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I II III
The Periodic Table
Chemical Reactivity
Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases
Chemical Reactivity
Period/RowFamilies/Groups/Columns
Elements in the same family has the SAME # of valence electrons
1
2
3
4 5
6
7
Atomic Radius is the distance from the nucleus to the outermost orbital
Increases to the LEFT and DOWN
Atomic Radius
Why larger going down?
Higher energy levels have larger orbitals
Why smaller to the right?
Increased nuclear charge
Atomic Radius
Which atom has the larger radius?
Be or Ba
Ca or Br
Ba
Ca
Examples
Ionization Energy- the energy required to remove 1 electron from the parent atom
Why opposite of atomic radius?
In small atoms, e- are close to the nucleus where the attraction is stronger
Ionization Energy
1
2
3
4
5
6
7
First Ionization Energy Increases UP and to the RIGHT
Ionization Energy
Which atom has the higher 1st I.E.?
N or Bi
Ba or Ne
N
Ne
Examples
1
2
3
4 5
6
7
Melting/Boiling Point – the temperature at which a substance changes states
Highest in the middle of a period.
Melting/Boiling Point
Which atom has the higher melting/boiling point?
Li or C
Cr or Kr
C
Cr
Examples
Ionic Radius
The distance between the center of the nucleus and the outer edge of the ion
Cations/Metals
-lose elections, so they have a positive charge
-small
Atoms
-neutrally charged elements
-medium
Anions/Nonmetals
-gain electrons, so they have a negative charge
-large
Electronegativity
*The measure of how strongly an atom attracts electrons when it is combined with another element
• Increases from left to right (except for noble gases) due to increased nuclear charge
• Increases as you move up a group due to the shorter distance between the nucleus and valence electrons.
Increases UP and to the RIGHT
1
2
3
4 5
6
7
Which particle has the largest electronegativity?
S or P
Al or Ga
S
Al
Examples