Chapter 5 Vocab

Front 1

Atomic Absorption Spectrum

Back 1

A band of light with bits missing out of it

Front 2

Amplitude

Back 2

the maximum deviation of an alternating current from its average value.

Front 3

Atomic Emission Spectrum

Back 3

a measurement of the intensity of every frequency of electromagnetic radiation that an element's atoms or a compound's molecules give off, when the atoms or molecules are at their lowest energy levels.

Front 4

Atomic Orbital

Back 4

a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom.

Front 5

Aufbau Principle

Back 5

is used to determine the electron configuration of an atom, molecule or ion.

Front 6

De Broglie Equation

Back 6

an equation used to describe the wave properties of matter, specifically, the wave nature of the electron:

Ex: λ = h/mv
where λ is wavelength, h is Planck's constant, m is the mass of a particle, moving at a velocity v

Front 7

Electromagnetic Radiation

Back 7

radiation consisting of electromagnetic waves, including radio waves, infrared, visible light, ultraviolet, x-rays, and gamma rays.

Front 8

Electromagnetic Spectrum

Back 8

the entire spectrum, considered as a continuum, of all kinds of electric, magnetic, and visible radiation, from gamma rays having a wavelength of 0.001 angstrom to long waves having a wavelength of more than 1 million km.

Front 9

Electron Configuration

Back 9

the composition of atoms in different elements

Front 10

Electron-Dot Structure

Back 10

valence electrons are represented by dots placed around the chemical symbol.

Front 11

Energy

Back 11

any source of usable power, as fossil fuel, electricity, or solar radiation.

Front 12

Energy Sublevel

Back 12

The energy level that it is at

Front 13

Frequency

Back 13

the number of cycles or completed alternations per unit time of a wave or oscillation.

Front 14

Ground State

Back 14

the state of least energy of a particle, as an atom, or of a system of particles.

Front 15

Heisenberg Uncertainty Principle

Back 15

the principle of quantum mechanics, formulated by Heisenberg, that the accurate measurement of one of two related, observable quantities, as position and momentum or energy and time, produces uncertainties in the measurement of the other, such that the product of the uncertainties of both quantities is equal to or greater than h/ 2 π, where h equals Planck's constant.

Front 16

Hund's Rule

Back 16

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Front 17

Orbital

Back 17

The region of space where there is a significant probability of finding a particular electron

Front 18

Orbital Notation

Back 18

a way to show how many electrons are in an orbital for a given element.

Front 19

Pauli Exclusion Principle

Back 19

the principle that in any system described by quantum mechanics no two identical particles having spin equal to half an odd integer can be in the same quantum state: first postulated for the electrons in atoms.

Front 20

Photoelectric Effect

Back 20

the phenomenon in which the absorption of electromagnetic radiation, as light, of sufficiently high frequency by a surface, usually metallic, induces the emission of electrons from the surface.

Front 21

Photon

Back 21

a quantum of electromagnetic radiation, usually considered as an elementary particle that is its own antiparticle and that has zero rest mass and charge and a spin of one.

Front 22

Planck's Constant

Back 22

the fundamental constant of quantum mechanics, expressing the ratio of the energy of one quantum of radiation to the frequency of the radiation and approximately equal to 6.624 × 10− 27 erg-seconds.

Front 23

Principle Energy Level

Back 23

The energy level denoted by the principal quantum number n. The first element in a period of the Periodic Table introduces a new principal energy level.

Front 24

Quantum

Back 24

the smallest quantity of radiant energy, equal to Planck's constant times the frequency of the associated radiation.

Front 25

Quantum Mechanical Model

Back 25

based on quantum mechanics (mathematical solutions of theoretical equations) quantum numbers are quantum solutions to quantum equations and are used to find the probable position and location of an electron in an atom

Front 26

Slater's Diagonal Rule

Back 26

the 1s sublevel has the lowest energy. So, hydrogen's electron configuration will be 1s1. Helium's two electrons are shown as 1s2. Now the first energy level is full and lithium's third (outer) electron will inhabit the 2s sublevel and is shown as 1s22s1. An observer will notice that the 4s sublevel will begin to fill before the 3d sublevel. Here is the electron configuration for scandium: 1s22s22p63s23p64s23d1.

Front 27

Valence Electron

Back 27

an electron of an atom, located in the outermost shell (valence shell) of the atom, that can be transferred to or shared with another atom.

Front 28

Wavelength

Back 28

the distance, measured in the direction of propagation of a wave, between two successive points in the wave that are characterized by the same phase of oscillation.