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Date:__________________
Name:_____________________
L3: 5.4 Characteristics of The Periodic Table and Much More
Look at the periodic table on page 646 of your text. (put a sticky on this page, you will need to refer to it often)
Where are the metals? _________________________
Where are the non-metals? ___________________________
What are the elements along the step called (coloured green)? __________________
What colour is hydrogen? _________. Why? _____________________________________________________________________
__________________________.
Properties of metals and non-metals:
Property
Lustre
Metals
Non-metals
Metalloids
Malleability
Conductivity
Reactivity with acid
State at room temperature
The periodic table is a structured arrangement of _______ that helps us explain and predict their _______ and ________ properties.
There are just over 100 known elements on the periodic table. However, these elements combine in different ways to make up
millions of substances of matter.
song: https://www.youtube.com/watch?v=zUDDiWtFtEM
Remember that one atom of any element is made up of ___________________________ Also, #p+ of an element = ____________.
The modern periodic table is arranged in order of ____________________.
HORIZONTAL ROWS
The rows of the periodic table are called ____________. Each row on the periodic table gives us two pieces of information:
(1) They represent the _____________________________________________.
(2) The number of elements in each row tell us ___________________________________________.
VERTICAL COLUMNS
Elements in the same vertical column are called chemical ______ or _______. The elements in the same chemical group /
family have similar chemical and physical properties. We will see some examples in the chart on the next page.
Valence Electrons:
The electrons in the ___________ are called ________ electrons. Look at the BR handout that you filled out for homework. Within
each group, all atoms have the ______ number of electrons in their outermost orbits. For example, all elements in group 1 have ___
_________ in their outermost orbit. How many valence electrons do group 2 elements have? ; Group 16? _ Group 17?_ Group 18?
Reactivity:
The reactivity of an atom depends on the number of valence electrons in an atom. An atom, whose valence shell is filled to its
maximum, is considered stable. It is reactive when it is ____________. Which groups would be most reactive? __Not reactive?__
Lewis Structures:
A Lewis Structure is a short-hand system used to represent the _________________ of an element, using the chemical symbol of the
element and a series of dots (representing valence electrons) drawn in clockwise direction starting from the top.
Example 1: Sodium
Example 2: Chlorine
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Periodic Trends, Bohr-Rutherford Diagrams, and Lewis Symbols
Group 1
(1st column from left)
Group 2
(2nd column from left)
Group 17
(2nd column from right)
Group 18
(1st column from right)
Group Name
Examples
BohrRutherford
Diagram
Number of
Valence
Electrons
Lewis
Structure
Physical
Properties
Chemical
Properties
*Groups 3-12 are called transition metals. They do not follow the same patterns as the other elements do. You will see more on
transitional metals in Grade 11.
**The two rows at the bottom of the Periodic table are considered rare earth metals.
Homework:
Complete Section 5.4 p.187 #1-9; Read Section 5.5