Untitled lesson

Xenon's electron configuration

[Xe]6s25d1

sublevel d

La = [Xe] 6s25d1

Lanthanum electronic configuration =
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1

Noble Gas Configuration – La:

5th energy level

1stelectron

Find 5d1 on the periodic table

[Ar]4s23d104p2

Core Electrons – go up one energy level and

over to the noble gas

Example – germanium

X X

X

X

X

X

X

X

X

X

X

X

X

X

Ar

You try one!

sodium

How about this one?

cadmium

Then, fill in the configuration for the level

where the element is located

[Ar] 4s2

Noble Gas Configuration

Element

[Ar] 4s2 3d3

[Rn] 7s2 5f14 6d4

[He] 2s2 2p5

[Kr] 5s2 4d9

[Kr] 5s2 4d10 5p5

[Kr] 5s2 4d10 5p6

Ca

V

Sg

F

Ag

I

Xe

Fe

[Ar] 4s23d6

O
8

16.00

Electron Configuration
1s22s22p4

8p+

8n0
2e- 6e-

Noble Gas Configuration
[He]2s22p4

Valence electrons are electrons
in the outer energy level.
ONLY s & p orbitals are valence
electrons!

Oxygen has 6
valence electrons.

Cl
17

35.45

Electron Configuration
1s22s22p63s23p5

Noble Gas Configuration
[Ne]3s23p5

Valence electrons are electrons
in the outer energy level.
ONLY s & p orbitals are valence
electrons!

Chlorine has 7
valence electrons.

17p+

18n0 2e- 8e- 7e-

5d

4f

The outer energy level will
only have s & p orbitals.

Follow energy level 6. (32 e-) You see that
sublevels s & p are the only sublevels in the

outer energy level. (8 e-)

6s

6p

Atoms tend to gain, lose, or

share electrons until they have

eight valence electrons.

ONLY s & p orbitals are valence electrons!

In this way, atoms fill the valence (outer)
energy level which gives the atom the
stability of the noble gases.

Atoms gain or lose electrons to become more stable.
This is referred to as Isoelectronic with the Noble Gases.

1+

2+

3+

3- 2- 1-

0
+/-
4

Isoelectronic two atoms

with the same # of

electrons.

Atoms gain or lose electrons to become more stable.
This is referred to as Isoelectronic with the Noble Gases.

1+

2+

3+

3- 2- 1-

0
+/-
4

P
P3-: [Ne]3s23p6
P: [Ne]3s23p3

5 valence e-

8 valence e-

(isoelectronic w/ argon)

Ar = 18e- (8 valence)
P3- = 18e-(8 valence)
Not the same
element!How do we know?

Different # of p+!

Atoms gain or lose electrons to become more stable.
This is referred to as Isoelectronic with the Noble Gases.

Write the noble gas
configuration for the

oxygen ion.

1+

2+

3+

3- 2- 1-

0
+/-
4

Mg

Mg2+: [He]2s2 2p6

Write the noble gas
configuration for the

magnesium ion.

O2-:[He]2s2 2p6
O

Identify these ions.

[Ar] 4s23d104p6, 2- charge
[Kr] 5s24d105p6, 1+ charge

34 Se2-

55Cs+

Se

Cs

In 1944, American Scientist, Glenn Seaborg,
suggested that the actinide series should be placed
below the periodic table along with the lanthanide
series. Our modern Periodic Table took form.

Periodic Table with lanthanide and
actinide elements included in the

main table.

[Xe] 6s25d14f1

[Kr] 5s24d105p4

[Rn] 7s25f146d107p4

[Rn] 7s26d15f2

[Rn] 7s26d15f7

[Xe] 6s24f145d7

[Rn] 7s25f146d6

Ce

T
e

Lv

Pa

Cm

Ir

Hs

Cn

[Rn] 7s25f146d10