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VocabElectron

ConfigurationOrbital

NotationElectron Dot Misc

Wavelength

The distance between peaks of a wave

Valence Electrons

Electrons in the outer shell involved in bonding

Principle Quantum Number

The shell or level that the electron is in

DAILY DOUBLE!!!

Represented by (l). Energy sublevel

Azimuthal

Before any second electron can be placed in a sub level, all the

orbitals of that sub level must contain at least one electron.

Hund’s Rule

What are the 4 metals that are

exceptions to the “rules”?

Cr, Cu, Ag, Au

Long hand e- configuration for:

Bromine

• 1s22s22p63s23p63d104s24p5

What is the “short hand” e- configuration

of:

W

[Xe]4f145d46s2

What element am I….

1s22s22p63s23p63d54s1

Chromium

What is the e- configuration of:

Ca2+

1s22s22p63s23p64s2

What 3 rules are followed for orbital

notation?

1. Aufbau2. Hunds3. Pauli Exclusion

Draw the “long hand” orbital notation for:

Fluorine

1s 2s 2p

F

“Short hand” orbital notation for:Arsenic -3

[Ar]3d 4s 4p

“Short Hand” orbital notation for: silver

Ag [Kr]

4d 5s

Daily Double!!!!!

__

1s 2s 2p

What rule does this break?

Hund’s(Bus)

No atom has more than _____ e-

8

. Cr .....

Correct or Not?

If not, give the correct e- dot

Incorrect

Cr.

(Cr is an exception, only 1 valence in 4s)

Draw the e- dot for Mg+1

Mg.

Draw the e- dot for:S2-

S........

Correct or Not?

If NOT, why??

:O:..

Must fill, NSEW

Draw a full Bohr model of: Chlorine

Write the “short hand” bohr model

for:Na

Na )2e- )8e- )1e-

Draw a picture showing how light is

produced

2 of Bohr’s contributions…..

1. He explained the atomic line spectra in terms of electron energies

2. He introduced the idea of quantized electron energy levels in the atom

Type # sublevels

Total # e Shape

s

p

d

f

Complete the Chart:

Type # sublevels

Total # e Shape

s 1 2 sphere

p 3 6 peanut

d 5 10 dumbbell

f 7 14 flower