Download CHEMISTRY

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CHEMISTRY
REVIEW OF GRADE 9 CONCEPTS
CLASSIFICATION OF MATTER
______________
Takes up space and mass
__________ SUBSTANCE
Made up of components
not found on the Periodic
Table
_______________
MIXTURE
Two or more
phases
Non-uniform
composition
_______ SUBSTANCE
Made up of components
found on the Periodic Table
Always contain one phase
(HOMOGENEOUS)
_______________
MIXTURE
One phase
Uniform
composition
_____________
Only one particle
Can not be broken
down further
_____________
Contains two or
more elements
WHAT IS THE PERIODIC TABLE OF ELEMENTS?
The Periodic Table of elements classifies elements and groups them according
to characteristics such as _____________, ________________ and
_________________.
The horizontal rows of the Periodic Table are called ____________ and there are
____ periods on the Periodic Table
Elements of a period have _____________ properties
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The vertical columns of the Periodic Table are called ____________ or
____________ and there are _____ Groups on the Periodic Table
Elements in the same group have the __________ number of electrons on the
____________ orbital/shell
The existing elements are separated into ____ different categories:
_______________ – Conduct electricity well
_______________ – Do not conduct electricity  Insulators
________________ (also known as SEMI-METALS) – Has properties of
both metals and non-metals
Some groups have a special name
Group 1  ____________________  Highly reactive metals
Group 2  ________________________  Less reactive metals than
Group 1
Group 3 – 12  ______________________  Some metallic properties
Group 17  __________________  Highly reactive non-metals
Group 18  _________________________  Very unreactive gases
And __________________  Gas at room temperature
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WHAT IS AN ATOM?
Atoms are ________________________________________________________
The Bohr - Rutherford model of the atom is often referred to as the “solar system
model” Using a Venn diagram, compare the atom to our solar system.
Inside the atom, three particles exist:
______________
_______________
______________
Found inside the
____________ of the
atom
Found “orbiting” the
nucleus in paths called
______________
Found in the _________
of the atoms
Has a charge of _____
Charge of _____
Charge of zero
Mass= ________ amu
Mass= ________ amu
Mass= ________ amu
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DRAWING ATOMS (BOHR-RUTHERFORD DIAGRAMS)
For any atom, we can use information provided by the periodic table to help us
draw Bohr-Rutherford Diagrams. To draw a correct diagram, the occupancy rules
must be known. What are the maximum number of electrons allowed in each
energy level?
1st : max ___ electrons
2nd : max ___ electrons
P
N
3rd : max ___ electrons
In addition, one must be able to determine the number of protons, electrons and
neutrons using an atom’s atomic number and mass number.
13
Al
27
ATOMIC NUMBER = # OF ____________ and the # OF _______________
MASS NUMBER is the number of ______________ + _______________
# OF NEUTRONS = ___________________ – ____________________
Identify the element above this box and determine it’s number of protons,
electrons and neutrons.
What are the rules for placing electrons in a Bohr-Rutherford diagram? (3)
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EXAMPLE
Drawing the Bohr-Rutherford Diagram for Aluminum
Number of protons = ______
13
Al
27
Number of electrons = ______
Number of neutrons = _______________ = ________
WHAT ARE VALENCE ELECTRONS?
Valence electrons are _____________________________________________
When valence electrons are present, an atom can _______ or ________
electrons, depending how many electrons it requires to become ____________
WHAT ARE IONS?
All atoms are ___________ until they ________ or __________ electrons.
[Recall that neutral atoms have the _________ number of protons and
electrons]
When an atom gains an electron, there are _________ electrons than
protons and a _____________ ion is created (also known as an ANION)
When an atom loses an electron, there are _________ electrons than
protons and a _____________ ion is created (also known as a CATION)
Practice Questions: pg 148 #3, 4a; pg 149 #1; pg 150 #1-3; pg 153 #3, 10, 11
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PHYSICAL AND CHEMICAL PROPERTIES
Chemistry relates the properties of substances to the structure of the particles that
make up those substances.
By recognizing and applying patterns in chemistry ______________________
_______________________________________________________________
Properties of substances are important because they determine what the
_________________________ and help scientists _____________________.
Physical properties are those that can be observed without chemically changing a
substance. Chemical properties are those observed when a substance undergoes a
________________________.
GROUP ACTIVITY: OBSERVING THE PROPERTIES OF MATTER
Consider three of the alkali metals; lithium, sodium and potassium.
