introduction to chemicals and safety. read pages 658-660 & 176-178 and answer the following...
TRANSCRIPT
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Section 5.2 Introduction to Chemicals and Safety
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Safety Skills
Read pages 658-660 & 176-178 and answer the following questions.1. What does HHPS stand for?2. What does WHMIS stand for?3. Name 5 household products that are not reactive.4. Why do you think we use hazardous chemicals when
safer methods and materials are known?5. Give an example of a hazardous substance that might be
found in the1. Kitchen2. Bathroom3. Garage4. garden
6. Make a list of safety rules that should be followed in the lab. What sort of consequences should be put in place for students who do not follow the lab safety rules?
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Assignment:
Label the HHPS and WHMIS symbols. (handout)
Read and sign the Lab Safety Contract and have it signed by a parent/guardian.
Lab Safety Worksheet
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HHPS (Hazardous Household Products Symbols)
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WHMIS (Workplace Hazardous Materials Information System)
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WHAT IS CHEMISTRY?
Chemistry Is the study of matter, its
properties, and its changes or transformations.
Matter Is anything that has mass and
takes up space. Everything around us is made
up of matter (water, sand, DNA, oxygen, etc)
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States of Matter There are four states of matter. They are:
Solid (s) Liquid (l) Gas (g) Plasma
▪ does not have a definite shape or volume unless enclosed in a container▪ it may form structures such as filaments, beams and double layers▪ some common plasmas are stars and neon signs.
As you move from solid to a gas some of the atoms spread apart and the matter gains energy
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Physical and Chemical Properties Song All matter has physical and chemical
properties.
1. Physical Properties of chemicals describe the way they look. Examples include: colour, shine, strength, and state. A change in the way something looks is called a physical change. These include:
Evaporation (liquid to a gas) Freezing (liquid to a solid) Sublimation (solid to a gas) Melting (solid to a liquid) Condensation (gas to a liquid)
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A physical change is not permanent. It is easily reversed and does not change the chemical formula or properties of the matter.
2. Chemical Properties are the behaviors that happen when a substance changes into a new one. The change itself is called a chemical change.
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Reactants are the starting materials in a reaction.
Products are the new materials made in the reaction.
ReactantsProducts
Physical & Chemical Changes Song
H2 O2 H2O
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Assignment:
Complete the handout “Physical or Chemical Change?”
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Physical or Chemical Changes?Change Type of Change?
1. The steel wool turned the block pot shiny silver.
2. Lightning flashed across the sky.
3. Acid caused limestone to fizz.
4. The back steps are rotting out.
5. The piece of lemon turned the tea cloudy.
6. Spilt gasoline dried, but left a bad odor in the room.
7. The gravy in the refrigerator jelled.
8. A blue-green lobster turned red as it cooked.
9. A cavity appeared in a tooth.
10. Flash cameras flashed after the wedding photo.
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Chemicals and Chemical ChangesSection 5.1
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Classifying Matter
Matter
Pure Substances
Compounds Elements
Mixtures
Homogeneous Mixtures(Solutions)
Heterogeneous Mixtures
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Definitions
Pure Substances All the particles are the same. The substance has
constant properties.
A. Elements Are pure substances that are made up of only 1 type of
atom. They can be identified with a chemical symbol. Ex. Carbon = C
B. Compounds Are pure substances that contain two or more different
elements in fixed amounts. They can be written as a chemical formula. Ex. Water = H2O
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Mixtures Video Clip
Mixtures Are a combination of two or more substances that
are not chemically combined. They are simply in the same place at the same time.
Homogeneous Mixtures Mixtures are uniform. It’s parts are not
distinguishable. Ex. Pop, salt water.
Heterogeneous Mixtures Mixtures are not uniform. It’s parts are easily
distinguishable. Ex. Pizza, salad, sand and water.
