Physical Science Semester 2

Unit 4 Matter

2/3/14Week of 2/3 to 2/7

• Entry Task

• What are the “two pillars of science” that Einstein’s famous equation joined with c2 ?

• Explain what Lavoisier became famous for. • Explain what Faraday became famous for.

Today’s Agenda

• Finish notes on movie. • Please take note of people, year and place, and what

they accomplished as a scientist. • You will turn your notes in tomorrow after

discussion.

2/3/14

• Exit Task

• Give a detailed example of how society influences science and technology and vice versa.

• This example can be from the movie or real life.

2/4/14

• Entry Task

• Describe what you know about the structure of atoms.

• Homework: read pages 278-290. Answer questions #1-7 on page 284 AND #1-6 on page 290. Due Friday 2/7/14.

1812 – Michael Faraday, electricity/magnetism, London, only gentleman are scientists1885 Einstein as a child – his family designed lighting for the city1771 – Antoine Lavoisier, France, Conservation of Mass, French Revolution, he gets guillotine—disliked tax collector1897 Einstein in high school, poor student, fascinated by light1846 – Faraday realizes electricity and magnetism are connected, invents electric motor, names the “invisible light” electromagnetism1722- Emilie du Chatalay, France, “before her time”, translated Newton’s principia and realized he had made an error, velocity should be squared, fell in love with poet Voltaire, died at 43 after childbirth1905 – Einstein’s miracle year, Germany, 5 papers, including E=mc2 in 3 pages 1919 – Fame finds Einstein via Max Planck. He divorces Mileva, marries cousin1907 – Berlin, Germany; Lisa Meitner becomes first woman professor (1912)of physics1920-30 “Golden Age of Nuclear Research”1930’s – Nazis drive out Jewish intellectuals; Einstein leaves in 1933; Meitner barely escapes in 19381938 – Sweden, Robert Frisch (nephew) and Meitner “split the atom” realizing that lost mass is converted directly to energy during nuclear fission1944 – Hann awarded prize for discovering nuclear fission (Meitner got little credit)1942 Manhattan Project in US; bombs contain only a couple pounds of Uranium and Plutonium

Today’s Agenda – create a timeline• You will be placed into a team.• Compile your notes so that everyone has complete notes to turn in. • 1 = Energy• 2 = mass• 3 = light• 4 = velocity (speed of light squared)• 5 = development of e=mc2,• 6 = confirmation of e=mc2• Nominate a recorder, facilitator, data person, speaker. • WRITE CATEGORY ON TOP OF CARD. • One scientist per notecard. • Fill in Year, NAME, Nationality, Concept, Experiment(s), Challenges

Faced. • These cards will go on timeline from 1700 to 1950. • Your team will present your cards.

2/4/14

• Exit Task

• Explain how one scientist’s ideas evolved based on the work of other scientists.

• Hold onto your notes!!! You will need them for the timeline project! To be continued Thursday.

2/5/14

• Entry Task

• Explain how Einstein’s equation led to the splitting of the atom.

• Hold onto your E=mc2 notes!!! You will need them for the timeline project! To be continued Thursday.

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 Friday 2/7/14.

• Also, in C-notes form, define the following terms:

• Electric charge• Proton• Neutron• Electron• Nucleus• Atomic number• Isotopes• Mass number• Energy level• Quantum theory

2/5/14

• Exit Task

• You may use a textbook: • Define atomic number and mass number.• Explain how they are different.

2/6/14

• Entry Task

• What further questions do you have after having completed “Einstein’s Big Idea”?

• Take out your notes. Assign groups….

Today’s Agenda – create a timeline• You will be placed into a team.• Compile your notes so that everyone has complete notes to turn in. • 1 = Energy• 2 = mass• 3 = light• 4 = velocity (speed of light squared)• 5 = development of e=mc2,• 6 = confirmation of e=mc2• Nominate a recorder, facilitator, data person, speaker. • WRITE CATEGORY ON TOP OF CARD. • One scientist per notecard. • Fill in Year, NAME, Nationality, Concept, Experiment(s), Challenges Faced. • These cards will go on timeline from 1700 to 1950. • Your team will present your cards. • Presentations Last 10 minutes of class. Each team 2 minutes!• YOU WILL BE GRADED ON YOUR PARTICIPATION AS YOU WORK!