What are some physical properties that these elements have in common?
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
What other physical properties could be determined for these substances?
____________________________________________________________________
____________________________________________________________________
To observe chemical properties we must allow the metals to chemically react. Let’s
observe and describe some of their chemical properties.
1. Reaction with air
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
2. Reaction with water
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
Common chemical properties include (p. 142): _________________________________
_______________________________________________________________________
master
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Atomic Structure and Properties
Atoms of the same group (family) have very similar properties (chemical and
physical)
In terms of atomic structure, what is common about the alkali metals involved in
the demo? (see page 150, figure 4.17)
_________________________________________________________________
_________________________________________________________________
What do you recall about the chemical properties of the noble gases?
_________________________________________________________________
What is common about their atomic structure?
_________________________________________________________________
The __________________________________ within an atom plays a big part in
determining the properties of an element.
Periodic Pattern: # of valence electrons
group
v-electrons
1
2
13
14
15
16
17
18
Lewis Symbols
These are a more convenient method of communicating the valence structure of
an atom. (These will be handy later when we learn about covalent bonding.)
Rules:
______________________
______________________
______________________
______________________
Example: phosphorous
Draw Lewis symbols for an element from group 1, 13, 16 and 18.
Groups 3 – 12
These elements follow a different and more complicated set of rules. We
generally ignore discussing their specific atomic structures until later courses.
Atom Builder: http://www.sciencesource2.ca/resources/flt_atom_builder.swf
Element Builder: www.explorelearning.com
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KNOWLEDGE CHECK
1. Identify the element that lives in …
a) group 2 and period 3.
b) Period 4 and has 7 valence electrons.
2. How many electrons are allowed in the 2nd energy level?
3. What is a chemical property that is shared be all alkali metals?
4. Write the Lewis symbol for …
a) nitrogen
b) iodine
5. Initially two or more elements were placed in the same group of the
periodic table because ?
6. How many neutrons does Uranium have?
7. Which section of the periodic table contains …
a) elements that conduct electricity?
b) Some gaseous elements?
8. The following diagram was drawn to show the electrons in boron. What is
wrong?
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THE QUEST FOR NOBILITY
Ions
Ions are atoms or “molecules” that carry a charge because the number of
protons does not equal the number of electrons. An atom becomes an ion when
it _________________________ electrons.
Atoms that lose electrons become ___________ ions (cations)
Atoms that gain electrons become ___________ ions (anions)
Explaining Ion Formation
Based on patterns, it seems that atoms lose/gain electrons such that their
electron structure matches their closest ______________________ neighbor.
Consider sulphur,
As an atom it has ___ protons and ___ electrons. The ion of sulphur has
16 protons and 18 electrons (like ____________). In gaining 2 electrons, the
charge on a sulphide ion would be _______.
The symbol for a sulphide ion is _______.
Periodic Pattern for ion charge
group
charge
1
2
3
14
15
16
17
18
Ion Nomenclature
1. Metals – add roman numerals that equal charge if multivalent*. Otherwise
use elemental name unchanged.
2. Non-metals – change ending to “ide”
*multivalent metals – those that can have more than one charge.
Examples,
K+ - potassium ion; N-3 – nitride ion; Cu+ - copper (I) ion (multivalent)
– Do Page 158 #1,2
– Choose five other elements and write the symbol and name for their ions
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IONIC COMPOUNDS
Recall – compounds are pure substances that contain more than one type of element
that are bonded together in a fixed ratio. Water (H2O) is an example of a compound. In
water, the two hydrogen atoms are stuck to the oxygen and can’t be separated without
undergoing a chemical change. There are two types of compounds; Ionic and Covalent.
Ionic Compound – A compound consisting of negatively and
positively charged ions held together ionic bonds. (ionic bonds –
force of attraction between two oppositely charged ions, opposites
attract).
Binary Ionic Compounds
These involve metal ions (+) bonded to non-metal ions (-). The ratio of the ions to each
is such that the total charge of the compound is ________. This ratio is shown in the
___________________ of a compound.
e.g.
Naming these compounds is easy. Simply name the metal ion (with roman numerals if
needed) and then the non-metal ion (‘ide’). All letters should be lower case.
