CHM 2046C Module-4ii Homework Packet Name: ____________________

Please complete the following homework packet before you actually attempt the pretest before or after class each day. This is homework, not the pretest. You attempt it before you take the exam. You grade it. This completed packet is due the day of the exam.

B._____ (05) Lewis Dot/Stick Structure via Octet Rule Steric#s 2-3-4 Sect 8.3/8.7Answer

E._____ (01) Polyatomic Ions Table 2.4 Page 85

L. ____ (01) Bond Angles/Bond Lengths Steric#s 2-3-4 Section 9.2 Answers

N. ____ (01) Geometry of Molecules- Steric#s 2-3-4 Section 9.1-9.2 Answers

O. ____ (01) Polarity of Molecules- Steri #s 2-3-4 Section 8.6, 9.3 Answers

P. ____ (01) Hybrid Orbital Recognition Steric#s 2-3-4-Sect 9.5-6 Answers

______(10) Total

Module Four II: Part B Dot Structures of Molecules Review 05 points

Choose Two from each question. Use the simple octet rule (but you may use formal charge method for a more accurate drawing-Required in M4iii B1). Using a periodic chart/octetrule draw the electron dot/stick structures of the following molecules:

1. NH₃ CH₄ H₂O₂ H₂O HCl H₂ O₂ N₂

2. H₂SO₄ H₂SO₃ H₃PO₄ H₃PO₃ HClO₄ HClO₃ HClO₂ HClO

3. HNO₃ H₂CO₃ HNO₂

4. CO₂ HCN SiO₂ SO₃

5. HC₂H₃O₂ H₂C₂O₄ HCHO₂

carbon to carbon by single covalent bond

6. C₂H₄ C₂H₂ C₃H₈ C₂H₆

bond carbons to carbon

7. CH₂O CH₃COCH₃

carbon to carbons by single covalent bonds above

8. CH₃OCH₃ CHONH₂

oxygen separates O & N both

the carbons bond to C

9. CH₂NH₂COOH CH₃CHNH₂COOH

carbon to carbons by single covalent bonds -NH₂ hooks to #2 carbon in both above

10. CH₃COOCH₂CH₃ CHOOCH₃

carbon to carbons by single covalent bonds (-CH₃ also hooks to an oxygen above)

(-CH₂CH₃ also hooks to an oxygen above)

Reading Reference: Sections 8.5 Octet Rule and 8.7 Formal Charge (page 374)

Reference: B. Dot Structures of Covalent Compounds Section 2.10, 6.6, 7.1, 7.5, 7.6

Answers: http://www.fccj.us/chm2045/SampleTest/45M4bAnswers.htm
Required List of Polyatomic Ions 0 Points

1

IA

IIA

H

IIIa

IVA

VA

VIA

VIIA

He

2

B

C*

N

Ne

3

Si

P

S

Cl

Ar

4

V

Cr

Mn

Fe

As

Se

Br

Kr

5

Mo

Sn

Sb

Te

I

Xe

6

W

Pb

Rn

7

Acetate ___________ Ammonium ___________ Antimonate ___________ Antimonite ___________ Arsenate ___________ Arsenite ___________ Azide ___________ Bicarbonate ___________ Borate ___________ Bromate ___________ Bromite ___________ Carbide __________ Carbonate __________ Carbonite __________ Chlorate __________ Chlorite __________ Chromate __________ Cyanate _________ Cyanide _________ Dichromate __________ Dihydrogen Arsenate __________ Dinhydrogen Phophate __________ Dihydrogen Phosphite __________ Ferrate ___________ Hydrogen carbonate ___________ Hydrogen arsenate ___________ Hydrogen phosphate ___________ Hydrogen phosphite __________ Hydrogen sulfate __________ Hydrogen sulfite __________ Hydronium __________ Hydroxide ___________