2/6/14

• Exit Task

• NONE – presentations for timeline.

• TURN IN YOUR NOTES on the way out of class…

2/7/14

• Entry Task

• Say Something Nice

• HW – Turn in. • Turn in Einstein Notes.• Turn in Entry/Exit Task Sheet

Today’s Agenda

• Finish any presentations from yesterday. • Take Unit 4 Pre Test• Complete the self-assessment side of the Unit

Map “blue sheet”– – Rate yourself 1-4 on each of the standards in the

“start unit” column

2/7/14

• Exit Task

• Trade and Grade• Please turn in your Entry/Exit task sheet for

the week.

2/10/14Week of 2/10 to 2/14

• Entry Task

• Describe the charges and relative locations of the particles in an atom. HINT: there are 3 particles.

• Per 3 and 4 – finish presentations• Per 1,3,4,6 – finish pretests• http://www.smithsonianmag.com/science-nature/how-

the-higgs-boson-was-found-4723520/

Today’s Agenda

• Mystery Boxes• Notes on Atomic Structure.

Mystery Boxes – in your comp books

• Purpose– Use the mystery boxes as models to demonstrate

how scientists comprehend the existence and structure of the atom without actually seeing all its parts.

Mystery Box Predictions and Confidence

BOXMusic On

predict % conf.

Music Off

predict % conf.

Look Inside

predict % conf.

See Objects

predict % conf.

WAIT

• Problem-Solve: Technological Design Process– Challenge: What else would you do to figure out

what is inside the mystery boxes? – Constraints: You cannot take the boxes apart.

Nor can you physically or chemically change them.

– Describe SEVERAL solutions to the problem.

2/10/14

• Exit Task

• CANCELLED – for mystery boxes

2/11/14

• Entry Task

• Draw and label a NITROGEN “square” from the periodic table.

• How many protons does each atom have? How many electrons?

Unit 4 Maps and Goals – “blue sheet”

• Complete your self-assessment for “start unit”• Graph your pre-test percentage. • Set goals for post-assessment. • Write down the TOP 3 standards you will need

to focus on. (These are the ones you feel the least confident about).

• Hold onto these until the end of the unit….

Today’s Agenda

• Finish Atomic Structure Notes.

2/11/14

• Exit Task

• Consider the periodic table…• Which element has just 1 proton? • Which element has 2 protons?

2/12/14

• Entry Task

• Draw and label an atom of Boron. Include all protons, neutrons and electrons. Assume it has no charge.

Today’s Agenda

• Finish atomic structure notes. • Atomic Structure Worksheet

Atomic Structure- History and the Nucleus

*take notes in your comp book

Atomic Structure video

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 is made up of a central charge surrounded by a cloud of orbiting electrons

– Bohr• electrons are in levels around the nucleus

– Quantum theory says that when things get very small, like the size of an atom, matter and energy do not obey Newton’s laws or other laws of classical physics.

• An electron appears in a wave-like “cloud and has no definite position.

Bohr model of the atom

Structure of the Atom

http://ut-images.s3.amazonaws.com/wp-content/uploads/2010/02/c-atom_e1.gif

Particle Charge Mass(atomic mass units)

(amu)

Location

Proton positive+

1 nucleus

Neutron neutralØ

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.

http://www.youtube.com/watch?v=bw85r24WW3s

• The nucleus– the center of the atom composed

of protons and neutrons– held together by four forces (electromagnetic,

strong , weak, and gravity)– 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– the atomic mass or mass number of an atom is

the sum of the protons and neutrons

Isotopesatoms with the same number of protons (and therefore the same element) but with a different number of neutrons.

Extra neutrons creates an isotope, what about more or less electrons?

• IONS: • An atom that has an

electric charge other than zero, created when an atom gains or loses electrons.

