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pre ap chemistry 1 > test 6 the periodic table > Flashcards

test 6 the periodic table Flashcards

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1
Q

Mendeleev

A

father of periodic table

arranged elements according to atomic mass

noticed pattern in the properties of elements

had gaps in his periodic table

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2
Q

Moseley

A

1909

arranged the elements according to increasing atomic number and gaps disappeared

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3
Q

period

A

a horizontal row, there are 7, each ends with a noble gas

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4
Q

what does each period number indicate

A

number of occupied energy levels

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5
Q

group

A

vertical column

also called families

8 with Roman numerals and 18 with numbers

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6
Q

elements in a group have

A

similar chemical properties

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7
Q

group number indicates

A

the number of valence electrons

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8
Q

group IA is

A

alkali metals

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9
Q

group IIA is

A

alkaline metals

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10
Q

group IIIA is

A

Boron group

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11
Q

group IVA is

A

carbon group

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12
Q

group VA is

A

Nitrogen group

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13
Q

group VIIA is

A

Halogens

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14
Q

group VIIIA is

A

Noble Gases

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15
Q

group number indicates

A

number of valence electrons

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16
Q

maximum nmber of valence electrons

A

8

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17
Q

helium has how many VE

A

2 valence electrons

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18
Q

main-group elements are also called

A

representative elements

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19
Q

main-group elements include groups

A

1,2, 13-18

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20
Q

main group elements…

A

lose or gain electrons in the outer energy level

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21
Q

alkali metals

A

group 1, has 1 valence electron, loses 1 valence electron so they have a 1+ charge

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22
Q

most reactive metals

A

alkali metals because it takes less energy to lose one electron

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23
Q

alkaline metals

A

group 1, has 2 valence electrons, loses 2 valence electrons to have a 2+ charge

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24
Q

alkaline metals are less

A

alkaline metals are less reactive than alkali metals because it takes more energy to lose 2 electrons

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25
Q

halogens

A

group 17 or VIIA, has 7 valence electrons, gains 1 valence electron so they have a 1- charge

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26
Q

halogens react with ___ to form ___

A

alkali metals to form salts

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27
Q

most reactive non metals

A

halogens are because it takes less energy to gain 1 electron

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28
Q

nobles gases

A

group 18, all noble gases except helium have 2 valence electrons, low reactivity because outer energy level is full

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29
Q

hydrogen

A

reacts with many elements because it has 1 valence electron

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30
Q

hydrogen is sometimes placed

A

is group 1 or 17 because it loses and gains 1 electron, sometimes placed at top center

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31
Q

hydrogen is…

A

flammable

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32
Q

transition metals

A

groups 3-12, form colorful compounds

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33
Q

transition metals are…

A

less reactive than groups IA and IIA because they are multivalent

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34
Q

what does it mean that inner transition metals are multivalent

A

they can lose 1,2, or 3 electrons to have charges of 1+, 2+ or 3+

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35
Q

inner transition metals also called

A

rare earth elements

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36
Q

inner transition metals are

A

the two rows at the bottom of periodic table to keep narrow

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37
Q

lanthanides

A

first row of inner transition metals, named after lanthanum

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38
Q

actinides

A

second row of inner transition metals, named after actinium

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39
Q

actinides are

A

radioactive because their nucleus is unstable

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40
Q

synthetic element

A

man-made element

41
Q

what are the synthetic elements

A

93-118

42
Q

the staircase

A

B, Si, As, Te, Ge, Sb

43
Q

metalloids

A

elements that border the staircase, have properties of metals and nonmetals

44
Q

what are the metals

A

on the left side of the staircase, including the inner transition metals, most elements

