Question

name
write the electron configuration for each element below. draw arrows within the orbital boxes to represent electron pairs
1.potassium (k) :

1. carbon (c) :
2. titanium (ti):

4.argon (ar) :

1. sulfur (s) :

Explanation:

1. Potassium (K)

Step1: Determine atomic number

Potassium has atomic number 19, so 19 electrons.

Step2: Apply Aufbau principle

Fill orbitals in order \(1s, 2s, 2p, 3s, 3p, 4s, 3d, \dots\).
\(1s\) holds 2: \(1s^2\); \(2s\) holds 2: \(2s^2\); \(2p\) holds 6: \(2p^6\); \(3s\) holds 2: \(3s^2\); \(3p\) holds 6: \(3p^6\); remaining \(19 - (2 + 2 + 6 + 2 + 6) = 1\) electron in \(4s\): \(4s^1\).
So electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^1\).

2. Carbon (C)

Step1: Atomic number

Carbon has atomic number 6, 6 electrons.

Step2: Aufbau principle

\(1s\) (2): \(1s^2\); \(2s\) (2): \(2s^2\); remaining \(6 - (2 + 2) = 2\) electrons in \(2p\): \(2p^2\).
Electron configuration: \(1s^2 2s^2 2p^2\).

3. Titanium (Ti)

Step1: Atomic number

Titanium has atomic number 22, 22 electrons.

Step2: Aufbau principle

\(1s^2\) (2); \(2s^2\) (2); \(2p^6\) (6); \(3s^2\) (2); \(3p^6\) (6); \(4s^2\) (2); remaining \(22 - (2 + 2 + 6 + 2 + 6 + 2) = 2\) electrons in \(3d\): \(3d^2\).
Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\) (or \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 4s^2\) – note \(4s\) fills before \(3d\) but is often written with \(3d\) after for transition metals, though Aufbau order is \(4s\) first).

4. Argon (Ar)

Answer:

s:

1. Potassium (K): \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^1\)
2. Carbon (C): \(1s^2 2s^2 2p^2\)
3. Titanium (Ti): \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\) (or \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 4s^2\))
4. Argon (Ar): \(1s^2 2s^2 2p^6 3s^2 3p^6\)
5. Sulfur (S): \(1s^2 2s^2 2p^6 3s^2 3p^4\)