Chemical Bonding

Consider the molecules \ce{CH4}, \ce{NH3} and \ce{H2O}. Which of the given statements is false?

Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

Predict the correct order among the following (repulsion between electron pairs as per VSEPR theory):

Match the compounds in Column I with the hybridization and shape in Column II and mark the correct option. Column I: (a) \ce{XeF6}, (b) \ce{XeO3}, (c) \ce{XeOF4}, (d) \ce{XeF4} Column II: (i) Distorted octahedral, (ii) Square planar, (iii) Pyramidal, (iv) Square pyramidal

The lone pair of electrons in the given carbanion, \ce{CH3-C#C^-}, is present in which of the following orbitals?

Which one of the following compounds shows the presence of intramolecular hydrogen bond?

The hybridizations of the atomic orbitals of nitrogen in \ce{NO2+}, \ce{NO3^-} and \ce{NH4+} respectively are

Which of the following pairs of ions is isoelectronic and isostructural?

The correct geometry and hybridization for \ce{XeF4} are

Among the following, which one is a wrong statement?

Which of the following pairs of compounds is isoelectronic and isostructural?

Choose the correct statement:

Which of the following statements is not correct about diborane?

Match the interhalogen compounds of Column I with the geometry in Column II and assign the correct code. Column I: (a) \ce{XX'}, (b) \ce{XX'3}, (c) \ce{XX'5}, (d) \ce{XX'7} Column II: (i) T-shape, (ii) Pentagonal bipyramidal, (iii) Linear, (iv) Square pyramidal, (v) Tetrahedral

The most suitable method of separation of a 1 : 1 mixture of ortho- and para-nitrophenols is

Which one of the following pairs of species have the same bond order?

Which one of the following elements is unable to form \ce{MF6^3-} ion?

In the structure of \ce{ClF3}, the number of lone pairs of electrons on the central atom Cl is:

Which of the following molecules represents the order of hybridisation $sp^2$, $sp^2$, $sp$, $sp$ from left to right atoms?

Carboxylic acids have higher boiling points than aldehydes, ketones and even alcohols of comparable molecular mass. This is due to their:

Consider the following species: \ce{CN^+}, \ce{CN^-}, \ce{NO} and \ce{CN}. Which of these will have the highest bond order?

The number of sigma ($\sigma$) and pi ($\pi$) bonds in pent-2-en-4-yne is

Which of the following diatomic molecular species has only $\pi$ bonds according to Molecular Orbital Theory?

Match the Xenon compounds in Column-I with their structure in Column-II and assign the correct code: Column-I: (a) \ce{XeF4}, (b) \ce{XeF6}, (c) \ce{XeOF4}, (d) \ce{XeO3} Column-II: (i) pyramidal, (ii) square planar, (iii) distorted octahedral, (iv) square pyramidal

Which amongst the following is an incorrect statement?

Aluminium chloride in acidified aqueous solution forms a complex 'A', in which the hybridisation state of Al is 'B'. What are 'A' and 'B', respectively?

Which of the following is paramagnetic?

Which of the following is the correct order of dipole moment?

The number of hydrogen bonded water molecule(s) associated with \ce{CuSO4.5H2O} is:

Identify a molecule which does not exist.

Which of the following set of molecules will have zero dipole moment?

\ce{BF3} is planar and an electron-deficient compound. The hybridization and number of electrons around the central atom, respectively, are:

Match List-I with List-II. List-I: (a) \ce{PCl5}, (b) \ce{SF6}, (c) \ce{BrF5}, (d) \ce{BF3} List-II: (i) Square pyramidal, (ii) Trigonal planar, (iii) Octahedral, (iv) Trigonal bipyramidal

The correct sequence of bond enthalpy of the C-X bond is:

Statement I: Acid strength increases in the order \ce{HF} < \ce{HCl} < \ce{HBr} < \ce{HI}. Statement II: As the size of the elements \ce{F}, \ce{Cl}, \ce{Br}, \ce{I} increases down the group, the bond strength of \ce{HF}, \ce{HBr} and \ce{HI} decreases and so the acid strength increases. In the light of the above statements, choose the correct answer from the options given below:

Which of the following molecules is non-polar in nature?

Identify the incorrect statement related to \ce{PCl5} from the following:

Amongst the following, which one will have maximum 'lone pair–lone pair' electron repulsion?

The correct order of dipole moments for molecules \ce{NH3}, \ce{H2S}, \ce{CH4} and \ce{HF}, is

Which one of the following statements is incorrect related to Molecular Orbital Theory?

Amongst the following, the total number of species NOT having eight electrons around the central atom in its outermost shell is: \ce{NH3}, \ce{AlCl3}, \ce{BeCl2}, \ce{CCl4}, \ce{PCl5}

The number of $\sigma$ bonds, $\pi$ bonds and lone pairs of electrons in pyridine (\ce{C5H5N}), respectively, are:

The correct order of energies of the molecular orbitals of the \ce{N2} molecule is:

Identify the correct answer.

Match List-I with List-II. List-I (Molecule): A. ethane; B. ethene; C. carbon molecule, \ce{C2}; D. ethyne List-II (Number and types of bond/s between the two carbon atoms): I. one $\sigma$-bond and two $\pi$-bonds; II. two $\pi$-bonds; III. one $\sigma$-bond; IV. one $\sigma$-bond and one $\pi$-bond Choose the correct answer from the options given below:

Match List-I with List-II. List-I (Compound): A. \ce{NH3}; B. \ce{BrF5}; C. \ce{XeF4}; D. \ce{SF6} List-II (Shape/geometry): I. Trigonal pyramidal; II. Square planar; III. Octahedral; IV. Square pyramidal Choose the correct answer from the options given below:

Intramolecular hydrogen bonding is present in which of the following compounds? (Structures (A), (B) and (D) are shown in the figure; (C) is \ce{HF}.)

Match List-I with List-II. List-I: A. \ce{XeO3}; B. \ce{XeF2}; C. \ce{XeOF4}; D. \ce{XeF6} List-II: I. $sp^3d$; linear; II. $sp^3$; pyramidal; III. $sp^3d^3$; distorted octahedral; IV. $sp^3d^2$; square pyramidal Choose the correct answer from the options given below:

Identify the correct orders against the property mentioned: A. \ce{H2O} > \ce{NH3} > \ce{CHCl3} — dipole moment B. \ce{XeF4} > \ce{XeO3} > \ce{XeF2} — number of lone pairs on central atom C. \ce{O-H} > \ce{C-H} > \ce{N-O} — bond length D. \ce{N2} > \ce{O2} > \ce{H2} — bond enthalpy Choose the answer from the options given below:

Match the species in List-I with their geometry in List-II. List-I: A. $\ce{PCl5}$, B. $\ce{BrF5}$, C. $\ce{BF4-}$, D. $\ce{[Ni(CN)4]^{2-}}$. List-II: I. Tetrahedral, II. Square planar, III. Trigonal bipyramidal, IV. Square pyramidal.

The correct statement is:

Identify the correct statement about \ce{ClF3} from the following options:

For the ozone (\ce{O3}) Lewis structure shown in the figure — a central O atom (1) doubly bonded to one terminal O atom (2) and singly bonded to the other terminal O atom (3) — the correct formal charges on the oxygen atoms numbered 2, 1 and 3 respectively are:

The highest occupied molecular orbital for $\ce{Ne2}$ is: