3-1 CHEM 100, Fall 2014 LA TECH Instructor: Dr. Upali Siriwardane e-mail: [email protected] Office:...
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Transcript of 3-1 CHEM 100, Fall 2014 LA TECH Instructor: Dr. Upali Siriwardane e-mail: [email protected] Office:...
3-1CHEM 100, Fall 2014 LA TECH
Instructor: Dr. Upali Siriwardane
e-mail: [email protected]
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
3-22CHEM 100, Fall 2014 LA TECH 2-25
Models of Ethanol
CHEM 100, Fall 2012 LA TECH
3-23CHEM 100, Fall 2014 LA TECH
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
3-27CHEM 100, Fall 2014 LA TECH
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:
3-28CHEM 100, Fall 2014 LA TECH
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?
3-29CHEM 100, Fall 2014 LA TECH
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
3-31CHEM 100, Fall 2014 LA TECH
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)