Ionic and Covalent Character

Q. Among $LiCl$, $BeC{l}_2$, $BC{l}_3$ and $CC{l}_4$, the covalent bond character follows the order:

1. $BeC{l}_2>BC{l}_3>CC{l}_4>LiCl$
2. $BeC{l}_2<BC{l}_3<CC{l}_4<LiCl$
3. $LiCl<BeC{l}_2<BC{l}_3<CC{l}_4$
4. $LiCl>BeC{l}_2>BC{l}_3>CC{l}_4$

Q.

Which Is More Covalent ${\mathrm{SnCl}}_2\mathrm{or}{\mathrm{SnCl}}_4$?

Q. If the electronegativity of atom A is 2.0 and atom B is 3.0, then what is the percentage ionic character of bond A-B?

1. 80.5 %
   
2. 12.5 %
3. 19.5 %
4. 87.5 %

Q. Based on lattice energy and other considerations which one of the following alkali metal chlorides is expected to have the highest melting point.

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

Q. The compound which contains both ionic and covalent bonds is:

1. $C{H}_4$
2. $H_2$
3. $KCN$
4. $KCl$

Q. Which of the following is not correct regarding electrolytic preparation of $H_2{O}_2$

1. Lead is used as cathode
2. 50% $H_{2}S{O}_4$ is used
3. Hydrogen is liberated at anode
4. Sulphur acid undergoes oxidation

Q. Amongst $LiCl$, $RbCl$, $BeC{l}_2$ and $MgC{l}_2$, maximum and minimum ionic character will be shown by the compounds:

1. $LiCl$, $MgC{l}_2$
2. $RbCl$, $BeC{l}_2$
3. $RbCl$, $MgC{l}_2$
4. $MgC{l}_2$, $BeC{l}_2$

Q. The melting point of NaBr is $682{}^{\circ }C$ while that of NaF is $988{}^{\circ }C$. The principle reason behind the melting point of NaF being higher than that of NaBr is:

1. The two crystal are not isomorphous
2. The molar mass of $NaF$ is lower than that of $NaBr$
3. The internuclear distance $(r_c+r_a)$ of $NaBr$ is greater than $NaF$
4. The bond in $NaBr$ has a higher covalent character than the bond in $NaF$

Q. is mgh2 ionic or covalent?

Q. Select the most ionic and most covalent compounds respectively from the following. $Cr{O}_5,M{n}_2{O}_7,PbO,Sn{O}_2$

1. $Cr{O}_5,M{n}_2{O}_7$
2. $PbO,M{n}_2{O}_7$
3. $Sn{O}_2,Cr{O}_5$
4. All of the above.

Q. The melting point of NaBr is $682{}^{\circ }C$ while that of NaF is $988{}^{\circ }C$. The principle reason behind the melting point of NaF being higher than that of NaBr is:

1. The two crystal are not isomorphous
2. The molar mass of $NaF$ is lower than that of $NaBr$
3. The internuclear distance $(r_c+r_a)$ of $NaBr$ is greater than $NaF$
4. The bond in $NaBr$ has a higher covalent character than the bond in $NaF$