Chem Test 3

Front 1

electron configuration

Back 1

properties of an element are determined by this.

Front 2

valence electrons

Back 2

outer electrons of an atom and are the ones involved in chemical bonding

Front 3

valence electron configuration

Back 3

directly affects the properties of the atoms of the representative elements

Front 4

Representative elements

Back 4

elements in groups 1a - 7a. Have incompletely filled s or p subshells of the highest principal quantum number, n, for the period

Front 5

noble gases

Back 5

Group 8a elements. Except helium, they have a completely filled p shell. Not reactive bc the outer ns and np subshells are completely filled, a condition that represents great stability

Front 6

transition metals

Back 6

elements in groups 1b - 8b, which have incompletely filled d subshells or produce cations with incompletely filled d subshells

Front 7

group 2b elements

Back 7

neither representative elements nor transition metals and have no special name. their d subshell is completely filled

Front 8

Lanthanide and actinide series

Back 8

... of elements are sometimes called f block transition elements bc the f subshells are being filled

Front 9

cations

Back 9

one or more electrons are removed from the highest occupied n shell.

Front 10

cations

Back 10

from transition metals, electrons are removed from the ns orbital before the d orbital.

Front 11

anions

Back 11

one or more electrons are added to the highest partially filled n shell.

Front 12

isoelectronic

Back 12

atoms and ions have the same number of electrons and thus the same ground state electron configuration

Front 13

atomic radius

Back 13

within a period, it decreases from left to right

Front 14

atomic radius

Back 14

within a group, it increases from top to bottom

Front 15

ionic radius

Back 15

increase from the top to bottom of the periodic table within a group

Front 16

ionization energy

Back 16

minimum energy required to remove an electron from a gaseous atom in its ground state. measure of how tightly an electron is held in an atom.

Front 17

ionization

Back 17

is always an endothermic process

Front 18

succesive electron

Back 18

more energy is required to remove each...

Front 19

alkali metals

Back 19

have the lowest first ionization energies

Front 20

noble gases

Back 20

have the highest first ionization energies

Front 21

electron affinity

Back 21

measure of the tendency of an atom to gain an electron

Front 22

Halogens

Back 22

have the highest electron affinities

Front 23

diagonal relationships

Back 23

are similarities in the chemical properties of pairs of elements that are diagonal to each other in the periodic table

Front 24

metallic character

Back 24

of elements decreases across a period from metals through the metalloids to the non metals. It increases from top to bottom within a group of representative elements

Front 25

metallic oxides

Back 25

are usually basic, nonmetallic oxides are usually acidic, and oxides of intermediate elements tend to be amphoteric (display both acidic and basic properties)

Front 26

Planck

Back 26

discovered that atoms and molecules emit energy only in certain quantities called quanta

Front 27

quantum

Back 27

smallest quantity of energy that can be emitted or absorbed the the form of electromagnetic radiation

Front 28

E

Back 28

= hv

Front 29

wavelength

Back 29

(upside down y) distance between 2 identical points on successive waves

Front 30

frequency

Back 30

(v) number of waves that pass through one point in 1 second

Front 31

amplitude

Back 31

vertical distance from the maxiumum or minimum point of a wave to the midline

Front 32

velocity of a wave

Back 32

u, is the product of the wavelength and frequency

Front 33

velocity of an electromagnetic wave

Back 33

equal to c, the speed of light

Front 34

electromagnetic wave

Back 34

has an electric field component and magnetic field component, which have the same wavelength and frequency but travel in perpendicular planes

Front 35

visible light

Back 35

ranges from a wavelength of approx. 400 nm to 700 nm

Front 36

photoelectric effect

Back 36

Einstein figured this out, which is observed when electrons are ejected from the surface of certain metals exposed to a light of a certain threshold frequency. He proposed that a beam of light is composed of a stream of particles called photons. E= hv

Front 37

emission spectra

Back 37

atoms in the gas phase give a series of bright lines in different parts of the visible light range

Front 38

Bohr

Back 38

provided an explanation of the emission spectra of hydrogen atoms.

Front 39

ground state

Back 39

lowest (most stable) energy state of a system

Front 40

excited state

Back 40

higher energy state of a system that can be produced by putting radiant energy into an atom or molecule

Front 41

electrons

Back 41

exhibit properties of both particles and waves

Front 42

DeBroglie

Back 42

proposed that if an electron behaves like a standing wave in a hydrogen atom, the length of the wave must fit the circumference of the orbit exactly. Related the particle and wave properties of a substance using wavelength=h/mu

Front 43

heisenbergs uncertainty principle

Back 43

states that its impossible to know simultaneously the momentum p and position,x, of a particle with certainty

Front 44

Schrodinger

Back 44

formulated an equation to describe the behavior and energies of electrons in terms of a wave function. Wave function uses 4 quantum numbers to describe the distribution of electrons in an atom

Front 45

atomic orbital

Back 45

can be considered as the wave function of an electron in an atom

Front 46

principal quantum number

Back 46

n, identifies the shell of the orbital. can have values 0-4

Front 47

angular momentum number

Back 47

l, identifies the shape of the orbital. L can have values from 0 to (n-1)

Front 48

magnetic quantum number

Back 48

mL, identifies the orientation of the orbital. Value can range from
-L, (-L=1), 0, (+L-1), +L

Front 49

electron spin quantum number

Back 49

ms, identifies the direction of spin of electron. value is either +1/2 or -1/2

Front 50

atomic orbitals

Back 50

have diff shapes

Front 51

s orbitals

Back 51

2 electrons

Front 52

p orbitals

Back 52

6 electrons

Front 53

d orbitals

Back 53

10 electrons

Front 54

f orbitals

Back 54

14 electrons