substance
DESCRIPTION
Substance. Mixture. Element. Heterogeneous mixture. Na. Fe. O 2. Neon. Gold. Carbon. H 2. Chicken soup. Italian dressing. granite. Compound. Homogeneous mixture. NaCl. Fe 2 O 3. H 2 O. Baking soda. Sugar. Sea water. Kool Aid. Grape juice. paint. bronze. - PowerPoint PPT PresentationTRANSCRIPT
Substance
Element
Compound
Na Fe O2 Neon GoldCarbon H2
NaCl Fe2O3 H2OBakingsoda
Sugar
Mixture
Heterogeneousmixture
Homogeneousmixture
Chicken soup
Italiandressing
granite
Sea water
KoolAid
Grapejuice
paint bronzeStainless
steel
PROPERTIES
500 mL25 oC
10 cm long
What could it be???
Anything!
EXTENSIVE PROPERTIES – depends on amount
1 g/mL
Clear, colorless
Odorless
MP 0oC
BP 100oC
What could it be?
We have an idea!
INTENSIVE PROPERTIES – do not depend on amount
PHYSICAL PROPERTIES
What can you observe WITHOUT CHANGING what it is?
Mass Size Magnetism
Volume Shape Solubility
Color Temperature
Odor MP, BP
Malleability, ductility
CHEMICAL PROPERTIES
What observations can you make by CHANGING what it is?
Reactivity (with another substance)
Corrosability
Flammability
Physical Changes and Separating MixturesWhat can you use to separate iron from cereal?
What can you use to separate sand, salt and water?
What can you use to separate sulfur, sugar, and iron filings?
In each case, decide if the change is a chemical or physical change.
A cup of household bleach changes the color of your socks from red to pink
Water vapor in your exhaled breath condenses in the air on a cold day
Plants use carbon dioxide from the air to make sugar
Chocolate melts when placed in the sun
A cup of household bleach changes the color of your socks from red to pink - chemical
Water vapor in your exhaled breath condenses in the air on a cold day - physical
Plants use carbon dioxide from the air to make sugar - chemical
Chocolate melts when placed in the sun - physical
UNITS OF UNITS OF MEASUREMENTMEASUREMENT
Use Use SI unitsSI units — based on the metric — based on the metric systemsystem
Length Length
MassMass
TimeTime
TemperatureTemperature
MeterMeter, m, m
KilogramKilogram, kg, kg
SecondsSeconds, s, s
Kelvin, K
Conversions
Commonly Used Prefixes: kilo = 1000 of something ( 1km= 1000m, kg) deci =0.1 of something (10 dm = 1m) centi = 0.01 of something (100 cm = 1m) milli = 0.001 of something (103 mm = 1m) micro = 0.000001 (106 µm = 1m) nano = 0.000000001 (109 nm = 1m) pico = 0.000000000001 (1012 pm = 1m)
Refer to Conversion Chart to additional prefixes.
Temperature ScalesTemperature Scales
Notice that 1 kelvin degree = 1 degree Celsius1 kelvin degree = 1 degree Celsius
Boiling point Boiling point of waterof water
Freezing point Freezing point of waterof water
CelsiusCelsius
100 ˚C100 ˚C
0 ˚C0 ˚C
100˚C100˚C
KelvinKelvin
373 K373 K
273 K273 K
100 K100 K
FahrenheitFahrenheit
32 ˚F32 ˚F
212 ˚F212 ˚F
180˚F180˚F
Temperature Temperature ScalesScales100 100 ooFF38 38 ooCC311 K311 K
oF oC K
Calculations Using Calculations Using TemperatureTemperature
•Generally require temp’s in Generally require temp’s in kelvinskelvins
•T (K) = t (˚C) + 273.15T (K) = t (˚C) + 273.15
•Body temp = 37 ˚C + 273 = 310 KBody temp = 37 ˚C + 273 = 310 K
•Liquid nitrogen = -196 ˚C + 273 = 77 KLiquid nitrogen = -196 ˚C + 273 = 77 K
DENSITYDENSITYDensity is an Density is an INTENSIVEINTENSIVE property property of matter.of matter.does does NOTNOT depend on depend on
quantity of matter.quantity of matter. temperaturetemperature
Contrast with Contrast with EXTENSIVEEXTENSIVE depends on quantity of depends on quantity of
matter.matter. mass and volume mass and volume
(separately).(separately).
StyrofoamStyrofoam BrickBrick
Significant Figures:
Digits in a measurement having values that are known with certainty plus one digit having a value that is estimated.
Measurements that contain a greater number of significant figures are more precise than measurements that contain fewer significant figures.
Always select an instrument that gives you the most significant figures. Only
report as many sig figs as that
instrument allows.
The Rules
All numbers 1-9 are significant. Zeros are sometimes significant, here's how you can
tell: If a decimal point is present, starts on the Pacific side,
move across until you get to a 1-9 digit, and start counting to the end
If a decimal point is absent, start on the Atlantic side, move across until you get to a 1-9 digit, and start counting to the end
1005 contains 4 sig. Figs., 23,000 has 2, 1,045,090 has 6
40.01 has 41.100 has 4 sig figs, 0.00540 has 3,
When multiplying or dividing measurements: round the answer to the same number of digits as the measurement having the fewest number of significant figures.
When adding or subtracting measurements: round the answer to the same number of decimal places as the measurement having the fewest number of decimal places.
Identify the LEAST PRECISE measurement. Identify the MOST PRECISE digit (place) within
that measurement. Round the answer to this digit (place).
123456.7890
Higher precision
Lower precision
Scientific Notation 10000000000000000000000 0.00000000000000000000000000001
There has to be a better way to write those numbers Rules for scientific notation
1) Write only the sig figs. Express the number starting with the one’s place followed by any decimal digits, times a power of 10.
2)To express a large number, count the number of decimal places needed to move to the one’s place, and make that number the exponent of ten.
3) To express a very small number, count the number of decimal places needed to move to the one’s place, and make that number the NEGATIVE exponent of ten.
4) You can always check it by writing out the expanded ten, and multiply it by the measured number.
Scientific Notation
Examples:0.0000000000000000000000000000000010
= 1.0 x 10-35
94140000000000000000000000000000000
= 9.414 x 1035