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Name: _________________________________________________ Date: __________________ Period: _____

Chemistry “I can accept failure, everyone fails at something. But I can’t

accept not trying.” – Michael Jordan

Packet#7 Unit#6: Covalent Bondingand Covalent Compounds

Edmodo Group Code: ozm60q (http://www.edmodo.com)Class Website: http://mrgchem.weebly.com

Mr. Gutierrez’s email: [email protected] Messaging Reminders: Text @aofchem to 23559

Note: You are expected to work on this packet during the allotted class practice time.

Packet Points/35 Completed Class

Notes/35 Completed

Classwork/5 Writing Name on

Every Page/25 Handed Packet in on

Time/ Homework

/ Followed Classroom Policies

/ Classwork Participation

/ TOTAL POINTS

Name of Chemist:__________________________________________________________________

Period: ___________

DUE _________________________“I can accept failure, everyone fails at something. But I can’t accept not trying.” – Michael Jordan

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Name: _________________________________________________ Date: __________________ Period: _____

*All Class Notes + Questions MUST be finished for HOMEWORK if not done in class.

Unit#7: Covalent Bonds

Table of Contents

Topic Pages Textbook Pages Supplementary Materials

(Video or Notes)Covalent Bonding 4 – 5 179 - 183

Electronegativity and Types of

Bonding

6 - 9 175 - 177

Lewis Dot Structures of

Covalent Compounds

10 - 16 184 - 189

Naming Covalent Compounds

17 - 21 228 – 229

Writing Chemical Formulas from

Covalent Compounds

22 - 25 228 – 229

“I can accept failure, everyone fails at something. But I can’t accept not trying.” – Michael Jordan

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Name: _________________________________________________ Date: __________________ Period: _____

ANNOUNCEMENTS• When emailing work to me, it is YOUR RESPONSIBILITY to make sure that it was sent.

You MUST write In the SUBJECT FIELD:• TITLE OF THE ASSIGNMENT p3 if you’re in period 3 p4 if you’re in period 4 p6 if you’re in period 6

Points will be deducted if you don’t.

Additional Resources:*Tutoring with Mr. Gutierrez: Meet Mr. Gutierrez in student cafeteria after school or during 9th or 10th period.


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Name: _________________________________________________ Date: __________________ Period: _____Date: _________________Objectives: 1) SWBAT explain why covalent bonds form. 2) SWBAT list the properties of covalent bonds.

Class NotesCovalent Bonds

Review:Octet Rule Atoms gain, lose, or _______________ electrons in order to have

_________ valence electrons.

Covalent Bonds Atoms of different elements ________________ _______________ to

form a ____________ _____________. They share electrons in order to have _________ valence electrons.

Atoms _________ electrons by _______________________ their orbitals.

Types of Covalent Bonds

1. In single bonds, atoms share _____ electrons

2. In double bonds, atoms share _____ electrons

3. In triple bonds, atoms share ______ electrons

All single bonds have ____________ bonds.

Double bonds have _____ sigma bond and _____ pi bond.

Triple bonds have _____ sigma bond and _____ pi bonds.

σ

πProperties of


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Name: _________________________________________________ Date: __________________ Period: _____Covalent Compounds

______________________________ ______________________________ ______________________________

Real world connection – Why should I care?

Summary

In your own words, summarize today’s main points.

Date: _________________


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Name: _________________________________________________ Date: __________________ Period: _____Objectives: 1) SWBAT define electronegativity. 2) SWBAT use electronegativity values to predict the type of bonding between different elements.

Class NotesElectronegativity

Electronegativity ________________________ is an atom’s ability to ________________

____________________.

Ionic, Polar-covalent, or Nonpolar-covalent

In most cases, you can predict whether a compound is ionic or covalent by checking if the compound has a metal. However, the differences in _____________________ will tell you more about the nature of that chemical bond.

Non-polar covalent bond: covalent bond in which the bonding electrons are ________________ ________________ by the bonded atoms, resulting in a _______________distribution of electrical charge. (0 to 0.3 electronegativity difference and 0% to 5% ionic character.)

Polar-covalent bond: covalent bond in which bonded atoms have an unequal attraction for the shared electrons. (0.3 to 1.7 electronegativity difference and 5% to 50% ionic character.)

Ionic bonding: one atom __________ electrons while another ____________ electrons, forming cations and anions. The atoms are bonded together through an _______________attraction. (1.7 to 3.3 electronegativity difference and 50% to 100% ionic character.)


