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DO NOW: Put away backpacks, silently work on catalyst:
Homework:
① Write Up due Wed
② E.Analysis due Thur
TABLE OF CONTENTS:
CATALYST:Lithium would likely gain 7 electrons to satisfy the octet rule or lose 1 electron? Why?
Unit 1: Atomic Theory and the Periodic Table
Pg Left Right
12 Concept Bubble Map (HW) Vocab Table
13 Unit 1 Practice Questions Notes: The Octet Rule & P. Table
14 Secret Agent Puzzle Notes: Periodic Trends
15 Unit 1 Practice Q’s Part 2 Podcast 4 Square
16 Quickwrites, Summary Notes: Sources of Energy
17 Practice Questions Notes: Radioactive Decay
18 EM Spectrum Discoveries Notes: EM Radiation
19 EM Wave Calculations Notes: EM Radiation (Part 2)
20 Draft of Write Up Write Up: Wave-Particle Principle
+
Reminder on Class Norms• Lining up outside (Line Monitors); Catalyst Procedures• Water and RR = You will lose extra credit (2 per semester) • Excessively off task or Ipad Misuse = detention without
warning• Bell = complete silence • Help each other but whisper. • Leave class clean and organized (pushed in chairs)
+
Important Discovering about the Atom
+ HEISENBERG UNCERTAINTY PRINCIPLE
• Heisenberg found that it is impossible to know both the exact position and momentum (velocity) of an electron at the same time.
• Werner Heisenberg …..won the the Nobel Prize for this.
+ Schrodinger’s Work• Erwin Schrodinger calculated the “probability”
of finding an electron in an atom. This disproved the Bohr Model of the atom.
• Electrons DON’T orbit the nucleus in orbits instead they are found in regions called electron clouds or orbitals.
+WAVE-PARTICLE DUALITY OF NATURE• Atoms absorb and release energy in the form
of photons or light energy. • Neils Bohr found that an electron has qualities
of both a particle and a wave. When measuring an electron’s position, it is found as a particle in space. But when you measure its velocity or momentum, it is treated as a wave.
+ Dr. Quantum: Wave-Particle Duality
Period 1 Group 1: Ismael (Leader) Melissa (Writer) Gem (Speaker)
Group 2: Norma R (Leader) Alfonso (Writer) Chris Flores (Speaker) Valerie (Speaker)
Group 3: Mathew (Leader) Alice (Writer) Kim (Speaker)
Group 4: (Outside) Miguel (Leader) Thea (Writer) Derek (Speaker)
Group 5: Cristian (Speaker) Leanne (Leader) Erwin (Writer)
Group 6 Daisy G (Leader) Esteban (Speaker) Angel (Writer)
Group 7: Aron (Writer) Anthony (Speaker) Heidi (Leader) Israel (Speaker)
Group 8: (Textbook Room) Ricky (Leader) Danae (Writer) Geronimo (Speaker) Samuel (Speaker)
Leader: facilitates, keeps group on task. Writer: Gathers info in the template/graphic organizerSpeaker: only person that can ask teacher questions and is the main reporter during class discussions
Period 3 Group 1: (Textbook Room) Mary Jane (Leader) Christopher (Writer) Julian (Speaker)
Group 2: Isabella (Leader) Stephanie (Writer) Jose Rodriguez (Speaker) Cristian (Speaker)
Group 3: Marcello (Leader) Daniel (Writer) Isaac(Speaker)
Group 4: Hannya (Leader) Abril (Writer) Leslie (Speaker)
Group 5: (Outside) Marco (Speaker) Adriana (Leader) Destiny (Writer)
Group 6 Jordan (Leader) Claudia (Speaker) Ana (Writer)
Group 7: Norma (Writer) Hilary (Speaker) Jessica (Leader)
Group 8: Kharoline (Leader) Mayra (Writer) Joshua (Speaker)
Leader: facilitates, keeps group on task. Writer: Gathers info in the template/graphic organizerSpeaker: only person that can ask teacher questions and is the main reporter during class discussions
Period 5 Group 1: Lupe (Leader) Ben (Writer) Chris (Speaker) Jesus (Speaker)
Group 2: Matthew(Leader) Ibrahim (Writer) Samantha (Speaker)
Group 3: Alanis(Leader) Nick (Writer) Sara (Speaker)
Group 4: Ashly (Leader) Kaela (Writer) Eduardo (Speaker) Amy (Speaker)
Group 5: Joel (Speaker) Andrea (Leader) Daniel (Writer)
Group 6 Lilly (Leader) Luis (Speaker) Art (Writer)
Group 7: Mark (Writer) Viviana (Speaker) Edgar (Leader)
Group 8: Seth (Leader) David (Writer) June (Speaker) Eric (Speaker)
