Unit 2: Light and Electrons

Electromagnetic Waves

100

When a wave absorbs energy it moves from this state and then jumps to the excited state

The ground state

200

This is the wave property that has an inverse relationship with energy

wavelength

300

This is the study of how matter interacts with light and other forms of electromagnetic radiation

Spectroscopy

400

This the the wave with the lowest wavelength on the spectrum

Gamma Rays

500

This is the acronym that will help me to keep the colors of light in order of increasing energy

ROY G BIV

EMS Math

100

This is the amount of waves that pass by a given point every second

Frequency

200

If I get a really small value for this measurement on my test I must have made a mistake in my calculation

The frequency

300

I solved for the wavelength using the speed of light equation using the equation 

v/c = λ and my answer is 2.92 x 10⁶ m

This is the mistake that I made.

I rearranged the formula wrong and should have divided c/v

400

These are the three units that I am going to use this unit and will always list with my numerical answers

Meters, Hertz, and Joules

500

This is the wave that travels at the greatest speed

Trick Question!!!

Electron Configuration

100

This is the element represented by the location 5f⁴

Uranium

200

An atom has the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁴. Without identifying the element, determine the highest occupied energy level and the number of valence electrons.

3rd Energy Level and 6 valence electrons

300

When drawing arrows in the orbital notation these are the rules that I need to follow

fill lower energy levels first, every orbital in a sublevel must get one electron before doubling up, arrows (electrons) must have opposite spins.

400

Electron configurations give chemists this information, which can later be used to predict properties such as bonding, ion formation, or magnetic behavior.

the arrangement of an atom’s electrons among its energy levels and orbitals

500

This is the number of electrons that you can have for each orbital

Two

Lewis Dots and Bohr Models

100

When converting a Bohr model into a Lewis dot diagram, these are the only electrons that carry over.

valence electrons

200

This is the goal for every element on the table and drives reactivity

To reach the lowest energy state possible which is most often an octet of electrons like noble gases have.

300

A bohr model helps you to understand why d block electrons are not counted toward the valence electrons because of this behavior of d block electrons

They will fill into the gaps of lower energy levels instead of the highest energy level

400

This report of distinct bands of color provided evidence for Bohr’s model of the atom and helps explain why his model is still useful today, even though we know it is no longer accurate.

The emission spectrum

500

This is the reason that lewis dot diagrams are useful

They model valence electrons, allowing us to predict how elements may react to achieve a stable octet.