56
Made the FIRST periodic table
Made the FIRST periodic table
1869 Mendeleev organized
the periodic table based on
the similar properties and
relativities of certain
elements
Later, Henri Moseley
organized the elements by
increasing atomic number
Periodic Table
Kr
Xe
Rn
Ar
Ne
He
8A
CaK Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Periods: the rows in the
periodic table
Groups: the
columns in the
periodic table
Elements in the
same group have
similar chemical
properties
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Main Group or
Representative
Elements
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Transition
Metals
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Lanthanide Series
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Actinide Series
ALKALI METALS
ALKALINE EARTH METALS
CHALCOGENS
HALOGENS
NOBLE GASES
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Alkali Metals
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Alkaline Earth
Metals
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Halogens
H
Li Be
Na Mg
CaK
Rb
Cs
Fr Ra
Ba
Sr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
XeITeSbSnInCdAgPdRhRuTcMoNbZrY
La
Ac Rf
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Db Sg Bh Hs Mt
LuYbTmErHoDyTbGdEuSmPmNdPrCe
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Ar
Ne
He
F
ClSPSiAl
B C N O
Noble Gases
AtPo
TeSb
AsGe
Si
B
METALS
METALLOIDS
NONMETALS
Metals
Left side of the periodic table
except H
Properties:
lustrous (shiny)
good thermal and electrical conductors
malleable
solids at RT
except Hg = liquid
Non-Metals
Right side of table
plus H
Properties:
Dull appearance
Brittle when solid
Do not conduct heat or electricity well
Primarily solids or gases at RT
Bromine = liquid
Metalloids
Stair step between metals and non-metals
Properties in between metals and non-metals
Si: brittle but semi-conductor
S
P
D
F
1. Aufbau Principle - an electron occupies the lowest-energy orbital that can receive it
3d
3p
3s
2p
2s
1s
Energ
y
2. Pauli Exclusion Principle - no two
electrons in the same atom can have the
same set of four quantum numbers
**Opposite spin states!!**
1s
3. Hund’s Rule – orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state
3p
Each electron has its own orbital
All are in the same spin state
Shortcut (shortened) Notation:
Use closest Noble Gas before the element
For bromine:
Closest Noble Gas before the element:
Argon:
Shortcut Notation:
1s22s22p63s23p6
1s22s22p63s23p6
[Ar] 4s23d104p5
4s23d104p5
• For sodium:
• For potassium:
[Ne]3s1
[Ar]4s1
1 valence electron!
1 valence electron!
For aluminum:
For gallium:
[Ne]3s23p1
[Ar]4s23d104p1
3 valence electrons!
3 valence electrons!
For chlorine:
For bromine:
1s22s22p63s23p64s23d104p5
1s22s22p63s23p5
7 valence electrons!
7 valence electrons!
A way to represent the number of valence
electrons an atom contains
Number of Electrons in the
Ending Configuration
Lewis Dot Diagram
1 Li
2 Mg
3 Al
4 Si
Number of Electrons in the
Ending Configuration
Lewis Dot Diagram
5 N
6 O
7 F
8 Ne
A few exceptions:Chromium
Would expect: 1s22s22p63s23p64s23d4
Actually: 1s22s22p63s23p64s13d5
1s 2s 2p 3s 3p
4s 3d
Periodicity – We can tell a lot about
particular properties of elements
simply based upon where they are on
the periodic chart.
There are five general trends that
can be predicted: atomic size,
ionization energy, electronegativity,
electron affinity, and reactivity.
It all relates to something called effective nuclear charge Zeff.
Think of the effective nuclear charge as the pull that the outer electrons feel from the nucleus.
Nuclear pull: The pull/attraction between the + protons and the – electrons.
Atomic Radius
Measures the size of an atom
Measured from one nucleus to the next
K has 19 +
charges
Br has 35 +
charges
As you go from left to right, the pull on the
outer electrons (from the nucleus) is greater. It
requires more energy to hold onto those
electrons, which causes the atomic size to be
smaller.
ATOMIC SIZE DECREASES
As you move
down the chart,
the number of
energy levels
increases.
Therefore, as you move down the chart the atomic size
increases.
http://encarta.msn.co
m
Ignore noble gases when going left to
right.
Memorize fluorine as the smallest
element on the chart.
Memorize francium as the largest
element on the chart.
Ionic Radius
The size of ions (charged atoms resulting from a change
in electrons)
1+2-
+: Cation: lost electron(s)
-: Anion: gain electron(s)
+2 < +1 < 0 < -1 < -2
•The amount of energy required to remove
valance electrons.
•The amount of energy required to create an
ion.
•The greater the effective nuclear charge (Zeff),
the tighter the valance electrons are being held.
•The tighter the electrons are being held, more
energy is required to remove them.
The amount of energy required to remove the
outermost electron from an atom
http://nanotech.sc.mahidol.ac.th/genchem/bonding1/ie.jpghttp://www.physchem.co.za/Atomic/Periodicity.htm
Zeff increases
Ionization Energy increases
Effective nuclear
charge decreases
(Zeff).
Ionization energy
decreases.
As the valance electrons get farther away, the force of attraction (Zeff)
between the nucleus and the electrons gets weaker. Thus, less energy is
required to remove the electrons. F will have the highest IE and Fr will
have the lowest.
• Affinity tends to increase across a period
• Affinity tends to decrease as you go down
a group
•Electrons farther from the nucleus
experience less nuclear attraction
•Some irregularities due to repulsive
forces in the relatively small p orbitals
Zeff increases
Electron Affinity increases
Effective nuclear
charge decreases
(Zeff).
Electron Affinity
decreases.
The attraction an atom has for an electron in a
bond
Increases with an increased effective nuclear
charge.
Decreases
with a
decreased
effective
nuclear
charge.
Defined as how easily an atom can lose or gain
electrons in order to complete the octet.
Metals will lose electrons until they’re left with
8 valance.
Nonmetals will gain electrons until they’re left
with 8 valance.
Metalloids can do both.
Since metals lose electrons, reactive metals are those
metals that can easily lose their electrons.
Reactivity decreases with increased
Zeff
Reactivity
increases
with
decreased
Zeff
Nonmetals gain electrons to complete the
octet.
Smaller nonmetals can gain electrons easier
than larger nonmetals due to an increased
effective nuclear charge (Zeff).
Summation of Periodic TrendsZeff, IE, and EN follow the same trends. Atomic Radius is opposite.
Electronegativity