2/12/14

• Exit Task

• INFORMATION: 6 protons, 7 neutrons, 6 electrons.

• Which element? • Ion, Isotope or common form of the atom?

2/13/14

• Entry Task

• Draw and label an isotope of Boron which has 6 neutrons. Include all protons, neutrons and electrons.

• Any questions on Atomic Structure WS? This will be due TOMORROW – Friday Feb 14th.

Today’s Agenda

• Computers to “construct an atom.”

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.

2/13/14

• Exit Task

• How is the mass number determined? Please be specific and use vocabulary: protons, neutrons, and isotopes.

• REMINDER: ATOMIC STRUCTURE WS due tomorrow.

2/14/14

• Entry Task

• Happy Valentine’s Day• Say Something Nice

• ATOMIC STRUCTURE WS due today.

Today’s Agenda

• Discuss questions on Atomic Structure WS. • Trade and Grade – turn in. • Electron Configuration Notes• Read 12.3 and 12.4.

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.

• therefore, we say they are found in an electron cloud or orbital– 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 very last or outermost energy level

• the properties of elements depends on how many electrons are in a particular atom’s different levels

Review

• Basic Atomic Structure video (39 sec.)

2/14/14Week of 2/10 to 2/14

• Exit Task

• Trade and Grade – turn in entry/exit task sheets.

2/19/14Week of 2/19 to 2/21

• Entry Task

• Define valence electrons and include a picture.

• HOMEWORK: Read pages 288-314. On page 296 answer #1-7. On page 306 answer #3,5,6 (left side of page). On page 314 answer #1-8. Due Friday 2/21/14

Today’s Agenda

• Finish Electron Configuration notes.• Receive your atom, isotope, ion assignment. • Build a model of one atom using marble

models. • Work on Atom, Isotope, Ion Drawings.

2/19/14

• Exit Task

• INFORMATION: Atomic # 3 and mass number 7.

• Name the element. Draw and label the isotope, including electrons, protons and neutrons.

2/20/14

• Entry Task

• INFORMATION: Atomic # 5 and mass number 11.

• Name the element. Draw and label the isotope, including electrons, protons and neutrons.

• REMINDER: HOMEWORK DUE FRIDAY!

Today’s Agenda

• Yesterday you asked for…– MORE ABOUT ORBITALS and the periodic table:

http://www.ptable.com/#Orbital– http://

www.learner.org/interactives/periodic/elementary3.html– https://

www.khanacademy.org/science/chemistry/orbitals-and-electrons/v/orbitals

• Receive your atom, isotope, ion assignment. • Build a model of one atom using marble models. • Work on Atom, Isotope, Ion Drawings.

2/20/14

• Exit task – CANCELLED – ran out of time.

• Relate the group number (heads the columns on the periodic table) to the number of valence electrons.

• PS Skip the transition elements (groups 3-11) for now. http://www.chem4kids.com/files/elem_transmetal.html

•

2/21/14

• Entry Task

• Say Something Nice

• Is your HW complete? We will trade and grade in a few minutes…

Today’s Agenda

• Trade and Grade HW• Review how to build an ION – you can only

take away or add electrons.• Complete Atom, Ion, Isotope Drawings. • REMINDER – before you turn it in, check that

you have completed ALL STEPS (especially #5!)• Finished early? Start on Periodic Table

assignment…OR study for Monday’s Quiz

2/21/14

• Exit Task

• Trade and Grade• Please turn in your exit task sheets

2/24/14Week of 2/24 to 2/28

• 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

• TURN IN Atom, Isotope, Ion Drawings• Hand back and organize papers into binder• What should you have in your comp books?

– Atomic Structure Notes– Mystery Boxes– PHET Questions– Electron Configuration Notes

• Study for quiz by playing JEOPARDY!

2/24/14

• Exit Task

• INFORMATION: -3 ion of Atomic #7 element with a mass # of 14.

• Name the element. Draw and label the atom including protons, neutrons, and electrons.