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A Chemical Reaction usually occurs when:
1. Color Change occurs2. Gas is formed (bubbles)3. Precipitate
▪ A solid that forms in a liquid
4. Energy change▪ Exothermic – heat/light is given off (feels
warm)▪ Endothermic – heat is absorbed (feels cold)
5. Very difficult to reverse
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Assignment:
Read pages 172-174 and complete questions 1, 2, 4, 5 on page 175.
Complete the handout “Elements, Compounds and Mixtures”
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Atoms and Elements
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The Atom
The atom is the smallest particle of an element that retains the same properties of that element (Democritus, 4th century BCE).
Atoms are the basis for everything in the Universe. Everything is made of matterand all matter is made of atoms.
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Dalton’s Atomic Theory
John Dalton (1700) stated the following ideas:
1. All elements are composed of tiny indivisible particlescalled atoms.
2. Atoms of the same element are identical.The atoms of any one element are differentfrom those of any other element.
3. Atoms of different elements can combine witheach other in simple whole number ratios toform compounds.
4. Chemical reactions occur when atoms are separated,joined, or rearranged. However, atoms of one elementare not changed into atoms of another by a chemical reaction.
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Elements and Atomic Structure
The Bohr-Rutherford model of the atoms suggests that atoms are composed of three types of subatomic particles:1. Protons: heavy, positively charged
particles found in the core of the atom called a nucleus.
2. Neutrons: heavy, neutral particles found in the nucleus.
3. Electrons: light, negatively charged particles with almost no mass that circle the nucleus at different energy levels called orbits or shells.
Particle Symbol Charge Approximate Mass
Proton p+ 1+ 1
Neutron n0 0 1
Electron e- 1- 1/1840
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Atomic Structure
Atomic Number is the number of protons. This number is constant, it does not change.
Mass Number is the number of protons and neutrons. The number of neutrons can change, so the mass number is not constant.
Standard Atomic Notationfor an element shows it’s mass numberat the top, it’s chemical symboland it’s atomic number at the bottom.
Since atoms are neutral:# of electrons = # of protons.
Therefore:mass number – atomic number = # of neutrons
12C
6
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Chemical Symbols
Each element has a one or two letter symbol (a few have three). The first letter is always capitalized, and the second it is always lowercase.
For many, it is the first letter or two of their name.
Some symbols came from the element’s name in Latin, so the letters don’t always match the name.• Lead = Plumbum = Pb
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You are responsible for knowing the name and thesymbol for the following elements (spelling counts):
Name Name Name Name
H He Li Be
B C N O
F Ne Na Mg
Al Si P S
Cl Ar K Ca
Mn
Sb Zn Rn
Co I Br Ra
Fe Xe Kr Pb
Ni W Ag Hg
Cu Pt Sn Au
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Assignment:
Subatomic Particles Worksheet (handout)
Quiz on the 40 elements (names/symbols)
The Elements Song
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ElementName
Atomic Number
Mass Number
StandardAtomic Notation
# of p
# of e
# of n
Aluminum
40 Ar18
4
5
40
Carbon
19
19
2
0
Subatomic Particles Worksheet (Blackline Master 3.3)
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ElementName
Atomic Number
Mass Number
StandardAtomic Notation
# of p
# of e
# of n
3
12
Neon
7
8
31
19
14
16
Sodium
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The Periodic TableSection 5.5The Elements Song-Animated Periodic Table
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History of the Periodic Table
The periodic table was first arranged by Mendeleev according to mass number.
Mosely (1913), a student of Mendeleev, decided to try to arrange the periodic table according to atomic number. This method worked better and it is how the periodic table is arranged today.
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Each element behaves in a different way from all other elements because it has different properties.
However, some behave similarly so they are grouped together and arranged in rows and columns.
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Horizontal rows (across) are called periods. There are 7 of them. Elements are arranged by increasing atomic number.
A column (down) is known as a group. Elements in a family group share similar chemical properties.
