Common origin
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Transcript of Common origin
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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.
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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
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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
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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
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STATES
OF M
AT
TER
Gas
Liquid
Solid
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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
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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
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HOW TO MEASURE IN CHEMISTRY Units of Measurement
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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)
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METRIC SYSTEM PREFIXES…
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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
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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?
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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
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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!
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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