Chemical Bonding & Molecular Structure · Chemistry · JEE Main

Bromine trifluoride autoionizes to form $\mathrm{BrF}_2^{\oplus}$ and $\mathrm{BrF}_4^{\ominus}$. The shapes of the cation and anion are respectively $\_\_\_\_$ and $\_\_\_\_$ .

Given below are two statements :

Statement I : The number of compounds among $\mathrm{SO}_2, \mathrm{SO}_3, \mathrm{SF}_4, \mathrm{SF}_6$ and $\mathrm{H}_2 \mathrm{~S}$ in which sulphur does not obey the Octet rule is 3 .

Statement II : Among $\left[\mathrm{H}_2 \mathrm{O}, \mathrm{ClF}_3, \mathrm{SF}_4\right],\left[\mathrm{NH}_3, \mathrm{BrF}_5, \mathrm{SF}_4\right],\left[\mathrm{BrF}_5, \mathrm{ClF}_3, \mathrm{XeF}_4\right]$ and [ $\mathrm{XeF}_4, \mathrm{ClF}_3, \mathrm{H}_2 \mathrm{O}$ ], the number of sets in which all the molecules have one lone pair of electrons on the central atom is 1 .

In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements :

Statement I : $\mathrm{F}_2 \mathrm{O}<\mathrm{H}_2 \mathrm{O}<\mathrm{Cl}_2 \mathrm{O}$ is the correct trend in terms of bond angle.

Statement II : $\mathrm{SiF}_4, \mathrm{SnF}_4$ and $\mathrm{PbF}_4$ are ionic in nature.

In the light of the above statements, choose the correct answer from the options given below :

The pairs among

$\mathrm{A}=\left[\mathrm{SO}_3^{2-}, \mathrm{CO}_3^{2-}\right], \mathrm{B}=\left[\mathrm{O}_2^{2-}, \mathrm{F}_2\right], \mathrm{C}=\left[\mathrm{CN}^{-}, \mathrm{CO}\right], \mathrm{D}=\left[\mathrm{NH}_3, \mathrm{H}_3 \mathrm{O}^{+}\right]$and $\mathrm{E}=\left[\mathrm{MnO}_4^{2-}, \mathrm{CrO}_4^{2-}\right]$ that do not have similar Lewis dot structure are

The covalent radii of atoms $A$ and $B$ are $r_A$ and $r_B$, respectively. The covalent bond length and total length of AB molecule are respectively

Which of the following pictorial diagram most correctly represents the $\pi^*$ ( $\pi$ antibonding) molecular orbital between two atoms if the internuclear axis is taken to be in the $z$-direction $(\xrightarrow{z \text {-axis }})$ ?

SF$_4$ is isostructural with :

A. BrF$_4^\ominus$

B. CH$_4$

C. IF$_4^{\oplus}$

D. XeF$_4$

E. XeO$_2$F$_2$

Choose the correct answer from the options given below :

Given below are two statements :

Statement (I): The correct sequence of bond lengths in the following species is :

$\ce{O2^{+}} < \ce{O2} < \ce{O2^{-}} < \ce{O2^{2-}}$

Statement (II): The correct sequence of number of unpaired electrons in the following species is :

$\ce{O2} > \ce{O2^{+}} > \ce{O2^{-}} > \ce{O2^{2-}}$

In the light of the above statements, choose the correct answer from the options given below :

Match List - I with List - II according to shape.

Choose the correct answer from the options given below :

Given below are two statements :

Statement I : The number of species among $\mathrm{BF}_4^{-}, \mathrm{SiF}_4, \mathrm{XeF}_4$ and $\mathrm{SF}_4$, that have unequal $\mathrm{E}-\mathrm{F}$ bond lengths is two. Here, E is the central atom.

Statement II : Among $\mathrm{O}_2^{-}, \mathrm{O}_2^{2-}, \mathrm{F}_2$ and $\mathrm{O}_2^{+}, \mathrm{O}_2^{-}$has the highest bond order.

In the light of the above statements, choose the correct answer from the options given below

Pair of species among the following having same bond order as well as paramagnetic character will be-

Given below are statements about some molecules/ions.

Identify the CORRECT statements.

