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History of the Atom
Scientists and Their
Discoveries
Democritus
(460 BC – 370 BC)
• Proposed an Atomic Theory
which states that all atoms
are small, hard, indivisible and
indestructible particles made
of a single material formed
into different shapes and
sizes.
• Aristotle did not support his
atomic theory
Image taken from: https://reichchemistry.wikispaces.com/T.+Glenn+
Time+Line+Project
Antoine Lavoisier
(1743 – 1794)
Image taken from:
www.ldeo.columbia.edu/.../v1001/geo
time2.html
 Known as the “Father of Modern
Chemistry”
 Was the first person to
generate a list of thirty-three
elements in his textbook
 Devised the metric system
 Married to a 13-year old MarieAnne Pierette Paulze; she
assisted him with much of his
work
 Was guillotined during the
French Revolution
 Discovered/proposed the Law of
Conservation of Mass
John Dalton
(1766 – 1844)
 In 1803, proposed an Atomic
Theory which states:
o All substances are made of
atoms; atoms are small
particles that cannot be
created, divided, or
destroyed.
o Atoms of the same element
are exactly alike, and atoms
of different elements are
different
o Atoms join with other atoms
to make new substances
 Calculated the atomic weights of
many various elements
Image taken from:
chemistry.about.com/.../JohnDalton.htm
J.J. Thomson
(1856 – 1940)
Image taken from:
www.wired.com/.../news/2008/04/d
ayintech_0430
 Proved that an atom can be
divided into smaller parts
 Discovered electrons
 Stated that the atom is neutral
 In 1897, proposed the Plum
Pudding Model which states that
atoms mostly consist of
positively charged material with
negatively charged particles
(electrons) located throughout
the positive material
 Won a Nobel Prize
Ernest Rutherford
(1871 – 1937)
 In 1909, suggested the following
characteristics of the atom:
o Has a nucleus that contains most
of the mass of the atom and is
made up of particles called
protons, which have a positive
charge
o The protons are surrounded by
negatively charged electrons,
but most of the atom is actually
empty space
 Did extensive work on radioactivity
and was referred to as the “Father
of Nuclear Physics”
 Won a Nobel Prize
 Was a student of J.J. Thomson
Image taken from:
http://www.scientificweb.com/en/Physics/Biographies/Er
nestRutherford.html
Niels Bohr
(1885 – 1962)
Image taken from:
commons.wikimedia.org/wiki/File:Ni
els_Bohr.jpg
 In 1913, proposed the Bohr
Model, which suggests that
electrons travel around the
nucleus of an atom in orbits or
definite paths. Additionally, the
electrons can jump from a path
in one level to a path in another
level (depending on their energy)
 Won a Nobel Prize
 Worked with Ernest Rutherford
Erwin Schrodinger
(1887-1961)
• In 1926, he further explained
the nature of electrons in an
atom:
– The exact location of an
electron cannot be stated
– It is more accurate to view
the electrons in regions
called electron clouds;
electron clouds are places
where the electrons are
likely to be found
• Won a Nobel Prize
Image taken from:
nobelprize.org/.../1933/schrodinger
-bio.html
James Chadwick
(1891 – 1974)
 Realized that the atomic mass of
most elements was double the
number of protons  discovery
of the neutron in 1932
 Worked on the Manhattan
Project
 Worked with Ernest Rutherford
 Won a Nobel Prize
Image taken from:
www.wired.com/.../news/2009/02/d
ayintech_0227
The Building Blocks of Matter:
Atoms
-
++ +
+ + +
+
+
-
-
-
-
Matter
• Anything that has mass and takes up
space (volume)
– Examples:
•
•
•
•
A brick has mass and takes up space
A desk has mass and takes up space
A pencil has mass and takes up space
Air has mass and takes up space
All of the above examples are considered matter because
they have mass and take up space. Can you think of
anything that would not be considered matter?
Atoms
• Atoms- smallest possible
unit into which matter can
be divided, while still
maintaining its properties.
-
+
+
+
+
-
• Made up of:
-
For example, what is the
+
– protons
smallest possible unit
into which a long essay can be
– neutrons
divided and still have some meaning?
– electrons
• The solar system is
commonly used as an
analogy to describe the
structure of an atom
Atoms are so small that…
• A stack of 50,000 aluminum
atoms = the thickness of a
sheet of aluminum foil from
your kitchen.
www.deckersfoods.com
• If you could enlarge a penny
until it was as wide as the US,
each of its atoms would be
only about 3 cm in diameter –
about the size of a ping-pong
ball
C-C-C-C-C-… + 999,995 more
• Human hair is about 1 million
carbon atoms wide.
1 trillion atoms 
• Typical human cell contains
roughly 1 trillion atoms.
.
Is made of approximately 3 trillion atoms
• A speck of dust might contain
3x1012 (3 trillion) atoms.
• It would take you around 500
years to count the number of
atoms in a grain of salt.
Just one of these grains
Let’s Experiment
In order to try to gain an idea of how small an
atom really is, you will complete the following
activity.
1.
2.
3.
4.
Cut a strip of 11 in. paper in half.
Discard one half.
