Download Chemistry Unit Outcomes

1
J. L. Ilsley High School
Chemistry in Action
Unit Outcomes
Instructor: R. K. Wamboldt
Texts:
Assignment 1
Safety Scavenger Hunt
After completing and studying Assignment 1 you should be able to:
1.
2.
3.
4.
5.
Identify and locate the following devices or pieces of equipment in the classroom/laboratory:
Fire extinguisher; Fire blanket; nearest Fire Alarm switch; safety goggles; aprons; eye wash
station; first aid kit; disposal container for broken glass.
Identify the warning labels on various chemicals and household products.
Outline the route (or draw a map) that you are to take to exit the school, and the location to
which you are to proceed, if the Fire Alarm rings while you are in Classroom/laboratory 318
or 316.
Outline the procedure to be followed if chemicals are spilled.
Outline the procedure to be followed before leaving the classroom/laboratory after you have
been working with chemicals.
Assignment 2
Common Laboratory Equipment Scavenger Hunt
After completing and studying Assignment 2 you should be able to:
1.
Identify each of the following pieces of common laboratory equipment:
ring stand; iron ring; test tube holder; test tube; beaker; Erlenmeyer flask; Florence flask;
mortar and pestle; wide-mouth bottle; graduated cylinder; thistle tube; pipet; funnel; wire
gauze; pneumatic trough; buret; gas measuring tube; evaporating dish; watch glass; buret
clamp; scoopula; crucible and cover; crucible tongs.
Assignment 3
Properties of Matter
After completing and studying Assignment 3 you should be able to:
1.
2.
3.
4.
List 5 ways in which the characteristics of matter can be observed.
Explain the meaning of the term physical property.
Outline what a physical property does not involve.
List 6 physical properties of matter and write and explanation or give an example of the meaning
of each physical property.
5. Explain the meaning of the physical property of matter known as state.
6. List the names of the 3 states of matter and describe how the shape and volume of each state of
matter is the same or different from each other.
7. Define each of the following terms as it relates to matter: hardness; malleability; ductility; melting
and boiling points; crystal form; solubility; viscosity; density (list 2 values of the density of water
– both mean the same)
8. Define the term chemical property of matter.
9. Describe what it means if a substance is combustible or flammable.
10. Outline what may occur or be observed if a material reacts with an acid.
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Lab 1
Examining a Piece of Gum
Lab 2
Observing a Peanut
After completing and studying Lab 1and Lab 2 you should be able to:
1.
2.
Define the terms qualitative observation and quantitative observation.
If provided with an object and the necessary equipment (eg: graduated cylinder, electronic
scale, ruler, etc) list 5 qualitative and 5 quantitative observations to describe the object.
Assignment 4
Physical and Chemical Changes
After completing and studying Assignment 4 you should be able to:
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2.
3.
4.
5.
6.
7.
8.
9.
10.
Describe what is known as a physical change.
List 7 types of physical changes.
Outline what it is possible to do with most physical changes.
Describe what happens to the original substance or substances during a chemical change.
Outline one thing that chemical changes always involve.
Explain one thing that it is very difficult to do with most chemical changes.
List 3 examples of chemical changes.
List 5 clues that might suggest that a chemical change has occurred. (Table 2 page 30)
If you are provided with a diagram or illustration of a type of change, identify: a) the specific
change that is occurring; b) type of change (physical or chemical); c) one clue or piece of
evidence that supports your choice of physical or chemical change.
Classify each of the following as a physical or chemical change. Provide one clue or piece of
evidence that supports your choice: garbage rotting; cutting up carrots; a silver spoon turning
black; making tea from tea leaves; bleaching a stain; boiling an egg; cooking a lobster.
Lab 3
Examining a Burning Candle
After completing and studying Lab 3 you should be able to:
1.
2.
List 5 qualitative and 3quantitative observations about the candle before it is lit.
Explain whether the candle changed chemically or physically or both physically and chemically
during the burning process. List one clue or piece of evidence to support your answer.
3. List 3 physical properties of the candle before it was burned.
4. List 3 physical properties of the candle after it was burned.
5. Give the name of the chemical reaction that describes the burning candle.
6. Name the reactants (ingredients) of this reaction.
7. Name the products (the things produced) of the reaction.
8. Explain whether heat was absorbed or produced during the reaction and provide one reason to
support your answer.
