unit 3 - matter - wikispaceskmaring.wikispaces.com/file/view/unit 3 -...
TRANSCRIPT
Unit 3 - Matter
Atomic Structure, Introductory Chemistry
12/8/14
• Entry Task None – prepare for quiz. You will need a pencil and calculator. When finished, stay seated and raise hand for test to be collected. Finished early? Begin homework. Answer questions #1-7 on page 284 AND #1-6 on page 290. Plus vocab and definitions on the next slide…
HW p 284, 290, VOCAB
• Class time to work on HW:
• Read pages 278-290. Answer questions #1-7 on page 284 AND #1-6 on page 290.
• Due Thursday 12/11/14.
• Also, in C-notes form, define the following terms:
• Electric charge • Proton • Neutron • Electron • Nucleus • Atomic number • Isotopes • Mass number • Energy level • Quantum theory
12/8/14
• Exit Task
• Make sure you write down the homework questions and vocabulary!!
• Due Thursday 12/11/14
12/9/14
• Entry Task
• Explain everything you know about atomic structure. Make sure to add information when we share answers
• Unit 2 Test Reflections should be turned in!!
Today’s Agenda
• Watch movie to introduce elements.
• Nova: Hunting the Elements https://www.youtube.com/watch?v=wsoZFTC02PY
• Extra time? Work time for homework!
12/9/14
• Exit Task
• How much of the periodic table is metals?
• How much is non-metals?
12/10/14
• Entry Task
• Use a textbook and translate to your own words if possible.
• Define ATOMIC NUCLEUS, PROTON, NEUTRON and ELECTRON and explain where they are in the atom.
Today’s Agenda
• Finish movie and questions
• Notes on Atomic Structure
Atomic Structure- History and
the Nucleus
*take notes in your comp book
History – Dalton
• atoms could not be divided • all atoms of a given element are the same • different atoms could join to form LOTS of compounds
– Thomson • the plum pudding model • negatively-charged "plums” surrounded by • positively-charged "pudding”
– Rutherford http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/ruther14.swf
• atom has central charge surrounded by a cloud of orbiting electrons
– Bohr • electrons are in levels around the nucleus
– Quantum theory –at very small sizes, like size of an atom, matter and energy do not obey Newton’s laws or laws classical physics. • An electron appears in a wave-like “cloud” and have no
definite position.
Bohr model of the atom
Structure of the Atom
Particle Charge Mass (atomic mass units)
(amu)
Location
Proton positive
+
1 nucleus
Neutron
neutral
Ø
1 nucleus
Electron negative
-
0.0006
(or none)
orbit, level,
cloud
The Nucleus
A 1946 test of an atomic bomb in the lagoon at Bikini atoll. The
explosion has just started; surplus ships moored nearby can still be
seen.
• The nucleus
– the center of the atom holds
protons and neutrons
– held together by electromagnetic and strong
force
– 99.9% of the atom’s mass is here
– about 100,000 times smaller than
the entire atom
– the atomic number of an atom is the number
of protons in the nucleus
– mass number of an atom is the sum of the
protons plus neutrons
Isotopes
atoms with the
same number of
protons (and
therefore the same
element) but with a
different number of
neutrons.
NOTE: changing
the # neutrons does
not change charge.
Extra neutrons creates an isotope, what about more or less electrons?
• More or less electrons makes an ION:
• An atom that has an electric charge other than zero, created when an atom gains or loses electrons.
• Note: this changes the charge!
12/10/14
• Exit Task
• Describe the charges and relative locations of the particles in an atom. HINT: there are 3 particles.
• Reminder: homework due tomorrow! On separate paper for trade and grade/turning in (not in comp books)
12/11/14
• Entry Task
• INFORMATION: 6 protons, 6 neutrons, 6 electrons.
• Which element? • How did you know?
• TOMORROW!! Trade and Grade homework! • Discuss movie Q
• Notes about Atomic Structure
12/11/14
• Exit Task
• You may use a textbook:
• Define atomic number and mass number.
• Explain how they are different.
12/12/14
• Entry Task
• Say something nice
Today’s Agenda
• Finish notes
• Phet Lab
pHet
Atomic Structure
• Google phet
• It will be your first result, phet.colorado.edu/
• Click on Play with sims…
• Click on the Chemistry simulation.
• Click on Build an Atom.
• Click on Run Now!
