1-1 CHEM 100, Fall 2011 LA TECH Instructor: Dr. Upali Siriwardane e-mail: [email protected] Office: CTH 311 Phone 257-4941 Office Hours: M,W, 8:00-9:00.

1-1CHEM 100, Fall 2011 LA TECH

Instructor: Dr. Upali Siriwardane

e-mail: [email protected]

Office: CTH 311 Phone 257-4941

Office Hours: M,W, 8:00-9:00 & 11:00-12:00 a.m Tu,Th,F 9:00 - 10:00 a.m.

Test Dates: March 25, April 26, and May 18; Comprehensive Fina

Exam: 9:30-10:45 am, CTH 328.

Chemistry 100(02) Fall 2011

October 3, 2011 (Test 1): Chapter 1 & 2

October 26, 2011 (Test 3): Chapter 3 & 4

November 16, 2011 (Chapter 5 & 6)

November 17, 2011 (Make-up test) comprehensive: Chapters 1-6

9:30-10:45:15 AM, CTH 328


REQUIRED :

Chemistry: The Molecular Science 4th Edition, John W. Moore, Conrad

L. Stanitski and Peter C. Jurs. 2010 Brooks and Cole ISBN-10:

1439049300 ISBN-13: 9781439049303

OWL: Students are required to buy access to OWL program offered by

Brooks/Cole's)

OPTIONAL :

Study Guide: 4th Edition, John W. Moore, Conrad L. Stanitski and Peter C. Jurs.

2010 Brooks and Cole Edited by Michael J. Sanger.

Student Solutions Manual: The Molecular Science, 4th by Moore/Stanitski/Jurs,

Edited by Jusy L. Ozment

Text Book & Resources


Chapter 1. 1. Why Care about Chemistry

2. Molecular Medicine

3. How Science is Done

4. Identifying Matter: Physical Properties

5. Chemical Changes and Chemical Properties

6. Classifying Matter: Substances and Mixtures

7. Classifying Matter: Elements and Compounds

8. Nanoscale Theories and Models

9. The Atomic Theory

10. The Chemical Elements


Chapter 1. KEY CONCEPTS What is chemistry?

Scientific Method. Scientific Measurement Physical changes and properties. Temperature Conversions. Factor label method. Conversion factors. Density Calculations. Chemical change and properties. Categories of matter. Separating Mixtures. Elements and Compounds Atomic symbols

Macro, micro and nano-scales Prefixes of unit of length Properties of the three states of matterKinetic-molecular theory Dalton's atomic theory Three chemical LawsDiscovery of elementsChemical Elements and propertiesChemical SymbolismInterpreting chemical formulas and chemical reaction.


What is chemistry?Chemistry deals with non-reversible

changes of matter.

Chemistry explains using atoms and molecules.

Chemical Concepts and Models improve your problem solving skills

Chemistry is a Central Science


Scientific Method


Kinetic Molecular Theory

Matter consists of particles (atoms or molecules) in continuous, random motion.


•can be compressed

•exert pressure on whatever surrounds them

•expand into whatever volume is available

•easily diffuse into one another

•can be described in terms of their temperatures and pressure, the volume occupied,

and the amount (number of molecules or moles) present

Properties of Gases


Gas Laws (This is not theory)

•Boyle's Law (V and P) •Charles Law (V and T)•Gay-Lussac's combined Gas Law • (V, P and T)•Avogadro's Law (V and n)

•Ideal Gas Law (V, P, n, R and T)

Scientific law is a summary or pattern

in observation


Kinetic Molecular Theory: Gases

particles in continuous, random, rapid motion

collisions between particles are elastic

volume occupied by the particles is negligibly small effect on their behavior

attractive forces between particles have a negligible effect on their behavior

gases have no fixed volume or shape, take the volume and shape of the container


Kinetic Molecular Theory: Solidparticles are tightly packed together in regular array

particles vibrate about average positions

seldom squeeze past other atoms

results in a rigid material with a small, fixed volume for a given mass

external shape often reflects internal arrangement of particles


Kinetic Molecular Theory: Liquid

particles are arranged more randomly than in solid

particles less confined so that they can move past one another

particles are a little further apart, thus slightly larger, fixed volume

particles are constantly interacting with one another


Development of Dalton’s Atomic Theory


Alchemist: Discovery of Elements

Early scientist observed chemical changes of matter. They called these changes chemical reactions when there are changes in substances or the physical & chemical properties of the matter. They also observed a pattern or a repeatable observation during chemical reactions.


•Law of Conservation of Mass:

•Law of Constant Proportions:

•Law of Multiple Proportions:

Three Observed Chemical Laws:


Law of Conservation of Mass

Total mass after a chemical reaction is same as before the reaction.

H2 + 1/2 O2 ---> H2OHydrogen (4g) + oxygen (32g) ----> water 36g after

the reaction.