A. The dipole moment value of $\mathrm{NF}_3$ is higher than that of $\mathrm{NH}_3$.

B. The dipole moment value of $\mathrm{BeH}_2$ is zero.

C. The bond order of $\mathrm{O}_2{ }^{2-}$ and $\mathrm{F}_2$ is same.

D. The formal charge on the central oxygen atom of ozone is -1 .

E. In $\mathrm{NO}_2$, all the three atoms satisfy the octet rule, hence it is very stable.

Choose the correct answer from the options given below:

Among the following, the CORRECT combinations are

A. $\mathrm{IF}_3 \rightarrow \mathrm{~T}$-shaped ( $\mathrm{sp}^3 \mathrm{~d}$ )

B. $\mathrm{IF}_5 \rightarrow$ Square pyramidal $\left(\mathrm{sp}^3 \mathrm{~d}^2\right)$

C. $\mathrm{IF}_7 \rightarrow$ Pentagonal bipyramidal $\left(\mathrm{sp}^3 \mathrm{~d}^3\right)$

D. $\mathrm{ClO}_4{ }^{-} \rightarrow$ Square planar ( $\mathrm{sp}^2 \mathrm{~d}$ )

Choose the correct answer from the options given below:

Which statements are NOT TRUE about $\mathrm{XeO}_2 \mathrm{~F}_2$?

A. It has a see-saw shape.

B. Xe has 5 electron pairs in its valence shell in $\mathrm{XeO}_2 \mathrm{~F}_2$.

C. The $\mathrm{O}-\mathrm{Xe}-\mathrm{O}$ bond angle is close to $180^{\circ}$.

D. The $\mathrm{F}-\mathrm{Xe}-\mathrm{F}$ bond angle is close to $180^{\circ}$.

E. Xe has 16 valence electrons in $\mathrm{XeO}_2 \mathrm{~F}_2$.

Choose the correct answer from the options given below :

Identify the molecule $(X)$ with maximum number of lone pairs of electrons (obtained using Lewis dot structure) among $\mathrm{HNO}_3, \mathrm{H}_2 \mathrm{SO}_4, \mathrm{NF}_3$ and $\mathrm{O}_3$. Choose the correct bond angle made by the central atom of the molecule $(X)$.

Among $\mathrm{H}_2 \mathrm{~S}, \mathrm{H}_2 \mathrm{O}, \mathrm{NF}_3, \mathrm{NH}_3$ and $\mathrm{CHCl}_3$, identify the molecule $(\mathrm{X})$ with lowest dipole moment value. The number of lone pairs of electrons present on the central atom of the molecule $(X)$ is :

Two p-block elements X and Y form fluorides of the type $\mathrm{EF}_3$. The fluoride compound $\mathrm{XF}_3$ is a Lewis acid and $\mathrm{YF}_3$ is a Lewis base. The hybridizations of the central atoms of $\mathrm{XF}_3$ and $\mathrm{YF}_3$ respectively are

The formal charges on the atoms marked as (1) to (4) in the Lewis representation of $\mathrm{HNO}_3$ molecule respectively are

The correct increasing order of C–H(A), C–O(B), C=O(C) and C≡N(D) bonds in terms of covalent bond length is :

Given below are two statements :

Statement I : The correct order in terms of bond dissociation enthalpy is Cl₂ > Br₂ > F₂ > I₂.

Statement II : The correct trend in the covalent character of the metal halides is [SnCl₄ > SnCl₂], [PbCl₄ > PbCl₂] and [UF₄ > UF₆].

In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements :

Statement I :

The number of species among $\mathrm{SF}_4, \mathrm{NH}_4^{+},\left[\mathrm{NiCl}_4\right]^{2-}, \mathrm{XeF}_4,\left[\mathrm{PtCl}_4\right]^{2-}, \mathrm{SeF}_4$ and $\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$, that have tetrahedral geometry is 3 .

Statement II :

In the set [ $\mathrm{NO}_2, \mathrm{BeH}_2, \mathrm{BF}_3, \mathrm{AlCl}_3$ ], all the molecules have incomplete octet around central atom.

In the light of the above statements, choose the correct answer from the options given below:

In SO₂, NO₂^$-$ and N₃^$-$, the hybridizations at the central atom are respectively :

Given below are two statements :

Statement (I) : is more polar than

Statement (II) : Boiling point of is lower than but it is more polar than .

In the light of the above statements, choose the most appropriate answer from the options given below :

Match the List I with List II.

Choose the correct answer from the options given below:

Given below are two statements:

Statement (I): For , all three possible structures may be drawn as follows.

Statement (II): Structure III is most stable, as the orbitals having the lone pairs are axial, where the lp – bp repulsion is minimum.

In the light of the above statements, choose the most appropriate answer from the options given below:

Given below are two statements.

In the light of the above statements, choose the correct answer from the options given below:

Which of the following molecule(s) show/s paramagnetic behavior?

