Question

1. how many f orbitals can there be in an energy level?
2. how many energy levels are partially or fully occupied in a neutral atom of calcium?
3. why do the fourth and fifth series of elements contain 18 elements, rather than 8 as do the second and third series?
4. which sublevels of the 3rd energy level are filled (a) in the element argon (b) in the element krypton?
5. why does it take more energy to remove an electron from al+ than from al?
6. what does the term principal quantum number refer to?
7. what is meant by the electron configuration of an atom?
8. what is the maximum number of electrons that can be present in an atom having three principal energy levels?
9. which of the following notations shows the electron - configuration of a neutral atom in an excited state? name the element and explain how you know it is excited:

(a) 1s² 2s²2p¹ (b) 1s² 2s²2p³ 3s¹ (c) 1s² 2s²2p⁶ 3s² 3p¹

1. isoelectronic species have similar electron configurations. which of these are isoelectronic?

(a) li⁺, h⁻, he (b) ca²⁺, ne, s²⁻

1. for the following elements list the electron configuration. if these is no charge listed, assume it is neutral.

a. oxygen b. cesium c. krypton d. titanium
e. scandium f. nitrogen g. chlorine h. fluorine¹⁻
i. arsenic j. francium k. selenium³⁻ l. copper¹⁺
m. potassium²⁻ n. antimony²⁺ o. thorium¹⁻ p. mercury²⁺

1. for the following elements list the shorthand electron configuration

a. boron b. cadmium c. phosphorus d. neon
e. radon f. iodine g. strontium h. chromium³⁺
j. nickel k. iron l. astatine m. molybdenum²⁻
n. rubidium³⁻ o. bromine¹⁺ p. xenon q. europium³⁺

1. for the following electron configurations choose possible elements or ions they may represent

a. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁴
b. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁵
c. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁶
d. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s¹
e. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁶ 5s²4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s² 5f¹⁴ 6d⁸
f. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁶ 5s²4d¹⁰ 5p⁶ 6s² 4f¹⁰
g. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁶ 5s²4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁴
h. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d⁵
i. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰ 4p⁶ 5s²4d¹⁰ 5p²
j. kr 5s² 4d¹⁰ 5p³
k. kr 5s² 4d¹⁰ 5p⁶
l. ar 4s¹
m. xe 6s² 4f¹⁰
n. xe 6s² 4f¹⁴ 5d⁷
o. ne 3s² 3p¹

Explanation:

Step1: Recall orbital - related rules

The number of f orbitals in an energy level is always 7, regardless of the energy - level number. This is because the angular momentum quantum number ($l$) for f orbitals is 3, and the magnetic quantum number ($m_l$) ranges from -$l$ to +$l$, giving $2l + 1=2\times3 + 1 = 7$ possible values for the orientation of the f orbitals.

Answer:

7