Studied by 47 PeopleTags & Description
Energy
The capacity to do work
Light
A form of radiation which can be defined as an energy that travels in the form of electromagnetic waves.
Wavelength
The shortest distance between two equidistant points on a wave.
Amplitude
A waves height from the origin to a crest or a trough
Crest
Highest point on a wave
Trough
Lowest point on a wave
Graph of Wave
Frequency
The number of waves that pass a fixed point in unit time
Qualities of Wavelength and Frequency
Wavelength and Frequency are inversely related Shorter wavelength=higher frequency= higher energy.Larger Wavelength=lower frequency=lower energy
Electromagnetic Spectrum
Represents all forms of electromagnetic radiation (light)
Visible Light Diagram
What are the different ways Light can be portrayed?
Light can be portrayed as Light Waves and Particles
Qualities of Light as a Wave
Waves are oscillations, meaning they wiggle , they transport energy from one place to another, waves don't really bounce off of but instead interfere with one another.
Qualities of Light as a Particle
Particles will move in straight lines until something changes their direction. Particles can bounce off other particles, and they can change trajectories.
Energy, Light, Wavelength, Frequency,
Speed of Light- 3.00x10^8 Energy- E Wavelength- Upside-down Y (Lambda) Frequency- v
Plank's constant
Plank's Constant- 6.626x10^-34 Plank's constant- h
Formulas
Ground State
The lowest allowable energy state for an atom
Visible Series
Balmer
Ultraviolet Series
Lyman
Infrared Series
Paschen
How do atoms gain energy?
Electrons move excitedly
How do atoms in their excited state return to their ground state?
By releasing energy in the form of light
What is Bohr's information largely based off of?
Atomic emission spectra observed for hydrogen and helium
Atomic Emission Spectra
Set of frequencies of the electromagnetic waves emitted by the atoms of the element
Qualuties of the Atomic Emission Spectra
Unique to each element
Can be used to identify an element.
Individual wavelengths of light, not a continuous mixture of all frequencies of the visible spectrum.
Atomic Orbital
Three dimensional region around the nucleus that is most probable to describe an electron's location
Energy Sublevels
Tells the shape of the orbital (s,p,d,f)
Principal Quantum Number (n)
Tells the size and energy of atomic orbitals
Principal Energy Levels
The energy levels increase in size and energy the farther they are from the nucleus.
KNOW HOW TO DO ELECTRON CONFIGURATION
BOTH WITH THE NUMBERS AND WITTH THE BOXES AND ARROWS/CIRCLES AND X'S
Hund's rule
in the P,D, and F sub levels, each orbital gets one electron before any orbital gets a second electron
Notable gas configuration
A shorthand method that shortens the configuration by referencing the noble gas that comes before the element and then finishing the remaining portion of the configuration.
Notable Gas examples
He, Ne, Ar, Kr, Xa, Rn
Valence Electrons
The electrons in the highest energy level of an atom
Valence Electrons more in depth
Electromagnetic Radiation
A form of energy that exhibits wavelike behavior as it travels through space
Objects with the Highest forms of Electromagnetic Radiation, Highest Frequencies, and Lowest Wavelength
Gamma Rays and X Rays
Objects with the Lowest Forms of Electromagnetic radiation, Lowest Frequencies, and Highest Wavelengths
Radios and Microwaves
Colors on the Electromagnetic Spectrum with the longest Wavelength
Red and Orange
Colors on the Electromagnetic Spectrum with the shortest Wavelength
Purple and Blue
What did Max Plank discover
Matter can gain or lose energy only in small and specific amounts of quanta.
Quantum
the minimum amount of energy that can be gained or lost by an atom.
Photoelectron Effect
Electrons, called photoelectrons, are emitted from a metal's surface when light of a certain frequency, or higher than a certain frequency, shines on the surface. Basically saying when light hits the metal surface of something in a certain way, an electron is lost from the metal.
Bohr's Model of the Electron
A quantum model for the hydrogen atom
The Limitation of the Bohr's model
It failed to explain the spectrum of any other element. It also did not take into account the chemical behavior of atoms.
The Quantum Mechanical Model
Louis de Broglie's proposed model that accounted for the fixed Energy levels of the Bohr's model
How did the Quantum Mechanical model describe electrons?
This model described electrons as waves
Heisenberg Uncertainty Principle
States that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.
Atomic Orbital
Describes the electron's probable location
Sublevel
The energy level contained within a principle energy level
