Question 1

What is the maximum number of unpaired electrons that can be accommodated in a 5d subshell?

Accepted Answer

A 5d subshell can hold a maximum of 10 electrons, and since it has 5 orbitals, the maximum number of unpaired electrons it can accommodate is 5, with one electron in each orbital.

Question 2

What is the maximum number of electrons that can be accommodated in the subshell for which n = 3 and l = 2?

Accepted Answer

The maximum number of electrons in a subshell is given by the formula 2(2l + 1). For n = 3 and l = 2, this gives 2(2*2 + 1) = 2(5) = 10.

Question 3

Calculate the maximum number of electrons that can fit into the n = 4 shell of orbitals.

Accepted Answer

The maximum number of electrons in a shell is given by the formula 2n^2, where n is the principal quantum number of the shell. For n = 4, the calculation is 2(4)^2 = 2(16) = 32.

Question 4

The Pauli exclusion principle states that:

Accepted Answer

The Pauli exclusion principle asserts that no two electrons in an atom can have the same set of four quantum numbers (principal, azimuthal, magnetic, and spin), ensuring each electron in an atom has a unique quantum state.

Question 5

Which of the following quantum numbers can have a value that is not an integer?

Accepted Answer

The quantum number $m_s$ (spin quantum number) can have values that are not integers, specifically +1/2 or -1/2, indicating the orientation of the spin of the electron.

Question 6

Which of the following subshells is filled first when electrons are added to the atomic orbitals on a xenon atom?

Accepted Answer

The 5s subshell is filled before the 4d, 4f, 5p, and 5d subshells according to the Aufbau principle, which states that electrons fill orbitals in order of increasing energy levels.

Question 7

Which of the following subshells would be filled first when electrons are added to a gold atom?

Accepted Answer

According to the Aufbau principle, electrons fill orbitals starting from the lowest energy level to the highest. For gold (Au), the 6s subshell is filled before the 5d subshell, which is in turn filled before the 6p and 6d subshells. The 4f subshell is filled even before the 5d, but since we're discussing the order for gold specifically, the 6s subshell is the first relevant one to be filled in this context.

Question 8

Determine the group of the periodic table in which an element with the following electron configuration belongs: 1s² 2s² 2p⁶3s² 3p⁶ 4s² 3d¹⁰4p⁴

Accepted Answer

The electron configuration ends in 4p^4, indicating the element is in Group VIA (16), as it has 6 valence electrons in the p-block.

Question 9

Determine the period and group in the periodic chart that contains the element with the following electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰4p⁴

Accepted Answer

The electron configuration ends in 4p^4, indicating the element is in the 4th period and group VIA (or group 16 in modern IUPAC numbering), which corresponds to the element selenium.

Question 10

In what group of the periodic table would an element with the following electron configuration belong? 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹

Accepted Answer

The electron configuration ends in 4p¹, indicating the element is in Group IIIA (13), which contains elements with a p¹ electron configuration in their outermost shell.

Question 11

A single atom of element 109 has been synthesized. Predict the electronic configuration of this element. Which of the following elements would 109 most resemble?

Accepted Answer

Element 109 is Meitnerium (Mt), which is in the same group as Iridium (Ir) in the periodic table. Elements in the same group have similar electronic configurations and chemical properties.

Question 12

A single atom of element 114 was recently synthesized. Predict the electronic configuration of this element. Which of the following elements would 114 most resemble?

Accepted Answer

Element 114 is flerovium (Fl), which belongs to group 14 of the periodic table, the same group as lead (Pb). Elements in the same group have similar properties due to their similar valence electron configurations.

Question 13

Theoreticians predict that the element with atomic number 120 will be more stable than the elements recently discovered with atomic numbers between 103 and 109. Based on the order of filling of atomic orbitals, the chemistry of this element should most closely resemble the chemistry of which of the following?

Accepted Answer

Element 120 is expected to be in Group IIA, below radium (Ra), because elements in the same group have similar chemical properties due to their similar valence electron configurations.

Question 14

In period 6 of the periodic table, the series of elements which differ in the number of electrons contained in f orbitals

Accepted Answer

The series of elements that differ in the number of electrons contained in f orbitals in period 6 of the periodic table is the lanthanide series, which begins with Cerium (Ce) and ends with Lutetium (Lu).

Question 15

A possible set of quantum numbers for the last electron added to form a gallium atom (Z = 31) in its lowest energy state is:

Accepted Answer

The answer of A possible set of quantum numbers for...

Question 16

A possible set of quantum numbers for the highest energy electron in an As³⁺ ion is:

Accepted Answer

The answer of A possible set of quantum numbers for...

Question 17

The outermost or highest energy electron in element 105 could be characterized by which of the following sets of n, l, m_l and m_s quantum numbers?

Accepted Answer

The answer of The outermost or highest energy electron in...

Question 18

Which of the following describes a possible set of quantum numbers for the last electron added to form an aluminum atom when atomic orbitals are filled?

Accepted Answer

The answer of Which of the following describes a possible...

Question 19

What is the lowest energy electronic configuration of a fluorine atom?

Accepted Answer

The lowest energy electronic configuration of a fluorine atom, which has 9 electrons, is 1s² 2s² 2p⁵.

Question 20

What is the value of x in the following electron configuration for silicon? 1s² 2s² 2p⁶ 3s² 3p^x

Accepted Answer

Silicon has an atomic number of 14, meaning it has 14 electrons. The given configuration accounts for 10 electrons (1s² 2s² 2p⁶ 3s²), so 4 electrons remain for the 3p subshell, making x = 2.

Quiz 3: Structure of the Atom