3-1CHEM 100, Fall 2014 LA TECH

Instructor: Dr. Upali Siriwardane

e-mail: upali@latech.edu

Office: CTH 311

Phone 257-4941

Office Hours: M,W, 8:00-9:30 & 11:30-12:30 a.m

Tu,Th,F 8:00 - 10:00 a.m.   Or by appointment

Test Dates:

Chemistry 100(02) Fall 2014

September 29, 2014 (Test 1): Chapter 1 & 2

October 20, 2014 (Test 2): Chapter 3 & 4

November 12, 2014 (Test 3) Chapter 5 & 6

November 13, 2014 (Make-up test) comprehensive: Chapters 1-6 9:30-10:45:15 AM, CTH 328

3-2CHEM 100, Fall 2014 LA TECH

REQUIRED :

Textbook:  Principles of Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro - Pearson Prentice

Hall and also purchase the Mastering Chemistry

Group Homework, Slides and Exam review guides and sample exam questions are available online:

http://moodle.latech.edu/ and follow the course information links.

OPTIONAL :

Study Guide: Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro 2nd Edition

Student Solutions Manual: Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro 2nd

Text Book & Resources

3-3CHEM 100, Fall 2014 LA TECH

3.1 Hydrogen, Oxygen, and Water……………………………. 78

3.2 Chemical Bonds…………………………………………… 80

3.3 Representing Compounds: Chemical Formulas and Molecular Models.. 82

3.4 An Atomic-Level View of Elements and Compounds…………….. 84

3.5 Ionic Compounds: Formulas and Names…………………… 87

3.6 Molecular Compounds: Formulas and Names……………………… 93

3.7 Formula Mass and the Mole Concept for Compounds………… 97

3.8 Composition of Compounds…………………………….. 100

3.9 Determining a Chemical Formula from Experimental Data……… 105

3.10 Writing and Balancing Chemical Equations…………………… 110

3.11 Organic Compounds………………………. 114

Chapter 3. Molecules, Compounds, and Chemical Equations

3-4CHEM 100, Fall 2014 LA TECH

Chapter 3. KEY CONCEPTS

• Writing Molecular and Empirical

Formulas (3.3)• Classifying Substances as Atomic

Elements, Molecular Elements, Molecular Compounds, or Ionic Compounds (3.4)

• Writing Formulas for Ionic Compounds (3.5)

• Naming Simple Ionic Compounds (3.5)• Naming Ionic Compounds Containing

Polyatomic Ions (3.5)• Naming Molecular Compounds (3.6)• Naming Acids (3.6)• Calculating Formula Mass (3.7)• Using Formula Mass to Count

Molecules by Weighing (3.7)• Calculating Mass Percent Composition

(3.8)

• Using Mass Percent Composition as a Conversion Factor (3.8)

• Using Chemical Formulas as Conversion Factors (3.8)

• Obtaining an Empirical Formula from Experimental Data (3.9)

• Calculating a Molecular Formula from an Empirical Formula and Molar Mass (3.9)

• Obtaining an Empirical Formula from Combustion Analysis (3.9)

• Balancing Chemical Equations (3.10)

3-5CHEM 100, Fall 2014 LA TECH

3-6CHEM 100, Fall 2014 LA TECH

Structural formula

Space-filling model

Methane, CH4

CHEMICAL BONDS: THE FORCE BETWEEN ATOMS

What Makes a Molecule?

3-7CHEM 100, Fall 2014 LA TECH

Nonmetal

Name the most “metallic” of the nonmetals first.

+ Nonmetal

Change the ending of the nonmetal to “IDE.” Indicate the number of atoms of the nonmetal by Latin prefixes.

·Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca ·Examples:

– P2O5: diphosphorous pentaoxide – CO: carbon monoxide

2-10

Molecular Compounds:

3-8CHEM 100, Fall 2014 LA TECH

For compounds composed of two non-metallic

elements the more metallic element is listed

To designate the multiplicity of an element Greek prefixes are used:

mono 1; di 2; tri 3; tetra 4; penta 5; hexa 6; hepta 7; octa 8

Naming Binary Molecular-Covalent Compounds

3-9CHEM 100, Fall 2014 LA TECH

1) H2O, Na3PO4, HCl, C2H6, NH3, KCl, CH4, NH4Cl, C6H12O6, Brass-

CuxZny, SO3, NaCl, CO2

Identify the types of compounds in the above list:

Molecular compound:

Ionic compound:

Alloy:

Organic:

Inorganic:

3-10CHEM 100, Fall 2014 LA TECH

H2O, Na3PO4, HCl, C2H6, NH3, KCl, CH4, NH4Cl, C6H12O6, Brass-

CuxZny, SO3, NaCl, CO2

2) Which of the above compounds have Molecular formula:

Ionic formula:

Distinct empirical formula:

3-11CHEM 100, Fall 2014 LA TECH

3) Indicating the type and number of atoms in a molecule of the covalent compound: C6H12O6.

a.C:

b.H:

c.O:

d.Molecular formula:

e. Empirical formula:

CHEM 100, Fall 2012 LA TECH 2-14

3-12CHEM 100, Fall 2014 LA TECH

H2O water (common name)

NH3 ammonia (common name)

N2O dinitrogen oxide (nitrous oxide) NO nitrogen monoxide (nitric oxide) NO2 nitrogen dioxide

N2O4 dinitrogen tetroxide CO carbon monoxide CS2 carbon disulfide

SO3 sulfur trioxide

CCl4 carbon tetrachloride PCl5 phosphorus pentachloride SF6 sulfur hexafluoride

Simple Binary Molecular Compounds

3-13CHEM 100, Fall 2014 LA TECH

4) Give systematic names to following binary inorganic molecular compounds

a) H2O: b) HCl: c) SF6:

d) BF3: e) N2O4: f) CCl4:

g) SO3: h) PCl3:

3-14CHEM 100, Fall 2014 LA TECH

5) Give the common name of the following molecular compounds

a.NH3:

b.CH3COOH:

c.C6H12O6:

d.C2H5OH:

3-15CHEM 100, Fall 2014 LA TECH

Types of acids ·Binary acids

·H+ and nonmetal anion

In aqueous solutions, acids contain

the H+ cation and

·Oxyacids ·H+ cation and polyatomic anion

anion.

2-19

ACIDS

3-16CHEM 100, Fall 2014 LA TECH

Formula starts with acidic H HCl Hydochloric acid HNO3 Nitric acid

H2SO4 Sulfuric acid HClO3 Chloric acid

H3BO3 Boric acid

H3PO4 Phosphoric acid

Naming Acids

3-17CHEM 100, Fall 2014 LA TECH

HClO2 chlorous ClO2¯ “chlortie”

HClO3 chloric ClO3¯ chlorate

HClO4 perchloric ClO4¯ perchlorate HNO3 nitric NO3 ¯ nitrate

HClO hypochlorous ClO ¯ ”hypochlorite”

HNO2 nitrous NO2 ¯ nitrite

Names of acids and ions

3-18CHEM 100, Fall 2014 LA TECH

formula ends with OH

Ba(OH)2 barium hydroxide

NaOH sodium hydroxide

KOH potassium hydroxide

Ca(OH)2 calcium hydroxide

NH4OH ammonium hydroxide

Naming bases

3-19CHEM 100, Fall 2014 LA TECH

6) Give the names of the following acids Formula Name Ion (s) Formula Name Ions(s)

a) HNO3:

b) H3PO4:

c) HNO2:

d) H3PO3:

e) H2SO4:

f) H2CO3:

g) H2SO3:

h) CH3COOH:

3-20CHEM 100, Fall 2014 LA TECH

Hydrocarbonsalkanes – CnH2n+2 E.g. C5H12 pentane alkenes – CnH2n E.g. C2H4 ethene alkynes – CnH2n-2 E.g. C2H2 ethyne

Alcohols ROH E.g C2H5OH ethanol

Hyd rocarbons and Alcohols

where R refers to the hydrocarbon radical backbone created by substituting an -OH functional group for a H atom in the hydrocarbon

