do now: put away backpacks, silently work on catalyst: homework: ① write up due wed ② e.analysi...

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

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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)


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)


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)


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)


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?


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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.


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Homework:

TABLE OF CONTENTS:

CATALYST: How many valence electrons does oxygen have?


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+ 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” .


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

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Homework:

TABLE OF CONTENTS:

Within a CEL paragraph, what is the LINK part of the paragraph?


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+ 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!


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

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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!

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!

do now: put away backpacks, silently work on catalyst: homework: ① write up due wed ② e.analysi...

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