Chemistry 1 // 1st Quarter SY 2011 - 2012

Units of MeasurementMetric System

- Unites used for scientific measurements- Developed in France during the late 18th

CenturySI Units

- Specified Metric Units Used in Scientific Measurements

- Has seven base units

SI BASE UNITSPhysical Quantity

Name of Unit

Abbreviation

Mass Kilogram kgLength Meter mTime Second s

Temperature Kelvin kAmount of Substance

Mole mol

Electric Current Ampere ALuminous Intensity

Candela cd

METRIC SYSTEMMetric Prefix

Metric System

Multiple

Tera T 1012

Giga G 109

Mega M 106

Kilo K 103

Hecto h 102

Deca da 101

Unit (base) 100

deci d 10-1

centi c 10-2

milli m 10-3

micro µ 10-6

nano n 10-9

pico p 10-12

6.02 x 1023 - Avogadra Law (Mole)

Types of MeasurementQualitative

- Associated with quality, kindex. Shades of color; degree of sweetness

Quantitative- Associated with numbers

ex. Mass, volume, length, area

Accuracy and Precision Accuracy

- Closeness to the true valuePrecision

- Repeatability, reproducibility of Measurement

One drop = 0.05 mL1 mL = 20 dropsFew drops = 1-2 dropsSeveral drops = 3-5 drops

Graduated Beakers & Erlenmeyer Flasks - Measures out volume accurately up to +/-

10 mL- Not good for determining volume

Graduated Cylinder

- Accurate to about +/- 0.5 mLBurettes

- Accurate to about +/- 0.01 mLVolumetric Flask & Transfer Pipettes

- Accuracy up to +/- 0.01 mL

Scientific Notation- A system of expressing numbers- Makes the writing of very big or very

small numbers easyex. 35,000,000,000,000,000 = 3.5 x 1016

Significant Digits or FiguresRules:

1. All non-zero digits are significant.2. Zeros between non-zero digits are

significant. 3. Leading zeros are not significant, trailing

zeros are. (This depends on presence of decimal point.)

4. Scientific notations remove the doubt in determining the number of significant figures.

Operations: 1. Multiplication and Division - Least number

of Significant Figures2. Addiction and Subtraction - Least number

of decimal places3. PEMDAS - Convert to the correct number

of Significant Figures only after doing the all operations.

Chemistry- The study of matter and the changes it

undergoesA. Health and Medicine

Sanitation Systems Surgery with Anesthesia Vaccines and Antibiotics

B. Energy and the Environment Fossil Fuels Solar Energy Nuclear Energy

C. Materials and Technology Polymers, ceramics, liquid crystals Room Temperature, Super

conductors? Molecular Computing?

D. Food and Agriculture Genetically Modified Crops “Natural” Pesticides Specialized Fertilizers

Matter - anything that occupies space and has mass

o Substance - form that a definite composition and distinct propertied

Element - substances that cannot be separated into simpler substances by chemical means

Compound - substance composed of atoms of two or more elements chemically united in fixed proportions

o Mixture - combination of two or more substances in which the substances retain their distinct identities Homogeneous - composition is the

same throughout

© PAT RIVERA

Chemistry 1 // 1st Quarter SY 2011 - 2012

Heterogeneous - composition is not uniform throughout

* 113 elements have been identified. * 83 occur naturally on Earth.* 37 have been created by scientists.

