15.The Rydberg constant for the Be3+ ion is 109731 cm–1. Calculate the ionization

energy of a ground-state Be3+ ion.

22.How many electrons can occupy the following subshells: (a) 2s, (b) 4d, (c) 6f,
(d) 6g, (e) 6h?

15. Just like the H formula, just add Z^2 to it

16. # electrons is 2 times the number of subshells; i.e., 1s so 2 electrons, 3p to 6 electrons, 5d so 10 electrons, etc.

what is the H formula?

is there a place I can look up list of subshells to # electrons

To calculate the ionization energy of a ground-state Be3+ ion, we can use the Rydberg constant formula:

Ionization energy = R(1/n_initial^2 - 1/n_final^2)

Where:
R = Rydberg constant (109731 cm–1)
n_initial = initial energy level (ground state)
n_final = final energy level (infinity)

For a Be3+ ion, the initial energy level is the ground state, which is when one electron is removed from the Be2+ ion. Since each Be2+ ion has 4 electrons, we have n_initial = 4.

The final energy level is infinity, as the electron is completely removed from the ion, so we have n_final = ∞.

Substituting the values into the formula:
Ionization energy = 109731 cm–1 * (1/4^2 - 1/∞^2)

Since 1/∞^2 is negligible, we can simplify the equation:

Ionization energy ≈ 109731 cm–1 * (1/16) = 6858.19 cm–1

Therefore, the ionization energy of a ground-state Be3+ ion is approximately 6858.19 cm–1.

Now, let's move on to the second question.

To determine the number of electrons that can occupy the given subshells, we need to know the maximum number of electrons allowed in each subshell.

(a) 2s subshell:
The 2s subshell can hold a maximum of 2 electrons.

(b) 4d subshell:
The 4d subshell can hold a maximum of 10 electrons.

(c) 6f subshell:
The 6f subshell can hold a maximum of 14 electrons.

(d) 6g subshell:
There is no 6g subshell in the electron configuration.

(e) 6h subshell:
There is no 6h subshell in the electron configuration.

So, to summarize:
(a) The 2s subshell can hold a maximum of 2 electrons.
(b) The 4d subshell can hold a maximum of 10 electrons.
(c) The 6f subshell can hold a maximum of 14 electrons.
(d) The 6g subshell does not exist.
(e) The 6h subshell does not exist.

15. To calculate the ionization energy of a ground-state Be3+ ion, we need to first understand what the ionization energy is. Ionization energy is the energy required to remove an electron from an atom or ion in its ground state.

In this case, the Be3+ ion has a charge of +3, which means it has lost 3 electrons compared to the neutral Be atom. The ionization energy can be calculated by using the Rydberg equation:

E = R_H * (1/n_final^2 - 1/n_initial^2)

Where:
E is the ionization energy,
R_H is the Rydberg constant,
n_final is the quantum number of the final energy level (in this case, it will be infinity since the electron is being completely removed),
n_initial is the quantum number of the initial energy level (in this case, it will be 1 since we are considering the ground state).

Plugging in the values:
R_H = 109731 cm–1 (given)
n_final = ∞
n_initial = 1

E = 109731 * (1/∞^2 - 1/1^2)

As n_final approaches infinity, the term 1/∞^2 becomes negligible, so we can ignore it:

E = 109731 * (0 - 1/1^2)

E = 109731 * (-1)

E ≈ -109,731 cm–1

Therefore, the ionization energy of the ground-state Be3+ ion is approximately -109,731 cm–1.

22. We need to determine the maximum number of electrons that can occupy each subshell mentioned:

(a) 2s: In the second energy level, the 2s subshell can hold a maximum of 2 electrons (since s subshells have a maximum of 2 electrons).

(b) 4d: In the fourth energy level, the 4d subshell can hold a maximum of 10 electrons (since d subshells have a maximum of 10 electrons).

(c) 6f: In the sixth energy level, the 6f subshell can hold a maximum of 14 electrons (since f subshells have a maximum of 14 electrons).

(d) 6g: There is no such subshell as 6g. The subshells are labeled s, p, d, f based on their specific orbital shapes.

(e) 6h: There is no such subshell as 6h. The labeling of subshells goes up to "g," and no further letters are assigned.

To summarize:
(a) 2s: 2 electrons
(b) 4d: 10 electrons
(c) 6f: 14 electrons
(d) 6g: Not applicable
(e) 6h: Not applicable