Cut the remaining piece in half.
Continue cutting the pieces in half and
discarding the strips as many times as you
can, counting the number of cuts you make
Results
• How many cuts were you able to make?
• Do you think you could keep cutting the
paper forever? Why or why not?
You would have to cut the paper in
half around 31 times to get to the size
of any atom.
http://www.miamisci.org/af/sln/phantom/papercutting.html
Protons (+)
• Protons- positively
charged particles
• Make up part of the
nucleus of the atom
• Identify the atom
• Equal to the atomic
number of the atom
• Contribute to the
atomic mass
• Equal to the number of
electrons
-
++ +
+ + +
+ +
-
-
-
+
-
-
Neutrons
-
++ +
+ + +
+ +
-
-
-
-
-
• Neutrons- neutral
particles; have no
electric charge
• Help make up the
nucleus of the
atom
• Contribute to the
atomic mass
Electrons (-)
• Electrons- negatively charged
particles
• Found outside the nucleus of
the atom in electron
orbits/levels
• Each orbit/level can hold a
maximum number of electrons
1st = 2, 2nd = 8, 3rd = 8
• When the orbitals are full,
the atoms are stable!
• This Octet Rule for atoms
with < 20 electrons is 2, 8,
8, 8
• > 20 disregard
-
++ +
+ + +
+ +
-
-
-
-
-
-
Electrons (-)
•Move so rapidly they create
an electron cloud
•Mass is insignificant
•Equal to the number of
protons
•Valence electrons- the
outermost electrons involved
in the formation of chemical
bonds
The Atom’s “Center”
• Protons and neutrons are grouped together to
form the “center” or nucleus of an atom.
Notice that the electrons are not apart of the nucleus
-
+
-
+ +
-
QUARKS
• Particles that make up protons and neutrons
Notice the
smaller
particles that
make up this
neutron after
you take a
closer look.
+
Notice the
smaller
particles that
make up this
proton after
you take a
closer look.
What do you notice about the number
of quarks in the neutron and proton?
Sub-Atomic Particles
Weight Comparison
(protons, neutrons, electrons)
Neutron = 1.6749286 x10-27 kg
Proton = 1.6726231 x10-27 kg
Electron = 9.1093897 x10-31 kg
- - - - - - - - - - - - - -
- - - - - - - - - - - - - -
1839 electrons = 1 neutron
+
1836 electrons = 1 proton
+
How do you think the mass of a neutron
compares to that of a proton?
1 neutron ≈ 1 proton
Sub-atomic Particles
Size Comparison
(protons, neutrons, electrons, & quarks)
Size in
atoms
-
Size in
meters
(m)
-
Atom
1
10-10
Nucleus
__1__
10,000
10-14
Proton or
Neutron
___1___
100,000
10-15
++ +
+ + +
+
+
Electron
or Quark
_____1____
100,000,000
10-18
-
-
-
(at largest)
-
-
Something to Think About
• You’ll never see life the same way
again
Elements
• Element- made up of
one kind of atom
that can’t be broken
down into simpler
substances by
physical or chemical
means
• 90 occur naturally on
Earth
• 25 were synthesized
(made) by scientists
1
2
3
4
5
6
7
1
18
1
H
2
13 14 15 16 17
1.008
2
He
4.003
3
4
5
6
7
8
9
10
Li
Be
B
15.999
F
9.012
14.007
O
6.941
12.001
N
Ne
10.811
C
18.998
11
12
13
14
15
16
17
18
Na
Mg
22.990
24.305
Al
26.982
Si
28.086
P
30.974
S
32.066
Cl
35.453
Ar
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Sc
40.078
44.956
Ti
47.87
V
50.942
Cr
Mn
39.098
Ca
51.996
54.938
Fe
Co
Ni
58.69
Cu
63.546
Zn
65.39
Ga
69.723
Ge
72.61
As
74.922
Se
78.96
Br
79.904
Kr
37
38
39
40
41
42
43
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Zr
Nb
Mo
95.94
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
87.62
92.906
Tc
85.468
102.906
106.42
107.868
112.4
114.818
118.710
121.760
127.60
126.904
131.29
55
56
Cs
Ba
132.905
3
Y
88.906
71
72
Hf
174.967
103
87
88
Ra
(223)
(226)
91.224
Lu
137.327
Fr
4
Lr
(262)
178.49
5
73
Ta
180.95
6
7
(98)
8
55.845
44
Ru
101.07
74
75
76
W
Re
Os
183.84
186.207
190.23
9 10 11 12
58.933
77
Ir
192.217
78
79
80
Pt
Au
Hg
112
Uub
195.078
196.967
104
105
106
107
108
109
110
111
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
(266)
(264)
(269)
(269)
(272)
(261)
Lanthanides
Actinides
(262)
(268)
200.59
(285)
81
82
Tl
Pb
204.383
207.2
20.180
39.948
83.80
83
84
85
86
Bi
Po
At
Rn
116
Uuh
117
118
Uus
Uuo
208.980
113
114
115
Uut
Uuq
Uup
(284)
(289)
(288)
(209)
(292)
(210)
(222)
57
58
59
60
61
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Pm
Sm
Dy
Er
158.925
164.930
167.26
168.934
Yb
151.964
162.50
Ho
140.908
157.25
Tb
140.116
(145)
Gd
138.906
150.36
Eu
Tm
144.24
173.04
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
232.038
231.036
238.029
(257)
(258)
(259)
(227)
(237)
(244)
(243)
(247)
(247)
(251)
(252)
The Periodic Table Elements
• Boxes in the periodic table contain a lot of
information. To understand this information, it is
necessary to refer to the periodic table’s key
8
O
Oxygen
15.999
Atomic Number
Element Symbol (a capital
letter or a capital followed
by a lower case letter)
Element Name
Atomic Mass
Atomic Number
• Atomic number- the number of protons in the
nucleus of an atom
• Equal to the number of electrons to make an atom
neutral
-
-
+
++
-
What would
be the atomic
number of this
atom?
