Chem Chapter 7 Vocab

Front 1

radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum

Back 1

electromagnetic radiation

Front 2

the distance between two consecutive peaks or troughs in a wave

Back 2

wavelength

Front 3

the number of waves (cycles) per second that pass a given point in space

Back 3

Frequency

Front 4

the constant relating the change in energy for a system to the frequency of the electromagnetic radiation absorbed or emitted; equal to 6.626 x 10-34 J x s

Back 4

Planck’s constant

Front 5

the concept that energy can occur only in discrete units called quanta

Back 5

quantization

Front 6

a quantum of electromagnetic radiation

Back 6

photon

Front 7

Einstein’s equation proposing that energy has a mass; E is energy, m is mass, and c is the speed of light

Back 7

E=mc2

Front 8

the statement that light exhibits both wave and particle properties

Back 8

dual nature of light

Front 9

the scattering of light from a regular array of points or lines, producing constructive and destructive interference

Back 9

diffraction

Front 10

a spectrum that exhibits all the wavelengths of visible light

Back 10

continuous spectrum

Front 11

a spectrum showing only certain discrete wavelengths

Back 11

line spectrum

Front 12

the lowest possible energy state of an atom or molecule

Back 12

ground state

Front 13

a stationary wave as on a string of a musical instrument; in the wave mechanical model, the electron in the hydrogen atom is considered to be a standing wave

Back 13

standing wave

Front 14

a function of the coordinates of an electron’s position in three dimensional space that describes the properties of the electron

Back 14

wave function

Front 15

a specific wave function for an electron in an atom. The square of this function gives the probability distribution for the electron

Back 15

orbital

Front 16

a model for the hydrogen atom in which the electron is assumed to behave as a standing wave

Back 16

quantum (wave) mechanical model

Front 17

a principle stating that there is a fundamental limitation to how precisely both the position and momentum of a particle can be known at a given time

Back 17

Heisenberg uncertainty principle

Front 18

the square of the wave function indicating the probability of finding an electron at a particular point in space

Back 18

probability distribution

Front 19

the quantum number relating to the size and energy of an orbital; it can have any positive integer value

Back 19

principal quantum number (n)

Front 20

the quantum number relating to the shape of an atomic orbital, which can assume any integral value from 0 to n-1 for each value of n

Back 20

angular quantum number- (l)

Front 21

the quantum number relating to the orientation of an orbital in space relative to the other orbital with the same l quantum number. It can have integral values between l and -l, including zero

Back 21

magnetic quantum number (ml)

Front 22

a set of orbital with a given azimuthal quantum number

Back 22

subshell

Front 23

an area of an orbital having zero electron probability

Back 23

node

Front 24

a group of orbital with the same energy

Back 24

degenerate orbitals

Front 25

a quantum number representing one of the two possible values for the electron spin; either +½ or -½

Back 25

electron spin quantum number

Front 26

in a given atom no two electrons can have the same set of four quantum numbers

Back 26

Pauli exclusion principle

Front 27

atom with more than one electron

Back 27

polyelectronic atoms

Front 28

the principle stating that as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to hydrogen-like orbitals

Back 28

aufbau principle

Front 29

the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli exclusion principle in a particular set of degenerate orbital, with all unpaired electrons having parallel spins

Back 29

Hund’s rule

Front 30

the electrons in the outermost principal quantum level of an atom

Back 30

valence electrons

Front 31

inner electrons in an atom; one not in the outermost (valence) principal quantum level

Back 31

core electrons

Front 32

several series of elements in which inner orbital (d or f) are being filled

Back 32

transition metals

Front 33

a group of 14 elements following lanthanum in the periodic table, in which the 4f orbital are being filled

Back 33

lanthanide series

Front 34

a group of 14 elements following actinium in the periodic table, in which the 5f orbital are being filled

Back 34

actinide series

Front 35

elements in the groups labeled 1A, 2A, 3A, 4A, 5A, 6A, 7A, and 8A in the periodic table. The group number gives the sum of the valence s and p electrons

Back 35

main-group elements (representative elements)

Front 36

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

Back 36

electron affinity

Front 37

half the distance between the nuclei in a molecule consisting of identical atoms

Back 37

atomic radii

Front 38

elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties.

Back 38

metalloids (semimetals)

Front 39

inner electrons in an atom; one not in the outermost (valence) principal quantum level

Back 39

core electrons

Front 40

several series of elements in which inner orbital (d or f) are being filled

Back 40

transition metals

Front 41

a group of 14 elements following lanthanum in the periodic table, in which the 4f orbital are being filled

Back 41

lanthanide series

Front 42

a group of 14 elements following actinium in the periodic table, in which the 5f orbital are being filled

Back 42

actinide series

Front 43

elements in the groups labeled 1A, 2A, 3A, 4A, 5A, 6A, 7A, and 8A in the periodic table. The group number gives the sum of the valence s and p electrons

Back 43

main-group elements (representative elements)

Front 44

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

Back 44

electron affinity

Front 45

half the distance between the nuclei in a molecule consisting of identical atoms

Back 45

atomic radii

Front 46

elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties.

Back 46

metalloids (semimetals)