Chemistry Thing

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