Home › NEET & JEE Chemistry MCQs › Chemical Bonding and Molecular Structure
NEET & JEE · Chemistry · Class 11

Chemical Bonding and Molecular Structure — NEET & JEE Chemistry MCQs

30 questions written by hand against the NCERT chapter. Every wrong option is explained, not just the right one.

30questions
10/14/6easy / medium / hard
₹0no login
Take the Chemical Bonding and Molecular Structure test →
Free · your all-India rank after you finish

Sample questions from this chapter

What do the dots in a Lewis symbol for an isolated atom represent?
  1. Valence-shell electrons ✓
  2. All electrons in the atom
  3. Only unpaired electrons
  4. Protons in the nucleus
Answer: A. A Lewis symbol displays the atom's valence electrons around its element symbol. Those electrons determine common bonding and valence; protected core electrons are not drawn.
Why not B: Inner electrons belong to the kernel and are omitted from a Lewis symbol.
Why not C: Paired valence electrons are also shown as dots, so the symbol is not restricted to unpaired electrons.
Why not D: Lewis dots track electrons involved in bonding, not nuclear particles.
In one canonical Lewis structure of O3, what formal charge is assigned to the central oxygen?
  1. -1
  2. 0
  3. +1 ✓
  4. +2
Answer: C. For central O, formal charge = 6 − 2 nonbonding electrons − 3 assigned bonding electrons = +1. The terminal single-bonded oxygen balances it with −1.
Why not A: The singly bonded terminal oxygen, not the central atom, carries −1 in that contributor.
Why not B: The double-bonded terminal oxygen has formal charge zero.
Why not D: Counting both bonds as fully owned by the central atom rather than half-shared produces an excessive charge.
What feature of the molecular-orbital configuration explains oxygen's paramagnetism?
  1. Two unpaired electrons occupy separate degenerate π*2p orbitals ✓
  2. A lone pair remains on each oxygen atom in localised orbitals
  3. The σ2p bonding orbital contains only one electron
  4. Both π2p bonding orbitals are half-filled
Answer: A. After filling the bonding orbitals, O2 places its last two electrons singly in degenerate π*2p orbitals by Hund's rule. Those two unpaired electrons make O2 paramagnetic.
Why not B: Lewis lone pairs are paired and cannot explain attraction to a magnetic field.
Why not C: The σ2p bonding MO is filled in O2 under the standard ordering.
Why not D: The bonding π orbitals are filled; the unpaired electrons occupy antibonding π* orbitals.

These are 3 of the 30 questions in the test. Take the full chapter test →

Read the chapter first

Every NCERT question in this chapter is solved, free: NCERT solutions — Chemical Bonding and Molecular Structure →

Other NEET Chemistry chapters

Some Basic Concepts of ChemistryStructure of AtomClassification of Elements and Periodicity in PropertiesThermodynamicsEquilibriumRedox Reactions

All 19 chapters →

Questions

How many NEET and JEE questions are there on Chemical Bonding and Molecular Structure?

This chapter test has 30 questions — 10 easy, 14 medium and 6 hard — all written against the NCERT Class 11 chapter.

Is this NEET and JEE Chemistry chapter test free?

Yes. Every chapter test is free with no login, and you get your all-India rank on every one. Nothing on the site is on sale right now.

Do the questions explain the wrong options?

Yes — every distractor carries its own explanation naming the specific misconception that makes a student pick it. That is the part most question banks skip, and it is the part that changes your next attempt.