9. List the name of the process that produces heat. (Refer to Glossary in your text page 616)
10. List the name of the process that absorbs heat. (Refer to Glossary in your text page 615)
11. Write a word equation to describe the reaction showing the reactants and the products.
12. List 3 things that you observed during this activity that provide evidence that indicate a chemical
change occurred during the process of burning the candle.
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Lab 4
Identifying Substances Using Physical and Chemical Properties
After completing and studying Lab 4 you should be able to:
1.
If provided with an appropriate data table, use the physical and chemical data on the table to
name each of those substances, if their identity is unknown.
Lab 5
Examining Physical and Chemical Changes
Lab 6
Identifying Physical and Chemical Changes
After completing and studying Lab 5and Lab 6 you should be able to:
1.
If provided with a complete description of a change, identify the change as being physical or
chemical and list 3 pieces of evidence to support the answer.
Assignment 5
Elements and Compounds
After completing and studying Assignment 5 you should be able to:
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22.
Outline what is meant in science as a model.
Define the scientific meaning of the term matter.
List the 4 Principles contained in the Particle Theory of Matter. (Table 1 page 44)
Explain what is meant by a pure substance.
List 2 examples of pure substances.
Explain what is meant by a mixture.
List 2 examples of a mixture.
Outline from what a solution can be made.
List 3 examples of solutions.
Explain what is meant as a heterogeneous mixture.
Explain what is meant by as a solution. (Figure 1, Part b, page 45)
Define the term element
List the name of 2 elements.
Define the term compound.
Outline how compounds are formed.
List 1 example of a compound.
Give a description of each of the following type of substance: pure substance (element); pure
substance (compound); mixture (solution); mixture (heterogeneous). (Table 2, page 46)
Explain what is known as an atom.
Outline from what elements are formed.
Explain what is known as a molecule.
Outline, exactly, how elements join together to form compounds.
List 2 specific examples of how elements join together to form compounds.
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Assignment 6
Chemical Symbols and Formulas
After completing and studying Assignment 5 you should be able to:
1.
List the names of the first persons to recognize that it would be convenient to represent chemical
substances using symbols?
2. Outline what John Dalton, an English chemist, did in 1808.
3. Explain how Dalton represented element and why there was a problem with Dalton’s system.
4. Define the term chemical symbol.
5. List the names and chemical symbols for the following elements: aluminum, calcium, carbon,
chlorine, copper, gold, hydrogen, iron, magnesium, nitrogen, oxygen, potassium, sodium, and
sulfur.
6. Define the term chemical formula.
7. Outline what a chemical formula indicates.
8. Explain what is represented by each symbol in a formula.
9. Outline what is done, if only one atom, or if two or more atoms of an element, are present in a
chemical formula.
10. Explain the meaning of the term subscript, what it represents in a chemical formula, and give a
specific example of a chemical formula containing a subscript.
Inside The Atom
Assignment 7
After completing and studying Assignment 7 you should be able to:
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Outline, according the nuclear model of the atom, the composition of most of an atom.
List several characteristics of the positive nucleus of the atom.
Explain what is meant by a subatomic particle.
List 2 subatomic particles.
Outline who James Chadwick was and explain what Chadwick discovered.
Precisely, explain the characteristics of protons, neutrons and electrons and where they are located
in terms of the atom.
Explain why protons are especially significant or important. List an example.
Outline why an atom has no net electric charge.
For the atoms of oxygen and copper list the following: number of protons; total positive charge;
number of electrons; total negative charge; net charge of the atom.
For any atom define each of the following: atomic number; mass number.
Write the formula or explain how the number of neutrons in an atom can be calculated if the mass
number of the atom and the atomic number of the atom is known.
Outline what is meant by standard atomic notation.
If provided with a periodic table, write an example of the standard atomic notation for the
following atoms: chlorine; sodium; oxygen; magnesium; uranium.
Explain what is meant by an ion and how an atom becomes an ion.
List 2 characteristics of ions.
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Assignment 8
A “Planetary” Model of the Atom
After completing and studying Assignment 8 you should be able to
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8.
