Periodic table

The Periodic Table
and the Elements

Penny Squires
Pisgah High School
2005
3.3 Periodic Table 9.17.00 1:37 PM

The Periodic Table and the Elements
What is the periodic table ?
What information is obtained from the table ?
How can elemental properties be predicted base on the PT ?


Dmitri Mendeleev (1869)
In 1869 Mendeleev and Lothar Meyer (Germany)
published nearly identical classification schemes
for elements known to date. The periodic table is
base on the similarity of properties and reactivities
exhibited by certain elements. Later, Henri
Moseley ( England,1887-1915) established that
each elements has a unique atomic number, which
is how the current periodic table is organized.

http://www.chem.msu.su/eng/misc/mendeleev/welcome.html

Periodic Law

The Periodic Law states that when elements are
arranged in order of increasing atomic number
their physical and chemical properties show a
periodic pattern.


The Periodic Table
A map of the building block of matter.
1 18
IA VIIIA
1 H
1 2
IIA
Periodic Table 13
IIIA
14
IVA
15
VA
16
VIA
17
VIIA He
2

1.00797 4.0026
3 4 5 6 7 8 9 10
2 Li Be B C N O F Ne
6.939 9.0122 10.811 12.0112 14.0067 15.9994 18.9984 20.179
11 12 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
3 Na Mg IIIB IVB VB VIB VIIB VIIIB IB IIB Al Si P S Cl Ar
22.9898 24.305 26.9815 28.086 30.9738 32.064 35.453 39.948
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
39.102 40.08 44.956 47.90 50.942 51.996 54.9380 55.847 58.9332 58.71 63.54 65.37 65.37 72.59 74.9216 78.96 79.909 83.80
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
85.47 87.62 88.905 91.22 92.906 95.94 [99] 101.07 102.905 106.4 107.870 112.40 114.82 118.69 121.75 127.60 126.904 131.30
55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
132.905 137.34 138.91 178.49 180.948 183.85 186.2 190.2 192.2 195.09 196.967 200.59 204.37 207.19 208.980 [210] [210] [222]
87 88 89 104 105 106 107 108 109
7 Fr Ra Ac Ku http://www.chemsoc.org/viselements/pages/periodic_table.html
[223] [226] [227] [260]


Arrangement
The modern Periodic Table is arranged
according to atomic number.

Remember that it is the atomic number,
or nuclear charge, that determines
the identity of the element.


Periodic Table Expanded View
The way the periodic table usually seen
is a compress view, placing the
Lanthanides and actinides at the
bottom of the stable.


Periodic Table: Metallic arrangement
Layout of the Periodic Table: Metals vs. nonmetals
1 18
IA VIIIA
2 13 14 15 16 17
1 IIA IIIA IVA VA VIA VIIA

2

3 4 5 6 7 8 9 10 11 12
3 IIIB IVB VB VIB VIIB VIIIB IB IIB

4
Nonmetals
5 Metals
6

7


METALS

Hard and Shiny

3 or less valence electrons

Form + ions by losing e-

Good conductors of heat and electricity


NONMETALS

Gases or dull, brittle solids

5 or more valence electrons

Form - ions by gaining e-

Poor conductors of heat and electricity


Metalloids

Appearence will vary

3 to 7 valence electrons

Form + and/or - ions

Conduct better than nonmetals but not as well as
metals


Periodic Table: The three broad Classes
Main, Transition, Rare Earth
Main (Representative), Transition metals, lanthanides and actinides (rare earth)


Reading the Periodic Table: Classification
Nonmetals, Metals, Metalloids, Noble gases


Across the Periodic Table
Periods: Are arranged horizontally across the
periodic table (rows 1-7)
1 These elements have the same number of valence shells. 18
IA VIIIA
2 13 14 15 16 17
1 IIA IIIA IVA VA VIA VIIA

2nd Period
2

3 4 5 6 7 8 9 10 11 12

4

5

6th Period
6

7


s block p block

d block

f block

3


Down the Periodic Table
Family: Are arranged vertically down the periodic table
(columns or group, 1- 18 or 1-8 A,B)
These elements have the same number electrons in the outer most
shells, the valence shell.
1 18
IA VIIIA
2 Alkali Family:
Alkali Family: 13 14 15 16 17
1 IIA
11e- in the valence shell
e- in the valence shell
IIIA IVA VA VIA VIIA

2

3 4 5 6 7 8 9 10 11 12

4
Halogen Family:
Halogen Family:
5 77e- in the valence shell
e- in the valence shell

6

7


Infamous Families of the Periodic Table
Notable families of the Periodic Table and some important members:
Alkali Halogen
Noble Gas
Alkaline Chalcogens
1
IA
(earth) 18
VIIIA
2 13 14 15 16 17
1 IIA
Transition Metals IIIA IVA VA VIA VIIA

2

3 4 5 6 7 8 9 10 11 12

4

5

6

7


Hydrogen:

A Unique Element 1s1
Shown Over Group 1A & 7A
Hydrogen is neither an alkali metal nor a
halogen
 However, hydrogen does show reactions
that are
similar to both alkali metals and
halogens

H. + .
Cl : H : Cl :

Hydrogen can also gain an electron to form an ion with a 1 - charge

H. + e- H: -
or H- called hydride


Group 1A: Alkali Metals
React with water easily to lose a valence electron.