Leader: facilitates, keeps group on task. Writer: Gathers info in the template/graphic organizerSpeaker: only person that can ask teacher questions and is the main reporter during class discussions
Period 4 Group 1: Jonathan (Leader) Daniel (Writer) Brian (Speaker) Lesley (Speaker)
Group 2: Sabrina (Leader) Ariel (Writer) Mia (Speaker) Victor (Speaker)
Group 3: Edrick (Leader) Armondo (Writer) Adrian (Speaker) Abel (Speaker)
Group 4: Group 5: Agustin (Speaker) Richard (Leader) Joshua (Writer) Joel
Group 6 Erwin (Leader) Marcos (Speaker) Marlene (Writer) Vanessa (Speaker)
Leader: facilitates, keeps group on task. Writer: Gathers info in the template/graphic organizerSpeaker: only person that can ask teacher questions and is the main reporter during class discussions
Period 6 Group 1: Andrew (Leader) Keanu (Writer) Joseph (Speaker)
Group 2: Isabel (Leader) Stephanie (Writer) Karina (Speaker) (Speaker)
Group 3: Amy (Leader) Ebony (Speaker) Daisy (Writer)
Group 4: (Outside) Silver (Leader) Sergio (Writer) Ivan (Speaker)
Group 5: Ambar (Speaker) Diana (Leader) Jaz (Writer)
Group 6 Kelsi (Leader) Jason (Speaker) Osman (Writer) Vanessa (Speaker)
Leader: facilitates, keeps group on task. Writer: Gathers info in the template/graphic organizerSpeaker: only person that can ask teacher questions and is the main reporter during class discussions
DO NOW: Backpacks away, silently work on catalyst:
Homework:
Test Correctio
ns due Thurs
TABLE OF CONTENTS:
CATALYST:Calcium is unstable because it has 2 valence electrons. How can calcium become stable with respect to the octet rule?
Unit 1: Atomic Theory and the Periodic Table
Pg Left Right
12 Concept Bubble Map (HW) Vocab Table
13 Unit 1 Practice Questions Notes: The Octet Rule & P. Table
14 Secret Agent Puzzle Notes: Periodic Trends
15 Unit 1 Practice Q’s Part 2 Podcast 4 Square
16 Quickwrites, Summary Notes: Sources of Energy
17 Practice Questions Notes: Radioactive Decay
18 EM Spectrum Discoveries Notes: EM Radiation
19 EM Wave Calculations Notes: EM Radiation (Part 2)
20 Error Walk Around Work Error Walk Around Work
+ Error-Correction Activity Norms
Go around to each poster See if you can identify the mistake. If you couldn’t
do it, write a tally on the board. Write down the common mistake or
misconception in your notebook found in the back of the sheet.
Don’t just give your partner(s) the answer, ask probing questions, hints.
Hints are provided in the envelopes.
Honors DO NOW: Backpacks away, silently work on catalyst:
Homework:
TABLE OF CONTENTS:
CATALYST:Using the formula, E = hv, if frequency goes up, then the energy will increase or decrease? Explain.
Unit 1: Atomic Theory and the Periodic Table
Pg Left Right
12 Concept Bubble Map (HW) Vocab Table
13 Unit 1 Practice Questions Notes: The Octet Rule & P. Table
14 Secret Agent Puzzle Notes: Periodic Trends
15 Unit 1 Practice Q’s Part 2 Podcast 4 Square
16 Quickwrites, Summary Notes: Sources of Energy
17 Practice Questions Notes: Radioactive Decay
18 EM Spectrum Discoveries Notes: EM Radiation
19 EM Wave Calculations Notes: EM Radiation (Part 2)
20 Error Walk Around Work Error Walk Around Work
DO NOW: Backpacks away, silently work on catalyst:
Homework:
TABLE OF CONTENTS:
CATALYST: How many valence electrons does oxygen have?
Unit 1: Atomic Theory and the Periodic Table
Pg Left Right
12 Concept Bubble Map (HW) Vocab Table
13 Unit 1 Practice Questions Notes: The Octet Rule & P. Table
14 Secret Agent Puzzle Notes: Periodic Trends
15 Unit 1 Practice Q’s Part 2 Podcast 4 Square
16 Quickwrites, Summary Notes: Sources of Energy
17 Practice Questions Notes: Radioactive Decay
18 EM Spectrum Discoveries Notes: EM Radiation
19 EM Wave Calculations Notes: EM Radiation (Part 2)
20 Error Walk Around Work Error Walk Around Work
+ Intro Activity to Bonding
• Follow the given directions carefully. • Find patterns as a group, do NOT ask me questions like, “Is the right?”
