Question 1

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of potassium, K.

Accepted Answer

D

Question 2

Select the correct electron configuration for Te (Z = 52).

Accepted Answer

Tellurium (Te) has an atomic number of 52, and its electron configuration is [Kr]5s²4d¹⁰5p⁴.

Question 3

Select the correct set of quantum numbers (n, l, m_l, m_s) for the first electron removed in the formation of a cation for strontium, Sr.

Accepted Answer

Strontium (Sr) has an electron configuration ending in 5s^2. The first electron removed during cation formation comes from the outermost shell, which is the 5s orbital. The quantum numbers for an electron in the 5s orbital are n=5 (principal quantum number), l=0 (azimuthal quantum number for an s orbital), m_l=0 (magnetic quantum number, which is 0 for s orbitals), and m_s can be either +½ or −½ (spin quantum number). Option E correctly represents these quantum numbers for the first electron removed.

Question 4

Which of the following electron configurations is impossible?

Accepted Answer

The answer of Which of the following electron configurations is...

Question 5

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸ refers to the ground state of:

Accepted Answer

The electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸ corresponds to Nickel (Ni), which has an atomic number of 28.

Question 6

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of tin, Sn.

Accepted Answer

The answer of Select the correct set of quantum numbers...

Question 7

Which one of the following statements about atomic structure and quantum numbers is incorrect?

Accepted Answer

The quantum number m_l (spin quantum number) can only have values of +1/2 or -1/2, regardless of the value of n or l. Therefore, there is no limit on the largest possible value of m_l for a given value of n.

Question 8

Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

Accepted Answer

A larger nuclear charge increases the attractive force between the nucleus and electrons, which lowers energy. However, when more electrons are added to an orbital, they repel each other, increasing energy. This is due to electron-electron interactions, and is known as electron-electron repulsion. Therefore, more electrons in an orbital increases energy.

Question 9

Which of the following sublevels is filled last?

Accepted Answer

The 4d sublevel is filled last according to the Aufbau principle, which states that electrons fill orbitals starting from the lowest energy level to the highest. The order is 4s, 3d, 4p, 5s, and then 4d.

Question 10

In the ground state of an atom of silver (Ag), how many electrons will there be with the quantum number l = 1? (The n, m_l and m_s quantum numbers may have any appropriate values.)

Accepted Answer

The answer of In the ground state of an atom...

Question 11

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

Accepted Answer

The answer of An atom of element number 33 (As)...

Question 12

In a single atom, what is the maximum number of electrons that can have quantum number n = 4?

Accepted Answer

The maximum number of electrons in a shell is given by 2n^2. For n = 4, the maximum number is 2(4)^2 = 32.

Question 13

The effective nuclear charge for an atom is less than the actual nuclear charge due to

Accepted Answer

Shielding occurs when inner electrons partially block the attraction between the positively charged nucleus and the outer electrons, reducing the overall attraction and therefore lowering the effective nuclear charge.

Question 14

In many-electron atoms, which quantum numbers specify the energy of an electron?

Accepted Answer

In many-electron atoms, the energy of an electron is primarily determined by its principal quantum number (n) and its azimuthal quantum number (l). The other quantum numbers (m_s) are related to the electron's angular momentum and spin, but do not have a direct impact on the electron's energy level. Therefore, the correct choice is A (n and l).

Question 15

Select the correct electron configuration for Cu (Z = 29).

Accepted Answer

Copper (Cu) has an electron configuration of [Ar]4s¹3d¹⁰ due to the stability provided by a fully filled d subshell.

Question 16

Which one of the following statements about orbital energies is incorrect?

Accepted Answer

The energy of a given orbital actually decreases as nuclear charge (Z) increases due to increased attraction between the nucleus and electrons. This is the opposite of what is stated in statement E.

Question 17

"Each electron in an atom must have its own unique set of quantum numbers" is a statement of

Accepted Answer

The statement "Each electron in an atom must have its own unique set of quantum numbers" is a restatement of the Pauli exclusion principle, which states that no two electrons in the same atom can have the same set of all four quantum numbers. This principle is a fundamental concept in quantum mechanics and explains many important properties of atoms and molecules, such as the fact that certain atoms and molecules are stable while others are highly reactive.

Question 18

d¹⁰np³?

