Expanding the Theory of the Atom

I. Expanding the Theory of the Atom

A. Sublevels – divisions within an E level

B. Sublevels are designated as:

s,p,d, or f

s = lowest E, f = highest E

C. Energy levels &Their Sublevels

1. The 1st E level has 1 sublevel

1s

2. The 2nd E level has 2 sublevels

2s, 2p

3. The 3rd E level has 3 sublevels

3s, 3p, 3d

4. The 4th E level has 4 sublevels

4s, 4p, 4d, 4f

D. Distribution of electrons in sublevels

s= 2 e

p= 6e

d= 10e

f= 14 e

E. Heisenberg Uncertainty Principle-

It is impossible to measure accurately both the position & E of an electron at the same time

F. Orbital-

Space in which there is a high probability of finding an electron

**Can hold a maximum of 2 e

G. Electron configuration

Most stable arrangement of electrons in sublevels & orbitals

II. The periodic Table & Atomic Structure

A. Building electron configurations:

III. Orbitals- compartments in sublevels

A. Shapes

s orbital P orbitals

Shape of the d orbital

Orbitals cont.

B. Each orbital can hold a max of 2 e-

C. As you move down a family on the periodic table, orbitals become larger like nested boxes. See pg 251

D. Orbitals in E levels

1. The 1st E level

a. Has 2 e-

b. Has 1s sublevel

c. Has 1s orbital with 2 e- in it

2. The 2nd E level

2. The 2nd E level

a. Holds 8 e- total

b. Has 2s & 2p sublevels

c. The 2s sublevel holds 2 e-,

The 2p sublevel holds 6 e-

d. The 2s sublevel has a 2s orbital holding 2 e-

It also has 3 p orbitals that hold 2 e-each.

3rd E level

1. Holds 18 e- total

2. 3s, 3p, 3d sublevels

3. 3s = 2

1 s orbital

4. 3p = 6

3 p orbitals

5. 3d = 10

5 d orbitals

Light cont.

� A photon or “packet of light” is produced when electrons jump to outer E levels, and then fall back.

� The bigger the jump, the more E released

ROYGBIV