chemical bonding unit 5

Chemical Bonding

Unit 5

Today…Today… Turn in:Turn in:

Sodium Party Reading Test (basket)Sodium Party Reading Test (basket) Goal Sheet (add test and find totals)Goal Sheet (add test and find totals)

• If you do not meet your goal write 2 things you’d do differentlyIf you do not meet your goal write 2 things you’d do differently

Our Plan:Our Plan: New CalendarNew Calendar Pre-LabPre-Lab Complete Inquiry LabComplete Inquiry Lab Wrap Up – Let’s Make a Venn DiagramWrap Up – Let’s Make a Venn Diagram

Homework (Write in Planner):Homework (Write in Planner): Lab due next classLab due next class


Get out your Lab & Note Booklet Get out your Lab & Note Booklet Our Plan:Our Plan:

Lab Discussion/NotesLab Discussion/Notes Find Someone WhoFind Someone Who Crash Course VideoCrash Course Video Notes – Ionic BondsNotes – Ionic Bonds Complete Worksheet #1Complete Worksheet #1 Wrap Up – Wrap Up – Clicker Review

Homework (Write in Planner):Homework (Write in Planner): Worksheet #1 due Next ClassWorksheet #1 due Next Class

Ionic CompoundsIonic CompoundsProperties:Properties:

HardHardCrystalline SolidsCrystalline SolidsBrittleBrittleWater-solubleWater-solubleHigh melting pointHigh melting pointCan conduct electricityCan conduct electricity

Molecular CompoundsMolecular Compounds

Properties:Properties:Soft, hard, or flexibleSoft, hard, or flexibleUsually less water-solubleUsually less water-solubleLower melting pointsLower melting pointsCannot conduct electricityCannot conduct electricity

Melting PointMelting Point

Ionic compounds have a higher Ionic compounds have a higher melting point because there is melting point because there is such a strong attraction in the such a strong attraction in the bonds. bonds.

It takes a higher temperature It takes a higher temperature (more energy) to break them.(more energy) to break them.

Conducting ElectricityConducting Electricity

Ionic compounds are able to conduct Ionic compounds are able to conduct electricity because they contain ions electricity because they contain ions (charged particles).(charged particles).

Electricity is the movement of Electricity is the movement of electrons and the ions spread out in electrons and the ions spread out in solution and allow electricity to be solution and allow electricity to be transferred.transferred.

Hairdryer in the bathtub exampleHairdryer in the bathtub example

Lab AnalysisLab Analysis

How does your Venn How does your Venn diagram compare to diagram compare to the true properties?the true properties?

Discuss with your Discuss with your team.team.

Turn in your LabTurn in your Lab

Find Someone WhoFind Someone WhoMove around the classroom to Move around the classroom to

find students who can answer find students who can answer the questions on your handout. the questions on your handout. Write their answer and obtain Write their answer and obtain their initials. You can not have their initials. You can not have the same student answer more the same student answer more than one question for you.than one question for you.

Crash Course IntroCrash Course Intro

http://www.youtube.com/watch?v=QXT4OVM4vXI

To 1:30To 1:30



CompoundCompoundA combination of two or A combination of two or more elementsmore elements

Elements form Elements form compounds because compounds because they want to be stable.they want to be stable.

Types of CompoundsTypes of Compounds There are three major types of There are three major types of

compounds:compounds: IonicIonic MolecularMolecular MetallicMetallic

IonicIonic compounds are made up of compounds are made up of ionic ionic bondsbonds, , molecular molecular compounds are made up compounds are made up of of covalent bonds, metallic covalent bonds, metallic compounds are compounds are made up of made up of metallic bondsmetallic bonds..

Types of CompoundsTypes of Compounds

Ionic Compounds – Metal & Ionic Compounds – Metal & NonmetalNonmetal

Molecular/Covalent Molecular/Covalent Compounds – Nonmetals OnlyCompounds – Nonmetals Only

Metallic Compounds – Metals Metallic Compounds – Metals OnlyOnly

Try It OutTry It Out

Which type of compound is:Which type of compound is:NaClNaClHH22SOSO44

PClPCl55KK22SS

Valence Electrons

• An atom’s outer An atom’s outer electronselectrons

• They are the ones that They are the ones that are available to be lost, are available to be lost, gained, or shared in a gained, or shared in a chemical bondchemical bond

Valence Electrons• The number of The number of

valence electrons valence electrons corresponds to corresponds to an atom’s group an atom’s group number!number!

