Draw the Classroom and Label All Safety Equipment. List Some Safety Rules

Name ______

Hour______

Ch 1 Scientific Method

Draw the classroom and label all safety equipment. List some safety rules.

MSDS Worksheet

Notes:

*Match the following Hazard Code title with its corresponding color:

1) Health Hazard A) Red

______2) Flammability Hazard B) Yellow

3) Stability or Reactivity Hazard C) Blue

______4) Special Information D) White

5) Which number on the Hazard Coding System is the most serious?

least serious?

6) Draw the Hazard Code symbol for a radioactive substance:

7) Draw the Hazard Code symbol for a substance that is highly reactive with water: *Look at the attached MSDS and answer the following questions:

8) What does MSDS stand for?

9) What is the name of this chemical?

10) Give the formula for this chemical:

11) What is the melting point of this chemical?

12) What does this chemical look like?

13) How do you extinguish a fire of this chemical?

14) What first aid should you do if someone swallows (ingests) some of this chemical?

15) What materials should you avoid with this chemical?

16) What special precautions should be used when storing this chemical?

Identify the following lab equipment:

Practice online at http://www.sciencegeek.net/Chemistry/taters/labequipment.htm

Notes:

Chemistry Lab #1-2

Laboratory Techniques

Procedure:

1. Bunsen Burner:

Obtain and connect a Bunsen burner to a gas jet.

- Light a match, turn on the gas, and raise the match until the burner is lit (in this order).

- Experiment with the flame by adjusting the amount of air entering the burner (the smaller the flame, the less air is needed). If there is too much air, the flame can “strike back” where gas may burn at the base of the burner. When this happens, turn off the gas, reduce the air intake, and relight the burner.

Reduce the air flow until you have a yellow flame.

- Hold an evaporating dish with forceps in the tip of the flame and record your observations.

- Adjust the gas to a flame of ~8 cm above the barrel.

- Adjust the air intake until you have a quiet, steady flame with a sharply defined inner cone.

- Use forceps to insert a piece of copper wire into the hottest part of the flame. Hold for a few seconds and observe whether the flame will melt the copper wire.

2. Measuring liquids:

When measuring liquids, always record the level at the bottom of the meniscus (curve of water – see figure to the right)
Measure approximately 40 mL of water into a 100 mL beaker.
Pour the water into a 100 mL graduated cylinder. Read the volume to the nearest 0.5mL and record on your data sheet.
Repeat using a 150mL beaker for your initial measurement

3. Massing solids:

NEVER touch laboratory chemicals with your hands (some chemicals readily pass through the skin barrier into the bloodstream and can cause serious health problems).

DO NOT PLACE YOUR HAND OR HEAVY OBJECTS ON THE PAN OF THE BALANCE. It is very easy to destroy the precision of the balance.

Obtain sand, a test tube, weighing boat, and chemical scoop. Bring to an electronic balance.
Zero the balance by pressing the “tare” or “rezero” button. Place the weighing boat on the balance and zero the balance again (this will subtract the mass of the weigh boat).
Use a chemical scoop to place between 3.5 – 3.7 grams of sand into the weighing boat. Record this mass in the data table. By bending the boat, form a trough and transfer the sand to the test tube.
Transfer the sand from the test tube back to the weighing boat and check the mass again. Record this mass as the second weighing of sand. Pour the sand back into the plastic bottle.

4. Filtration:

Add ~10mL of solution A (CaCl2) to a 100 mL beaker. Add ~10mL of solution B (Na2CO3) to the beaker and observe the formation of a solid in the container.
Support a funnel on a clay triangle with the step of the funnel just touching the inside wall of the beaker. Fold a circular piece of filter paper (as demonstrated by your instructor) and place the filter paper in the funnel. Wet the paper to hold it in place.
Pour the solution along a stirring rod to transfer the liquid and solid from the beaker to the filter. Do not overfill the filter and stir the solution to make transfer easier. Use a small amount of distilled water from your wash bottle to wash the remaining solid from the bottom of the beaker. If the liquid from the stem of the filter is clear, it has been properly filtered. Discard as indicated by your instructor.