Physical Means - separate a mixture into its simpler substancesChemical Means - separates compounds into its pure components

Physical Change - does not alter composition or identity of a substanceChemical Change - alters composition or identity of a substance

Extensive Property - depend upon how much matter is being consideredIntensive Property - does not depend upon how much matter is being considered

Mass - measure of quantity of matterWeight - force that gravity exerts on an objectVolume - SI derived unit for volume in cubic meters

Acids - substance that yield Hydrogen ions (H+),

when dissolved in water - have sour taste- cause color changes in plant dyes- react with certain metals to produce

Hydrogen gas- react with carbonates and bicarbonates

to produce Carbon Dioxide gas- Oxoacids contain hydrogen, oxygen and

another element- Aqueous acid solutions conduct

electricityBase

- substance that yields hydroxide ions (OH-) when dissolved in water

- has bitter taste- feels slippery (most soap contain bases)- cause color changes in plant dyes- Aqueous base solutions - conduct

electricity

pH - measures acidity- means “Power of Hydrogen”

Neutral - pH = 7 Acidic - pH < 7 Basic - pH > 7

Neutralization - Acid + Base Salt + WaterSalt & Water

- product of Neutralization- electrically neutral- equal amount of cations (postitive) and

anions (negative)

Solution - end product of solvent + solute- homogeneous mixture- formed by 2 substances or more

Solvent - present in larger amountSolute - present in smaller amountColloids - particles do not settle

Colloids - tyndall effectParticles - bigger than solution; smaller

than suspensionCoarse mixture - mixture of substances which when you mix all the substances you can see that the substances that are mixed were not dissolved

John Dalton- Father of Modern Atomic Theory- Also known for his research on color

blindnessDalton’s Atomic Theory (1808)

1. • Elements are composed of extremely small particles called atoms.• All atoms of a given element are identical.• The atoms of one element are different from the atoms of all other elements.

2. • Compounds are composed of atoms of more than one element combined together.• The relative number of atoms of each element in a given compound is always the same.

3. • Chemical reactions only involve rearrangement of atoms.• Atoms are not created or destroyed in chemical reactions.

Law of Definite Proportions “Proust’s Law” Made by French Chemist Joseph

Proust A chemical compound always

contains exactly the same proportions of elements by mass

One of the basic Laws of Stoichiometry

Law of Multiple Proportions “Dalton’s Law” One of the basic Laws of

Stoichiometry If two elements form more than one

compounds between them. Then the ratio of the masses of the 2nd element combined with the 1st element will be ratios of small whole numbers.

Law of Conservation of Mass “Lomonosov-Lavoisier Law” Masses of substances in a closed

system will remain constant, no

© PAT RIVERA

Matter

Substance

Mixture

Elements

Compounds

Homogeneous

Heterogeneous

PHYSICAL MEANS

CHEMICAL MEANS

MEDIUM

DISPERSED

Gas Liquid SolidGas none Liquid aerosol

Ex. fog; mistSolid Aerosol

Ex. smokeLiquid foam

Ex. whipped cream

emulsionEx. milk

SolEx. Blood

Solid Sold FoamEx. Styrofoam

GelEx. Gelatin

Solid SolEx: Glass

Chemistry 1 // 1st Quarter SY 2011 - 2012

matter what processes are acting inside the system.

The mass of the reactants must always be equal to the mass of the products.

Limiting Reactants - limits the production of products- totally consumed in a reaction- determines that amount of products

X - ElementY - Atomic Number = #pZ - Atomic Mass = #p + #nW - Charge = #p - #ep - Protons (Positively Charged); e - Electrons (Negatively Charged); n - Neutrons (Neutral)

Atomic Mass - (Abundance)(Mass1)+(Abundance)(Mass2) Isomers - Compounds with same molecular structure but different structural formula

Isotopes - elements with different numbers of atomic numberIsobars - atoms or ions with the same atomic number mass but different atomic numbersAllotropes - different forms of the same element in the same physical stateMolecule - combination of two or more atoms in a definite arrangement held together by chemical bonds

Diatomic Molecule - contains only two atoms

“Have No Fear Of Ice Cold Beer!”Polyatomic Molecule - more than two

atomsIon - Atom or group of atoms with a positive/negative charge

Cation - positiveAnion - negative

Monoatomic ion - contains only one atomPolyatomic ion - contains more than one

atom

© PAT RIVERA

XY

Z

W