Chapter 6

orbital

A region of space around the nucleus where an electron is likely to be found.

amplitude

Amplitude is the displacement of a wave from zero. The maximum amplitude for a wave is the height of a peak or the depth of a trough, relative to the zero displacement line.

Pauli Exclusion Principle

An atomic orbital may describe at most two electrons, each with opposite spin direction

valence shell

Outermost electron shell

wavelength / energy relationship

Simple answer: as the wavelength gets shorter, the energy increases; as the wavelength gets longer, the energy decreases.

Electromagnetic spectrum

The electromagnetic spectrum encompasses a continuous range of frequencies or wavelengths of electromagnetic radiation, ranging from long wavelength, low energy radio waves to short wavelength, high frequency, high-energy gamma rays. The electromagnetic spectrum is traditionally divided into regions of radio waves, microwaves, infrared radiation, visible light, ultraviolet rays, x rays, and gamma rays.

emission

The emission spectrum of a chemical element or chemical compound is the spectrum of frequencies of electromagnetic radiation emitted due to an atom or molecule making a transition from a high energy state to a lower energy state.

wave/particle duality

Wave-particle duality is the fact that every elementary particle or quantic entity exhibits the properties of not only particles, but also waves. It addresses the inability of the classical concepts "particle" or "wave" to fully describe the behavior of quantum-scale objects.

speed of light

a fundamental physical constant that is the speed at which electromagnetic radiation propagates in a vacuum and that has a value fixed by international convention of 299,792,458 meters per second —symbol c.

excited state

a higher energy state than ground state

Hunds Rule

all sub shells must have at least 1 e- in each orbital before placing another e- and filling

white light

apparently colorless light, for example ordinary daylight. It contains all the wavelengths of the visible spectrum at equal intensity.

Heisenberg Uncertainty Principle

it is impossible to know exactly both the velocity and the position of a particle at the same time

quantum numbers

n, l, ml, ms specify the properties of atomic orbitals and the properties of electrons in orbitals

node

point in the atom where the electron density is zero.

orbital shapes

s,p,d,f sub shells are the orbital shape

Beers Law

solution's absorbance of light at a certain wavelength is directly proportional to the concentration of that solution. Beer s Law is mathematically expressed as M1/A1=M2/A2.

ground state

the lowest energy or most stable state

frequency

the number of times per second that one complete awe passes at a given point

valence electrons

the outermost electrons in an orbital

photon

the smallest increment of radiant energy. a photon of light with a frequency "v" has an energy equal to "hv"

absorption

(physics) the process in which incident radiated energy is retained without reflection or transmission on passing through a medium

Electromagnetic radiation

(radiant energy) a form of energy that has wave characteristics and that propagates through a vacuum at the characteristic speed of 3.00 x 10^8 m/s

Bohr Theory and terms shell

Danish physicist (1885-1962) who studied atomic structure and radiations; created a new atomic model; described electrons as moving around the nucleus in fixed orbits and having a set amount of energy

wavelength / frequency relationship

The wavelength and frequency of light are closely related. The higher the frequency, the shorter the wavelength. Because all light waves move through a vacuum at the same speed, the number of wave crests passing by a given point in one second depends on the wavelength.

line spectrum

a spectrum that contains radiation at only specific wavelengths

Schroedinger

- Quantum Mechanical Model of Atom - uses probability in determining the location of electron

Planck

Max Planck, FRS (April 23, 1858 - October 4, 1947) was a German theoretical physicist who originated quantum theory, which won him the Nobel Prize in Physics in 1918.

frequency / energy relationship

The greater the energy, the larger the frequency and the shorter (smaller) the wavelength. Given the relationship between wavelength and frequency — the higher the frequency, the shorter the wavelength — it follows that short wavelengths are more energetic than long wavelengths.

wavelength

the distance between identical point on successive waves

quantized

to apply quantum theory to, especially form into quanta, in particular restrict the number of possible values of (a quantity) or states of (a system) so that certain variables can assume only certain discrete magnitudes.