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12/2/16
1
Chemistry Monday, November 28, 2016
Do-Now: “A-G Overview” 1. Write down today’s FLT
2. What classes do you need to take to graduate from Lawndale?
3. Are these requirements the same or different than college requirements?
4. When you apply to colleges, what can they see from your transcript?
Take out your planner and ToC
Announcements • ROCKSbuybacktomorrow• Usedojopoints• Unit3ExamnextweekJ
– Ch.5,6,7,8• Finals
– Oddperiods12/15– Evenperiods12/16
Planner: • Packet & Study for Unit test + final exam • 12/1 retake/make-up deadline
Table of Contents #3: 15. A-G Overview
FLT • I will be able to describe the differences
between HS graduation and CSU/UC requirements by completing A-G Overview
Standard N/A
Use this paper for A-G Requirements
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2
A-G Requirements • a – History/Social Science (Swearingen) • b – English (Pina) • c – Math (Schulze) • d – Science (Schulze) • e – Language (Swearingen) • f – Arts (Pina) • g – Electives (Hicks)
Use this paper for Reading Transcripts
Reading a Transcript • Highlights
– A/UC and B/UC – Sem 1 and Sem 2 – Credit Counts – Current Schedule
Reading a Transcript • GPAs
– Where are they? – Unweighted – Weighted – Cal Grant
LookatStudentx’stranscript
1) Counta-GClasses2) HowmanyAPclasses
didStudentxtake?3) WhatwasStudentX
rankinginhis/herClass?
4) PredictwhatschoolsStudentwasaccepted
intO.
15 A-G Classes
Required To apply for Cal States
and UC
UNIVERSITIES
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One year of world or European history One year of U.S. History AP/IB classes accepted
Does “2 Years Required” mean that it’s the recommended number?
No more than one year of ESL-type courses may be counted towards this
requirement
Including advanced algebra and geometry
Foundational subjects: biology
chemistry, physics
Sign language and classical languages (Latin and Greek) are accepted
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Dance, drama/theater, music, or visual art May be chosen from arts, social science,
English, advanced mathematics, laboratory sciences, and languages
AP Scores Credit Recovery Options • Summer School • E2020 • Adult School • Community College
• Note: Counselors refer to and counsel on these options. Please defer to counselors for student guidance in this area.
Connecting with a Counselor • Call Lorri Peterson (x3105) • Counselors
– Swearingen: BCA & A-Garcia, G – Hicks: AMA & Garcia, J. – Lopez, K. – Pina: ASLA & 9th Grade – Rojas: AVID & Lopez, R. – Portillo – Schulze: MSA & Prado – Z
SAT and ACT Tests • You can take the tests multiple times • I had to pay…at Lawndale you can get
a fee waiver from Mr. Orendain
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Other Notes
• Educational Prep Programs • Volunteer & Community Service
• Work Experience • Sports/Extra-curriculars • Awards & Honors
On Paper 1. Identify two differences between
graduation and A-G requirements. 2. In what ways are you meeting
graduation and A-G requirements? 3. If you could improve your transcript,
what would you do and why? 4. Explain what can make a student a
competitive UC/CSU applicant in 3-5 sentences
Finished? Quietly work on stamps or read Ch. 8
Chemistry Tuesday, November 29 – Wednesday,
November 30, 2016
Do-Now: “BrainPOP: Chemical Bonds” 1. Write down today’s FLT
2. Distinguish between an ionic bond and a metallic bond.
3. Can calcium and phosphorous form an ionic bond? Why or why not?
4. Write down the formula for calcium phosphide.
5. What are the four types of orbitals in an atom?
Take out your planner and ToC
Announcements • Unit3ExamnextweekJ
– Ch.5,6,7,8• Finals
– Oddperiods12/15– Evenperiods12/16
Planner: • Finish SA • Catch up on stamps
Table of Contents #3: 15. A-G Overview 16. BrainPOP: Chemical Bonds 17. 8.1 Cornell Notes
12/2/16
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BrainPOP:ChemicalBonds• WatchtheBrainPOPvideo• ANerthevideo,answerthequesPonsinyourgroup–everymembermustcopydownthesameanswer
• Thegroupwiththemostcorrectanswersà+5dojopointseach
hOps://www.brainpop.com/science/maOerandchemistry/chemicalbonds/
FLT • I will be able to describe the
arrangement of atoms in a covalent bond by completing 8.1 Cornell Notes
Standard HS-PS1-1:UsetheperiodictableasamodeltopredicttherelaRveproperResofelementsbasedonthepaOernsofelectronsintheoutermostenergylevelofatoms.