Outline, according to the planetary model of the atom, how electrons orbit the nucleus of an atom.
Outline what atoms and rainbows have in common.
Define the term spectrum.
Outline what happens when elements are heated in a flame.
Outline Who Niels Bohr was and explain what he proposed.
List 6 things that Bohr suggested in his “planetary” model of the atom.
Draw a diagram of Bohr’s model of the helium atom.
Draw and label a diagram showing an electron jumping out of its regular orbit, then returning of
its regular orbit, and explain what is produced when the atom return to its ground state.
9. Explain what is meant when it is said an electron is in an excited state.
10. Explain what is meant when it is said an electron is in the ground state.
Assignment 9
The Bohr Model of Electron Arrangement
After completing and studying Assignment 9 you should be able to:
1.
2.
3.
Explain what is represented by Bohr diagrams.
Describe the procedure for writing Bohr diagrams.
If provided with a periodic table, construct Bohr models for the electron arrangement for atoms of
hydrogen, nitrogen and phosphorus.
4. If provided with a periodic table, construct Bohr-Rutherford models for the electron arrangement
for atoms of Mg-24 and Cl-35.
5. Define the term ion.
6. Explain how many elements form ions.
7. Outline exactly how a magnesium atom becomes an ion.
8. Outline exactly how a chlorine atom becomes an ion.
9. If given a periodic table, construct a Bohr-Rutherford diagram for Mg-24 and Cl-35 ions.
10. Explain how the Bohr-Rutherford diagrams of the Mg-24 and Cl-35 atoms are different from the
Bohr-Rutherford diagrams of the Mg-24 and Cl-35 ions.
11. If provided with a periodic table, construct Bohr-Rutherford diagrams for oxygen, aluminum,
calcium, fluorine-20, boron 11, and potassium-40.
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Assignment 10
The Periodic Table
After completing and studying Assignment 10 you should be able to:
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2.
3.
4.
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6.
7.
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9.
10.
11.
12.
Define the term synthetic.
List the name of 3 items that are synthetic.
Name the building block of all substances, whether they are natural or synthetic.
Define the term compound.
Outline who Dmitri Mendeleev was, and list the name of his most significant invention.
Explain what is meant by the Periodic Table.
List the property that John Dalton and other scientists found that could be measured for an
element.
Define the term atomic mass.
Describe how Mendeleev organized his first periodic table.
Define a scientific law.
Outline what Mendeleev’s periodic law states.
Describe the process by which a scientific law is tested.
Assignment 11
Exploring The Modern Periodic Table
After completing and studying Assignment 11 you should be able to:
1.
2.
3.
4.
5.
Outline the basis on which Mendeleev had to choose to place an element in the periodic table.
State the contents of the modern periodic law.
Outline the properties of elements that are shown in the modern periodic law.
Define the term atomic radius.
If provided with a copy of the Periodic Table of the Elements, list the chemical symbol, the
melting point, the boiling point and state of several elements, and state whether each is a liquid,
solid, or gas at room temperature.
Assignment 12
Exploring the Modern Periodic Table
After completing and studying Assignment 12 you should be able to:
1.
2.
If provided with a copy of the periodic table, list the chemical symbol, atomic number and atomic
mass of specifically identified elements.
If provided with a copy of the periodic table, list the name, give the chemical symbol, and draw a
Bohr diagram for each element in group 1 and group 2.
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Assignment 13
Exploring the Modern Periodic Table
After completing and studying Assignment 13 you should be able to:
1.
2.
3.
4.
If provided with a copy of the periodic table, list the name, give the chemical symbol, and draw a
Bohr diagram for each of the elements in period or row 1.
Describe any general pattern that you can observe about the elements in any row as you move
across the periodic table.
Explain how the following properties of the elements generally change as you go from left to right
on the periodic table: atomic number; melting temperature; atomic radius.
Explain how the following properties of the elements generally change as you go down the
columns on the periodic table: atomic number; melting temperature; atomic radius.
Assignment 14
Exploring the Modern Periodic Table
After completing and studying Assignment 14 you should be able to:
1.
2.
3.
4.
