Download Periodic Table

Periodic Table
DEVELOPMENT OF MODERN TABLE
METALS VS. NONMETALS
GROUPS VS. PERIODS
TRENDS
GLENCOE SCIENCE CHEMISTRY
Development of the Modern Periodic Table
 Antoine Lavoisier (late 1700s)
Organized the 33 known elements into four categories.
 List what the categories are and give examples: (look on pg 174, table 6.1)
 ________________________________________________
 ________________________________________________
 ________________________________________________
 ________________________________________________
 John Newlands (look on pg 176, table 6.2)
 Arranged elements by ___________________________________
 Noticed the repetition of properties every ______________________
 Created the law of ___________ which means (look on pg. 175)
___________________________________________________

Development of the Modern Periodic Table
 Lothar Meyer
 Demonstrated a connection between ________________
and _______________________
 Arranged the elements in order of increasing ___________
 Dmitri Mendeleev
 Demonstrated a connection between ________________
and _______________________
 Arranged elements in order of _____________________
 ________ the existence and properties of _____________
elements
 Who usually gets more credit for their work?
Cont.
 Henry Moseley
 Discovered that atoms contain a unique number of ________
called the _______________________
 Arranged elements in order of increasing
______________________________ which resulted in
a _________________ of properties
The Modern Periodic Table
 Consists of squares or boxes
 Arranged in order of increasing ______________
 Columns are called ________ or ____________
 There are _____ columns numbered from left to ________
 Columns also have names for their families. On your periodic
table, write the names above each column.
 Rows are called ___________
 There are ____ rows.
 But there are two rows that seem to be out of place. They are
the ______________ and _____________ series
These Are the Elements

http://www.sciencegeek.net/tables/tables.shtml
Metals vs. Nonmetals
Metals (pg. 177)
 Location


Groups 1-12; part of
groups 13-15
Always left of the stairstep
 Physical Properties

List physical properties of
metals
 Chemical Properties

List chemical properties
Nonmetals (pg. 179)
 Location
Most are _____ of the stairstep except _____
 Found in groups
_________________
 Physical Properties


List physical properties of
nonmetals
 Chemical Properties

List chemical properties
Metals, Nonmetals, Metalloids
Metals, Nonmetals, Metalloids
 There is a zig-zag or
staircase line that
divides the table.
 Metals are on the left
of the line, in blue.
 Nonmetals are on
the right of the line,
in orange.
Metals
 Metals are lustrous
(shiny), malleable,
ductile, and are good
conductors of heat
and electricity.
 They are mostly
solids at room temp.
 What is one
exception?
Nonmetals
 Nonmetals are the
opposite.
 They are dull, brittle,
nonconductors
(insulators).
 Some are solid, but
many are gases, and
Bromine is a liquid.
Metalloids
 Metalloids, aka semi



metals are just that.
They have characteristics
of both metals and
nonmetals.
They are shiny but brittle.
And they are
semiconductors.
What is our most
important semiconductor?
Periodic Table Trends
 Atomic numbers are at the ________ of each square and go





in order 1-118
Each element has its own symbol and an average atomic
_____________
Elements tend to get ___________ in atomic radius as you
go down the group.
Atomic number gets larger as you go across the row from
_________to _________ (period) and down the _______.
Some of the elements are named after ________, _______,
countries, and their Latin or Greek names.
Hydrogen and Helium are separate from the other elements
in their group. Why?
The Periodic Law
 Atoms with similar properties appear in groups or
families (vertical columns) on the periodic table.
 They are similar because they all have the same
number of valence (outer shell) electrons, which
governs their chemical behavior.
Periodic Trends
 The first and most important is atomic radius.
 Radius is the distance from the center of the
nucleus to the “edge” of the electron cloud.

Atomic radii are usually measured in picometers (pm) or
angstroms (Å).
A picometer is 1 x 10-12 m.
 An angstrom is 1 x 10-10 m.

Atomic Radius – Family Trend
 The trend for atomic radius in a vertical column is to
go from smaller at the top to larger at the bottom of
the family.
 Why?
 With each step down the family, we add an entirely
new principal energy level (PEL) to the electron
cloud, making the atoms larger with each step.
Atomic Radius
 On your help sheet, draw arrows like this:
Atomic Radius – Help Sheet
How big is an atom?
Atomic radius decreases across a period from left to right due to
increased effective nuclear .charge (ENC).
Atomic radius increases down a group because of the addition
of more energy levels.
Atomic Radius
Arrange the following sets of atoms in order of increasing size:
Se, Sr, Ne:
Na, Ba, F:
La, C, Pd
Ne < Se < Sr
Review so far
 http://www.chemistryland.com/CHM151S/02-
Atoms/Chaos/Chaos.htm
Ions
 Elements can __________ or ___________
electrons.
 Atoms that gain electrons:


Nonmetals
Called anions
 Atoms that lose electrons:
 Metals
 Called cation
 To gain or lose electrons, __________ is required.
 CW/HW complete ionization practice worksheet.
Ions
 Here is a simple way to remember which is the cation
and which the anion:
+
This is Ann Ion.
She’s unhappy and
negative.
+
This is a cat-ion.
He’s a “plussy” cat!
Cation Formation
Na atom
Remaining e- are
pulled in closer to
the nucleus. Ionic
size decreases.
1 valence electron
Valence elost in ion
formation
Result: a smaller
sodium cation, Na+
11p+
Cations are
always smaller
than the original
atom.
Anion Formation
A chloride ion is
produced. It is
larger than the
original atom.
Chlorine
atom with 7
valence e17p+
One e- is added
to the outer
shell.
Effective nuclear charge is
reduced and the e- cloud
expands.
Anions are always
larger than the
original atom.
 Electrons are
added to the outer
PEL.
Ionization Energy
 The energy required to
remove an electron from an
atom is ionization energy.

Measured in kilojoules, kJ
 The larger the atom is, the
easier its electrons are to
remove.
 Ionization energy and
atomic radius are
inversely
proportional.
Ionization Energy (Potential)
 Draw arrows on your help sheet like this:
Electronegativity
 Electronegativity is a measure of an atom’s
attraction for another atom’s electrons.
 Generally, metals are electron givers and have low
electronegativities.
 Nonmetals are electron takers and have high
electronegativities.
 What about the noble gases?
Electronegativity
 Your help sheet should look like this:
0