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NEET CHEMISTRYOrganic Chemistry – Some Basic Principles and Techniques Medium

Question

Which one of the following bonds produces a solid that reflects light in the visible region and whose electrical conductivity decreases with temperature and has a high melting point?

A

Metallic bonding

B

Van der Waals' bonding

C

Ionic bonding

D

Covalent bonding

Step-by-Step Solution

  1. Metallic Luster (Reflects Light): Metals have a unique luster and reflect light due to the presence of free, mobile electrons (sea of electrons) that interact with incident light.
  2. Electrical Conductivity vs Temperature: Metals are excellent conductors due to these free electrons. However, metallic (electronic) conductance decreases with an increase in temperature [Class 12 Chemistry, Unit 2, Sec 2.4.1]. This occurs because increasing temperature increases the thermal vibration of the positive metal kernels, which hinders the flow of electrons.
  3. High Melting Point: Strong metallic bonding (electrostatic attraction between positive kernels and the electron sea) generally results in high melting points [Class 12 Chemistry, Unit 4, Sec 4.3.1].
  4. Comparison: Ionic solids are insulators in the solid state. Covalent network solids (like diamond) have high melting points but are insulators. Molecular solids (Van der Waals) have low melting points.

Exam Context & Concepts Covered

This question aligns with the NEET CHEMISTRY syllabus, specifically targeting concepts from Organic Chemistry – Some Basic Principles and Techniques . Mastering this topic is crucial for scoring well in the upcoming medical entrance examinations. Solving conceptually related problems will help you understand the nuances of these concepts and improve your problem-solving speed.

CHEMISTRYOrganic Chemistry – Some Basic Principles and Techniques followingproducesreflectsvisibleregion

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Which one of the following pairs is isostructural (i.e., having the same shape and hybridization)?

A.$\text{BCl}_3$ and $\text{BrCl}_3$
B.$\text{NH}_3$ and $\text{NO}_3^-$
C.$\text{NF}_3$ and $\text{BF}_3$
D.$\text{BF}_4^-$ and $\text{NH}_4^+$
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Among the following, isoelectronic species are:

A.$CO_{2}, NO_{2}$
B.$NO_{2}^{-}, CO_{2}$
C.$CN^{-}, CO$
D.$SO_{2}, CO_{2}$
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Which one of the following pairs of species have the same bond order?

A.$\text{CO}$, $\text{NO}$
B.$\text{O}_2^-$, $\text{CN}^-$
C.$\text{CN}^-$, $\text{NO}^+$
D.$\text{N}^+$, $\text{CN}^+$
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In a regular octahedral molecule, $MX_{6}$, the number of $X–M–X$ bonds at 180º is:

A.Two
B.Six
C.Four
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Which of the following pairs of ions are isoelectronic and isostructural?

A.CO₃²⁻, SO₃²⁻
B.ClO₃⁻, CO₃²⁻
C.SO₃²⁻, NO₃⁻
D.ClO₃⁻, SO₃²⁻
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Which orbital does the additional electron occupy when $O_{2}$ is converted to the $O_{2}^{-}$ ion?

A.$\pi$ orbital
B.$\sigma^{*}$ orbital
C.$\sigma$ orbital
D.$\pi^{*}$ orbital
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A species that does not exhibit paramagnetism is:

A.$N_{2}^{+}$
B.$O_{2}^{-}$
C.$CO$
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The total number of $\pi$-bond electrons in the following structure is:

A.4
B.8
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