If provided with a copy of the periodic table with the properties of an element omitted, use your
understanding of the regularities of the periodic table to predict the exact or approximate
properties of that element. (eg: atomic number, atomic mass, boiling point, etc.)
If provided with a copy of the periodic table, draw/construct a data table showing the atomic
radius and the atomic number of the first 20 elements..
Use the graphical analysis program and your data table (number 2 outcome above) to plot a graph
(best fit straight line) of atomic radius vs. atomic number for the first 20 elements on the periodic
table.
Use your completed graph (number 3 outcome above) to describe any general trends or
observations regarding the atomic radius and the atomic number of an element.
Assignment 15
Groups of Elements
After completing and studying Assignment 15 you should be able to:
1.
2.
3.
4.
5.
6.
7.
8.
Outline why the people who work with chemicals must know the properties of those chemicals.
Explain how scientists and people in other professions communicate about chemicals.
Define the terms chemical equation.
List 3 things for the periodic table is used.
Outline how scientists symbolize chemical elements such as the elements hydrogen and oxygen in
the compound water.
Define the terms physical property and chemical property of a substance.
List 3 physical properties that are shared by hydrogen and oxygen.
List 2 physical properties that hydrogen and oxygen have that are different.
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9.
Draw/construct a diagram of an atom of hydrogen and oxygen showing the nucleus, the location
of protons and neutrons, the location of electrons, and the electrical charges of each of the
subatomic particles
10. List one chemical property of both hydrogen and oxygen.
Assignment 16
Patterns in the Periodic Table
After completing and studying Assignment 16 you should be able to:
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Explain the meaning of the term bond.
Describe what occurs when the elements hydrogen and oxygen bond.
List the name of the horizontal rows and the vertical columns on the periodic table.
Draw/construct a diagram of the periodic table showing the periods and groups. Use colored
pencils or markers to show the location of metals, metalloids, and nonmetals. Draw in the
dark staircase.
Explain what is shown by the dark staircase near the right hand side the periodic table.
Describe the characteristic of the elements that border the dark staircase.
List the general name of the elements that border the dark staircase.
Draw a table showing metals, non-metals, and metalloids and the state, appearance,
conductivity, and malleability and ductility of each.
Define the term electron.
Explain what is known as an electron shell.
List the number of electrons that can be held in the first, second, third, and fourth electron
shell.
List the number of electron shells in the 2 elements of Period 1.
List the number of electron shells in the 8 elements of Period 2.
List the number of electron shells in the 8 elements of Period 3.
List the number of electron shells in the 2 elements shown of Period 4.
Describe the pattern that exists about the period and the number of electron shells.
If you are provided with a copy of the periodic table, count the number of outer-shell
electrons in Groups 1, 2, 3, 4, 5, 6, 7, and 8. Describe the pattern that you have discovered.
Assignment 17
Predicting Chemical Reactivity
After completing and studying Assignment 17 you should be able to:
1.
2.
3.
4.
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6.
7.
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9.
10.
11.
12.
Explain why electron shell diagrams are useful.
Outline why elements in the same group have similar properties.
Explain what knowing the number of outer shell electron in an element allows you to predict.
Describe how a chemical bond between 2 atoms forms.
Explain the meaning of what is known as a valence shell and valence electrons.
Outline to what chemical properties of elements are related.
Describe what is what is known as a metal in terms of valence electrons.
List 3 characteristics of an alkali metal of Group 1.
Describe what happens if one electron is removed from an alkali metal.
Define the term ion and cation.
If provided with a copy of the periodic table, draw/construct a diagram of a neutral sodium
atom and a charged sodium ion.
Explain the process by which a sodium atom becomes an ion.
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13.
14.
15.
16.
17.
18.
19.
20.
Describe the complete process, in terms of the number of protons and electrons, by which the
sodium atom become a sodium ion.
Explain why all the alkali metals of Group1 form cations easily and are chemically very
reactive.
Describe how the reactivity changes as you move down the alkali elements in Group 1.
Explain why this trend in chemical reactivity (explained in outcome number 15) occurs.
List an example of 2 elements that show this trend in chemical activity as you move down the
alkali elements in Group 1 of the periodic table.
Summarize why one atom is may be more reactive than another.
