Chemical Bonding and Structure

When atoms form a chemical bond, the system moves to a lower energy state to achieve stability, meaning energy is released and the total potential energy decreases.

Phosphorus in PCl3 has 5 valence electrons. It forms 3 bonds with chlorine atoms, leaving one lone pair on the phosphorus atom.

A water molecule has two hydrogen atoms (each can act as a donor) and two lone pairs on the oxygen atom (each can act as an acceptor), allowing for a maximum of 4 hydrogen bonds.

Metallic bonding allows layers of metal ions to slide over each other without breaking the bonds, which is why metals are malleable and ductile.

Xe has 8 valence electrons. In XeF2, Xe forms 2 bonds, leaving 6 electrons (3 lone pairs). In XeO3, Xe forms 6 bonds, leaving 1 lone pair. In XeF4, Xe forms 4 bonds, leaving 2 lone pairs. In XeF6, Xe forms 6 bonds, leaving 1 lone pair.

Calcium carbide (CaC2) contains the carbide ion C2(2-). The bond between the two carbon atoms is a triple bond, consisting of one sigma bond and two pi bonds.

According to Fajan's rules, covalent character increases with the charge density of the cation. Al(3+) has the highest charge among the choices, leading to the highest polarization of the chloride ion.

Paramagnetic species have unpaired electrons. NO has 15 valence electrons (an odd number), meaning it must have at least one unpaired electron.

As established previously, the C2(2-) ion contains a triple bond between the carbon atoms, which consists of one sigma bond and two pi bonds.

The sp3d2 hybridization involves six hybrid orbitals arranged in an octahedral geometry to minimize repulsion. This configuration is characteristic of molecules like SF6.