Understanding Electron Configuration

The image shows the electron configuration of an atom. The configuration is written as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s² 5f¹⁴ 6d¹⁰ 7p⁶. To identify the element, we need to find its total number of electrons, which is its atomic number (Z).

Step-by-Step Solution:

Step 1: List all the orbitals and their electron counts.

1s² = 2 electrons
2s² = 2 electrons
2p⁶ = 6 electrons
3s² = 2 electrons
3p⁶ = 6 electrons
4s² = 2 electrons
3d¹⁰ = 10 electrons
4p⁶ = 6 electrons
5s² = 2 electrons
4d¹⁰ = 10 electrons
5p⁶ = 6 electrons
6s² = 2 electrons
4f¹⁴ = 14 electrons
5d¹⁰ = 10 electrons
6p⁶ = 6 electrons
7s² = 2 electrons
5f¹⁴ = 14 electrons
6d¹⁰ = 10 electrons
7p⁶ = 6 electrons

Step 2: Sum all the electrons to find the atomic number (Z).

Let's add them up:

$Z = 2 + 2 + 6 + 2 + 6 + 2 + 10 + 6 + 2 + 10 + 6 + 2 + 14 + 10 + 6 + 2 + 14 + 10 + 6$

Step 3: Calculate the total.

Grouping the numbers can make this easier:

s-orbitals: There are 7 s-orbitals (1s to 7s), each with 2 electrons: $7 \times 2 = 14$

p-orbitals: There are 6 p-orbitals (2p to 7p), each with 6 electrons: $6 \times 6 = 36$

d-orbitals: There are 4 d-orbitals (3d to 6d), each with 10 electrons: $4 \times 10 = 40$

f-orbitals: There are 2 f-orbitals (4f, 5f), each with 14 electrons: $2 \times 14 = 28$

Now, add these group totals:

$Z = 14 + 36 + 40 + 28 = 118$

Final Answer: The atomic number Z is 118. Therefore, the element is Oganesson (Og). Among the options provided (Z, R, S, E), the correct one is Z, which stands for atomic number.

Related Topics:

Electron Configuration: The distribution of electrons of an atom or molecule in atomic or molecular orbitals.
Aufbau Principle: Electrons occupy the lowest energy orbitals first.
Hund's Rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied.
Pauli Exclusion Principle: No two electrons can have the same set of four quantum numbers.
The Periodic Table: Elements are arranged in order of increasing atomic number.

Important Formulae & Theory:

Maximum Electrons in a Shell: The maximum number of electrons that can occupy a shell (principal quantum number n) is given by $2 n^{2}$ .

Orbital Types per Shell:

s subshell: 1 orbital, holds 2 electrons.
p subshell: 3 orbitals, hold 6 electrons.
d subshell: 5 orbitals, hold 10 electrons.
f subshell: 7 orbitals, hold 14 electrons.

Order of Filling: The order for filling orbitals is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p... This can be remembered using the Aufbau diagram or the n+l rule.