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Group A Elements
Representative elements. Group 1A - Alkali metals react with water to form basic or
alkaline solutions. Group 2A - Alkaline Earth Metals react with oxygen to then
react with water to form alkaline solutions. Group 7A – Halogens combine with other elements to form
salts. Groups 8A - Noble Gases or Inert Gases are chemically
unreactive.
For Group A elements ONLY,if you know the group #, thenyou know the number of electronsin the outer shell or orbit.
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Group B Elements
Transition elements. Found in the middle of the periodic table. The group number does not indicate the
number of electrons in the outer shell.
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METALS
Elements found to the left of the “staircase” are metals. Common properties include: Shiny Conduct electricity Melt when heated Malleable (can be
beaten into thin sheets) Tend to lose electrons Ductile (can be formed
into wire)
NONMETALS
Elements found to the right of the “staircase” are nonmetals. Common properties include: Not shiny Not malleable Low melting point Poor conductor of
electricity Brittle Tend to gain electrons
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Metalloids
Elements found touching either side of the staircase are called metalloids or semi-metals. Have properties of both metals and nonmetals. Common properties include:
- Solids- Can be shiny or dull- Ductile- Malleable- Conduct electricity better than nonmetals
but not as good as metals.
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Assignment:
Classification of Elements Worksheet Periodic Table Puzzle (crossword)
Test on Thursday, March 10th (safety-ions)
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Elements 43, 61, and from 84 on are all radioactive.
Elements 43, 61, and from 93 on have been made by man (synthetic).
There are 11 gases: Hydrogen, Helium, Nitrogen, Oxygen, Fluorine, Neon, Chlorine,
Argon, Krypton, Xenon, Radon
There are 2 liquids: Bromine, Mercury
Inner Transition Elements Lanthanide Series – Begins at Cerium #58 Actinide Series – Begins at Throrium #90
Blank spots on the table are for elements that have notbeen made yet.
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Lanthanide SeriesActinide Series
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Electron Orbits and Energy Levels
Electrons are arranged in orbits around the nucleus of the atom. The orbits are also known as energy levels.
Orbits or Energy Levels Number of Electrons/Level
1 2
2 8
3 8
4 18
5 18
6 32
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Drawing Bohr-Rutherford Diagrams
Electron orbits are filled from the inside out. (The orbits closest to the nucleus fill first.)
Atoms are stable (do not react with other atoms) when their outermost orbit is full.
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Assignment:
Complete the sheet on Bohr-Rutherford Diagrams.
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BOHR-RUTHEFORD
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Lewis Dot Structures
Lewis Dot Structure shows only the valence electron arrangement for each element.
Valence electrons are electrons that are in the outermost energy level only. These are the electrons that will determine the ionic charge of an atom.
To draw Lewis dot diagrams write the symbol for the element, then draw dots around the symbol to represent the number of valence electrons. Electrons are placed one on each side going around the symbol.
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Lewis Dot:
Oxygen Fluorine
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HOMEWORK
1. Draw the Lewis Dot Structure for the first 20 elements
2. List all elements that are stable.3. List all elements that have only 1
electron in their outer level.4. List all elements that are only 1
electron short of a full outer level.5. Look for patterns on your periodic
table.
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LEWIS DOT
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Isotopes Isotopes are atoms that have the same number of
protons, but different numbers of neutrons. Therefore, they also have different mass numbers and different atomic masses. Isotopes are still chemically alike because they have identical numbers of protons and electrons.
Ex. Three Isotopes of Carbon are Carbon-12, Carbon-13, and Carbon-14. Complete the table for each.Symbol 12C
6
13C 6
14C 6
# neutrons 6
#protons 6
# electrons 6
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Ions
Normally, atoms have no charge because the number of protons (+) equals the number of electrons (-). When forming a compound, an atom can gain or lose 1 or more electrons.
Ion - an atom which has a positive or negative charge.
Remember - atoms want a full outer orbit, so they tend to lose or gain electrons to do this.