45
Q

characteristic of metals

A
  • most are solids except Hg
  • conductors
  • ductile
  • malleable
  • have luster
46
Q

metals form…

A

positive ions by losing electrons

47
Q

metals react with

A

nonmetals

48
Q

where are non metals `

A

on the right side of the staircase, including hydrogen

49
Q

characteristics of nonmetals

A
  • solids, liquids and gases
  • insulators
  • not ductile
  • brittle
  • dull
50
Q

nonmetals form

A

negative ions by gaining electrons

51
Q

nonmetals react with

A

metals OR nonmetals

52
Q

what are diatomic elements

A

elements that exist as 2 atoms in nature

can be written with subscript 2 like 02

53
Q

name the diatomic elements

A

H, N, O, F, Cl, Br, I

54
Q

energy level

A

abbreviated n, also called shell, found in the electron cloud

55
Q

n=1 is also called

A

shell K

56
Q

n=2 is also called

A

shell L

57
Q

n=3 is also called

A

shell M

58
Q

n=4 is also called

A

shell N

59
Q

sublevel

A

found in an energy level, holds orbitals

60
Q

orbital

A

found in a sublevel and can hold a max of 2 electrons

61
Q

sublevels

A

s,p,d,f

62
Q

s sublevel

A

1 orbital, 2 electrons, groups 1,2 and He

63
Q

p sublevel

A

3 orbitals, 6 electrons, groups 13-18

64
Q

d sublevel

A

5 orbitals, 10 electrons, groups 3-12

65
Q

f sublevel

A

7 orbitals, 14 electrons, lanthanides and actinides

66
Q

aufbau principle

A

electrons fill orbitals from low energy to high energy

67
Q

pauli exclusion principle

A

no more than 2 electrons in an orbital, electrons have opposite spin

68
Q

Hund’s Rule

A

unpaired electrons have parallel spins

69
Q

electron configuration

A

shows distribution of electrons within sublevels

70
Q

periodic trend

A

pattern based on the location of an element on the periodic table

71
Q

shielding

A

when inner electron block protons from pulling electrons close to the nucleus

72
Q

radius

A

the size of an atom or ion measured from half the nucleus to the outermost electron

73
Q

atomic radius

A

increases from right to left

increases down

74
Q

why does atomic radius increase from right to left

A

because nuclear charge decreases so protons cannot pull electrons close to the nucleus

75
Q

why does atomic radius increase down

A

because energy levels are added so inner electrons shield protons from pulling electrons close to the nucleus

76
Q

ionic radius

A

increases from right to left

increases down

77
Q

why does ionic radius increase from right to left

A

because nuclear charge decreases so protons cannot pull electrons close to the nucleus

78
Q

why does ionic radius increase down

A

because energy levels are added so inner electrons shield protons from pulling electrons close to the nucleus

79
Q

a cation is ___ than its parent atom

A

smaller

80
Q

why is a cation smaller than its parent atom

A

because a cation loses electrons so there are more protons to pull electrons close to the nucleus

81
Q

an anion is ___ than its parent atom

A

larger because an anion gains electrons so there a not enough protons to pull electrons close to the nucleus

82
Q

electronegativity defnition

A

ability of an atom to gain an electron

83
Q

most electronegative element

A

F

84
Q

electronegativity

A

increases from left to right

increases up

85
Q

why does electronegativity increase from left to right

A

because nuclear charge increase so protons pull electrons close to the nucleus

86
Q

why does electronegativity increase up

A

because energy levels decrease so there are not enough inner electrons to shield protons from pulling electrons close to the nucleus

87
Q

ionization energy definition

A

energy needed to remove an electron

88
Q

ionization energy

A

increases from left to right

increases up

89
Q

why does ionization energy increase from left to right

A

because nuclear charge increases so protons pull electrons close to the nucleus making it harder to remove an electron

90
Q

why does ionization energy increase up

A

because energy levels decrease so there are not enough inner electrons to shield protons from pulling electrons close to the nucleus making it harder to remove an electron

91
Q

metal reactivity means

A

metals lose electrons

92
Q

metal reactivity

A

increases from right to left

increases down

93
Q

why does metal reactivity increase from right to left

A

because nuclear charge decreases so protons can not pull electron close to the nucleus making it easier to lose an electron

94
Q

why does metal reactivity increase down

A

because energy levels are added so electrons shield protons from pulling electrons close to the nucleus making it easier to remove an electron

95
Q

nonmetal reactivity means

A

nonmetals gain electrons

96
Q

nonmetal reactivity

A

increases from left to right

increases up

97
Q

why does nonmetal reactivity increase from left to right

A

nuclear charge increases so protons pull electrons close to the nucleus

98
Q

why does nonmetal reactivity increase up

A

because energy levels are decrease so there are not enough inner electrons to shield protons from pulling electrons close to the nucleus

pre ap chemistry 1 (12 decks)

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