The correct answer is (4) A-IV, B-III, C-II, D-I.
Let's discuss each pair in detail:
A. Mg in solid state: IV. Electronic conductor
Magnesium (Mg) in its solid state behaves as an electronic conductor. In metals like Mg, the electrons are delocalized and can move freely throughout the crystal lattice. This gives rise to metallic conductivity, where electrons can carry an electric current.
B. \(MgCl_2\) in molten state: III. Electrolytic conductor
In the molten state, magnesium chloride (\(MgCl_2\)) undergoes a process called electrolysis. In this state, the ionic bonds between magnesium and chloride ions are broken due to the high temperature. The resulting molten salt contains free ions, allowing it to conduct electricity. It acts as an electrolytic conductor because the ions in the molten state can migrate and carry an electric current.
C. Silicon with phosphorus: II. n-type Semiconductor
Silicon (Si) is a semiconductor, and when it is doped with phosphorus (P), which has one more electron in its outer shell than silicon, it becomes an n-type semiconductor. The extra electron from the phosphorus atom, which is a donor impurity, provides mobile charge carriers (electrons) in the silicon crystal lattice. These electrons contribute to the electrical conductivity of the semiconductor.
D. Germanium with boron: I. p-type Semiconductor
Germanium (Ge) is another semiconductor, and when it is doped with boron (B), which has one less electron in its outer shell than germanium, it becomes a p-type semiconductor. The boron atoms act as acceptor impurities, creating "holes" in the crystal lattice. These holes represent missing electrons and contribute to the electrical conductivity of the semiconductor.
So, the correct match is: 4. A-IV, B-III, C-II, D-I |
