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Indian Navy SSR (Sailor) Chemical Bonding and Molecular Structure — practice questions

Explore 29 free Chemical Bonding and Molecular Structure questions in Indian Navy SSR (Sailor) 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 1–29 of 29.

Arrange the bond angles of $\mathrm{H_2O}$, $\mathrm{NH_3}$ and $\mathrm{CH_4}$ in decreasing order.Read the answer and worked solution →The octet rule states atoms tend to:Read the answer and worked solution →Lattice energy of an ionic crystal depends on:Read the answer and worked solution →In benzene C₆H₆, each C is:Read the answer and worked solution →The shape of the methane (CH$_4$) molecule is:Read the answer and worked solution →Match each scientist to their contributionRead the answer and worked solution →Ionic or covalent?Read the answer and worked solution →Complete the driver of bond formationRead the answer and worked solution →Single, double and triple bondsRead the answer and worked solution →True or false: Lewis structuresRead the answer and worked solution →Complete the definition of resonanceRead the answer and worked solution →Tap every bond parameter the chapter namesRead the answer and worked solution →True or false: ionic solidsRead the answer and worked solution →Assertion and reasonRead the answer and worked solution →Two are true, one is notRead the answer and worked solution →Three of these are wrong. Find the one that holds.Read the answer and worked solution →Bonded pair or lone pair?Read the answer and worked solution →Flip and pair: term with meaningRead the answer and worked solution →Spot the one that does not belongRead the answer and worked solution →Order the reasoning: why resonance is neededRead the answer and worked solution →Reading the definitions backRead the answer and worked solution →True or false: what bond parameters affectRead the answer and worked solution →Bond parameters in useRead the answer and worked solution →Which parameter answers this?Read the answer and worked solution →True or false: resonanceRead the answer and worked solution →Order the steps: draw a Lewis structureRead the answer and worked solution →Spot the one that does not belongRead the answer and worked solution →Assertion and reason: structureRead the answer and worked solution →Flip and pair: parameter with what it measuresRead the answer and worked solution →

Worked practice questions

Arrange the bond angles of $\mathrm{H_2O}$, $\mathrm{NH_3}$ and $\mathrm{CH_4}$ in decreasing order.

  1. $\mathrm{CH_4} > \mathrm{H_2O} > \mathrm{NH_3}$
  2. $\mathrm{NH_3} > \mathrm{CH_4} > \mathrm{H_2O}$
  3. $\mathrm{H_2O} > \mathrm{NH_3} > \mathrm{CH_4}$
  4. $\mathrm{CH_4} > \mathrm{NH_3} > \mathrm{H_2O}$
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Correct answer: D. $\mathrm{CH_4} > \mathrm{NH_3} > \mathrm{H_2O}$

All three central atoms are $sp^3$ hybridised so the base bond angle is $109.5°$. Lone pairs compress that angle (the lone-pair-to-bond-pair repulsion is stronger than bond-pair-to-bond-pair). Approximate bond angles: - $\mathrm{CH_4}$ (0 lone pairs): $109.5°$ - $\mathrm{NH_3}$ (1 lone pair): $107°$ - $\mathrm{H_2O}$ (2 lone pairs): $104.5°$ More lone pairs means more compression, so the order is $\mathrm{CH_4} > \mathrm{NH_3} > \mathrm{H_2O}$.

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The octet rule states atoms tend to:

  1. Achieve 8 electrons in their outermost shell (valence)
  2. Lose all electrons
  3. Have only 1 electron
  4. Become radioactive
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Correct answer: A. Achieve 8 electrons in their outermost shell (valence)

Most atoms become chemically stable when their valence shell has 8 electrons (like noble gases). They achieve this by losing, gaining, or sharing electrons. Hydrogen/helium follow a 2-electron 'duet' rule.

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Lattice energy of an ionic crystal depends on:

  1. Charges of ions and inter-ionic distance
  2. Temperature only
  3. Number of moles
  4. Color of ions
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Correct answer: A. Charges of ions and inter-ionic distance

Lattice energy ∝ (q⁺ × q⁻)/r. Higher charges and smaller ions give more lattice energy (more stable crystal). E.g. MgO (both ions ±2) has much higher lattice energy than NaCl (both ions ±1).

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