ELECTRON CONFIGURATIONS & QUANTUM

NUMBERS

STANDARDS

SC3. Students will use the modern atomic

theory to explain the characteristics of atoms.

b. Use the orbital configuration of neutral

atoms to explain its effect on the atom’s

chemical properties.

f. Relate light emission and the movement of

electrons to element identification.

TO KNOW FOR TEST:

Know colors of light (ROYGBV).

Red-high wavelength; low frequency (energy)

Violet- low wavelength; high frequency (energy)

Quantum numbers (POMS).

Sublevels (s,p,d,f)-shapes

Relationship between energy level, sublevel, slots, electrons.

Electron configurations, orbital notations, electron dot diagrams.

ELECTRONS AND THEIR ENERGIES

Bohr model was a one dimensional model

describing the structure of the atom.

Atoms are ___ _____________.

Quantum numbers describe the _________of

electrons in atoms.

Exact ____________of electrons can not be

determined. Which energy level an electron is

on is only a highly __________ or likely location.

FACTS ABOUT ELECTRONS

1. They can only move certain _________from

the nucleus.

2. They can only move at certain _______.

3. They give off (_______) energy when moving

to a lower level and gain energy (_______) when

moving to a higher level.

4, They cannot jump down to a level with a

_____ _______of electrons.

PHOTON- A BUNDLE OR PACKET OF ENERGY IN

THE FORM OF ELECTROMAGNETIC RADIATION.

When an atom gains photons, it becomes excited and the electrons move to a _______ energy level.

When it loses photons, it gives off photons, e- move to _______ level.

Atoms become _______ ( and gain ________) by heating them or passing ___________ through them. When they lose these photons, the electrons give off ______, depending on amount of _________ given off (related to ___________ and ________).

The color depends on distance the electron

travels, or___________.

When electron falls back to lower energy level,

it releases energy (________) in the form of

________.

Elements release a ________ ________ when

heated in a _______ that is determined by their

electron configurations.

Ex. Na- yellow-orange

Ne- red

QUANTUM NUMBERS- DESCRIBE THE ENERGY

AND ARRANGEMENT OF ELECTRONS

1. (P) --(n)--

2. (O) -(l)--

3. (M)--

4. (S) --(+1/2, -1/2)--

PRINCIPAL QUANTUM NUMBER

Represented by n.

Describes the

Identifies the particular_______ _____. Same

as the

4 is farther away than 3, etc.

A ________, ___________ number.

ORBITAL QUANTUM NUMBER

Identifies the ___________(s,p,d,f).

Each sublevel (orbital) has its own shape.

s-

p-

d-

f- ?

ORBITAL (SHAPE) IS DEPENDENT ON PRINCIPAL

QUANTUM NUMBER

1st level has __ possible shape

2nd level has __ possible shapes

3rd level has __ possible shapes

4th level and up has __ possible shapes

n tells us what energy level AND how many

possible________ or __________.

MAGNETIC QUANTUM NUMBER

Tells how many positions on the sublevels; the _______________in space. (x, y, or z axis)

Sublevel # positions # electrons

s

p

d

f

Ex. The 2nd energy level can have s and p sublevels for a total of ___possible positions. S = 1 p = 3 = 4

The total number of possible positions in an

energy level = n2.

SPIN QUANTUM NUMBER

Electrons can spin or __________ or

____________.

Only ___electrons can occupy each ________,

one spins clockwise, the other spins

counterclockwise.

EXAMPLES

The first energy level can only have “s” sublevel which has only one position.

represents that these electrons have

opposite spins.

max. of 2 e- on each level.

The second energy level has s and p sublevels.

The maximum number of electrons in a certain energy level =_____.

No 2 electrons can have the same set

of________________ _______________.

No 2 electrons can have exactly the same

amount of __________if they come from the

same atom.

n – energy level

(principal)

sublevel (Shape) Total slots n2 Total electrons

2(n2)

1

2

3

4

LIGHT EQUATIONS

Speed = wavelength (nm) X frequency (Hz)

Frequency = 1/wavelength