BeCl2 has two bonding pairs and no lone pairs, resulting in a linear shape.

CH4 has a tetrahedral shape due to sp3 hybridization of the carbon atom.

PCl5 has five bonding pairs and no lone pairs, resulting in a trigonal bipyramidal geometry.

C2H4 (ethylene) has a carbon-carbon double bond, and each carbon is sp2 hybridized.

O2+ has a bond order of 2.5, which is higher than O2 (2), O2- (1.5), and O2 2- (1).

In the given reaction, MnO4- is reduced to Mn^2+.

Colligative properties depend on the number of solute particles in a solution, not their identity.

In dynamic equilibrium, the rates of the forward and reverse reactions are equal, but the concentrations of reactants and products may not be equal.

Electrons have a negligible mass compared to protons and neutrons.

Enthalpy is an extensive property, meaning it depends on the amount of substance present.

Entropy is a measure of disorder in a system.

The equilibrium constant K is dependent on temperature; changing the temperature will change the value of K.

Ideal solutions obey Raoult's law at all concentrations, meaning their vapor pressures are proportional to the mole fractions.

Liquids are incompressible and have a fixed volume, but they do not have a definite shape.

In metallic bonding, electrons are delocalized, allowing for conductivity and malleability.

Molarity is defined as moles of solute per liter of solution, and it can change with temperature due to volume changes.

Molecular orbitals are indeed formed by the overlap of atomic orbitals.

Not all molecular orbitals are degenerate; some can have different energy levels.

Molecular orbitals are indeed formed by the overlap of atomic orbitals.

Colligative properties depend on the number of solute particles, not their type.

Strong acids completely dissociate in solution, producing a high concentration of H+ ions, which allows them to conduct electricity.

The Arrhenius equation relates temperature to the rate constant and includes the activation energy.

The boiling point is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure.

The common ion effect states that the solubility of a salt decreases in the presence of a common ion.

Electrons fill orbitals in order of increasing energy, and the 4s orbital is filled before the 3d orbital.

The equilibrium constant K is dependent on temperature; it changes if the temperature of the system changes.

In the quantum mechanical model, electrons are described by wave functions, which give the probability of finding an electron in a certain region.

The rate of reaction generally increases with increasing concentration of reactants.

Ksp is temperature dependent; it changes with temperature.

Viscosity generally decreases with an increase in temperature.