test 6 the periodic table Flashcards
(98 cards)
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
2
Q
Moseley
A
1909
arranged the elements according to increasing atomic number and gaps disappeared
3
Q
period
A
a horizontal row, there are 7, each ends with a noble gas
4
Q
what does each period number indicate
A
number of occupied energy levels
5
Q
group
A
vertical column
also called families
8 with Roman numerals and 18 with numbers
6
Q
elements in a group have
A
similar chemical properties
7
Q
group number indicates
A
the number of valence electrons
8
Q
group IA is
A
alkali metals
9
Q
group IIA is
A
alkaline metals
10
Q
group IIIA is
A
Boron group
11
Q
group IVA is
A
carbon group
12
Q
group VA is
A
Nitrogen group
13
Q
group VIIA is
A
Halogens
14
Q
group VIIIA is
A
Noble Gases
15
Q
group number indicates
A
number of valence electrons
16
Q
maximum nmber of valence electrons
A
8
17
Q
helium has how many VE
A
2 valence electrons
18
Q
main-group elements are also called
A
representative elements
19
Q
main-group elements include groups
A
1,2, 13-18
20
Q
main group elements…
A
lose or gain electrons in the outer energy level
21
Q
alkali metals
A
group 1, has 1 valence electron, loses 1 valence electron so they have a 1+ charge
22
Q
most reactive metals
A
alkali metals because it takes less energy to lose one electron
23
Q
alkaline metals
A
group 1, has 2 valence electrons, loses 2 valence electrons to have a 2+ charge
24
Q
alkaline metals are less
A
alkaline metals are less reactive than alkali metals because it takes more energy to lose 2 electrons
25
halogens
group 17 or VIIA, has 7 valence electrons, gains 1 valence electron so they have a 1- charge
26
halogens react with ___ to form ___
alkali metals to form salts
27
most reactive non metals
halogens are because it takes less energy to gain 1 electron
28
nobles gases
group 18, all noble gases except helium have 2 valence electrons, low reactivity because outer energy level is full
29
hydrogen
reacts with many elements because it has 1 valence electron
30
hydrogen is sometimes placed
is group 1 or 17 because it loses and gains 1 electron, sometimes placed at top center
31
hydrogen is...
flammable
32
transition metals
groups 3-12, form colorful compounds
33
transition metals are...
less reactive than groups IA and IIA because they are multivalent
34
what does it mean that inner transition metals are multivalent
they can lose 1,2, or 3 electrons to have charges of 1+, 2+ or 3+
35
inner transition metals also called
rare earth elements
36
inner transition metals are
the two rows at the bottom of periodic table to keep narrow
37
lanthanides
first row of inner transition metals, named after lanthanum
38
actinides
second row of inner transition metals, named after actinium
39
actinides are
radioactive because their nucleus is unstable
40
synthetic element
man-made element
41
what are the synthetic elements
93-118
42
the staircase
B, Si, As, Te, Ge, Sb
43
metalloids
elements that border the staircase, have properties of metals and nonmetals
44
what are the metals
on the left side of the staircase, including the inner transition metals, most elements
45
characteristic of metals
- most are solids except Hg
- conductors
- ductile
- malleable
- have luster
46
metals form...
positive ions by losing electrons
47
metals react with
nonmetals
48
where are non metals `
on the right side of the staircase, including hydrogen
49
characteristics of nonmetals
- solids, liquids and gases
- insulators
- not ductile
- brittle
- dull
50
nonmetals form
negative ions by gaining electrons
51
nonmetals react with
metals OR nonmetals
52
what are diatomic elements
elements that exist as 2 atoms in nature
can be written with subscript 2 like 02
53
name the diatomic elements
H, N, O, F, Cl, Br, I
54
energy level
abbreviated n, also called shell, found in the electron cloud
55
n=1 is also called
shell K
56
n=2 is also called
shell L
57
n=3 is also called
shell M
58
n=4 is also called
shell N
59
sublevel
found in an energy level, holds orbitals
60
orbital
found in a sublevel and can hold a max of 2 electrons
61
sublevels
s,p,d,f
62
s sublevel
1 orbital, 2 electrons, groups 1,2 and He
63
p sublevel
3 orbitals, 6 electrons, groups 13-18
64
d sublevel
5 orbitals, 10 electrons, groups 3-12
65
f sublevel
7 orbitals, 14 electrons, lanthanides and actinides
66
aufbau principle
electrons fill orbitals from low energy to high energy
67
pauli exclusion principle
no more than 2 electrons in an orbital, electrons have opposite spin
68
Hund's Rule
unpaired electrons have parallel spins
69
electron configuration
shows distribution of electrons within sublevels
70
periodic trend
pattern based on the location of an element on the periodic table
71
shielding
when inner electron block protons from pulling electrons close to the nucleus
72
radius
the size of an atom or ion measured from half the nucleus to the outermost electron
73
atomic radius
increases from right to left
increases down
74
why does atomic radius increase from right to left
because nuclear charge decreases so protons cannot pull electrons close to the nucleus
75
why does atomic radius increase down
because energy levels are added so inner electrons shield protons from pulling electrons close to the nucleus
76
ionic radius
increases from right to left
increases down
77
why does ionic radius increase from right to left
because nuclear charge decreases so protons cannot pull electrons close to the nucleus
78
why does ionic radius increase down
because energy levels are added so inner electrons shield protons from pulling electrons close to the nucleus
79
a cation is ___ than its parent atom
smaller
80
why is a cation smaller than its parent atom
because a cation loses electrons so there are more protons to pull electrons close to the nucleus
81
an anion is ___ than its parent atom
larger because an anion gains electrons so there a not enough protons to pull electrons close to the nucleus
82
electronegativity defnition
ability of an atom to gain an electron
83
most electronegative element
F
84
electronegativity
increases from left to right
increases up
85
why does electronegativity increase from left to right
because nuclear charge increase so protons pull electrons close to the nucleus
86
why does electronegativity increase up
because energy levels decrease so there are not enough inner electrons to shield protons from pulling electrons close to the nucleus
87
ionization energy definition
energy needed to remove an electron
88
ionization energy
increases from left to right
increases up
89
why does ionization energy increase from left to right
because nuclear charge increases so protons pull electrons close to the nucleus making it harder to remove an electron
90
why does ionization energy increase up
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
metal reactivity means
metals lose electrons
92
metal reactivity
increases from right to left
increases down
93
why does metal reactivity increase from right to left
because nuclear charge decreases so protons can not pull electron close to the nucleus making it easier to lose an electron
94
why does metal reactivity increase down
because energy levels are added so electrons shield protons from pulling electrons close to the nucleus making it easier to remove an electron
95
nonmetal reactivity means
nonmetals gain electrons
96
nonmetal reactivity
increases from left to right
increases up
97
why does nonmetal reactivity increase from left to right
nuclear charge increases so protons pull electrons close to the nucleus
98
why does nonmetal reactivity increase up
because energy levels are decrease so there are not enough inner electrons to shield protons from pulling electrons close to the nucleus