Accepted Answer

The code consists of sequences of letters and numbers, with each letter indicating a different action to be taken (S = step, U = turn up, P = turn down) and each number indicating the number of steps to be taken. Counting the number of steps taken in each sequence gives the following pattern: 1+1+0+1+1+0+1+3+1+1+0 = 10. Therefore, the answer is D) 10. However, there is an alternative interpretation of the code where the number following each action letter indicates the number of times that action is taken before moving on to the next letter. Using this interpretation, we get: (S1U1P1)(10 times)S1U1P1S1S1(0 times)S1U1P1(3 times)S1S1P1(0 times). Counting the number of steps taken in this case gives: 3+3+3+3+3+3+3+3+3+3 = 30. But since the question specifically asks for the number of steps taken, not the total number of actions, we should only count the number of steps taken in each sequence, which gives: 1+1+0+1+1+0+1+3+1+1+0 = 10. Therefore, the best choice is C) 5, which is half of the total number of steps taken in the code.

Question 19

Select the correct electron configuration for sulfur (Z = 16).

Accepted Answer

Sulfur has 16 electrons. The correct electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁴, which adds up to 16 electrons.

Question 20

"Electrons added to atomic orbitals of the same energy will remain unpaired with parallel spins until the subshell is more than half-filled" is a statement of

Accepted Answer

Hund's rule states that when electrons are added to atomic orbitals of the same energy, they will remain unpaired with parallel spins until the subshell is more than half-filled. The other answer choices are not relevant to this statement.

Quiz 8: Electron Configuration and Chemical Periodicity

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of potassium, K.

Select the correct electron configuration for Te (Z = 52) .

Select the correct set of quantum numbers (n, l, m_l, m_s) for the first electron removed in the formation of a cation for strontium, Sr.

Which of the following electron configurations is impossible?

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸ refers to the ground state of:

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of tin, Sn.

Which one of the following statements about atomic structure and quantum numbers is incorrect?

Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

Which of the following sublevels is filled last?

In the ground state of an atom of silver (Ag) , how many electrons will there be with the quantum number l = 1? (The n, m_l and m_s quantum numbers may have any appropriate values.)

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

In a single atom, what is the maximum number of electrons that can have quantum number n = 4?

The effective nuclear charge for an atom is less than the actual nuclear charge due to

In many-electron atoms, which quantum numbers specify the energy of an electron?

Select the correct electron configuration for Cu (Z = 29) .

Which one of the following statements about orbital energies is incorrect?

"Each electron in an atom must have its own unique set of quantum numbers" is a statement of

d¹⁰np³?

Select the correct electron configuration for sulfur (Z = 16) .

"Electrons added to atomic orbitals of the same energy will remain unpaired with parallel spins until the subshell is more than half-filled" is a statement of

Quiz 8: Electron Configuration and Chemical Periodicity

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of potassium, K.

Select the correct electron configuration for Te (Z = 52) .

Select the correct set of quantum numbers (n, l, ml, ms) for the first electron removed in the formation of a cation for strontium, Sr.

Which of the following electron configurations is impossible?

The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of:

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of tin, Sn.

Which one of the following statements about atomic structure and quantum numbers is incorrect?

Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

Which of the following sublevels is filled last?

In the ground state of an atom of silver (Ag) , how many electrons will there be with the quantum number l = 1? (The n, ml and ms quantum numbers may have any appropriate values.)

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

In a single atom, what is the maximum number of electrons that can have quantum number n = 4?

The effective nuclear charge for an atom is less than the actual nuclear charge due to

In many-electron atoms, which quantum numbers specify the energy of an electron?

Select the correct electron configuration for Cu (Z = 29) .

Which one of the following statements about orbital energies is incorrect?

"Each electron in an atom must have its own unique set of quantum numbers" is a statement of

d10np3?

Select the correct electron configuration for sulfur (Z = 16) .

"Electrons added to atomic orbitals of the same energy will remain unpaired with parallel spins until the subshell is more than half-filled" is a statement of

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of potassium, K.

Select the correct set of quantum numbers (n, l, m_l, m_s) for the first electron removed in the formation of a cation for strontium, Sr.

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸ refers to the ground state of:

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of tin, Sn.

In the ground state of an atom of silver (Ag) , how many electrons will there be with the quantum number l = 1? (The n, m_l and m_s quantum numbers may have any appropriate values.)

d¹⁰np³?