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MHT-CET Chemical Bonding and Molecular Structure — practice questions — page 2

Explore 100 free Chemical Bonding and Molecular Structure questions in MHT-CET Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Chemical Bonding and Molecular Structure questions and exercises with answers

Showing questions 31–60 of 100.

Why does a stable He2 molecule not exist?Read the answer and worked solution →Which homonuclear diatomic molecule does MO theory predict cannot exist?Read the answer and worked solution →In the C2 molecule, what makes up the double bond?Read the answer and worked solution →O2 has 10 bonding and 6 antibonding electrons. What is its bond order?Read the answer and worked solution →How many unpaired electrons does an O2 molecule have?Read the answer and worked solution →Hydrogen bonding is strongest when hydrogen is bonded to which atoms?Read the answer and worked solution →Which common cation in ionic compounds is not derived from a metal?Read the answer and worked solution →The octet rule applies mainly to elements of which period?Read the answer and worked solution →Which is a known drawback of the octet theory of bonding?Read the answer and worked solution →Which molecule breaks the octet rule by having an odd number of electrons?Read the answer and worked solution →Which two chemists developed the VSEPR theory in 1957?Read the answer and worked solution →In VSEPR theory, valence electron pairs around an atomRead the answer and worked solution →How does VSEPR theory count a double bond on the central atom?Read the answer and worked solution →What is the steric number of a central atom?Read the answer and worked solution →Sulfur in SF4 has four ligands and one lone pair. What is its steric number?Read the answer and worked solution →Why is the H–O–H angle in water 104.5° and not 109.5°?Read the answer and worked solution →In VSEPR theory, which repulsion is the strongest?Read the answer and worked solution →NH3 has three bond pairs and one lone pair. Its electron pairs are arrangedRead the answer and worked solution →Iodine heptafluoride has a steric number of 7. Its base geometry isRead the answer and worked solution →XeF4 has six electron pairs, two being lone pairs. Its shape isRead the answer and worked solution →In octahedral hexaaquo complexes of V3+ to Zn2+, the d-electron lone pairs areRead the answer and worked solution →Why are the X–A–X angles in SOCl2 not all equal?Read the answer and worked solution →In the carbonate ion, each O–C–O angle isRead the answer and worked solution →Which alternative name is used for the VSEPR theory?Read the answer and worked solution →How many p orbitals mix with the 2s orbital in sp2 hybridisation?Read the answer and worked solution →After sp hybridisation of carbon, how many pure p orbitals remain?Read the answer and worked solution →In methane formation, an electron is promoted from carbon'sRead the answer and worked solution →Carbon's ground state electron configuration isRead the answer and worked solution →The octet rule is based on the chemical inertness of which elements?Read the answer and worked solution →Compounds like XeF2 weaken the octet idea that noble gases areRead the answer and worked solution →

Worked practice questions

Why does a stable He2 molecule not exist?

  1. It has two unpaired electrons
  2. Its bond order is one
  3. Its bond order is zero
  4. Helium has no 1s orbital
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Correct answer: C. Its bond order is zero

He2 would place two electrons in σ1s and two in σ*1s, giving a bond order of zero.

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Which homonuclear diatomic molecule does MO theory predict cannot exist?

  1. B₂
  2. Li₂
  3. Be₂
  4. C₂
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Correct answer: C. Be₂

Be2 has equal numbers of bonding and antibonding electrons, so its bond order is zero and it does not exist.

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In the C2 molecule, what makes up the double bond?

  1. Two pi bonds only
  2. Two separate sigma bonds
  3. One sigma and one pi bond
  4. One sigma bond only
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Correct answer: A. Two pi bonds only

The four bonding electrons of C2 occupy two pi molecular orbitals, so both components of its double bond are pi bonds.

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