Chem 31: Chapter 12

Contains electrical and magnetic fields that simultaneously oscillate in perpendicular planes through space, allowing energy to propagate mediums

The distance between two consecutive crests or troughs of a wave

Number of cycles per second that pass a given point in space

Common unit for frequency

Radiation that originates solely from an idealized object that absorbs all radiation

A radiation profile with no maximum that goes to infinite intensity at very short wavelengths

The phenomenon by which electrons are emitted from the surface of a metal when light strikes it

The phenomenon by which light exhibits properties of both waves and particles

Derived the relationship between a particle's wavelength and momentum

The scattering of light from a regular array of points or lines

Contains all the wavelengths of visible light; not quantized (ex. white light)

Only a few lines result, each corresponding to a discrete wavelength (ex. hydrogen emission spectrum)

The electron in a hydrogen atom moves around the nucleus only in certain "allowed" orbits

Lowest possible energy state

Approach to describing atoms taken by deBroglie and Schrodinger, in which emphasis was given to the wave properties of the electron

An electron's coordinates in (x,y,z) form

A set of mathematical instructions for describing wave function

A specific wave function for an electron

There is a fundamental limitation to just how precisely we can know both the position and momentum of a given particle at a given time.

indicates the probability value of an electron at a given point in space

Total probability of finding the electron in a hydrogen atom at a particular distance from the nucleus

Related to the size and energy of an orbital

Relates to the shape of an orbital's subshell

Relates to the orbital's orientation in space

Orbital areas with zero probability of having an electron

All orbitals with the same energy

fourth quantum number; can equal +1/2 or -1/2

In a given atom, no two electrons can have the same set of four quantum numbers.

Atoms with more than one electron

The apparent nuclear charge

A method in which a given electron is assumed to be moving in a potential energy field that is a result of the nucleus and the average "electron density" of all other electrons

Groups of three elements with similar properties, as discovered by Johann Dobereiner

An arrangement by John Newlands that suggested properties of elements repeat in eights

Protons are added one by one to the nucleus, to "build up" the elements; electrons are similarly added to these atomic orbitals.

The lowest-energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals.

the electrons in the outermost principal quantum level of an atom

The inner electrons

A group of 14 elements corresponding to the 4f orbitals

A group of 14 elements corresponding to the 5f orbitals

The lanthanide and actinide series

Groups 1A-8A

An outer electron can "penetrate" the core electrons and "feel" more of the nuclear charge

The process by which inner electrons can protect outer electrons from partially feeling nuclear charge

The energy required to remove an electron from a gaseous electron or ion

The ionization energy of an atom is equal to the energy of the orbital from which it came

The energy change associated with the addition of an electron to a gaseous atom

Half the distance between atoms

Elements thta exhibit both metallic and nonmetallic properties