• Open the 3 + green boxes
PHET QUESTIONS – Answer in comp books….
1. What is the charge of a proton, neutron, and
electron? Prove it.
2. What is the mass of a proton, neutron, and electron?
Prove it.
3. How is the mass number determined? Prove it.
4. Why is an atom sometimes unstable? Prove it.
5. What causes an atom to be neutral, (+) charged ion,
and (–) charged ion? Prove it.
6. Click on the Cloud. What is it trying to show you?
7. Look at the Symbol box. What do the numbers in it
represent? Prove it.
PHET QUESTIONS – Answer in comp books….
1. What is the charge of a proton, neutron, and
electron? Prove it.
2. What is the mass of a proton, neutron, and electron?
Prove it.
3. How is the mass number determined? Prove it.
4. Why is an atom sometimes unstable? Prove it.
5. What causes an atom to be neutral, (+) charged ion,
and (–) charged ion? Prove it.
6. Click on the Cloud. What is it trying to show you?
7. Look at the Symbol box. What do the numbers in it
represent? Prove it.
12/12/14
• Exit Task
• Trade and Grade
• Please turn in your entry/exit task sheet for the week.
12/15/14 • Entry Task
• Draw and label a NITROGEN “square” from the periodic table.
• Yours should be
similar to this example:
• How many protons does each nitrogen atom have?
• How many electrons does a neutral nitrogen atom have?
Today’s Agenda
• Work time for atomic structure worksheet.
• Finished early?
• Read pages 291-296.
• On page 296 answer #1-7.
• Read pages 311-314.
12/15/14
• Exit Task
• Consider the periodic table…
• Which element has just 1 proton?
• Which element has 2 protons?
12/16/14
• Entry Task
• If an atom had 7 protons, how many electrons would it have to be neutral? Explain.
• What element is it?
• Read pages 291-296. On page 296 answer #1-7. Due Thursday 12/18/14.
• Atomic Structure Worksheet also due Thursday
Today’s Agenda
• Review a few questions from the Atomic Structure worksheet.
• Electron Configuration Notes.
• Consider a Model of an Atom which uses marbles for particles.
ELECTRON CONFIGURATION: 12.2 Rules for energy levels
…take notes in your comp books.
Inside an atom, electrons always obey these rules:
1. The energy of an electron must match one of the energy levels in the atom.
2. Each energy level can hold only a certain number of electrons, and no more.
3. As electrons are added to an atom, they settle into the lowest unfilled energy level.
12.2 Energy levels
• In the Bohr model of the atom, the first energy level can accept up to two electrons.
• The second and third energy levels hold up to eight electrons each.
• The fourth and fifth energy levels hold 18 electrons.
• their exact location around the nucleus is not known--Heisenberg’s uncertainty principle
• So the electron orbitals represent a volume of space where an electron would have a 95% probability of being found
• many orbitals can make up an electron level – as electrons are added to an atom, they settle into
the lowest unfilled energy level
Valence electrons
• valence electrons are the electrons in the outermost energy level
• the properties of elements depends on how many electrons are in a particular atom’s different levels
• Atomic Structure worksheet due Monday.
• Paper Models of Atoms, an isotope of the atom and an ion of the atom.
12/16/14
• Exit Task - CANCELLED
• Define valence electrons and include a picture.
12/17/14
• Entry Task
• Define valence electrons.
• How many valence electrons does Group 1 have? Group 2? Group 3? Group 4? Group 5? Group 6? Group 7?
• The noble gases? What can you say about their outer shell?
ANSWERS
• Define valence electrons – are the electrons in the outer level.
• How many valence electrons does: • Group 1 has 1 valence electron. • Group 2 has 2 valence electron • Group 3 has 3 valence electron • Group 4 has 4 valence electron • Group 5 has 5 valence electron • Group 6 has 6 valence electron • Group 7 has 7 valence electron • The noble gases HAVE A FULL OUTER SHELL however many
it can take!
Today’s Agenda
• Trade and Grade Atom Structure Worksheet and homework.
• Receive your ATOM MODEL assignment.
• Build a model of one atom using marble models.
• Work on ATOM MODEL Drawings.
12/17/14
• Exit Task
• Draw the atom which has 3 protons, 4 neutrons, and 2 electrons.
• Is this an ion? How do you know?
• REMINDER HW and ATOMIC STRUCTURE WS due tomorrow!
