Study your flashcards anywhere!

Download the official Cram app for free >

  • Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off

How to study your flashcards.

Right/Left arrow keys: Navigate between flashcards.right arrow keyleft arrow key

Up/Down arrow keys: Flip the card between the front and back.down keyup key

H key: Show hint (3rd side).h key

A key: Read text to speech.a key


Play button


Play button




Click to flip

29 Cards in this Set

  • Front
  • Back
Electronic Structure
Describes the energies and arrangement of electrons around the atom or molecule
Electromagnetic Radiation
A form of energy that has wave characteristics and propagates through a vacuum at a speed of 3.00*10 to the 8th meters/sec
Electromagnetic spectrum
the complete range of electromagnetic waves, from radio waves to gamma rays
The distance between two crests of a wave
Blackbody radiation
The electromagnetic radiation emitted by a heated object
A small, discrete packet of light energy
Photoelectric effect
the emission of electrons from a metal surface induced by light
Work function
the amount of energy required for an electron to overcome the attractive forces that hold it to the metal
Planck's constant (h)
the constant that relates the energy and frequency of a photon. the value of planck's constant is 6.63*10 to the -34 J-sec
another term for a single quantum of light, a name chosen to emphasize the particulate nature of light
the distribution among various wavelengths of the radiant energy emitted or absorbed by an object
continuous spectrum
a spectrum that contains radiation distributed over all wavelengths
line spectrum
spectrum that contains radiation at only certain specific wavelengths
ground state
the lowest energy or most stable state
excited states
a higher energy state than the ground state
matter waves
describes the wave characteristics of a particle
Heisenberg Uncertainty principle
There is an inherent uncertaint in the precision with which we can simultaneously specify the position and the momentum of a particle. This uncertainty is significant only for extremely small particles such as electrons
Wave function
a mathematical description of an allowed energy state (an orbital) for an electron in the quantum mechanical model of the atom. It is usually symbolized by the greek letter psi
probability density
a value that represents the probablility that an electron will be found at a given point in sapce
probability cloud
the pattern of electron positions plotted over time to show the likelihood of an electron's being at a given position at a given time
allowed wave functions of the hydrogen atom, described by a combination of an integer and a letter, corresponding to values of three quantum numbers
the set of one or more orbitals with the same n and l values
electron shell
the set of all orbitals with the same value of n, such as 3s, 3p, and 3d
radial probablility function
tells us the probability that the electron will be found at a certain distance from the nucleus
the point at which the amplitude of the wave function is zero
f-block metals
the antinides and lanthanides
rydberg constant
determined when measuring the spectrum of hydrogen, relates the values of hydrogen's principle quantum numbers to their energy
term used to describe orbitals within the same subshell are degenerate which have the same energy
Hund's rule
states that the lowest energy is attained by maximizing the number of electrons with the same electron spin