Electronic Configurations Of Elements And The Periodic Table

Correct answer: Modern periodic table

Explanation:
In the Modern Periodic Table, elements are arranged in the increasing order of their atomic numbers, which is the number of protons in an atom. This arrangement solves the limitations of earlier periodic laws and explains the periodicity of chemical properties more accurately.

- Dobereiner's Law of Triads: Elements were grouped into triads based on similar properties, not strictly by atomic number.
- Newland's Law of Octaves: Elements were arranged by increasing atomic mass, not atomic number.
- Mendeleev's Periodic Table: Also based on atomic mass, not atomic number.

Therefore, only the Modern Periodic Table follows the correct ascending order of atomic numbers.

Correct answer: All of the above

Explanation:
The electronic configuration of an element is determined using the following three principles:

1. Aufbau Principle:
Electrons fill the lowest energy orbitals first before moving to higher ones.

2. Hund's Rule:
Electrons occupy all degenerate orbitals singly first, with parallel spins, before pairing begins.

3. Pauli's Exclusion Principle:
No two electrons in an atom can have the same set of four quantum numbers; i.e., an orbital can hold a maximum of 2 electrons with opposite spins.

Hence, the correct answer is: All of the above.

Correct answer: 6

Explanation:
A p-orbital consists of three degenerate orbitals (i.e., ). Each orbital can hold a maximum of 2 electrons with opposite spins.

So, the maximum number of electrons in all three p-orbitals is:
Hence, the correct answer is: 6.

Correct answer: 1 sigma bond and bonds

Explanation:
In a nitrogen molecule ( ), the two nitrogen atoms are connected by a triple bond. A triple bond consists of:
- 1 sigma (σ) bond: formed by the head-on overlap of orbitals
- 2 pi (π) bonds: formed by the side-by-side overlap of p orbitals

Therefore, the triple bond in contains 1 sigma bond and 2 pi bonds.

The element "S" refers to sulfur. The atomic number of sulfur is 16, meaning it has 16 electrons. The electron configuration for sulfur is: This corresponds to the first option, which shows sulfur's correct electron configuration.

The correct option is (A):

First, let's determine the total number of electrons in the given electronic configuration:

Total electrons = 2 + 2 + 6 + 2 + 6 = 18 electrons

(1) : Phosphorus (P) has an atomic number of 15, so it has 15 electrons. gains 3 electrons, resulting in 15 + 3 = 18 electrons.

(2) : Chlorine (Cl) has an atomic number of 17, so it has 17 electrons. gains 1 electron, resulting in 17 + 1 = 18 electrons.

(3) : Sulfur (S) has an atomic number of 16, so it has 16 electrons. gains 2 electrons, resulting in 16 + 2 = 18 electrons. Because the configuration given is ,

The configuration of the options, is none of them.

The O²⁻ ion is formed when a neutral oxygen atom gains two additional electrons. Oxygen, with an atomic number of 8, has 8 protons in its nucleus and normally possesses 8 electrons in its neutral state. The electronic configuration of a neutral oxygen atom is: $ 1s^2 2s^2 2p^6 $ This configuration reflects the fact that the O²⁻ ion has the same electron arrangement as the noble gas neon (Ne), which also has 10 electrons.