12/18/14
• Entry Task
• INFORMATION: Atomic # 5 and mass number 11.
• Name the element. Draw and label an atom of this isotope, including electrons, protons and neutrons.
Today’s Agenda
• Trade and grade – Atomic Structure WS and Book homework.
• Build on of your isotope or ions using the marble models.
• Complete Atom Model Drawings
12/18/14
• Exit Task
• Draw and label the atom with 9 protons, 9 neutrons and 9 electrons.
• Will this atom be reactive? How do you know? (Hint: consider its valence electrons!)
1/5/15
• Entry Task
• INFORMATION: Atomic # 3, mass number 7, charge of +1.
• Name the element. Draw and label the ion, including electrons, protons and neutrons.
• How do you know this is an ION?
Today’s Agenda
• REMINDER: If you have not turned in your ATOM DRAWING (3 atoms of same element), it is DUE! Come see me if you have questions.
• TODAY: Review and reflect on ENERGY QUIZ.
• These reflections can also be completed at home because you can keep the original quiz.
• Start “Periodic Trends” assignment – color-coding the periodic table.
1/5/15
• Exit Task
• INFORMATION: Atomic # 9 and mass number 18 and charge -1.
• Name the element. Draw and label the ion, including electrons, protons and neutrons.
1/6/15
• Entry Task
• Using information from the textbook, Record several chemical properties of each group:
• Alkali Metals (1A)
• Alkali Earth Metals (2A)
• Halogens (7A)
• Noble Gases (8A)
Today’s Agenda
• Continue work on periodic table trends assignment. Today you should work on #1-8.
• Last 15 Minutes
• Start film and take notes on periodic table – chemical reactivity and trends – IN YOUR COMP BOOKS.
Ms. M’s notes – Periodic Table Movie with British Scientist
• Groups or families
• Chlorine - HALOGEN
• Hydrogen – ALKALI METAL
• Helium – NOBLE GAS
• How the elements are organized into columns based on chemical properties – Example Oxygen needed
during chemical reaction: combustion
• Used as war gas – halogen very toxic
• Very reactive and flammable, exploded Hindenburg
• NON-reactive – good for blimps
• Sulfur – non metal
• METALS – have metallic properties
• Dmitri Mendeleev – Russian
• Groups and Periods
• Non-metals Non-conductive
• Aluminum – metal – conducts electricity
• Mercury – liquid metal
• Iron – high melting point
• First organized elements into a table BUT did this by atomic mass. Noticed chemical similarities for groups.
• Columns and Rows
• Noble Gases • 6 Gases He, Ne, Ar, Kr, Xe, Rn – all colorless and odorless
• Atomic # and mass increases down column (density increases)
• Helium, Ne and Ar are lighter than air; Kr and XENON heavier than air and SINK
• Alkali Metals • All soft metals which can be cut by knife
• OXIDIZE on contact with air (have to be kept in oil) React more quickly down group
• REACTIVE – in H20 give of H2 gas
• Cesium exploded the whole beaker
Periodicity
• Comparing right and left
• Valence electrons
• Fluorine is super reactive
• Magnesium very reactive
• Determine periodicity across row – how many atoms will combine with how many other atoms
1/6/15
• Exit Task
• Describe where and how much of the periodic table is metals, nonmetals and metalloids.
• (You may use general terms like left, right, and fractions such as 1/3 or 2/3)
1/7/15
• Entry Task
• Consider page 294. Compare Halogens and Noble Gases.
• Can you relate their reactivity to their number of valence electrons? IOW how close are they to having a full outer shell?
• Now consider the Alkali metals. How would they achieve a full outer shell?
Add these definitions to your comp book notes LEFT SIDE…
• Ionic charge is the positive or negative charge an atom would have if it gained or lost valence electrons to be similar to a noble gas.
• SHOW IONIC CHARGE as a number and + or -. Example: Be 2+.
• Groups on left side of the table tend to lose electrons.
• Groups on the right side of the table tend to gain electrons.
• SHOW THIS TREND WITH ARROWS on your periodic table.
Today’s Agenda
• Complete Periodic Trends assignment – staple instructions to your colored/keyed periodic table.
• Info for #9 and 10:
• What is IONIC CHARGE?
• http://www.sciencegeek.net/tables/PT_ions.pdf
• Will the group tend to gain or lose electrons?
• http://dl.clackamas.edu/ch104-07/gaining.htm
• Complete movie and notes on Periodic Table.
