1. UNIT ONE: INTRODUCTION TO CHEMISTRY

2. Chemistry – the science that investigates and explains the structure and properties of matter 
Remember that EVERYTHING is made of matter – matter is anything that has mass and takes up space (volume)
- What is the difference b/n mass and weight?
- mass is the amt of matter in an object
- weight is the pull of gravity on an objects mass.
We will be studying many different properties of many different types of matter
- examples of properties: color, density, chemical reactivity, composition, state of matter - (solid, liquid or gas), flammability

3. Lab write up procedures
Title
Purpose: Should state why you are doing the lab and any hypotheses you have for the concept being tested.
Safety
Materials: See handouts
Procedure: See handouts
Data: Prepare a data table to record the required data as described in the procedure.
Calculations: Show any work done for the lab.
Conclusions: Using Strong Answer Format, use your data to explain if your hypothesis is supported or not.

4. What is Strong Answer Format and how do I use it?
SAF is how you should answer all questions that require support, data, or evidence.
Claim - What are you claiming? What are you trying to prove?
Data - Include data from the text to support, or prove, your claim. This should be in the form of a quote (with a citation) or specific examples from the text. If it is not a text-based question, then you must use data from your own readings, observations, or personal experiences.
Warrant - Connect the data to the claim. How does your data prove/support your claim? Elaborate as needed.
Conclusion - Make a concluding statement to bring your answer to an end.

5. MASS AND CHANGE

6. Mass and Change lab
The lab groups should report their results for each procedure on the overhead so that the entire class data can be recorded. Change should be recorded as + (for a gain) or – (for a loss).  
Station 1:
Part 1 – Mass of steel wool
Apparatus : Balance, Small wad of steel wool (~ 1/4 of a pad of #1 steel wool)
Hypothesis: Predict whether the mass will change if the wad of steel wool is pulled apart.
Procedure: Determine the mass of the wad of steel wool. Record.
Carefully pull the wad apart so that it occupies a volume roughly twice as great as before.
Determine the mass of the expanded wad of steel wool. Record.
Record any observations of the steel wool during the procedure.

7. Mass and Change (slide 2)
Station 2
Part 2 – Mass of ice and water
Apparatus : Balance, small vial and chip of ice
Hypothesis: What happens to the mass of the container when the ice melts?
Procedure: Find the mass of the vial + a small piece of ice. Record.
Warm the vial in your hands to melt the ice.
Determine mass when ice is melted. Record.

8. MASS AND CHANGE (slide 3)
Station 3
Part 3 – Mass of a precipitate
Apparatus : Balance, two small test tubes, 0.1M solutions of Ca(NO3)2 and Na2CO3
Hypothesis: Does the mass change when the solid is formed?
Procedure: Find the mass of both tubes together. Record.
Carefully pour the contents of one tube, into the other, then put both tubes and caps back on the balance pan and mass. Record.
Leave tubes in the test tube rack. Be careful, if solution is spilled , the mass will appear to decrease.

9. MASS AND CHANGE (slide 4)
Station 4
Part 4 – Mass of burning steel wool
Apparatus: Balance, Bunsen burner, Small tuft of steel wool, Crucible tongs, aluminum foil
Hypothesis: Predict what will happen to the mass of the steel wool when it is heated.
Procedure: Find the mass of the steel wool left over from Part Record.
Roll it into a tight ball. Light the burner, place the foil under the burner, then holding the steel wool by the tongs over the flame, heat the steel wool until it glows. Turn the steel wool around in the flame so that all sides are exposed. Heat for a minimum of 4 minutes.
Any pieces of the steel wool that break free during heating should fall into the dish and then be transferred to the balance pan.
Allow the ball to cool and determine the mass. Record.
Record how the appearance of the steel wool changes when it is heated strongly. Pay close attention.

10. MASS AND CHANGE (SLIDE 5)
Station 5
Part 5 – Mass of dissolved sugar
Apparatus: Balance, Vial with cap, Sugar
Hypothesis: Predict what will happen to the mass when sugar dissolves in water.
Procedure: Fill a vial about 1/2 full of water, then put about a 1/4 tsp of sugar in the cap of the vial.
Place the vial, water, cap and sugar on the pan of the balance. Record the mass.
Carefully pour the sugar into the vial, taking care not to spill any.
Gently swirl the vial to get the sugar to dissolve. If you shake too vigorously, you risk solution leaking out of the vial.
When the sugar has completely dissolved, find the mass of the vial and contents again. Record.

11. MASS AND CHANGE (slide 8)
Station 6
Part 6 – Mass of dissolved Alka-Seltzer
Apparatus : Balance, Vial with cap, ~1/4 tablet of Alka-Seltzer
Hypothesis: What will happen to the mass of a solution containing a dissolved Alka-Seltzer tablet?
Procedure: Fill a vial about 1/2 full of water, then put about the 1/4 tablet of Alka-Seltzer in the cap of the vial.
Place the vial, water, cap and tablet on the pan of the balance. Record the mass.
Put the Alka-seltzer into the vial, and loosely cap the vial.
Observe what occurs when the tablet appears to dissolve.
When the piece of tablet has completely dissolved, find the mass of the vial and contents again. Record.

12. MASS AND CHANGE: CONCLUSIONS
Using Strong Answer Format explain any loss/gain in mass for each procedure. Account for any possible errors that may have occurred in each procedure.
Remember to reference your data to support your answers!!

