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of the LiCl 2 Make sure your balance is left in the same condition as you found it 3 Be careful that your burner and clamp are cooled before putting them away 4 Carefully return all laboratory equipment to the proper place and dispose of all waste in the designated containers
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and heat it with a low flame until the NaCl melts, or for 2 minutes, whichever comes first If the salt melts within the 2-minute period, record the melting point as low If the salt does not melt within 2 minutes, record the melting point as high 3 In the fume hood, and using the same apparatus shown in Figure A, repeat step 2 for sugar (Note: Like most compounds in living organisms, sugar is nonionic) Make sure the flame is the same setting as your burner in step 2
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LAB 81
LABORATORY MANUAL
Data and Observations
Part A: Crystal Lattice
Observations about the coarse and fine NaCl Observations about the pieces of NaCl after breaking the coarse salt
Part B: Melting Point
Observations about the melting point of NaCl (high or low melting point) Observations about the melting of sugar (high or low melting point)
Part C: Conductivity
Test Substance Solid NaCl Distilled water
Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
Conductivity Indicator (Record light as off, dull, bright, or blinking)
Conductor Rating (good, poor, or none)
NaCl dissolved in distilled water Sugar dissolved in distilled water Solid LiCl Molten LiCl
1 From the results of Part A, and using words like soft, ductile, malleable, brittle, hard, or
pliable, how would you describe sodium chloride
2 Sodium chloride and lithium chloride are typical ionic compounds, while sugar represents
a typical nonionic compound In general, how do these two types of compounds compare in their melting points
3 In Part C, why was it important to use distilled water instead of tap water for the
conductivity measure
Laboratory Manual
Chemistry: Matter and Change 8
Name
Date
Class
LAB 81
LABORATORY MANUAL
Analyze and Conclude
1 Recognizing Cause and Effect In a crystal lattice structure, the electrons are held
tightly by the ions, which are rigidly held in place by electrostatic attraction Discuss how this characteristic explains why ionic compounds generally (a) have high melting points and (b) do not conduct electricity in the solid state
2 Comparing and Contrasting Nonionic compounds do not exist in crystal lattice struc-
tures but rather as individual particles, which are affected by other particles In other words, nonionic compounds experience forces between particles Based on what you learned in Part B about the melting points of ionic versus nonionic compounds, how do you think the attractive energy between particles compares with the energy of the crystal lattice
3 Thinking Critically Explain how ionic compounds, which do not conduct electricity in
the solid form, can conduct electricity when they are in the molten state or dissolved in water
4 Drawing a Conclusion All ionic compounds exist in only one state at room temperature
From what you learned in this investigation, what is that state and why do you think they do not exist in the other states at room temperature
5 Error Analysis What could be done to improve the precision and accuracy of your
investigation
Real-World Chemistry
1 The human body is mainly composed of non-
ionic compounds, such as water, carbohydrates, lipids, and proteins Why then are people such good conductors of electricity 2 Magnesium carbonate, an ionic compound, is sometimes used as a thermal insulator in
buildings Why would you expect ionic compounds to be good thermal insulators 3 Ionic compounds often have higher melting points than metals Using at least two properties of ionic compounds, explain why cookware is not made from ionic compounds
Chemistry: Matter and Change 8
Laboratory Manual
Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
Name
Date
Class
LABORATORY MANUAL
Use with Section 82
Formation of a Salt
lease pass the sodium chloride! It is amazing that food is seasoned with an ionic compound that is composed of two deadly elements sodium and chlorine The gain or loss of electrons can make a big difference in properties Reacting sodium hydrogen carbonate, which is baking soda, with hydrochloric acid (HCl), the acid found in your stomach, produces salt, carbon dioxide, and water, according to the following equation:
NaHCO3(cr) HCl(aq) 0 NaCl(cr) CO2(g) H2O(l)
If we evaporate the water, then all that should remain is the salt, NaCl
Problem
How can we form a salt
Objectives
Observe the reaction of NaHCO3 with HCl Draw the Lewis electrondot diagrams for Na and Cl Give examples of how to identify an ionic compound such as NaCl
Materials
6M HCl NaHCO3 100-mL beaker 10-mL graduated cylinder dropper phenol red indicator distilled water Bunsen burner ring stand ring clamp wire gauze microscope or hand lens balance
Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
Safety Precautions
Always wear safety goggles and a lab apron Hot objects will not appear to be hot Be careful when handling the cooling beaker Do not touch or taste any chemicals used or formed in the laboratory 6M HCl is toxic by ingestion or inhalation and corrosive to the skin and eyes
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