2/25/14

• Entry Task

• NONE• PREPARE FOR QUIZ – you may use your comp

book for notes.

• END OF CLASS – turn in comp book to shelf.

2/26/14

• 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

• Watch film and take notes on periodic table – chemical reactivity and trends.

• Handout and work on Periodic Trends assignment.

• Please complete 1-10 carefully and in color or shading to show differences.

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 lighter than air; Ar and 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

• Flourine is super reactive

• Magnesium very reactive

• Determine periodicity across row – how many atoms will combine with how many other atoms

2/26/14

• 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)

2/27/14

• 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?

Today’s Agenda

• Continue work on periodic table trends assignment. Today you should work on #1-8.

• Watch “Hunting the Elements” video and answer Q/A.

2/27/14

• Exit Task

• Would the Alkali Metals (Group 1A) tend to gain or lose electrons? Why?

2/28/14

• Entry Task

• Say Something Nice

Today’s Agenda

• Watch “Hunting the Elements” video and answer Q/A.

• NOTE – The other periodic table movie notes will be turned in with this sheet!

• ALSO – your periodic table assignment will be due Monday AT THE END OF CLASS. But work on it over the weekend because we’ll only have 20 min

2/27/14

• Exit Task

• Trade and Grade Entry/Exit Task Sheets for the week of 2/23-2/27/14.

3/3/14Week of 3/3 to 3/7

• 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.

Today’s Agenda

• Finish movie and Q/A• Extra time? Work time for periodic tables. • SCHEDULE change: Periodic table assignment

will be due tomorrow after a total of 20 minutes work time.

3/3/14

• Exit Task

• How are the atoms arranged in COPPER or BRONZE?

3/4/14

• Entry Task

• Describe 2 patterns shown in the periodic table.

• HOMEWORK: (RE)Read pages 308-314 and 315-320. Answer #2,3,4,5,6 on page 330. And #15, 16, 17 and #2 on page 331. Due Friday 3/7/14.

Finish Movie…

• Start at 59 minutes. • Answer question 6, 7 and 8. • STOP MOVIE at 1:21. • TURN IN: You should STAPLE your first periodic

table move notes to your “NOVA – Hunting the elements” Q/A.

Get out your periodic table assignment.

• ON YOUR SHEET, WRITE DOWN ANSWERS 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 • 20 minutes work time• Extra time? Work on HOMEWORK!

To complete #9 and 10 on your periodic table assignment

• 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 a + 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.

3/4/14

• Exit Task

• How many valence electrons do alkali metals have?

• Are they likely to gain or lose electrons? • What would their ionic charge be?

3/5/14

• Entry Task

• Define IONIC BOND. Draw a picture. • Define COVALENT BOND. Draw a picture.• What is the difference?

• HOMEWORK: (RE)Read pages 308-314 and 315-320. Answer #2,3,4,5,6 on page 330. And #15, 16, 17 and #2 on page 331. Due Friday 3/7/14.

Today’s Agenda

• Checking in – Did you turn in BOTH movie notes and your Q/A?

• Please turn in your periodic table assignment – half sheet stapled on top with your name.

• GO OVER QUIZ ANSWERS. • Work time for reflections…• NOT REFLECTING? You can work on the

homework…• Extra Time? Work on Bonding Practice WS

3/5/14

• Exit Task

• Calculate your QUIZ PERCENTAGE: your score/30 x 100.• If you got 18 points or less (60% or less) you are REQUIRED to

complete a reflection. • If you do not like your percent, you may OPT to do a reflection. • Write down if will be doing a reflection and your reason.

• HOMEWORK: (RE)Read pages 308-314 and 315-320. Answer #2,3,4,5,6 on page 330. And #15, 16, 17 and #2 on page 331. Due Friday 3/7/14.

3/6/14• Entry Task

• If I told you a carbon atom is sharing electrons with 4 hydrogen atoms (CH4), would you say that is an ionic bond or covalent bond? WHY?