1/7/15
• Exit Task
• Would the Alkali Metals (Group 1A) tend to gain or lose electrons? Why?
• Periodic Trends Assignment – TURN IN BY FRIDAY.
1/8/15
• Entry Task
• Tomorrow’s quiz will cover:
– Atomic structure – including particles, charges and locations
– Understanding key terms: atomic #, mass #, isotope, ion, energy level
– Drawing and labeling atoms based on information
– Periodic Table Basics
• What do you understand the most?
• What do you understand the least?
Today’s Agenda
• Complete quiz study guide.
• Finished? Your Periodic Table assignment is due tomorrow.
1/8/15
• Exit Task
• How is mass number found? How is this different than atomic mass given on the periodic table?
• Study TONIGHT! Chapter 12 and all your assignments I handed back!!
1/9/15
• Entry Task
• Say Something Nice
• Prepare for the quiz – you’ll need a pen/pencil and may use a calculator.
• PLEASE turn in your PERIODIC TABLE assignment.
1/9/15
• Exit Task
• Trade and Grade – if all are done with their quizzes.
• Please turn in your entry/exit task sheets for the week.
1/12/15
• Entry Task
• Read p 310 in your textbook. • Summarize and discuss why atoms form chemical
bonds. • Explain which groups are the most reactive and
why. • HOMEWORK: Read pages 308-317. And read
pages 334-338. Answer #1-8 on page 314 and #1-5 on page 342. Due Thursday 1/15/15.
Today’s Agenda
• Watch Bozeman Science “How to draw Lewis Dot Diagrams” https://www.youtube.com/watch?v=ulyopnxjAZ8
• WRITE ALL RULES AND EXAMPLES IN YOUR COMP BOOK.
• Work time for the worksheets on Covalent and Ionic Bonds.
1 2 3 4 5 6 7 0 8
# valence electrons
1+ 2+ 3+ 4+ 4-
3- 2- 1- 0 ionic charge
1/12/15
• Exit Task
• Draw a Lewis Dot Diagram for Hydrogen and one for Iodine.
1/13/15
• Entry Task
• Define IONIC BOND.
• Define COVALENT BOND.
• How are they similar? What is the difference?
• Consider pages 308-309 (or the glossary).
Today’s Agenda
• Discuss Ionic Bonding pages of worksheet.
• Ionic bonds involve a TRANSFER of electrons and attraction between + and – IONS.
• Covalent bonds involve sharing or pairs of electrons.
• Work time for Bonding Worksheets.
• Finished? Try some more…
1/13/15
• Exit Task
• Draw the lewis dot diagrams for hydrogen and carbon. Then show the compound CH4 (showing the covalent bonds as shared electrons).
1/14/15 • Entry Task
• Define chemical formula.
• Explain what the chemical formula C6H12O6 means
• How would you know if elements will form an ionic crystal or a covalent bond? Look at page 317.
Today’s Agenda
• Complete the next practice sheets on the ½ sheets AND in your comp book.
• potassium and bromine – Chemical formula:
• magnesium and oxygen – Chemical formula:
• lithium and oxygen – Chemical formula:
• calcium and chlorine – Chemical formula:
• magnesium and bromine – Chemical formula:
• calcium and nitrogen – Chemical formula:
Ionic Bonding – draw lewis dot for both elements, next show electron transfer, and write the chemical formula
• potassium and bromine – Chemical formula:
• magnesium and oxygen – Chemical formula:
• lithium and oxygen – Chemical formula:
• calcium and chlorine – Chemical formula:
• magnesium and bromine – Chemical formula:
• calcium and nitrogen – Chemical formula:
Ionic Bonding – draw lewis dot for both elements, next show electron transfer, and write the chemical formula
• 2 hydrogens and oxygen • Chemical formula:
• 1 oxygen and 1 oxygen – Chemical formula:
• 1 sulfur and 3 oxygen – Chemical formula:
• 1 sulfur and 2 oxygen – Chemical formula:
• 1 hydrogen and 1 carbon and 1 nitrogen Chemical formula:
Covalent Bonding – draw lewis dot for both elements, next show electron sharing, and write the chemical formula
• 2 hydrogens and oxygen • Chemical formula:
• 1 oxygen and 1 oxygen – Chemical formula:
• 1 sulfur and 3 oxygen – Chemical formula:
• 1 sulfur and 2 oxygen – Chemical formula:
• 1 hydrogen and 1 carbon and 1 nitrogen Chemical formula:
Covalent Bonding – draw lewis dot for both elements, next show electron sharing, and write the chemical formula
1/14/15 • Exit Task
• Draw the lewis dot diagrams for Calcium and for
Chlorine. • What would the chemical formula be for a compound
of Calcium and Chlorine? • Is this ionic or covalent?
