Transcript The Periodic Table/Trends Chapter 5

The Periodic Table
and
Periodic Trends
Chapter 5
Standard #1:
Atomic and Molecular Structure
THE FAMILIES OF THE PERIODIC TABLE
Alkaline Earth Metals
Alkali Metals
B
Si
Ge As
Transition
Metals
Sb
Inner Transition Metals
Te
Po
Noble Gases
Halogens
Metalloids/
Semi-metals
At
The Blocks of the periodic table
The valence electrons
spin in a sphere
sblock
The valence
electrons spin in a
four lobe pattern
d-block
f-block
Too complex
The valence
electrons spin a
figure 8 pattern
p-block
RIDDLE:
What does Sodium Oxide and
Rihanna have in common?
They both
are called
Oh Na Na
Some Facts about the periodic table:
II.
III.
FAMILY /GROUP
PERIOD
18 vertical columns
7 Horizontal rows
Can you do this??
Tom Lehrer
the elements song
pianist, musician and retired
mathematician ,
UC Santa Cruz
Take out a sheet of paper
Characteristics of METALS
1. GOOD Conductors of heat and electricity
2. Solid at Room Temperture
Except Mercury (Hg)
3.Malleable
(to make into
sheets)
Pure
Copper Metal
4. Ductile
(to make into a
wire)
chemical properties of metals video
Characteristics of Non-Metals
1.Poor Conductors of heat and electricity
2.Mostly Gases
Iodine
Chlorine
4. Texture Varies
Carbon
Bromine
Sulfur
Carbon
chemical properties of
non metals video
The Metalloids or Semimetals
have some characteristics of both
1.
2.
3.
Can be shiny or dull.
Some are malleable/ductile.
Some conduct heat and electricity.
Silicon
Johann Dobereiner
Try Ni 59
Pd X
Pt 195
You can calculate the mass of the middle
element by knowing the one above it an below it!
John Newlands
Law of OCTAVES
He arranged the 62 known
elements in order of
increasing atomic weights
Every 8th
element repeats
in pattern
A.K.A
The
Father
of
Chemistry
Gets credit for publishing the
First Periodic Table
Mendeleev’s Periodic table
Henry Moseley
Corrected periodic table by arranging it
according to the atomic number.
Video Organizing the Elements
Mendeleevs Table clip
Stop!
Review of metals/Non-metals
Video clips
Review before the
periodic trends
Periodic Trends
A.The Atomic Radius: The distance from the center of the
nucleus to the valence electron.
1. Down a group
Going down a group, the
electron orbitals (shell)
increase, causing the radius
to get BIGGER!
2.
Going Across the (period)
There is a greater attraction which will
cause the radius to get smaller.
Ionic Radius:. The distance from center of nucleus to
valence electron for the ion.
1.
Cation: An atom that loses electrons (+)
e-
The cation is smaller than the
original atom because it
loses an electron and orbital.
atomic radius: .152nm
ionic radius (1+ ion): .060nm
1.
Anion: An atom that gains electrons (-)
F-1
anion
-
F atom
e-
-
-
-
-
-
The anion will be larger than the atom because
it will have greater electron repulsion
anion
cation
atom
atom
C.
Ionization Energy
1.
The amount of energy needed to
remove an electron (to make a
cation)
Going down a Family:
Requires LESS Ionization
Energy because valence
electron is further away from
the nucleus.
1. Going across a period:
It takes MORE ionization energy
because the electrons are held closer
to the nucleus.
Can Lithium lose more than 1 electron?
.
.
.
Li +1
(looks like He with 2 e-)
520.2
KJ/mol
7290.1
KJ/mol
11,815.0
KJ/mol
Li+3 (11,815.0KJ/mol)
Li+2 (7298.1KJ/mol)
Li+1 (520KJ/mol)
Electronegativity:
Reflects the atoms ability to attract electrons
A.
Going down a family:
NOT attracting electrons….too big
and wants to get rid of electrons
High electronegativity
Low
electronegativity
B.
Going across a period:
Has a high attraction for electrons…
.small and needing electrons
Fluorine
_____________is
the most
electronegative element
Francium
and _______________is
the least