• They are labeled at the They are labeled at the bottom of each column on bottom of each column on your PT (1 e-, 2 e-, etc.)your PT (1 e-, 2 e-, etc.)

Remember?

• The Octet Rule – Eight is The Octet Rule – Eight is Great, Except for Hydrogen Great, Except for Hydrogen and Helium, Two will Do!and Helium, Two will Do!

• Atoms gain, lose, or share Atoms gain, lose, or share electrons (BOND) so that electrons (BOND) so that they have an octetthey have an octet

Electron Dot Structures

• An element’s An element’s symbol with it’s symbol with it’s valence valence electrons drawn electrons drawn around itaround it

Electron Dot Notation• To Draw:To Draw:

1.1. Write the element’s symbolWrite the element’s symbol

2.2. Draw a dot for each valence Draw a dot for each valence electron around the symbolelectron around the symbol

3.3. Draw the dots singly before Draw the dots singly before doubling them up (Hund’s doubling them up (Hund’s Rule)Rule)

Electron Dot Notation

• After you write the symbol, the After you write the symbol, the areas around the symbol areas around the symbol represent the orbitals and axis:represent the orbitals and axis:

Ss orbital

px orbital

py orbital

pz orbital

Example

• CarbonCarbon

C

Carbon can make 4 bonds for a total of 8 electrons!

Example

• AluminumAluminum

AlHow many bonds can Al make?

3

Example

• BromineBromine

BrHow many bonds can Br make?

1

Try it Out!

• NitrogenNitrogen

• KryptonKrypton

N

Kr

How many bonds can N make?

3

How many bonds can Kr make?

0

Ionic BondsIonic BondsBond in which one atom Bond in which one atom

gains an egains an e-- & one loses an & one loses an ee--

Between a cation & an Between a cation & an anionanion

Ionic BondsIonic BondsBonds are made when opposite Bonds are made when opposite

charges are attracted to one charges are attracted to one another by electrostatic forcesanother by electrostatic forces

Though ionic compounds are made Though ionic compounds are made from ions (charged particles) they from ions (charged particles) they are electrically neutralare electrically neutral

The total charge of the compound is The total charge of the compound is 00

Ionic BondIonic Bond

cost.georgiasouthern.edu/. ../molecule/polar.htm

http://cost.georgiasouthern.edu/chemistry/general/molecule/polar.htm

Ionic BondIonic Bond

Chemical FormulaChemical FormulaThe subscripts in the formula tell you The subscripts in the formula tell you

how many atoms of each element how many atoms of each element are present in the compound.are present in the compound. HH22O – 2 Hydrogens + 1 OxygenO – 2 Hydrogens + 1 Oxygen

CC66HH1212OO66 – 6 Carbons + 12 – 6 Carbons + 12

Hydrogens + 6 OxygensHydrogens + 6 Oxygens NaCl – 1 Sodium + 1 ChlorineNaCl – 1 Sodium + 1 Chlorine

EXAMPLE – EXAMPLE – don’t write don’t write words, just pictureswords, just pictures

Lithium + BromineLithium + Bromine

Li Br1.Draw the electron dot structure for

each element.

EXAMPLEEXAMPLE Lithium + BromineLithium + Bromine

Li Br2.Draw an arrow to show the transfer of

electrons and move the electron to its new location.

EXAMPLEEXAMPLE Lithium + BromineLithium + Bromine

LiLi+1 +1 BrBr-1-1

LiBrLiBr3.Determine the charge for each ion and

write the formula.

Try it Out!Try it Out! Calcium + 2 FluorineCalcium + 2 Fluorine

Ca F1.Draw the electron dot structure for

each element.

F


Ca F2.Draw an arrow to show the transfer

of electrons and move the electron to its new location.

F


CaCa+2 +2 FF-1-1

CaFCaF22

3.Determine the charge for each ion and write the formula.