• Reminder: HOMEWORK due tomorrow
1/15/15
• Entry Task
• Define chemical reaction. • Label the reactants and products in this equation: • Ba(NO3)2(aq) + K2CO3(aq) --> BaCO3(s) + 2KNO3(aq)
(page 336)
• Trade and grade homework. • Also turn in your Covalent/Ionic Bonds WS. • The ½ sheet should be in your COMP BOOKS
Today’s Agenda • Read the text. “Rearranging Atoms in Chemical Reactions”
Write this title in your comp books. • Write the 3 chemical reactions from the card in your comp
book • Using the “atom” cards, arrange the reactants. OF THE
FIRST EQUATION! • CHEMICAL REACTION! Place the arrow… • Rearrange the “atom” cards to make the products. • REPEAT ABOVE STEPS FOR SECOND EQUATION. • REPEAT ABOVE STEPS FOR THIRD EQUATION. • Was law of conservation of mass maintained? How do you
know? • Answer all questions at the end of the text in your comp
book. • Discuss.
1/15/15
• Exit Task
• Label the reactants and products in this equation:
• 6CO2 + 6H2O ------> C6H12O6 + 6O2
• How many CARBON atoms are on the reactant side?
• How many CARBON atoms are the product side?
1/16/15
• Entry Task
• Say Something Nice
• Please make sure it is NICE and regarding someone’s positive behavior in academics, community service, or friendship! This shouldn’t be a flirting contest!
Today’s Agenda
• Reflections on Atomic Structure Quiz
• “Rearranging Atoms” article and activity
1/16/15
• Exit Task
• Trade and Grade
• Please turn in your entry/exit task sheets.
1/20/15
• Entry Task
• Once a chemical reaction is complete, how much of the reactants will be left?
• If none, where did they go?
• Explain using this chemical equation as your example:
• 4 Fe + 3 O2 --> 2 Fe2O3
• NOTE: ALL WORK FOR THIS SEMESTER DUE THIS FRIDAY, January 23rd. Grades final for semester January 30th.
Today’s Agenda
• You will be reacting steel wool (iron) in oxygen.
• SET UP lab and during the 15 minutes of WAIT TIME you will finish assembling reactant molecules and rearranging into products
• Answer the 4 questions at the end of the “Rearranging Atoms” article in your comp books.
• When finished, complete the lab.
Lab Set-Up • Cut a 2 cm by 2 cm piece of steel wool from the beaker of vinegar on
front counter (this removes any grease).
• Cut 2 holes out of the index card – just bigger than the test tubes (see diagram)
• Pour 150 mL of water into other beaker
• Tape notecard to top. Invert one test tube.
• Push steel wool to bottom of other test tube with pencil. Invert this test tube. Tape down both test tubes.
• Record water level and appearance on Student Sheet
• WAIT 15 MINUTES – While waiting complete the “Rearranging Atoms” activity and questions in your comp book.
• Return to lab stations. Record your observations on the front page.
• CLEAN-UP: all steel wool and tape in garbage. Notecard in recycling. All glass materials rinsed. All items in tubs for next class.
• Answer questions on back of sheet.
Lab Set-Up • Cut a 2 cm by 2 cm piece of steel wool from the beaker of vinegar on
front counter (this removes any grease).
• Cut 2 holes out of the index card – just bigger than the test tubes (see diagram)
• Pour 150 mL of water into other beaker
• Tape notecard to top. Invert one test tube.
• Push steel wool to bottom of other test tube with pencil. Invert this test tube. Tape down both test tubes.
• Record water level and appearance on Student Sheet
• WAIT 15 MINUTES – While waiting complete the “Rearranging Atoms” activity and questions in your comp book.
• Return to lab stations. Record your observations on the front page.
• CLEAN-UP: all steel wool and tape in garbage. Notecard in recycling. All glass materials rinsed. All items in tubs for next class.
• Answer questions on back of sheet.