Atomic Mass
• Atomic mass- the total number of protons and
neutrons in an atom’s nucleus
• Expressed in Atomic Mass Units (amu)
• Each proton or neutron has a mass of 1 amu
What would be the atomic
mass of this atom?
+
-
 3
 4
+
++
3 protons + 4 neutrons =
an atomic mass of 7 amu
Why did we not account for the
electrons when calculating the
atomic mass?
-
-
How to Obtain the Number of Sub-Atomic Particles in
an atom using a Periodic Table
-
+
-
++ +
+ + +
+
+
= 8
= 8
-
-
= 8
-
Protons
Neutrons
+
Electrons
-
Equal to the atomic #
on the Periodic Table
Equal to the atomic mass
(rounded to a whole #)
minus the # of protons
Equal to the # of
protons
Example: Determine the # of protons, neutrons, and electrons in an atom of oxygen.
Protons = 8 (Atomic #)
Neutrons = 8 (Rounded atomic mass minus atomic #)
Neutron Calculations = 16 (P + N) – 8 (P) = 8 N
Electrons = 8 (# of P)
Building Atoms
Atoms
Carbon
Beryllium
Oxygen
Lithium
Sodium
Protons
6
4
8
3
11
Neutrons Electrons
6
6
5
4
8
8
4
3
12
11
Hydrogen (H) Atom
• Bohr electron diagrams- show ALL the electrons in
an atom. Notice the 1 electron in the 1st orbital
• The rule is 2 in the first orbital, then 8, 8 = full
and stable (unreactive)
+ =1
-
=0
-
=1
+
Even though there are no neutrons present,
Hydrogen is still considered an atom
How many
more
electrons
can fit in
the 1st
orbital/
level?
Oxygen (O) Atom
• Notice the two electrons in the first orbital/level
and the six in the second
+ =8
=8
-
-
=8
++ +
+ + +
+
+
-
-
-
-
How many
more
electrons
can fit in
the 2nd
orbital/
level?
Sodium (Na) Atom
• Notice the two electrons in the first orbital/level,
eight in the second, and one in the third
-
+ = 11
= 12
-
-
= 11
++ +
+ + +
+
+
-
-
-
-
-
How many
more
electrons
can fit in
the 3rd
orbital/
level?
Lewis Structure
(Electron Dot Diagram)
• Valence electrons- the electrons in the outermost
shell that are responsible for how an atom will
behave chemically
• Lewis Dot Structure- way of drawing ONLY the
valence electrons of an atom
• Element symbol surrounded by as many dots as
there are valence electrons
• Examples
Al :
Aluminum
.
.N :
.
.
Nitrogen
Mg :
Magnesium
How many valence electrons do each of these atoms have?
Counting Valence Electrons
-
-
-
+
-
+
+
++ +
+ + +
+
+
+
+
-
-
+
+
-
-
+ +
-
+
-
-
-
-
-
-
Carbon
Oxygen
Beryllium
4 valence
electrons
6 valence
electrons
2 valence
electrons
Check for Understanding
How Many Valence Electrons?
• Hydrogen
• Potassium
• Neon
• Sulfur
• Calcium
1 Valence
Electron
1 Valence
Electron
8 Valence
Electrons
6 Valence
Electrons
2 Valence
Electrons
Making an Electron Dot Diagram
Element “X” has 8 valence electrons
Write down the element’s symbol
and place the first two dots on any
side of the symbol.
.
X
X:
If this were an atom of an element
from group 1, you would just place the
one dot on any side of the element.
.
.X :
.
..
.X :
.
.
X:
.
.X :
Place the rest of the dots in either a
clockwise or counter clockwise manner around
the symbol, with no side receiving two dots
until each side gets one.
..
: X. :
..
:.X.:
Check for Understanding
1 Valence Electron
6 Valence Electrons
H
O
How many valence
electrons does
each atom have?