• No side conversations, on task. Time ticks!
• If you are NOT near the same pace as others, you were off task and your teacher won’t be happy with you. Once done, you are to annotate the “America’s Energy Crisis Project Handout” .
DO NOW: Backpacks away, silently work on catalyst:
Homework:
TABLE OF CONTENTS:
Which of the following is emitted in all forms of radioactive decay?A) energyB) beta particlesC) particlesD) electronsUnit 1: Atomic Theory and the Periodic Table
Pg Left Right
12 Concept Bubble Map (HW) Vocab Table
13 Unit 1 Practice Questions Notes: The Octet Rule & P. Table
14 Secret Agent Puzzle Notes: Periodic Trends
15 Unit 1 Practice Q’s Part 2 Podcast 4 Square
16 Quickwrites, Summary Notes: Sources of Energy
17 Practice Questions Notes: Radioactive Decay
18 EM Spectrum Discoveries Notes: EM Radiation
19 EM Wave Calculations Notes: EM Radiation (Part 2)
20 Error Walk Around Work Error Walk Around Work
DO NOW: Backpacks away, silently work on catalyst:
Homework:
TABLE OF CONTENTS:
Within a CEL paragraph, what is the LINK part of the paragraph?
Unit 1: Atomic Theory and the Periodic Table
Pg Left Right
12 Concept Bubble Map (HW) Vocab Table
13 Unit 1 Practice Questions Notes: The Octet Rule & P. Table
14 Secret Agent Puzzle Notes: Periodic Trends
15 Unit 1 Practice Q’s Part 2 Podcast 4 Square
16 Quickwrites, Summary Notes: Sources of Energy
17 Practice Questions Notes: Radioactive Decay
18 EM Spectrum Discoveries Notes: EM Radiation
19 EM Wave Calculations Notes: EM Radiation (Part 2)
20 Error Walk Around Work Error Walk Around Work
+ America’s Energy Crisis Project Annotate the Handout Begin Phase 1 on a Google Doc so you don’t lose
your project information This is a 2 month project, please don’t lose this
handout!
DO NOW: Backpacks away, silently work on catalyst:
Homework:
CEL Paragraph
Questions/Summary
TABLE OF CONTENTS:
Write the title of the new unit on the new table of contents.
Unit 2: Chemical Bonding, Reactions, Stoichiometry
Pg Left Right
21 Questions, Summary Notes: Chemical Bonding
FOCUS QUESTION – HOW DO VALENCE ELECTRONS ALLOW CARBON TO FORM BONDS IN DIAMONDS?
Ion Formation•When atoms gain/lose electrons, they gain a charge. # protons ≠ # of e-•Ion – An charged atom due to unequal number of protons and electrons•Cation – A positively charged ion•Anion – A negatively charged ion
+1+2 +3 ±4 -3 -2 -1
0Tend to lose electrons creating a positive charged cation.
Tend to gain electrons forming a negatively charged anion
Lithium would most likely lose an electron (NOT gain 7!) to become stable.
When it looses an electron, it becomes positively charged
So ,
Li +1 cation will form
Fluorine would most likely GAIN an electron (NOT lose 7!) to become stable.
When it gains an electron, it becomes negatively charged
So ,
F-1 anion will form
Element Group # of Valence Electrons
Gain or lose electrons to satisfy octet
rule
What ion forms?
Cation or Anion?
Calcium 2A 2 valence electrons
Lose 2 Ca+2 Cation
Phosphorus
Chlorine
Francium
Barium
Try on your own and when your teacher tells you to compare answers, THEN you will do that.
Exam Question #7
…..Explain the chemistry behind why elements in the same group demonstrate similar chemical properties.
All have the same # of valence electrons, so they will react in a similar way
Lewis Dot Structures
•Bohr diagrams take too long to draw – they’re boring!
•Lewis Dot structures only show the valence electrons.•Group number (Group 1A, 2A, 7A, 8A) tells us the number of valence electrons
One dot on each side, THEN pair up.
WRONG!
White Board Expectations!
• When using whiteboards:• Rule 1: Only academic drawing and writing is
allowed• Rule 2: Don’t hold up the white board until Mr.
