Bond order of $\mathrm{O}_2=2, \mathrm{O}_2^{+}=2.5, \mathrm{H}_2{ }^{+}=0.5, \mathrm{NO}=2.5$
NCERT 125
2 RBTS PAPER
160818
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
1 $\mathrm{CO}_2$
2 $\mathrm{HI}$
3 $\mathrm{H}_2 \mathrm{O}$
4 $\mathrm{SO}_2$
Explanation:
Thus, $\mathrm{H}_2 \mathrm{O}$ has highest dipole moment.
Mod. NEET
2 RBTS PAPER
160819
An ionic bond $A^{+} B^{-}$is most likely to be formed when:
1 the ionization energy of $A$ is high and the electron affinity of $B$ is low
2 the ionization energy of $A$ is low and the electron affinity of $B$ is high
3 the ionization energy of $A$ and the electron affinity of $B$ is high
4 the ionization energy of $A$ and the electron affinity of $B$ is low
Explanation:
If I.E. of $A$ is less, it will lose electron easily and E.A of $B$ is high it will gain electron easily so ionic bond is easily formed.
NCERT 102
2 RBTS PAPER
160820
Which of the following compounds of elements in group IV is expected to be most ionic ?
1 $\mathrm{PbCl}_2$
2 $\mathrm{PbCl}_4$
3 $\mathrm{CCl}_4$
4 $\mathrm{SiCl}_4$
Explanation:
Ionic character of a covalent bond $\propto \frac{1}{\phi}$ $\phi=\frac{\text { charg e }}{(\text { radius })^2}=\mathrm{C}^{4+}>\mathrm{Si}^{4+}>\mathrm{Pb}^{4+}>\mathrm{Pb}^{2+}$
Bond order of $\mathrm{O}_2=2, \mathrm{O}_2^{+}=2.5, \mathrm{H}_2{ }^{+}=0.5, \mathrm{NO}=2.5$
NCERT 125
2 RBTS PAPER
160818
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
1 $\mathrm{CO}_2$
2 $\mathrm{HI}$
3 $\mathrm{H}_2 \mathrm{O}$
4 $\mathrm{SO}_2$
Explanation:
Thus, $\mathrm{H}_2 \mathrm{O}$ has highest dipole moment.
Mod. NEET
2 RBTS PAPER
160819
An ionic bond $A^{+} B^{-}$is most likely to be formed when:
1 the ionization energy of $A$ is high and the electron affinity of $B$ is low
2 the ionization energy of $A$ is low and the electron affinity of $B$ is high
3 the ionization energy of $A$ and the electron affinity of $B$ is high
4 the ionization energy of $A$ and the electron affinity of $B$ is low
Explanation:
If I.E. of $A$ is less, it will lose electron easily and E.A of $B$ is high it will gain electron easily so ionic bond is easily formed.
NCERT 102
2 RBTS PAPER
160820
Which of the following compounds of elements in group IV is expected to be most ionic ?
1 $\mathrm{PbCl}_2$
2 $\mathrm{PbCl}_4$
3 $\mathrm{CCl}_4$
4 $\mathrm{SiCl}_4$
Explanation:
Ionic character of a covalent bond $\propto \frac{1}{\phi}$ $\phi=\frac{\text { charg e }}{(\text { radius })^2}=\mathrm{C}^{4+}>\mathrm{Si}^{4+}>\mathrm{Pb}^{4+}>\mathrm{Pb}^{2+}$
Bond order of $\mathrm{O}_2=2, \mathrm{O}_2^{+}=2.5, \mathrm{H}_2{ }^{+}=0.5, \mathrm{NO}=2.5$
NCERT 125
2 RBTS PAPER
160818
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
1 $\mathrm{CO}_2$
2 $\mathrm{HI}$
3 $\mathrm{H}_2 \mathrm{O}$
4 $\mathrm{SO}_2$
Explanation:
Thus, $\mathrm{H}_2 \mathrm{O}$ has highest dipole moment.
Mod. NEET
2 RBTS PAPER
160819
An ionic bond $A^{+} B^{-}$is most likely to be formed when:
1 the ionization energy of $A$ is high and the electron affinity of $B$ is low
2 the ionization energy of $A$ is low and the electron affinity of $B$ is high
3 the ionization energy of $A$ and the electron affinity of $B$ is high
4 the ionization energy of $A$ and the electron affinity of $B$ is low
Explanation:
If I.E. of $A$ is less, it will lose electron easily and E.A of $B$ is high it will gain electron easily so ionic bond is easily formed.
NCERT 102
2 RBTS PAPER
160820
Which of the following compounds of elements in group IV is expected to be most ionic ?
1 $\mathrm{PbCl}_2$
2 $\mathrm{PbCl}_4$
3 $\mathrm{CCl}_4$
4 $\mathrm{SiCl}_4$
Explanation:
Ionic character of a covalent bond $\propto \frac{1}{\phi}$ $\phi=\frac{\text { charg e }}{(\text { radius })^2}=\mathrm{C}^{4+}>\mathrm{Si}^{4+}>\mathrm{Pb}^{4+}>\mathrm{Pb}^{2+}$
Bond order of $\mathrm{O}_2=2, \mathrm{O}_2^{+}=2.5, \mathrm{H}_2{ }^{+}=0.5, \mathrm{NO}=2.5$
NCERT 125
2 RBTS PAPER
160818
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
1 $\mathrm{CO}_2$
2 $\mathrm{HI}$
3 $\mathrm{H}_2 \mathrm{O}$
4 $\mathrm{SO}_2$
Explanation:
Thus, $\mathrm{H}_2 \mathrm{O}$ has highest dipole moment.
Mod. NEET
2 RBTS PAPER
160819
An ionic bond $A^{+} B^{-}$is most likely to be formed when:
1 the ionization energy of $A$ is high and the electron affinity of $B$ is low
2 the ionization energy of $A$ is low and the electron affinity of $B$ is high
3 the ionization energy of $A$ and the electron affinity of $B$ is high
4 the ionization energy of $A$ and the electron affinity of $B$ is low
Explanation:
If I.E. of $A$ is less, it will lose electron easily and E.A of $B$ is high it will gain electron easily so ionic bond is easily formed.
NCERT 102
2 RBTS PAPER
160820
Which of the following compounds of elements in group IV is expected to be most ionic ?
1 $\mathrm{PbCl}_2$
2 $\mathrm{PbCl}_4$
3 $\mathrm{CCl}_4$
4 $\mathrm{SiCl}_4$
Explanation:
Ionic character of a covalent bond $\propto \frac{1}{\phi}$ $\phi=\frac{\text { charg e }}{(\text { radius })^2}=\mathrm{C}^{4+}>\mathrm{Si}^{4+}>\mathrm{Pb}^{4+}>\mathrm{Pb}^{2+}$
