Chapter 6 SPECTROSCOPY, LIGHT AND ELECTRONS

Schrödingers equation

Schrödingers equation

________ required the use of three quantum numbers to describe each electron within an atom, corresponding to the orbital size, shape, and orientation in space.

Electromagnetic spectrum

________- radiant energy composed of gamma rays, x- rays, ultraviolet light, visible light, etc.

Frequency

________-- the number of waves that pass a point per second.

Wavelength

________ is the distance between two identical points on a wave.

X ray photons

________ can excite core electrons.

wave function

Squaring the ________ (orbital) gives the volume of space in which the probability of finding the electron is high.

Bohr model

The ________ postulated a ground state for the electrons in the atom, an energy state of lowest energy, and an excited state, an energy state of higher energy.

Equation l

________= h /mv, which indicates a mass (m) moving with a certain velocity (v) would have a specific wavelength (l) associated with it.

Schrödinger

________ developed a mathematical description of the electrons motion called a wave function or atomic orbital.

Amplitude

________ is the height if the wave and is related to the intensity amd amplitude of a wave.

quantum number

The first ________ is the principal quantum number (n)

angular momentum quantum number

The second quantum number is the _____________________________ (l). Its value is related to the principal quantum number and has allowed values of 0 up to (n - 1).

magnetic quantum number

The third quantum number is the ________________ (ml). It describes the orientation of the orbital around the nucleus.

spin quantum number

The fourth quantum number, the _______________________ (ms), indicates the direction the electron is spinning.