Ne
8 Valence Electrons
Mg
2 Valence Electrons
Ion
• Charged particle that
typically results from a
loss or gain of
electrons
• Two types:
– Anion = negatively +
charged particle
– Cation = positively
charged particle
-
-
= 8
-
++ +
+ + +
+
+
-
-
= 8
= 968
Now
Now
that
that three
this
atom
electrons
ofof
oxygen
were just
lost,
Currently,
this
atom
oxygen
is
gained
the
number
an
electron,
of
electrons
it
is
no
(6)
longer
and
neutral because it has an equal
protons
neutral
(8)
an
is atom.
still (8)
unbalanced;
It
is protons
now
number
of or
electrons
and
considered
therefore, an
it is
ionstill
(anion).
but ion
nowhas
it
(8).an ion,This
ismore
specifically
electrons
referred
(9) thantoprotons
as a cation.
(8).
-
-
2+
Symbol
Symbol == O
O1-
Building Ions
Ions
Protons
Neutrons
Electrons
Carbon (C³¯)
6
6
9
Hydrogen (H¹+)
1
0
0
Oxygen (O²¯)
8
8
10
Lithium (Li³+)
3
4
0
Sodium (Na¹¯)
11
12
12
Be aware that the atomic and atomic mass are not
impacted by the loss or gain of electrons.
Isotopes
• Isotopes- atoms that have the same number of
protons, but have different numbers of neutrons
• Examples Notice that each of these atoms have one proton;
therefore they are all types of hydrogen. They
just have a different atomic mass
+
Hydrogen (Protium)
+
-
Hydrogen (Deuterium)
+
Hydrogen (Tritium)
Isotopes
• Recall that the atomic mass is the number of
neutrons and protons in an atom
• Example
-
+
Hydrogen (Protium)
Atomic mass # = 1 amu
+
-
Hydrogen (Deuterium)
Atomic mass # = 2 amu
+
-
Hydrogen (Tritium)
Atomic mass # = 3 amu
FORCES IN THE ATOM
• Gravitational Force
• Electromagnetic Force
• Strong Force
• Weak Force
Gravitational Force
• The force of
attraction of
objects due to
their masses
• The amount of
gravity between
objects depends on
their masses and
the distance
between them
Do you think this force plays a significant
role in holding the atom together?
Electromagnetic Force
• The force that
results from the
repulsion of like
charges and the
attraction of
opposites
• The force that holds
the electrons around
the nucleus
Why are neutrons not
pictured above?
+ +
+
- -
Notice how the
particles with the
same charge move
apart and the
particles with
different charges
move together.
Strong Force
• The force that
holds the atomic
nucleus together
• The force that
counteracts the
electromagnetic
force
• This force is only
strong if the
protons and
neutrons are close
together
Notice how the
electromagnetic force causes
the protons to repel each
other but, the strong force
holds them together.
+
+
+
+
Would an atom have a
nucleus if the strong
force did not exist?
Weak Force
• Plays a key role in the
possible change of subatomic particles.
– For example, a
neutron can change
into a proton(+) and an
electron(-)
Notice how the original
particle changes to something
new.
n
-
+
• The force responsible
for radioactive decay.
– Radioactive decayprocess in which the
nucleus of a
radioactive (unstable)
atom releases nuclear
radiation.
If you need help
remembering
weak force, just
think of…
Atoms Forces and Elements
• Forces video
The Periodic Table of
Elements
1
1
18
1
H
2
13 14 15 16 17
1.008
2
3
6
4
5
6
7
8
9
10
Be
B
C
N
O
F
Ne
6.941
9.012
11
12
Na
Mg
24.305
3
4
5
6
7
8
9 10 11 12
10.811
12.001
14.007
15.999
18.998
20.180
13
14
15
16
17
18
Al
26.982
Si
28.086
P
30.974
S
32.066
Cl
35.453
Ar
39.948
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
44.956
V
Cr
Mn
40.078
Ti
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
47.87
50.942
51.996
54.938
37
38
39
40
41
42
43
Rb
Sr
Y
Zr
Nb
Mo
85.468
87.62
92.906
95.94
Tc
55
88.906
91.224
56
71
72
73
Cs
Ba
Lu
137.327
174.967
Hf
Ta
87
88
103
Fr
Ra
(223)
(226)
132.905
7
4.003
3
39.098
5
He
Li
22.990
4
2
Lr
(262)
55.845
44
Ru
72.61
74.922
78.96
79.904
83.80
45
46
47
48
49
50
51
52
53
54
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
107.868
112.4
114.818
118.710
121.760
127.60
126.904
131.29
74
75
76
77
78
79
80
81
82
83
84
85
86
Tl
Pb
Bi
Po
At
Rn
116
Uuh
117
118
Uus
Uuo
Os
104
105
106
107
Rf
Db
Actinides
69.723
106.42
Re
Lanthanides
65.39
102.906
W
(262)
63.546
101.07
183.84
(261)
58.69
(98)
180.95
178.49
58.933
186.207
192.217
195.078
Pt
Au
Hg
108
109
110
111
Mt
112
Uub
190.23
Sg
Bh
Hs
(266)
(264)
(269)
Ir
(268)
196.967
Ds
Rg
(269)
(272)
200.59
(285)
204.383
207.2
208.980
113
114
115
Uut
Uuq
Uup
(284)
(289)
(288)
(209)
(292)
(210)
(222)
57
58
59
60
61
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
140.116
140.908
164.930
167.26
168.934
Yb
138.906
144.24
Pm
173.04
(145)
150.36
151.964
157.25
158.925
162.50
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
232.038
231.036
238.029
(257)
(258)
(259)
(227)
(237)
(244)
(243)
(247)
(247)
(251)
(252)
Periodic Table
• Something “periodic” occurs at regular or
generally predictable intervals
• Periodic law - physical and chemical
properties of the elements are periodic
functions of their atomic numbers
• Periodic Table of Elements – a table of
the elements, arranged by atomic number,
that shows the patterns in their
properties; based on the periodic law
Can you think of anything that is periodic?