Metallic Bonds• Best characterized by Best characterized by

the phrase, “a sea of the phrase, “a sea of electrons”electrons”

• The valence electrons The valence electrons are mobile and can drift are mobile and can drift freely from one part of freely from one part of the metal to anotherthe metal to another

Metallic Bonds• The fact that electrons The fact that electrons

flow freely helps to flow freely helps to explain some of the explain some of the characteristics of metals:characteristics of metals:• Good conductorsGood conductors• Malleable Malleable • DuctileDuctile

AlloysAlloys Mixtures composed of two or more Mixtures composed of two or more

elements, at least one of which is a elements, at least one of which is a metalmetal

Their properties are often superior to Their properties are often superior to those of their component elementsthose of their component elements

Examples:Examples: Sterling Silver – 92.5% silver, 7.5% copperSterling Silver – 92.5% silver, 7.5% copper Bronze – 7 parts copper : 1 part tinBronze – 7 parts copper : 1 part tin Steel – Iron, Carbon, and small amounts of B, Steel – Iron, Carbon, and small amounts of B,

Cr, Mn, Mo, Ni, W, VCr, Mn, Mo, Ni, W, V

STOP!STOP!

Complete Worksheet #1Complete Worksheet #1Use the “helpful hints” handout Use the “helpful hints” handout

in your packet to complete #4in your packet to complete #4

Wrap UpWrap UpClicker Review


Worksheet #1– get out to checkWorksheet #1– get out to check Draw the structures for the bonding that occurs between Draw the structures for the bonding that occurs between

Barium and 2 Iodines on the bottom of your worksheet. Barium and 2 Iodines on the bottom of your worksheet. Include ions and formula.Include ions and formula.

Our Plan:Our Plan: Notes – Covalent Compounds & Lewis StructuresNotes – Covalent Compounds & Lewis Structures Begin Worksheet #2 (you can work on it again on Begin Worksheet #2 (you can work on it again on

Monday)Monday) Wrap Up – Pass the Paper ReviewWrap Up – Pass the Paper Review

Homework (Write in Planner):Homework (Write in Planner): Work on WorksheetWork on Worksheet

Molecular CompoundsMolecular Compounds

Covalent- sharing of electrons (tug of war)non polar covalentpolar covalent

Covalent BondCovalent Bond


http://cost.georgiasouthern.edu/chemistry/general/molecule/polar.htm

Covalent Bond

FormulasFormulasMolecular Formula – Shows how Molecular Formula – Shows how

many atoms of each element a many atoms of each element a molecule containsmolecule contains

Diatomic Molecule – molecule Diatomic Molecule – molecule consisting of two of the same atom consisting of two of the same atom (O(O22))

The formula does not tell you about a The formula does not tell you about a molecule’s structuremolecule’s structure

Covalent BondingCovalent BondingCovalent Bonds can be single, Covalent Bonds can be single,

double, or even triple (they can double, or even triple (they can share 1, 2, or 3 pairs of electrons)share 1, 2, or 3 pairs of electrons)

Bonds between atoms are Bonds between atoms are represented by a line. A double represented by a line. A double bond is two lines and a triple bond is bond is two lines and a triple bond is three.three.

Example : H-HExample : H-H

EXAMPLEEXAMPLE Iodine + IodineIodine + Iodine

I

1.Write the element in electron dot notation.

I


I

2.Rearrange the electrons to pair up electrons from each atom

I


I

3.Draw circles to show the sharing of electrons.

I


I

4.Draw the bond structure using symbols and lines. Use one line for each pair of electrons that are shared.

I I-I


I

5.Write the chemical formula for each molecule.

I I2

Try it Out!Try it Out! Nitrogen + NitrogenNitrogen + Nitrogen

N

1.Write the element in electron dot notation.

N


2.Rearrange the electrons to pair up electrons from each atom

N N


3.Draw circles to show the sharing of electrons.

N N


4.Draw the bond structure using symbols and lines. Use one line for each pair of electrons that are shared.

N N N-N


5.Write the chemical formula for each molecule.

N N N2

Stop!Stop!Complete Worksheet #2 in class Complete Worksheet #2 in class

(p. 7)(p. 7)

Crash Course IntroCrash Course Intro

http://www.youtube.com/watch?v=a8LF7JEb0IA Stop at 1:23Stop at 1:23

http://www.youtube.com/watch?v=a8LF7JEb0IA


Energy In BondsEnergy In BondsWhen bonds are made, energy When bonds are made, energy

(heat) is (heat) is releasedreleased..When bonds are broken, energy is When bonds are broken, energy is

requiredrequired.. It takes more energy to break stronger It takes more energy to break stronger

bonds. Triple bonds are the bonds. Triple bonds are the strongest. Single bonds are the strongest. Single bonds are the weakest.weakest.

