Noble gases behave most ideally because they have minimal intermolecular forces and occupy a larger volume relative to their number of moles.

Tetrahedral geometry corresponds to sp3 hybridization, where one s and three p orbitals mix to form four equivalent sp3 hybrid orbitals.

As the positive charge increases, the ionic radius decreases; Si4+ has the smallest radius.

At equilibrium, the rates of the forward and reverse reactions are equal, but the concentrations of reactants and products do not have to be equal.

Real gases exhibit intermolecular forces, which affect their behavior, especially at high pressures and low temperatures.

Cathodic protection is a technique that prevents corrosion by making the metal surface the cathode of an electrochemical cell.

Electrolysis is commonly used for water splitting to produce hydrogen and oxygen gases.

The correct expression for Gibbs free energy change is ΔG = ΔH - TΔS, where T is the temperature in Kelvin.

An alkaline battery is a type of primary battery that cannot be recharged.

All of the above factors—temperature, pressure, and concentration—affect the rate of an electrochemical reaction.

Corrosion prevention techniques, such as cathodic protection, are practical applications of electrochemistry.

Enthalpy calculations are crucial in designing refrigeration systems to ensure efficient heat transfer.

The ideal gas law can be used to calculate the pressure in a tire by relating volume, temperature, and the number of moles of gas.

Enthalpy is measured in energy units such as Joules, Kilojoules, or Calories, but not in pressure units like Atmospheres.

H2O exhibits hydrogen bonding due to the presence of highly electronegative oxygen atoms bonded to hydrogen.

CO2 has a linear geometry due to its two double bonds and no lone pairs on the central atom, resulting in a bond angle of 180 degrees.

O2 has a nonpolar covalent bond because it consists of two identical oxygen atoms sharing electrons equally.

BF3 has three bonding pairs and no lone pairs, resulting in a trigonal planar geometry.

H2O has a bent shape and significant electronegativity difference between H and O, resulting in a higher dipole moment compared to CO2, CH4, and NH3.

CO2 is linear and symmetrical, leading to cancellation of dipole moments, making it nonpolar.

The d orbital can hold a maximum of 10 electrons (5 orbitals, each can hold 2 electrons).

Dissolving ammonium nitrate in water absorbs heat from the surroundings, making it an endothermic process.

The melting of ice is an endothermic process, which absorbs heat and results in a positive enthalpy change (ΔH > 0).

Reduction occurs at the cathode, where electrons are gained.

Corrosion is a spontaneous redox reaction where metals oxidize, often leading to deterioration.

Electrochemical cells convert chemical energy into electrical energy during spontaneous reactions.

Electrolysis involves the decomposition of a compound through the application of electrical energy.

Ionic bonds result from the transfer of electrons from one atom to another, typically between metals and nonmetals.

Reaction rates can change with time as reactants are consumed and products are formed, affecting the concentration of reactants.

Resonance structures differ only in the arrangement of electrons, while the positions of the nuclei remain the same, contributing to the overall hybrid structure.