Data:

1. Bunsen Burner

Observations:

What may cause the burner to “strike back”?

Use your observations during the operation of the Bunsen burner to support your answers of the following:
Is the burner hot enough to melt the copper?

A yellow flame is less desirable than a blue flame.

2. Measuring liquids

Observations:

Volume of water in:

40 mL from the 100 mL beaker measured by the graduated cylinder / 40 mL from the 150 mL beaker measured by the graduated cylinder

Why is a beaker not used to make volume measurements in chemistry?

Why is using a beaker for measurement a source of experimental error?

Why is the graduated cylinder most accurate at measuring volumes?

3. Massing Solids: Observations:

First mass of sand ______

Second mass of sand______

How are errors made in the transfer of chemicals?

4. Filtration

Observations:

Does filtration remove all the white substances from the water?
How do you know?

Section 1.2 Chemistry and Matter

In your textbook, read about chemistry and matter.

Notes:

Define each term:

1. Chemistry

______

2. Matter

______

3. Mass

______

Write each term below under the correct heading. Use each term only once.

Air / Magnetic field / Car / Feeling / Heat / Human body
Light / Radio / Radio wave / Flashlight / Textbook / Thought

Made of matter

4. ______

5. ______

6. ______

7. ______

8. ______

9. ______

Not made of matter

10. ______

11. ______

12. ______

13. ______

14. ______

15. ______

For each statement below, write true or false.

16. ______The mass of an object can vary with the object’s location.

17. ______A mass measurement includes the effect of the Earth’s gravitational pull on the object being measured.

18. ______Scientists measure the amount of matter in terms of mass.

19. ______Subtle differences in weight exist at different locations on Earth.

20. ______Your mass on the Moon would be smaller than your mass on Earth.

Understanding Main Ideas (Part A)

Circle the letter of the choice that best completes the statement or answers the question.

1. Which of the following is NOT matter?

a. Atoms b. ultraviolet radiation c. air d. the Sun

2. At the end of an experiment, the scientist forms a conclusion based on the

a. Variable b. scientific law c. data obtained d. control

3. Which of the following is a set of controlled observations that tests a hypothesis?

a. Mass b. experiment c. weight d. constant

4. The branch of chemistry that focuses on carbon-containing chemicals is called

a. Analytical chemistry c. biochemistry

b. Inorganic chemistry d. organic chemistry

5. How should you prepare an acid solution?

a. Add the water to the acid all at once c. add the water to the acid very slowly

b. Add the acid to the water all at once d. add the acid to the water very slowly

Understanding Main Ideas (Part B)

Qualitative and Quantitative measurements:

Notes:

Identify each piece of data as either qualitative or quantitative.

______1. Red

______2. 100 pounds

______3. 105°C

______4. Tall

______5. Round

______6. Smells like bananas

______7. 40 mph

______8. Pink with polka dots

______9. Cold

______10. 78 books

Lab: Six White Powders

Purpose: To identify an unknown substance

Materials:

Safety goggles

Acetate sheet

7 craft sticks

3 pipets

Solutions:

Water

Vinegar

Iodine solution

White powders:

Chalk

Powdered sugar

Talcum powder

Baking powder

Baking soda

Cornstarch

Unknown

Procedure:

1. Place a clear sheet of acetate over the lab grid provided.

2. Using a separate craft stick for each, place a small amount of the white powders indicated in the appropriate area on the acetate sheet.

3. Place 3 drops of the appropriate solutions on each of the white powders as indicated by the lab grid, carefully recording all observations after each addition in the data table below.

Data:

WATER / VINEGAR / IODINE
CHALK
POWDERED SUGAR
TALCUM POWDER
BAKING POWDER
BAKING SODA
CORNSTARCH
UNKNOWN POWDER

Conclusion:

Based on the information gained in this lab, what was the identity of the unknown white powder at your station?

Unknown ______

Lab station _____

What clues helped you identify the unknow? Please list 4 clues:

4.
Paper Dragon Experiment

Supplies:

A ruler

A piece of wide lined notebook paper A marble

A bent strip of tag board

Masking tape

Set up:

Make a ramp with the ruler by propping one end on a book.

