Rubidium (Rb) has an atomic number of 37, and its outermost electron is in the 5th shell (n=5).

The outermost electron in sodium (Na) is in the 3s orbital, which corresponds to a principal quantum number of n=3.

Potassium has an electron configuration of [Ar] 4s1, so the principal quantum number for the outermost electron is 4.

Chlorine has an atomic number of 17, and its outermost electrons are in the n=3 shell.

Potassium (K) has an atomic number of 19, and its outermost electrons are in the n=4 level.

Sodium has an electron configuration of 1s2 2s2 2p6 3s1, so the principal quantum number is 3.

Potassium has an atomic number of 19, and its outermost electrons are in the 4th shell (n=4).

Chlorine has an atomic number of 17, and its outermost electrons are in the 3rd shell (n=3).

Quantum mechanics in chemistry is based on the principles that particles exhibit wave-like properties and that energy is quantized.

The salt bridge maintains charge balance by allowing ions to flow between the two half-cells.

The salt bridge maintains charge balance by allowing ions to flow between the two half-cells.

For a first-order reaction, k = 0.693 / t1/2. Thus, k = 0.693 / 10 min = 0.0693 min^-1.

The rate law is determined by the order of the reaction with respect to each reactant. For first order in A and second order in B, the rate law is Rate = k[A]^1[B]^2.

The rate law is determined by the stoichiometry of the rate-determining step. For second order in A and first order in B, the rate law is Rate = k[A]^2[B].

The rate law is determined by the orders of the reactants. For second order in A and first order in B, the rate law is Rate = k[A]^2[B].

For a second-order reaction with respect to A, the rate law is Rate = k[A]^2.

Atomic radius and ionization energy are inversely proportional; as atomic radius increases, ionization energy decreases.

Metallic character increases with atomic size, as larger atoms can lose electrons more easily.

At constant pressure, the change in enthalpy (ΔH) is related to the change in internal energy (ΔU) and the pressure-volume work done (PΔV) by the equation ΔH = ΔU + PΔV.

The enthalpy change (ΔH) for a reaction can be calculated as the sum of the bond dissociation energies of the reactants minus that of the products.

At constant pressure, the change in enthalpy (ΔH) is equal to the heat exchanged (Q).

The change in enthalpy (ΔH) is directly related to the heat capacity at constant pressure (Cp) and the change in temperature (ΔT) as ΔH = Cp * ΔT.

Spontaneity is determined by both enthalpy and entropy changes, as described by the Gibbs free energy equation.

A negative Gibbs free energy change (G < 0) indicates that a reaction is spontaneous.

The relationship is given by ΔG = -nFE, where n is the number of moles of electrons and F is Faraday's constant.

The relationship is given by the equation G = -nFE, where G is Gibbs free energy, n is moles of electrons, F is Faraday's constant, and E is cell potential.

The relationship is given by ΔG = -nFE, where n is the number of moles of electrons and F is Faraday's constant.

According to Gay-Lussac's Law, pressure is directly proportional to temperature when volume is held constant.

Gay-Lussac's Law states that the pressure of a gas is directly proportional to its absolute temperature when volume is held constant.

Boyle's Law states that for a given mass of gas at constant temperature, the pressure of the gas is inversely proportional to its volume (P1V1 = P2V2).