Calculate the quantity of lime (80% purity) and soda (90% purity) required for softening of 1 million litre of above water sample.

In an experiment to determine the hardness of a sample of water, 25 ml of N/50 $ \text{Na}_2\text{CO}_3 $ solution was added to 100 ml of water sample. After complete precipitation of insoluble carbonate, the unreacted $ \text{Na}_2\text{CO}_3 $ was titrated against N/50 $ \text{H}_2\text{SO}_4 $ solution, when 10 ml of acid was required. Calculate the hardness and comment on the nature of hardness so determined.

Write notes on the following:

Differentiate between the following:

Explain the following:

Arrange the following carbocations in order of increasing stability with suitable reasons:

$ \text{C}_6\text{H}_5\text{CH}_2^+ $
$ (\text{CH}_3)_3\text{C}^+ $
$ (\text{C}_6\text{H}_5)_2\text{CH}^+ $
$ \text{CH}_3\text{CH}_2^+ $

State de Broglie's principle.

What is an orbital?

Arrange the covalent bonds C—F, C—Br, C—Cl and C—I in increasing order of strength.

Which of $ \text{NH}_3 $, $ \text{PH}_3 $, $ \text{AsH}_3 $ and $ \text{SbH}_3 $ possesses largest bond angle? Give reason.

Out of $ \text{Cr}^{2+} $ and $ \text{Cr}^{3+} $, which one is stable in aqueous solution?

$ \text{Cu}^+ $ is colourless, but $ \text{Cu}^{2+} $ is coloured. Why?

What is selection rule?

A gas expands against vacuum. What is the work done on it?

What is the condition for a reaction to be in equilibrium?

The presence of $ \text{CO}_2 $ in boiler feed water should be avoided. Why?

Write short notes on the following:

Discuss photoelectric effect (with mathematical equations) for explaining the particle nature of light.

How many photons of light having a wavelength of 4000 Å are necessary to provide 1 J of energy? $ (h = 6.626 \times 10^{-34} \, \text{J s}) $

Which of the following two molecules has a higher bond length? (i) $ \text{O}_2 $ (ii) $ \text{O}_2^+ $ (iii) $ \text{O}_2^- $ Explain using molecular orbital theory.

Draw the MO energy level diagram for NO molecule. Using this diagram, calculate and explain bond order and magnetic behaviour of (i) NO, (ii) $ \text{NO}^+ $ and (iii) $ \text{NO}^- $.

The internuclear distance of NaCl is $ 2.36 \times 10^{-10} \text{ m} $. Calculate the reduced mass and moment of inertia of NaCl. (Atomic mass of Cl = $ 35 \times 10^{-3} \text{ kg mol}^{-1} $ and Na = $ 23 \times 10^{-3} \text{ kg mol}^{-1} $).

Calculate the force constant for CO, if it absorbs at $ 2.143 \times 10^{5} \, \text{m}^{-1} $. (Atomic mass of C = $ 12 \times 10^{-3} \, \text{kg mol}^{-1} $ and O = $ 16 \times 10^{-3} \, \text{kg mol}^{-1} $)

Which type of electronic transition(s) is/are observed in UV-visible spectrum of phenol in the range 200 nm to 900 nm? Justify your answer.

How many types of $ ^{1}\text{H} $ NMR signals are expected for (i) $ \text{CH}_2\text{BrCH}_2\text{Cl} $ and (ii) $ \text{CH}_3\text{OCH}_3 $? Mention relative intensity ratio for the signal(s) observed for (i) and (ii).

At what frequency shift from TMS, would a group of nuclei with δ = 1:5 resonate in NMR spectrometers operating at 60 MHz and 400 MHz?

2 mol of $ \text{NH}_3 $ at 300 K occupy a volume of $ 5 \times 10^{-3} \, \text{m}^3 $. Calculate the pressure using van der Waals equation $ (a = 0.417 \, \text{Nm}^4 \, \text{mol}^{-2} $ and $ b = 0.037 \times 10^{-3} \, \text{m}^3 \, \text{mol}^{-1}) $. Compare the above result with the pressure calculated using ideal gas equation.

7 mol of a monatomic ideal gas are compressed reversibly and adiabatically. The initial volume is 16 dm³ and the final volume is 7 dm³. The initial temperature is 27 °C.

Given, $ C_v = 20 \cdot 91 \, \text{JK}^{-1} \, \text{mol}^{-1} $, $ \gamma = 1 \cdot 4 $.

Write a cell (in proper cell representation) whose cell reaction is $ \text{AgCl} \rightarrow \text{Ag}^+ + \text{Cl}^- $, using the following standard electrode potentials at 298 K:

$ E°_{\text{AgCl}/\text{AgCl}^-} = 0 \cdot 22 \, \text{V} $, $ E°_{\text{Ag}^+/\text{Ag}} = 0 \cdot 80 \, \text{V} $

Calculate $ E° $ of the cell. Calculate solubility product (or solubility constant) of AgCl and its solubility at 298 K.

