Download Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table

Grade 9 Science
Unit: Atoms and Elements
Topic 4: Periodic Table & Compounds
Topic
Using the Periodic 
Table
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Metals, NonMetals &
Metalloids
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“I can…”
Explain and identify the periods of the Periodic Table.
Explain and identify the groups or families of the Periodic Table.
Identify Elements by their symbol and their name.
State the Atomic Number, Mass Number and Atomic Mass for any
element, given the Periodic Table.
State how many protons, neutrons and electrons are in an element,
given the Periodic Table.
Explain what an isotope is.
State the Atomic Mass, Mass Number, Number of Neutrons, Protons
and Electrons for an isotope of an element.
Explain how an ion is formed.
State the ion charge of an element, given the Periodic Table.
Identify Metals on the Periodic Table.
State the physical properties of most metals.
State the chemical properties of most metals.
Identify Non-Metals on the Periodic Table.
State the physical properties of most non-metals.
State the chemical properties of most non-metals.
Identify Metalloids on the Periodic Table.
Element Families
Classification of
Matter
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Types of
Compounds
Compound
Symbols
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State the physical properties of most metalloids.
State the chemical properties of most metalloids.
Identify the Alkali Metals; explain their similarities and differences.
Identify the Alkaline-Earth Metals; explain their similarities and
differences.
Identify the Halogens; explain their similarities and differences.
Identify the Noble Gases; explain their similarities and differences.
Distinguish between Pure Substances and Mixtures; give examples of
both.
Distinguish between Compounds and Elements; give examples of both.
Distinguish between Homogeneous Mixtures and Heterogeneous
Mixtures; give examples of both.
Explain how a solid solution can exist and give an example of a solid
solution.
Explain the properties of Ionic Compounds.
Explain how the atoms are bonded in Ionic Compounds.
State which types of atoms create Ionic Compounds.
Explain the properties of Molecular Compounds.
Explain how the atoms are bonded in Molecular Compounds.
State which types of atoms create Molecular Compounds.
Explain what atoms create Diatomic Molecules.
State any elements are in a compound, given the symbolic formula.
State the quantity of elements within a compound, given the symbolic
formula.
Sketch a rough diagram of each compound.
Explain how no atoms are lost in a chemical change; that the mass and
the atoms balance going into a reaction and coming out of a reaction.
4.1 - Using the Periodic Table
_________________ knew that some elements were very similar, and it made sense to him to
group them together. For example, he grouped together _____________, _____________, and
other metals that reacted violently with _____________. In 1886, the element
_____________was discovered. This element had the exact properties of a
__________________________on Mendeleev’s table.
__________________________rearranged the elements to the table we have now based on
the __________________of the elements.
Label the following onto the blank periodic table:
- Periods, groups
- Solid, liquid, gas
- Metal, metalloid, non-metal
- Alkali Metals, Alkaline Earth metals, Halogens, Nobel Gases, Transitional Metals
Use the Sask. Science 9 (pg 177-187) to complete the notes below:
Period
- _________________ row of elements in the periodic table
- They are numbered from _____ to _____
- The most ___________ metals start on the ___________, as you move __________ the
metals become less reactive
Group/Family
- _________________ column of elements in the periodic table
- They are numbered from _____ to _____
- Elements in the same group have ______________________
Element Symbol & Name (Pg 160 – 161)
- Element symbols are used to describe elements because
___________________________ __ and it will make ________________________
- An element symbol consists of _____ or _____ letters
- The ____________ letter is capitalized, and if there is a second letter it is
________________
- The rule about capitalization is very important. Ex. The symbol _________ stands for
_____________, while _______ represents ________________ (a compound that
contains both ___________ and _____________)
- The symbol is sometimes an __________________ of the elements English name, other
times it abbreviates the elements ______________ name. Ex/ the symbol for Silicone is
_______ where as the symbol for Silver is ______ because its Latin name is
_____________.
- Some elements are named based on where they were discovered, like
_______________ which was discovered at the University of California.
- _________________ is a strong yet light metal element. It is named for the
___________, powerful gods of Greek mythology.
Atomic Number
- The atomic number is typically found _______________________ of each element
square
- It shows how many ___________ are in one atom of that element.
- Atoms have a ____________ charge, therefore the number of __________________
equals the number of __________________
- As you move across the periodic table from left to right the atomic number
_____________
by ___________
Ex/ Nickel’s atomic number is____________, therefore it has _____________ protons and
______________ electrons
Atomic Mass
- Typically found ___________ the elements name in each element square
- Atomic mass is always expressed as a _____________, because each element, except for
_____________, can form _____________, which are atoms with different numbers of ____________ in them and therefore different ______________.
- Atomic mass is the average _____________of all an element’s different _____________
- Mass is measured in _____________ _____________ _____________ (amu)
- Hydrogen has an atomic mass of _____________and iron has an atomic mass of
_____________. This means that iron is _____________times heavier than hydrogen
atoms.