Element
• A pure substance made up of one kind of
atom that cannot be broken down into
simpler substances by physical or
chemical means
• 90 occur naturally on earth
• 25 were synthesized (made) by scientists
• The Element Song
http://www.privatehand.com/flash/elements.html
Dmitri Mendeleev
• In the 1860’s he
devised a periodic
table where the
elements were
ordered by their
atomic masses
• He did this by
grouping elements
together according to
their similarities
• Draft of Mendeleev's
Periodic Table
Image taken from:
http://jscms.jrn.columbia.edu/cns/2006-04-18/fido-luxuriantflowinghair/mendeleev/
Mendeleev’s Published Periodic Table of Elements
Why do you think there are question marks here?
Image taken from: http://www.chemsoc.org/networks/learnnet/periodictable/post16/develop/mendeleev.htm
Mendeleev’s Predictions
• Although Mendeleev’s Periodic Table of Elements
had missing elements or “gaps,” he was able to
predict the characteristics of these missing
elements because of Periodic Law.
“Ekasilicon”
Date
Predicted
Atomic Mass
1871
72
Germanium
Date
Discovered
1886
Atomic Mass
72.6
Density
5.5 g/cm3
Density
5.47 g/cm3
Bonding
Power
4
Bonding
Power
4
Color
Dark Gray
Color
Grayish
White
Notice how
Mendeleev’s
predictions (orange
column) were very
accurate when
compared to
Germanium’s actual
characteristics
(green column)
Henry Moseley
• In 1914, his work led
to a revision of the
periodic table by
rearranging the
elements by their
atomic numbers
• He concluded that the
number of protons in
an atom is its atomic
number
Image taken from:
http://dewey.library.upenn.edu/sceti/smith/
3 Classes of Elements
1
1
1
H
2
1.008
2
3
3
4
Li
Be
6.941
9.012
11
12
Na
Mg
22.990
4
6
4
5
6
7
8
9
10
17
2
He
4.003
5
6
7
8
9
10
B
C
N
O
F
Ne
10.811
3
15 16
11 12
20.180
12.001
14.007
15.999
18.998
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
26.982
28.086
30.974
32.066
35.453
39.948
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
44.956
V
Cr
Mn
40.078
Ti
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
47.87
50.942
51.996
54.938
37
38
39
40
41
42
43
Rb
Sr
Y
Zr
Nb
Mo
85.468
87.62
92.906
95.94
Tc
88.906
91.224
(98)
55.845
44
Ru
101.07
58.933
58.69
63.546
65.39
69.723
72.61
74.922
78.96
79.904
83.80
45
46
47
48
49
50
51
52
53
54
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
102.906
106.42
107.868
112.4
114.818
118.710
121.760
127.60
126.904
131.29
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Ta
137.327
174.967
Hf
W
Re
Os
190.23
Ir
192.217
Pt
195.078
Au
Hg
200.59
Tl
204.383
Pb
207.2
Bi
208.980
Po
At
Rn
103
112
Uub
113
114
115
117
118
Uut
Uuq
Uup
116
Uuh
Uus
Uuo
(284)
(289)
(288)
68
69
70
132.905
7
13 14
19
39.098
5
24.305
18
Classas a guide,
Color color
Using this
Metal
code your
periodic table to
Non-Metal
show the three classes. Start
Metalloid
by highlighting
the “zig-zag.”
87
88
Fr
Ra
(223)
(226)
Lr
(262)
178.49
180.95
183.84
104
105
106
107
108
109
110
111
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
(266)
(264)
(269)
(269)
(272)
(261)
Lanthanides
Actinides
(262)
57
58
186.207
59
60
Nd
La
Ce
Pr
138.906
140.116
140.908
144.24
(268)
61
62
Pm
Sm
(145)
150.36
196.967
63
Eu
151.964
(285)
64
Gd
157.25
65
Tb
158.925
66
Dy
162.50
67
(209)
(292)
(210)
(222)
Er
Tm
164.930
167.26
168.934
173.04
Ho
Yb
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
232.038
231.036
238.029
(257)
(258)
(259)
(227)
(237)
(244)
(243)
(247)
(247)
(251)
(252)
3 Classes of Elements
Metals
Location
• Found on the left of the
zigzag line/staircase on
the periodic table
(exception  Hydrogen)
Chemical Properties
• Have few electrons in
their outer energy level,
thus lose electrons
easily
Physical Properties
• Ductile, good
conductors, malleable,
shiny, most are solid @
room temperature
79
Au
196.967
11
Na
22.990
Image taken from:
http://chemistry.about.com/od/periodictableelements/ig/E
lement-Photo-Gallery.--98/Sodium.htm
What metal is not a solid
@ room temperature?
