Lattice Energy

Q. Which of the following compound has the highest lattice energy?

1. $NaCl$
2. $CaO$
3. $KCl$
4. $MgO$

Q. 44. In any ionic crystal A has formed cubic close packing and B atoms are present at every tetrahedral voids. If any sample of crystal contain `N number of B atoms then number of A atoms in that sample is

Q.

The cell in which the following reactions occurs:

has = 0.236 V at 298 K.

Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Q. In which of the sols, the colloidal particles are with negative charge?

1. $Ti{O}_2$
2. Hydrated $A{l}_2{O}_3$
3. Starch
4. Haemolglobin

Q. Which of the following alkali metal chlorides is expected to have the highest melting point?

1. LiCl
2. NaCl
3. KCl
4. RbCl

Q. $KCl$ easily dissolves in water because:

1. It is a salt of potassium
2. It reacts with water
3. It gets hydrolyzed by water
4. Its ions are easily solvated

Q. Aqueous solutions in the order of their increasing boiling points 1) 0.0001 M NaCl 2)0.001 M MgCl2 3)0.001 M urea 4) 0.001 M Nacl

Q. Arrange $NaF,Mg{F}_2$ and $Al{F}_3$ in the increasing order of their lattice energies.

1. $Al{F}_3<NaF<Mg{F}_2$
2. $NaF<Al{F}_3<Mg{F}_2$
3. $NaF<Mg{F}_2<Al{F}_3$
4. $Al{F}_3<Mg{F}_2<NaF$

Q.

The combustion of benzene$\left(\mathrm{l}\right)$ gives ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ and${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$. Given that heat of combustion of benzene at constant volume is$-3263.9\mathrm{kJ}{\mathrm{mol}}^{-1}$ at ${25}^{°}\mathrm{C}$, the heat of combustion (in $\mathrm{kJ}{\mathrm{mol}}^{-1}$) of benzene at constant pressure will be
($\mathrm{R}=8.314\mathrm{J}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$)

1. $-452.46$

2. $3260$

3. $-3267.6$

4. $4152.6$

Q. Assertion: $BeS{O}_4$ is soluble in water while $BaS{O}_4$ is not.
Reason : Hydration energy decreases down the group from Be to Ba and lattice energy remains almost constant.

1. If both assertion and reason are true but reason is not the correct explanation of assertion
2. If assertion is true but reason is false
3. If both assertion and reason are true and reason is the correct explanation of assertion
4. If both assertion and reason are false

Q.

Calcium carbonate dissociates into CaO and CaCO3, = ∆H=110kj in a closed vessel.The pressure of Co2

a) increases if temperature increases

b) decreases with increase in temperature

Q. When two atoms to combine to form a molecule, energy is:

1. released
2. absorbed
3. neither released nor absorbed
4. can't predict

Q. Data given for the following reaction is as follows:

$Fe{O}_{\left(s\right)}+C_{\left(graphite\right)}⟶F{e}_{\left(s\right)}+C{O}_{\left(g\right)}$

Substance	${\Delta }_f{H}^o$ $\left(kJ{\text{mol}}^{-1}\right)$	$\Delta S^o$ $\left(J{\text{mol}}^{-1}{K}^{-1}\right)$
$Fe{O}_{\left(s\right)}$	-266.3	57.49
$C_{\left(graphite\right)}$	0	5.74
$F{e}_{\left(s\right)}$	0	27.28
$C{O}_{\left(g\right)}$	-110.5	197.6

The minimum temperature in K at which the reaction becomes spontaneous is

Q. Which of the following statement is false regarding the ionic solids $CaO$ and $KI$?

1. $CaO$ has high melting point
2. The lattice energy of $CaO$ is much larger than that of $KI$
3. $KI$ has low melting point
4. $KI$ is soluble in benzene

Q. The magnitude of the lattice energy of a solid increases if

1. The charges on both the ions are small
2. The size of the ions are large
3. The size of the ions are small
4. The ions are of equal size

Q. 52. An aqueous solution containing 288gm of a non-volatile compound having the stoichiometric composition C_nH_{2n}O_n in 90gm of water boils at 101.26degree celcius at 1atm pressure.what is molecular formula of the compound.

Q. Which of the following is not true for $NaCl$ and $MgO$?

1. $NaCl$ has higher lattice energy than $MgO$.
2. Magnesium oxide has a higher melting point than sodium chloride.
3. Magnesium oxide is used to prevent and treat low levels of magnesium in the blood.
4. The lattice energy associated with $MgO$ is higher as compared to $NaCl$.

Q. What will be the order of the lattice energy of the following: CaO, MgBr2, NaCl, CaCl2, MgCl2? Also does the compounds with smaller cation and larger anion have more lattice energy or those with the ions of comparable size as they would fit better in a lattice?

Q. The order of solubility in water for sodium phosphate, sodium sulphate and sodium chloride is:

1. sulphate > phosphate > chloride
2. chloride > sulphate > phosphate
3. chloride > phosphate > sulphate
4. phosphate > chloride > sulphate

Q. Assertion: Lattice energy of $CaO$ is higher than that of $NaCl$.

Reason: The lattice energy of an ionic compund is directly proportional to the product of the charges of ions.

1. Both the assertion and the reason are true but the reason is not the correct explanation of the assertion
2. The assertion is true but the reason is false
3. Both the assertion and the reason are true and the reason is the correct explanation of the assertion
4. Both the assertion and the reason are false

Q. Sodium sulphate is soluble in water whereas Barium sulphate is sparingly soluble because :

1. The hydration energy of sodium sulphate is less than its lattice energy
2. The lattice energy of Barium sulphate is more than its hydration energy
3. The lattice energy has no role to play in solubility
4. None of these

Q.

Which compound will show the highest lattice energy?

1. RbF

2. CsF

3. KF

4. NaF

Q.

Which is more ionic $\mathrm{NaCl}\mathrm{or}{\mathrm{MgCl}}_2$?

Q.

Between NaCl and CsCl, which has greater strength of ionic bond? Justify.

Q. Which of the following pairs.will form the most stable ionic bond.li and f. 2 .mg and.f

Q. Which of the following statements is incorrect regarding lattice energy?

1. Greater is the charge on the ions, more is the lattice energy.
2. Lattice energy is inversely proportional to the size of an ion.
3. Lattice energy for $KCl$ is greater than $CaC{l}_2$.
4. Formation of ionic bond depends upon the ionisation energy of cation, electron gain energy of anion and lattice energy.

Q. In a crystal, cations and anions are held together by:

1. Electrostatic force
2. Electron
3. Nuclear force
4. Covalent bond

Q.

One small crystal of Potassium permanganate may contain particles of :

1. More than ${10}^3$

2. More than ${10}^4$

3. More than${10}^5$

4. More than ${10}^6$

Q.

The splitting of degeneracy of d orbital due to ligands is known as

1. Crystal field splitting

2. Degeneracy splitting

3. Octahedral splitting

4. Splitting

Q.

The electrostatic force of attraction between oppositely charged ions is known as ……………………………………….