A water sample had the following constituents per litre:

$ \text{CaCO}_3 = 65 \, \text{mg} $, $ \text{MgHCO}_3 = 80 \, \text{mg} $

$ \text{CaSO}_4 = 155 \, \text{mg} $, $ \text{MgSO}_4 = 135 \, \text{mg} $

$ \text{NaCl} = 8 \, \text{mg} $

Calculate the quantity of temporary and permanent hardness in the water sample. Calculate the quantity of lime (80% purity) and soda (90% purity) required for softening of 1 million litre of above water sample.

In an experiment to determine the hardness of a sample of water, 25 ml of N/50 $ \text{Na}_2\text{CO}_3 $ solution was added to 100 ml of water sample. After complete precipitation of insoluble carbonate, the unreacted $ \text{Na}_2\text{CO}_3 $ was titrated against N/50 $ \text{H}_2\text{SO}_4 $ solution, when 10 ml of acid was required. Calculate the hardness and comment on the nature of hardness so determined.

Write notes on the following:

Differentiate between the following:

Explain the following:

Arrange the following carbocations in order of increasing stability with suitable reasons:

$ \text{C}_6\text{H}_5\text{CH}_2^+ $
$ (\text{CH}_3)_3\text{C}^+ $
$ (\text{C}_6\text{H}_5)_2\text{CH}^+ $
$ \text{CH}_3\text{CH}_2^+ $

What are the shapes of $ \text{NF}_3 $, $ \text{BF}_3 $ and $ \text{ClF}_3 $ molecules?

How many $ \text{sp}^3 $-, $ \text{sp}^2 $- and sp-hybridized carbon atoms are present in $ (\text{CH}_3)_2\text{CH}-\text{CH}=\text{CH}-\text{C}=\text{C}-\text{CH}=\text{CH}_2 $?

Arrange molecular species $ \text{N}_2 $, $ \text{N}_2^+ $, $ \text{N}_2^- $ and $ \text{N}_2^{2-} $ in increasing order of stability.

Transition metal ions like $ \text{Cu}^+ $ and $ \text{Ag}^+ $ are colourless. Why?

What type of magnetism is exhibited by $ [\text{Mn(H}_2\text{O)}_6]^{2+} $ ion?

How are exhausted zeolite regenerated?

Name any two coagulants.

A gas expands against vacuum. What is the work done on it?

Under what condition, $ \Delta H = \Delta U $?

What type of transition can take place in $ \text{CH}_3\text{NO}_2 $ in UV spectroscopy?

Discuss photoelectric effect and explain equations involved with this effect.

How many photons of light having a wavelength of 4000 Å are necessary to provide 1 J of energy? $ (h = 6 \cdot 626 \times 10^{-34} \, \text{J-s}) $.

If the electron in an unexcited hydrogen atom is excited by absorption of $ 1.76 \times 10^{-18} \, \text{J} $ per atom, what would be the wavelength of radiation emitted when the atom returns to its ground state? $ (c = 3 \times 10^8 \, \text{m s}^{-1}, \, h = 6 \cdot 626 \times 10^{-34} \, \text{J-s}) $

Draw the MO energy level diagram for $ \text{B}_2 $ and based on the diagram, explain the magnetic property observed in $ \text{B}_2 $.

Which type of isomerism is observed with the metal complex having molecular formula, $ \text{CoBr(SO}_4) \cdot \text{5NH}_3 $? Draw their structures. Write one chemical test (reaction) in favour of each structure.

Calculate the frequency (in Hz and cm⁻¹) of O-H bond, if the force constant and reduced mass of the atom pair are 770 N m⁻¹ and $ 1.563 \times 10^{-27} \, \text{kg} $ respectively.

Microwave spectrum of gaseous HCl molecule exhibits a series of equally spaced lines with interspacing of 20-7 cm⁻¹. Calculate the internuclear distance of HCl molecule.

Draw a relative energy diagram showing $ \sigma $, $ \pi $, $ n $, $ \pi^* $ and $ \sigma^* $ energy levels. Using this diagram, discuss the variation of energy levels for $ \pi \rightarrow \pi^* $ and $ n \rightarrow \pi^* $ transitions with increase in solvent polarity qualitatively.

At what frequency shift from TMS, would a group of nuclei with δ = 7.50 resonate in an NMR spectrometer operating at 500 MHz?

