Transcript Elements and the Periodic Table

Chapter 6
Elements and
the Periodic
Table
Development of the Periodic
Table
• Lavoisier compiled a list of 23
elements in the 1790s
• In 1864 John Newlands
arranged the known elements
by increasing atomic mass
The Periodic Table
• By 1850, approximately 60
elements are known
• Dmitri Mendeleev in 1869
publishes the first periodic
table
– Lists the physical and
chemical properties of the
known elements
– Places elements with
similar properties in
families
Mendeleev’s Periodic Table
GRUPPE I
GRUPPE II
GRUPPE III
GRUPPE IV
GRUPPE V
GRUPPE VI
GRUPPE VII
GRUPPE VIII
R2O
RO
R2O3
RO2
RH4
R2O5
RH3
RO3
RH2
RH
R2O7
RO4
H=1
1
Be = 9.4 B = 11
C = 12
N = 14
O = 16
F = 19
2 Li = 7
Na = 23 Mg = 24
Al = 27.3
Si = 28
P = 31
S = 32
Cl = 35.5
3
Ca = 40
- = 44
Ti = 48
V = 51
Cr = 52
Mn = 55
Fe = 56, Co = 59
4 K = 39
Ni = 59, Cu = 63
Zn = 65
As = 75
Se = 78
Br = 80
5 (Cu = 63)
- = 68
- = 72
Sr = 87
?Yt = 88
Zr = 90
Nb = 94
Mo = 96
Ru = 104, Rh = 104
6 Rb = 85
- = 100
Pd = 106, Ag = 108
In = 113
Sn = 118
Sb = 122
Te = 125
7 (Ag=107) Cd = 112
8 Cs = 133 Ba = 137 ?Di = 138 ?Ce = 140 -
J = 127
- - - -
(La)
9
10 -
(-)
-
-
-
-
-
?Er = 173 ?Lu = 180 Ta = 183
W = 184
(Yb)
Ti = 204
Pb = 207
Bi = 208
11 (Au=199) Hg = 200
Th = 231
U = 240
12 -
Os = 195, Ir = 197
Pt = 198, Au = 199
-
- - - -
Published in 1871, St. Petersburg, Russia by Dmitrii I. Mendeleev
Why Repeating Patterns?
• The part of the atom another atom sees is
the electron cloud.
• More importantly the outside orbitals.
• The orbitals fill up in a regular pattern.
• The outside orbital electron configuration
repeats.
• The properties of atoms repeat.
H
Li
1
3
Na
11
K
19
Rb
37
Cs
55
Fr
87
1s1
1s22s1
1s22s22p63s1
1s22s22p63s23p64s1
1s22s22p63s23p64s23d104p65s1
1s22s22p63s23p64s23d104p65s24d10
5p66s1
1s22s22p63s23p64s23d104p65s24d105p66s2
4f145d106p67s1
1s2 He 2
Ne
2
2
6
1s 2s 2p
10
1s22s22p63s23p6 Ar18
1s22s22p63s23p64s23d104p6 Kr
36
1s22s22p63s23p64s23d104p65s24d105p6 Xe
54
1s22s22p63s23p64s23d104p65s24d10 Rn
5p66s24f145d106p6 86
Henry Moseley
• Upon the discovery of new elements,
Mendeleev’s table was proven incorrect
• In 1913, Moseley discovered that
elements contain a unique number of
protons
• Moseley arranged the elements according
to atomic number which resulted in a clear
periodic pattern of properties
The Modern Periodic Table
• Periodic law - periodic repetition of
chemical and physical properties of the
elements when arranged by increasing
atomic number
• groups/families - columns on periodic table
• periods - rows on the periodic table
The known elements
112 elements are currently known
• 89 are metals
• 11 occur as gases
• 2 occur as liquids
• 31 are radioactive
• 22 are synthetic (all radioactive) video
– Let’s take a look at them on the table.
The Modern Periodic Table
Why do we have those
rows at the bottom?
H
He
Li Be
B
Na Mg
Al Si P
C
N
O
F Ne
S Cl Ar
K Ca Sc
Ti
Rb Sr Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
I
Xe
Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
This arrangement takes too
much space and is hard to read.
Periods
H
He
Li Be
B
Na Mg
Al Si P
C
N
O
F Ne
S Cl Ar
K Ca Sc
Ti
Rb Sr Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
I
Xe
Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
There are 7 periods represented on the
Periodic Table
Main-group elements are also called
Representative elements.
