1-1CHEM 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

1-2CHEM 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

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Chapter 1. Matter, Measurement, and Problem Solving

1. 1 Atoms and Molecules………………………………….. 1

1 .2 The Scientific Approach to Knowledge…………….. 3

1 .3 The Classification of Matter…………………………… 5

1 .4 Physical and Chemical Changes and Physical and Chemical

Properties…………………………………….. 9

1 .5 Energy: A Fundamental Part of Physical and Chemical

Change…………………………………………………….. 12

1 .6 The Units of Measurement……………………………... 13

1 .7 The Reliability of a Measurement……………………… 20

1 .8 Solving Chemical Problems……………………………. 27

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Chapter 1. KEY CONCEPTS

• What is chemistry?• Scientific Method.• Properties of the three states of

matter• Physical changes and

properties.• Chemical change and

properties.• Categories of matter. • Elements and Compounds• Atomic symbols• Chemical Elements and

properties• Chemical Symbolism• Separating Mixtures.• Scientific Measurement

• Prefixes of SI units• Macro, micro and nano-scales • Conversion factors.• Factor label method.• Uncertainty and significant

figures• Temperature Conversions.• Density Calculations.• Three chemical Laws• Dalton's atomic theory • Interpreting chemical formulas

and chemical reaction.• Concept of mole• Gram to mole conversion

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•SOLIDS

–have rigid shape, fixed volume. External shape can reflect the atomic and molecular

arrangement.

•Reasonably well understood

•LIQUIDS

–have no fixed shape and may not fill a container completely.

•Not well understood

•GASES

–expand to fill their container.

•Good theoretical understanding

The States of Matter

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Matter Classifications

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1) Describe the classification of matter based on state of matter and composition.

 

 

 

 

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2) What is a pure substance? (Describe it generally and given two examples)

 

 

 3) What is a chemical element? (Describe it generally and given an example)

 

 

 

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4) What is an allotrope of an element? (Describe it generally and given an example)

 

 

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5) What is a chemical compound? (Describe it generally and given an example)

 

 

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Physical Changes• Phase changes

• Substance does not change into a new substance.• Example:

– Ice (s) going to water (l) going to steam (g)

Physical properties• Density• Color intensity• Particle size• Melting/ Freezing point• Boiling point• Texture• Magnetism

Physical Changes and Properties of Matter

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Separating Mixtures to Pure SubstancesFlotation/buoyancy

Depend on the density, of substances.

Filtration/sedimentation

Depend on the physical state (sloid/liquid)

Distillation/evaporation

Depend on the boiling points of substances.

Chromatographic Separations

Dependent of the affinity to substrate (paper).

Magnetic Separations

Dependent of the magenetic properties.

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6) What properties are used to separate mixtures into pure substances?

 

 

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Atomic SymbolsEach element is assigned a unique symbol.

arsenic As potassium Kbarium Ba nickel Nicarbon C nitrogen Nchlorine Cl oxygen Ohydrogen H radon Rnhelium He titanium Tigold Au uranium U

Each symbol consists of 1 or 2 letters. The first is capitalized and the second is lower case.

Symbol may not match the name - often had a different name to start with.

Some elements (about 11) the names were not in English. E.g., Sodium-Na (natrium-latin), potassium-K(kalium-latin).

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7) How are the elements given symbols? (Give three examples)

 

 8) How are the compounds given formulas? (Give three examples)

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Physical Change of Matter

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•Chemical change or chemical

reaction:

•Making a NEW compound

•The transformation of one or more atoms or

molecules into one or more different

molecules

Chemical Changes and Properties of Matter

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Physical and Chemical Changes and Physical and Chemical Properties

9) What is a physical change? Describe it generally and given an example.

 

 

10) What is a chemical change? Describe it generally and given an example.

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11) List physical properties: Describe it generally giving an example.

a)

b)

c)

d)

e)

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12) List chemical properties: name them and give an example.

 

a)

b)

c)

d)

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Extensive and Intensive Properties

Extensive properties

Depend on the quantity of sample measured.

Example - mass and volume of a sample.

Intensive properties

Independent of the sample size.

Properties that are often characteristic of the substance being measured.

Examples - density, melting and boiling points.

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13) What is the difference between intensive and extensive properties? Give examples

 

 

 

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14) Identify following as physical and chemical change:

 

 

 

Frying an egg

Vaporization of dry ice

Burning Gasoline

Breaking Glass

Boiling water

Souring Milk Compression of a spring

Melting Glass

Cutting grass

Vine fermentation

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Introduction to Energy

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The energy of the universe is CONSERVED.

1st Law of Thermodynamics

All matter possesses energy.

Energy is classified as either kinetic or potential.

Kinetic energy: energy associated with movement

KE = I/2 mv2

Potential energy: energy associated with storage

PE = mhg

Energy can be converted from one form to another.

When matter undergoes a chemical or physical change, the amount of energy in the

matter changes as well.

Energy

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Changes in matter, both physical and chemical, result in the matter either gaining or

releasing energy.

Energy is the capacity to do work.

Work is the action of a force applied across a distance.

A force is a push or a pull on an object.

Electrostatic force is the push or pull on objects that have an electrical charge.

Energy and Matter: One and the Same

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15) What is law of conservation of energy and how it applies to physical and chemical change given below?

a) H2O(l) H2O (g)

 

 

b) CH4 + 2O2 CO2 + 2H2O

 

 

 

Energy: A Fundamental Part of Physical and Chemical Change