Chapter 5 Test

Front 1

one of the 14 elements with atomic numbers from 90 (thorium, Th) through 103(lawrencium, Lr)

Back 1

actinide

Front 2

one of the 14 elements with atomic numbers from 58 ( cerum) to 71 eutetium, li

Back 2

lanthanides

Front 3

the physical and chemical properties of the elements are periodic functions of their atomic numbers

Back 3

periodic law

Front 4

an arrangement of the elements in order of their atomic numbers so that elements with similar properties fal in the same column or group

Back 4

periodic table

Front 5

one of the elements of Group 1 of the periodic table ( lithium, sodium, potassium, rubidium , cesium, francium)

Back 5

alkali metals

Front 6

one of the elemnts of Groups 2 of the periodic table

Back 6

alkaline earth metals

Front 7

one of the elements of Group 17

Back 7

halogen

Front 8

an element in the sblock or p block

Back 8

main group elements

Front 9

one of the dblock elements that is a metal with typical metallic properties

Back 9

transition element

Front 10

a negative ion

Back 10

anion

Front 11

one half the distance between the nuclei of identical atoms that are bonded together

Back 11

atomic radiu

Front 12

a positive ion

Back 12

cation

Front 13

the energy change that occurs when an electron is acquired by a neutral atom

Back 13

electron affinity

Front 14

a measure of thee ability of an atom in a chemical compound to attract electrons

Back 14

electronegativity

Front 15

an atom of group of bonded atoms that have a positive or negative charge

Back 15

ion

Front 16

ionization

Back 16

the formation of ions from solute molecules by the action of the solvent; any process that results in the formation of anions

Front 17

ionization energy

Back 17

the energy required to remove an electron from a neutral atom of an elemetn

Front 18

valence electrons

Back 18

an electron that is available to be lost gained or shared in the formation of chemical compounds

Front 19

created a periodic table of the elemnts according to increasing atomic mass
- was able to predict the existnec of and prop of undiscovered eelements
-a few didn't fit in w/ the right group

Back 19

Dmitri Mendeleev

Front 20

arranged the periodic table according to increasing atomic number

Back 20

henry moseley

Front 21

the physical and chemical properties of the elemts are periodic functions of their atomic numbers

Back 21

periodic law

Front 22

an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column

Back 22

periodic table

Front 23

the veritcal columns of elements in the periodic table that have similar physical and chemical properties

Back 23

group(family)

Front 24

the horizontal rows of elements in the periodic table that have the same number of principal energy levels

Back 24

period

Front 25

period length (row) is determined by ___

Back 25

electron configuration

Front 26

number of electrons per period

Back 26

2, 8, 8, 18, 18, 32, 23

Front 27

metlas found in groups 1 and 2

Back 27

s block

Front 28

silvery appearance, soft, 1 e- in outer s orbital, extremely reactive

Back 28

alkali metals

Front 29

2e- in outer s orharder denser and stronger than alkali metals, reactive but less than group 1

Back 29

alkaline earth metals

Front 30

unique properties, sometimes included iwth the group 1e- in 1s level, has nonmetal properties does not act like group 1, not part of sblock

Back 30

hydrogen

Front 31

found in group 18 rather than 2 because it is stable,
not part of s or p block
is a noble gas

Back 31

helium

Front 32

d orbitals filled
transition metals( malleable and ductile)
typical metallic properties
less reactive

Back 32

d block 3-12

Front 33

p orbitals filled
wide variety of properties

Back 33

p block 13-18

Front 34

most reactive nonmetals
react vigorously with metlas to produce salts

Back 34

halogens 17

Front 35

least reactive of all elements
fill highest main energy level

Back 35

noble gases 18

Front 36

p block together with s block elements

Back 36

main group elements

Front 37

lanthanides and actinides
f orbitals filling

Back 37

f block

Front 38

decrease because higher energy levels put electrons further from the pull of the nucleus

Back 38

group trend

Front 39

negative ions, nonmetals
gain e-

Back 39

high ionization enrgy

Front 40

positive ions, metals
give e-

Back 40

low ionizations metals

Front 41

the enrgy change that occurs when an electron is acquired by a neutral atom

Back 41

electron affinity

Front 42

A+ e- ----> A- + energy

Back 42

exothermic (release)

Front 43

A+ e- + energy ---> A-

Back 43

endothermic ( absorb)

Front 44

period trend/group trend of electron affinity

Back 44

increase because of increasing nuclear charge- period trend
generally decrease- group trend

Front 45

measure of the ability of an atom in a chemical compound to attract electrons

Back 45

electronegativity
periodic trend- increase
group trend - decrease

Front 46

cation

Back 46

positive ions lose e-

Front 47

anion

Back 47

negative ions gain e-

Front 48

ionic radii perio and group trend

Back 48

periodic trend- metals decrease, previous energy level
non metals- larger radii but decrease, grater charge
group trend increases