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Name: _________________________________________________ Date: __________________ Period: _____

How to determine if compound is ionic, polar-covalent, nonpolar-covalent:

Example#1: HCl

H - Hydrogen has electronegativity value of ___________ Cl - Chlorine has electronegativity value of ____________

Electronegativity difference = _____________________

0.9 is between 0.3 and 0.7 so it is ___________________

Example#2: LiF


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Name: _________________________________________________ Date: __________________ Period: _____

Date: _________________Objectives: 1) SWBAT define electronegativity. 2) SWBAT use electronegativity values to predict the type of bonding between different elements.

Class WORKClass Work (Independent Practice) Directions: Finish as many questions as you can during class. Refer to your notes and ask at least three classmates before asking me for help. If you do not finish these questions in class, you must finish them for homework.

Using the electronegativity chart on the back of this packet to determine whether the following compounds are ionic, polar-covalent, or non-polar covalent. Include the difference in electronegativity values.

1. NaCl

2. ZrBr2

3. Potassium chloride

4. Lithium Oxide

5. Scandium oxide

6. CoCl2


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Name: _________________________________________________ Date: __________________ Period: _____

7. AlP

8. Silver Iodide

9. Zinc chloride

10. HCl

11. KI

12. CsBr

13. Magnesium oxide

14. Magnesium nitride

15. SrS

16. A compound has a percentage ionic character of 76%. Is

this compound ionic, polar-covalent, or nonpolar-covalent?


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Name: _________________________________________________ Date: __________________ Period: _____

Date: _________________Objectives: 1) SWBAT draw the Lewis dot structures of covalent compounds.

Class NotesLewis Dot Structures of Covalent Compounds

Review:Covalent Bonds

Atoms of different elements ________________ _______________ to form a ____________ _____________. They share electrons in order to have _________ valence electrons.

Atoms _________ electrons by _______________________ their orbitals.

Most covalent compounds are made of nonmetals only.

Lewis Dot Structures

Lewis Dot Structures is a type of electron configuration notation in which only ______________ electrons are shown.

Example:


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Name: _________________________________________________ Date: __________________ Period: _____

How to Draw Lewis Dot Structures of Covalent Compounds

Example#1:

CH3I

STEP EXAMPLE1. Draw the Lewis dot structure for

each atom.

2. Count the number of valence electrons.

3. Draw the skeletal structure of the molecule with least electronegative element in the center. (except Hydrogen, it is NEVER the central atom!)

4. Add covalent bonds between center atom and outer atoms.

5. Add lone pairs to outer atoms so that it each atom has 8 valence electrons.

6. Add lone pairs to the center atom.

7. Count the total number of valence electrons and make sure it matches up with step #2.

8. Check if all atoms have at least 8 valence electrons (or 2 valence


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Name: _________________________________________________ Date: __________________ Period: _____electrons for Hydrogen)

Drawing Lewis Dot Structures of Covalent Compounds

Example#2:

PI3

Example#3:

CO2

Summary

In your own words, summarize today’s main points.


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Name: _________________________________________________ Date: __________________ Period: _____

Date: _________________Objectives: 1) SWBAT draw the Lewis dot structures of covalent compounds.

LEWIS DOT STRUCTURES OF COVALENT COMPOUNDS


Directions: Draw the Lewis dot structures for each of the following compounds. Show all your work.

1. PCl3

Once you are finished, have Mr. Gutierrez check your work before continuing to the next question.

2. HF


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Name: _________________________________________________ Date: __________________ Period: _____

3. PBr3

4. CO2

5. F2


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Name: _________________________________________________ Date: __________________ Period: _____

6. HCN

7. N2

8. CH2O


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Name: _________________________________________________ Date: __________________ Period: _____

9. SiCl4

10. F2O

11. NBr3


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Name: _________________________________________________ Date: __________________ Period: _____

Date: _________________Objectives: 1) SWBAT write the names of covalent compounds using numerical prefixes given its chemical formula.

Class NotesNaming Covalent Bonds

Covalent Bonds Covalent compounds are made of

__________________________.

Naming Naming Covalent Compounds

A prefix is ______________________________________________.

WARNING!!! WARNING!!! WARNING!!!PREFIXES ARE ONLY USED FOR COVALENT COMPOUNDS (compounds without metals)!

No prefixes for ionic compounds.


