Atomic Theories

Radiant energy

________ emitted by atoms occurred in small bundles called quantum.

Heavy objects

________ have short wavelengths, tiny particles with low masses have longer wave lengths.

Electrons

________ are paired with a standing wave.

Atoms

________ could only absorb or emit radiant energy in one or multiples of one quantum (discrete quantities only)

Electron

3: ________ can travel in an orbit without radiating energy.

electromagnetic wave

Light is a(n) ________ consisting of a continuous series of wavelengths.

Relaxation

________: electron releases energy (electromagnetic radiation) and moves to a lower energy level.

Excitation

________: electron absorbs energy (heat, light, electricity) and moves to a higher energy level.

Waves

________ are continuous travelling disturbances, Particles are discrete bundles.

Ground state

________: the lowest energy for that electron (closest to the nucleus)

Bands

________ of light occur when the waves reinforced each other (in phase) and underwent constructive interference.

Bands

________ of dark occur when the waves cancel each other (out of phase) and underwent deconstructive interference.

Light consisted of a stream of energy packets/quanta

later called photons

1

Atoms and electrons can only exist in specific energy states

2

Each energy level corresponds to an orbit

3

Electron can travel in an orbit without radiating energy

4

Electron may only change its energy by jumping from one allowed energy state to another

Atomic spectra

Absorption spectra & Emission spectra

Absorption Spectra (dark line spectrum)

Excitation (photons absorbed)

Emission Spectra (bright line spectrum)

Relaxation (photons released)

Continuous Spectrum

contains all frequencies of visible light (white light)

UV

Lyman series

IR

Paschen series

Excitation

electron absorbs energy (heat, light, electricity) and moves to a higher energy level

Relaxation

electron releases energy (electromagnetic radiation) and moves to a lower energy level

Ground state

the lowest energy for that electron (closest to the nucleus)

Quantized energy

atoms can only absorb or release the exact amount of energy required for electrons to move from one allowed energy state to another

Wavelength of a matter wave

λ = h / mv