The sum of bond order of $\mathrm{O}_2^{2+}, \mathrm{O}_2^{2-}, \mathrm{O}_2^{+}, \mathrm{O}_2^{-}, \mathrm{O}_2$ and sum of the unpaired electrons present in them respectively are

$ \text { Which of the following sets are correctly matched? } $

$ \begin{array}{llll} \hline & \text { Molecule } & \text { Hybridisation } & \text { Geometry } \\ \hline \text { I. } & \mathrm{BrF}_5 & s p^3 d^2 & \text { Square pyramidal } \\ \hline \text { II. } & \mathrm{XeF}_6 & s p^3 d^3 & \text { Distorted octahedral } \\ \hline \text { III. } & \mathrm{SF}_4 & d s p^2 & \text { Square planar } \\ \hline \text { IV. } & \mathrm{PbCl}_2 & s p & \text { Linear } \\ \hline \end{array} $

The order of dipole moments of $\mathrm{H}_2 \mathrm{O}(A), \mathrm{CHCl}_3(B)$ and $\mathrm{NH}_3(C)$ is

$ \text { Match the following } $

The correct answer is

$ \text { Which of the following sets are correctly matched? } $

$ \begin{array}{llcc} \hline & \text { Molecule } & \begin{array}{c} \text { Number of lone } \\ \text { pair of electrons } \\ \text { on central atom } \end{array} & \text { Hybridisation } \\ \hline \text { (I) } & \mathrm{PCl}_3 & 1 & s p^3 \\ \hline \text { (II) } & \mathrm{SO}_2 & 2 & s p^3 \\ \hline \text { (III) } & \mathrm{SF}_4 & 2 & s p^3 d^2 \\ \hline \text { (IV) } & \mathrm{ClF}_3 & 2 & s p^3 d \\ \hline \end{array} $

The number of molecules having lone pair of electrons on central atom in the following is

$\mathrm{BF}_3, \mathrm{SF}_4, \mathrm{SiCl}_4, \mathrm{XeF}_4, \mathrm{NCl}_3, \mathrm{XeF}_6, \mathrm{PCl}_5, \mathrm{HgCl}_2, \mathrm{SnCl}_2$

Observe the following molecules/ions $\mathrm{NH}_4^{+}, \mathrm{NH}_3, \mathrm{BF}_3, \mathrm{OH}^{-}, \mathrm{CH}_3^{+}, \mathrm{H}^{+}, \mathrm{CO}, \mathrm{C}_2 \mathrm{H}_4$.

The number of Lewis bases in the above list is

Identify the set containing isoelectronic species

A molecules has T -shape. The total number of electron pairs in the valence shell of central atom of it is

How many of the following molecules have two lone pairs of electrons on central atom?

$\mathrm{SF}_6, \mathrm{BF}_3, \mathrm{ClF}_3, \mathrm{PCl}_5, \mathrm{BrF}_5, \mathrm{XeF}_4, \mathrm{H}_2 \mathrm{O}, \mathrm{SF}_4$

The pair of molecules / ions with the same bond order value is

How many of the following molecules / ions have trigonal planar structure?

$ \mathrm{BO}_3^{3-}, \mathrm{NH}_3, \mathrm{PCl}_3, \mathrm{BCl}_3, \mathrm{ClF}_3, \mathrm{XeO}_3 $

Consider the following

Assertion (A) Dipole moment of $\mathrm{NF}_3$ is lesser than $\mathrm{NH}_3$.

Reason (R) In $\mathrm{NF}_3$, the orbital dipole due to lone pair of electrons is in the opposite direction to the resultant dipole moment of the three $\mathrm{N}-\mathrm{F}$ bonds.

The correct answer is

Consider the following changes I and II

$ \mathrm{O}_2^{-} \underset{\text { II }}{\longleftarrow} \mathrm{O}_2 \xrightarrow[\text { I }]{ } \mathrm{O}_2^{+} $

The correct statements about these changes (I) and (II) in accordance with MO theory are

(A) In (I) bond order increases by 0.5 from the existing value

(B) In (II) bond order decreases by 1.0 from the existing value

(C) In both (I) and (II) magnetic property is not changed

(D) In both (I) and (II) magnetic property is changed

The increasing order of number of lone pair of electrons on the central atom of the following molecules is

(I) $\mathrm{ClF}_3$

(II) $\mathrm{XeF}_2$

(III) $\mathrm{SF}_4$

(IV) $\mathrm{SiH}_4$

Identify the correct set of molecules with zero dipole moment

Which of the following sets are correctly matched?

(i) $\mathrm{B}_2 \mathrm{H}_6$ - electron deficient hydride

(ii) $\mathrm{NH}_3$ - electron precise hydride

(iii) $\mathrm{H}_2 \mathrm{O}$ - electron rich hydride

Which of the following is /are ionic in nature?