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Name: _________________________________________________ Date: __________________ Period: _____

Writing the Name of a Covalent Compound from its Chemical Formula:

Example#1:

P4O10

STEP EXAMPLE1. Look at the first number at the bottom and look up its prefix using the numerical prefix chart. (See prefix chart above.)

2. Write the prefix followed by the name of the first element. (Note: If there is no subscript for the first element, the prefix “mono-“ is NOT written.)

3. Look at the second number at the bottom and look up its prefix using the numerical prefix chart.

4. Write the prefix followed by the root of the second element name with the –ide at the end. If prefix ends with the letter ‘a’ or ‘o’, drop that letter.


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Name: _________________________________________________ Date: __________________ Period: _____FINAL ANSWER

Sample#2:

CO

Sample#3:

P2O5

Sample#4:

PBr5


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Name: _________________________________________________ Date: __________________ Period: _____


Date: _________________Objectives: 1) SWBAT write the names of covalent compounds using numerical prefixes given its chemical formula.


Directions: Write the name of the following covalent compounds given its chemical formula.

1. N2O

2. As2O5

3. P4S5

4. Si2Br6

5. SCl4


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Name: _________________________________________________ Date: __________________ Period: _____ 6. B2Si

7. NF3

8. CCl4

9. N2O4

10. C2Cl8

11. ICl3

12. PBr3

13. SiCI4

14. PCl3

15. N2O3

16. Si2N4


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Name: _________________________________________________ Date: __________________ Period: _____

17. P2O3

Date: _________________Objectives: 1) SWBAT write the chemical formulas of covalent compounds given its name.

Class Notes Covalent Bonds

From name to formula

Writing the Chemical Formula of Covalent Compound Given its Name

Example#1:

dinitrogen pentoxide

STEP EXAMPLEExample:

1. Look up what the first prefix means in terms of numbers.


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Name: _________________________________________________ Date: __________________ Period: _____

2. Write the number at the bottom of the symbol of the first element written.3. Look up what the second prefix means in terms of numbers.

4. Write the number at the bottom of the symbol of the second element.

FINAL ANSWER

Sample#2:

Carbon monoxide

Sample#3:

Diphosphorus pentoxide

Sample#4:


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Name: _________________________________________________ Date: __________________ Period: _____Nitrogen trifluoride


Date: _________________Objectives: 1) SWBAT write the chemical formulas of covalent compounds given its name.


Directions: Write the chemical formula of the following covalent compounds given its name.

1. dinitrogen trioxide

2. sulfur hexafluoride

3. carbon tetrachloride

4. phosphorus pentafluoride

5. silicon tetraflouride

6. sulfur hexoxide


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Name: _________________________________________________ Date: __________________ Period: _____

7. nitrogen trichloride

8. boron tribromide

9. sulfur hexafluoride

10.sulfur trioxide

11. arsenic pentaflouride

12. diphosphorus tetroxide

13. chlorine dioxide

14. phosphorus triiodide

15. chlorine dioxide

16. iodine trichloride

17. phosphorus pentabromide


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Name: _________________________________________________ Date: __________________ Period: _____18. Arsenic trioxide

Make sure Mr. Gutierrez stamps/signs this by the end of the period. You CANNOT get the stamp/signature for a day later on. It is your responsibility to remind Mr. Gutierrez. You will NOT receive a stamp if you did not follow all classroom policies or actively work on the practice problems during the allotted class time. A stamp means you received all 10 points. No stamps means you’ve received zero points. If you completed some work, I may give you partial credit based on my discretion. If you are absent, write the date on the day you were absent and write the word “Absent.” DO NOT LOSE THIS SHEET!!! (If you lose this sheet, you will lose all of your participation points. NO EXCEPTIONS.)

Day of Week Followed All Classroom Policies (Respectful, on time, prepared, engaged…)

Class work Participation Homework

Monday /10 /10 /10

Tuesday /10 /10 /10

Wednesday /10 /10 /10

Thursday /10 /10 /10


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Name: _________________________________________________ Date: __________________ Period: _____

Friday /10 /10 /10


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Name: _________________________________________________ Date: __________________ Period: _____

Classroom Policy Violation Codes

P = PhoneC = CursingT = TalkingL = Late to classO.T. = Off TaskH.D. = Head DownN.iP = Did not bring iPadUnp = Unprepared (no pencil, no iPad, no emergency passes, no periodic table, etc.)

Teacher Comments:


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