Define the term noble gas.
Describe how Group 1 (alkali metals) and Group 2 elements (alkaline earth metals) obtain a
noble gas valence shell arrangement.
Lab 7
Using Electrons to Identify Elements
After completing and studying Lab 7 you should be able to:
1.
Explain why atoms of different chemical elements give off characteristically different colors
of light when they are heated in a flame.
Assignment 18
Negatively Charged Ions: Anions
After completing and studying Assignment 18 you should be able to:
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Outline the pattern upon which Group 1 and Group 2 elements are based.
Explain what neutral atoms of Group 1 and Group 2 elements must do to become positively
charged cations.
Describe, as well as becoming positively charged, what can also happen to atoms.
List the general name of the materials that have the greater number of valence shell electrons.
Outline what non-metals have to do to fill their valence shells.
If provided with a periodic table, list the name of the elements in Group 17.
Outline the process by which Group 17 elements develop a noble gas electron arrangement.
Define the term anion.
Summarize the process by which a chlorine atom becomes a chlorine anion.
If provided with a copy of the periodic table, draw/construct a diagram showing the process
by which a chlorine atom becomes a chlorine anion.
Outline what halogens do when they gain an electron.
Explain how halogens are characterized in term of reactivity.
Outline how reactivity changes as you move down a group that is located in the center of the
periodic table.
Describe the process by which elements in Group 16 fill their valence shells.
Outline how Group 16 elements compare in terms of reactivity to the halogens in Group 17.
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Assignment 19
Electron Dot Diagrams
After completing and studying Assignment 19 you should be able to:
1.
2.
3.
4.
5.
6.
List one characteristic common to the atoms of all elements in any group of the periodic table.
Explain what is meant by an electron dot or Lewis diagram.
Explain, precisely how, an electron dot or Lewis diagram is drawn.
If provided with a copy of the periodic table, draw/construct an electron dot or Lewis diagram for the
atoms of Lithium and Fluorine.
Outline the reason why electron dot or Lewis diagrams are valuable tools.
If provided with a periodic table, draw electron dot or Lewis diagrams of specifically identified
atoms.
Assignment 20
Forming Compounds
After completing and studying Assignment 20 you should be able to:
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2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
Explain why the noble gases of Group 18 are very unlikely to take part in a chemical reaction.
Outline the very important clue to understanding how the atoms of elements combine in chemical
reactions.
List 3 things that happen when 2 atoms collide.
List and explain 3 ways in which an atom may acquire a valence shell like that of its closest noble
gas.
Define the term ionic compound.
Outline what is meant by an ionic bond.
Describe the relationship between a metal cation and an atom of the closest noble gas with a lower
atomic number. List 3 examples.
Define the term covalent bond.
Outline the meaning of the term molecule.
Explain the meaning of the term molecular compound.
List one characteristic of most molecular compounds.
List 2 ways in which non-metals may acquire the stability of a noble gas valence shell arrangement.
Outline the meaning of the term diatomic molecule.
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Assignment 21
Chemical Names and Formulas
After completing and studying Assignment 21 you should be able to:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
Outline what is meant by a binary compound.
Explain what occurs during the process of bonding.
Explain how you use the periodic table to predict the number of electrons that are transferred or
shared by an atom.
If you are provided with the names of several compounds, state whether or not they are binary
compounds.
List the name the types of elements that combine to form ionic compounds.
List 3 characteristics of ionic compounds
Name the types of elements that combine to form molecular compounds.
List 2 characteristics of molecular compounds.
If provided with the names and chemical formulas of several compounds, state whether each name
or formula belongs to an ionic compound or a molecular compound.
If provided with the chemical formulas for several compounds, identify the formulas that are written
correctly, and write correct formulas for those that are written incorrectly.
If provided with a table of ionic charges and a table of polyatomic ions, write chemical formulas for
specifically identified chemical compounds
Explain the reason why many ionic compounds are not binary.
Define the term polyatomic ion.
List the name of 1 polyatomic anion.
List the name of the only 3 common polyatomic cations.
Assignment 22
Chemical Equations and Chemical Reactions
After completing and studying Assignment 21 you should be able to:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
List the name of the simplest form of a chemical equation.