A. $\mathrm{O}_2$

B. $\mathrm{N}_2$

C. $\mathrm{F}_2$

D. $\mathrm{S}_2$

E. $\mathrm{Cl}_2$

Choose the correct answer from the options given below:

Given below are two statements:

Statement I : Wet cotton clothes made of cellulose based carbohydrate takes comparatively longer time to get dried than wet nylon polymer based clothes.

Statement II : Intermolecular hydrogen bonding with water molecule is more in nylon-based clothes than in the case of cotton clothes.

In the light of above statements, choose the correct answer from the options given below

A molecule with the formula $\mathrm{AX}_4 \mathrm{Y}$ has all it's elements from p-block. Element A is rarest, monoatomic, non-radioactive from its group and has the lowest ionization enthalpy value among $\mathrm{A}, \mathrm{X}$ and Y . Elements X and Y have first and second highest electronegativity values respectively among all the known elements. The shape of the molecule is:

Among $\mathrm{SO}_2, \mathrm{NF}_3, \mathrm{NH}_3, \mathrm{XeF}_2, \mathrm{ClF}_3$ and $\mathrm{SF}_4$, the hybridization of the molecule with nonzero dipole moment and highest number of lone-pairs of electrons on the central atom is

Consider the following molecules:

The correct order of rate of hydrolysis is :

Consider ' n ' is the number of lone pair of electrons present in the equatorial position of the most stable structure of $\mathrm{ClF}_3$. The ions from the following with ' n ' number of unpaired electrons are

A. $\mathrm{V}^{3+}$

B. $\mathrm{Ti}^{3+}$

C. $\mathrm{Cu}^{2+}$

D. $\mathrm{Ni}^{2+}$

E. $\mathrm{Ti}^{2+}$

Choose the correct answer from the options given below:

The molecules having square pyramidal geometry are

Given below are two statements :

Statement (I) : Experimentally determined oxygen-oxygen bond lengths in the $\mathrm{O}_3$ are found to be same and the bond length is greater than that of a $\mathrm{O}=\mathrm{O}$ (double bond) but less than that of a single $(\mathrm{O}-\mathrm{O})$ bond.

Statement (II) : The strong lone pair-lone pair repulsion between oxygen atoms is solely responsible for the fact that the bond length in ozone is smaller than that of a double bond $(\mathrm{O}=\mathrm{O})$ but more than that of a single bond $(\mathrm{O}-\mathrm{O})$.

In the light of the above statements, choose the correct answer from the options given below :

Which of the following linear combination of atomic orbitals will lead to formation of molecular orbitals in homonuclear diatomic molecules [internuclear axis in $z$-direction] ?

A. $2 \mathrm{p}_{\mathrm{z}}$ and $2 \mathrm{p}_{\mathrm{x}}$

B. 2 s and $2 \mathrm{p}_{\mathrm{x}}$

C. $3 d_{x y}$ and $3 d_{x^2-y^2}$

D. 2 s and $2 \mathrm{p}_{\mathrm{z}}$

E. $2 p_z$ and $3 d_{x^2-y^2}$

Choose the correct answer from the options given below:

Which of the following statement is true with respect to $\mathrm{H}_2 \mathrm{O}, \mathrm{NH}_3$ and $\mathrm{CH}_4$ ?

A. The central atoms of all the molecules are $\mathrm{sp}^3$ hybridized.

B. The $\mathrm{H}-\mathrm{O}-\mathrm{H}, \mathrm{H}-\mathrm{N}-\mathrm{H}$ and $\mathrm{H}-\mathrm{C}-\mathrm{H}$ angles in the above molecules are $104.5^{\circ}, 107.5^{\circ}$ and $109.5^{\circ}$, respectively.

C. The increasing order of dipole moment is $\mathrm{CH}_4<\mathrm{NH}_3<\mathrm{H}_2 \mathrm{O}$.

D. Both $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{NH}_3$ are Lewis acids and $\mathrm{CH}_4$ is a Lewis base.

E. A solution of $\mathrm{NH}_3$ in $\mathrm{H}_2 \mathrm{O}$ is basic. In this solution $\mathrm{NH}_3$ and $\mathrm{H}_2 \mathrm{O}$ act as Lowry-Bronsted acid and base respectively.

Choose the correct answer from the options given below:

Match the List - I with List - II

Choose the correct answer from the options given below:

Arrange the following compounds in increasing order of their dipole moment :

$\mathrm{HBr}, \mathrm{H}_2 \mathrm{~S}, \mathrm{NF}_3$ and $\mathrm{CHCl}_3$

The correct increasing order for bond angles among $$\mathrm{BF}_3, \mathrm{PF}_3$$ and $$\mathrm{ClF}_3$$ is :

In which one of the following pairs the central atoms exhibit $$\mathrm{sp}^2$$ hybridization ?

