Orbital Diagrams, Noble Gas (Abbreviated) Electron Configuration, Electron Configurations

Mg (Magnesium)

What element is represented by this orbital diagram?

S (Sulfur)

What element is represented by this orbital diagram?

O (Oxygen)

What element is represented by this orbital diagram?

N (Nitrogen)

What element is represented by this orbital diagram?

Si (Silicon)

What element is represented by this orbital diagram?

F (Fluorine)

What element is represented by this orbital diagram?

P (Phosphorus)

What element is represented by this orbital diagram?

V (Vanadium)

What element is represented by this orbital diagram?

Pauli Exclusion Principle

2 electrons in the same orbital must have opposite spins

Hund's Rule

Electrons don't pair up in orbitals of equal energy until they have to, and all electrons in singly occupied orbitals have the same spin.

orbital diagram for nitrogen

orbital diagram for fluorine

orbital diagram for carbon

orbital diagram for lithium

orbital diagram for sodium

Aufbau Principle

Electrons enter orbitals with the least amount of energy first

Aufbau Principle

Fill orbital diagrams from the bottom up

Hund's Rule

Put 1 electron in each connected box before you double them up

Pauli Exclusion Principle

If you have to put 2 arrows in a box, point 1 up and 1 down

₁H

1s¹

₂He

1s²

₃Li

[He]2s¹

₄Be

[He]2s²

₅B

[He]2s²2p¹

₆C

[He]2s²2p²

₇N

[He]2s²2p³

₈O

[He]2s²2p⁴

₉F

[He]2s²2p⁵

₁₀Ne

[He]2s²2p⁶

₁₁Na

[Ne]3s¹

₁₂Mg

[Ne]3s²

₁₃Al

[Ne]3s²3p¹

₁₄Si

[Ne]3s²3p²

₁₅P

[Ne]3s²3p³

₁₆S

[Ne]3s²3p⁴

₁₇Cl

[Ne]3s²3p⁵

₁₈Ar

[Ne]3s²3p⁶

₁₉K

[Ar]4s¹

₂₀Ca

[Ar]4s²

The electron configuration for hydrogen (H)

1s¹

The electron configuration for bromine (Br)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵

The electron configuration for aluminum (Al)

1s² 2s² 2p⁶ 3s² 3p¹

The electron configuration for silver (Ag)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d⁹

The electron configuration for Ne

1s² 2s² 2p⁶

The electron configuration for lithium cation (Li 1+)

1s²

The electron configuration for sulfur anion (S 2-)

1s² 2s² 2p⁶ 3s² 3p⁶

The electron configuration for calcium cation (Ca 2+)

1s² 2s² 2p⁶ 3s² 3p⁶

The electron configuration for bromine anion (Br 1-)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶

The electron configuration for nitrogen anion (N 3-)

1s² 2s² 2p⁶

How do elements determine what charge to become when they become ions?

Elements want to have the same electron configuration as noble gases.

This is because noble gases are the most stable elements.

They will lose or gain electrons (whichever is easiest) in order to have the same electron configuration as the CLOSEST noble gas.

Which noble gas does fluorine (F) want to be like?

What will it do to look like this noble gas?

What charge will it form?

Neon

Will gain 1 electron.

F = 1-

Which noble gas does potassium (K) want to be like?

What will it do to look like this noble gas?

What charge will it form?

Argon

Will lose one electron.

K = 1+

Which noble gas does aluminum (Al) want to be like?

What will it do to look like this noble gas?

What charge will it form?

Neon.

Will lose 3 electrons.

Al = 3+

Which noble gas does sulfur (S) want to be like?

What will it do to look like this noble gas?

What charge will it form?

Argon.

Will gain 2 electrons.

S = 2-

Which noble gas does astatine (At) want to be like?

What will it do to look like this noble gas?

What charge will it form?

Radon.

Will gain 1 electron.

At = 1-

Hydrogen

Lithium

Beryllium

Boron

Oxygen

Sodium

Magnesium

Aluminum

Silicon

Sulfur

Argon

Scandium

Chromium

Iron

Cobalt

Copper

Germanium

Selenium

Bromine

Krypton

Zirconium

Hund's Rule

Every orbital is singly occupied with one electron before its doubled

names of sublevels

s, p, d, f

1s sublevel

sphere shape

closest to the nucleus

least amount of energy

"p" sublevel shape

teardrop/ dumbell

how many electrons can each orbital hold?

2

how many orbitals are in an "s" sublevel?

1 orbital, so it can hold 2 electrons

how many orbitals are in a "p" sublevel?

3 orbitals, so it can hold 6 electrons

how many orbitals are in a "d" sublevel?

5 orbitals, so it can hold 10 electrons

how many orbitals are in a "f" sublevel?

7 orbitals, so it can hold 14 electrons

electron configuration notation

number= energy level

letter= sublevel

little number= number of electrons in the sublevel

the 4s sublevel comes BEFORE ___

the 3d sublevel

goes in order: 3s, 3p, 4s, 3d, 4p, 4d, 4f

The electron configuration for hydrogen (H)

1s¹

The electron configuration for bromine (Br)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵

The electron configuration for aluminum (Al)

1s² 2s² 2p⁶ 3s² 3p¹

The electron configuration for silver (Ag)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d⁹

The electron configuration for Ne

1s² 2s² 2p⁶

The electron configuration for lithium cation (Li 1+)

1s²

The electron configuration for sulfur anion (S 2-)

1s² 2s² 2p⁶ 3s² 3p⁶

The electron configuration for calcium cation (Ca 2+)

1s² 2s² 2p⁶ 3s² 3p⁶

The electron configuration for bromine anion (Br 1-)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶

The electron configuration for nitrogen anion (N 3-)

1s² 2s² 2p⁶

How do elements determine what charge to become when they become ions?

Elements want to have the same electron configuration as noble gases.

This is because noble gases are the most stable elements.

They will lose or gain electrons (whichever is easiest) in order to have the same electron configuration as the CLOSEST noble gas.

Which noble gas does fluorine (F) want to be like?

What will it do to look like this noble gas?

What charge will it form?

Neon

Will gain 1 electron.

F = 1-

Which noble gas does potassium (K) want to be like?

What will it do to look like this noble gas?

What charge will it form?

Argon

Will lose one electron.

K = 1+