Ionic Compounds with Polyatomic Ions
Some ions are polyatomic (multi-atom ions). Most of these are negative. Some common
ones are in table 4.7 on page 161. Copy these on the back of your periodic table.
e.g.
The subscripts in these ions cannot be changed except through some chemical
reactions. Writing formulas for these follows the same rules as for binary compounds.
Total charge = 0!
e.g.
Naming these compounds is also easy. How do you know a polyatomic ion is involved
when looking at a chemical formula/chemical name?
page 159 #1-4; page 160 #1-4; page 161 #1-4; page 163 #1-4; page 164 #1-4
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Chemistry: Ions in Chemical Compounds
Complete the following table by writing a formula so that the total charge on the resulting
compound is zero. Also write the name for each compound.
Ions
Hydroxide
Cl1-
Carbonate
Sulfate
NO31-
Hydrogen
H1+
Sodium
Na1+
Ammonium
NH41+
Potassium
K1+
Calcium
Ca2+
Magnesium
Mg2+
Aluminum
Al3+
Iron (II)
Fe2+
Iron (III)
Fe3+
Pb2+
Tin (IV)
Cu1+
Copper (II)
Ionic Bond Gizmo: www.explorelearning.com
S2-
PO43-
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MOLECULAR COMPOUNDS (COVALENT)
Some atoms achieve a ______________ electron structure by sharing electrons
with another element. The mutual attraction that each atom has for the shared
electrons is called a ___________________. One covalent bond consists of 2
shared electrons.
Generally, covalent bonds exist between __________________ elements. A
structure that consists of two or more covalently bonded atoms is called a
___________________.
Perhaps the simplest molecules are the diatomic elements such as H2. The
bonding that holds an H2 molecule together can be illustrated using Lewis
structures or structural diagrams which are derived from Lewis Symbols.
Rough Work using Lewis
symbols
Lewis Structure
Structural Diagrams
Illustrating the bonding in O2 and N2;
Rough Work using Lewis
Lewis Structure
symbols
Structural Diagrams
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What about molecules containing different atoms? Consider HCl.
Rough Work using Lewis
symbols
Lewis Structure
Structural Diagrams
Single bond – ____ shared electrons between two atoms
Double bond – ____ shared electrons between two atoms
Triple bond – ____ shared electrons between two atoms
Naming Molecular Compounds
Prefix Method is used
prefix
1
2
3
4
5
6
7
8
If the compound your naming contains two different non-metal elements it is a
molecular compound!!
Simply name the first element followed by the second, each with a prefix
indicating how many of each element are in a molecule.
Annoying Rule – If there is only one of the first element, do not use a prefix
for it. If there is only one of the second element, you must use a prefix.
Examples
Questions: page 168 # 1-4 (top and bottom); page 171 # 6-10, 12-13
Do molecular modeling activity on page 170
Covalent Bond Gizmo: www.explorelearning.com
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PERIODIC TABLE COLOUR CODING
Colour code your periodic table so that it identifies the following;
•
•
•
•
•
•
•
•
•
•
•
•
Alkali metals
Alkaline earth metals
Halogens
Noble gases
Metals
Non-metals
Transition metals
Semi-metals (metalloids)
Liquid elements
Gaseous elements
Diatomic elements
Multivalent metals (no non-metals)
Be sure to make a legend. You may want to do this on a separate piece of paper.
Use pages 146 - 148 and page 165 (table 4.11) in your text as a reference.
You will be allowed access to this periodic table for your next test. Please do not add
any other information unless asked to do so.
PERIODIC TABLE COLOUR CODING
Colour code your periodic table so that it identifies the following;
•
•
•
•
•
•
•
•
•
•
•
•
Alkali metals
Alkaline earth metals
Halogens
Noble gases
Metals
Non-metals
Transition metals
Semi-metals (metalloids)
Liquid elements
Gaseous elements
Diatomic elements
Multivalent metals (no non-metals)
Be sure to make a legend. You may want to do this on a separate piece of paper.
Use pages 146 - 148 and page 165 (table 4.11) in your text as a reference.
You will be allowed access to this periodic table for your next test. Please do not add
any other information unless asked to do so.
