Covalent Bonding Notes--Resonance and VSEPR Day 3 …

Covalent Bonding Notes--Resonance and VSEPR Day 3 COMPLETE.notebookCovalent Bonding NotesResonance and VSEPR Day 3 COMPLETE.notebookFebruary 20, 2020
Answer the following (I'll call on people to answer / write their answer):
1. Draw the Lewis structure for NBr3.
2. What is wrong with this Lewis structure for HCl?
3. How many shared electron pairs are in the molecule?
4. How many lone electron pairs are in the molecule?
5. What is name of CuSO4?
1. Draw the Lewis structure for NBr3.
2. What is wrong with this Lewis structure for HCl?
3. How many shared electron pairs are in the molecule?
4. How many lone electron pairs are in the molecule?
5. What is name of CuSO4?
HBr Draw the Lewis structure.
How many lone electron pairs are present?
K2S Molecule or Formula unit?
Draw the Lewis dot or Lewis structure for this compound.
Reminders Quarter 2 Recovery due TOMORROW (2/21)
ACT Tuesday (2/25)
SAT March 4th
Course Verification forms due MONDAY (2/24) let me know if you want me to change your recommendation
Activity Period Tomorrow (2/21) Black History Program $1 in the cafeteria during ILT
Quia 8.1 due Tuesday night (2/25) @ 11:59 pm: https://www.quia.com/quiz/7540043.html
1. Draw Lewis structures to represent molecules and polyatomic ions (including resonance).
2. Build molecular models to predict their shape (molecular geometry).
• H.C.3A.1: Construct explanations for the formation of molecular compounds via sharing of electrons and for the formation of ionic compounds via transfer of electrons.
• H.C.3A.2: Use the periodic table to write and interpret formulas and names of chemical compounds— binary ionic compounds, binary covalent compounds, and straightchain alkanes up to six carbons).
• H.C.3A.3: Analyze and interpret data to predict the type of bonding (ionic or covalent) and the shape of simple compounds using the Lewis dot structures and oxidation numbers.
• IV.4.a: Use Lewis dot diagrams to represent bonding in ionic and covalent compounds • IV.4.b: Draw Lewis structures for molecules and polyatomic ions, including those that must be
represented by a set of resonance structures.
Objectives and Indicators Part 2 Notes: Covalent Bonding, Lewis Structures, & Resonance
Unit 8: Bonding CP Chemistry 20192020
Covalent Bonding NotesResonance and VSEPR Day 3 COMPLETE.notebookFebruary 20, 2020
Diatomic Molecules
Molecule: a group of covalently bonded atoms (nonmetals)
Formula unit: simplest unit of an ionic compound (metal + nonmetal)
Ion: a charged particle
Polyatomic ion: a group of covalently bonded atoms that has an overall charge.
Drawing Lewis Structures for Polyatomic Ions
1. Chlorate [ClO3] 1
• Account for the charge on the ion
• Divide the total # of valence electrons by 2. This is how many pairs needed.
• Draw the Lewis structure.
Drawing Lewis Structures for Polyatomic Ions
Carbonate [CO3] 2
Carbonate [CO3] 2
Find the Lewis Structure for Carbonate CO3 2 that you drew.
Does it matter where the double bond is drawn?
Resonance Sometime, there are molecules and ions whose structure is not adequately described by one Lewis structure. Consider ozone:
We expect the = bond to be shorter than the bond Where should the double bond go?
Equivalent Lewis structures are called resonant structures The real molecule is a hybrid of the two resonance structures
Resonance
Analogy: Green paint is made of both blue and yellow paint green paint doesn't oscillate between blue and yellow it is an equal blend of the two colors.
The electrons are not "locked" into place. The arrangement of electrons is a blend of each resonant structure
Resonance
Resonance is a term used to describe Lewis structures that have a double or triple bond that is not "locked" into place.
The electrons in those double and triple bonds are delocalized. That means than can move throughout the molecule.
The double bonds in this molecule of benzene are NOT locked in place. The electrons in the double bonds are delocalized. Where else could the double bonds be drawn?
These are the RESONANCE STRUCTURES for CO3 2.
The MOST accurate diagram is the bottom one that shows the delocalized electrons.
The double bond is NOT "locked" into 1 location in the molecule
Draw ALL possible resonance structures for the nitrate ion (NO3
1).
Draw ALL possible resonance structures for the nitrate ion (NO3
1).
Draw the MOST accurate resonance structure of this ion.
VSEPR Theory and Molecular Geometry 1. Draw the orbital notation that the ion of nitrogen would form in
ionic bonding.
2. Draw the Lewis dot structure for BCl3 and indicate the molecular geometry (shape).
3. Draw the Lewis dot structure for NH3 and indicate the molecular geometry (shape).
Practice with Lewis Structures and Resonance
Whiteboards
Review Question #1 Compare OCl2 and CO2.
Draw the Lewis structure for both to support your answer.
Review Question #2 Compare CO3
2 and CO2.
Review Question #3 What do these chemical species have in common?
SO4 2, PO4
3, CHCl3, NH4 +
Review Question #4 Compare the electron configurations of the ions of calcium and phosphorus.
Write the standard and orbital notations of each.
Review Question #5 M is an unknown metal that forms the following compounds:
MOH and M2CO3
1. How many valence electrons does metal M have?
2. Draw the Lewis dot diagram to show how metal M and oxygen would form ionic bonds.
Write the formula for silver nitride.