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There are two kinds of ions:
1. Cations An atom or group of atoms with a positive charge. Compared to a neutral atom, cations have less electrons. Metals tend to lose electrons and form cations.
2. Anions An atom or group of atoms with a negative charge. Compared to a neutral atom, anions have more electrons. Nonmetals tend to gain electrons and form anions. Names of anions end in “ide”
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Using the Periodic Table to Find Ionic Charges
1. Metals: groups IA (1A), IIA (2A), and IIIA (3A)
Lose electrons when they form ions. Their ionic charge is positive (cations). Their charge equals the group number.
Ex. Group 1A = 1+ Li+
Group 2A = 2+ Mg2+
Group 3A = 3+ Al3+
Elements in groups 4A and 8A usually don’t form ions
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2. Nonmetals: groups 5A, 6A, and 7A Gain electrons when they form ions (anions).
The charge is found by subtracting the 8 from the group number.
Ex. Group 5A = 5 - 8 = 3- N 3-
Group 6A = 6 - 8 = 2- O 2-
Group 7A = 7 - 8 = 1- F-
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3. Transition Metals (Group B) These charges can’t be read from the
periodic table. These metals can have more than one charge, so a roman numeral must be used to indicate which ion is used.
Ex. Iron (II) – Fe2+ and Iron (III) – Fe3+
Lead (II) – Pb2+ and Lead (IV) – Pb4+
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Ionic CompoundsSection 5.8
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Ionic Compounds
Binary Ionic Compounds Only contain two elements
Two ions held together by electrical attraction.
Made of a cation (metal) and a anion (nonmetal)
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Writing Formulas for Ionic Compounds
1. Write the symbol for your metal and nonmetal
2. Write the charges for each3. Cross-over the charges from top to
bottom4. Remove the charges5. Simplify the numbers and remove
the 1’s
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1. Sodium Chloride
2. Calcium Oxide
3. Calcium Phosphide
4. Mercury (II) Nitride
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Naming Ionic Compounds
1. Name the cation first!
2. Figure out if you need a Roman Numeral next to the cation (Group B Metal)
3. Name the anion (ending in the suffix “ide”)
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Formula Name
LiF Lithium Flouride
NaCl
CaCl2
Al2O3
CuBr2
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Polyatomic IonsSection 5.9
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Polyatomic Compounds
Ternary Ionic Compounds Contain three or more elements
Joined by an electrical attraction Pure substances that join:
1. A metal with a polyatomic ion2. A polyatomic ion with a nonmetal3. Two polyatomic ions
Polyatomic ions Groups of atoms that stay together and
carry an overall charge
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Common Polyatomic Ions and their Charges
Polyatomic Ion
Formula Charge
Hydroxide OH 1-
Nitrate NO3 1-
Chlorate ClO3 1-
Bicarbonate HCO3 1-
Carbonate CO3 2-
Sulfate SO4 2-
Phosphate PO4 3-
Ammonium NH4 1+
Fluorate FO3 1-
Iodate IO3 1-
Bromate BrO3 1-
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Writing Polyatomic Formulas
Following the same rules as for Ionic Compounds we….
1. Write the symbol for your metal and polyatomic ion
2. Write the charges for each3. Cross-over the charges from top to bottom
(if needed)4. Remove the charges5. Simplify the numbers and remove the 1’s
When you are adding a subscript to a polyatomic ion you must put brackets around it.
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1. Lithium nitrate
2. Sodium sulfate
3. Calcium carbonate
4. Ammonium chlorate
5. Aluminum hydroxide
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Naming Polyatomic Compounds
1. Name the cation and the polyatomic ion
Cation is always named first!2. Figure out if you need a Roman
Numeral in the name3. Which Roman Numeral4. Check your work
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Formula Name
K2CO3
Na2SO4
AgNO3
Ni2(CO3)3
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Comparing Ionic CompoundsIonic Compounds Formulas
2 elements(metal + nonmetal)
Names Name always has
an–ide ending
Polyatomic Compounds Formulas
3 or more elements(Metal + polyatomic ion)
If there are brackets it is automatically a polyatomic compound
Names Name always has an –ate
or –ite ending
EXCEPTIONSOH – hydroxideCN - cyanide
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Molecular CompoundsSection 5.10
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Molecular Compounds
Molecular Compounds Made of two nonmetals
and have no charge. Formed using covalent
bonds.