Place the lined paper on the table in front of the ramp with the lines perpendicular to the ruler. Place the bent strip on its side directly in front of the ramp so that the point of the "V" is facing away from the end of the ruler.

Problem:

You must be able to predict where the paper "V" will stop on the notebook paper after it is pushed by a marble that has rolled down the ramp starting from any point on the ramp.

To do this, you must:

1. decide what controls you need in order to make an accurate prediction.

2. identify the independent and dependent variables.

3. set up a system that will allow you to predict what space on the notebook paper the "V" will stop if the ball starts from any point on the ruler.

Test:

When you are ready, the teacher will place the ball at a point on the ruler and ask you to predict which line on the paper the "V" will stop after it is pushed by the marble. if you have controlled variables, the "V" should stop where you predicted at least 3 times out of 5,

Questions:

1. Variables are things that can change during an experiment. If there is more than one thing being changed, the results will be inconsistent. What variables would you control in this experiment to help improve your results and make them more consistent? List at least three:

2. The independent variable in an experiment is the value that you change on purpose. In this experiment, what is the independent variable?

3. The dependent variable is the data that changes as a result of you changing the independent variable amount. What is the dependent variable?

4. When graphing the results of an experiment, the independent variable always goes on the X axis, the dependent on the Y axis. Make a graph of your results, connecting the data points with a smooth curve. .

5. If you place the marble at exactly 5cm on the ruler and release it, shouldn't it always stop the paper at the same place? What does this tell you about how a scientist must approach any experiment? Is it important that scientists be able to reproduce their results? Write a short paragraph explaining what you have learned:

Chemistry Lab #1-1 The Scientific Method

Introduction:

Chemistry is a basic science which deals with matter and energy relationships, the composition of matter, and the changes matter undergoes. One factor that distinguishes chemistry as a science is the use of scientific methods to solve problems. Scientific methods are organized, systematic ways to determine answers through experimentation. In using methods to solve a problem, observation, investigation, analysis, and interpretation are most important.

As chemists, we investigate the properties and changes of matter using our senses and devices available in the laboratory. We observe carefully during these investigations and record all findings. These observations are then analyzed using such tools as organized data tables, graphs, and mathematical equations. These interpretations or conclusions can be used to formulate theories.

Purpose:

To observe a burning candle as conditions are changed. To test the behavior of the candle under a variety of conditions. To determine the products formed by a burning candle using a series of tests and observations.

Procedure:

A. Mass Change During Candle Combustion

1. Place a candle on a can lid. Measure the mass of the candle and lid using a laboratory balance. Record the mass in the data table.

2. After completing parts B and C, measure the mass of the candle and lid again.

B. The Behavior of a Candle Flame Under Various Conditions

1. Light the candle (CAUTION: Long hair or loose clothing can swing into the candle flame.) Invert a large beaker over the burning candle. Record the time needed to extinguish the flame. Repeat with a larger or smaller beaker.

2. Lower a piece of coiled copper wire around the candle flame. Record your observations.

C. Determination of Products Formed as a Candle Burns

1. Place a drop of water on a piece of cobalt chloride test paper. It will turn pink in the presence of water.

2. While the candle is burning, invert a large beaker over the flame for a few seconds. Test any liquid formed in the beaker with cobalt chloride test paper. Record.

3. Examine the bottom of the beaker used in steps 1 and 2 of part B for any charred deposits. Record observations.

4. CAUTION: Limewater causes burns; avoid skin and eye contact.) Invert a 250 cm Erlenmeyer flask over a burning candle until the flame is extinguished. Quickly invert the flask to an upright position. Add 20 ml of limewater, stopper the flask, and shake the solution. Watch for changes in the solution. Carbon dioxide gas causes limewater to turn cloudy.

5. Obtain a test tube, test tube holder, and thermometer. Half fill the test tube with tap water. Check the temperature of the water and record. Using the test tube holder, hold the test tube just above the candle flame for one minute. Record the new temperature of the water in the test tube.