Energy In BondsEnergy In Bonds

Bond dissociation energy – the Bond dissociation energy – the energy required to break a bond energy required to break a bond between two covalently bonded between two covalently bonded atomsatoms

The larger the bond dissociation The larger the bond dissociation energy, the stronger the bondenergy, the stronger the bond

Lewis Structures

• Using electron dot Using electron dot structures, we can draw structures, we can draw Lewis structures – formulas Lewis structures – formulas that show how elements that show how elements bond and where their bond and where their electrons goelectrons go

Lewis StructuresLewis StructuresThey only work to show They only work to show

COVALENTCOVALENT bonding because bonding because they show how atoms they show how atoms SHARESHARE electrons.electrons.

For For IONICIONIC compounds we draw compounds we draw dot models demonstrating how dot models demonstrating how electrons move electrons move (like last class)(like last class)

Ionic Bonding Structures

• Realize that electrons Realize that electrons are NOT being sharedare NOT being shared

• The more The more electronegative atom electronegative atom gains electronsgains electrons

Lewis Structures

• Lone pair – pair of electrons Lone pair – pair of electrons not involved in bonding (aka not involved in bonding (aka unshared pair)unshared pair)

• Bonds – can be single, Bonds – can be single, double, or even triple (share double, or even triple (share 1, 2, or 3 pairs of electrons)1, 2, or 3 pairs of electrons)

Preview of Lewis Structures

• We will be counting valence We will be counting valence electrons:electrons:

• For NHFor NH33 … …• Nitrogen= 5 valence electronsNitrogen= 5 valence electrons• Hydrogen= 1 valence electron Hydrogen= 1 valence electron

eacheach


• N: 1x 5e- = 5e-N: 1x 5e- = 5e-• H: 3x 1e- = 3e-H: 3x 1e- = 3e-

total e- = 8e-total e- = 8e-


• Organize the atoms so there Organize the atoms so there is a central atom (usually is a central atom (usually the least electronegative) the least electronegative) surrounded by the other surrounded by the other atomsatoms

• Hydrogen is never the Hydrogen is never the central atomcentral atom

The Steps We’ll Use

1) Count the total valence 1) Count the total valence electrons for the molecule:electrons for the molecule: To To do this, find the number of do this, find the number of valence electrons for each atom valence electrons for each atom in the molecule, and add them up.in the molecule, and add them up.


2) 2) Figure out how many octet Figure out how many octet electrons the molecule should electrons the molecule should have, using the octet rule:have, using the octet rule: The The octet rule tells us that all atoms octet rule tells us that all atoms want eight valence electrons want eight valence electrons (except for hydrogen, which (except for hydrogen, which wants only two), so they can be wants only two), so they can be like the nearest noble gas. like the nearest noble gas.

Step 2 (Continued)

• Use the octet rule to figure out Use the octet rule to figure out how many electrons each how many electrons each atom in the molecule should atom in the molecule should have, and add them up. have, and add them up. The The only weird element is boron - it only weird element is boron - it wants six electrons.wants six electrons.


3) Subtract the valence 3) Subtract the valence electrons from octet electrons:electrons from octet electrons: Or, in other words, subtract the Or, in other words, subtract the number you found in #1 above number you found in #1 above from the number you found in #2 from the number you found in #2 above. The answer you get will be above. The answer you get will be equal to the number of bonding equal to the number of bonding electrons in the molecule. electrons in the molecule.


4) Divide the number of 4) Divide the number of bonding electrons by two:bonding electrons by two: Remember, because every bond Remember, because every bond has two electrons, the number of has two electrons, the number of bonds in the molecule will be bonds in the molecule will be equal to the number of bonding equal to the number of bonding electrons divided by two. electrons divided by two.