Narez says “Boards Up!• Rule 3: You must attempt to write something!
“You miss 100% of the shots you don’t take!”-Wayne Gretzky
Class Example
•Draw the Lewis structure for fluorine
Partner Talk
•Draw the Lewis Structure for Carbon
Partner Talk
•Draw the Lewis Structure for oxygen
Stop and Jot•2 things: Draw the Lewis structure for Mg. What would the charge of a magnesium ion be after the Octet Rule is satisfied?
• Lose 2 electrons so Mg 2+ cation• Metal? Nonmetal?
Semi-metal?
• Conductor? Insulator?
• Cation or Anion?
• Alkaline earth metal?
• Metal! Nonmetal? Semi-metal?
• Conductor? Insulator?
• Cation or Anion?
• Alkaline earth metal?
• Conductor? Insulator?
• Cation or Anion?
• Alkaline earth metal?
• Conductor! Insulator?
• Cation or Anion?
• Alkaline earth metal?
• Cation or Anion?
• Alkaline earth metal?
• Cation! or Anion?
• Alkaline earth metal?
• Alkaline earth metal?
• Alkaline earth metal!
3 types of Bonding
Ionic Bonds
Metallic Bonds
CovalentBonds
Electrons can be either shared or transferred between elements to gain a full octet
How do you make table salt?
Ionic Bonds•Ionic Bond – A bond that forms between ions as a result of the elements transferring electrons. (NOT sharing!)OR•Bond forms due to cation – anion attraction that results from transferring electrons•Formed between metals and non-metals
Honors: How do ionic bonds link to what
we learned about ionization energy?
•Ionic bonds form because an atom with a low ionization energy loses its electron to an element with a high IE.
Lewis Structures for Ionic Bonds
Na Cl
Lewis Structures for Ionic Bonds
Na+ Cl-
Salts are always ionicly bonded!
Sodium Pure sodium metal reacts violently (and sometimes explosively) with water, producing sodium hydroxide, hydrogen gas, and heat:
2Na (s) + 2H2O (l) 2 NaOH (aq) + H2 (g)
ChlorideWorld War I Warfare
Table Salt
Check off the compounds in the list that are held by ionic bonds:
C and H K and Br F and F Ca and Cl O and H Li and F N and O
Ionic bonds are formed between metals and nonmetals
Check off the compounds in the list that are held by ionic bonds:
C and H K and Br F and F Ca and Cl O and H Li and F N and O
Ionic bonds are formed between metals and nonmetals
Don’t forget that H is a non-metals!
Crystal Lattice Investigation
Crystal Lattice
•Crystal lattices are salt crystals made of repeating units (like legos).
Na+Cl- Structure
+
+
+
+
+
-
--
-
Electrostatic Attraction•Positive ions are attracted to negative ions•This attraction holds crystal lattices together.•This attraction is known as electrostatic attraction
Electrostatic Attraction
Stick a Fork In It?!
Justify- Use your prior knowledge of metals
•Why don’t you put a fork in a power outlet? What property of the fork are you trying to avoid?
Chemical Bonding
Ionic Bonds
Metallic Bonds
CovalentBonds
Metallic Bonds•Forms between many metal atoms, where valence electrons are freely “jumping” between atoms (delocalized)
“Sea of Electrons”•This ability of valence e- to easily move around creates a “sea of electrons” within a metallic bond •Therefore, heat, charge/electricity can be easily transferred from one atom to another. •This is why metals on the left side of the PT are good conductors.
WHAT ARE COVALENT BONDS?
Chemical Bonding
Ionic Bonds
Metallic Bonds
CovalentBonds
Quickwrite: Without my help, write what you observe below. What is bonding? Why do you think they are bonding? What does the line represent? What else do you observe? (4-5 sentences)
Covalent Bonding•This is a bond between only non-metals (right side of PT) including hydrogen! •Electrons are shared between the elements so that each element can satisfy the octet rule and become stable.•Most molecules in biology are covalent compounds especially sugars!!• C-H bonds are always covalent. Atoms bonded to a twin are covalent N-N, C-C, O2
•More examples: OH, HCl, CF4 (ALL
nonmetals)
COVALENT BONDS PLAY WELL TOGETHER
Covalent Bonds Share!
Remember, bonding electrons are shown by lines instead of dots, and dots represent lone pairs
Are all the elements below held by covalent bonds in this amino acid?
Honors: How is electronegativity and covalent
bonding linked?• Covalent bonds form between
molecules that have similar electronegativities
• If one atom has a low EN and another a high EN, what bond would most likely form and why?