Metals’ Chemical Properties
Notice: only 1
electron in outer
level
-
+
-
+ +
-
++
+
+
++
+ +
++ +
-
Notice: only
2 electrons
in outer level
-
-
Be
22.990
-
-
9.012
Na
-
+
4
11
-
-
-
Metals’ Physical Properties
• Good conductorelectrons
(electricity) flow
easily through the
substance
• Malleable- able to
be hammered or
pressed out of
shape without
breaking
Non-Metals
Location
• Most found to the right of
the zigzag line/staircase on
the periodic table
Chemical Properties
• Most have almost full outer
energy levels, thus they
tend to gain electrons;
some have completely full
outer level
Physical Properties
• Not ductile or malleable,
not shiny, poor conductors,
most are solid, but some
are gas at room
temperature
17
Cl
35.453
Image taken from:
http://nobel.scas.bcit.ca/resource/ptable/cl.htm
16
S
32.066
Image taken from:
https://www.dmr.nd.gov/ndgs/rockandmineral/sulfur.asp
Non-metals’ Chemical
Properties
8
-
O
-
15.999
-
++ +
+ + +
+ +
-
-
-
-
Notice: 2
electrons in
outer level –
FULL
-
+
+
-
2
-
He
-
4.003
-
Notice: 6
electrons in
outer level –
almost full
+++
+ + +
++ +
-
9
F
18.998
-
-
Notice: 7
electrons in
outer level –
almost full
Metalloids
Location
• Border the zigzag
line/staircase on the
periodic table
Chemical Properties
• Most atoms have ½ (≈)
complete set of
electrons in outer
level
Physical Properties
• have properties of
both metals and nonmetals
14
Si
28.086
Image taken from:
http://library.thinkquest.org/C0113863/bios.shtml
5
B
10.811
Image taken from:
http://library.thinkquest.org/C0113863/bios.shtml
Metalloids’ Chemical Properties
Notice: only 4
electrons in outer
level
5
B
-
-
10.811
++
+ +
+
-
-
-
-
Notice: only 3
electrons in outer
level
-
+ +++ +
+
++
+ +
+ + ++
-
-
-
-
14
Si
-
28.086
-
-
Important Features of the Periodic
Table
• Period- each horizontal row of elements on the
periodic table
1
18
1
1
H
2
13 14
15 16
17
1.008
2
3
4
5
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
6.941
9.012
11
12
Na
Mg
4
5
6
7
8
9
10
11 12
14.007
15.999
18.998
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
26.982
28.086
30.974
32.066
35.453
39.948
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
40.078
37
38
Rb
Sr
87.62
44.956
47.87
50.942
51.996
54.938
39
40
41
42
43
Y
Zr
Nb
Mo
92.906
95.94
Tc
88.906
91.224
(98)
55.845
44
Ru
101.07
58.933
58.69
63.546
65.39
69.723
72.61
74.922
78.96
79.904
83.80
45
46
47
48
49
50
51
52
53
54
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
106.42
107.868
112.4
114.818
118.710
121.760
127.60
126.904
131.29
102.906
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Ta
137.327
174.967
Hf
W
Re
Os
Ir
Pt
Au
Hg
200.59
Tl
204.383
Pb
207.2
Bi
208.980
Po
At
Rn
103
112
Uub
113
114
115
117
118
Uut
Uuq
Uup
116
Uuh
Uus
Uuo
(284)
(289)
(288)
132.905
7
3
20.180
12.001
K
85.468
6
24.305
10.811
19
39.098
5
4.003
3
22.990
4
2
He
87
88
Fr
Ra
(223)
(226)
Lr
(262)
178.49
180.95
183.84
190.23
192.217
195.078
104
105
106
107
108
109
110
111
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
(266)
(264)
(269)
(269)
(272)
(261)
Lanthanides
Actinides
(262)
186.207
(268)
196.967
(285)
(209)
(292)
(210)
(222)
57
58
59
60
61
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Sm
Dy
Er
158.925
164.930
167.26
168.934
Yb
151.964
162.50
Ho
140.908
157.25
Tb
140.116
150.36
Gd
138.906
(145)
Eu
Tm
144.24
Pm
173.04
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
232.038
231.036
238.029
(257)
(258)
(259)
(227)
(237)
(244)
(243)
(247)
(247)
(251)
(252)
FROM LEFT TO RIGHT OR RIGHT TO LEFT
How many
periods
(rows)
are on the
Periodic
Table
Of
Elements?
Period (Row) Properties
• Seven periods on a periodic table (numbered
from the top down)
• Atomic numbers and atomic masses increase as
you move from the left to the right in a period
• All atoms of the elements in the same period
have the same number of orbitals/levels
• All atoms of the elements in a specific period
have that respective number of orbitals/levels
– Example
• Period 1 = 1 orbital
• Period 2 = 2 orbitals
• Period 3 = 3 orbitals
• Etc…
Examples of Period (Row) elements having the same
number of orbitals/levels in their atoms
-
-
-
In what period
(row) do
you think these
atoms
reside?