5) Draw an arrangement 5) Draw an arrangement of the atoms for the of the atoms for the molecule that contains the molecule that contains the number of bonds you number of bonds you found in #4 abovefound in #4 above

Step 5 (Continued)Some handy rules to remember are these: Some handy rules to remember are these:

Hydrogen and the halogens bond once. Hydrogen and the halogens bond once. The family oxygen is in can bond twice. The family oxygen is in can bond twice. The family nitrogen is in can bond three The family nitrogen is in can bond three

times. So can boron. times. So can boron. The family carbon is in can bond four The family carbon is in can bond four

times. times.

Step 5 (Continued)

• A good thing to do is to A good thing to do is to bond all the atoms together bond all the atoms together by single bonds, and then by single bonds, and then add the multiple bonds until add the multiple bonds until the rules above are the rules above are followed.followed.


6) Arrange lone pairs around 6) Arrange lone pairs around the atoms until all of them the atoms until all of them satisfy the octet rule:satisfy the octet rule:

Remember, ALL elements EXCEPT Remember, ALL elements EXCEPT hydrogen want eight electrons around hydrogen want eight electrons around them, total. Hydrogen only wants two them, total. Hydrogen only wants two electrons electrons

Examples

•CHCH44

Examples

•COCO22

Try It Out

•SiSSiS22

Try it Out!

•NHNH3 3

Exceptions to the Octet RuleExceptions to the Octet Rule There are some atoms that are stable There are some atoms that are stable

without an octet.without an octet. Boron is stable with 6 electronsBoron is stable with 6 electrons Phosphorus and Sulfur can allow 10 or Phosphorus and Sulfur can allow 10 or

12 electrons sometimes.12 electrons sometimes. This method does This method does NOTNOT work for work for

elements that do not obey the octet rule. elements that do not obey the octet rule. If you want to know how to do those, ask If you want to know how to do those, ask

me!me!

For Charged Compounds…

• For negative charge, add For negative charge, add valence electrons. For valence electrons. For positive charge, subtract positive charge, subtract them.them.

• Write the charge outside of Write the charge outside of the structurethe structure

Example

•OHOH-1-1

Resonance Structures

• Compounds that are Compounds that are represented by more represented by more than one Lewis structurethan one Lewis structure

ExampleExampleNONO22

-1-1

STOP!STOP!Complete Worksheet Complete Worksheet #3– First two columns #3– First two columns ONLY.ONLY.

Wrap UpWrap UpPass the Paper

Today…Today… Get Out:Get Out:

Worksheet #3Worksheet #3 Our Plan:Our Plan:

Crash Course ReviewCrash Course Review Ionic & Covalent Bonding Group ActivityIonic & Covalent Bonding Group Activity Review Lewis StructuresReview Lewis Structures Worksheet #3Worksheet #3 Wrap Up – Exit TicketWrap Up – Exit Ticket

Homework (Write in Planner):Homework (Write in Planner): Make sure all Lewis structures are done on WS#3!Make sure all Lewis structures are done on WS#3!

The Octet Rule Song…The Octet Rule Song…

http://www.youtube.com/watch?v=WzWk-mx_14E&feature=related



Crash Course ReviewCrash Course Review

http://www.youtube.com/watch?v=a8LF7JEb0IA 4:30 – 9:304:30 – 9:30



Review Lewis StructuresReview Lewis Structures

Let’s try ONCl….Let’s try ONCl….

Wrap Up – Exit TicketWrap Up – Exit TicketDraw as many resonance

structures as you can for HN3. (HINT: the three nitrogen atoms are bonded in a row and the hydrogen atom is bonded to a nitrogen atom at the end of the row of nitrogen.)


Get out Notes & Periodic TableGet out Notes & Periodic Table Do one Lewis Structure from the labDo one Lewis Structure from the lab

Our Plan:Our Plan: Clicker Review Notes – VSEPRNotes – VSEPR Complete Worksheet #3 – DUE TODAYComplete Worksheet #3 – DUE TODAY Begin VSEPR LabBegin VSEPR Lab Clicker Review

Homework (Write in Planner):Homework (Write in Planner): Complete all Lewis Structures on Lab (optional)Complete all Lewis Structures on Lab (optional)

ReviewReview

Clicker Review

VSEPR• VValence alence SShell hell EElectron lectron PPair air

RRepulsionepulsion• The repulsion between electron The repulsion between electron

pairs causes molecular shapes to pairs causes molecular shapes to adjust so that the electrons are as adjust so that the electrons are as far away from each other as far away from each other as possible.possible.