Mass Number
The mass number of an element is the atomic number rounded to a whole number
- Is the total number of ______________ and ________________ in an atom
- __________ are too small, therefore they have very little effect on the total mass of the
atom
- To determine the number of neutrons an element has subtract the _______________
from the ________________
___________________ - __________________ = ____________________
Isotopes
- A form of an atom that has a different number of _____________than the common
form of that atom
- Ex. The most common form of hydrogen has _____________proton and _____________
electron but _____________neutrons. A small percentage of hydrogen atoms have
_____________ proton, _____________electron, and _____________neutron. An even
smaller percentage of hydrogen atoms have _____________proton,
_____________electron and _____________ neutrons.
- The most common form of carbon contains _____ protons and _______ neutrons,
therefore has a mass number of _________. Carbon-14 is an isotope of carbon that has
a mass number of 14. Because it isn’t the most common form of carbon, its mass
number is indicated with “-14” at the end of the element name. Carbon-14 is used for
_____________________
Ion Charge
- Ions are formed when atoms or groups of atoms _____________or
_____________electrons.
- Ion charge is the _____________charge that an atom takes on when it loses or gains
electrons.
- Elements that gain electrons become _____________charged, whereas elements that
lose electrons become _____________charged.
- Elements with atoms that form similar _____________are grouped together in the
periodic table. For example, elements in the first column on the left side of the periodic
table all form _____________ions of ion charge _____________.
Complete the table below:
Element
Element
Atomic
Atomic
Mass
Ion
# of
# of
# of
Name
Symbol
Number
Mass
Number
Charge
Protons
electrons
neutrons
Hydrogen
Bromine – 81
Iron
Titanium-46
Lead
Uranium-235
Vanadium
Phosphorus
Argon
Magnesium
Uranium
Carbon
Helium
Assignment: Complete Chart above and complete questions from Saskatchewan Science 9
page 188#3, 4, 8.
4.2 – Metals, Non-metals, Metalloids
Metals
- Metals are found of the ______________ side of the periodic table
Physical Properties
o Most are ____________ and ______________
o Excellent conductors of ___________ and ___________
o They are also ______________ and _________________
o Most metals are ____________ at room temperature. ______________ is a
metal that is ______________ at room temperature.
Chemical Properties
o Some metals react explosively with ____________ (Ex. ______________)
o Others will not react even if mixed with ________________ (Ex.
______________)
Non – Metals
- Only __________ of the known elements are classified by scientists as non-metals.
- These elements are not grouped because of their similarities but because
_______________________________
- Non-Metals are found of the ______________ side of the periodic table
Physical Properties
- __________of the non-metals are gases at room temperature, _________ are solid, and
________ is liquid.
- Solid non-metals do not conduct _____________or ____________.
- Solid non-metals are ____________________ and not ____________________
elements
- Solid non-metals have little or no ________________
Chemical Properties
- Some non-metals are very reactive.
- _____________ is a Yellow solid. It is a very reactive _____________ gas and will
________ in air. It will melt into a liquid with __________ heat.
- Pure _________________ is very _____________ and ______________.
Metalloids
- Have both _______________ and ________________ properties
- They are often used in _________________, such as __________________
Physical Properties
- Metalloids ______________ electricity but _______________, they are called
_______________
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_________________ is the most common metalloid. It is _____________ and
___________, but unlike a metal, it is ____________. About 40% of the mass of any
_____________ comes from silicon. It is also a major component in _______________
Assignment: complete questions from Saskatchewan Science 9 page 165 #1, 3, 6, 7.
4.3 – Element Families
Alkali Metals
- Group ______ elements.
Similarities
- _____________in colour.
- Like other metals, they are _____________ and _____________; they conduct
_____________and _____________.
- Unlike other metals, they have _____________melting points and melt below
_____________
- These are the ___________________ metals.
- These metals react when exposed to ______________ or _____________
Differences
- From top to bottom, _____________increases, and _____________decreases.
Alkaline-Earth Metals
- Group ______ elements
- _____________in colour.
- These elements also react when exposed to __________ or ____________, however
their reactivity is not as _______________ as alkali metals
- They are _____________ and have a _____________ than sodium and potassium
- Alkaline-Earth Metals have _____________ melting points that alkali metals
Halogens
- Group _____ elements
Similarities
- Each has a _____________ but _____________ colour.
- They all have a low _____________ point
- They are the most ____________ non-metals
Differences
- Moving from top to bottom, the colours of the vapours grow in _____________
- Also, melting points _____________
Noble Gases
- Group ______ elements
Similarities
- All exist naturally as _____________ gases, but will glow with bright colours if
_______________________________________
- They are the most ___________________ elements
Differences
- From top to bottom, the _____________ increases
Assignment: complete questions from Saskatchewan Science 9 page 184 #1-3.
4.4 - Classification of matter
All __________
_______________ ____________________
- Contain only one type of particle
- can exist in three __________ ___ __________:
solid, liquid and gas
_______________
- Examples:
water, salt,
_______________
- contain two or more pure
substances
_______________
_________________
_________________
(Solutions)
- Examples: iron,
gold, oxygen
- appear to be one
substance
sugar
- particles of different
substances are
intermingled
- examples: vinegar,
clear air
_________________
_________________
(Mechanical
Mixtures)
- two ore more parts
can be seen
- different kinds of
particles stay
together
- examples: soil,
blood, concrete
_____________
Identify each mixture as homogeneous or heterogeneous.
