Chemistry - Unit 3 review

Electromagnetic Spectrum, Visible light spectrum, The 3 rules for orbitals, Energy useage

What happens when an electron absorbs energy?

The electron gains energy and move from it;s ground state (lowest state) to a higher energy level called excited state. This means it jumps farther away from the nucleus, the electrons usually back down to the ground state when it does it release energy often as light ( a photon)

What happen if the electron goes up and down?

absorbs energy - jumps to excited state

releases energy- returns to ground state

What can be observed when an electron in a atom released energy in a visible region ?

the electron falls from a higher energy level ( excited energy) to a lower energy level (ground state). The energy difference between those levels is released as a photon of a visible light. The color of the light depends on how much energy is released. More energy has shorter wave lengths blue/violet. Less energy has longer wave lengths red/orange.

What are the seven electromagnetic spectrum in in order from highest to to lowest

energy/frequency - gamma rays, x-rays, ultra Violet (UV), visible light, infrared, microwaves, radiowaves

wavelengths- radiowaves, microwaves, infrared, visible light, ultra Violet (UV), x-rays, gamma rays

Write the colors in the visible light spectrum from highest to lowest?

energy/ frequency - violet, indigo, blue, green, yellow, orange, red

wavelengths- red,orange, yellow, green, blue, indigo, violet

What is Aufbau’s Rule ?

orbitals of the lowest energy and fill them up first 

What’s Hund’s rule?

multiple orbitals of same energy, more than one way to distribute them ( doesn’t share a box spread out first)

What’s Pauli’s Rule?

The arrow can’t face the same way. no two electrons in an atom have the same 4 quantum number can’t face the same direction.