• HOMEWORK: (RE)Read pages 308-314 and 315-320. Answer #2,3,4,5,6 on page 330. And #15, 16, 17 and #2 on page 331. Due Friday 3/7/14.

Today’s Agenda

• QUIZ REFLECTIONS• Model LEWIS DOT DIAGRAMS and Ionic Bonds • WORK TIME:• HOMEWORK• Ionic Bonds WS• Covalent Bonds WS

Ions and Ionic Bond Activity

1 2 3 4 5 6 7 08# valence electrons

1+ 2+ 3+ 4+4-

3- 2- 1- 0ionic charge

• sodium and sodium ion• chlorine and chloride• magnesium and magnesium ion• nitrogen and nitride• aluminum and aluminum ion• argon

Elements and their ions

3/6/14

• Exit Task

• Draw a lewis dot diagram for Be and its ION.

3/7/14

• Entry Task

• Say Something Nice

• Trade and Grade • Please turn in your homework.• DID YOU TURN IN YOUR PERIODIC TABLE

ASSIGNMENT?

3/7/14

• Exit Task

• Trade and Grade entry/exit task sheets. • Please turn in your entry/exit task sheets for

the week.

3/10/14

• Entry Task

• Which electrons are involved in chemical bonds?

• Explain 2 reasons.

Today’s Agenda

• Watch Bozeman Science “How to draw Lewis Dot Diagrams” – NOTE he is giving all covalent bond examples.

• Consider 2 examples: – Ionic Bonds. – Covalent Bonds.

• Work time for the worksheets.

3/10/14

• Exit Task

• Draw the lewis dot diagrams for H2O (showing the covalent bonds as shared electrons).

3/11/14• Entry Task

• Define chemical formula. • Using C6H12O6 as an example, explain what this

chemical formula means.

• HOMEWORK: Read pages 323-325. On page 322 Answer #1-6. Read pages 334-340. On page 342 Answer #1-5. Due Friday 3/14/14.

• Bond WS due Wednesday. ANY QUESTIONS?

Today’s Agenda

• Draw Lewis Dot, convert to Ionic Bonds.• Record the chemical formula• Draw Lewis Dot, convert to Covalent Bonds.• Record 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 – lewis dot, compounds, 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 – lewis dot, compounds, chemical formula

Covalent Bonds - lewis dot, compounds, 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 nitrogenChemical formula:

Covalent Bonds - lewis dot, compounds, 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 nitrogenChemical formula:

3/11/14

• Exit Task

• How are chemical formulas for ionic crystals and molecules similar? Different?

3/12/14

• Entry Task

• How are chemical formulas for ionic crystals and molecules similar? Different?

• How do you think molecules and ionic crystals are similar? Different?

• Make a venn diagram!• http://

hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond2.html

Today’s Agenda

• Trade and Grade Bonds WS.• Class work time to practice ionic/covalent

bonds• Notes on Molecules, Ionic Crystals, and

Covalent Bonds in Carbon

3/12/14

• Exit Task

• Explain the meaning of the chemical formula for the ionic crystal CaCl2.

• HINT: what is the ratio of calcium atoms to Chlorine atoms? How do you know?

3/13/14

• Entry Task

How many covalent bonds can carbon form? • Draw a CO2 molecule and a methane CH4

molecule.

Today’s Agenda

• Finish classwork on ionic and covalent bonds. • Take notes in comp books on Chemical

Formulas, Carbon and Macromolecules.

3/13/14

• Exit Task

• What is the overall electrical charge of a compound?

• Review and complete classwork page.• https://

www.youtube.com/watch?v=REugD0mJxPk

3/14/14

• Entry Task

• Say Something Nice

• Is your homework complete? • We will trade and grade after SSN!

Today’s Agenda

• Trade and grade HW• Discuss classwork practice. • Finish notes.• Write down things to conduct lab on Monday.

Today’s Agenda

• Finish lab conclusions using data from the lab. • Start notes on chemical reactions.

3/14/14

• Exit Task

• Trade and Grade.• Please turn in your entry and exit task sheet

for the week.