Write an example of a word equation showing the elements, reactants, + sign (what it means),
arrow (what it means), and products.
Outline why word equations provide limited information about a chemical reaction.
Explain what is meant by skeleton equation.
Outline what is summarized in a skeleton equation.
Outline what Lavoisier’s law and Dalton’s theory demand.
Explain what you must always do with a skeleton equation.
List the steps to be followed to make a chemical equation balanced.
Explain what a coefficient in front of the formula for a compound means.
Outline what is sometimes needed to be known about the chemicals in a chemical equation.
If provided with the appropriate information, list or draw/construct a table showing the states,
abbreviations, and an example of reactants and products of a chemical reaction.
List 5 guidelines that help in the balancing of chemical reactions.
Complete Problems 3 and 4 on page 174.
Chemical Equations and Chemical Reactions
Assignment 23
12
1.
2.
3.
Name the elements present, and the number of atoms of each
element, in each of the following:
a)
chloromethane, CH3Cl
b)
ammonium nitrate, NH4NO3
c)
glucose, C6H12O6
d)
sodium sulfate, Na2SO4
e)
calcium phosphate, Ca3(PO4)
Write the chemical formula for each of the following:
a)
ammonium bromide
b)
lead(II) carbonate
c)
barium sulfate
d)
ferrous nitrate
e)
strontium iodide
State whether each of the following is balanced:
a)
P + 5Cl2
 PCl5
b) H2SO4 + FeS  FeSO4 + H2S
c)
HBr + Fe(OH)3  FeBr3 + 3H2O
d) Zn + 2HCl
4.
(OVER)
 ZnCl2 + 2H2
a)
P4 + 5O2  P4O10
b)
C2H5OH + O2  2CO2 + H2O
c)
2Fe + O2  Fe2O3
Balance each of the following skeleton equations:
a)
HCl +
b) C3H8 +
Na2CO3 
O2 
NaCl +
CO2 +
H2O +
H2O
CO2
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c)
K2CO3 
HF +
d) CO2 +
e)
H2O

HCl 
Al(OH)3 +
5.
KF +
H2O +
C6H12O6 +
O2
AlCl3 +
H2O
CO2
The rusting of iron produces a compound with the formula Fe 2O3 . 3H2O. This is an iron
compound combined with 3 water molecules.
a)
Name the elements present and the number of atoms of each element in rust.
b)
The skeleton equation for the reaction is:
Fe +
O2 +
H2O 
Fe2O3 . 3H2O
Balance the skeleton equation for the rusting of iron.
Science 10
Name:
______________________________
Chemistry In Action
Chemical Formulas and Chemical Equations
Review
Assignment 24
a.
Write the name of each of the following compounds:
a)
P2O3
I)
Fe(ClO3)3
b) CrF3
j)
KC2H3O2
c)
l)
N2S3
d) (NH4)3P
m)
CaO
e)
Fe(OH)3
o)
HBr
f)
BaCO3
p)
ZnSO4
q)
Ag3P
K3PO4
g) As2O4
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h) Al(HSO4)3
b.
r)
HCl
Write chemical formulas for the following compounds:
a)
Magnesium Sulfate
b)
Mercury (II) Nitrate
c)
Zinc Sulfate
d)
Aluminum Fluoride
e)
Ammonium Carbonate
f)
Iron (III) Hydroxide
g)
Potassium Oxide
h)
Copper (II) Phosphate
i)
Tin (IV) Sulfide
j)
Nickel (III) Hydooxide
3.
Balance the following skeleton chemical equations:

a)
C4H8 +
O2
b)
Ag3PO4 +
Ba
c)
N2 +
d)
P4O10
e)
CuBr2 +
f)
NaClO3 
g)
NaOH +
(NH4)2SO4
h)
H2SO4 +
Al2O3
i)
Zn +
j)
C3H4 +
CO2 +

Ba3(PO)4 +

H2

O2

Fe2O3
CuO +
NaCl +
H2
Ag
NH3
P +
FeCl2
H2O
O2



Na2SO4 +
Al2(SO4)3 +
ZnCl2

FeBr3
+
C3H8
Fe
NH3 +
H 2O
H2O
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