Form a +1 ion

Soft

Found in nature combined with other elements

Good conductors of heat and electricity


Group 2A: Alkaline Earth Metals
Forms compounds with Oxygen (Oxides)

React with water

Shiny solids that are heavier than Alkalis

React with Oxygen or other metals found in the earth

Lose valance electrons to form +2 ions
Ca (g) Ca+ (g) + e- First Ionization Step

Ca+ (g) Ca2+ (g) + e- Second Ionization Step


Group 3A: Boron Group
Always found combined with other elements in
nature.

Found as oxides in the earth’s crust.

B, Al, Ga, and In form +3 ions

Tl only forms a +1 ion


Group 4A: Carbon Group
Few rules apply to this group!!!!


Group 5A: Nitrogen Group
Wide variety of Chemical and Physical properties.

N forms a –3 ion

Bi forms a +3 ion


Group 6A: Oxygen Group or
Chalcogens
Act like nonmetals

Tend to gain 2 e- to form –2 ions.

Can also share 2 e-


Group 7A: Halogens
Form compounds with almost all metals

Salts (NaCl)

Have different Physical properties

Very reactive and found combined in nature

Tend to share or gain 1 e- to form a –1 ion


Group 8A: Noble Gases
•Colorless

•Unreactive

•Last to be discovered

•Rarely react (1st time was in a lab in 1962)


Rare Earth Metals
1. Lanthanides –
Named because they follow lanthanum
Silvery metals with high melting points
Found mixed in nature – very hard to seperate

2. Actinide –
Named because they follow actinium
Radioactive elements
Only 3 exist in nature – the rest are synthetic


Transition Metals
Share conductivity, luster and malleability with
other metals.

Closein atomic size, electronegativity and ionization
energy

Different physical properties (determined by their
electron configuration)

Can lose 2 e- to form +2 ion or 3 to form a +3 ion

Ifthey form more than one type of ion the element
will have a different color when combined.

Periodic Table
e- configuration from the periodic periodic table

1 18
IA VIIIA
2 13 14 15 16 17
1 H IIA IIIA IVA VA VIA VIIA He
1s1 1s2
2 Li Be B BC N O F Ne
2s1 2s2 2p1 2p 2p 2p4
1
2 3 2p5 2p6
3 Na Mg
3
IIIB
4
IVB
5
VB
6
VIB
7
VIIB
8 9
VIIIB
10 11
IB
12
IIB Al Si P S Cl Ar
3s1 3s2 3p1 3p2 3p3 3p4 3p5 3p6
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Be Kr
4s1 4s2 3d1 3d2 3d3 4s13d5 3d5 3d6 3d7 3d8 4s13d10 3d10 4p1 4p2 4p3 4p4 4p5 4p6
5 Rb Sr Y Zr Nb Mo Tc Ru Rh Ni Ag Cd In Sn Sb Te I Xe
5s1 5s2 4d1 4d2 4d3 5s14d5 4d5 4d6 4d7 4d8 5s14d10 4d 10
5p1 5p2 5p3 5p4 5p5 5p6
6 Cs Ba La Hf Ta W Re Os Ir Ni Au Hg Tl Pb Bi Po At Rn
6s1 6s2 5d1 5d2 5d3 6s15d5 5d5 5d6 5d7 5d8 6s15d10 5d 10
6p1 6p2 6p3 6p4 6p5 6p6
7 Fr Ra Ac Rf Db Sg Bh Hs Mt
7s1 7s2 6d1 6d2 6d3 7s16d5 6d5 6d6 6d7


Periodic Table: electron behavior
The periodic table can be classified by the behavior of their electrons

West (South) Mid-plains East (North)
METALS METALLOID NON-METALS
Alkali Noble gas
Alkaline Halogens
Transition Calcogens
These elements These elements These elements
tend to give up will give up e- or tend to accept
e - and form accept e- e - and form
1
CATIONS ANIONS 18
IA VI A
II
2 13 14 15 16 17
1 IA
I II
IA I A
V VA VA
I VI
IA

2

3 4 5 6 7 8 9 10 11 12
3 II
IB I B
V VB VB
I VI
IB VI B
II IB IB
I

4

5

6

7


2. Trend in Atomic Radius
Atomic Radius:
The size of at atomic species as
determine by the boundaries of the
valence e-.
Largest atomic species are those
found in the lower left corner since
these atoms have the largest n.


Trend in Ionic Radius
Ionic Radius:
Atoms can gain or lose electrons to
form ions.

Electrons are negative so if they gain
or lose one they will have a charge.
(Cation = lose to form + ion/becomes
smaller
and
Anion = gains to form – ion/becomes
larger)


Ionic Radius (cont.)


3. Trend in Ionization Energy
Ionization potential:
The energy required to remove the
valence electron from an atomic
species. Largest toward top right
corner of PT since these atoms hold
on to their valence e- the tightest.


4. Trend in Electron Affinity

Electron Affinity:
The energy release
when an electron is
added to an atom.
Most favorable
toward NE corner of
PT since these atoms
have a great affinity
for e-.


Summary of Trend
Periodic Table and Periodic Trends
1. Electron Configuration 3. Ionization Energy: Largest toward NE of PT
4. Electron Affinity: Most favorable NE of PT

2. Atomic Radius: Largest toward SW corner of PT

Summary

Periodic Table: Map of the Building block of matter
Table
Type: Metal, metalloid and Nonmetal
Type
Groupings: Representative or main, transition and
Lanthanide/Actanides
Family: Elements in the same column have similar
Family
chemical property because of similar valence
electrons
Alkali, Alkaline, chalcogens, halogens, noble gases
Period: Elements in the same row have valence
electrons in the same shell.


Periodic table

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