Upload
tony-mcdonald
View
217
Download
2
Embed Size (px)
Citation preview
Periodic Table of Element
Mrs. Clendenon
The Periodic TableName as many things as you can about what you remember about the periodic table of
elements
1IA
18VIIIA
11H
1.00797
2IIA
Periodic Table 13IIIA
14IVA
15VA
16VIA
17VIIA
2He
4.0026
23
Li6.939
4Be
9.0122
5B
10.811
6C
12.0112
7N
14.0067
8O
15.9994
9F
18.9984
10Ne
20.179
311
Na22.9898
12Mg24.305
3IIIB
4IVB
5VB
6VIB
7VIIB
8 9VIIIB
10 11IB
12IIB
13Al
26.9815
14Si
28.086
15P
30.9738
16S
32.064
17Cl
35.453
18Ar
39.948
419K
39.102
20Ca40.08
21Sc
44.956
22Ti
47.90
23V
50.942
24Cr
51.996
25Mn
54.9380
26Fe
55.847
27Co
58.9332
28Ni58.71
29Cu63.54
30Zn65.37
31Ga65.37
32Ge72.59
33As
74.9216
34Se78.96
35Br
79.909
36Kr83.80
537
Rb85.47
38Sr87.62
39Y
88.905
40Zr91.22
41Nb
92.906
42Mo95.94
43Tc[99]
44Ru
101.07
45Rh
102.905
46Pd106.4
47Ag
107.870
48Cd
112.40
49In
114.82
50Sn
118.69
51Sb
121.75
52Te
127.60
53I
126.904
54Xe
131.30
655Cs
132.905
56Ba
137.34
57La
138.91
72Hf
178.49
73Ta
180.948
74W
183.85
75Re186.2
76Os190.2
77Ir
192.2
78Pt
195.09
79Au
196.967
80Hg200.59
81Tl
204.37
82Pb
207.19
83Bi
208.980
84Po[210]
85At[210]
86Rn[222]
787Fr[223]
88Ra[226]
89Ac[227]
104Ku[260]
105 106 107 108 109http://www.chemsoc.org/viselements/pages/periodic_table.html
Periodic Table: It is arranged by metals, nonmetals and metalloids
1IA
18VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
MetalsMetals
Metalloids
NonmetalsNonmetals
Metals How would you describe metals?
Metals are lustrous (shiny), malleable, ductile, and are good conductors of heat and electricity.
They are mostly solids at room temp.
Nonmetals – How would you describe these?
Nonmetals are the opposite.
They are dull, brittle, nonconductors (insulators).
Some are solid, but many are gases, and Bromine is a liquid.
Metalloids – How would you describe these?
Metalloids, aka semi-metals are just that.
They have characteristics of both metals and nonmetals.
They are shiny but brittle.
And they are semiconductors.
Across the Periodic Table
Elements are arranged horizontally across the periodic table (rows 1-7), what is
this arrangement called?
PeriodsPeriods
These elements have the same number of valence shells. How many shells are in
period 2? 6?
Period 2 would have two shells, while period 6 would have 6.Period 2 would have two shells, while period 6 would have 6.
1IA
18VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
2nd Period
6th Period
Down the Periodic Table Elements are arranged vertically down the periodic table (columns or group, 1- 18 or 1-8 A,B), what Elements are arranged vertically down the periodic table (columns or group, 1- 18 or 1-8 A,B), what are they called? are they called?
Family/Groups Family/Groups What do these elements have in common? What do these elements have in common?
Same number of valence electrons.Same number of valence electrons.
1IA
18VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
Alkali Family: 1 e- in the valence shell
Alkali Family: 1 e- in the valence shell
Halogen Family: 7 e- in the valence shell
Halogen Family: 7 e- in the valence shell
The roman numerals represent the number of valence electrons each family have.
How many valence electrons are in the Alkali Earth Family?
1IA
18VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
Alkali Family: Alkali Family:
Halogen Family: Halogen Family:
1 valence electron
1s1
1s22s1
1s22s22p63s1
1s22s22p63s23p64s1
1s22s22p63s23p64s23d104p65s1
1s22s22p63s23p64s23d104p65s24d10 5p66s1
1s22s22p63s23p64s23d104p65s24d105p66s2
4f145d106p67s1
H1
Li3
Na11
K19
Rb37
Cs55
Fr87
Do you notice any similarity in these configurations of the alkali metals?
