Download The Periodic Table of the Elements

The Periodic Table of the
Elements
All matter is composed of elements.
All of the elements are composed of
atoms.
An atom is the smallest part of an
element which still retains the properties
of that element.
All of the elements are listed on the Periodic
Table by their Chemical Symbol
• The chemical symbol for every element
is either one capital letter or one capital
letter plus a small letter
For example:
C = carbon
Ca = calcium
Cl = chlorine
Cr = chromium
Chemical Symbols
Chemical Symbols
• represent name of element
• consist of one to two letters and start with capital
1-Letter Symbols 2-Letter Symbols
C carbon
Co cobalt
N nitrogen
Ca calcium
F fluorine
Al aluminum
O oxygen
Mg magnesium
3
Refer to Table 4.2 on Page 97
for list of the more common elements
and their symbols.
All of the elements on the Periodic Table
are arranged in vertical columns called
“Groups”, and in horizontal rows called
“Periods”.
All of the groups have numbers and they are
either “A” groups or “B” groups running from
left to right on the Periodic Table
Periodic Table of the Elements
Group**
Period
1
IA
1A
1
1
H
1.008
2
3
4
5
2
IIA
2A
13
14 15 16
17
IIIA IVA VA VIA VIIA
3A 4A 5A 6A 7A
2
He
4.003
3
4
5
6
7
8
9
10
Be
B
C
N
O
F
Ne
6.941
9.012
11
12
Na Mg
22.99
24.31
19
20
K
Ca
39.10
40.08
37
38
Rb
Sr
85.47
87.62
56
10.81 12.01 14.01 16.00 19.00
8
9
10 11 12
3
4
5
6
7
IIIB IVB VB VIB VIIB ------- VIII --- IB IIB
---3B
4B 5B 6B 7B
1B 2B
------- 8 ------21
Sc
22
23
24
25
26
39
Y
40
41
42
44
72
73
74
(98)
30
16
17
P
S
Cl
26.98 28.09 30.97 32.07 35.45
31
32
33
34
35
45
46
47
48
49
50
51
52
75
53
I
101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9
76
137.3
(223)
29
Al Si
15
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
88.91 91.22 92.91 95.94
57
43
132.9
88
28
14
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Ba La* Hf Ta W Re Os
Fr
27
13
44.96 47.88 50.94 52.00 54.94 55.85 58.47 58.69 63.55 65.39 69.72 72.59 74.92 78.96 79.90
Cs
87
7
8A
Li
55
6
18
VIIIA
77
Ir
78
79
80
81
82
83
84
85
Pt Au Hg Tl Pb Bi Po At
138.9 178.5 180.9 183.9 186.2 190.2 190.2 195.1 197.0 200.5 204.4 207.2 209.0 (210) (210)
107
(222)
118
()
()
()
60
61
62
63
64
111
86
Rn
---
(265) (266)
110
Xe
131.3
116
59
109
54
---
(257) (260) (263) (262)
108
Kr
83.80
114
58
106
36
---
Lanthanide
Series*
105
Ar
39.95
112
(227)
104
18
Ra Ac~ Rf Db Sg Bh Hs Mt --- --- --(226)
89
20.18
()
()
()
65
66
67
68
69
70
71
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
140.1 140.9 144.2 (147) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Actinide Series~ Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
232.0 (231) (238) (237) (242)
(243) (247) (247) (249) (254) (253) (256) (254) (257)
Learning Check
Give the names of the elements with the following symbols:
A. P
B. Al
C. Mn
D. H
E. K
7
Solution
Give the names of the elements with the following symbols:
A. P
= phosphorus
B. Al
= aluminum
C. Mn
= manganese
D. H
= hydrogen
E. K
= potassium
8
Groups
Columns of elements define element groups.
Elements within a group share several
common properties.
Periods
Rows of elements are called periods. The
period numbers increase as you go from top
to bottom on the periodic table. The number
of elements in a period increases as you
move down the periodic table.
Using grid coordinates (like a
checkerboard) each element can
be located on the Periodic Table.
Refer to Figure #4.2 on Page 100
Solution
Identify the element described by the following:
1. Group 7A, Period 4
bromine
2. Group 2A, Period 3
magnesium
3. Group 5A, Period 2
nitrogen
11
Learn the names of
the groups:
Ia = alkali metals
IIa = alkaline earth metals
All “B” groups = Transition metals
VIIA = halogens
VIIIA = noble (inert) gases
Classification of Groups
Page 101
13
Refer to Page 102
Identify each of the following elements as metal, nonmetal, or
metalloid.