The shape of carbocation is :

When $$\psi_{\mathrm{A}}$$ and $$\psi_{\mathrm{B}}$$ are the wave functions of atomic orbitals, then $$\sigma^*$$ is represented by :

Match List I with List II

Choose the correct answer from the options given below:

Match List I with List II

Choose the correct answer from the options given below:

Match List I with List II

Choose the correct answer from the options given below:

Match List I with List II.

Choose the correct answer from the options given below :

Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).

Assertion (A) : $$\mathrm{NH}_3$$ and $$\mathrm{NF}_3$$ molecule have pyramidal shape with a lone pair of electrons on nitrogen atom. The resultant dipole moment of $$\mathrm{NH}_3$$ is greater than that of $$\mathrm{NF}_3$$.

Reason (R) : In $$\mathrm{NH}_3$$, the orbital dipole due to lone pair is in the same direction as the resultant dipole moment of the $$\mathrm{N}-\mathrm{H}$$ bonds. $$\mathrm{F}$$ is the most electronegative element.

In the light of the above statements, choose the correct answer from the options given below :

Number of $$\sigma$$ and $$\pi$$ bonds present in ethylene molecule is respectively :

The correct statement/s about Hydrogen bonding is/are

A. Hydrogen bonding exists when H is covalently bonded to the highly electro negative atom.

B. Intermolecular H bonding is present in $$o$$-nitro phenol

C. Intramolecular $$\mathrm{H}$$ bonding is present in HF.

D. The magnitude of $$\mathrm{H}$$ bonding depends on the physical state of the compound.

E. H-bonding has powerful effect on the structure and properties of compounds

Choose the correct answer from the options given below:

The number of species from the following that have pyramidal geometry around the central atom is _________

$$\mathrm{S}_2 \mathrm{O}_3^{2-}, \mathrm{SO}_4^{2-}, \mathrm{SO}_3^{2-}, \mathrm{S}_2 \mathrm{O}_7^{2-}$$

Number of molecules/ions from the following in which the central atom is involved in $$\mathrm{sp}^3$$ hybridization is ________.

$$\mathrm{NO}_3^{-}, \mathrm{BCl}_3, \mathrm{ClO}_2^{-}, \mathrm{ClO}_3^{-}$$

Which one of the following molecules has maximum dipole moment?

Which of the following is least ionic?

The linear combination of atomic orbitals to form molecular orbitals takes place only when the combining atomic orbitals

A. have the same energy

B. have the minimum overlap

C. have same symmetry about the molecular axis

D. have different symmetry about the molecular axis

Choose the most appropriate from the options given below:

Given below are two statements:

Statement - I: Since Fluorine is more electronegative than nitrogen, the net dipole moment of $$\mathrm{NF}_3$$ is greater than $$\mathrm{NH}_3$$.

Statement - II: In $$\mathrm{NH}_3$$, the orbital dipole due to lone pair and the dipole moment of $$\mathrm{NH}$$ bonds are in opposite direction, but in $$\mathrm{NF}_3$$ the orbital dipole due to lone pair and dipole moments of N-F bonds are in same direction.

In the light of the above statements, choose the most appropriate from the options given below:

The molecule / ion with square pyramidal shape is

Aluminium chloride in acidified aqueous solution forms an ion having geometry

Match List I with List II.

Choose the correct answer from the options given below :

Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).

Assertion (A) : There is a considerable increase in covalent radius from $$\mathrm{N}$$ to $$\mathrm{P}$$. However from As to Bi only a small increase in covalent radius is observed.

Reason (R) : Covalent and ionic radii in a particular oxidation state increases down the group. In the light of the above statements, choose the most appropriate answer from the options given below:

The difference in energy between the actual structure and the lowest energy resonance structure for the given compound is

Choose the polar molecule from the following:

Given below are two statements :

Statement I : $$\mathrm{SO}_{2}$$ and $$\mathrm{H}_{2} \mathrm{O}$$ both possess V-shaped structure.

Statement II : The bond angle of $$\mathrm{SO}_{2}$$ is less than that of $$\mathrm{H}_{2} \mathrm{O}$$.

In the light of the above statements, choose the most appropriate answer from the options given below:

In which of the following processes, the bond order increases and paramagnetic character changes to diamagnetic one ?

