Explanation

• Silicon has atomic number 14, with the electronic configuration 1s² 2s² 2p⁶ 3s² 3p².
• When two electrons are removed from silicon, they are removed from the 3p subshell, producing Si²⁺ with the configuration 1s² 2s² 2p⁶ 3s².
• The outermost occupied orbital is then the 3s orbital, which is spherical in shape.

Last verified on 27-10-2026

Explanation

• Aluminium chloride (AlCl₃) is trigonal planar in its monomeric form, with aluminium at the centre and three chlorine atoms around it.
• The central aluminium atom is described as sp²-hybridized, forming three sigma bonds arranged at approximately 120°.
• Aluminium chloride can also form a dimer, Al₂Cl₆, under certain conditions.
• In the dimer, bridging chlorine atoms change the bonding arrangement.

Last verified on 27-10-2026

Explanation

• The azimuthal quantum number (l) identifies the subshell: l=0 for s, l=1 for p, l=2 for d, and l=3 for f.
• The number of orbitals in a subshell is calculated using 2l+1.
• For l=2, the number of orbitals is 2(2)+1=5.
• These five d orbitals are degenerate in an isolated atom, meaning they have the same energy.

Last verified on 27-10-2026

Explanation

• Acetic acid (CH₃COOH) is a weak acid that partially ionizes in water, producing hydrogen ions (H⁺) and acetate ions (CH₃COO⁻).
• Hydrogen sulphide (H₂S) is also a weak acid.
• Its presence does not directly add a common ion to the acetic acid ionization equilibrium.

Last verified on 27-10-2026

Explanation

• The degree of ionization is the fraction of electrolyte molecules that form ions in solution.
• Increasing concentration generally decreases the degree of ionization of a weak electrolyte because the equilibrium shifts toward the undissociated form.
• Dilution generally increases the degree of ionization of weak electrolytes.
• The effect of temperature depends on whether ionization is endothermic or exothermic.

Last verified on 27-10-2026

Explanation

• Ethanol (CH₃CH₂OH) is a primary alcohol that can be oxidized to ethanal (CH₃CHO).
• Ethanal reacts with iodine in the presence of an alkali to produce yellow iodoform (CHI₃) precipitate.

Last verified on 27-10-2026

Explanation

• The principal quantum number (n) indicates the main energy level or shell occupied by an electron.
• In hydrogen-like atoms, electron energy depends primarily on the principal quantum number.
• A higher value of n corresponds to a higher energy level.

Last verified on 27-10-2026

Explanation

• Paramagnetism mainly occurs due to the presence of unpaired electrons in atoms, ions, or molecules.
• Unpaired electrons have magnetic moments that can align with an external magnetic field, causing the substance to be attracted to the field.
• Substances with all electrons paired are generally diamagnetic, meaning they are weakly repelled by a magnetic field.

Last verified on 27-10-2026

Explanation

• A nitrogen atom has the electronic configuration 1s² 2s² 2p³.
• In the nitrogen molecule (N₂), the first bond is a sigma (σ) bond, formed by head-on overlap of p orbitals.
• The other two bonds are pi (π) bonds, formed by sideways or parallel overlap of p orbitals.
• Therefore, nitrogen has a triple bond consisting of one sigma bond and two pi bonds.

Last verified on 27-10-2026

Explanation

• Phosphorus (P), atomic number 15: Electronic configuration is [Ne] 3s² 3p³, with 3 unpaired electrons, one in each 3p orbital.

Additional information:

• Boron (B), atomic number 5: Electronic configuration is 1s² 2s² 2p¹, with 1 unpaired electron.
• Chlorine (Cl), atomic number 17: Electronic configuration is [Ne] 3s² 3p⁵, with 1 unpaired electron.

Last verified on 27-10-2026