They all have 1 valence electron
Valence electrons for ElementsValence electrons for ElementsRecall that the valence electrons for the elements Recall that the valence electrons for the elements can be determined based on the elements position can be determined based on the elements position on the periodic table. This is based on the on the periodic table. This is based on the family/group they are found infamily/group they are found in
Infamous Families of the Periodic Table
Name all 6 families.
1IA
18VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
Alkali
Alkaline (earth)
Transition MetalsTransition Metals
Noble GasNoble GasHalogenHalogen
HalogensHalogens
Trend in Atomic Radius
Atomic Radius: Atomic Radius:
The size of at atomic radius decrease the closer the element are to the noble gases (to the right).
The atomic radius increases as the elements increase in the number of periods (moving down).
Which atom is larger in size? K or Kr? ___________
K In or Rb ? ________
Rb
Periodic Table: electron behaviorThe periodic table can be classified by the behavior of their electrons
1IA
18VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
METALS METALLOID NON-METALS Alkali
Alkaline Transition
Noble gas Halogens Halogens
These elements tend to give up
e- and form CATIONS become +
These elements will give up e- or accept e-
These elements tend to accept e- and form ANIONS
become negative
Trends in Atomic and Ionic Size
152
186
227
Li
Na
K
60
Li+
95
Na+
133
K+
e
e
e
F1-
136
Cl1-
181
Br-1-
195
F
Cl
Br
64
99
114
e
e
e
Metals NonmetalsGroup 1
Al
143
50
ee
e
Group 13 Group 17
Cations are smaller than parent atoms Anions are larger than parent atoms
Al3+
Trend in Electronegativity
Electronegativity: Electronegativity: •Electronegativity is a measure of an atom’s attraction for another atom’s electrons.•Elements with a high electronegatvity (EN) means it pulls the electron towards itself strongly! •Metals are electron givers and have low EN while nonmetals are electron takers and have high EN.
•What about the noble gases?•They have no EN because they have a full outer electron orbital
Electronegativity
F
Cs
Which element has the highest EN?
Fluorine
Which element has the least EN?
Cesium
1
2
3
4
5
6
1
2
3
4
5
6
Electronegativity
7
Be
1.5
Al
1.5
Si
1.8
Ti
1.5
V
1.6
Cr
1.6
Mn
1.5
Fe
1.8
Co
1.8
Ni
1.8
Cu
1.9
Zn
1.7
Ga
1.6
Ge
1.8
Nb
1.6
Mo
1.8
Tc
1.9
Ag
1.9
Cd
1.7
In
1.7
Sn
1.8
Sb
1.9
Ta
1.5
W
1.7
Re
1.9
Hg
1.9
Tl
1.8
Pb
1.8
Bi
1.9
1.5 - 1.9
N
3.0
O
3.5
F
4.0
Cl
3.0
3.0 - 4.0
C
2.5
S
2.5
Br
2.8
I
2.5
2.5 - 2.9
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Ba
0.9
Fr
0.7
Ra
0.9
Below 1.0
H
2.1
B
2.0
P
2.1
As
2.0
Se
2.4
Ru
2.2
Rh
2.2
Pd
2.2
Te
2.1
Os
2.2
Ir
2.2
Pt
2.2
Au
2.4
Po
2.0
At
2.2
2.0 - 2.4
Per
iod
Actinides: 1.3 - 1.5
Li
1.0
Ca
1.0
Sc
1.3
Sr
1.0
Y
1.2
Zr
1.4
Hf
1.3
Mg
1.2
La
1.1
Ac
1.1
1.0 - 1.4
Lanthanides: 1.1 - 1.3
1A
2A
3B 4B 5B 6B 7B 1B 2B
3A 4A 5A 6A 7A
8A
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373
8B
Trend in Ionization Energy
Definition – amount energy needed to remove the outer most electronAs you go down a group, the first IE decreases because...The electron is further away from the attraction of the nucleus, and
The larger the atom is, the easier its electrons are to remove.Trend from left to right – increasesTrend from top to bottom – decreases
Firs
t Ion
izat
ion
ener
gy
Atomic number
H
HeHelium is a noble gas, the energy to
remove its outer valence electron will be extremely high
Why does Lithium have a low IE? Lithium would have a lower IE because it
has a larger atomic radius than H
Why do atoms steal electrons or give them away?
Atoms behave in ways to try and achieve a noble gas configuration.
Would Beryllium have a higher first or second ionization energy level?