The bond order and magnetic property of acetylide ion are same as that of

Match List - I with List - II:

Choose the correct answer from the options given below:

The compound which does not exist is

Match List I with List II

Choose the correct answer from the options given below:

$$\mathrm{O}-\mathrm{O}$$ bond length in $$\mathrm{H}_{2} \mathrm{O}_{2}$$ is $$\underline{\mathrm{X}}$$ than the $$\mathrm{O}-\mathrm{O}$$ bond length in $$\mathrm{F}_{2} \mathrm{O}_{2}$$. The $$\mathrm{O}-\mathrm{H}$$ bond length in $$\mathrm{H}_{2} \mathrm{O}_{2}$$ is $$\underline{Y}$$ than that of the $$\mathrm{O}-\mathrm{F}$$ bond in $$\mathrm{F}_{2} \mathrm{O}_{2}$$.

Choose the correct option for $$\underline{X}$$ and $$\underline{Y}$$ from those given below :

Match List I with List II

Choose the correct answer from the options given below :

For $$\mathrm{OF}_{2}$$ molecule consider the following :

A. Number of lone pairs on oxygen is 2 .

B. FOF angle is less than $$104.5^{\circ}$$.

C. Oxidation state of $$\mathrm{O}$$ is $$-2$$.

D. Molecule is bent '$$\mathrm{V}$$' shaped.

E. Molecular geometry is linear.

correct options are:

Match List I with List II

Choose the correct answer from the options given below :

According to MO theory the bond orders for $$\mathrm{O}$$$$_2^{2 - }$$, $$\mathrm{CO}$$ and $$\mathrm{NO^+}$$ respectively, are

The magnetic behaviour of $$\mathrm{Li_2O,Na_2O_2}$$ and $$\mathrm{KO_2}$$, respectively, are :

The bond dissociation energy is highest for

Statement I : Dipole moment is a vector quantity and by convention it is depicted by a small arrow with tail on the negative centre and head pointing towards the positive centre.

Statement II : The crossed arrow of the dipole moment symbolizes the direction of the shift of charges in the molecules.

In the light of the above statements, choose the most appropriate answer from the options given below :

What is the number of unpaired electron(s) in the highest occupied molecular orbital of the following species : $$\mathrm{{N_2};N_2^ + ;{O_2};O_2^ + }$$ ?

Decreasing order of the hydrogen bonding in following forms of water is correctly represented by

A. Liquid water

B. Ice

C. Impure water

Choose the correct answer from the options given below :

Order of Covalent bond;

$$\mathrm{A.~KF > KI ; LiF > KF}$$

$$\mathrm{B.~KF < KI ; LiF > KF}$$

$$\mathrm{C.~SnCl_4 > SnCl_2 ; CuCl > NaCl}$$

$$\mathrm{D.~LiF > KF ; CuCl < NaCl}$$

$$\mathrm{E.~KF < KI ; CuCl > NaCl}$$

Choose the correct answer from the options given below :

Which of the following pair of molecules contain odd electron molecule and an expanded octet molecule?

Number of lone pairs of electrons in the central atom of $$\mathrm{SCl}_{2}, \mathrm{O}_{3}, \mathrm{ClF}_{3}$$ and $$\mathrm{SF}_{6}$$, respectively, are :

Match List - I with List - II.

Choose the correct answer from the options given below :

Given below are two statements.

Statement I: $$\mathrm{O}_{2}, \mathrm{Cu}^{2+}$$, and $$\mathrm{Fe}^{3+}$$ are weakly attracted by magnetic field and are magnetized in the same direction as magnetic field.

Statement II: $$\mathrm{NaCl}$$ and $$\mathrm{H}_{2} \mathrm{O}$$ are weakly magnetized in opposite direction to magnetic field.

In the light of the above statements, choose the most appropriate answer from the options given below.

Arrange the following in increasing order of their covalent character.

A. $$\mathrm{CaF}_{2}$$

B. $$\mathrm{CaCl}_{2}$$

C. $$\mathrm{CaBr}_{2}$$

D. $$\mathrm{CaI}_{2}$$

Choose the correct answer from the options given below.

Match List-I with List-II :

Choose the correct answer from the options given below :

Match List I with List II:

Choose the correct answer from the options given below:

Consider the species CH₄, NH$$_4^ + $$ and BH$$_4^ - $$. Choose the correct option with respect to the these species.

Number of lone pair(s) of electrons on central atom and the shape BrF₃ molecule respectively, are

In the structure of SF₄, the lone pair of electrons on S is in.

Identify the incorrect statement for PCl₅ from the following.

