unit 6 - periodic table

Question 1

father of periodic table

Answer 1

Mendeleev

Question 2

why do elements in a group have similar chemical properties

Answer 2

same # of valence electrons

Question 3

atomic number

Answer 3

number of protons (nuclear charge)

Question 4

periodic table is arranged according to what

Answer 4

atomic number

Question 5

as you move down a group, atomic number…

Answer 5

increases

Question 6

atomic radius

Answer 6

distance between the nucleus and farthest electron

Question 7

what is the atomic radius group trend

Answer 7

atomic radius increases as you go down the group

Question 8

why does the atomic radius increase as you go down a group

Answer 8

more occupied principal energy levels, creates a greater distance between the atom’s nucleus and its furthest electron

Question 9

first ionization energy

Answer 9

the amount of energy needed to remove the most loosely bound electron from the valence shell

(measures how easy/hard an atom loses electrons)

Question 10

IE trend of a group

Answer 10

decreases as you go down a group

Question 11

why does IE decrease as you go down a group

Answer 11

atoms with a larger radius have valence electrons that are farther away from their nucleus, so its easier to lose electrons

Question 12

electronegativity

Answer 12

a measure of the attraction of a nucleus of one atom for another atom’s valence electrons

Question 13

EN group trend

Answer 13

decreases as you go down the group

Question 14

why does EN decrease as you go down a group

Answer 14

atoms with a BIG RADIUS, have a LOW EN. attraction for another atom’s electrons decreases with more occupied rings, because its nucleus is further from another atom’s valence shell

Question 15

metallic property

Answer 15

measure of how easily an element loses electrons

Question 16

trend of metallic property in groups

Answer 16

the metallic property increases as you go down the group; lose electrons easily

Question 17

why do metallic properties increase as you move down a group

Answer 17

elements on the bottom of the group have Low I.E. and Low E.N. so they lose electrons very easily/react easily

Question 18

group 1 is called

Answer 18

alkalai metals

Question 19

characteristics of alkalai metals

Answer 19

• extremely active
• form strong bases

Question 20

group 2 is called

Answer 20

alkaline earth metals

Question 21

characteristics of alkaline earth metals

Answer 21

• very active; but not as much as the alkalai metals

Question 22

properties of groups 1 & 2

Answer 22

• found only in compounds in nature
• are the most active metals on the periodic table
• lose electrons easily (low IE & EN)
• form only ionic compounds
• from stable compounds (hard to decompose)
• group 1 elements are more active than group 2

Question 23

group 3 to 12 (transition metals)

Answer 23

• have multiple oxidation states
• can form compounds which have colored ions inwater
• some transition elements are found commonly in the elemental form nature
• Hg (Mercury) only metal - liquid at room temperature

Question 24

group 13 - boron’s family

Answer 24

boron is metalloid, rest are metal

Question 25

group 14 - carbon's family

Answer 25

C - non metal Si & Ge - metalloid Sn & Pb - metal

Question 26

group 15 - nitrogen's family

Answer 26

N & P - nonmetal As & Sb - metalloid Bi - metal nitrogen is gas, rest solid

Question 27

group 16 - oxygen's family

Answer 27

O, S, Se - nonmetal Te - metalloid Po - metal oxygen is gas, rest solid

Question 28

group 17 - halogens

Answer 28

- ALL halogens have 7 valence electrons (gain 1 electron to become -1 ions) F - gas Cl - gas Br - liquid at room temp I - solid At - solid

Question 29

properties of groups 15, 16, and 17

Answer 29

- high electronegativity (gain another atom's electrons easily) - high ionization energy (do not lose their electrons easily)

Question 30

group 18 - noble gases

Answer 30

- all are non metals and gases at room temp - DO NOT react with other elements because they have filled/stable outer shell **8 valence electrons = full shell (except He)

Question 31

characteristics of a period

Answer 31

elements in the same period: - number of occupied PEL's is same

Question 32

as one move --> across a period, atomic number

Answer 32

increases

Question 33

as one move --> across a period, number of valence electrons

Answer 33

increases

Question 34

as one move --> across a period, atomic radius

Answer 34

decreases because energy levels are kept closer to the nucleus, because of a greater nuclear charge - more protons pull electrons closer to the nucleus and atomic radius decreases

Question 35

as one move --> across a period, ionization energy

Answer 35

increases, takes more energy to remove electrons from nonmetals (right) than metals (left) **nonmetals are more attracted to their electrons

Question 36

why does IE increase as you move across a period

Answer 36

greater nuclear charge; electrons are held closer to the nucleus due to a smaller radius

Question 37

as one move --> across a period, electronegativity

Answer 37

increases, the attraction for another atom's electrons increases ***atomic radius decreases; atom's nucleus is closer to another atom's valence electrons

Question 38

why does EN increase as you move across a period

Answer 38

greater nuclear charge, distance between that atom's nucleus and another atom's electrons decreases

Question 39

what percent of all elements are metals

Answer 39

75% of all elements are Metals

Question 40

where are most active metals found

Answer 40

lower left of the table (Francium)

Question 41

properties of metals

Answer 41

- have luster (shine); mobile electrons - ductile: can be drawn into a wire - malleable: can be hammered into shape - good conductor of heat and electricity - all are solids at room temp, except Hg (liquid) - lose electrons become (+) ions - low IE and low EN

Question 42

compare ionic radius and atomic radius of a metal

Answer 42

ionic radius is smaller than atomic radius

Question 43

what is the most reactive metal

Answer 43

Francium (Fr)

Question 44

properties of nonmetals

Answer 44

- found on the right of the staircase - most are gases; some are solids - Br is the only liquid nonmetal - I is a solid nonmetal at room temp - F is the most reactive nonmetal - lack luster; have a dull surface - not malleable or ductile, tend to be brittle - poor conductors of electricity or heat - nonmetals gain electrons become (-) ions

Question 45

what's the most reactive non-metal

Answer 45

F or Fluorine

Question 46

compare the ionic radius and atomic radius of nonmetals

Answer 46

ionic radius is larger than atomic radius

Question 47

properties of metalloids (semi-metals)

Answer 47

- elements at the staircase between the metals and nonmetals - have some properties of both ex: malleable, bad conductors - 6 metalloids to know: B, Si, As, Te, Ge, Sb

Question 48

highest EN

Answer 48

Fluorine

Question 49

highest IE

Answer 49

Helium