 Dirt____________
 Sterling silver bracelet ________________
 Sample of pond water _______________
 Recycled paper ________________
Answer each question with a full sentence.
 To the unaided eye, a mixture appears to be a white liquid with no visible
substances floating around. Can this mixture be classified as homogeneous?
Explain why or why not.
 Air can be classified as heterogeneous or homogeneous. Explain why this
statement is true.
Read the descriptions below. In the space provided, indicate whether each mixture is a
mechanical mixture (MM) or a solution (S)
 The different substances in this mixture can be distinguished from each other
with the unaided eye or a magnifying glass _______
 The substances in this mixture cannot be separated by filtering________
 When this mixture is left to stand undisturbed, the substances do not separate
by floating to the top or settling to the bottom. ________
 This mixture appears cloudy or opaque. You cannot see through it clearly.
______
Combining Metals (Pg 159)
Some metals, such as __________ and ___________, are too ___________ to be used alone
for some purposes. Therefore, to make a substance stronger, some metals are often melted
and mixed with other melted metal elements. The mixture is cooled to become a solid
____________. A solution of two or more metals is called an ____________. Common alloys
include a combination of ____________ and _____________ or _____________, this is often
called ________________ because it has a lighter colour than pure gold. White gold is often
used in engagement rings and wedding bands to give them ______________ and
_______________. Alloys are used in _____________, __________________, ______________
and many other household items.
Assignment: complete questions from Saskatchewan Science 9 page 127 #2-4, 7 and page 146
#3, 15.
4.5 –Types of Compounds
Ionic Compounds
Properties
- Ionic compounds have ______________ melting points (they are solid at room
temperature)
- When dissolved in water, they are good ______________
- They all form ______________
How they are formed
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Ionic compounds are pure substances formed as a result of the attraction between ions
of opposite charges
______________ atoms tend to lose electrons, therefore they become ______________
ions. Whereas, ______________atoms tend to gain electrons, therefore they become
______________ ions.
Ex) When ______________ combines with ______________, an electron from the
highest energy level of a sodium atom moves to the outer level of the chlorine atoms.
This causes the atoms to become ______________.
Molecular Compounds
- Composed of 2 ______________
- May be ______________, ______________ or ______________ at room temperature
- Tend to be ______________ or poor conductors of electricity
- They have relatively ______________ melting and boiling points due to the weak forces
between molecules
- In a molecular compound, atoms join together by ______________ electrons in the
highest energy level
Diatomic Molecules
- Molecules composed only of ________ ___________ are _______________
___________________. Common diatomic molecules are ______________,
_____________, ________________, _____________________,
____________________, ___________________, _________________, and
_______________________.
Assignment: complete questions from Saskatchewan Science 9 page 173 #1-4, 9.
4.6 – Compound Symbols
Physical State of Compounds
- Commonly a chemicals state ___ _____________ ________________ will be indicated
behind the element compound as a subscript, ____ – solid, _____ – liquid, _____ – gas,
_____ – aqueous (dissolved in water)
Symbols
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The symbol of each ____________ that is contained in a compound will be written in
the _______________ _____________________ of that compound
Ex/ NaCl
***Remember – there are 1 or 2 letters in each compound symbol and the first letter is
capitalized, the second is lowercase
Therefore the two symbols in NaCl are Na and Cl, which means that ________________
and ____________ are contained in NaCl
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There are sometimes ________________ behind a chemical symbol, these numbers
show how many ___________ of each chemical are in the compound.
Ex/ H2O
2 Hydrogen and 1 Oxygen molecule
Complete the table below
Compound Element in
compound
CaO
Molecular or
Ionic
Number of Atoms Drawing of Compound
in Each Element
CaCl2
Al2O3
Na2O
AlCl3
NaOH
Chemical Formula
- Matter cannot be ____________________ ____ ______________________.
- In _____________ ___________________, both sides must contain the same number of
atoms of each ___________________.
- _____________ _________________ in front of a compound indicate how many
____________ of the compound are used in the _____________ ___________.
Ex/ 2CH3OH + 3O2 -2CO2 + 4 H2O
In CH3OH, there is ____ carbon, _____ Hydrogen, and ____ Oxygen and in O2 there are
____ oxygen. The formula uses _____ of CH3OH molecules and 3 _____, therefore on the
left side of the formula…
2 – Carbon
8 – Hydrogen
8 – Oxygen
On the left side of the equation, there are 2 molecules of CO2 and 4 molecules of H2O.
Therefore there are:
2 – Carbon
8 – Hydrogen
8 – Oxygen
- In addition to matter being conserved, the ________ is also conserved.
Ex/ Mg + S  MgS
24.3g 32.1g
56.4
Assignment: complete questions from Saskatchewan Science 9 page 173 #7, 11.