Second
Li
Be
B
Ionization Energy
F
Cs
Noble
Gas
Summary of Trend
Atomic Radius: Largest toward SW corner of PTAtomic Radius: Largest toward SW corner of PT
Ionization Energy: Largest toward FluorineIonization Energy: Largest toward FluorineElectronegativity: Most favorable FluorineElectronegativity: Most favorable Fluorine
Review Game
Round 1
White board
How many valence electrons does Krypton have?
8
What is the family name of the group 2A elements?
Alkaline Earth Metals
Name three characteristics of a metal.
Metals are lustrous (shiny), malleable, ductile, and are good conductors of heat and electricity.
They are mostly solids at room temp.
What is the family name of the group 8A elements?
Nobel Gases
Draw the Lewis Dot structure for chlorine.
How many valence electrons does this element have?
Ca 1s22s22p63s23p64s2
2
Where are metalloids located?
They are the elements touching the staircase.
What is the family name of the group 7A elements?
Halogens
A vertical column ( ↓ ) of elements on the
periodic table may also be referred to as a:
Family or Groups
What is the family name of the group 1A elements?
Alkaline metals
Describe three characteristics of a nonmetal.
Nonmetals are the opposite.
They are dull, brittle, nonconductors (insulators).
Some are solid, but many are gases, and Bromine is a liquid
Draw the lewis dot structure for Bromide.
A horizontal row ( → ) of elements on the periodic table may also be referred to as a:
Period
Review Game
Round 2
clickers
Cations have a ______________ charge and are ______________ than the atoms from which they formed.
A. negative/larger
B. positive/smaller
C. positive/larger
D. negative/smaller
B
Given the representation of a chlorine atom, which circle might represent an atom of bromine?
A. Circle C
B. None of these
C. Circle D
D. Circle B
c
Of the following elements, which one would have the largest radius?
A. Hydrogen (H)
B. Potassium (K)
C. Sodium (Na)
D. Cesium (Cs)
d
The elements with the smallest atomic radii are found in the:
A. lower left-hand corner of the periodic table
B. lower right-hand corner of the periodic table
C. upper left-hand corner of the periodic table
D. upper right-hand corner of the periodic table
d
Anions have a ______________ charge and are ______________ than the atoms from which they formed.
A. positive/smaller
B. negative/smaller
C. positive/larger
D. negative/larger
d
Of the following elements, which one would have the largest ionization energy?
A. Hydrogen (H)
B. Potassium (K)
C. Cesium (Cs)
D. Sodium (Na)
a
The energy required to remove an electron from an atom is known as:
A. electronegatvity
B. radioactivity
C. electron affinity
D. ionization energy
D
Given the representation of a chlorine atom, which circle might represent an atom of fluorine?
A. Circle C
B. None of these
C. Circle B
D. Circle D
b
The most active metals are located in the:
A. upper right hand corner of the periodic table
B. lower left hand corner of the periodic table
C. upper left hand corner of the periodic table
D. lower right hand corner of the periodic table
B
Of the following elements, which one would have the smallest radius?
A. Bromine (Br)
B. Fluorine (F)
C. Chlorine (Cl)
D. Iodine (I)
B
As one moves down ( ↓ ) a group on the periodic table, the ionization energy of the elements encountered tends to:
A. stay the same
B. decrease
C. increase
B
Of the following elements, which one would have the largest electronegativity energy?
A. Chlorine (Cl)
B. Fluorine (F)
C. Iodine (I)
D. Bromine (Br)
B
Of the following elements, which one would have the largest radius?
A. Lithium (Li)
B. Nitrogen (N)
C. Boron (B)
D. Neon (Ne)
A
Given the representation of a chlorine atom, which circle might a chloride ion, Cl-?
A. Circle C
B. Circle B
C. Circle D
D. None of these
D
As one moves from left to right ( → ) within a
period across the periodic table, the atomic
radius of the elements encountered tends to:
A. increase
B. stay the same
C. decrease
C
Which of these elements would have the lowest first ionization energy?
A. Element D
B. Element C
C. Element A
D. Element B
A
The least electronegative elements are the:
A. Transition metals
B. Alkali metals
C. Halogens
D. Metalloids
B
As one moves from left to right ( → ) within a period across the periodic table, the ionization energy of the elements encountered tends to:
A. decrease
B. increase
C. stay the same
B
The measure of the attraction that an atom has for electrons involved in chemical bonds is known as:
A. electron affinity
B. radioactivity
C. electronegatvity
D. ionization energy
C