U5 Electron Vocabulary Flashcard

The height of a wave from the origin to a crest or from the origin to a trough.
Atomic Emission Spectrum
Colors of light given off when atoms of an element absorb energy. When atoms become “excited” by heat or electricity, their electrons hop up to higher energy levels. And when the electrons fall back to their normal energy level, they emit photons. And this light given off by excited atoms has distinctive colors.
Atomic orbital
A three-dimensional region all around the nucleus that helps us estimate where the possible location of an electron could be. First level is closest to the nucleus.
Aufbau Principle
Used to determine electron configuration of an atom. An atom builds up itself by adding more electrons, starting with the lowest electron level, until the atom assumes it’s most stable condition
Balmer Series
A series of lines in the visible spectrum of hydrogen.
The maximum displacement point of a wave.
Color spectrum
Also known as the visible spectrum. Different colors make up white light and this is the distribution of colors when light is dispersed by a prism. As we move up the frequency increases and wavelenght decreases.
De Broglie Equation

this is an equation used the explain and describe the wave nature of an electron.

? = h/mv

(wavelength= constant/mass x velocity)

Electromagnetic Radiation
this is a form of energy that comes from charged particles; it is described and categorized by the electromagnetic spectrum
Electromagnetic spectrum
The range of wavelengths or frequencies over which electromagnetic radiation extends
Electron configuration
The electron configuration of an atom is the particular distribution of electrons among available shells.
Electron dot diagram
A structural formula in which electrons are represented by dots; two dots between atoms represent a covalent bond. Also known as electron-dot formula; Lewis formula.
Energy sub-level
Energy Sub-levels are Energy levels divided up into four letter going s
Flame test
An experiment that identifies metals by the color the metal emits when heated
the measurement of the number of times that a repeated event occurs per unit time
Ground state
The lowest energy state of an atom
Heisenberg Uncertainty Principle
This principle states that you can either know the position or momentum of an electron, but not both.
Hund’s rule
Hunds rule is when every orbital In a subshell has one electron before a single orbital is double occupied with two. 
Lyman Series
set of ultraviolet emission lines that go hand in hand with electron movement from higher energy levels to lower
Pashen series
infrared wavelength series; a series of lines in the infrared spectrum; electrons drop in the N = 3 orbit
Pauli’s exclusion Principle
Principle that states electrons cannot have the same four quantum numbers. At least the final quantum number has to be different.
Photoelectric effect


Effect when electromagnetic radiation, such as light (photons), is exposed to matter, it causes electrons to be emitted from the matter (bounce off).

A quantum amount of energy that an electron gains as it tracs around the nucleus and releases as the electron jumps back to its original energy level; it creates light and other waves
Planck’s constant

It’s the constant proportion relating a photon’s energy to its frequency; it’s expressed by h.


The formula follows:

h=6.626069 EE -34 m^2 kg/s

Principal energy level
A major energy ring of an atom that is marked by the quantum number nvaries in range for each element depending on how many of these there are in each element.
the minimum amount of energy that can be gained or lost by an atom. 1 photon of light is equal to one quantum of energy. It’s as measured amount.
Quantum mechanical model of the atom
A model that shows electrons having a movement that is associated with waves. The model is related to Schrodinger’s equation and follows quantum theory.
Quantum numbers
Speed of light
Valence electron
Delocalized electron
Electrons in a molecule ion or atom that aren’t associated with a single atom or covalent bond
The act of one giving a blowjob while the recipient is taking a shit.

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