COMMON ORIGIN1. All things have a common origin2. Atomic models and the behavior of the

atom3. Atomic structure and the correlation of

element’s physical and chemical properties.

WHY WHY STUDY CHEMISTRY?STUDY CHEMISTRY?

Chemistry is how the world works!

? What are some ways

chemistry effects our lives?1- Health Care2- Conservation of natural resources3- environmental protection5- everyday needs

ALL THINGS HAVE A COMMON ORIGIN The atom is the building block of all matter.

Basic structure of an element.

Atoms in all different forms make up elements

Elements make up all matter in the universe

Most matter is composed of different combinations of only about 100 different elements

Molecules: 2 or more atoms

COMMON ORIGIN CONT.

A quick run down of Atoms, Elements and Molecules. http://www.youtube.

com/watch?v=fND0ps4EtBg

Sub atomic particles Proton, neutron,

electron What 5 Elements

make up 97% of life? Carbon, Hydrogen, Nitrogen, Oxygen, Phosphorus, and Sulfur

STATES

OF M

AT

TER

Gas

Liquid

Solid

MORE CLASSIFICATIONS OF MATTER

Elements Can’t be broken

down any smaller Compounds

Composed of 2 or more elements

Law of Constant Composition

Solutions 2 or more

substances Retain own chemical

identity Homogeneous

Pure Substance Mixture

PROPERTIES OF MATTER

Can measure it without changing the identity and composition

Change in physical appearance

Changes of State

Chemical Reactions The way a substance may

change, or react, to form another substance.

Physical Properties Chemical Properties

HOW TO MEASURE IN CHEMISTRY Units of Measurement

LENGTH AND MASS

Length SI Unit: meter (m)

Slightly longer than a yard, which is 3 feet.

Mass SI Unit: Kilogram (kg) Equal to ~ 2.2 pounds (lb) Not the same as weight Mass = volume (cm3) x density (g/cm3)

METRIC SYSTEM PREFIXES…

TEMPERATURE…FAHRENHEIT, CELSIUS, KELVIN

Measures the hotness or coldness of an object.

Physical property: heat flow

For scientific use: Freezing point 0˙C Boiling point 100˙C SI Unit Kelvin: 0˙K = -273.15˙C

Absolute zero

K = ˚C + 273.15

DERIVED SI UNITS

Volume Cubic Centimeters

(cm3) (length cubed)

Calculate the volume of 65.0 g of the liquid methanol (wood alcohol) if its density is 0.791 g/mL

Density Density =

mass/volume g/cm3 or g/mL 1 mL = 1 cm3

Calculate the density of mercury if 1.00 X 102 g occupies a volume of 7.36 cm3

What is the mass in grams of cube of goal (density = 19.32 g/cm3) if the length of the cube is 2.00 cm?

UNCERTAINTY IN MEASUREMENT

A measure of how closely individual measurements agree with one another.

Refers to how closely individual measurements agree with the correct or “true,” value.

Illustrate

Good accuracy/good precision

Poor accuracy/good precision

Poor accuracy/poor precision

PRECISION ACCURACY

SIGNIFICANT FIGURES

Definition: all digits of a measured quantity, including the uncertain one (± 0.0001 g) How many Significant Figures…?

2.2 g ??? 2.2405 g ???

What is the difference…? 4.0 g ??? 4.00 g

To read significant figures you read the number from left to right, counting the digits starting with the first digit that is not zero!

ZER000000’S IN SIGNIFICANT FIGURES

1. Zer0s between nonzero digits are always significant

1005 kg 1.03 kg

2. Zer0s at the beginning of a number are never significant; they merely indicate the position of a decimal point

0.02 g 0.0026 g

3. Zer0s at the end of a number are significant if the number contains a decimal point

0.0200 g 3.0 cm