Hypobromite __________ Hypochlorite __________ Hypoiodite __________ Hypophosphite __________ Hyposulfite ___________ Periodate __________ Iodate __________ Iodite __________ Mercury (I) __________ Manganate __________ Molybdate _________ Nitrate __________ Nitrite __________ Oxalate __________ Perbromate __________ Perchlorate __________ Permanganate __________ Phosphate __________ Phosphite __________ Plumbate __________ Plumbite __________ Selenate ___________ Selenite ___________ Silicate ___________ Stannate ___________ Stannite ___________ Sulfate ___________ Sulfite ___________ Tellurate ___________ Thiocyanate ___________ Tungstate ___________ Vanadate ___________

Reference Online Homework: Polyatomic Ions-Section 2.12 Answers e

http://www.northcampus.net/Nomenclature/PolyatomicIonFormula/ProgressivePolyatomicIonFormula.html

Required List of Polyatomic Ions

1

IA

IIA

H

IIIa

IVA

VA

VIA

VIIA

He

2

B

C*

N

Ne

3

Si

P

S

Cl

Ar

4

V

Cr

Mn

Fe

As

Se

Br

Kr

5

Mo

Sn

Sb

Te

I

Xe

6

W

Pb

Rn

7

The following Polyatomic Ions should be in you chemistry vocabulary:

Acetate CH3COO^− or C2H3O2^− Ammonium NH4^+ Antimonate SbO4^3− Antimonite SbO3^3− Arsenate AsO4^3− Arsenite AsO3^3− Bicarbonate HCO3^− Borate BO3^3− Bromate BrO3^− Bromite BrO2^− Carbide C2^2− Carbonate CO3^2− Carbonite CO2^2− Chlorate ClO3^− Chlorite ClO2^− Chromate CrO4^2− Cyanate OCN^− Cyanide CN^− Dichromate Cr2O7^2−

Dihydrogen Arsenate H2AsO4^− Dinhydrogen Phophate H2PO4^− Dihydrogen Phosphite H2PO3 Hydrogen carbonate HCO3^− Hydrogen arsenate HAsO4^2− Hydrogen phosphate HPO4^2− Hydrogen phosphite HPO3^2− Hydrogen sulfate HSO4^− Hydrogen sulfite HSO3^− Hydronium H3O^+ Hydroxide OH^− Hypobromite BrO^− Hypochlorite ClO^− Hypoiodite IO^− Hypophosphite PO2^3− Hyposulfite SO2^2−

Iodate IO3^− Iodite IO2^− Manganate MnO4^2- Mercury (I) Hg2^2+ Nitrate NO3^− Nitrite NO2^− Perbromate BrO4^− Perchlorate ClO4^− Periodate IO4^− Permanganate MnO4^− Phosphate PO4^3− Phosphite PO3^3− Plumbate PbO3^2− Selenate SeO4^2− Selenite SeO3^2− Silicate SiO3^2− Stanate SnO3^2− Sulfate SO4^2− Sulfite SO3^2− Tungstate WO4^2−

Bonus 1 point Each: Using a current CRC Handbook of Chemistry/Physics find a polyatomic ion list in an inorganic compound that is not on the list below:

The Complete Polyatomic Ions List http://www.fccj.us/PolyatomicIons/CompletePolyatomicIonList.htm

Taylor’s ¾ Rule: http://www.fccj.us/PolyatomicIons/Taylor34OxygenRuleHandout.htm

Taylor’s Charge Rule: http://www.fccj.us/PolyatomicIons/TaylorChargeRuleHandout.htm

National Publication 2YC3 Newsletter (2014 vol iii)

http://www.2yc3.org/Newsletters/2014/2014iii.pdf

Jespersen’s Common Polyatomic Ions

CHM 2046C Progressive Polyatomic Ions Jespersen 1 Point

Name:_____________________

Write the formula and the charge for the following polyatomic ions: Jespersen(Table 2.4 page 85)

Name	Formula with charge	Name	Formula with charge
Ammonium		Sulfite
Mercury(I)		Hydrogen Sulfite
Hydronium		Sulfate
Cyanide		Hydrogen Sulfate
Nitrite		Thiocyanate
Nitrate		Thiosulfate
Hypochlorite		Chromate
Chlorite		Dichromate
Chlorate		Phosphate
Perchlorate		Monohydrogen Phosphate
Permanganate		Dihydrogen Phosphate
Acetate		Hydrogen Carbonate
Oxalate		Carbonate