Periodic Table
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Review
compounds flow chart.doc
naming compounds relay.doc
http://www.learner.org/interactives/periodic/basics_interactive.html
Quiz #1 – written
Quiz #1 – m/c
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CHEMICAL REACTIONS
PHYSICAL VS. CHEMICAL CHANGES
2DCHEM_-_WS_3_(Changes_in_Matter_Concept_Map).pdf
CHEMICAL REACTIONS
2minute video
animated chemical reaction
REPRESENTING CHEMICAL REACTIONS USING EQUATIONS
A chemical equation is an efficient method of communicating what happens in a
particular chemical reaction.
When magnesium is ignited in the presence of oxygen it burns to produce solid
magnesium oxide.
word equation: magnesium + oxygen → magnesium oxide
(reactants)
(products)
chemical equation: Mg(s) + O2(g) → MgO(s)
•
In a skeletal equation, the states of matter are often communicated in
brackets behind each reactant and product.
(s) – solid
(v) - vapour
(l) – liquid (aq) – aqueous (dissolved in water)
(g) - gas
**Remember the diatomic elements (7-up)
Page 175 #1-5; page 187 #4; handout
THE LAW OF CONSERVATION OF MASS
THE TOTAL MASS DURING A CHEMICAL REACTION CANNOT CHANGE
TOTAL MASS OF REACTANTS = TOTAL MASS OF PRODUCTS
ALL ATOMS MUST BE ACCOUNTED FOR IN A CHEMICAL REACTION
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Examples;
1. 5 grams of chemical A reacts with 7 grams of chemical B to produce
chemical C.
a) What is the equation?
A + B → C
b) What mass of C must have been produced?
A + B → C
5g 7g
?g
12g = 12g (LCM)
** 12 grams of C must have been produced.
2. How much of chemical X must have been added to 4 grams of chemical Y
to produce 7 grams of chemical Z?
Word equation:
Masses:
Total Mass:
Missing mass:
X + Y → Z
?g
4g
7g
7g
7g
X=7–4=3g
http://www.saskschools.ca/curr_content/science10/unitb/lawmasqs.html
BALANCING CHEMICAL EQUATIONS
Task – place an appropriate coefficient in front of each reactant or product to
ensure that all atoms are conserved.
Rule – you may only change coefficients. Subscripts cannot be changed as this
would change the identity of a reactant or product.
Page 187 #5,6
Counting Atoms Worksheet.doc
balancing.pdf
balancing answers.pdf
http://web.jjay.cuny.edu/~acarpi/NSC/6-react.htm
GIZMO
http://antoine.frostburg.edu/chem/senese/101/kits/kit_chemical_equation.html
SNOWMAN BALANCING ACTIVITY: PG. 1
CHAPTER 4 REVIEW
CHAPTER 4 QUIZ
PG. 2
Page 190 #5, 6, 8, 11,14,15-20
PG. 3
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REACTION TYPES
Can you see the pattern?
Hopefully you realize the importance of knowing the many patterns that exist in
the periodic table. Patterns help reduce the amount of things we need to
memorize and also allow us to acquire information quickly. For example, knowing
that an element is in group 2 tells us a lot about that element. We know it has
two valence electrons, it’s a fairly reactive metal and it forms an ion with a +2
charge.
There are millions of different chemical reactions that occur in the Universe. It
would be quite a task to memorize the details of all of them separately. To
reduce the amount that we have to know, scientists classify reactions into types.
Every reaction within a type follows a particular pattern. So, instead of
memorizing specific individual reactions we memorize the types of reactions and
the patterns they follow.
In this activity you will work in groups to try to identify things in common
between different reactions of the same type.
Type 1 – Synthesis Reactions
2Mg + O2  2MgO
What is common about these reactions?
2Na + Cl2  2NaCl
MgO + CO2  MgCO3
2H2 + O2  2H2O
Type 2 – Decomposition Reactions
2KClO3  2KCl + 3O2
2Al2O3  4Al + 3 O2
H2CO3  H2O + CO2
NO3  NO + O2
What is common about these reactions?
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Type 3 – Single Displacement Reactions
Mg +
Zn(NO3)2 
Mg(NO3)2 + Zn
What is common about these reactions?
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
2Na +
K
+
CuCl2 
LiI
2NaCl
KI

+
+
Cu
Li
Type 4 – Double Displacement Reactions
Zn(NO3)2 + CuCl2
AgNO3 +
 ZnCl2 + Cu(NO3)2
What is common about these reactions?
