Originate from the movement of electrical charges

Do not require a medium to move

________________- the distance of one wave cycle Often taken from one crest to the next but only has to be

two identical points Symbol is Length units

__________________- # of wave cycle that pass a given point in a given unit of time Symbol is Units: cycles/sec, sometimes written as 1/s, also equals

1 Hertz (Hz)_____________________

Distance between the zero amplitude line and the top of the crest

Waves with higher amplitudes carry more energy

_________________ is the wavelength in meters is the frequency in s-1 (or Hz)c is the speed of the wave

For electromagnetic radiation, use the speed of light 2.99792458 x 108 m/s (round this to 3.00 x 108 m/s)

There is an _____________ relationship between wavelength and frequency

Light can be passed through a prism and makes a rainbow. This is a ________________ spectrum.

Proposed that electromagnetic energy comes in discreet amounts (or _____________________)

The energy of a quantum is expressed by ____________where h= 6.626 x

10-34 J sEnergy can only increase by

multiples: 1 h, 2 h, 3 h, and so on

Applied the idea of quanta to explain how light can cause electricity:Tiny packets of light (photons) hit an atom. If they have enough energy, they can kick an

electron out of an atom (photoelectric effect)So light is a wave and a “packet”

Remember: Bohr revised Rutherford’s model, putting the electrons in orbitals like planets around the sun

Excited electrons could jump orbital levelsWhen electrons returned to their original

level (ground state), they emit energyCreates a ________ spectrum

Created when only a few wavelengths of the electromagnetic spectrum are seen

Gases of each element will make them when electricity passes through them or they’re heated up.

The lines can be seen when the light is passed through a prism.

Lines are different for each element (_____________________________)

Mercury

Calcium

Sodium

Helium

Hydrogen

BRIGHT LINE SPECTRA

7500 7000 6500 6000 5500 5000 4500 4000 A

7500 7000 6500 6000 5500 5000 4500 4000 A

Electron behave like ____________ (matter) and ____________ (electromagnetic radiation)

If this is true, electrons can’t be tied to a fixed orbit

We can’t even be certain of both an electron’s momentum and position at any one point in time (Heisenberg uncertainty principle)

Can only create shaded areas around the nucleus where there is a high _________________ of finding electrons

System of numbers that gives each electron a unique address in any atom

Also called ______Represents the primary energy levels around

the nucleus (kind of like Bohr’s rings)There are 7 energy levels so _____________Electrons with a higher n are in higher

energy orbital and spend more time away from the nucleus

Electrons with the same n are in the same principle shell

Also called l or ___________Determines the shape of the orbital

____ sublevel _____ sublevel_____ sublevel_____ sublevel

Spherical in shape

Look like a dumbbell in each axis (x, y, and z)

Also called ml or the orbitalIf

s subshell……_____ orbitalp subshell……_____ orbitalsd subshell……_____ orbitalsf subshell…..______ orbitals

Two electrons can fill each orbitalAnother quantum number is needed so every

electron has its own numberElectron Spin Quantum Number

Also called ms

Electron can spin _________________________________

An orbital with two electrons has one of eachAlso represent them with ___________

Silver has 47 electrons (odd number). On

average, 23 electrons will have one spin, 24 will

have the opposite spin.

The magnet splits the beam.

These silver atoms each have 24 +½-spin electrons and 23 –½-spin electrons.

These silver atoms each have 23 +½-spin electrons and 24 –½-spin electrons.

Description of the placement of all the electrons in an atom of an element

RulesElectrons occupy the lowest energy orbitals

available (ground state). Filling order is determined by Aufbau Principle.

Orbitals can only hold 2 electrons and they must have opposing spins (Pauli exclusion principle)

Electrons will fill empty orbitals when possible. Half-filled orbitals all have parallel spin. (Hund’s rule)

Remember this is the real location of the f block

RegularEnergy level is written as a

numberSubshell letter is written

nextNumber of electrons in

subshell is given as an exponent

ExtendedSame as regular, but

subshells are divided into the individual orbitals

RegularHe _________O ______________Cl ________________________

ExtendedHe __________O _____________________Cl _______________________________

Same as spdf configuration but it starts from the noble gas of the previous period

ExamplesBe _______________K _______________Br ________________

Same as spdf configuartions exceptNumber of electron in subshell is not writtenEach orbital within subshell is given a line↑ and ↓ arrows are drawn on the lines to

represent the electrons (fourth quantum number)

Make sure to follow Hund’s ruleExamples:

N _________________________O __________________________

Electrons in the __________________of an atomElectrons in lower energy levels are called

______ electrons

Can be predicted by the periodic table for representative elements

Helium only has 2.

D and f-block elements have 2, but can vary

Dots are placed around the element symbol to represent to valence electrons

To be stable, atoms want __________ in their outer shell

Noble gases already have 8 and don’t usually react with anyone

Others will lose or gain electrons to get to 8 Said to be isoelectronic with the Nobel gas from the last

periodIon will have the same electron configuration as this noble gas

Atoms that gain or lose electrons to become isoelectronic with Helium follow the duet rule (2 electrons in valence shell)

Group 1- 1 valence electron Lose 1 electron, become +1 cation

Group 2- 2 valence electrons Lose 2 electrons, become +2 cation

Group 13- 3 valence electrons Lose 3 electrons, become +3 cation

Group 15- 5 valence electrons Gain 3 electrons, become -3 anion

Group 16- 6 valence electrons Gain 2 electrons, become -2 anion

Group 17- 7 valence electrons Gain 1 electron, become -1 anion

Transition metals form cations, but the charge cannot be predicted

Group 14 does not commonly form ions

Group 18 does not form ions

The metal properties of the elements increase as you move to the left and move down on the periodic table

Metals Nonmetals

Conduct electricity well Don’t conduct electricity well

Malleable Brittle

Ductile Not ductile

Tend to lose electrons Tend to gain electrons

Low electronegativity High electronegativity

Slightly negative electron affinity Very negative electron affinity

Found in bases Found in acids

Shiny Dull

Ionization energy is the amount of energy needed to remove an electron

Need more energy as you move up and to the right of the periodic table

Electronegativity is the ability of an atom to attract electrons

Increases as you move up and to the right of the periodic table (noble gases sit out)

Atomic size increases as you move down and to the left of the periodic table