Covalent Bonds Shared pairs of electrons
between two nonmetal elements that hold the atom together.
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Diatomic Elements If these elements are
alone they pair up with another of their kind.
They are written with the subscript 2 (H2)
Share electrons in a covalent bond instead of existing alone by themselves.
These elements are known as the Magic 7 (they make the shape of a 7 on the periodic table…except for H)
I Have No Bright Or Clever Friends.
I2, H2, N2, Br2, O2, Cl2, F2
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Naming Molecular Compounds
1. The first element in the name is named using the full name
2. The second element is named using the ending –ide.
3. Prefixes are used for each element to indicate the number of atoms present.
4. The prefix –mono is only used to name the second element
CO = Carbon monoxide NOT Monocarbon monoxide.
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Prefixes in Molecular Compounds
Prefix Number Example
Mono- 1 Carbon monoxide CO
Di- 2 Carbon dioxide CO2
Tri- 3 Sulfur trioxide SO3
Tetra- 4 Carbon tetrafluoride CF4
Penta- 5 Phosphorus pentabromide
PBr5
Hexa- 6 Sulfur hexafluoride SF6
Hepta- 7 Dichlorine heptoxide Cl2O7
Octa- 8 Trichlorine octoxide Cl3O8
Nona- 9 Nonaphosphorus dichloride
P9Cl2
Deca- 10 Tetraphosphorus decoxide
P4O10
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Many molecular compounds have both common names and scientific names.Common
NameScientific Name
Water Dihydrogen monoxide
H2O
Ammonia Nitrogen trihydride NH3
Ozone Trioxide O3
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Writing Formulas for Molecular Compounds
1. Write the symbol for each element2. Write the subscript from the prefix
(no criss cross)
Do not write 1’s.
Do not reduce any numbers.
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Try the Following:
Dinitrogen tetrahydride
Heptafluorine hexoxide
Se8Cl3
S9I
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Characteristics of Ionic and Molecular Compounds
Ionic Compounds
High melting and boiling points
Usually solid at room temperature
Will dissolve in water Conduct electricity Atoms held together by
strong bonds Made of metals and
nonmetals Examples:
NaCl, AgI, Fe2O3
Molecular Compounds
Low melting and boiling points
Many are gases at room temperature
Will not dissolve in water, but can dissolve in non-aqueous solutions (don’t contain H2O)
Cannot conduct electricity Weak bonds between
molecules Made of nonmetals Examples:
H2O, CO2, CI2
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Naming Compounds Review
What is it made of?
2 elements (metal +
nonmetal)Name the
metalName the nonmetal
(“ide” ending)Do you need
Roman Numeral
s?
3 or more elements
Name the metal
Name the polyatomic ion (“ate or
“ite” ending)Do you need
Roman Numeral
s?
2 elements(nonmetals)Put prefixes in front of the names to tell how
many atoms there are.
*No Mono in the first name
The second name
ends in “ide”
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Writing Formulas Review
What is it made of?
2 elements (metal +
nonmetal)“ide” ending1. Write the
symbols2. Write the
Charges3. Cross
the Charges4. Remove
the Charges
5. Reduce and
Remove 1’s
3 or more elements
“ate or ite” ending
1. Write the symbols
2. Write the Charges3. Cross
the Charges4. Remove
the Charges
5. Reduce and
Remove 1’s*Brackets if necessary
2 elements(nonmetals)“ide” ending1. Write the
symbol2. Write the
subscript for the prefix.
3. Repeat for the next
element.
