1. Chapter 1- Matter and Measurement
Chemistry
Chapter 1- Matter and Measurement

2. What is Chemistry?

3. Chemistry is the science concerned with the composition, structure, and properties of matter.

4. Matter
Physical material of the universe; it is anything that has mass and occupies space.
Classified by:
Physical State
Gas
Liquid
Solid
?????
Composition
Gas – no volume no shape large distance between molecules Ca CO3 container
Liquid -

5. Composition
Heterogeneous – visually distinctive parts - a mixture that is not uniform in composition, properties, and appearance throughout.
Homogeneous – mixtures that are uniform throughout.
Mixture (solution)- matter that is uniform throughout and can be separated.
Pure substance - matter that has distinct properties and composition that does not vary from sample to sample and can not be separated.
Element – simplest form of matter
Compound – composed of two or more elements

6. Can it be broken down into
Matter NO
YES
Uniform distribution?
Heterogeneous
Mixture
Homogenous
YES NO
Fixed composition
Pure substance
Solution/mixture
Can it be broken down into
Simpler substances? NO
YES
element
compound

7. Properties
Physical Properties – can be measured without changing the identity and composition of the substance.
Chemical Properties - describes the way a substance may change or react to form other substances.
Intensive Properties – not dependent on amount of substance and used for identification.
Extensive Properties – depend on amount of the substance.

8. Chemical/Physical Changes
Physical changes – changes in the physical appearance of a substance.
Chemical changes – changes in the substance such that it forms a new substance.
Formation of a light
Formation of a gas
Formation of a precipitate
Change in temperature
Permanent change in color

9. Scientific Notation
A method of expressing a number as a product of a number between 1 and 10 and the appropriate power of 10.
Ex in scientific notation is
9.4 x 103
in scientific notation is
9.43 x 10-5

10. Multiplication of Scientific Notation
Ex. (4.6 x 105) x ( 3.2 x 103)
Multiply the numbers
Add the exponents
Rewrite in correct notation
(4.6 x 3.2) x 10(5+3)
=14.72 x 108
=1.472 x 109

11. Division of Scientific Notation
Ex. (4.6 x 105) ÷ ( 3.2 x 103) =
Divide the numbers
Subtract the exponents
Rewrite in correct notation
(4.6 / 3.2) x 10(5-3) = x 102

12. Uncertainty in Measurements
Exact numbers – defined values
Conversion factors
Date
Time
Counting small number of objects
Inexact numbers – uncertainty in numbers
All measurements

13. Limits of Measurements
Precision- is a measure of how closely individual measurements agree with one another. Accuracy- refers to how closely individual measurements agree with the correct value. Significant figures –all numbers recorded in a measurement with all numbers certain plus 1 uncertain number (the last number)
Use graduated cylinders and beakers and have do
Have three bottles with the same volume

14. Precision vs. Accuracy

15. Rules for Significant Figures
The only numbers that can be non-significant are zeros.
Any zero at the beginning of a number is not significant. It serves only to locate the decimal.
Any zero on the right hand end of a number is only significant if followed by a decimal or on the end of a decimal number.
Any zero between numbers is significant.
Exact numbers are significant.

16. Example Mass of an eyelash is 0.000304 Length of a skid mark is 123.0
125 gram sample of chocolate chip cookies contains 10 grams of chocolate
The volume of soda remaining in a can after a spill is liters
A dose of antibiotic is cm3

17. Adding and Subtracting Numbers Scientifically
When you add or subtract numbers, you can have no more decimal places in the answer than the fewest decimal places in the numbers that are added or subtracted.
Ex. =
13.90 – = = =

18. Multiplying and Dividing
When multiplying or dividing. You can have no more significant figures in the answer than the fewest number of significant figures in any number used to multiply or divide.
Ex.
45.34 ÷ 17.1 =
(11.01)(34.2)/12.34=
(45.0)/(45.689)=

19. Units Measurements English system
SI units – International System of Units or Metric system
Measurement SI
Symbol
English
Length
meter m
yard
Volume
liter L
Gallon
gal
Mass
gram g
pound lb
Temp
Celsius °C
Fahrenheit °F
Time
second s

20. Prefixes for Metric Units
Symbol
Meaning
Multiply unit by…
Example meter
giga G
billion (109)
1,000,000,000 Gm
mega M
Million (106)
1,000,000 Mm
kilo K
Thousand (103)
1,000 Km
Base 1
meter
deci d
Tenth (10-1)
0.1 dm
centi c
Hundredth (10-2)
0.01 cm
milli m
Thousandth (10-3)
0.001 mm
micro μ
Millionth (10-6)
μ m
Mm = 1,000,000 meter
Km=1000 meters
dm=tenth=o,1 meters
cm=0.01 meters
mm= of a meter

21. Ex. 1 meter (m) = 1000 millimeters (mm) 1 meter (m) = 100 centimeters (cm) 1000 meters = 1 Kilometer (km) 1000 grams (g) = 1 kilogram (kg) 1 liter (l) = 1000 milliliters (ml) 1000 milliliters = 1 liter

22. Dimensional Analysis
Conversion Factors -ratio of equivalent measurements to convert from one unit to another. Ex. 1 meter = 100 centimeters 1 inch = 2.54 centimeters 1 gallon = 4 quarts 1 meter = yards

23. Using Dimensional Analysis
Problem- How many meters in 3.4 cm?
3.4 cm = ? m
Need a conversion factor between cm and m
3.4 cm x cf = ? m

24. Dimensional Analysis
Problem: inches equals how many centimeters?

25. Dimensional Analysis
Problem: How many seconds are in one day?
86400

26. Dimensional Analysis
Problem: Your car has a 5.00 liter engine. What is the size of this engine in cubic inches?

27. Temperatures
Temperature can be measured in °F, °C, and K K=the absolute or Kelvin scale Water freezes at 0°C, 32 °F, and 273 K Water boils at 100°C, 212 °F, and 373 K °C = 5/9 (°F ) °F = 9/5 (°C) K = °C + 273

28. Temperature
What is 65.3 °F in °C? What is 56 °C in K?

29. Density
Which is heavier a pound of lead or a pound of feathers? Weight = mass = pounds Density = mass/volume So one needs larger volume of feathers to make a pound than lead.
Do a presentation with different liquids/ talk about Bermuda triangle

30. Density
The amount of matter in a given volume of a substance.

31. Density
What is the density of a metal rod that weighs grams and has a volume of 34 ml?

32. Density
What is the density of a metal medallion that weighs 13 grams? How do you find volume?

33. Water Displacement Method
Used to determine the volume of an irregular shaped object.

34. Density
What is the volume of a metal medallion with a density of g/ml that weighs 2.5 g ?

35. Select an equation to solve for a different unknown.
d = m/v
Solve for density
m = dv
Solve for mass
v = m/d
Solve for volume

36. Density
A block of metal is 3.45 cm by 2.78 cm by 7.98 cm. If this block of metal weighs g, what is the density of the metal?