The correct order of increasing intermolecular hydrogen bond strength is :

Based upon VSEPR theory, match the shape (geometry) of the molecules in List-I with the molecules in List-II and select the most appropriate option.

Consider the ions/molecule

O$$_2^ + $$, O₂, O$$_2^ - $$, O$$_2^ {2-} $$

For increasing bond order the correct option is :

Bonding in which of the following diatomic molecule(s) become(s) stronger, on the basis of MO Theory, by removal of an electron?

(A) NO

(B) N₂

(C) O₂

(D) C₂

(E) B₂

Choose the most appropriate answer from the options given below :

Number of electron deficient molecules among the following

PH₃, B₂H₆, CCl₄, NH₃, LiH and BCl₃ is

The correct order of bond orders of $${C_2}^{2 - }$$, $${N_2}^{2 - }$$ and $${O_2}^{2 - }$$

Consider the following species:

$$ \mathrm{BrF}_5, \mathrm{XeF}_5^{-}, \mathrm{BF}_4^{-}, \mathrm{ICl}_4^{-}, \mathrm{XeF}_4, \mathrm{SF}_4, \mathrm{NH}_4^{+}, \mathrm{ClF}_3, \mathrm{XeF}_2, \mathrm{ICl}_2^{-} $$

Number of species having $\mathrm{sp}^3 \mathrm{~d}$ hybridized central atom is $\_\_\_\_$ .

According to Lewis theory, the total number of $\sigma$ bond-pairs and lone pair of electrons around the central atom of $\mathrm{XeO}_6{ }^{4-}$ ion is $\_\_\_\_$ .

Total number of non-bonded electrons present in NO₂^$-$ ion based on Lewis theory is ______.

The number of molecules/ions that show linear geometry among the following is __________.

$\mathrm{SO}_2, \mathrm{BeCl}_2, \mathrm{CO}_2, \mathrm{~N}_3^{-}, \mathrm{NO}_2, \mathrm{~F}_2 \mathrm{O}, \mathrm{XeF}_2, \mathrm{NO}_2^{+}, \mathrm{I}_3^{-}, \mathrm{O}_3$

Total number of electrons present in $$\left(\pi^*\right)$$ molecular orbitals of $$\mathrm{O}_2, \mathrm{O}_2^{+}$$ and $$\mathrm{O}_2^{-}$$ is ________.

The total number of species from the following in which one unpaired electron is present, is _______.

$$\mathrm{N}_2, \mathrm{O}_2, \mathrm{C}_2^{-}, \mathrm{O}_2^{-}, \mathrm{O}_2^{2-}, \mathrm{H}_2^{+}, \mathrm{CN}^{-}, \mathrm{He}_2^{+}$$

Number of molecules having bond order 2 from the following molecules is _________.

$$\mathrm{C}_2, \mathrm{O}_2, \mathrm{Be}_2, \mathrm{Li}_2, \mathrm{Ne}_2, \mathrm{~N}_2, \mathrm{He}_2$$

Number of molecules from the following which are exceptions to octet rule is _________.

$$\mathrm{CO}_2, \mathrm{NO}_2, \mathrm{H}_2 \mathrm{SO}_4, \mathrm{BF}_3, \mathrm{CH}_4, \mathrm{SiF}_4, \mathrm{ClO}_2, \mathrm{PCl}_5, \mathrm{BeF}_2, \mathrm{C}_2 \mathrm{H}_6, \mathrm{CHCl}_3, \mathrm{CBr}_4$$

Consider the following reactions

The number of protons that do not involve in hydrogen bonding in the product B is _________.

Total number of species from the following with central atom utilising $$\mathrm{sp}^2$$ hybrid orbitals for bonding is ________.

$$\mathrm{NH}_3, \mathrm{SO}_2, \mathrm{SiO}_2, \mathrm{BeCl}_2, \mathrm{C}_2 \mathrm{H}_2, \mathrm{C}_2 \mathrm{H}_4, \mathrm{BCl}_3, \mathrm{HCHO}, \mathrm{C}_6 \mathrm{H}_6, \mathrm{BF}_3, \mathrm{C}_2 \mathrm{H}_4 \mathrm{Cl}_2$$

Number of molecules from the following which can exhibit hydrogen bonding is _________. (nearest integer)

Number of compounds from the following with zero dipole moment is _________.

$$\mathrm{HF}, \mathrm{H}_2, \mathrm{H}_2 \mathrm{~S}, \mathrm{CO}_2, \mathrm{NH}_3, \mathrm{BF}_3, \mathrm{CH}_4, \mathrm{CHCl}_3, \mathrm{SiF}_4, \mathrm{H}_2 \mathrm{O}, \mathrm{BeF}_2$$

In the lewis dot structure for $$\mathrm{NO}_2^{-}$$, total number of valence electrons around nitrogen is _________.

