O2 has two unpaired electrons in its π* orbitals, making it paramagnetic.

O2 is paramagnetic due to the presence of two unpaired electrons in its molecular orbitals.

O2 is paramagnetic due to the presence of two unpaired electrons in its molecular orbitals.

N2 has a triple bond, with a bond order of 3 according to molecular orbital theory.

The 3s orbital has the highest principal quantum number (n=3), indicating it has the highest energy.

The combustion of gasoline releases a large amount of energy, resulting in a large enthalpy change.

The reaction N2(g) + 3H2(g) → 2NH3(g) results in a decrease in the number of gas molecules, leading to a negative change in entropy.

A liquid with high molecular weight and strong intermolecular forces will have a higher boiling point.

A liquid typically exhibits the highest density at room temperature, as it is not at the extremes of phase change.

The entropy of the system decreases when water freezes, as the molecules become more ordered in the solid state.

During a phase transition, such as melting or boiling, ΔG equals ΔH because the system is at equilibrium.

When a gas is compressed, the number of microstates decreases, leading to a decrease in entropy.

Viscosity generally decreases with increasing temperature, so a liquid would have the highest viscosity at low temperatures.

O2 has unpaired electrons in its molecular orbital configuration, making it paramagnetic.

Liquids generally exhibit the highest density at low temperatures.

In solids, particles are closely packed and have limited movement.

The freezing of water results in a decrease in the entropy of the system as it transitions from liquid to solid.

The Gibbs Free Energy of a system is at its minimum at equilibrium, indicating stability.

ΔG = 0 occurs at equilibrium, where the forward and reverse reactions occur at the same rate.

ΔG equals ΔH when the entropy change (ΔS) is zero, indicating no change in disorder.

ΔG is zero at equilibrium, indicating no net change in the concentrations of reactants and products.

In solids, molecules are closely packed and have the least freedom of movement.

Plasma has the highest kinetic energy as the particles are highly energized and ionized.

In an endothermic reaction, the change in enthalpy is equal to the heat absorbed at constant pressure.

Expanding gives 3x - 3 = 2x + 8. Rearranging gives x = 11.

Dividing both sides by 3 gives x - 2 = 4, thus x = 6.

Subtracting 3x from both sides gives 2x + 2 = 10, then subtracting 2 gives 2x = 8, leading to x = 4.

The equation factors to (x - 3)(x + 3) = 0, giving solutions x = 3 and x = -3.

Subtracting 8 from both sides gives 4y = 16, then dividing by 4 gives y = 4.

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