Elemental states at
room temperature
Solid
Liquid
Gas
H
Li
He
Be
B
C
N
O
F
Ne
Na Mg
Al
Si
P
S
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
K
Ca Sc
Rb Sr
Y
Ti
V
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba *Lu Hf Ta W Re Os
Ir
Xe
Pt Au Hg Tl Pb Bi Po At Rn
+
Fr Ra Lr
I
*
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb
+
Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No
Three Main Classifications for
the Elements
• Metals
• Nonmetals
• Metalloids (Semimetals)
Metals, Metalloids or
(Semimetals) & Nonmetals
H
Li
He
Be
B
C
N
O
F
Ne
Na Mg
Al
Si
P
S
Cl
Ar
K
Ca Sc
Rb Sr
Y
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba *Lu Hf Ta W Re Os
Ir
Xe
Pt Au Hg Tl Pb Bi Po At Rn
+
Fr Ra Lr
I
*
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb
+
Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No
Metals
• Shiny when smooth
and clean
• Good conductor of
electricity
• solid at room temp.
except for Hg
• Good conductor of
heat
• ductile
• malleable
Nonmetals
• Generally gases at room temperature
• Brittle, dull looking solid
except Bromine Br is a liquid
• poor conductors of heat and electricity
Metalloids
• Have characteristics of metals and
nonmetals
• Silicon and Germanium are the two most
important (Computers… Silicon Valley)
• Video
Groups are assigned
Roman numerals
with an A or B
IA
A group or family
II A
III A IV A V A VI A VIIA VIIIA
He
H
Li
Be
B
C
N
O
F
Ne
Al
Si
P
S
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
Na Mg III B IVB V B VIB VIIB
K
Ca Sc
Rb Sr
Y
Ti
V
IB
IIB
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba Lu Hf Ta W Re Os
Fr Ra Lr
VIII
Ir
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb
Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No
Hydrogen
• One valence
electron
• Is its own group
• Has properties
of metals and
nonmetals
Alkali metals
Alkaline earth metals
Common group names
Halogens
Noble gases
IA
II A
III A IV A V A VI A VIIA VIIIA
H
Li
He
Be
B
C
N
O
F
Ne
Al
Si
P
S
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
Na Mg III B IVB V B VIB VIIB
K
Ca Sc
Rb Sr
Y
Ti
V
IB
IIB
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba Lu Hf Ta W Re Os
Fr Ra Lr
VIII B
Ir
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb
Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No
Group 1/IA: Alkali Metals
• One valence electron
• highly reactive
• Form 1+ ions
• Video
Group 2/IIA: Alkaline Earth Metals
• 2 valence electrons
• harder than alkali metals
• less reactive than alkali metals
• Forms a 2+ ion
Group 13/IIIA: Boron
• 3 valence electrons
• Always found combined with
other elements in nature
• Most form a 3+ ion video
Group 14/IVA: Carbon Group
• 4 valence electrons
• A wide variety of characteristics
• Allotropes - forms of an element in the
same physical state that have different
structures and properties (graphite and
diamond)
Group 15/VA: The Nitrogen Group
• 5 valence electrons
• gain three electrons
to form a 3- ion
Group 16/VI: The Oxygen Group
• 6 valence electrons
• Act as nonmetals
• Gain 2 electrons to form 2ion
Group 17/VIIA: Halogens
• 7 valence electrons
• “salt formers”
• Gain 1 electron to form a 1- ion
• Most reactive nonmetals
Group 18/VIIIA: Noble Gases
• 8 valence electrons
• colorless and unreactive
• Most stable elements
Transition Metals, d-block
• Groups 3-12, d-block members
• electrical conductivity, luster, and
malleability
• Video1, Video 2
Inner Transition Metals,
f-block
• lanthanide - f-block elements in period 6
• actinide - f-block elements in period 7
Metal Locations Around the World
The Elements in the Human
Body
Carbon
Hydrogen
Oxygen
Nitrogen
Calcium
Phosphorus
Sulfur
Potassium
Sodium
Chlorine
Iron
23%
10%
61%
2.6%
1.4%
trace
trace
trace
The Elements in the Human
Body Dry Weight
Voet Biochemistry
Carbon
62%
Hydrogen
9.3%
Oxygen
11%
Nitrogen
5.7%
Phosphorus
3.3%
Sulfur
1.0%
Percent dry weight
Calcium
Potassium
Sodium
Chlorine
Iron
5.0%
1.3%
trace
trace
trace