-
+
+++ ++
+ +
-
-
-
+
++
+
-
-
-
-
-
-
In what period
(row) do
you think these
atoms
reside?
-
-
-
-
-
-
+++
+
++ +
+
++ +
++ +
+
+++ ++
+
++ ++
-
-
-
-
-
-
-
-
-
-
-
Important Features of the Periodic
Table
•Group- each column of elements on the periodic
1
18
How manytable
groups
(families)
1
1
H
2
1.008
2
3
4
3
4
Li
Be
6.941
9.012
2
He
4.003
5
6
7
8
9
10
B
C
N
O
F
Ne
10.811
20.180
12.001
14.007
15.999
18.998
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
12
Mg
22.990
24.305
26.982
28.086
30.974
32.066
35.453
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
40.078
37
38
Rb
Sr
87.62
3
44.956
4
47.87
5
50.942
6
51.996
7
54.938
39
40
41
42
43
Y
Zr
Nb
Mo
92.906
95.94
Tc
88.906
91.224
(98)
8
55.845
44
Ru
101.07
9
58.933
10
58.69
11 12
63.546
65.39
69.723
72.61
74.922
78.96
79.904
39.948
83.80
45
46
47
48
49
50
51
52
53
54
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
106.42
107.868
112.4
114.818
118.710
121.760
127.60
126.904
131.29
102.906
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Ta
137.327
174.967
Hf
W
Re
Os
Ir
Pt
Au
Hg
200.59
Tl
204.383
Pb
207.2
Bi
208.980
Po
At
Rn
103
112
Uub
113
114
115
117
118
Uut
Uuq
Uup
116
Uuh
Uus
Uuo
(284)
(289)
(288)
132.905
7
17
11
85.468
6
15 16
Na
39.098
5
13 14
are on the
Periodic Table
Of Elements?
87
88
Fr
Ra
(223)
(226)
Lr
(262)
178.49
180.95
183.84
190.23
192.217
195.078
104
105
106
107
108
109
110
111
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
(266)
(264)
(269)
(269)
(272)
(261)
Lanthanides
Actinides
(262)
186.207
(268)
196.967
(285)
(209)
(292)
(210)
(222)
57
58
59
60
61
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Sm
Dy
Er
158.925
164.930
167.26
168.934
Yb
151.964
162.50
Ho
140.908
157.25
Tb
140.116
150.36
Gd
138.906
(145)
Eu
Tm
144.24
Pm
173.04
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
232.038
231.036
238.029
(257)
(258)
(259)
(227)
(237)
(244)
(243)
(247)
(247)
(251)
(252)
FROM TOP TO BOTTOM OR BOTTOM TO THE TOP
Group (Family) Properties
• Eighteen groups on the periodic table (numbered
from left to right)
• Atomic numbers and atomic masses increase as
you move from the top down in a group (family)
• Atoms of elements in the same group have the
same number of electrons in the outer orbitals of
their atoms (known as valence electrons)
– Exceptions:
• Transition elements (3-12)
• Helium (actually has 2 valence electrons)
• Elements in groups usually have similar physical
and chemical properties
Determining the Number of Valence
Electrons by Using the Periodic Table
*Atoms of elements in Groups 1 and 2 have the
same number of valence electrons as their group
number.
*Atoms of elements in Group 3-12 do not have a
general rule relating their valence electrons to
their group number. However, they typically have
between 1 or 2 valence electrons.
*Atoms of elements in Groups 13-18 have 10
fewer valence electrons than their group number.
(Exception - helium atoms have only 2 valence
electrons, even though they are in group 18)
Examples of Group Elements with the
same # of valence electrons
How many electrons do
each of these atoms have
in their outer
orbital/level?
-
1
H
1.008
+
3
Li
6.941
11
Na
-
22.990
-
-
19
-
K
-
39.098
-
++
+
++ +
+ +
++ +
-
+
37
Rb
-
+ +
-
85.468
55
Cs
132.905
87
-
-
Fr
(223)
-
What group (family) do
these elements reside in?