8.1: Covalent Bonding
Recall
Compounds • Compounds = substances made of
atoms of 2+ elements chemically combined in fixed ratios
Examples: MgCl2 H2O
Mg(NO3)2
Compounds • Compounds are held together by
chemical bonds
CH4
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Compounds • There are different types of chemical bonds,
including… – Ionic
Covalent
– Metallic
Ionic vs. Covalent Bonds • Ionic bonds involve the transfer of vse-s (gained or lost)
Ø Forms salts Ø Metal + Nonmetal
Ionic vs. Covalent Bonds • Covalent bonds involve the sharing of vse-s.
Ø Forms molecules (molecular compounds)
Ø Nonmetals
Check-In Would the following pairs of atoms most likely form a covalent or an ionic bond? 1. N and O 2. Na and O 3. Al and Cl 4. H and Cl
Covalent Bonds • Two electrons shared together have the
strength to hold two atoms together in a bond.
• Covalent bonds may form between atoms of the same element or different elements – H2 – O2 – CO2 – C6H12O6
Molecules § Manyelementsarenaturallyfoundasmolecules(covalentlybondedatoms)
§ Diatomicmolecules=twocovalentlybondedatoms(ex/N2)
§ Ex/Aircontainsoxygenmolecules,whicharediatomic(O2)
12/2/16
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How does H2 form?
• The nuclei repel each other, since they both have a positive charge (like charges repel).
++
(diatomic hydrogen molecule)
+ +
How does H2 form?
++
• But, the nuclei are attracted to the electrons
• They share the electrons, and this is called a �covalent bond�, and involves only NONMETALS!
Covalent Bonds: Recap • When nonmetals bond, they hold on to
their own valence e-s • In order to achieve a noble gas
configuration, they share their valence e-s with other nonmetals (covalent bonding)
Covalent bonding
• Fluorine has seven valence electrons (but would like to have 8)
F
Covalent bonding
• Fluorine has seven valence electrons
• A second atom also has seven
F F
Covalentbonding● Fluorinehassevenvalenceelectrons● Asecondatomalsohasseven● Bysharingelectrons…
F F
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Covalentbonding● Fluorinehassevenvalenceelectrons● Asecondatomalsohasseven● Bysharingelectrons…
F F
Covalentbonding● Fluorinehassevenvalenceelectrons● Asecondatomalsohasseven● Bysharingelectrons…
F F
Covalentbonding● Fluorinehassevenvalenceelectrons● Asecondatomalsohasseven● Bysharingelectrons…
F F
Covalentbonding● Fluorinehassevenvalenceelectrons● Asecondatomalsohasseven● Bysharingelectrons…
F F
Covalentbonding● Fluorinehassevenvalenceelectrons
● Asecondatomalsohasseven
● Bysharingelectrons…
● …bothendwithfullorbitals
F F
Covalentbonding● Fluorinehassevenvalenceelectrons
● Asecondatomalsohasseven
● Bysharingelectrons…
● …bothendwithfullorbitals
F F 8Valenceelectrons
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Covalentbonding● Fluorinehassevenvalenceelectrons
● Asecondatomalsohasseven
● Bysharingelectrons…
● …bothendwithfullorbitals
F F8Valenceelectrons
Covalentbonding● Drawthisexample:
F2
F F
Molecular Compounds • Properties: • Strong bond • Tend to have lower melting and boiling
points than salts • Typically liquids or gases at room
temperature – Recall: salts are typically solids
Molecular Compounds • Molecular formulas = show the # of
atoms of each element in a molecule • Ex/
H2O CO2
C2H6O
Molecular Compounds • What would the formula be for this
molecule?
