The document provides guidance for teaching students about trends in the periodic table. It outlines objectives for students to understand periodic trends, chemical bonding types, and the historical development of the periodic table. Activities are described where students will construct their own periodic table and analyze trends within periods and groups. Tables should be created showing how properties vary within periods and groups.

1. Karlene Bisnott
February 10, 2009

2.  Students should be familiar with the concept
of the atom as the basic building block of
matter.
 Students should be able to:
 Explain the basis of the arrangement of
elements in the periodic table
 Identify trends in Period 3 using gradation
from metallic to non- metallic properties

3.  Identify trends in Group II
 Identify trends in Group VII
 Predict properties of unknown elements
based on group trends
 Identify metals and non-metals in the
Periodic Table
 Define metallic bonding
 Define covalent bonding

4.  Define giant molecular crystals
 Explain the term allotropy

5.  In groups of four or
five, students will be
asked to sequence a
deck of cards in rows
and columns.
 They will then
discuss their
arrangements.
 A historical
background of the
Periodic Table
 This was developed
by Dimitri
Mendeleev in 1869.
 Elements were
arranged into rows
and columns.

6.  We are going to construct our own table.
 Step 1: Place the atoms in ascending order
using the number of protons
 Step 2: Arrange them in eight columns and
three rows.
 Step 3:Atoms with only one electron in the
outer shell are placed on the left.
 Step 4: Atoms with a filled shell are placed on
the right.

7.  Your constructed table should look like this:
 http://www.chem.iastate.edu/group/Greenbo
we/sections/projectfolder/flashfiles/reaction
/bonding1.swf

8.  Elements found to the left of the table are
called metals.
 They react by losing electrons from their
valence shells to obtain a full outer shell.
 Elements found from the middle to the right
of the table are called non-metals.
 They react by either gaining electrons or
sharing electrons to obtain a full outer shell.

9.  Let us take a closer look at the Periodic Table
 http://www.chem.iastate.edu/group/Greenbo
we/sections/projectfolder/flashfiles/reaction
/bonding1.swf
 The metals are located to the left.
 The non-metals are located from the middle
to the right.

10.  The vertical columns in the periodic table are
called groups.
 The elements in each group have similar
properties.
 The chief similarity is the fact that they have
the same number of electrons in the outer
shell.
http://www.teachnet.ie/tburke/periodic/elem
ent/html

11.  Look at this periodic table
 http://www.teachnet.ie/tburke/periodic/elem
ent/html
 Each group of elements is assigned a name.
 Give the names assigned to Groups I, II,VII
and 0.
 List the elements found in Group II and Group
VII.

12.  The horizontal rows of elements in the
Periodic Table are called periods. For the first
twenty elements, there are four periods.
 The elements in each period have properties
that are similar.
 The chief similarity is the number of shells in
the atom.

13.  Let us take a closer look at the periods.
 http://www.teachnet.ie/tburke/periodic/elem
ent/html
 The elements in the same period have the
same number of shells of electrons.

14.  Look at the periodic table.
 List the elements found in Period 3, stating
how many electrons are in the outer shell.

15.  Let us examine how
the following vary
down group II and
group VII
 Atomic size
 Ease of ionization
 Melting points
 Boiling points
 Density
 http://www.learners
tv.com/animation/a
nimation.php?ani=1
84&cat=chemistry

16.  Let us examine how
the following vary
across Period 3:
 Atomic size
 Electronegativity
 Electropositivity
 Conductivity
 Melting points
 http://www.chem.ia
state.edu/group/Gre
enbowe/sections/pr
ojectfolder/flashfiles
/reaction/bonding1.
swf

17.  Create a table to show how the following vary
across Period 3: Melting point, conductivity,
atomic size, electronegativity,
electropositivity
 Create a table showing how the following vary
down Group II: atomic size, density, melting
point, boiling point, ease of ionization.
 Create a similar table for Group VII

18.  This type of bonding is found in metals. The
atoms in metals are packed so tightly that the
electrons on the outer shell are knocked off.
These free electrons form a ‘sea’ around the
nuclei. An attraction occurs between the
positive nuclei and the negative sea of
electrons. This attraction is called metallic
bonding.

19.  Here is a diagram showing the bonding in
metals.

20.  Non-metals form covalent bonds.
 This type of bond is formed when carbon
atoms bond with each other. Two structures
formed are:
 Graphite and diamond.
 Click on the link to observe these structures.

21.  Allotropes are different structures of the
same element.
 Therefore carbon has two allotropes:
 Diamond and graphite

22.  Elements are arranged logically in a table.
 This arrangement of elements in ascending
order of atomic number is called a Periodic
Table.
 The elements are organized into families
called groups and periods.
 The elements in each family have similar
properties.

23.  The elements in the Periodic Table can be
classified as metals and non-metals.
 The bonding found in metals is called
metallic bonding.
 The bonding found in non-metals is called
covalent bonding.
 The non-metals can form simple molecules
or giant molecular crystals.

24.  Different structures of the same element are
called allotropes.
 The Periodic Table provides a wealth of
information about the elements.

25.  http://chemistry.about.com/od/testsquizzes
/l/bltrendsquiz.htm
 Click on the link above to try this quiz on the
Periodic Table.

26.  Ferguson & Hart: CXC Chemistry, Oxford
University Press, 1994
 Gallagher & Ingram: Complete Chemistry,
Oxford University Press, 1997
 Tindale Anne : Chemistry – A Concise
Revision Course for CXC, Stanley Thornes
(Publishers) Ltd., 1998
 The Internet