Chemistry 100(02) Fall 2014
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 :
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
CHEM 100, Fall 2014 LA TECH 1-1

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
CHEM 100, Fall 2014 LA TECH 1-2

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
CHEM 100, Fall 2014 LA TECH 1-3

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
CHEM 100, Fall 2014 LA TECH 1-4

• 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
CHEM 100, Fall 2014 LA TECH 1-5

CHEM 100, Fall 2014 LA TECH 1-6

1) Describe the classification of matter based on state of matter and composition.
CHEM 100, Fall 2014 LA TECH 1-7

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)
CHEM 100, Fall 2014 LA TECH 1-9

5) What is a chemical compound? (Describe it generally and given an example)
CHEM 100, Fall 2014 LA TECH 1-10

CHEM 100, Fall 2014 LA TECH 1-11

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
CHEM 100, Fall 2014 LA TECH 1-12

Flotation/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.
CHEM 100, Fall 2014 LA TECH 1-13

6) What properties are used to separate mixtures into pure substances?
CHEM 100, Fall 2014 LA TECH 1-14

Each element is assigned a unique symbol .
arsenic barium carbon chlorine hydrogen helium gold
As
Ba
C
Cl
H
He
Au potassium nickel nitrogen oxygen radon titanium uranium
K
Ni
N
O
Rn
Ti
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).
CHEM 100, Fall 2014 LA TECH 1-15

7) How are the elements given symbols? (Give three examples)
8) How are the compounds given formulas? (Give three examples)
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CHEM 100, Fall 2014 LA TECH 1-17

• Chemical change or chemical reaction:
• Making a NEW compound
• The transformation of one or more atoms or molecules into one or more different molecules
CHEM 100, Fall 2014 LA TECH 1-18

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.
CHEM 100, Fall 2014 LA TECH 1-19

11) List physical properties: Describe it generally giving an example. a) b) c) d) e)
CHEM 100, Fall 2014 LA TECH 1-20

12) List chemical properties: name them and give an example. a) b) c) d)
CHEM 100, Fall 2014 LA TECH 1-21

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.
CHEM 100, Fall 2014 LA TECH 1-22

13) What is the difference between intensive and extensive properties? Give examples
CHEM 100, Fall 2014 LA TECH 1-23

14) Identify following as physical and chemical change:
Frying an egg
Vaporization of dry ice
Souring Milk Compression of a spring
Burning
Gasoline
Melting
Glass
Breaking
Glass
Cutting grass
Boiling water
Vine fermentation
CHEM 100, Fall 2014 LA TECH 1-24

CHEM 100, Fall 2014 LA TECH 1-25

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.
CHEM 100, Fall 2014 LA TECH 1-26

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.
CHEM 100, Fall 2014 LA TECH 1-27

Energy: A Fundamental Part of Physical and
Chemical Change
15) What is law of conservation of energy and how it applies to physical and chemical change given below?
a) H
2
O(l)  H
2
O (g) b) CH
4
+ 2O
2
 CO
2
+ 2H
2
O
CHEM 100, Fall 2014 LA TECH 1-28