Group (Family) Names
Alkali
Alkaline
MetalsEarth
Noble
Boron
Nitrogen
Carbon
Oxygen
Gases
GroupGroupGroupGroup
Halogens
Metals
Transition Metals
1
1
1
H
18
2
13 14
15 16
17
1.008
2
3
3
4
5
6
7
8
9
10
Be
B
C
N
O
F
Ne
6.941
9.012
11
12
Na
Mg
6
3
4
5
6
7
8
9
10
11 12
20.180
12.001
14.007
15.999
18.998
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
26.982
28.086
30.974
32.066
35.453
39.948
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
44.956
V
Cr
Mn
40.078
Ti
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
47.87
50.942
51.996
54.938
37
38
39
40
41
42
43
Rb
Sr
Y
Zr
Nb
Mo
85.468
87.62
92.906
95.94
Tc
88.906
91.224
(98)
55.845
44
Ru
101.07
58.933
58.69
63.546
65.39
69.723
72.61
74.922
78.96
79.904
83.80
45
46
47
48
49
50
51
52
53
54
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
102.906
106.42
107.868
112.4
114.818
118.710
121.760
127.60
126.904
131.29
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Ta
137.327
174.967
Hf
W
Re
Os
190.23
Ir
192.217
Pt
195.078
Au
Hg
200.59
Tl
204.383
Pb
207.2
Bi
208.980
Po
At
Rn
103
112
Uub
113
114
115
117
118
Uut
Uuq
Uup
116
Uuh
Uus
Uuo
(284)
(289)
(288)
68
69
70
132.905
7
24.305
10.811
19
39.098
5
4.003
Li
22.990
4
2
He
87
88
Fr
Ra
(223)
(226)
Lr
(262)
178.49
180.95
183.84
104
105
106
107
108
109
110
111
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
(266)
(264)
(269)
(269)
(272)
(261)
Lanthanides
Actinides
(262)
57
58
186.207
59
60
Nd
La
Ce
Pr
138.906
140.116
140.908
144.24
(268)
61
62
Pm
Sm
(145)
150.36
196.967
63
Eu
151.964
(285)
64
Gd
157.25
65
Tb
158.925
66
Dy
162.50
67
(209)
(292)
(210)
(222)
Er
Tm
164.930
167.26
168.934
173.04
Ho
Yb
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
232.038
231.036
238.029
(257)
(258)
(259)
(227)
(237)
(244)
(243)
(247)
(247)
(251)
(252)
Identify the Element
1
1
18
1
H
2
13 14
15 16
17
1.008
2
3
5
6
3
4
5
6
7
8
9
Be
B
14.007
O
15.999
F
9.012
12.001
N
6.941
10.811
C
18.998
11
12
13
14
15
16
17
18
Na
Mg
Al
Si
P
S
Cl
Ar
24.305
3
4
5
6
7
8
9
10
11 12
26.982
28.086
30.974
32.066
35.453
10
Ne
20.180
39.948
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Sc
40.078
44.956
Ti
47.87
V
50.942
Cr
Mn
39.098
Ca
51.996
54.938
Fe
Co
Ni
58.69
Cu
63.546
Zn
65.39
Ga
69.723
Ge
72.61
As
74.922
Se
78.96
Br
79.904
Kr
37
38
39
40
41
42
43
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Y
Zr
Nb
Mo
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
87.62
95.94
Rh
85.468
92.906
Tc
102.906
106.42
107.868
112.4
114.818
118.710
121.760
127.60
126.904
131.29
88.906
91.224
(98)
55.845
44
Ru
101.07
58.933
83.80
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Ta
137.327
174.967
Hf
W
Re
Os
Ir
Pt
Au
Hg
200.59
Tl
204.383
Pb
207.2
Bi
208.980
Po
At
Rn
103
112
Uub
113
114
115
117
118
Uut
Uuq
Uup
116
Uuh
Uus
Uuo
(284)
(289)
(288)
132.905
7
4.003
Li
22.990
4
2
He
87
88
Fr
Ra
(223)
(226)
Lr
(262)
178.49
180.95
183.84
190.23
192.217
195.078
104
105
106
107
108
109
110
111
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
(266)
(264)
(269)
(269)
(272)
(261)
Lanthanides
Actinides
(262)
186.207
(268)
196.967
(285)
(209)
(292)
(210)
(222)
57
58
59
60
61
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
140.116
140.908
164.930
167.26
168.934
Yb
138.906
144.24
Pm
173.04
89
90
91
Ac
Th
232.038
(227)
(145)
150.36
92
93
Pa
U
Np
231.036
238.029
(237)
151.964
157.25
94
95
Pu
Am
(244)
(243)
158.925
162.50
96
97
98
99
100
101
102
Cm
Bk
Cf
Es
Fm
Md
No
(257)
(258)
(259)
(247)
(247)
(251)
(252)
Carbon - C
Strontium
Astatine
- At
- Sr- Rf
Period 4
Group
17
2 –––Period
5
Group
Period2
14
76
 Rutherfordium
Using the Periodic Table
• The boxes that make up the periodic table contain a
significant amount of information. To understand this
information, it is necessary to refer to the periodic table’s
key(s)
8
Atomic Number
O
Element Symbol
Oxygen
Element Name
15.999
Class
Metal
Non-Metal
Metalloid
Color
Which class
does Oxygen
fall into?
(Number of protons)
(Written with a capital letter or a capital
followed by a lower case if two letters )
Atomic Mass
(Rounded to a whole number, equals
the number of protons and neutrons)
State
(@ Room Temp.)
Solid
Liquid
Gas
Symbol
Color
What is
Oxygen’s
physical state
of matter?
Compare:
He
H
Fr
Check for Understanding
• What is the smallest atom in regards to
mass in the periodic table? Circle it.
• What is the largest atom (in size in atomic
radius) in the periodic table? Put a dot by
it.
• What is the most massive atom in the
periodic table? Put a star by it.
• What is the most metallic element? Put a
box around it.
Check for Understanding
• What is the smallest atom in regards
to mass in the periodic table? H
• What is the largest atom (in size) in
the periodic table? Fr
• What is the most metallic element?
Put a box around it. Fr