The bond angle in H2O is approximately 104.5 degrees due to the two lone pairs on oxygen.

The bond angle in water (H2O) is approximately 104.5 degrees.

CO has a bond order of 3, calculated as (10 bonding - 3 antibonding)/2.

O2- has a bond order of 1, calculated as (10 bonding electrons - 7 antibonding electrons)/2 = 1.

B2 has a bond order of 1, calculated as (2 bonding - 0 antibonding)/2.

B2 has a bond order of 1, calculated from its molecular orbital configuration.

CO has a bond order of 3, calculated as (10 bonding electrons - 2 antibonding electrons)/2 = 3.

He2 has a bond order of 0, as it has no net bonding electrons.

N2 has a bond order of 3, calculated as (10 bonding - 0 antibonding)/2 = 3.

O2 has 12 total electrons, leading to a bond order of (10 bonding - 6 antibonding)/2 = 1.

Brewster's angle can be calculated using the formula tan(θ_B) = n, where n is the refractive index. For n = 1.5, θ_B = arctan(1.5) ≈ 53 degrees.

Brewster's angle can be calculated using the formula tan(θ_B) = n, where n is the refractive index. For n = 1.5, θ_B = arctan(1.5) ≈ 53 degrees.

Brewster's angle can be calculated using the formula tan(θ_B) = n2/n1, which gives approximately 53 degrees.

Brewster's angle θ_B can be calculated using θ_B = arctan(n2/n1) = arctan(1.5) ≈ 56.31 degrees.

Brewster's angle is the angle of incidence at which light is reflected with maximum polarization.

The bulk modulus measures a material's resistance to uniform compression, indicating how much it resists volume change.

C = ε₀ * ε_r * A / d = (8.85 × 10^-12 F/m) * 5 * (0.01 m²) / (0.001 m) = 4.425 × 10^-10 F.

Capacitance C = ε₀ * A / d = (8.85 × 10^-12 F/m) * (0.1 m²) / (0.01 m) = 8.85 × 10^-10 F.

The capacitance C of a parallel plate capacitor is given by the formula C = ε₀ * A / d, where ε₀ is the permittivity of free space.

The capacitance C of a parallel plate capacitor is given by the formula C = ε₀A/d, where ε₀ is the permittivity of free space.

In an endothermic reaction, heat is absorbed from the surroundings, resulting in a positive change in enthalpy.

In an exothermic reaction, heat is released, resulting in a negative change in enthalpy.

In an isothermal process, the temperature remains constant, and for an ideal gas, the change in enthalpy is zero.

The change in entropy for an isothermal and reversible expansion of an ideal gas is given by ΔS = nR ln(V2/V1). For 1 mole, n = 1, hence ΔS = R ln(V2/V1).

The change in entropy for an isothermal expansion of an ideal gas is given by ΔS = nR ln(V2/V1). For 1 mole, it simplifies to ΔS = R ln(V2/V1).

In an isochoric process, the change in internal energy is equal to the heat added to the system, ΔU = Q.

In an isochoric process, the change in internal energy is equal to the heat added to the system, ΔU = Q.

In an isochoric process, the volume remains constant, and the change in internal energy is equal to the heat added to the system.

In an isochoric process, the volume remains constant, and any heat added to the system increases the internal energy of the gas.

The oxidation state of carbon changes from -4 in CH4 to +4 in CO2.