NaCl  AgCl + NaNO3
Pb(NO3)2 + KI  PbI2 +
KNO3
BaCl2 + Na2SO4  BaSO4 + NaCl
Classify these reactions;
2NaBr + Ca(OH)2  CaBr2 + 2NaOH
2NH3 + H2SO4  (NH4)2SO4
Pb + H3PO4  H2 + Pb3(PO4)2
Type of reaction: _______________________
Type of reaction: _______________________
Type of reaction: _______________________
Li3N + 3NH4NO3  3LiNO3 + (NH4)3N
Type of reaction: _______________________
2H2O2  2H2O + O2
Type of reaction: _______________________
Page 229 # 4, 6, 7, 9, 10
Page 240 # 4 abdef, 7abd, 8, 9, 10
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A
C
+
B
 A

+
C
B
A + BC  AC + B
AB + CD  AD + CB
A
C
+
B
 A

+
C
B
A + BC  AC + B
AB + CD  AD + CB
A
C
+
B
 A

+
C
B
A + BC  AC + B
AB + CD  AD + CB
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HYDROCARBON COMBUSTION
Read page 232 in the textbook and then answer the following questions.
1. What is common about all combustion reactions?
_________________________________________________________________
_________________________________________________________________
2. What is a hydrocarbon?
_________________________________________________________________
3. What is the general equation for the combustion of a hydrocarbon?
_________________________________________________________________
4. What importance does hydrocarbon combustion have in our lives?
_________________________________________________________________
_________________________________________________________________
5. What environmental issue is related to hydrocarbon combustion?
_________________________________________________________________
6. Sometimes the combustion of a hydrocarbon is “incomplete”. When
this happens carbon monoxide is produced. What problem is
associated with this?
_________________________________________________________________
_________________________________________________________________
7. Write the balanced chemical equation for the combustion of;
a) methane (CH4)
_________________________________________________________________
b) propane (C3H8)
_________________________________________________________________
c) candle wax (C25H52)
_________________________________________________________________
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Chemical Reactions Practice Quiz
Balance and classify the following equations as either i) synthesis (S)
ii) decomposition (D)
iii) single displacement (SD)
iv) double displacement (DD)
TYPE
v) combustion (C)
O2 →
1.
__ Cu +
CuO
2.
__H2O → _____H2 + _____O2
_______ 3. _____Fe + _____H2O → _____H2 + _____Fe2O3
_______ 4. _____AsCl3 + _____H2S → _____As2S3 + _____HCl
_______ 5. _____CaCO3 → _____CaO + _____CO2
_______ 6. _____Fe + _____S8 → _____FeS
_______ 7. _____H2S + _____KOH → _____HOH + _____K2S
_______ 8. _____NaCl → _____Na + _____Cl2
_______ 9. _____Al + _____H2SO4 → _____H2 + _____Al2(SO4)3
_______ 10. _____H3PO4 + _____NH4OH → _____HOH + _____(NH4)3PO4
_______ 11. _____C3H8 + _____O2 → _____CO2 + _____H2O
_______ 12. _____Al + _____O2 → _____Al2O3
_______ 13. _____CH4 + _____O2 → _____CO2 + _____H2O
_______ 14. _____Al(NO3)3 + _____LiOH → _____LiNO3 + _____Al(OH)3
_______ 15. _____NaOH + _____HCl → _____NaCl + _____H2O
_______ 16. _____CuCO3 → _____CuO + _____CO2
_______ 17. _____K + _____O2 → _____K2O
_______ 18. _____Cl2 + _____KI → _____KCl + _____I2
_______ 19. _____KNO3 → _____KNO2 + _____O2
_______ 20. _____Zn + _____O2 → _____ZnO
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PREDICT THE PRODUCTS
1.
C10H16 + O2  ______________________________
Type of Reaction: combustion
2.
MgO  ______________________________
Type of Reaction: decomposition
3.
Ca + CuCl2  ______________________________
Type of Reaction: single displacement
4.
Al(OH)3 + H2SO4  ______________________________
Type of Reaction: double displacement
5.
Rb + Br2  ______________________________
Type of Reaction: synthesis
6.
Na + H2O  ______________________________
Type of Reaction: single displacement
7.