13. ATOMIC THEORY
We will be studying some properties directly and others we will use models to represent a property that is difficult to see or hazardous
- a scientific model is a thinking device that helps us to understand and explain something
Remember, everything is made up of matter - early scientists thought matter was composed of 4 fundamental elements – air, earth, fire and water
smallest particle of matter is the atom
the idea of an atom was first proposed by a Greek named Democritus ( BC) – said matter was made up of empty space and small indivisible particles called atoms Atomic Theory
unfortunately his theory was ignored for almost 2000 years
Your project will explain the journey made from Democritus to our present model of the atom

14. early scientists did not test their theories – later scientists tested hypotheses in a very rigid manner using the scientific method
- Scientific Method:
Define the problem
State a hypothesis – a hypothesis is an educated guess
Experiment to test the hypothesis
Make and record observations
Draw conclusions
- if conclusions support hypothesis repeat experiments to give evidence to the hypothesis
- if the conclusions DO NOT support hypothesis, hypothesis changed and steps 3-5 are repeated
If multiple experiments show support to a hypothesis it may become a theory – a theory is NOT a fact – over time, if further evidence is found in support of the theory it may become a law and be accepted as fact – BOTH a theory and a law may be changed if evidence is found to do so

15. DATA ANALYSIS: THE METRIC SYSTEM
universal system of scientific measurement – allows all scientists to understand measurements made by other scientists regardless of language - based on units of ten – each unit is 10X larger or 10X smaller
BASIC UNITS
Length – unit = meter (m) – 1m = 39.4 inches – we will usually measure things in centimeters or millimeters
Volume – amount of space an object takes up – unit = liter (L) – we will usually use milliliters in lab – the volume of a solid can also be measured in a unit called cubic centimeters (cm3) which are also equal to ml – L = dm3
Mass – the amount of matter in an object – unit = kilogram (kg) – we will usually use grams (g) or milligrams (mg) in lab

16. Density – the amount of matter in a unit of space – the mass per unit volume of a substance – because the units do NOT cancel out you have a derived unit
  Density = mass D = M
volume V
Temperature – measured on the Celsius scale – water freezes at 0oC and boils at 100oC
in chemistry we will use the Kelvin scale for calculations
  oC = K
K – 273 = oC
  - absolute zero – 0 K = -273oC – temperature at which all molecular
motion stops – has NOT been reached so is still a theory –WHY???
Dimensional analysis – conversion from one unit of measure to another – requires a conversion factor linking the 2 units you are converting between

17. ACCURACY AND PRECISION
- accuracy – how close a measured value is to the accepted value.
- precision – how close a set of measurements is to each other
when analyzing data it is important to be able to determine the percent error:
actual value – experimental value x 100 = % error
actual value
 CHEMISTRY PRACTICE PROBLEMS
An object has a mass of 57.7 g and occupies a volume of cm3. Calculate its density.
A sample of a substance with a density of 4.19 g/cm3 occupies 0.11 cm3. What is the mass of this sample? 
What is the volume of a 29.6 g sample of a metal that is known to have a density of 5.15 g/cm3? 

18. MATTER
Because everything in the universe is made up of matter, classification is essential
- composition – broadest means of classification – is qualitative (no measurement) or quantitative (measurement) – may also be classified as a pure substance (element or a compound (cmpd)) or a mixture physical combo of differing amts of different subs) - most matter is mixtures – remember each subs maintain own properties
mixtures can be separated into individual subs through a physical change (the identity of the subs DO NOT change) ex: boiling, freezing, melting, dissolving, etc.
 when mixtures are separated they form pure subs
2 types of pure subs:
elements – cannot be broken down into simpler subs – building blocks for ALL matter – scientists have identified 111 so far, 90 occur naturally the others have be made in a lab during nuclear experiments - elements are listed on the periodic table – each element has its own symbol – the symbol may be one capital letter or two letters with the first capital and the second lowercase
- You will learn many of these elements – You must be able to give the symbol and spell the name correctly

19. cmpds – can be broken down into simpler subs but only through chemical means – chem combo of 2 or more elements in a fixed proportion – this gives a cmpd unique chem and physical properties (diff from elements in them) – cmpds represented by formulas that show the ratio of atoms of elements in the cmpd
 PROPERTIES AND CHANGES OF MATTER
2 types of properties:
physical properties – don’t involve changes in composition – ex: color, boiling point, freezing point, density
chemical properties – can only be observed when there is a change in the composition of the subs – describe the ability of a sub to react with other subs – ex: reactivity, tendency to breakdown, flammability

20.  STATES OF MATTER
4 states of matter:
solid – has a definite shape and volume
liquid – has a definite volume but not a definite shape – shape is determined by its container
gas – no definite shape or volume – both are determined by its container
plasma – high energy sub – not very common
TYPES OF MIXTURES
2 main types of mixtures:
heterogeneous – made up of different compositions depending on where you look – ex: salad dressing, soil, orange juice – different areas are called phases
homogeneous – composition is the same throughout the sub – ex: salt water, tea – also called a solution (sol’n) – may be made up of any combination of any of the states of matter – REMEMBER water is NOT always the solvent

21. SEPARATING MIXTURES
- since mixtures are physically combined they can be separated using physical means based on their physical properties
- types-
1) filtration – uses a porous barrier to separate a solid from a liquid
2) distillation – based on differences in the boiling points of the substances involved – a mixture is heated until the subs w/the lowest bp changes to a vapor that can then be condensed and collected.
3) crystallization – formation of pure solids of a subs from a sol’n containing the dissolved subs – produces highly pure subs
4) chromatography – separates parts of a mixture based on the tendency of each to be drawn across the surface of another material