3/17/14

• Entry Task

• Do you think the Alkaline Earth metals (Group 2A) will be more reactive down the group or up the group? Why?

Today’s Agenda

• Finish notes on Chemical Formulas, Carbon and Macromolecules.

• Prepare for lab. – Write pre-lab in comp books– Set up stations

Alkaline Earth Metals

• Question– Given four compounds containing an alkaline

earth metal (Mg, Ca, Sr, and Ba) what is the ranking of reactivity when mixed with three potassium compounds?

• Materials– safety goggles and spot plate– alkaline earth metal compounds and potassium

compounds• Mg(NO3)2 K2CO3

• Ca(NO3)2 K2SO4

• Ba(NO3)2 K2CrO4

• Sr(NO3)2

• Hypothesis• Procedure

– in one well of the spot plate, mix 5 drops of alkaline earth compound with 5 drops of a potassium compound. Do this for all 4 alkaline earth compounds combining with 3 potassium compounds. Total of 12 wells.

– record qualitative and quantitative data• precipitate (ppt.) color• strength of reaction (on a scale of 1-5)

– rinse down DRAIN when done• Data Collection• Conclusion

– results with data to support

Ba (NO3)2 Ca (NO3)2 Sr (NO3)2 Mg(NO3)2

K2CO3FOR EXAMPLE ONLY:white ppt.5

K2SO4

K2CrO4

Averagereaction

0 = no reaction <-> 5 = most reaction

EXAMPLE ONLY

• Conclusion (not real, do not copy, just an example of what to write)

– Ca(NO3)2 reacted the strongest with three potassium compounds with an average “score” of 4.3 on our scale of 1-5.

– Ba(NO3)2 reacted the next strongest with…

3/17/14

• Exit Task

• Using details from the notes, why do you think some biological molecules are called “macromolecules”?

3/18/14 – per 1,3,5 and 3/19/14 – per 2,4,6

• Entry Task

• What evidence of chemical reaction might you notice in today’s lab?

• Explain what the following chemical formula tells you:

• K2CO3

• Would this be ionic or covalent? How do you know?

Today’s Agenda

• 3-4 more slides on biological macromolecules• Pre-lab written in comp books• Conduct Lab and record data• Possibly time for conclusions.

• Exit Task

• Using evidence from the lab, rank the alkaline earth metals from most reactive to least reactive.

3/18/14 – per 1,3,5 and 3/19/14 – per 2,4,6

3/20/14

• Entry Task

• Explain what each of the following chemical formulas tell you:

• K2SO4

• K2CrO4

• Are these ionic or covalent compounds? How do you know?

Today’s Agenda

• Share data• Complete your conclusions.

– Was your hypothesis supported?– What can you conclude?– Most reactive and evidence– Least reactive and evidence– 2nd most reactive and evidence– 3rd most reactive and evidence– How does this evidence support your conclusion?

• Extra time? Consider your grade and complete any missing assignments.

Today’s Agenda

• Share data• Complete your conclusions.

– Was your hypothesis supported?– What can you conclude?– Most reactive and evidence– Least reactive and evidence– 2nd most reactive and evidence– 3rd most reactive and evidence– How does this evidence support your conclusion?

• Extra time? Consider your grade and complete any missing assignments.

3/20/14

• Exit Task

• What are the reactants and what are the products in the following chemical equation?

• Ba(NO3)2(aq) + K2CO3(aq) --> BaCO3(s) + 2KNO3(aq)

3/21/14

• Entry Task

• Say Something Nice

• Conclusions due MONDAY! Any Questions?

Today’s Agenda

• Read the text. • Using the “atom” cards, arrange the reactants. • CHEMICAL REACTION! Place the arrow…• Rearrange the “atom” cards to make the

products. • Was law of conservation of mass maintained?

How do you know?• Answer all questions on your own paper.

3/21/14

• Exit Task

• Trade and Grade• Please turn in Entry/Exit tasks

3/24/14Week of 3/24 to 3/28

• Entry Task

• What information can you understand from this chemical equation?