3-21CHEM 100, Fall 2014 LA TECH

Types of Chemical Formula Molecular Shows ratio of atoms each element in the

: C2H6O Condensed

Shows groups of atoms bonded together in the formula. E.g ethyl alcohol: CH3CH2OH

Structural Shows bonding of important groups in the formu

E.g ethyl alcohol:

a

compound. E.g ethyl alcohol

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Models of Ethanol

CHEM 100, Fall 2012 LA TECH

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7) Given the structural formula of an organic compound, write the for the following: CH3CHClCH2OH

a.molecular formula

b.condensed formula

c.structural formula

d.line formula

CHEM 100, Fall 2012 LA TECH 2-26

3-24CHEM 100, Fall 2014 LA TECH

Catenation The formation of chains of atoms of the same

This key feature of carbon permits a vast number of compounds to exist.

Four types of hydrocarbons 1.Alkanes (saturated): single C-C bonds 2.Alkenes (unsaturated): double C=C

bond 3.Alkynes (unsaturated): triple bond 4.Aromatic (unsaturated): benzene rings

e lement.

Hydrocarbons

3-25CHEM 100, Fall 2014 LA TECH

methane – CH4

ethane – C2H6

propane – C3H8

butane – C4H10

pentane – C5H12

hexane – C6H14

heptane – C7H16

octane – C8H18

nonane – C9H20

decane – C10H22

Alkanes CnH2n+2

3-26CHEM 100, Fall 2014 LA TECH

Meth- 1

Eth- 2 Prop- 3 But- 4 Pent- 5 Hex- 6 Hept- 7Oct- 8Non- 9 Dec- 10

I see much memorization in

your future!

Prefix Carbons

Base names of hydrocarbons

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8) Name, molecular, condensed and line formula of straight chain alkane (saturated hydrocarbons) or n-alkanes.

a.4 carbon n-alkane:

b.7 carbon n-alkane:

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Compounds with the same number and type of atoms but with different arrangements are called constitutional isomers

Condensed formulas

Molecular Formula C5H12

CH3CH2CH2CH2CH3 pentane

CH3CH(CH3)CH2CH3 2-methylbutane

(CH3)4C 2,2-dimethylpropane

All are isomers of C5H12.

What is an Isomer?

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Alkane Isomers is there a formula?

3-30CHEM 100, Fall 2014 LA TECH

9) Draw the structural formula of constitutional isomers of butane with molecular formula C4H10.

a.n-butane: CH3CH2CH2CH3

b.isobutene: (CH3) 3CH

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Butane

Butane molecules are present in the liquid and gaseous states in the lighter

3-32CHEM 100, Fall 2014 LA TECH

Determine empirical formulas for the following:

1. An ionic compound that has two aluminum ions for every three oxide ions

2.Hexane, C6H14

3.Arabinose, C5H10O5

4.Hydrogen peroxide,

Al2O3

(C3H7)n where n = 2

(CH2O)n where n = 2

(HO)n where n = 2

3-33CHEM 100, Fall 2014 LA TECH

Classifying Organic Compounds

Examples Functional Group Ending

Hydrocarbons C and H only -aneAlcohols R-OH -olAcids R-COOH -oic acid

Amines R-NH2 -amine

Ketones R(C=O)R’ -oneAldehydes R-CHO -al

3-34CHEM 100, Fall 2014 LA TECH

10) Classification and the name of the following

Classification Name

a.CnH2n+2 where n is 8:

b. CH3CH2CH2CH2-OH:

c. CH3CH2CH2-COOH:

d. CH3CH2CH2CH2CH2CH2-NH2:

a.CH3CH2-(C=O)-CH3:

d) CH3CH2-CHO:

3-35CHEM 100, Fall 2014 LA TECH

The Many Representations of a Molecule

3-36CHEM 100, Fall 2014 LA TECH Carbohydrate: Glucose

Linear form Cyclic form

3-37CHEM 100, Fall 2014 LA TECH Fats: triglycerides

Saturated fats

Unsaturated fats

3-38CHEM 100, Fall 2014 LA TECH

11) Identify the classification or name of the following biologically important molecules

a) b) c)

d) e) f)