Ca + O2  ______________________________
Type of Reaction: synthesis
8.
Zn + NaOH  ______________________________
Type of Reaction: single displacement
9.
Hg(OH)2 + H3PO4  ______________________________
Type of Reaction: double displacement
10.
C2H6 + O2  ______________________________
Type of Reaction: combustion
11.
Al + FeO  ______________________________
Type of Reaction: __________________
12.
Mg + N2  ______________________________
Type of Reaction: __________________
13.
Fe2(SO4)3 + KOH  ______________________________
Type of Reaction: __________________
14.
Ca3(PO4)2 + Si(CO3)2  ____________________________
Type of Reaction: __________________
15.
H2O2  ______________________________
Type of Reaction: __________________
______________________________________________________________________
LAB #2: SINGLE DISPLACEMENT
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ACIDS AND BASES: THE pH SCALE
ACID/BASE POWERPOINT
_________________ solutions are created when acids are dissolved in water to create
aqueous _________________. The “acidity” of the solution is a measure of how many
H+ ions are present per ________________. This largely determines how
__________________ the solution is. Solutions that are very acidic are very dangerous.
Strong acids are those that are needed in a relatively ____________quantity to
generate __________________ solutions. _______________________ is considered to
be a strong acid. ______________________ is a weak acid.
It takes a __________________amount of hydrochloric acid to make a highly acidic
solution. It takes a _________________ amount of carbonic acid to make a highly acidic
solution.
Basic solutions are created when a base is dissolved in water creating aqueous OHions. The ___________________ of the solution depends on how much base is
dissolved and on the strength of the base.
Neutral solutions are those that contain neither a dissolved acid or a base.
To communicate how acidic or basic a solution is scientists use the pH scale. See figure
5.5 on page 196.
The pH scale details;
•
•
•
•
•
•
•
___________________________________________________
7 represents the pH of a solution that is neither ___________________. The
solution is said to be __________________.
Any solution with a pH below 7 is _______________.
Any solution with a pH above 7 is _____________.
The more acidic or basic a solution is, the ________________________.
A difference of 1 on the pH scale represents a factor of _____ in terms of acidity
or basicity.
A difference of 2 on the pH scale represents a factor of ______ in terms of
acidity or basicity.
Using figure 5.5, answer the following,
1.
2.
3.
4.
5.
What is the strongest acidic solution shown? ___________________________
What is the strongest basic solution shown? _______________________
What do most of the acidic solutions have in common? _____________________
What do most of the basic solutions have in common? _____________________
How much more/less acidic/basic is/are
a) Stomach acid than lemon juice?
b) Milk than acid rain?
c) lemon juice than milk?
__________________________
__________________________
__________________________
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d) sea water than toothpaste?
__________________________
ACID-BASE INDICATORS
Acid-base indicators are substances whose colour is pH dependent.
For example, a substance called litmus which is derived from plant material can be
obtained in two different colours, blue and red. Blue litmus turns red in acidic solutions
and red litmus turns blue in basic solutions.
pH paper is a material whose colour not only indicates whether a solution is acidic or
basic but also allows one to estimate pH by matching it’s colour to a chart.
There are many substances that are indicators. Investigate those provided and record
their colour in acidic, basic and neutral environments.
Indicator
Neutral Colour
Colour in Acidic
Solution
Colour in Basic
Solution
Page 197 #1-4
Recognizing Acids and Bases
Above, we saw how indicators can be used to test whether a solution is acidic or basic.
Acids and bases can also be recognized by their unique properties. Using the textbook,
perform the cut and paste activity which will help you learn the properties that are
characteristic of acids and bases.
Acids and bases can also be identified by their chemical formulas.
The chemical formula of an acid often begins with at least one “H”.
e.g.
HCl
HNO3
H2SO4
However, not all compounds that begin with H are acids (e.g. water).
Another type of acid contains a carboxyl group. The formula for this acid type ends in
COOH. Acetic acid in vinegar is this type and has the formula CH3COOH.
Most common bases contain the hydroxide ion, OH-.
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e.g.
NaOH, Ca(OH)2
NOMENCLATURE
Bases – these are easy. Just name them as normal “metal hydroxide” compounds.
Acids – two types
i)
Binary – no polyatomic ion
procedure: use prefix “hydro”, suffix “ic” and “acid”
e.g.