• Is this equation balanced? How can you tell?

CuSO4 + Fe => FeSO4 + Cu

Today’s Agenda

• Review and turn in 4 questions about conservation of mass in chemical reactions.

• Prepare for Copper Sulfate Lab.

• Purpose– To break the bonds between the copper (Cu) and

sulfate (SO4) in order to see the copper• Materials

– copper sulfate (CuSO4) and Fe filings– water– beakers, mortar and pestle, graduated cylinder,

stirring rod– hot plate

Extracting Copper from Copper Sulfate

CuSO4 + Fe => FeSO4 + Cu

• Procedure1. Measure out about 3.5-4.0 g of CuSO4 crystals and place

in a beaker.2. Add 20 ml of water to the CuSO4 in the beaker.

3. Use the hot plate with a setting of med-hi to help dissolve the crystals. Stir and do not allow it to boil.

4. Measure out 1.0 g of iron (Fe) filings and leave in small plastic tray.

5. Once the CuSO4 is dissolved, remove from heat and slowly add the iron and then stir on and off for 3-4 minutes.

6. Carefully pour the liquid down the drain (not the metal!). Rinse the “new” metal a few times.

• Observations/Questions1. Describe the “new solid” in the bottom of beaker

and what do you think it is?2. Where did the iron go?3. What tests could you do in order find out what the

new metal is?4. How did it get there (or where did it come from)?5. How could you make the reaction go “backwards”

(get the iron metal and CuSO4 crystal back again?

6. Is this the way we get this metal (or any metal for that matter?) If not, how do we get it?

CuSO4 + Fe => FeSO4 + Cu

describe describe describe describe

3/24/14

• Exit Task

• 6CO2 + 6H2O ------> C6H12O6 + O2

• Is this chemical equation balanced? If not, how could you balance it?

• HINT: count the C’s, O’s and H’s on the reactant side and compare to the product side.

3/25/14

• Entry Task

• 6CO2 + 6H2O ------> C6H12O6 + O2

• Is this chemical equation balanced? If not, how could you balance it?

• Try balancing this one: • __N2 + __F2 __NF3

Today’s Agenda

• Conduct the copper sulfate lab. • Finished with the lab? Sit down and answer

the 6 questions AND be sure to describe each of the reactants and products.

• Extra time? Begin work on the “Balancing Equations” Worksheet.

3/25/14

• Exit Task

• In the lab, describe which bonds were broken and which bonds formed. You may use information from the chemical equation to help you:

CuSO4 + Fe => FeSO4 + Cu

3/26/14

• Entry Task

• When balancing chemical equations, which numbers can you change?

• Which numbers can you not change?

Today’s Agenda

• Read pages 338-341 in your textbook. • Work on the “Balancing Equations” worksheet. • NOTE: Please focus on the easy ones first: • #2,6,8,11,14,16,18• Once you master those, work on the rest! • Remember your multiplication facts and if your

first plan doesn’t work….erase and try again• You may help each other but STAY SEATED and

working quietly.

3/26/14

• Exit Task

• Balance this chemical equation:• __P4 + __O2 __P2O3

3/27/14

• Entry Task

• Is mowing the lawn a physical, chemical or nuclear reaction?

• What about the combustion of gasoline in the engine?

• The sun shining?

• Please take out your “Balancing Equations” sheet.

Today’s Agenda

• Review “Balancing Equations” sheet. You will be asked to share – be willing You may fix your answers. TURN THESE IN!

• Discuss Copper Sulfate lab Q/A• FIGURE OUT: Complete “Chemical, Physical,

Nuclear” Worksheet.

3/27/14

• Exit Task

• Explain the difference between chemical reactions and nuclear reactions.

3/28/14

• Entry Task

• Say Something Nice

• “Chemical, Physical, Nuclear?” due Monday 3/31/14.

Today’s Agenda

• SHORT notes on fusion, fission, and radioactive decay.

• Conduct activity to generate a decay curve. • Answer questions at end.

3/28/14

• Exit Task

• Please turn in your entry/exit tasks.