Transcript Atomic Properties and the Periodic Table

Atomic Properties and the
Periodic Table
Metallic Property
Trend
 generally increases from top to
bottom of the periodic table
generally decreases from left to right
Metals are found in the left hand side
where as nonmetals are in the far
right hand of the periodic table
He
H
Li
Be
Na
Mg
K
Ca
Rb Sr
Cs
Ba
Fr
Ra
B
C
N
O F
Ne
Al
Si
P
S
Cl
Ar
Ge
As
Se
Br
Kr
Sb
Te
I
Xe
Po
At
Rn
Metals
 3 or less valence electrons
 Electron donor
 High densities and melting
temperature
 Oxides are often soluble in
acidic solution
 Good conductors
 Ductile and malleable
Non-metals
 5 or more valence electron
 Electron acceptor
 Low densities and melting
points
 Oxides are soluble in basic
solutions
 Poor conductors
 Not shiny,malleable and
ductile
Atomic Size
Trend
Top to bottom increases
Left to right decreases
Reasons
Due to additional energy level as you
go down
Due to increasing nuclear charge
Ionization Energy
Amount of energy required to remove
the electrons in an atom
Trend
top to bottom decreases
 Left to right increases
Ionic Size
When an atom combine with another
atom to form cation, are always
smaller than their atom
Anions are always bigger than their
atom Mg + O
Mg2+
O2-
Classwork
Using a periodic table, classify each element as
metal or nonmetal
Mg, K, Si, Br, Mn
Arrange the following elements into increasing
metallic property
Ba, Sr, Be,Mg, Ca & Ra
In each of the following sets, tell which will be
the largest
a) S, S2-
b) Al, Al 3+ c) Ca, Ca2+, Se, Se2+
Arrange the following elements into decreasing
ionization energy
a) P, Si,Ar, Cl & Al
b) Rb, K, Cs, Na, Fr, Li
Homework
In each set which one has the
highest ionization energy?
a) He, Ne, Ar, Kr
b) Mg, As, Al, F
c) K, K+, Ca, Ca2+
Arrange the trends in atomic size in
increasing order for the following
ions:
Be2+, Mg2+, Ca2+ & Sr2+
Additional Practice
Arrange the succeeding elements
according to increasing atomic size
Ar, S2-, P3-, Mg2+
Answer the focus questions 3 through
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