Write the formula for aluminum sulfate.
Write the orbital notation for the ANION in #1.
Write the noble gas configuration for the CATION in #2.
Answer the following questions for H2S.
a. Draw the Lewis structure.
b. What is the molecular geometry?
c. What are the bond angle measurements?
d. What is the number of shared pairs?
e. What is the number of lone pairs?
f. How many electrons are involved in bonding?
Opening Directions
• You have an ionic compound naming quiz today. • Study for that before the bell rings.
• Ag2CO3 silver carbonate
• Pb(NO3)2 lead(II) nitrate
• CuCl copper(I) chloride
• K2S potassium sulfide
• NiPO4 nickel(III) phosphate
1. Ag2SO4
2. Ni2(CO3)3
3. NaBr
4. CuNO3
5. K3PO4
2. Build molecular models to predict their shape (molecular geometry).
• H.C.3A.2: Use the periodic table to write and interpret formulas and names of chemical compounds— binary ionic compounds, binary covalent compounds, and straightchain alkanes up to six carbons).
• IV.4.a: Use Lewis dot diagrams to represent bonding in ionic and covalent compounds • IV.4.b: Draw Lewis structures for molecules and polyatomic ions, including those that must be
represented by a set of resonance structures.
Objectives and Indicators
Linear Trigonal planar
Bent Trigonal pyramidal
2. Use VSEPR theory to predict their shape (geometry).
• H.C.3A.2: Use the periodic table to write and interpret formulas and names of chemical compounds—binary ionic compounds, binary covalent compounds, and straightchain alkanes up to six carbons).
• IV.4.a: Use Lewis dot diagrams to represent bonding in ionic and covalent compounds • IV.4.b: Draw Lewis structures for molecules and polyatomic ions, including those that must be represented by a set of
resonance structures.
Opening Question 2/25/2019 What is the name of this chemical species?
What is being illustrated? What does that mean?
Example
How many lone electron pairs are present?
K2S Molecule or Formula unit?
Draw the Lewis dot or Lewis structure for this compound.
Reminders and Opening Directions: Wednesday, January 18th
• Quia Quiz #3: due Thursday 1/19 at 11:59 p.m. • Naming Quiz tomorrow: ionic compounds • Test Unit 8 Bonding: Friday • Quiz TODAY: Bonding Review
• Opening Question • Compare NF3 and BF3. Draw Lewis structures as part of your answer.
1. Evaluate your understanding of chemical bonding using review questions.
2. Draw Lewis structures of molecules and polyatomic ions.
H.C.3: The student will demonstrate an understanding of the structures and classification of chemical compounds. • H.C.3A.1: Construct explanations for the formation of molecular compounds via sharing of electrons and for the formation of ionic compounds via transfer of electrons.
• H.C.3A.2: Use the periodic table to write and interpret formulas and names of chemical compounds—binary ionic compounds, binary covalent compounds, and straightchain alkanes up to six carbons).
Review Question #1 Compare OCl2 and CO2.
Review Question #2 Compare CO3
2 and CO2.
Review Question #3 What do these chemical species have in common?
SO4 2, PO4
3, CHCl3, NH4 +
Review Question #4 Compare the electron configurations of the ions of calcium and phosphorus.
Write the standard and orbital notations of each.
Review Question #5 M is an unknown metal that forms the following compounds:
MOH and M2CO3
1. How many valence electrons does metal M have?
2. Draw the Lewis dot diagram to show how metal M and oxygen would form ionic bonds.
Quiz Time
Draw the dang Lewis structure! Don't guess. . . draw it out!
Closing Questions
PopQuiz
b. How many lone pairs of electrons are there?
c. How many shared pairs of electrons are there?
d. What is the VSEPR shape (molecular geometry)?
Closing Questions
1. Draw the Lewis structure for phosphorus trichloride. How many lone electron pairs are present? How many shared electron pairs are present? What is the molecular geometry? Bond angles?
2. Draw the Lewis structure(s) for NO2 1. If resonance exists, show the
best structure. What is the molecular geometry? Bond angles?
Opening Questions: Friday, January 23rd
1. Draw the orbital notation that the ion of nitrogen would form in ionic bonding.
2. Draw the Lewis dot structure for BCl3 and indicate the molecular geometry (shape).
3. Draw the Lewis dot structure for NH3 and indicate the molecular geometry (shape).
Pop Quiz: 12/9/15
Write the orbital notation for the ANION in #1.
Write the noble gas configuration for the CATION in #2.
Answer the following questions for H2S.
b. What is the molecular geometry?
c. What are the bond angle measurements?
d. What is the number of shared pairs?
e. What is the number of lone pairs?
f. How many electrons are involved in bonding?
Draw Lewis structures for molecules and polyatomic ions. Predict the geometry of molecules and polyatomic ions. Predict bond angles using Lewis structures and geometry.
IV. Building Models of Matter 3. Intermolecular Forces and Types of Bonds • e. Describe the unique features of bonding in carbon compounds
4. Orbital Theory Applied to Bonding • b. Draw Lewis structures for molecules and polyatomic ions, including those that must be represented by a set of resonance structures. • c. Use VSEPR theory to explain geometries of molecules and polyatomic ions • d. Describe how orbital hybridization models relate to molecular geometry • e. Describe the molecular orbital models for double bonds, triple bonds, and delocalized pi electrons
Practice with Lewis Structures and Resonance
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Covalent Bonding Notes--Resonance and VSEPR Day 3 …