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Word EquationsSection 6.1
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Word Equations
A word equation is one way of representing a chemical reaction. It tells you what reacts and what is produced. Word equations are written like this:
Reactants -> Products
When hot steel wool (iron) is put into a bottle of oxygen, there is a spectacular reaction and iron (III) oxide is produced. The word equation would be:
Iron + Oxygen -> Iron (III) oxide
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Try These…
Write the word equations for each of the following examples:
1. A coil of copper wire is placed in a glass of colorless silver nitrate solution. Silver ions form on the coil, and the solution turns into copper (II) nitrate (which is blue).
2. Hydrogen and zinc chloride are produced when zinc is added to hydrochloric acid.
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Assignment
Do questions 1, 2, 3 & 4 on page 219
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Conserving MassSection 6.3
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Conserving Mass
The Law of Conservation of Mass states that in a chemical reaction, the total mass of the reactants is always equal to the total mass of the products.
Example 1:Methane + oxygen -> water + carbon dioxide
The mass of the methane and the oxygen combined should equal the mass of the water and the carbon dioxide.
If methane = 20g, oxygen = 30 g, and water = 40g what is the mass of the carbon dioxide?
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Example 2:Solution A has a mass of 50g. Solution B has a mass of 30g. When they are mixed together a chemical reaction occurs and a gas and a liquid are produced. If the mass of the final liquid is 60g, then how much gas was produced?
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Assignment
Do questions 1-5 on page 223.
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Counting Atoms
1. Subscripts C N2
2. Coefficients 3C 2N2H4
3. Brackets Al2(SO4)3
3Ca3(PO4)2
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Complete the examples below:
Type of Atom
# of Atoms Type of Atom
# of Atoms
CaF2 NH4NO3
Type of Atom
# of Atoms Type of Atom
# of Atoms
2CaF2
3Be(OH)2
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Balancing Chemical EquationsSection 6.5
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Skeleton Equations
A skeleton equation represents all chemicals by their formulas. It is NOT balanced. Skeleton equations and chemical equations are universal. They can be understood in every language all over the world!
Word Equation:
Methane + oxygen -> water + carbon dioxide
Skeleton Equation:
CH4 + O2 -> H2O + CO2
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Skeleton Equations
A skeleton equation is NOT balanced. These equations are universal and can be understood all over the world!
Word Equation:
Methane + oxygen -> water + carbon dioxide
Skeleton Equation:
CH4 + O2 -> H2O + CO2
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Balanced Chemical Equations In a balanced chemical equation
the reactants and the products are equal in the number of atoms. (This follows the Law of Conservation of Mass)
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Rules:
1. Begin balancing with the most complicated-looking group. A polyatomic ion, or the group that has the most elements and
numbers in it. 2. Lock this in with a coefficient of 1 and balance any uneven elements.3. Save any single elements in the reactant and products for
last. Especially if it is hydrogen or oxygen.
4. If you get stuck, double the most complicated-looking group and try again. 5. Make sure that all coefficients are in the lowest-possible ratio.
Know when to quit! None of the reactions you will encounter will be that difficult. If the coefficients are getting wild, double-check what you’ve done since you may have a simple mistake.
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Rules:
1. Begin balancing with the most complicated-looking group. A polyatomic ion, or the group that has the most elements and
numbers in it. 2. Lock this in with a coefficient of 1 and balance any
uneven elements.3. Save any single elements in the reactant and products for
last. Especially if it is hydrogen or oxygen.
4. If you get stuck, double the most complicated-looking group
and try again. 5. Make sure that all coefficients are in the lowest-possible
ratio.
