Which of the following bonds is present in diamond?
A. Hydrogen bond
B. Ionic
C. Metallic
D. Covalent network
Answer: Option D
Solution (By JKSSB Mock Tests)
Diamond has a three-dimensional network of strong covalent bonds between carbon atoms (sp³ hybridization). This giant covalent structure gives diamond its extreme hardness, high melting point, and electrical insulating property. Graphite also has covalent bonds within layers but conducts due to delocalized electrons. Ionic bonds are in NaCl, metallic bonds in metals, hydrogen bonds in water.
Explanation:
The acidic behavior of HCl is due to the presence of H⁺ (or H₃O⁺) ions, which are generated only when it dissolves in water. Without moisture, HCl doesn't dissociate to produce H⁺, so it doesn't change the color of dry litmus. Both statements are correct and R explains A.
Explanation:
The mass of an atom is almost entirely concentrated in its tiny central nucleus. This is because the nucleus contains protons and neutrons, which are much heavier than the extranuclear electrons. Since electrons have negligible mass, R correctly explains why the mass is localized in the nucleus.
Explanation:
N₂ has a triple bond (N≡N), consisting of one sigma and two pi bonds. This is the strongest type of covalent bond, giving N₂ high stability and low reactivity. Bond order is 3. The molecule is diatomic and nonpolar.
No comments yet. Be the first to start the discussion!