Transcript Unit B - Chemistry

Unit B - Chemistry
Week 1
1.2 Organizing Matter
I Can…
 Understand the dangers of caustic and explosive
materials
Introduction to Chemistry
 Matter is anything that has mass and takes up
space
 What are the states of matter?
I Can…
 Describe materials in terms of physical and
chemical properties
 Distinguish between pure substances, solutions
and mechanical mixtures
What do you remember?
 What are the states of matter?
 What are the phases between the states of matter?
 Write in what you remember in your notes.
States of Matter
 Matter exists as a solid, liquid or gas.
 The state of the matter depends on the temperature
 Explain this using water…
Pure Substances
 Is made up of only one kind of matter
 There are two types of pure substances
 1) Element- cannot be broken down into any
simpler substance. Found on the Period Table
 2) Compound- more than one element
combined chemically together
Types of Mixtures
 A mixture is a combination of pure substances
 There are four types of mixtures
 1) Mechanical mixture- the different substances that make up the mixture
are visible. (heterogeneous) Example?
 2) Solution- the different substances that make it up are not separately
visible. (homogeneous) Example?
 3) Suspension- a cloudy mixture in which tiny particles of one substance
are held within another. Example?
 4) Colloid- a cloudy mixture, but the particles are so small that they
cannot be easily separated out from other substances. Example?
Properties
 To understand how substances differ, you need to
observe their properties
 Properties are characteristics that can be used to
describe a substance
 All matter has two types of properties: physical
and chemical
Physical Properties of Matter
 Colour
 Luster (shininess)
 Melting Point
 Boiling Point
 Hardness- Mohs’ hardness scale
 Malleability- ability of a substance to be made
into a sheet
 Ductility- ability of a substance to be made into
a wire
 Crystal Shape- can be cubes, diamonds, etc.
 Density- amount of mass in a volume (g/mL)
 Conductivity- can it conduct electricity
 Solubility- ability of a substance to be dissolved
in another
Chemical Properties
 Chemical properties describe how a substance
interacts with other substances
 A chemical change occurs when a new substance
is formed
 Example?
Chemical Properties of Matter
 Reaction with acids
 Ability to burn
 Reaction with water
 Behaviour in air
 Reaction to heat
Physical Changes
 A physical change occurs when a substance
changes but its chemical make-up does not
change
 Examples?
Chemical Changes
 A chemical change is when the chemical make up changes
 Examples?
Take a Break!
 Complete the table in your notes.
Aqueous Solution
 A substance that is dissolved in water
 It is represented like this
 CH3COOH(aq)
2.1Evolving Theories of Matter
I Can…
 Identify theories of the periodic table and the atom
 Understand the origins and patterns of organization of
the periodic table
Textbook Scavenger Hunt!
 Answer the Questions using your textbook
 Read through Section 2.1 in the Chemistry Unit
 http://www.learnalberta.ca/content/secsu/html/matter_a
nd_chemical_change/ChemistryPuzzle/index.html Bohr
Model Puzzle
Ted Ed Video
 Answer the Questions!
https://www.youtube.com/watch?v=O-48znAg7VE
 It is said that some chemists were able to predict the existence of some
elements that were not yet discovered. How did they do this?
 Who is known as the father of chemistry?
 What was the first element to be "discovered"?
 Which element reacts violently with water?
2.2 Organizing the Elements
I Can…
 Understand the origins and patterns of
organization of the periodic table
2.2/2.3 – Origins and Organizing the
Periodic Table
I Can…
 Understand the origins and patterns of organization of
the periodic table
 Understand how rows (periods) in the periodic table reflect
different atomic structures and columns (families/ groups)
reflect similar atomic structures
 Use the periodic table to find out the number of protons and
electrons, and other information about elements
Ted Ed Video
 https://www.youtube.com/watch?v=fPnwBITSmgU
 Who is credited with creating the periodic table?
 What did he do that set him apart?
 How do you think Mendeleev was able to so accurately estimate the
properties of undiscovered elements?
 In 1963, what did scientists officially name the element at 101 on the
periodic table?
 How many scientists have an element named after them?
 Lots of scientists had worked on the periodic table other than
Mendeleev. What do you think would have changed had they all worked
closely together to figure out the best way to arrange the periodic table?
Do you think collaboration is always the best answer?
Organizing the Table
 One of the first attempts by scientists to create a better
system for organizing the elements was made by John
Dalton
 He used a set of symbols for the elements
A better way…
 Jons Jacob Berzelius suggested using letters rather
than pictures to represent each element.
 The Atomic Symbol
 Each element is named by 1 or 2 letters
 The first letter is always capitalized and the
second letter is always small
 Example: H- Hydrogen
 Example: He- Helium
Putting the Elements in Order
 Atomic Mass is the mass of one atom of an element.
 Scientists were able to determine the average mass of an
atom
 John Newlands recognized a pattern when elements were
listed by increasing atomic mass.
 Atomic mass is compared to the mass of a carbon which is
12.0
How The Modern Day Table is
Organized
On the Periodic Table
 Staircase line-division between metals and non-metals
 Metals- on the left side of the staircase line
 They are shiny, malleable and ductile
 Non-metals- on the right side of the staircase line, can be
solid, liquid or gas
 The solids are dull and brittle and don’t conduct
 Metalloids- elements on the staircase line
 Have both metallic and non-metallic properties
 Groups/ Families- groupings in the periodic table
going down
 They have similar reactivity
 Rows/ Periods- groupings in the periodic table
going across
 They have similar mass
Groups/ Families
 Family 1: Alkali Metals- very reactive, even with water,
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

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all solids
(http://www.youtube.com/watch?v=83eq5HyG-tI)
Family 2: Alkaline Earth Metals- reactive, all solids
Family 17: Halogens- reactive non-metals, most are
gases
Family 18-: Noble Gases- non reactive gases
Family 3-12: Transition Metals- have numerous
different properties
Rows/ Periods
 6- Lanthanide series- starts at element 57
 7- Actinide series- starts at element 90
Reactivity
 Non-metals- gets more reactive as we move to
the right and get higher (excluding the noble
gases)
 Most reactive non-metal is fluorine
 Metals- gets more reactive as we move to the left
and get lower
 Most reactive metal is francium
Important Parts of the Periodic Table
 Atomic Symbol- the letters symbolizing the
element, used globally
 Atomic Number- how the periodic table is
ordered, is the number of protons in each
element
 Atomic Mass- how much mass an element has,
number of protons and neutrons together
Where are these parts?
 Circle the Symbol, Put a star beside the atomic number and
underline the atomic mass
Inside an Element
 Protons- same as the atomic number, is the
defining characteristic of the element
 The positive part of the element
 Neutrons- found by subtracting the atomic
number from the atomic mass
 Electrons- for an atom, is the same number as the
protons
Where are these parts?
 For these elements, how many protons, neutrons and
electrons are in each element?
 Make a Bohr model for each element listed
To Do:
 1) Colouring the Table (Grab 8 pencil crayons!)
 2) Complete Protons, Electrons and Neutrons Table