Covalent, Ionic, or Metallic Bond?
•If it is made of a metal and a non-metal, then it is an ionic bond•If it is made of only non-metals, then it is a covalent bond•If it is made of only metals, then it is metallic bonding.
Identify that Compound on # 6-10 of your study
guide
Classwork and Homework:
Complete 1-13 of your study guide
• Try on your own first • Share answers with partner• Talk about differences in answers
Exit Ticket
1.Draw the Lewis structure for boron.
2.Draw the Lewis structure for nitrogen. How many electrons will it gain/lose to satisfy the Octet Rule?
3.What is wrong with the Lewis structure below:Ca
+10 minutes max to complete:Catalyst: (Answer only)
Update Table of Contents: (label page #’s!!!!)Pg 40-41 Notes: Bonding (PPT Slides)Pg 44 - Quickwrite: Covalent BondsPg 45-46 – Lewis Dot StructuresHW: Complete 2nd row on the Lewis Dot Structure Worksheet
(3 sentences please) A “man atom” and a “woman atom” went out on a date. Describe the type of bond they are forming, and why there is a bond. Do charges form? Are they both metals? Nonmetals? Or one of each?
Amazing Bending Water!
Justify •What caused the water to bend?
Covalent Bonds can be polar or nonpolar
•Nonpolar Covalent Bond – Electrons shared equally between the atoms•Polar Covalent Bond – Electrons shared unequally due to difference in electronegativity•Electrons reside closest to the atom that is most electronegative
H FBecause fluorine is drastically more electronegative, it holds electrons closer to itself when in a covalent
bond with hydrogen.
H FHydrogen is given a partial positive
charge and fluorine is given a partial negative charge because it’s more
electronegative.
δ-δ+
Class Example•Label the location of the partial positive and partial negative charges in OH
Elbow Partner TalkLabel the location of the partial positive and partial negative charges in water.
Dipole Moments•Polar compound leads to the concentration of charge at the poles of the element.•This is known as a dipole moment
Exit TicketIndicate the dipole moment (if
any) for all molecules below after your drawing is complete
1.Draw the Lewis structure for H2O
2.Draw the Lewis structure for NH3
3.Draw the Lewis structure for HCN
Drawing Lewis Dot StructuresNot easy, don’t give up, keep trying
1. Connect elements using a line. C is always in the middle. Nitrogen is usually in the middle. H always on the outside.
2. Count all the valence e-s for the entire compound. Add them all up. Those are the # of electrons available! (Add electrons if anion, subtract electrons if cation)
3. Subtract that number from the # of electrons already used when you drew the lines.
Drawing Lewis Dot StructuresNot easy, don’t give up, keep trying
4. The remaining electrons are placed in pairs around the compound. 5. Make sure all elements are stable (octet rule). H needs 2. All others need 8. (Remember each line represents 2 bonding electrons) 6. If atoms are not stable (you used too many electrons that are not available) then erase a lone pair from that atom and draw a double bond on that atom If that doesn’t work then a triple bond may be needed. Use trial and error until all atoms follow the octet rule and the total number of electrons equals that of the available electrons you calculated in Step 2.
Hover Cam
• 5 Examples are demonstrated using HoverCam
• 20 pratice examples are for students to use to master the process of drawing lewis structures for compounds.
+10 minutes max to complete:Catalyst: (Answer only)In a chemical reaction, on the left side you have the stuff you start with, on the right the product or what you end up with. However, the equation must be balance meaning that the same # of atoms for one element must equal the # of atoms for that element on the other side. Here’s an example, Unbalanced: N2 + H2 NH3 You add coeffiences, big #’s till it’s balanced
Balanced: N2 + 3H2 2NH3
This requires trial and error. Try balancing this one: Unbalanced: Fe + Cl2 FeCl3
Balanced: ___________________
Update Table of Contents: (label page #’s!!!!))Pg 45-46 – Lewis Dot StructuresPg 47-48 – Silly Putty Lab
HW: Complete #14-22 over the weekend
Additional NotesPlease write on Pg 43 next to the slides where there is space: • When salts are added to water, the water
separates the ions because water is partially charged. (you’ll learn why next week)
• These separated ions allow water to conduct electricity.
Norms of Engagement: Silly Putty Lab
• Do NOT break anything• Do NOT touch hotplate • Do NOT place anything on hotplate, it will smell if you do and the fire alarm will go off.
• Use brain; use common sense • You fool around = Stay in the office • Do not spill anything• Clean up as much as possible, even if you didn’t dirty something!