•A given chemical compound always contains exactly the same proportion of elements by

weight.

• 36g of water contains

• 4g of hydrogen and 32g of oxygen

•take any other chemical compound.

Law of Constant (Definite) Proportions


When two elements make a series of chemical compounds, the ratio of the masses of the second

elements that combine with 1 gram of the first element can always be reduced to simple whole

numbers.

C O

E.g. carbon monoxide 1g 1.33g

carbon dioxide 1g 2.66g

Law of Multiple Proportions


Dalton’s atomic theoryAll matter is composed of atoms -- the smallest

particle of an element that takes part in a chemical reaction.

All atoms of an element are alike.

Compounds are combinations of atoms of one or more elements. The relative number of atoms each element is always the same.

Atoms cannot be created or destroyed by a chemical reaction. They only change how they combine with each other.


What is an Atom?

Very small particle.Smallest particles of elements and molecules

There about 110 types of elements or Atoms.

Different atoms have different physical properties and chemical reactivity


Models of matter

Models are commonly used to help visualize atoms and molecules.

Atom - The smallest unit of an element that has all of the properties of an element.

Molecule -The smallest unit of a pure substance that has the properties of that substance. It may contain more that one atom and more than one element.

Ions - Charged particles formed by the transfer of electrons between atoms or molecules


Molecular Medicine


Properties of SubstancesPhysical properties:

Physical properties are descriptions of matter such as color, density, viscosity, boiling point, and melting point.

Chemical properties:

Chemical properties relates to the changes of substances making up the matter. For example, corrosiveness, Flammability


one that can be observed without changing the substances present in the sample

Examples

– color density– odor melting point– taste boiling point– feel compressibility

Properties of Matter: Physical Properties


Properties of MatterChemical Property

the tendency to react and form new substances

reactants undergo chemical change to produce products: Chemical Reaction

sucrose => carbon + water

reactant products


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.


Chemical Change: caramelizing sugar


Chemical verses Physical change

Sodium reacting Iodine changing

with chlorine. from a solid to a gas


Pure substances

Element• Cannot be converted to a simpler form by a chemical

reaction.• Example hydrogen and oxygen

Compound• Combination of two or more elements in a definite,

reproducible way.

• Example water - H2O

Both elements and compounds have characteristic properties such as color, boiling point and reactivity


Allotropes

GraphiteDiamond

Buckminsterfullerine

Forms of element that has different bonding pattern


Scheme for the Classification of Matter


Mixtures Mixtures

HeterogeneousHeterogeneous HomogenousHomogenous

CompoundsCompounds

AtomsAtoms

ElectronsElectrons

NucleusNucleus

ProtonsProtonsNeutronsNeutrons

Pure SubstancesPure Substances

ElementsElements

Hierarchy of Matter


Mixtures• A combination of two or more pure

substances.

• Homogeneous - Uniform composition (solution)

• Heterogeneous - Non-uniform composition

Which are homogeneous or heterogeneous?

• Blood Urine “T-Bone” steak

• Gasoline Twinkie Salad Dressing


Types of Elementsmetals

nonmetals

metalloids – semimetals

Artificial Elements


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).


Areas of Chemistry“The study of matter and the changes it undergoes.”

Major divisions

Inorganic Compounds of elements other than carbon

Organic Compounds of carbon

Biochemistry Compounds of living matter

Physical Theory and concepts

Analytical Methods of analysis


How do you Separate Mixtures?

Flotation: based on density

Filtration: Solid- liquid

Distillation- Liquid-liquid

Magnetic Separation- Magnetic

Chromatography:1) Paper 2) Column 3) Gas


Separation of Mixtures

Filtration

distillation

chromatography


Separate a solid (precipitate) form suspension:_________________

separate solids by differences in melting points:_________________

separate materials based on their differences in absorption on a support:______________

Separation of Mixtures (continued.)


Chromatography

Liquid-column

Paper

thin-layer (TL Chromatography-TLC)

Gas

HPLC (high pressure liquid chromatogarphy)

Electrophoresis (DNA mapping)


Physical States

Solid• fixed volume and shape

Liquid• fixed volume• shape of container, horizontal top

surface

Gas• takes shape and volume of container


Nanoscale representations of the three states of matter


Macroscale, Microscale, and Nanoscale


Sample Sizes

macroscale• physical properties that can be observed by

the unaided human senses

microscale• samples of matter that have to be viewed with

a microscope

nanoscale• samples that are at the atomic or molecular

scale where chemical reactions occur

1-1 CHEM 100, Fall 2011 LA TECH Instructor: Dr. Upali Siriwardane e-mail: [email protected] Office: CTH 311 Phone 257-4941 Office Hours: M,W, 8:00-9:00.

Documents

chemical properties

la tech chapter

navogadros law v

pboyles law v

tcharles law v

chemical changes

p charles law v

tideal gas law v