Question

1. The ni = 2 to nf = 6 transition in the Bohr hydrogen atom corresponds to the a)_______ of a photon with a wavelength of b)_______ nm.

Is this transition of energy state absorption of photon or emission of photon?

2. The lowest orbital energy is reached when the number of electrons with the same spin is maximized. This statement describes ________________________.

3. (a) Predict the number of subshells in the fourth shell, that is, for n = 4

(b) Give the label for each of these subshells .

(c) How many orbitals are in each of these subshells? Write each orbital number (ml) for each subshells.

4. [Ne]3s23p3 is the electron configuration of a(n) ________ atom .

5. All of the alkaline metals have a valence shell electron configuration ___________.

6. At maximum, an d-subshell can hold ________ electrons.

7. The complete electron configuration of sulfur, element 16, is _________________.

8. The angular momentum quantum number for the outermost electrons in a manganese atom in the ground state is ________.

9. The electron configuration of the valence electrons of an atom in its ground state is ns2np3. This atom is a group ________ element.

Answer 1

1. The n_i = 2 to n_f = 6 transition in the Bohr hydrogen atom corresponds to the a) absorption of a photon with a wavelength of b) 410.2 nm.

Is this transition of energy state absorption of photon or emission of photon? Absorption of a photon (n_f > n_i)

2. The lowest orbital energy is reached when the number of electrons with the same spin is maximized. This statement describes Hund' s rule.

3. (a) Predict the number of subshells in the fourth shell, that is, for n = 4: The number of subshells corresponds to the possible number of l: l can take the values integer numbers between 0 and (n-1) () = 0, 1, 2, 3: 4 subshells

(b) Give the label for each of these subshells: 4s (l=0), 4p (l=1), 4d ((l=2), and 4f (l=3).

(c) How many orbitals are in each of these subshells? Write each orbital number (ml) for each subshells.

4s: 1 orbital: l=0 and m_l =0

4 p: 3 orbitals: l=1, m_l = -1, 0, 1

4d: 5 orbitals: l=2, m_l = -2, -1, 0, 1, 2

4f: 7 orbitals: l=3, m_l = -3, -2, -1, 0, 1, 2  

4. [Ne]3s23p3 is the electron configuration of a(n) Phosphorus (Z = 10+2+3 = 15) atom .

5. All of the alkaline metals have a valence shell electron configuration ns¹.

6. At maximum, an d-subshell can hold 10 (5 orbitals, each 2 electron: 5x2 =10) electrons.

7. The complete electron configuration of sulfur, element 16, is: In ground state ₁₆S: 1s²2s²2p⁶3s²3p⁴ or [Ne]3s²3p⁴.

8. The angular momentum quantum number for the outermost electrons in a manganese atom in the ground state is l =2 (3d)

9. The electron configuration of the valence electrons of an atom in its ground state is ns²np³. This atom is a group of nitrogen (5 A or 15) element.