A. sodium
metal
B. chlorine
nonmetal
C. silicon
metalloid
D. iron
metal
E. carbon
nonmetal
14
STRUCTURE OF THE ATOM:
Particles that are smaller than the
atom are called subatomic particles.
• The three main subatomic particles that
form an atom are protons, neutrons, and
electrons. The center of the atom is called the
nucleus.
Protons and neutrons make up the nucleus of
an atom.
The atomic
number
Atomic
Number
• is specific for each element.
• is the same for all atoms of an element.
• is equal to the number of protons in an atom.
• appears above the symbol of an element.
Atomic Number
Symbol
11
Na
16
14 ----------Atomic number
Si
28.09 -------- Mass number
An atom is the smallest part of an
element which still retains the
properties of that element.
An isotope is another form of an
element having a different number
of neutrons.
An element's or isotope's atomic
number tells how many protons
are in its atoms.
An element's or isotope's mass
number tells how many protons
and neutrons in its atoms.
Subatomic
Particle
Mass
Electrical
Charge
P
1
+1
N
e
1
0
0
-1
Subatomic Particles in the Atom
See Page 108
4.5
21
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
• Protons have a positive electrical
charge, so they are often represented
with the mark of a "+" sign.
• Neutrons have no electrical charge
Learning Check
Identify each statement as describing a
1) proton, 2) neutron, or 3) electron.
A. found outside the nucleus
B. has a positive charge
C. is neutral
D. found in the nucleus
23
Atomic Number
The atomic number
• is specific for each element
• is the same for all atoms of an element
• is equal to the number of protons in an atom
• appears above the symbol of an element in the Periodic
Table
Atomic Number
Symbol
11
Na
24
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Every element, standing alone, in its
neutral or uncombined state, MUST have
an overall electrical charge of ZERO.
• That means that the number of
electrons (negatives) must equal the
number of protons (positives).
Atoms Are Neutral
For neutral atoms, the net charge is zero.
number of protons = number of electrons
Aluminum has 13 protons and 13 electrons. The net
(overall) charge is zero.
13 protons (13+) + 13 electrons (13–) = 0
26
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Composition of Some Atoms of
Different Elements
See Page 110
Table 4.6
27
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Learning Check
Use the periodic table to fill in the atomic number, number of
protons, and number of electrons for each of the following
elements:
Element Atomic
Number
Protons
Electrons
N
Zn
S
28
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Solution
Use the periodic table to fill in the atomic number, number of
protons, and number of electrons for each of the following
elements:
Element Atomic
Number
Protons
Electrons
N
7
7
7
Zn
30
30
30
S
16
16
16
29
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
• Elements: Each element has a fixed
number of positively charged protons in
its nucleus and an equal number of
electrons orbiting the nucleus. For
example, hydrogen (H) has one proton
and one electron, but lead (Pb) has 82
protons and 82 electrons. There are
about 115 known elements of which 82
are naturally abundant.
Study Tips: Protons and Neutrons
Number of protons = atomic number
Number of protons + neutrons = mass number
Number of neutrons = mass number – atomic number
Note: Mass number is given for specific isotopes only.
31
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Learning Check
An atom of lead (Pb) has a mass number of 207.
A. How many protons are in the nucleus?
B. How many neutrons are in the nucleus?
C. How many electrons are in the atom?
32
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Solution
An atom of lead (Pb) has a mass number of 207.
A. How many protons are in the nucleus?
atomic number = 82; number protons = 82
B. How many neutrons are in the nucleus?
mass number – number protons = number neutrons
207 – 82 = 125 neutrons
33
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Solution
An atom of lead (Pb) has a mass number of 207.
C. How many electrons are in the atom?
An atom is neutral, which means that the
number of electrons is equal to the number of
protons. An atom of Pb has 82 protons and
82 electrons.
34
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
This would be the Periodic Table Representation for the
normal (stable) isotope of carbon:
6
C
12
This indicates that the normal
isotope of carbon has 6 protons and
6 neutrons
Atoms of the same element can
have different numbers of
neutrons; the different possible
versions of each element are called
isotopes.
Isotopes
Isotopes
• are atoms of the same element
• have different mass numbers
• have same number of protons but different numbers of
neutrons
37
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Atomic Symbols and Subatomic
Particles
Examples of number of subatomic particles for atoms:
Atomic symbol
16
31
O
8
8 p+
8n
8 e-
P
15
15 p+
16 n
15 e-
65
Zn
30
30 p+
35 n
30 e38
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Atomic Symbols for Isotopes of
Magnesium
Mass Numbers
24
12
Mg

25
12
Mg

Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
26
12
Mg
39
Copyright © 2012 by Pearson Education, Inc.
