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chemistry > unit 6 - periodic table > Flashcards

unit 6 - periodic table Flashcards

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1
Q

father of periodic table

A

Mendeleev

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2
Q

why do elements in a group have similar chemical properties

A

same # of valence electrons

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3
Q

atomic number

A

number of protons (nuclear charge)

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4
Q

periodic table is arranged according to what

A

atomic number

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5
Q

as you move down a group, atomic number…

A

increases

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6
Q

atomic radius

A

distance between the nucleus and farthest electron

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7
Q

what is the atomic radius group trend

A

atomic radius increases as you go down the group

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8
Q

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

A

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

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9
Q

first ionization energy

A

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

(measures how easy/hard an atom loses electrons)

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10
Q

IE trend of a group

A

decreases as you go down a group

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11
Q

why does IE decrease as you go down a group

A

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

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12
Q

electronegativity

A

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

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13
Q

EN group trend

A

decreases as you go down the group

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14
Q

why does EN decrease as you go down a group

A

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

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15
Q

metallic property

A

measure of how easily an element loses electrons

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16
Q

trend of metallic property in groups

A

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

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17
Q

why do metallic properties increase as you move down a group

A

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

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18
Q

group 1 is called

A

alkalai metals

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19
Q

characteristics of alkalai metals

A
  • extremely active
  • form strong bases
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20
Q

group 2 is called

A

alkaline earth metals

21
Q

characteristics of alkaline earth metals

A
  • very active; but not as much as the alkalai metals
22
Q

properties of groups 1 & 2

A
  • 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
23
Q

group 3 to 12 (transition metals)

A
  • 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
24
Q

group 13 - boron’s family

A

boron is metalloid, rest are metal

25
Q

group 14 - carbon’s family

A

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

26
Q

group 15 - nitrogen’s family

A

N & P - nonmetal
As & Sb - metalloid
Bi - metal

nitrogen is gas, rest solid

27
Q

group 16 - oxygen’s family

A

O, S, Se - nonmetal
Te - metalloid
Po - metal

oxygen is gas, rest solid

28
Q

group 17 - halogens

A
  • 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

29
Q

properties of groups 15, 16, and 17

A
  • high electronegativity (gain another atom’s electrons easily)
  • high ionization energy (do not lose their electrons easily)
30
Q

group 18 - noble gases

A
  • 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)
31
Q

characteristics of a period

A

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

32
Q

as one move –> across a period, atomic number

A

increases

33
Q

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

A

increases

34
Q

as one move –> across a period, atomic radius

A

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

35
Q

as one move –> across a period, ionization energy

A

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

36
Q

why does IE increase as you move across a period

A

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

37
Q

as one move –> across a period, electronegativity

A

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

38
Q

why does EN increase as you move across a period

A

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

39
Q

what percent of all elements are metals

A

75% of all elements are Metals

40
Q

where are most active metals found

A

lower left of the table (Francium)

41
Q

properties of metals

A
  • 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
42
Q

compare ionic radius and atomic radius of a metal

A

ionic radius is smaller than atomic radius

43
Q

what is the most reactive metal

A

Francium (Fr)

44
Q

properties of nonmetals

A
  • 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
45
Q

what’s the most reactive non-metal

A

F or Fluorine

46
Q

compare the ionic radius and atomic radius of nonmetals

A

ionic radius is larger than atomic radius

47
Q

properties of metalloids (semi-metals)

A
  • 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
48
Q

highest EN

A

Fluorine

49
Q

highest IE

A

Helium

chemistry (11 decks)

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