Pair-Share-Respond1. Whathappenstothevalenceelectrons
inionicbonding?2. Whathappenstovalenceelectronsin
covalentbonding?3. Anionicbondoccursbetween_____
and______4. Acovalentbondoccursbetween_____
and_____5. Definetheterm“molecule”
12/2/16
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CW1. Pg.216:8.1SecPonAssessment1-6
– Samepaperasyournotes
2. Read8.2-8.3–harder!– LastsecPonsbeforetheexam
3. Finished?WorkonToCorstudyquietly
Chemistry Thursday, December 1– Friday, December 2,
2016
Do-Now: “8.2/8.3 Cornell Notes” 1. Write down today’s FLT
2. Remind me: how can you tell if atoms will form an ionic or a covalent bond?
3. Draw the electron dot diagram for Sulfur. 4. Use a pro-talk sentence frame to explain
the concept of covalent bonding. Take out your planner and ToC
Announcements • Unit3ExamnextweekJ
– Ch.5,6,7,8• Monday12/12willbeallperiods(nolatestart)
• Finals– Oddperiods12/15– Evenperiods12/16
Planner: • All stamps by end of next week! • Schedule final ahead of time if you will be
absent
Table of Contents #3: 18. 8.2/8.3 Cornell Notes 19. Lewis Structure WS
FLT • I will be able to describe the arrangement
of electrons covalent bonds using lewis dot structures by completing 8.2/8.3 Cornell Notes
Standard HS-PS1-1:UsetheperiodictableasamodeltopredicttherelaRveproperResofelementsbasedonthepaOernsofelectronsintheoutermostenergylevelofatoms.
12/2/16
12
8.2/8.3: The Nature of Covalent Bonding
Recall
Recall • Compounds are held together by
chemical bonds • Ionic Bond = electrostatic attraction
due to the transfer of vse-s between a metal and nonmetal
• Covalent Bond = formed from the sharing of vse-s between nonmetals
Molecules vs. Salts • NaCl • KBr • CO2 • HBr • NH3 • AlCl3
Single, Double, Triple Bonds
Single, Double, Triple Bonds • Covalent Bonds involve the sharing
of valence electrons • These electrons form strong single,
double, or triple covalent bonds between the atoms
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Single Bonds • Single Bonds = Formed when atoms
share one pair of vse-s (2 total) • Drawn as a line between atoms
• Ex:
Single, Double, Triple • However, sometimes atoms can
share more than one pair of electrons.
• When this happens, double or triple bonds form.
Single, Double, Triple • Double Bonds = atoms share two
pairs of vse-s (4 total) • Stronger and shorter than single bonds • Noted as two lines
Single, Double, Triple • Triple Bonds = atoms share three
pairs of vse-s (6 total) • Strongest, shortest, and most rigid • Noted as three lines
Lewis Structures
Remind me… • How any valence electrons in… 1. Li 2. S 3. Al 4. Br 5. Sr
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Lewis Structures • We can
represent the covalent bonding patterns in atoms using Lewis structures
Rules for Drawing Lewis Structures 1. Determine the total # of vse-s
ex/ PBr3
Rules for Drawing Lewis Structures 2. Place most metallic atom in center and connect with single bonds. Carbon is always in the center if present. Hydrogen is never in the center.
Rules for Drawing Lewis Structures 3. Use remainder of vse-s to fill in octets around outer atoms* *Atoms in 1s or 2s, like H, can only have 2 e-s
Rules for Drawing Lewis Structures 4. Place extra vse-s around the central atom
Rules for Drawing Lewis Structures 5. If you run out of vse-s, form double or triple bonds ex/ C2H4
12/2/16
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Extra Notes • Never add extra vse-s to H
Extra Notes • Charges must be +/- from total
vse-s • Ex/ NO3
-
Extra Notes • Indicate charges with brackets • Ex/ NO3
-
Extra Notes • Resonance occurs when there are
multiple possible structures • Ex/ NO3
-
Extra Notes • There are always exceptions
Extra Notes • Boron is a moron
12/2/16
16
Try This: SiBr4
1. Find the total number valence electrons
2. Draw the Lewis structure 3. Compare with your neighbor
CW1. LewisStructureWS2. StudyCh.83. Finished?WorkonToCorstudy
quietly