Write the number of $ ^{1}\text{H} $-NMR signals and splitting pattern of the signals (singlet, doublet, etc.) due to spin-spin coupling for the following molecules with proper justification:

Use the equation of state of van der Waals to calculate the pressure of 5 moles of $ \text{NH}_3(g) $ occupying a volume of 7 L at 373 K. (Given, $ a = 4 \cdot 17 \, \text{L}^2 \, \text{atm mol}^{-2} $, $ b = 0 \cdot 0371 \, \text{L mol}^{-1} $). Compare the above result with the pressure calculated using ideal gas equation.

1 mole of an ideal gas expands isothermally and reversibly from 5 dm³ to 10 dm³ at 300 K. Calculate $ q $, $ w $, $ \Delta U $, $ \Delta H $, $ \Delta G $ and $ \Delta A $.

Design electrochemical cells (in proper cell representation/notation) in which each of the following reactions occurs:

Write the principle for lime soda process for softening of hard water.

Calculate the amount of lime and soda required for the softening of a million litres of hard water containing $ \text{CaCO}_3 = 25 \, ppm $, $ \text{MgCO}_3 = 144 \, ppm $, $ \text{CaCl}_2 = 111 \, ppm $, $ \text{MgCl}_2 = 95 \, ppm $, $ \text{Na}_2\text{SO}_4 = 15 \, ppm $, $ \text{Fe}_2\text{O}_3 = 25 \, ppm $.

The hardness of 50000 litres of water sample was removed by passing it through a zeolite softener. The softener then required 200 L of NaCl solution, containing 125 g/L of NaCl for regeneration. Calculate the hardness of the sample of water.

Distinguish between the Pauling and Mulliken electronegativity scales.

Draw all the optical isomers of tartaric acid. Identify the pair(s) of enantiomers and diastereomers from the above optical isomers.

Explain the following:

0.5 g of $ \text{CaCO}_3 $ was dissolved in HCl and the solution was made up to 500 mL with distilled water. 50 mL of this solution required 48 mL of EDTA solution for titration. 50 mL of water sample required 15 mL of EDTA and after boiling and filtering required 10 mL of EDTA solution. Calculate total hardness, non-carbonate hardness and carbonate hardness of the water sample.

What are the shapes of $ \text{NF}_3 $, $ \text{BF}_3 $ and $ \text{ClF}_3 $ molecules?

How many $ \text{sp}^3 $-, $ \text{sp}^2 $- and sp-hybridized carbon atoms are present in $ (\text{CH}_3)_2\text{CH}-\text{CH}=\text{CH}-\text{C}=\text{C}-\text{CH}=\text{CH}_2 $?

Arrange molecular species $ \text{N}_2 $, $ \text{N}_2^+ $, $ \text{N}_2^- $ and $ \text{N}_2^{2-} $ in increasing order of stability.

Transition metal ions like $ \text{Cu}^+ $ and $ \text{Ag}^+ $ are colourless. Why?

What type of magnetism is exhibited by $ [\text{Mn(H}_2\text{O)}_6]^{2+} $ ion?

How are exhausted zeolite regenerated?

Name any two coagulants.

A gas expands against vacuum. What is the work done on it?

Under what condition, $ \Delta H = \Delta U $?

What type of transition can take place in $ \text{CH}_3\text{NO}_2 $ in UV spectroscopy?

Discuss photoelectric effect and explain equations involved with this effect.

How many photons of light having a wavelength of 4000 Å are necessary to provide 1 J of energy? $ (h = 6 \cdot 626 \times 10^{-34} \, \text{J-s}) $.

If the electron in an unexcited hydrogen atom is excited by absorption of $ 1.76 \times 10^{-18} \, \text{J} $ per atom, what would be the wavelength of radiation emitted when the atom returns to its ground state? $ (c = 3 \times 10^8 \, \text{m s}^{-1}, \, h = 6 \cdot 626 \times 10^{-34} \, \text{J-s}) $

Draw the MO energy level diagram for $ \text{B}_2 $ and based on the diagram, explain the magnetic property observed in $ \text{B}_2 $.

Which type of isomerism is observed with the metal complex having molecular formula, $ \text{CoBr(SO}_4) \cdot \text{5NH}_3 $? Draw their structures. Write one chemical test (reaction) in favour of each structure.

Calculate the frequency (in Hz and cm⁻¹) of O-H bond, if the force constant and reduced mass of the atom pair are 770 N m⁻¹ and $ 1.563 \times 10^{-27} \, \text{kg} $ respectively.

Microwave spectrum of gaseous HCl molecule exhibits a series of equally spaced lines with interspacing of 20-7 cm⁻¹. Calculate the internuclear distance of HCl molecule.

Draw a relative energy diagram showing $ \sigma $, $ \pi $, $ n $, $ \pi^* $ and $ \sigma^* $ energy levels. Using this diagram, discuss the variation of energy levels for $ \pi \rightarrow \pi^* $ and $ n \rightarrow \pi^* $ transitions with increase in solvent polarity qualitatively.