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
10. which isoelectronic species have similar electron configurations. which of these are isoelectronic? (a) li⁺, h⁻, he (b) ca²⁺, ne, s²⁻
11. for the following elements list the electron configuration. if there is no charge listed, assume it is neutral. a. oxygen b. cesium c. krypton d. titanium e. scandium f. nitrogen g. chlorine h. fluorine i. arsenic j. francium k. selenium³⁻ l. copper¹⁺ m. potassium²⁻ n. antimony²⁺ o. thorium¹⁺ p. mercury²⁺
12. 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⁺
13. for the following electron configurations choose possible elements or ions they may represent. a. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁴ b. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁵ c. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁶ d. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁶ 5s² 4d¹⁰5p⁶ 6s² 4f¹⁴5d¹⁰6p⁶ 7s¹ e. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁶ 5s²4d¹⁰5p⁶ 6s² 4f¹⁴5d¹⁰6p⁶ 7s² 5f¹⁴6d⁸ f. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁶ 5s²4d¹⁰5p⁶ 6s² 4f¹⁰ g. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁶ 5s²4d¹⁰5p⁶ 6s² 4f¹⁴5d¹⁰6p⁴ h. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d⁵ i. 1s² 2s²2p⁶ 3s²3p⁶ 4s² 3d¹⁰4p⁶ 5s²4d¹⁰5p² j. kr 5s² 4d¹⁰5p³ k. kr 5s² 4d¹⁰5p⁶ l. ar 4s¹ m. xe 6s² 4f¹⁰ n. xe 6s² 4f¹⁴5d⁷ o. ne 3s² 3p¹

Explanation:

36. How many f orbitals can there be in an energy level?

Step1: Recall orbital - type rule

The number of orbitals for a given angular - momentum quantum number $l$ is given by $2l + 1$. For f orbitals, $l=3$.

Step2: Calculate the number of f orbitals

Substitute $l = 3$ into the formula $2l+1$. So, $2\times3 + 1=7$.

Step1: Recall electron - capacity formula for each shell

The maximum number of electrons in a principal energy level $n$ is given by $2n^{2}$.

Step2: Calculate electrons for $n = 1$

For $n = 1$, the number of electrons $N_1=2\times1^{2}=2$.

Step3: Calculate electrons for $n = 2$

For $n = 2$, the number of electrons $N_2=2\times2^{2}=8$.

Step4: Calculate electrons for $n = 3$

For $n = 3$, the number of electrons $N_3=2\times3^{2}=18$.

Step5: Sum up the electrons

The total number of electrons $N=N_1 + N_2+N_3=2 + 8+18=28$.

Step1: Analyze option (a)

For $1s^{2}2s^{2}2p^{1}$, it is the ground - state electron configuration of boron (B) with atomic number 5. The electrons are filled in the lowest - energy orbitals first as per the Aufbau principle.

Step2: Analyze option (b)

For $1s^{2}2s^{2}2p^{3}3s^{1}$, the ground - state configuration of nitrogen (N) with atomic number 7 should be $1s^{2}2s^{2}2p^{3}$. Here, an electron has been promoted from the 2p orbital to the 3s orbital, which is a higher - energy orbital. So, it is an excited - state electron configuration of nitrogen.

Step3: Analyze option (c)

For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}$, it is the ground - state electron configuration of aluminum (Al) with atomic number 13. The electrons are filled in the lowest - energy orbitals first as per the Aufbau principle.

Answer:

7

43. What is the maximum number of electrons that can be present in an atom having three principal energy levels?