HCl – hydrochloric acid
ii) Oxyacid – polyatomic ion
procedure: no prefix, suffix “ic” and “acid”
e.g.
HClO3 – chloric acid
(just change the “ate” to “ic”)
Page 200 #1,2; page 201 #1,2; page 203 #3,4,7-9, 11
ACID – BASE NEUTRALIZATION
When separate acidic and basic solutions are mixed, the H+ from the acidic solution
combines with the OH- from the basic solution to form ___________. The H+ and OHare said to neutralize each other. The pH of the mixture would become closer to _____.
Most neutralization reactions follow a double displacement pattern. Can you predict the
products of the following acid-base reaction?
HF(aq) + KOH (aq)→
General equation: _____________________________________________
The salt is made of the ____________ from the base and the ________of the acid.
An application of this is in the use of antacids which people consume when they
experience “heartburn”. Heartburn is caused by the production of too much stomach
acid resulting in a pH that is too ______ for comfort. Consuming an antacid tablet which
contains a base neutralizes some of the acid and thus ___________ the pH.
Page 206 # 1-3
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If time; ..\..\Young 10D\Chemistry\2DCHEM_-_WS_9_(Acids_&_Bases).pdf
Note: use pages 196-200 and don’t worry about task #3 – refers to a different textbook.
ACID PRECIPITATION
REFERENCE: PAGE 208 - 210
1. At what pH is rain classified as “acid rain”?
2. What two atmospheric gases react to form acidic rain?
3. List the human and industrial activities that contribute to the production of acid
rain.
4. What problems are created by acid rain?
5. Write the word equations for the two reactions that result in the production of
atmospheric H2SO4. Classify these reactions.
6. Why can some lakes resist pH changes when acid rain falls?
7. What can be added to lakes to revive them from damage caused by acid rain?
Why is this not an ideal, long term solution?
8. Write the balanced neutralization equation that describes the reaction between
sulphuric acid and calcium hydroxide.
9. Briefly describe two technologies that help reduce the amount of acid
precipitation.
_______________________________________________________________________
LAB #3 – ACID/BASE NEUTRALIZAITON
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CHEMISTRY UNIT REVIEW
What is the difference between a chemical property and a physical property? Give examples.
How are elements and compounds similar? How are they different?
Describe the structure of an atom in words and with a picture. What rules govern the arrangement
of electrons in an atom?
What name is given to the electrons in the outermost energy level?
What information does the periodic table provide?
Brainstorm the patterns and relationships in the periodic table.
Draw a Bohr – Rutherford diagram for calcium and sulfur.
Draw a Lewis symbol for carbon and selenium.
What is a monatomic ion? How is a monatomic ion formed? What rules are involved?
What is a multivalent metal? Give an example.
What is a polyatomic ion? Give an example.
What are the rules for naming ions?
What is the symbol or name of the following;
a)
b)
c)
d)
e)
f)
magnesium ion? _________
phosphide ion? _________
phosphate ion? _________
copper (II) ion? _________
nitrite ion? __________
Fe+3? __________
What are the differences between ionic and molecular compounds in terms of
a) Their structure?
b) Nomenclature?
c) Properties?
What do you look for in an formula or name when determining whether a compound is ionic or
covalent?
What is a diatomic molecule? Provide an example.
What determines thesubscripts in the formula of an ionic compound? Give an example.
Name or provide the formula for the following;
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a)
b)
c)
d)
e)
f)
CaI2
Barium sulfide
Silver sulfate
Fe2(CO3)3
Carbon dioxide
NO
How are Lewis symbols used to determine the structure of a molecule? Draw the structure for
water and carbon dioxide.
What are the indicators of chemical change?
What is the Law of Conservation of Mass? In terms of a chemical reaction, what are the
implications?
Who are the reactants/products in a chemical reaction? Provide an example of a chemical reaction
by writing the word and skeletal equations.
When balancing a chemical equation, what are you allowed to change? Write and balance the
equation that describes the combustion of propane (C3H8).
What are the 6 types of reactions studied in this course? Provide the general “pattern” equation
and an example for each type.
What issues are associated with the combustion of a hydrocarbon?
How do you identify an acid/base from it’s formula?
What are the naming rules for binary acids and oxyacids? Provide examples for each.
What are the details of the pH scale?
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