Question

electron configurations worksheet
write the complete ground - state electron configurations and orbital notations for the following:

of e element (atom) e configuration orbital notation/ diagrams

1. lithium
2. oxygen
3. calcium
4. nitrogen
5. potassium
6. chlorine
7. hydrogen
8. copper
9. neon
10. phosphorus

write the abbreviated ground - state electron configurations for the following:

of electrons element

1. helium
2. nitrogen
3. chlorine
4. iron
5. zinc
6. barium
7. bromine
8. magnesium
9. fluorine
10. aluminum

Explanation:

Step1: Recall electron - filling rules

Use the Aufbau principle, Pauli - exclusion principle, and Hund's rule to write electron configurations.

Step2: Determine atomic numbers

Find the atomic number of each element, which is equal to the number of electrons in a neutral atom.

Step3: Write complete electron configurations

Lithium (Li, atomic number = 3)

$1s^{2}2s^{1}$

Oxygen (O, atomic number = 8)

$1s^{2}2s^{2}2p^{4}$

Calcium (Ca, atomic number = 20)

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}$

Nitrogen (N, atomic number = 7)

$1s^{2}2s^{2}2p^{3}$

Potassium (K, atomic number = 19)

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}$

Chlorine (Cl, atomic number = 17)

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}$

Hydrogen (H, atomic number = 1)

$1s^{1}$

Copper (Cu, atomic number = 29)

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{10}$ (due to stability of half - filled and fully - filled subshells)

Neon (Ne, atomic number = 10)

$1s^{2}2s^{2}2p^{6}$

Phosphorus (P, atomic number = 15)

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}$

Step4: Write abbreviated electron configurations

Helium (He, atomic number = 2)

$[He]$

Nitrogen (N, atomic number = 7)

$[He]2s^{2}2p^{3}$

Chlorine (Cl, atomic number = 17)

$[Ne]3s^{2}3p^{5}$

Iron (Fe, atomic number = 26)

$[Ar]4s^{2}3d^{6}$

Zinc (Zn, atomic number = 30)

$[Ar]4s^{2}3d^{10}$

Barium (Ba, atomic number = 56)

$[Xe]6s^{2}$

Bromine (Br, atomic number = 35)

$[Ar]4s^{2}3d^{10}4p^{5}$

Magnesium (Mg, atomic number = 12)

$[Ne]3s^{2}$

Fluorine (F, atomic number = 9)

$[He]2s^{2}2p^{5}$

Aluminum (Al, atomic number = 13)

$[Ne]3s^{2}3p^{1}$

Answer:

Complete electron configurations:

1. Lithium: $1s^{2}2s^{1}$
2. Oxygen: $1s^{2}2s^{2}2p^{4}$
3. Calcium: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}$
4. Nitrogen: $1s^{2}2s^{2}2p^{3}$
5. Potassium: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}$
6. Chlorine: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}$
7. Hydrogen: $1s^{1}$
8. Copper: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{10}$
9. Neon: $1s^{2}2s^{2}2p^{6}$
10. Phosphorus: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}$

Abbreviated electron configurations:

1. Helium: $[He]$
2. Nitrogen: $[He]2s^{2}2p^{3}$
3. Chlorine: $[Ne]3s^{2}3p^{5}$
4. Iron: $[Ar]4s^{2}3d^{6}$
5. Zinc: $[Ar]4s^{2}3d^{10}$
6. Barium: $[Xe]6s^{2}$
7. Bromine: $[Ar]4s^{2}3d^{10}4p^{5}$
8. Magnesium: $[Ne]3s^{2}$
9. Fluorine: $[He]2s^{2}2p^{5}$
10. Aluminum: $[Ne]3s^{2}3p^{1}$