1. Unit 1
Matter and Measure

2. Measure

3. Scientific Measurement
Two main systems
English
Based on arbitrary measurements that have lasted through history
Conversions are harder to remember
Metric
Based on powers of ten
Prefixes determine magnitude of power of ten

4. International System (SI)
Scientific Community has accepted certain units as base units
Dimension
Unit
Symbol
Length
Meter m
Mass
Gram g
Time
Second s
Temperature
Kelvin K
Amount
Mole
mol

5. Metric System Prefixes
Power
Symbol
Giga
109 G
Mega
106 M
kilo
103 k
deci
10-1 d
centi
10-2 c
milli
10-3 m
micro
10-6 μ
nano
10-9 n
pico
10-12 p

6. Measuring Digital Displays are recorded as is
Digital Mass Balance, pH meter
Visually Read Scales can always be estimated to smaller increment than marked
Rulers, Thermometers, Graduated Cylinders
Meter stick Example

7. Example
Length=??
0.3m 0.31m 0.314m 0m
0.1m
0.2m
0.3m
0.4m

8. Significant Figures (sigfigs)
Not all digits(#’s) in a measurement are significant(important)
Suppose the mass of an object is estimated to be 2.5 grams
The volume of that object is measured accurately to cm3
How many decimal places should the density have? 4.0g/cm3 or g/cm3

9. Significant Figures (cont)
Rules on pages of textbook
Shorthand
If the decimal point is present, start counting digits from the Pacific (left) side, starting with the first non-zero digit. 
(3 sig. figs.)

10. Significant Figures (cont)
Shorthand
If the decimal point is absent, start counting digits from the Atlantic (right) side, starting with the first non-zero digit. 
31,400 (3 sig. figs.)

11. SigFigs for Math Addition and Subtraction Example
Answer has to have the same number of decimal places as least decimal places in what you are adding or subtracting
Example
= ???
Calculator  8.372
Science  8.37

12. SigFigs for Math Multiplication and Division Example
Answer has to have same number of Sigfigs as least number of Sigfigs in what you are multiplying or dividing
Example
7.55*0.34 = ???
Calculator  2.567
Science  2.6

13. Scientific Notation
Short hand way of writing very large and very small numbers
Uses only sigfigs
Examples:
602,000,000,000,000,000,000,000
6.02 x 1023
5.67 x 10-10

14. Accuracy How close a measurement is to correct or accepted value
Bull's-eye on a dartboard
Poor Accuracy
Good Accuracy

15. Precision How close a measurement is to other measurements
Darts close to each other
Poor Precision
Poor Accuracy
Good Precision
Poor Accuracy
Good Precision
Good Accuracy

16. Percent Error

17. Temperature Measure related to the heat of an object
Measured in °Celsius or Kelvin(no degrees)
Conversion

18. Density Amount of matter in a given amount of space
Amount of mass in a given volume

20. Matter

21. Chemistry What is Chemistry? Branches
Study of matter and the changes it undergoes
Branches
Organic
Physical
Analytical
Biochemical
Inorganic

22. IUPAC International Union of Pure and Applied Chemistry
Group that names elements and compounds
Meets every few years

23. Matter Anything that has mass and takes up space, volume
Classified into two categories
Substances (Pure)
Mixtures

24. Atom Simplest form of matter Made up of Subatomic Particles
Different atoms have different properties

25. Pure Substances Element
simplest form of matter that has a unique set of properties.
arranged into a table, called the periodic table
Can’t be broken down by chemical means
denoted using chemical symbols, O, Cu, Fe
Symbols always have the first letter capitalized
If needed, any additional letters are not capitalized

26. Pure Substances (Cont)
Compounds
substance of two or more elements chemically combined in a fixed proportion
Ex. H2O, C6H12O6
Can be broken down by chemical means

27. Mixtures Physical blend of two or more substances Two Types:
Homogeneous
Heterogeneous

28. Mixtures (cont) Homogeneous Heterogeneous
Composition is uniform throughout
Examples: Air, Olive Oil, Stainless Steel
Solution is a homogeneous mixture
Aqueous Solution is something mixed in water
Heterogeneous
Composition is not uniform throughout
Examples: Salad Dressing, Chicken Noodle Soup

29. Separating Mixtures
Differences in physical properties can be used to separate mixtures
Filtration – Separates solids from liquids in heterogeneous mixtures
Distillation – Separates homogeneous liquid mixtures based on different boiling points

30. Separating Mixtures Evaporation – evaporate away liquid to leave solid
Chromatography – separation of substances based on polarity

31. Phases(States) of Matter
Solid
Definite shape and volume
Particles are packed tightly together in a regular geometric pattern
(s) used after chemical formulas
Cu(s)

32. Phases of Matter Liquid Definite volume, takes shape of container
Particles can slide past each other
(l) used after chemical formulas
H2O(l)

33. Phases of Matter Gas Takes shape and volume of container
Particles are spread very far apart
(g) used after chemical formulas
H2O(g)

34. Aqueous Solutions Dissolved in water (aq) used after chemical symbols
NaCl(aq)

35. Phase Changes Solid  Liquid Melting Liquid  Solid Freezing
Liquid  Gas Vaporization
Gas  Liquid Condensation
Solid  Gas Sublimation
Gas  Solid Deposition
Temperature does NOT change during a phase change

36. Identifying Substances
Physical Property
quality or condition of a substance that can be observed or measured without changing the substance’s composition
Ex: Color, shape, size, mass
Physical Change
some properties change, but the composition remains the same
Can be reversible or irreversible
Ex: melting, freezing, tearing

37. Identifying Substances (cont)
Chemical Change
change that produces matter with a different composition than the original matter
Ex. burning, rusting, decomposing, exploding, corroding
Chemical property
property that can only be observed by changing the composition of the substance.
Ex: Reactivity with acids, reactivity with oxygen

38. Physical or Chemical ? Boiling Point Physical Green color Physical
Shiny Physical
Conductivity Physical
Solubility Physical
Reacts with acid Chemical
Reacts with O2 Chemical

39. Describing Matter Extensive Properties Intensive Properties
property that depends on the amount of matter in a sample.
Ex: mass, weight, volume
Intensive Properties
property that depends on the type of matter in a sample, not the amount of matter
Ex: Density, hardness, viscosity

40. Energy Capacity to do work Ability to do something Types: Chemical
Electrical
Mechanical
Potential
Kinetic

41. Energy Exchanges Exothermic Endothermic
Process when energy is released or given off
Ex: Burning, freezing
Endothermic
Process when energy is absorbed or taken in
Ex: Melting

42. Scientific Method Observation Hypothesis Experiment
using five senses to make observations.
Hypothesis
proposed explanation for an observation.
Experiment
procedure used to test a hypothesis.

43. Scientific Method (cont)
Analyze Data
check to see if results support hypothesis.
Theory
well tested explanation for a broad set of observations.
Law
concise statement that summarizes the results of many observations and experiments.

44. Scientific Laws Law of Conservation of Mass
Mass can not be created or destroyed, only changed into different forms
Law of Conservation of Energy
Energy can not be created or destroyed, only changed into different forms