1/20/15
• Exit Task
• What 2 elements have probably combined together in the test tube containing the steel wool (iron)?
1/21/15
• Entry Task
• FINISH YESTERDAY’s EXIT TASK • What are the reactants and what are the
products in this chemical equation? • CuSO4 + Fe => FeSO4 + Cu
• Which of the above are compounds and which are pure elements?
• What do you think the iron will look like? The copper?
Today’s Agenda
• Complete and discuss the questions from the “Rearranging Atoms in Chemical Reactions” Text.
• Complete and discuss the questions from the steel wool (iron) and oxygen lab.
• Turn in these Steel Wool Lab Sheets. • Write down information to conduct the Copper
Sulfate Lab. • If 25 minutes remaining, conduct lab. • Less than 25 min? Read pages 343-346 “Types of
Reactions.”
• Purpose
– To react copper sulfate with iron, producing iron sulfate and copper.
• Materials
– copper sulfate (CuSO4) and Fe filings
– water
– beakers, mortar and pestle, graduated cylinder, stirring rod
– hot plate
– goggles
Write in your comp books –
Extracting Copper from Copper Sulfate
CuSO4 + Fe => FeSO4 + Cu
• Procedure 1. Wear your goggles. 2. Measure out about 3.5-4.0 g of CuSO4 crystals and place in a
beaker. 3. Add 20 ml of water to the CuSO4 in the beaker. 4. Use the hot plate with a setting of med-hi to help dissolve the
crystals. Stir and do not allow it to boil. 5. Measure out 1.0 g of iron (Fe) filings and leave in small plastic
tray. 6. Once the CuSO4 is dissolved, remove from heat and slowly add
the iron and then stir on and off for 3-4 minutes. 7. Carefully pour the liquid into waste container on the front
counter (not the metal!). 8. Rinse the “new” metal a few times. 9. Answer all questions. 10. Clean up – rinse all glassware. Dump copper in garbage.
Return all materials to bins for next class.
• Observations/Questions – answer in your comp books. 1. Describe the reactants (copper sulfate crystals and iron)
prior to the chemical reaction. 2. What happened to the copper sulfate when combined with
water? Do you think this step is a physical or chemical change?
3. Where did the iron go during the reaction? What happened to the copper sulfate?
4. List and describe all pieces of evidence you have that a chemical reaction occurred.
5. Describe the “new solid” in the bottom of beaker. What do you think it is?
6. Where did this product come from? 7. Look at the chemical equation. What other product was
formed? 8. Could you make the reaction go “backwards” -get the iron
metal and CuSO4 crystal back again? 9. Is this the way we extract this metal (or any metal for that
matter) in industry? If not, how do we get it?
1/21/15
• Exit Task
• List and describe evidence you MIGHT observe if a chemical reaction occurred?
1/22/15
• Entry Task
• Changes in matter can occur in 3 ways: physical changes, chemical changes or nuclear changes.
• Can you think of an example of each?
Today’s Agenda
• Complete Copper Sulfate Lab and Questions if you have not.
• When finished, work on “Physical, Chemical or Nuclear?” changes WS.
1/22/15
• Exit Task
• Is reacting copper sulfate and iron a chemical, physical or nuclear change?
• What evidence do you have?
1/23/15
• Entry Task
• Say Something Nice
Today’s Agenda
• Finish answering Q from Copper Sulfate Lab
• Complete and discuss “Chemical, Physical, or Nuclear WS”
• Review what should be finished in your comp books for Unit 3: Matter
• Monday we will do a study guide for the Unit 3 Test.
• Unit 3 Test will be given during your finals time.
Unit 3 Matter - Comp Books
• Atomic Structure Notes
• Phet Lab Q – Building Atoms
• Electron Configuration Notes
• Periodic Table Notes from Movie
• “How to Draw Lewis Dot Diagrams” Notes from Video
• Bond Practice ½ sheets – ionic/covalent
• Rearranging Atoms in Chemical Reactions – 3 equations and 4 Q
• Copper Sulfate Lab – Purpose and Procedure
• Copper Sulfate Lab – Observations and Questions
1/23/15
• Exit Task
• Trade and Grade
• Handout Unit Test 3 Study Guide
3/11/14
• Exit Task
• How are chemical formulas for ionic crystals and molecules similar? Different?
• Limewater Lab
• http://mattson.creighton.edu/Download_Folder/MattsonGasBook4thEdCO2.pdf