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Question

You have three solids. One is a metal; one is an ionic compound; one is a molecular/covalent compound. You test all three solid samples to identify their bonding.
Sample Appearance Melting Point $(^{\circ} C)$ Conductivity
A Shiny $962$ conductive
B Crystalline $801$ conductive in aqueous solution
C Powdery $186$ not conductive
Based on this data, identify the type bonds present in each sample.

A

Sample A is a metal.
Sample B is a salt.
Sample C is a molecule.

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B

Sample A is a molecule.
Sample B is a metal.
Sample C is a salt.

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C

Sample A is a salt.
Sample B is a metal.
Sample C is a molecule.

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D

Sample A is a molecule.
Sample B is a salt.
Sample C is a metal.

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Solution

The correct option is D Sample A is a metal.
Sample B is a salt.
Sample C is a molecule.
Ans : (A) Sample $A$ is metal
(B) Sample $B$ is a salt
(C) Sample $C$ is a molecule
Note : - (1) We know that metal possers shiny properties and it is a good conductor of electricity.
(2) Ionic salt is dissolved in water make an electrically conductive solution. Ionic compound is formed from strong electrostatic interaction between ions which result in a higher melting point.
(3) Molecule do not have free $e^{⊖}$ to conduct the Electricity.

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