(i) $\mathrm{GeF}_4$

(ii) $\mathrm{SnF}_4$

(iii) $\mathrm{PbF}_4$

The correct option is

$ \text { In the given structure of diborane } \theta_1, \theta_2 \text { are respectively } $

Which of the following orders are correct regarding their covalent character?

(i) $\mathrm{KF}<\mathrm{KI}$

(ii) $\mathrm{LiF}<\mathrm{KF}$

(iii) $\mathrm{SnCl}_2<\mathrm{SnCl}_4$

(iv) $\mathrm{NaCl}<\mathrm{CuCl}$

The correct option is

$ \text { Observe the following sets. } $

$ \begin{array}{lll} \hline \text { Order } & \text { Property } \\ \hline \text { (i) } \mathrm{NH}_3>\mathrm{H}_2 \mathrm{O}>\mathrm{SO}_2 & \text { Bond angle } \\ \hline \text { (ii) } \mathrm{H}_2 \mathrm{O}>\mathrm{NH}_3>\mathrm{H}_2 \mathrm{~S} & \text { Dipole moment } \\ \text { (iii) } \mathrm{N}_2>\mathrm{O}_2>\mathrm{H}_2 & \text { Bond enthalpy } \\ \hline \text { (iv) } \mathrm{NO}^{+}>\mathrm{O}_2>\mathrm{O}_2^{2-} & \text { Bond order } \\ \hline \end{array} $

$ \text { Observe the following structure, } $

$ \text { The formal charges on the atoms 1,2,3 respectively are } $

In the Lewis dot structure of carbonate ion shown under the formal charges on the oxygen atoms 1, 2 and 3 are respectively

The set of species having only fractional bond order values is

The set of molecules in which the central atom is not obeying the octet rule is

The formal charges of atoms (1), (2) and (3) in the ion is

The hybridisations of carbon in graphite, diamond and $\mathrm{C}_{60}$ are respectively

Choose the correct option from the following.

The bond lengths of $\mathrm{C}_2, \mathrm{~N}_2$ and $\mathrm{B}_2$ molecules are $X_1, X_2$ and $X_3 \mathrm{~pm}$ respectively. The correct order of their bond lengths is

A covalent molecule '$X Y^{\prime}$' is found to have a dipole moment of $1.5 \times 10^{-29} \mathrm{C} \cdot \mathrm{m}$ and $a$ bond length of $150 ~\mathrm{pm}$. The percent ionic character of the bond will be

The hybridisation of $\mathrm{Se}$ in $\mathrm{SeF}_4$ and its geometry respectively are :

Incorrect matching amongst the following is (according to geometry of molecules)

The element with maximum bond energy is

The correct order of electronegativity of carbon in various hybridisation states is

Bond order is an inverse measure of

Which of the following molecule has the maximum dipole moment?

Which compound among the following will have a permanent dipole moment?

The correct order of sulphur-oxygen bond in $\mathrm{SO}_3, \mathrm{~S}_2 \mathrm{O}_3^{2-}$ and $\mathrm{SO}_4^{2-}$ is

Which compound among the following has the highest dipole moment?

How many among the given species have a bond order of 0.5 ?

$\mathrm{H}_2^{+}, \mathrm{He}_2^{+}, \mathrm{He}_2^{-}, \mathrm{B}_2^{+}, \mathrm{F}_2^{-}, \mathrm{Be}_2^{2-}$

Match the following.

The structure of diborane B$_2$H$_6$ is given below. Identify the bond angles of x and y. In diborane, ........... are commonly known as banana-bonds.

The incorrect statement(s) among the following is/are

Due to $p \pi-p \pi$ bonding interactions, nitrogen for $\mathrm{N}_2$. But phosphorus forms .................. and does not form a diatomic molecule.

Identify the incorrect statements among the following?

(i) $\mathrm{SF}_6$ does not react with water.

(ii) $\mathrm{SF}_6$ is $s p^3 d$ hybridised.

(iii) $\mathrm{S}_2 \mathrm{O}_3^{2-}$ is a linear ion.

(iv) There is no $\pi$-bonding in $\mathrm{SO}_4^{2-}$ ion.

Given that ionisation potential and electron gain enthalpy of chlorine are 13eV and 4 eV respectively. The electronegativity of chlorine on Mulliken scale, approximately equals to

Which of the following will have maximum dipole moment?

In which of the following molecules/ions, the central atom is sp$^2$ hybridised?

BF$_3$, NO$_2^-$, NH$_2^-$ and H$_2$O

For which molecules among the following, the resultant dipole moment ($\propto$) $\ne$ 0 ?