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Balancing Examples
H2 + N2 -> NH3
Type of Atom
Reactants Products
H
N
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Balancing Examples
NaCl + BeF2 -> NaF + BeCl2
Type of Atom
Reactants Products
Na
Be
Cl
F
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Balancing Examples
K2O + H2O -> KOH
K2O + HOH -> KOHType of
AtomReactants Products
K
O
H
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Balancing Examples
FeCl3 + Be3(PO4)2 -> BeCl2
+ FePO4
Type of Atom
Reactants Products
Fe
Be
Cl
PO4
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Try These:
1. Mg + HNO3 -> H2 + Mg(NO3)2
2. Zn + HCl -> ZnCl2 + H2
3. Al + Fe3N2 -> AlN + Fe
4. Fe + O2 -> Fe2O3
5. KClO3 -> KCl + O2
6. O2 + C6H12O6 -> H2O + CO2
7. S8 + F2 -> SF6
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Assignment:
Complete the Hydrocarbons assignment and pass it in to be marked by Thursday, March 31st.
Answer the questions on a separate piece of paper and please use complete sentences!
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Types of ReactionsSection 6.6
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There are five main categories of chemical reactions:
1. Combustion2. Synthesis3. Decomposition4. Single Displacement5. Double Displacement
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Combustion
Combustion is the very rapid reaction of a substance with oxygen to produce compounds called oxides (CO2 and H2O). We often call this process burning.
The fuel can be a variety of things but it is often a hydrocarbon such as gasoline, natural gas, kerosene, or candles.
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Complete Combustion
The formula for combustion of a hydrocarbon is:
CX HX + O2 -> CO2 + H2O + energy
When you light a lighter the following reaction occurs:Butane + oxygen -> carbon + water +
energy dioxide
2C4H10 + 13O2 -> 8CO2 + 10H2O + energy
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Incomplete Combustion
Incomplete combustion occurs when there is not enough oxygen. The formula is:
CXHX + O2 -> CO2 + CO + C + H2O + energy
Carbon monoxide is an odourless, colourless gas that is extremely poisonous. It blocks the bodies ability to use oxygen, suffocating it and causing death.
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Synthesis and DecompositionSection 6.7
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Synthesis
Synthesis Reactions involve the combination of smaller atoms or compounds into larger compounds. They are also known as combination reactions. They have the following general formula:
A + B ➜ AB
If both reactants are element, then the reaction MUST be synthesis.
Eg. A B AB2H2 + O2 ➜ 2H2O
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Synthesis reactions sometimes involve joining two compounds into a larger one.
Eg.Hydrogen + ammonia ➜
ammonia chloride chloride
HCl + NH3 ➜ NH4Cl
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Decomposition
Decomposition Reactions involve the splitting of a large compound into smaller molecules or elements. They have the following general formula:
AB ➜ A + B
If there is only 1 reactant, then the reaction MUST be decomposition.
Eg. AB A B2H2O ➜ 2H2 + O2
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Single and Double ReplacementSection 6.9
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Single Replacement/Displacement
Single Displacement - The reactants MUST be an element and a compound. The general formula is:
A + BC ➜ B + AC
Single displacement can involve metals:
Eg. Na + KCl ➜ K + NaCl
Single displacement can involve nonmetals:
Eg. F2 + LiCl ➜ LiF + Cl2
Remember: If the single element is a metal it will replace the metal.
If the single element is a nonmetal it will replace the nonmetal.
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Double Replacement/Displacement
Double Displacement - The reactants are two compounds. Two elements replace one another to create new products.
AB + CD ➜ AD + CB
Eg.
NaOH + FeCl3 ➜ Fe(OH)3 + NaCl
When you write the two new compounds formed, you must cross charges to get the correct new formulas.
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synthesis
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Reaction Types Review:
Questions to Ask:
One Reactant?
Two Elements?
A Hydrocarbon and oxygen?
An Element and a compound?
Two Compounds
Yes
Yes
Yes
Yes
Yes
No
No
No
No
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HydrocarbonsSection 5.12
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Organic compounds are molecular substances that contain carbon and hydrogen atoms as building blocks. Methane is the simplest organic compound (CH4) and there are tens of thousands of others.
