Studied by 14 peopleWavelength
The distance between two waves
Amplitude
The height of a wave
Frequency
How often a wave goes up and down
The speed of light
c = 3.0 x 10^8 m/s
FOR THE LEFT SIDE: say if it has (short or long) or (lowest or highest): wavelength, energy, and frequency
Short Wavelength High energy High frequency
FOR THE RIGHT SIDE: say if it has (short or long) or (lowest or highest): wavelength, energy, and frequency
Long Wavelength Low energy Low frequency
FOR THE LEFT SIDE: say if it has (short or long) or (least or most) (lowest or highest): wavelength, energy, and frequency
Short wavelength Most energy Highest frequency
FOR THE RIGHT SIDE: say if it has (short or long) or (least or most) (lowest or highest): wavelength, energy, and frequency
Long wavelength Least energy Lowest frequency
In order for an electron to move to another level they have to...
...absorb a specific amount of energy
Excited State
When electrons absorbs energy and moves to a higher energy level
Ground State
When electrons "fall" back to their original energy level, they release light
Are excited states stable or unstable?
Unstable
How does the Emission Spectra connect to changing the color of light?
The higher the fall the more energy is released, changing the color of light produced.
What are the 3 rules for Electron Configurations?
• Aufbau principle • Pauli Exclusion Principle • Hund’s Rule
Aufbau
Electrons occupy orbitals of lower energy first.
Pauli Exclusion Principle
An orbital can hold only two electrons and they must have opposite spin.
Hund's Rule
In a set of orbitals, the electrons will fill the orbitals in a way that would give the maximum number of parallel spins (maximum number of unpaired electrons).
In the configuration: 1s^2, what does 1 mean?
The MAIN energy level
In the configuration: 1s^2, what does "s" mean?
Sublevels
In the configuration: 1s^2, what does ^2 mean?
Number of electrons in the sublevel
What is the block for the blue area?
s
What is the block for the red area?
d
What is the block for the orange area?
p
What is the block for the green area?
f
How to calculate the noble gas abbreviation.
Use the last noble gas that is located in the periodic table right before the element.
Write the symbol of the noble gas in brackets.
Write the remaining configuration after the brackets. Ex: Fluorine: [He] 2s^2 2p^5
A family is a ? on the periodic table
Column
Where are the alkali metals?
First column
Where are the alkaline earth metals?
Second column
Where are the transition metals?
Middle section
Where are the metalloids?
Staircase
Where are the halogens?
Second to last column
Where are the noble gases?
Last column
Atomic radius
the size of the atom. PLURAL : Atomic radii
Atomic radius gets (smaller/larger) going down a group and why?
Larger, because we are adding another valence shell.
Atom raduis get (smaller/larger) across a period and why?
Smaller, because the charge in the nucleus is increasing.
Electronegativity
A measure of the attraction an atom has for electrons when bonded.
Electronegativity gets (smaller/larger) going down a group.
Smaller
Electronegativity gets (smaller/larger) going across.
Larger
Which element has the most electronegativity?
F (Fluorine) has the greatest electronegativity at 4.0
Ionization Energy
The energy required to remove an electron from a gaseous atom or ion.
Ionization Energy gets (smaller/larger) going across.
Larger
Ionization Energy gets (smaller/larger) going down.
Smaller
Electron Affinity
Energy released when an electron is added to the atom.
Electron shielding
Atoms with more energy levels can't hold onto their valence electrons as strongly. The pull from the nucleus is partially blocked by each layer of electrons.
(Easier/harder) to remove an electron with more shielding?
Easier
Cation
When atoms lose valence electrons, they become positively charged ions.
Cations are always (smaller/larger) than the original atom.
Smaller
Anions
Atoms that gain electrons become negatively charged ions. Atoms gain electrons in their outermost shell.
Anions are always (smaller/larger) than the original atom.
Larger
Most reactive NON-metal?
Fluorine - F
Most reactive METAL?
Francium - Fr
Note
Flashcard