Chemistry Chapter 4

Front 1

Electromagnetic radiation

Back 1

a form of energy that exhibits wavelike behavior as it travels through space. C=v

Front 2

Electromagnetic spectrum-

Back 2

all forms of electromagnetic radiation

Front 3

Wavelength

Back 3

() distance between corresponding points an adjacent wavelengths.

Front 4

Frequency

Back 4

Number of waves that pass a given point in a specific time,usually 1 second

Front 5

Photoelectric effect

Back 5

emission of electrons from a metal when light shines on the metal

Front 6

Quantum

Back 6

minimum quantity of energy that can be lost or gained by an atom

Front 7

Photon

Back 7

particle ofelectomagnetic radiation having zero mess and carrying a quantum of energy

Front 8

Ground state

Back 8

lowest energy state of an atom

Front 9

Excited state

Back 9

a state in which an atom has a higher potential energy than it has in its ground state

Front 10

Emission line spectrum

Back 10

diagram or graph that indicates the degree to which a substance emits radiant energy with respect to wavelength

Front 11

Continuous spectrum

Back 11

emission of a continuous range of frequencies of electromagnetic radiation

Front 12

Diffraction

Back 12

bending of a wave as it passes by the edge of an object or through a small opening

Front 13

Interference

Back 13

occurs when waves overlap

Front 14

Heisenberg uncertainty principle

Back 14

states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle

Front 15

Quantum theory

Back 15

describes mathematically the wave properties of electrons and other very small particles

Front 16

Orbital

Back 16

three dimensional region around the nucleus that indicates the probably location of an electron

Front 17

Quantum numbers

Back 17

specify the properties of atomic orbitals and the properties of electrons in orbitals

Front 18

principal quantum number

Back 18

indicates main energy level occupied by the electron

Front 19

angular momentum quantum number

Back 19

indicates shape of the orbital

Front 20

Magnetic quantum number

Back 20

indicates the orientation of an orbital around the nucleus

Front 21

Spin quantum number

Back 21

has only 2 possible values (+1/2, -1/2) which indicate the 2 fundamental spin sates of an electron in an orbital

Front 22

electron configuration

Back 22

arrangement of electrons in an atom

Front 23

Ground state electron configuration

Back 23

lowest energy arrangement of the electrons for each element

Front 24

Aufbau principle

Back 24

an electron occupies the lowest energy orbital that can receive it

Front 25

Pauli exclusion principle

Back 25

no 2 electrons in the same atom can have the same set of 4 quantum numbers

Front 26

Hund's rule

Back 26

orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals much has the same spin state

Front 27

Highest occupied energy level

Back 27

electron containing main energy level with the highest principal quantum number

Front 28

Inner shell electrons

Back 28

electrons that are not in the highest occupied energy level

Front 29

Noble gases

Back 29

group 18 elements (helium, neon, argon, krypton, xenon, and radon)

Front 30

Noble gas configuration

Back 30

refers to an outer main energy level occupied, in most cases by 8 electrons