Carbon is the element that is most commonly found in molecules. That is because of it’s great combining capacity. Carbon has four lone valence electrons so it would like to bond or share with 4 other atoms. This is the maximum number of bonds a single atom can make!
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Most foods, and most of our bodies, are made up of organic compounds. The two main sources of organic compounds are:1. The ones that plants produce during photosynthesis
including sugars, carbohydrates, and fats.2. Fossil fuels found underground that were made
millions of years ago from decaying plant and animal material.
Hydrocarbons are compounds with only hydrogen and carbon in them. They are also known as fossil fuels. (Methane - CH4 , butane - C4H10 , propane - C5H12)
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Synthetic SubstancesSection 5.13
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Chemical Wizardry: Synthetic Substances
Natural products are obtained from natural sources like animals, plants, and minerals. Leather, wool, and cotton are examples.
Synthetic products are made by man. Lycra, kevlar, and vulcanized rubber are just a few examples.
Polymers are long thin molecules formed from smaller molecules linked together. They have very different properties than the molecules they are formed from. There are natural and artificial polymers. Plastics are made from polymers and so are starches found in potatoes.
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Acids and BasesSection 8.2 & 8.3
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Acids and bases are molecular compounds that break into ions in water.
An acid: - tastes sour- reacts with some metals to produce hydrogen gas- is a good conductor of electricity- reacts with a base to produce salt and water
Common acids include:Common Name Found in
vinegar (acetic acid) salad dressing
citric acid oranges and lemons
ascorbic acid vitamin C
lactic acid sour milk
carbonic acid carbonated drinks, pop
acetylsalicylic acid aspirin
sulfuric acid car batteries
hydrochloric acid your stomach for digestion
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A base: - tastes bitter- feels slippery- is a good conductor of electricity- reacts with an acid to produce salt
and water
Common bases include:Common Name Found in
sodium hydroxide drain cleaner
potassium hydroxide soap, cosmetics
aluminum hydroxide antacids (Tums)
ammonium hydroxide window cleaner
sodium bicarbonate baking soda
potassium sulfite food preservatives
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Bases react with proteins to break them into smaller molecules. A hair clogged drain may be cleared by treating it with a drain cleaner that contains sodium hydroxide.
Indicators are substances that turn different colours to indicate the presence of acids or bases. Litmus paper is one example of an indicator. Phenolphthalein is another popular indicator.
Chemists use the pH scale to represent how acidic or basic a solution is. It was developed in 1909 to allow scientists to compare the hydrogen ion concentration in various solutions. (pH stands for percent Hydrogen) The scale goes from 1 to 14. Most acids and bases can be ranked on this scale.
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pH 1.0 Highly AcidicpH 1.5 stomach acidpH 2.0 lemonspH 3.0 applespH 5.6 normal rainpH 6.5 milkpH 7.0 NeutralpH 8.2 baking sodapH 10.0 milk of
magnesiapH 12.4 bleachpH 13.5 drain cleanerpH 14.0 Highly Basic
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http://www.brainpopjr.com/science/matter/solidsliquidsandgases/grownups.weml
http://science.pppst.com/matter.html http://www.chem4kids.com/files/matter_states.html
http://images.google.ca/imgres?imgurl=http://www.designsuperhighway.com/Flash/thumbnails/labsafety.jpg&imgrefurl=http://www.designsuperhighway.com/Flash/labsafety.html&usg=___ai-qbmKGozRRmi4VFyI5RtILpA=&h=200&w=200&sz=66&hl=en&start=73&tbnid=0vom6O-8Y8V5aM:&tbnh=104&tbnw=104&prev=/images%3Fq%3DChemistry%2Blab%2Bsafety%26gbv%3D2%26ndsp%3D18%26hl%3Den%26safe%3Dactive%26sa%3DN%26start%3D72
http://listverse.com/2008/03/04/top-10-amazing-chemical-reactions/
http://www.nclark.net/ChemicalReactions