Atomic Symbols for Isotopes of
Magnesium
Table 4.7
See Page 112
40
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Learning Check
Naturally occurring carbon consists of three isotopes: 12C,
13C, and 14C. State the number of protons, neutrons, and
electrons in each of the following:
Isotope
12C
13C
14C
protons
neutrons
electrons
41
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Solution
Naturally occurring carbon consists of three isotopes: 12C,
13C, and 14C. State the number of protons, neutrons, and
electrons in each of the following:
Isotope
12C
13C
14C
protons
6
6
6
neutrons
6
7
8
electrons
6
6
6
42
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition
Copyright © 2012 by Pearson Education, Inc.
Which element does “X” represent in the following symbol ?
80
35
A.) mercury
X
B.) chlorine C.) scandium D.) bromine E.) selenium
Correct
answer
Nuclear Notation
Standard nuclear notation shows
the chemical symbol, the mass
number and the atomic number of
the isotope.
C
12
6
C
Normal
Isotope
14
6
This notation represents the isotope of
carbon which has 8 neutrons, rather than
6 neutrons in the normal (stable)isotope
See Page 102
See Page 114
All atoms of any given element have the
same mass. The mass of an element is the
number beneath its chemical symbol on
the periodic table.
It represents the average mass of the
isotopes that compose that element,
weighted according to the natural
abundance of each isotope of that
element.
See Page 113
The atomic mass of
chlorine is:
•1.) due to all the Cl
isotopes.
•2.) not a whole
number.
•3.) the average of
two isotopes: 35Cl
and 37Cl.
Electrons spin and rotate around the
outside of the nucleus.
Only a certain number of electrons can be in
an energy level at the same time.
The octet rule says that atoms can only
have a limited number of electrons in each
electron shell.
Octet Rule:
The first (innermost) shell is
filled with 2 electrons.
All of the rest of the shells are
filled with 8 electrons
The octet rule:
Shell Number
1
2
3
4
5
Number of electrons
2
8
8
8 (18)
8 (32)
Helium atom model
This helium (He) model displays two valence electrons
located in its outermost energy level.
Helium is a member of the noble gases and contains
two protons, neutrons, and electrons.
The valence electrons are the
electrons in the last shell or energy
level of an atom.
For the “A” Groups on the Periodic Table, the Group
Number indicates the number of valence electrons
for every element in that group.
Elements in group IA have 1 valence
electron. Elements in group IIA have 2
valence electrons.
• The number of valence electrons of an
element is determined by its periodic table
group (vertical column) in which the
element is categorized. FOR THE “A”
GROUPS ONLY, the number of the group
identifies how many valence electrons are
contained within the elements listed under
that particular column.
In the electron level arrangement for the first 18
elements
• electrons are placed in energy levels (1, 2, 3,
etc.), beginning with the lowest energy level
• there is a maximum number in each energy level
according to the octet rule.
Energy level
Number of electrons
1
2 (up to He)
2
8 (up to Ne)
3
8 (up to Ar)
4
2 (up to Ca)
58
Example: 1
The electronic configurations of some
of the elements are detailed below. How
many valence electrons do the following
have?
(a) Al : 2, 8, 3 (Group 3A)
(b) Mg: 2, 8, 2 (Group 2A)
(c) Cl : 2, 8, 7 (Group 7A)
(d) Ca : 2, 8, 8, 2 (Group 2A)
Learning Check
Write the electron level arrangement for each:
N = 2, 5
Cl = 2, 8, 7
K = 2, 8, 8, 1
60
All atoms will tend to gain or lose
electrons in order to complete their outer
shell.
Metals will generally lose their outer
(valence) electrons to complete their
outer shell.
Nonmetals will tend to gain electrons to
complete their outer shell.
Metalloids may do either.
Recommended problems for chapter 4:
Page 104 . . . . # 4.7 through #4.12
Page 108 . . . . # 4.15 - #4.16
Page 111 . . . . # 4.23 - #4.30
Page 114 . . . . # 4.31 - #4.34
Page 115 . . . . # 4.35 - #4.36
Page 119 . . . . # 4.43 - #4.46
Page 130 . . . . # 4.87 - #4.90
Page 131 . . . . # 4.91 - #4.100