Nuclear instability and Light

Nuclear instability and Light

Mrs.King

Nuclear decay

• Alpha decay- loss of alpha particle

• beta decay- neutron and loss of e^-

• gamma decay- nuclear fission and excess energy

• Alpha and beta are nuclear changes

• gamma is caused by alpha and energy

Light

c=the speed of light

Light are wave particles

• Photons

• electromagnetic wave particles-electric field and magnetic field

• quantum

Components of light waves

•  $\lambda$   $\nu$  =C

•  $\lambda$  wavelength

•  $\nu$  frequency

• c the speed of light constant 3.00 x 10^8

• amplitude

Wavelength

• distance of one crest to another

frequency

• the number of waves that occur in per unit time

amplitude

• distance between origin and creat

Speed of light

• the constant speed that light travels in a vacuum

• 3.00 x 10⁸

electromagnetic spectrum

• increase frequency=increase in energy

• wavelengths increase as energy increases

Multiple Choice

what is the frequency

• the distance of one crest to another

• the number of waves that occur in per unit time

• the distance between the origin and crest

Multiple Choice

A news broadcast on a statin that transmits at 780.0 kHz (convert to Hz) what is the wavelength?

• 384.6 m

• 3.846 x 10³ m

• 3.846 x 10⁸ m

Orbitals and electrons

Multiple Choice

a photon is

• a particle of light

• energy released by an electron as it returns to the ground state

• all of the above

Electrons

• the gain loss or sharing of electrons create chemical bonding

• are found in orbitals around the nucleus

Valence shells

• outermost energy shell

• the reactive e^- 's

• the bonding force

Orbitals

• dense electron clouds where e^-'s are most likely to be found

• they increase the diameter of the atom

• S,P,D,F

S orbital

• spherical

• 2 e^-

• 1S (1S₁ 1S₂)

• 2S (2S₁ 2S₂)

S orbital examples

• Hydrogen has 1e^- (1S₁)

• Helium has 2e^- (1S₂)

• Lithium has 3e^- (2S₁)

• Beryllium has 4e^- (2S₂)

Filling orbitals

• must fill orbitals in order from lowest ground state

• Aufbau principle

P orbitals

• dumbbell shaped

• hold 6 e^-

• 2P, 3P, 4P, 5P, 6P

P orbital examples

• boron 5 e^- (1S₂2S₂2P₁)

• Carbon 6e^- (1S₂2S₂2P₂)

• Nitrogen 7e^- (1S₂2S₂2P₃)

• Oxygen 8e^- (1S₂2S₂2P₄)

• Fluorine 9e^- (1S₂2S₂2P₅)

• Neon 10 e^- (1S₂2S₂2P₆)

Multiple Choice

What is the electron configuration for Neon (Ne)

• 1S₂2S₂2P₆

• 1S₂2S₂2P

• 1S₂2S₂1P₅

• not enough information

Multiple Choice

What is the electron configuration for Aluminum (Al)

• 1S₂2S₂2P₆3S₂4P₁

• 1S₂2S₂2P₆3S₂3P₁

• 1S₂2S₂1P₆3S₁

• 1S₂2S₂2P₆3S₂3P

D orbital

• shapes vary a little

• hold 10 e^-

• make great catalyst

F orbitals

hold 14 e^-

Pauli exclusion principle

• e^- can only share an orbital if their spin is in opposite directions

Hund's Rule

electrons will fall into empty orbitals of the same energy before electrons begin to pair up into the same orbital.

electron configuration

unpaired- paramagnetic

paired- diamagnetic

Quantum numbers

• Principle- size of energy level

• angular momentum- shape of the orbital

• spin- spin of e^-

• magnetic- orbital orientation