Chemistry

Top of the wave to the origin lineCarries the energy – does not impact either frequency or wavelength

Chapter 6.1 - 6.4 Review

Distance between 2 successive peaks of 2 waves Represented by the Greek letter (lambda)


Number of complete waves passing a fixed point in a given time Represented by the Greek letter (nu)


Radiant energy emitted across a wide variety of wavelengths


3 x 108 m/s


c = x

So c = wavelength times frequency


Inverse relationship – As one variable increases, the other variable decreases


Red at 750 nm


Violet at 400 nm


Gamma Rays


Radio waves (specifically, AM radio)


Gamma Rays – X Rays – Ultraviolet (UV) – Visible Light – Infrared (IR) –Microwaves – Radio Waves


ROYGBIVRed – Orange – Yellow – Green – Blue – Indigo - Violet


“Chunk” or fixed minimum amount of energy absorbed or emitted



hchE

Chapter 6.1 - 6.4 Review – Period 7

h = 6.6262 x 10-34 J∙s

Light consist of quanta called photons that carries energy equal to h


Sunlight striking a sheet of metal will knock off and move electrons, thereby causing an electric current


Both electrons and photons sometimes act as if they are particles (mass) and sometimes act like they are waves (energy) – Dual wave/particle nature


Radiation composed of only one wavelength


A spectrum


A spectrum of only certain wavelengths – not all of them


Specific energy levels that electrons existed in


When electrons are excited (added energy), jump into higher energy levels. When they moved back into lower energy levels - gave off light.


No. They absorb and emit only a quantum (fixed amount) of energy.



hEEE if


2218 11

J 1018.2

if nn

hchE

Absorbed


Emitted


Principal quantum number

Denotes energy level


Ground State


Excited State



mv

hWhere v = velocity

It is impossible to know the position, direction, and speed of an electron at any one point in time – can know two variables, but not the third


Sports