Module Four II: Part L Bond Angles 1 point

What is the bond Angle in the following structures:

___1. ___4.

___2. ___5.

___3. ___6.

___7. ___8. ____9.

___10. ____11.

___12. ___13. ___16.

___14.

___15.

___17. ___20.

____18. _____19.

Bonus:

___21. ___23.

___22. ___24.

Steric Numbers do not predict bond angles within rings of carbons

Reading Reference: Jespersen 7^th Section 9.2;

Work End of Chapter Problems #9.83-9.84 page 461

Module Four II - Part N: Geometry of Molecules 1 point

Use the dot/stick structures on the Part L page to state the geometry of the molecules:

Steric # = 2, 3,or 4:

Bent Linear Trigonal Planer Planer Trigonal Pyramidal Tetrahedral

Steric # = 5 or 6

Trigonal-bipyramidal Square Planer Seesaw T-shaped Octahedral

_____________1. H2O _____________2. CO2 _____________3. C2H4 _____________4. SO2 _____________5. SO3 _____________6. HCN _____________7. CH4 _____________8. NH3 _____________9. CH2O _____________10. C2H2 ______________ 11. PF5 _____________ 12. SF6

.

Reading Reference: Jespersen 7^th Section 9.1/9.2 See Example 9.1 Page 409 See Steps page 413; See Example 9.4 Page415
Practice Exercise 9.1 page 406; Practice Exercises 9.2/9.3 Page 409; Practice Exercises9.4-9.6 Page 415

Look at End of Chapter Exercises #9,1-#9,7 page 458; Wrk Review Problems #9.73-#9.82 page 460-1

Module Four II: Part O: Polarity of Molecules 1 point

Draw the dot structure for the following compounds, then state whether the molecule is polar or nonpolar:

_____________1. H2O _____________2. CO2 __________ _ _3. C2H4 _______ ______4. SO2 __________ ___5. SO3 ________ _____6. HCN _________ ____7. CH4 ________ _____8. NH3 ______________9. CH2O ______________10. C2H2 _______________ 11. PF5 ______________ 12. SF6

.

Reading Reference: Section 8.6; Section 9.3

See Example 9.5 page 419 Work Practice Exercises 9.7/9.8 Page 420

Module Four II - Part P: Hybrid Orbitals of Molecules 1 points

Use the dot/stick structures in the table to predict the hybrid orbitals that overlap to form the covalent bond:

_____________1. H2O the sigma bond between either H-O _____________2. CO2 the sigma bond between either C=O _____________2a. CO2 the pi bond between either C=O _____________3. C2H4 the sigma bond between the two carbons _____________3a. C2H4 the pi bond between the two carbons _____________4. SO2 the sigma bond between S=O _____________4a. SO2 the pi bond between S=O ____________4b. SO2 the sigma bond between S-O ____________ 5. SO3 either sigma bond between S-O ____________ 5a. SO3 the sigma bond between S=O ____________ 5b. SO3 the pi bond between S=O ____________6. HCN the single (sigma) bond between H-C ____________6a. HCN the sigma bond between C=N ____________6b. HCN either pi bond between C=N ____________7. CH4 the sigma bond between any of the H-C ____________8. NH3 the sigma bond between any of the H-N ___________ 9. CH2O either sigma bond between the H-C ____________9a. CH2O the sigma bond between the C=O ____________9b. CH2O the pi bond between the C=O ___________ __10. C2H2 the sigma bond between the C=C _________ ____10a. C2H2 either pi bond between the C=C _____________ 10b. C2H2 the sigma bond between any of the H-C

.

What is difference between a Sigma (σ) and a pi (π) bond? What is a delta(Δ) Bond

Reading Reference Jespersen 7^th : Section 9.5 and 9.6
Try Practice Exercise 9.11 and 9.12 page 427; Look at Example 9.6 page 428 and 9.7 page 430-431

Try Practice Exercise 9.14 and 9.15 Page 431 Study Example 9.8Page 432 Do Practice Exercises 9.16 and 9.17 page 433, the 9.20 and 9.21 page 440