Number of compounds / species from the following with non-zero dipole moment is _________.

$$\mathrm{BeCl}_2, \mathrm{BCl}_3, \mathrm{NF}_3, \mathrm{XeF}_4, \mathrm{CCl}_4, \mathrm{H}_2 \mathrm{O}, \mathrm{H}_2 \mathrm{~S}, \mathrm{HBr}, \mathrm{CO}_2, \mathrm{H}_2, \mathrm{HCl}$$

Number of molecules/species from the following having one unpaired electron is ________.

$$\mathrm{O}_2, \mathrm{O}_2^{-1}, \mathrm{NO}, \mathrm{CN}^{-1}, \mathrm{O}_2^{2-}$$

A diatomic molecule has a dipole moment of $$1.2 \mathrm{~D}$$. If the bond distance is $$1 \mathrm{~A}^{\circ}$$, then fractional charge on each atom is _________ $$\times 10^{-1}$$ esu.

(Given $$1 \mathrm{~D}=10^{-18}$$ esucm)

The number of species from the following in which the central atom uses $$\mathrm{sp}^3$$ hybrid orbitals in its bonding is __________.

$$\mathrm{NH}_3, \mathrm{SO}_2, \mathrm{SiO}_2, \mathrm{BeCl}_2, \mathrm{CO}_2, \mathrm{H}_2 \mathrm{O}, \mathrm{CH}_4, \mathrm{BF}_3$$

The total number of molecular orbitals formed from $$2 \mathrm{s}$$ and $$2 \mathrm{p}$$ atomic orbitals of a diatomic molecule is __________.

The total number of molecules with zero dipole moment among $$\mathrm{CH}_4, \mathrm{BF}_3, \mathrm{H}_2 \mathrm{O}, \mathrm{HF}, \mathrm{NH}_3, \mathrm{CO}_2$$ and $$\mathrm{SO}_2$$ is ________.

The total number of anti bonding molecular orbitals, formed from $$2 s$$ and $$2 p$$ atomic orbitals in a diatomic molecule is _______.

The number of species from the following which are paramagnetic and with bond order equal to one is _________.

$$\mathrm{H}_2, \mathrm{He}_2^{+}, \mathrm{O}_2^{+}, \mathrm{N}_2^{2-}, \mathrm{O}_2^{2-}, \mathrm{F}_2, \mathrm{Ne}_2^{+}, \mathrm{B}_2$$

Number of compounds with one lone pair of electrons on central atom amongst following is _________.

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

The number of non-polar molecules from the following is _________. $$\mathrm{HF}, \mathrm{H}_2 \mathrm{O}, \mathrm{SO}_2, \mathrm{H}_2, \mathrm{CO}_2, \mathrm{CH}_4, \mathrm{NH}_3, \mathrm{HCl}, \mathrm{CHCl}_3, \mathrm{BF}_3$$

Sum of bond order of CO and NO$$^+$$ is ________.

The maximum number of lone pairs of electrons on the central atom from the following species is ____________.

$$\mathrm{ClO}_{3}{ }^{-}, \mathrm{XeF}_{4}, \mathrm{SF}_{4}$$ and $$\mathrm{I}_{3}{ }^{-}$$

The number of molecules from the following which contain only two lone pair of electrons is ________

$$\mathrm{H}_{2} \mathrm{O}, \mathrm{N}_{2}, \mathrm{CO}, \mathrm{XeF}_{4}, \mathrm{NH}_{3}, \mathrm{NO}, \mathrm{CO}_{2}, \mathrm{~F}_{2}$$

The number of bent-shaped molecule/s from the following is __________

N$$_3^-$$, NO$$_2^-$$, I$$_3^-$$, O$$_3$$, SO$$_2$$

The sum of lone pairs present on the central atom of the interhalogen IF$$_5$$ and IF$$_7$$ is _________

The number of species from the following carrying a single lone pair on central atom Xenon is ___________.

$$\mathrm{XeF}_{5}^{+}, \mathrm{XeO}_{3}, \mathrm{XeO}_{2} \mathrm{~F}_{2}, \mathrm{XeF}_{5}^{-}, \mathrm{XeO}_{3} \mathrm{~F}_{2}, \mathrm{XeOF}_{4}, \mathrm{XeF}_{4}$$

The number of following factors which affect the percent covalent character of the ionic bond is _________

(A) Polarising power of cation

(B) Extent of distortion of anion

(C) Polarisability of the anion

(D) Polarising power of anion

The number of species having a square planar shape from the following is __________.

$$\mathrm{XeF}_{4}, \mathrm{SF}_{4}, \mathrm{SiF}_{4}, \mathrm{BF}_{4}^{-}, \mathrm{BrF}_{4}^{-},\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+},\left[\mathrm{FeCl}_{4}\right]^{2-},\left[\mathrm{PtCl}_{4}\right]^{2-}$$

In an ice crystal, each water molecule is hydrogen bonded to ____________ neighbouring molecules.

