1. Quantum
2. Quantum number

1. A packet of energy associated with a specific wavelenght of electromagnetic radiation.
2. A number used to describe the energy levels available to an electron. Each electron in an atom has a unique set of four.

Planck's constant

Planck's constant (h) is equal to:

6.63 x 10^-34J-sec/particle

1. Emission spectrum
2. Absorption spectrum

1. A bright line spectrum formed when energy absorbed by an element is emitted at specific wavelenghts. Each element has a unique spectrum
2. A dark-line spectrum formed when white light is passed through a vaporized element and a few specific wavelenghts are absorbed.

Quantum theory equation relating:

Wavelenght to frequency

c = fλ

c = speed of light (3x10⁸meters/sec)

f = frequency in hertz

λ = wavelenght in meters

Quantum theory equation relating:

Energy to frequency

E = hf

E = energy in joules

h = 6.63x10^-34 J-sec/particle (Plank's Constant)

f = frequency in hertz

Quantum theory equation relating:

Energy to wavelenght

E = hc/λ

h = 6.63x10^-34 J-sec/particle (Plank's Constant)

c = 3x10⁸ meters/sec (speed of light)

λ = wavelenght in meters

Lyman, Balmer, and Paschen series

Group of lines in the emission spectrum of hydrogen.

Lyman - ultraviolet, 6 lines

Balmer - visible, 5 line

Paschen -  infra red, 4 lines

List 3 basic postulates of the Bohr model for the hydrogen atom.

1. e- are present only in specific energy states
2. A quantum of energy is absorbed or emitted to change the energy levels.
3. A quantum- smallest amount of energy that can be gained or lost.

1. Ground state
2. Excited state

1. Electron is at its lowest energy level, as close to the nucleus as possible
2. An electron absorbs energy and moves to a higher energy level above the ground state

List four quantum numbers and their symbols

1. Principal energy level: "n"
2. sublevel: "l"
3. orbital: "m_l"
4. spin: "m_s"

List the names of the first four energy levels (or shells)

#1 or K

#2 orr L

#3 or M

#4 or N

What is the electrin capacity of the energy levels 1 to 7? What is the basic formula for electron capacity?

for level #1 e- capacity equals 2.

#2 - 8; #3 - 18; #4 - 32; #5 - 50; #6 - 72; #7 - 98

fomula for electron capacity

e- capacity = 2n² (n = level#)

List the names of the four sublevels and their electron capacities

s holds 2

p holds 6

d holds 10

f holds 14

Orbital

How many orbitals in each sublevel?

An orbital is contained in a sublevel and holds 2 e-

s - 1

p - 3

d - 5

f - 7

Which sublevels are present in energy levels #1, #2, #3, #4, - #7?

#1: s

#2: s, p

#3: s, p, d

# 4-7: s, p, d, f

Describe the shapes of the orbitals.

1. s
2. p
3. d
4. f

1. s - sphere
2. p - dumbell shape with 2 lobes
3. d - double dumbbell; most have 4 lobes
4. f - most have 8 lobes

Pauli exclusion principle

How does it relate to electron spin?

No two e- in an atom have an identical set of 4 quantum numbers.

The 2 e- in any orbital must have opposite spins (+1/2 or -1/2)

What is the order for filling sublevels (Aufbau process) form lowest to highest energy?

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d

1. Electron configuration
2. Write the electron configuration for Lithium and Iron

1. The distribution of electrons into shells and subleves for an atom of an element. Each element has a unique electron configuration
2. Lithium - 1s²2s²
3. 1s²2s²2p⁶3s²3p⁶4s²3d⁶

Hund's Rule

Within a sublevel the order of filling orbitlas is chosen to maxime half filled orbitals. All single electrins have parallel spins.

Valence

What are the valance of the elements of families IA throught VIIA?

the number of e- in the atom's highest numbered or outermost shell.

the valences of elements in groups IA - VIIIA are the element's column number. For the example, the valence pf Na (sodium) is 1; O (Oxygen) is 6

Write valences of:

1. Na
2. Cl
3. O
4. Al

1. 1 (Na)
2. 7 (Cl)
3. 6 (O)
4. 3 (Al)

Lewis dot structure

Consists of the atom's surronded by the same number of dots atom's valence. May be used for elements, compounds or polyatomic ions.

Photon

An individual packet or quantum of radiant energy of a specific wavelenght.

1. Paramagnetic
2. Diamagnetic

1. An atom or group of atoms which has magnetic properties due to unpaired electrons in its orbitals.
2. A term indicating a substance which does not contain unpared electrons and is therefore not attracted to a magnetic field.

Spectroscope

Instrument which disperses light emitted by energized atoms and allows examination of their spectra.