• Shows “geometry” of moleculesShows “geometry” of molecules

HybridizationHybridizationWhen bonds form orbitals overlapWhen bonds form orbitals overlapVideo Explanation:Video Explanation:

http://www.mhhe.com/physsci/http://www.mhhe.com/physsci/chemistry/essentialchemistry/chemistry/essentialchemistry/flash/hybrv18.swfflash/hybrv18.swf

VSEPR Rules

1. Central atom determines where atoms bond

2. Consider unpaired electrons (repulsion)

• Lone pairs still occupy space, but do not determine the shape of the molecule

VSEPR Rules

3. All shared pairs are oriented as far away from each other as possible

4. Table in Note Packet

Linear • 2 atoms total2 atoms total

OR 3 atoms with OR 3 atoms with no lone pairs on no lone pairs on central atomcentral atom

Hybridization: spHybridization: sp Angle: 180Angle: 180ºº

Bent• 2 atoms around the central 2 atoms around the central

atom with lone pairs on the atom with lone pairs on the central atom occupying spacecentral atom occupying space

Hybridization: spHybridization: sp33/sp/sp22

Angle: 104.5Angle: 104.5ºº

Triangular Planar• 3 atoms around the central atom 3 atoms around the central atom

with no lone pairs around the with no lone pairs around the central atomcentral atom

Hybridization: spHybridization: sp22

Angle: 120Angle: 120ºº

Triangular Pyramidal•3 atoms around the central atom with a lone pair on the central atomHybridization: sp3

Angle: 107.5º

Tetrahedral•4 atoms around the central atom with no lone pairs on the central atom.Hybridization: sp3

Angle: 109.5º

Other ShapesOther Shapes

PolarityPolarity

The different electronegativies The different electronegativies of the atoms in a compound of the atoms in a compound determine whether the determine whether the molecule is polar or nonpolarmolecule is polar or nonpolar

Polarity only exists in Polarity only exists in molecular compoundsmolecular compounds

Nonpolar BondsNonpolar Bonds

• Exists when 2 electrons Exists when 2 electrons are shared equally by 2 are shared equally by 2 nonmetallic atomsnonmetallic atoms

Balanced distribution of Balanced distribution of electrical chargeelectrical charge

Nonpolar BondNonpolar Bond


Nonpolar BondsNonpolar Bonds• Electron Density of 2 Chlorine Electron Density of 2 Chlorine

AtomsAtoms

Polar Bonds

• Bonded atoms have an unequal attraction for the shared electrons

•Charge IS NOT distributed equally

Polar Bonds•Example = hydrogen and oxygen in WATER

• There is a moderate difference in electronegativity, so O pulls the electron of the H atom closer to itself

• Result is a polar covalent bond

Polar BondsPolar Bonds


Polar Bonds•WATER

PolarityPolarity• Whether a molecule is polar or Whether a molecule is polar or

not can be determined by it’s not can be determined by it’s shape.shape.

• If it is symmetrical (uniform all If it is symmetrical (uniform all around) it is nonpolar.around) it is nonpolar.

• If it is not symmetrical (un-If it is not symmetrical (un-uniform around) it is polar.uniform around) it is polar.

IMPORTANT NOTE!IMPORTANT NOTE!

If a compound has If a compound has charge, no matter it’s charge, no matter it’s shape, it is POLARshape, it is POLAR

Example• Use VSEPR to predict the Use VSEPR to predict the

shape, polarity, & hybridization shape, polarity, & hybridization of these molecules:of these molecules:• BClBCl33• SiClSiCl33BrBr

BClBCl33

BCl

Cl

Cl

Triangular Planar

sp2

nonpolar

SiClSiCl33BrBr

Si Cl

Cl

ClBr

Tetrahedralsp3

polar

PIPI33

PI

I

I

Triangular Pyramidal

sp3

polar

CClCCl44

C Cl

Cl

ClCl

Tetrahedralsp3

nonpolar

Stop!Stop!Complete Worksheet #3! Complete Worksheet #3! It is due in 10 minutes. It is due in 10 minutes.