The number of species from the following which have square pyramidal structure is _________

$$\mathrm{PF}_{5}, \mathrm{BrF}_{4}^{-}, \mathrm{IF}_{5}, \mathrm{BrF}_{5}, \mathrm{XeOF}_{4}, \mathrm{ICl}_{4}^{-}$$

The number of molecules or ions from the following, which do not have odd number of electrons are _________.

(A) NO$$_2$$

(B) ICl$$_4^ - $$

(C) BrF$$_3$$

(D) ClO$$_2$$

(E) NO$$_2^ + $$

(F) NO

The total number of lone pairs of electrons on oxygen atoms of ozone is __________.

Consider, $$\mathrm{PF}_{5}, \mathrm{BrF}_{5}, \mathrm{PCl}_{3}, \mathrm{SF}_{6},\left[\mathrm{ICl}_{4}\right]^{-}, \mathrm{ClF}_{3}$$ and $$\mathrm{IF}_{5}$$.

Amongst the above molecule(s)/ion(s), the number of molecule(s)/ion(s) having $$\mathrm{sp}^{3}\mathrm{~d}^{2}$$ hybridisation is __________.

The number of paramagnetic species among the following is ___________.

$$\mathrm{B}_{2}, \mathrm{Li}_{2}, \mathrm{C}_{2}, \mathrm{C}_{2}^{-}, \mathrm{O}_{2}^{2-}, \mathrm{O}_{2}^{+}$$ and $$\mathrm{He}_{2}^{+}$$

The number of interhalogens from the following having square pyramidal structure is :

$$\mathrm{ClF}_{3}, \mathrm{IF}_{7}, \mathrm{BrF}_{5}, \mathrm{BrF}_{3}, \mathrm{I}_{2} \mathrm{Cl}_{6}, \mathrm{IF}_{5}, \mathrm{ClF}, \mathrm{ClF}_{5}$$

The number of molecule(s) or ion(s) from the following having non-planar structure is ____________.

$$\mathrm{NO}_{3}^{-}, \mathrm{H}_{2} \mathrm{O}_{2}, \mathrm{BF}_{3}, \mathrm{PCl}_{3}, \mathrm{XeF}_{4}, \mathrm{SF}_{4}, \mathrm{XeO}_{3}, \mathrm{PH}_{4}^{+}, \mathrm{SO}_{3},\left[\mathrm{Al}(\mathrm{OH})_{4}\right]^{-}$$

Amongst the following, the number of oxide(s) which are paramagnetic in nature is

$$\mathrm{Na}_{2} \mathrm{O}, \mathrm{KO}_{2}, \mathrm{NO}_{2}, \mathrm{~N}_{2} \mathrm{O}, \mathrm{ClO}_{2}, \mathrm{NO}, \mathrm{SO}_{2}, \mathrm{Cl}_{2} \mathrm{O}$$

According to MO theory, number of species/ions from the following having identical bond order is ________.

$$\mathrm{CN}^{-}, \mathrm{NO}^{+}, \mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{2+}$$

The sum of number of lone pairs of electrons present on the central atoms of XeO₃, XeOF₄ and XeF₆, is ______________

Among the following species

$$\mathrm{N}_{2}, \mathrm{~N}_{2}^{+}, \mathrm{N}_{2}^{-}, \mathrm{N}_{2}^{2-}, \mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{-}, \mathrm{O}_{2}^{2-}$$

the number of species showing diamagnesim is _______________.

Amongst the following, the number of molecule/(s) having net resultant dipole moment is ____________.

NF₃, BF₃, BeF₂, CHCl₃, H₂S, SiF₄, CCl₄, PF₅

The hybridization of P exhibited in PF₅ is sp^xd^y. The value of y is __________.

Amongst SF₄, XeF₄, CF₄ and H₂O, the number of species with two lone pairs of electrons is _____________.

Amongst BeF₂, BF₃, H₂O, NH₃, CCl₄ and HCl, the number of molecules with non-zero net dipole moment is ____________.