Lab TimeLab Time Start the VSEPR Lab…Start the VSEPR Lab…

Lab KEYLab KEY

Black = C, N, SBlack = C, N, S Blue = PBlue = P Red = ORed = O Yellow = HYellow = H Green/Purple/Orange = Cl, FGreen/Purple/Orange = Cl, F Stick = Single BondStick = Single Bond 2 Springs = Double Bond2 Springs = Double Bond 3 Springs = Triple Bond3 Springs = Triple Bond

Wrap UpWrap Up

Clicker ReviewClicker Review


Get out lab & notebookletGet out lab & notebooklet Our Plan:Our Plan:

Song to ReviewSong to Review Find Someone WhoFind Someone Who VSEPR Lab – Due TODAYVSEPR Lab – Due TODAY Vocab Slap JackVocab Slap Jack

Homework (Write in Planner):Homework (Write in Planner): VSEPR LabVSEPR Lab

Another sweet chemistry Another sweet chemistry song…song…

http://www.youtube.com/watch?http://www.youtube.com/watch?v=wWUYHHo-zB0v=wWUYHHo-zB0

Crash Course ReviewCrash Course Review

http://www.youtube.com/watch?http://www.youtube.com/watch?v=QXT4OVM4vXIv=QXT4OVM4vXI Skip Coulomb’s LawSkip Coulomb’s Law

VSEPR LabVSEPR Lab

Must have signatures for all Must have signatures for all compounds and then turn into compounds and then turn into basket. basket. DUE TODAY!DUE TODAY!

Today…Today… Turn in:Turn in: Fill out U5 Goal SheetFill out U5 Goal Sheet

Our Plan:Our Plan: Roundtable Review with CardsRoundtable Review with Cards Work DayWork Day

• VSEPR Lab – VSEPR Lab – DUE TODAYDUE TODAY• Missing Assignments – WorksheetsMissing Assignments – Worksheets• Test ReviewTest Review

Wrap Up - MemoryWrap Up - Memory Homework (Write in Planner):Homework (Write in Planner):

Test Review due Next ClassTest Review due Next Class TEST NEXT CLASSTEST NEXT CLASS

Dogs Teaching ChemistryDogs Teaching Chemistry

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Today…Today… Turn in:Turn in: Get Out Test Review to check – mark questions Get Out Test Review to check – mark questions

that you havethat you have Our Plan:Our Plan:

Bonding WS RaceBonding WS Race Go over Test Review Questions – turn inGo over Test Review Questions – turn in TestTest Complete the first section of Unit 1 Notes with the Complete the first section of Unit 1 Notes with the

printed slides and use a PT to complete WS#1printed slides and use a PT to complete WS#1 Homework (Write in Planner):Homework (Write in Planner):

WS#1 due next classWS#1 due next class

After the Test…After the Test…

Take from the side table:Take from the side table: Slides HandoutSlides Handout NotesNotes Worksheet PacketWorksheet Packet

Take the notes in your booklet and return Take the notes in your booklet and return them to the side table. Then use your them to the side table. Then use your Periodic Table and textbook to complete Periodic Table and textbook to complete Worksheet #1. It is due on MONDAY!Worksheet #1. It is due on MONDAY!

LinearBentTriangular PyramidalTriangular PlanarTetrahedral

LinearBentTriangular PyramidalTriangular PlanarTetrahedral

Number 4Number 4

ElectronsElectrons

Number 7Number 7

NN

XeXe

MgMg

SiSi

Number 8Number 8

CC

BrBr

NHNH44++11

OCNOCN-1-1

CFCF22HH22

FF22OO

CHCH22OO

NHNH33

CICI44

Show the ionic bonding Show the ionic bonding between magnesium and 2 between magnesium and 2

chlorines then write the formula chlorines then write the formula and ions.and ions.

Lab KEYLab KEY

Black = C, N, SBlack = C, N, S Blue = PBlue = P Red = ORed = O Yellow = HYellow = H Green/Green/Purple/Purple/OrangeOrange = Cl, F = Cl, F Stick = Single BondStick = Single Bond 2 Springs = Double Bond2 Springs = Double Bond 3 Springs = Triple Bond3 Springs = Triple Bond

LinearBent

TetrahedralTriangular Planar

Triangular Pyramidal

chemical bonding unit 5

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