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I Want to Be Like You-oo-oo!!
Oh, oobee-doo
I wanna be like you-u-u
I wanna walk like you
Talk like you, to-oo-oo-oo
You'll see it's true
An element like me-e-e
Can learn to be a gas….like you toooo-oo
(badly modified from Disney’s ‘Jungle
Book’)
https://www.youtube.com/watch?v=9JDzlhW3XTM

Group IA metals (alkali metals)
1.1. Write the electron Configurations for the following elements:
Alkali metals
Li:
Na:
K:
Rb:
Cs:
Fr:
Noble Gases
He:
Ne:
Ar:
Kr:
Xe:
Rn:
1.2. Procedure: Go to the Open Learn Science website and make observations of the physical
and chemical changes that occur during the demonstration
http://www.open.edu/openlearn/science-maths-technology/science/chemistry/alkali-metals
1.3. Observations:
1.4. Reaction Equations:
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1.5. Based upon your review of the above website, what do you observe is the order of
reactivity for each of the alkali metals?
1.6. What do you think might account for those differences-It’s an atom ‘thing’?

Group IIA Metals (Alkaline Earth Metals)
pH and Conductivity
Preparation: Alkaline earth metal chlorides Testing Solutions:
A 50 ml solution of 0.1 M, Magnesium hydroxide solution Mg(OH)2
A 50 ml solution of 0.1 M, Calcium hydroxide solution Ca(OH)2
100 ml graduated cylinder
100 ml beakers
Measuring solutions
Transfer and test with pH and conductivity probes
2.1. Before you conduct the next investigation, think about your first set of observation. Based
upon what you observed, what do you hypothesize will be the differences between the pH
and conductivity of IIA hydroxide solutions?
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2.2.Test the pH and conductivity of each solution using the Vernier pH and conductivity probes
pH
Conductivity
Mg(OH)2 _______________________
_______________________
Ca(OH) ________________________
_______________________
2.3.How would you compare your results to what you predicted about the pH and conductivity
of IIA metal solutions?
2.4.What do you think might account for those differences?

Solubility
Preparation: Alkaline earth metal chlorides Testing Solutions:
a.
b.
c.
d.
e.
f.
g.
h.
Barium chloride solution, 0.1 M, BaCl2,
Ammonium oxalate solution, 0.25 M, (NH4)2C2O4
Calcium chloride solution, 0.1 M, CaCl2
Potassium iodate solution, 0.2 M, KIO3
Magnesium chloride solution, 0.1 M, MgCl2
Sodium carbonate solution, 1 M, Na2CO3
Strontium chloride solution, 0.1 M, SrCl2
Sodium sulfate solution, 1 M, Na2SO4
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8 disposable pipets
1 testing plate
i.
Fill each pipet with the soln’s, invert pipet and store in a beaker
Follow steps i and ii, look for the production of a precipitate
Add several (approximately 5) drops of an alkaline earth metal chloride solution to
each well in a horizontal row, as follows (see Figure 1):
• magnesium chloride to wells A1–A5
• calcium chloride to wells B1–B5
• strontium chloride to wells C1–C5
• barium chloride to wells D1–D5
ii.
Add several drops of testing solution to each well in a vertical column, as follows
(see Figure 1):
• potassium iodate to wells A1–D1
• sodium sulfate to wells A2–D2
• ammonium oxalate to wells A3–D3
• sodium carbonate to wells A4–D4
iii.
Record results on the following table. If a solid appears, record as ‘ppt’ in the circle.
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3.1. Based upon your observations, where the any patterns that emerged between the elements.
3.2. What do you think might account for those differences?

Group VIIA Nonmetals (The halogens):
4.1.First, compare the visible physical properties of the three elements Cl2, Br2, and I2, which
are displayed in bottles on the side shelf. Be sure to notice the colored vapors above the
liquid and solid.
Element
Physical State
Color
Cl2
________________
________________
Br2
________________
________________
I2
__________________
__________________
4.2.Which of these three elements is most volatile (most easily vaporized)? ___________
4.3. How does the volatility of the elements vary with the atomic mass of the Cl2, Br2, and I2
molecules?
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4.4.In 50 ml beakers, measure the conductivity of the aqueous solutions of the 0.1 M sodium
halides using the conductivity probe (use the 0-20,000 toggle setting).
Solution
Conductivity
20 ml. NaCl(aq)
__________________
20ml NaBr(aq)
__________________
20 ml. NaI(aq)
__________________
5.2. Based upon your observations, where there any patterns that emerged between the VIIA
elements.
5.3. What do you think might account for those differences?

Solubility
5.1. Preparation of Solutions:
a. Chlorine Water: To prepare 100 mL of chlorine water, mix 13 mL of 5% sodium
hypochlorite solution (bleach) with 30 mL of 1 M hydrochloric acid. Dilute to 100
mL with distilled water and stir to mix. Store in a labeled glass bottle or stoppered
flask until needed. Work with chlorine water in the hood.
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b. Bromine Water: To prepare 100 mL of bromine water, mix 30 mL of 1 M sodium
bromide solution with 30 mL of 1 M hydrochloric acid. Add 15 mL of 5% sodium
hypochlorite solution (bleach) followed by 25 mL of distilled water and stir well to
mix. Store in a labeled glass bottle or stoppered flask until needed. Work with
bromine water in the hood.
c. Iodine Solution: _______________________________
5.1. Procedure
I.
Label six square glass bottles 1–6
II.
Using a graduated cylinder, measure and add 5 mL of chlorine water to each bottle 1 and
2. Cap the bottles.
III.
Draw a line to mark the level of liquid in bottles 1 and 2, and mark off a line at the same
height in each bottle 3–6.
IV.
Add bromine water to the 5-mL line in each bottle 3 and 4.
V.
Add iodine solution to the 5-mL line in each bottle 5 and 6.
VI.
Record the color of each aqueous halogen solution in Data Table A.
VII.
Using a clean graduated cylinder, measure and add approximately 10 mL of hexane to each
test tube 1–6.
VIII.
Place a stopper in each test tube and carefully invert each tube several times to mix the
liquids. There should be two layers—the top organic layer (hexane), and the bottom
aqueous layer (water).
IX.
For each aqueous halogen/hexane mixture, record the colors of the upper and lower liquid
layers in Data Table A.
X.
Add 5 mL of sodium bromide solution to the chlorine mixture in bottle 1. Cap the bottle
and carefully invert several times to mix the liquids. Observe any reaction that occurs—
look for changes in color to either layer. Record all observations in Data Table B. If no
change is apparent, write no reaction (NR) in the data table.
XI.
Using the information in the following chart, repeat step 10 for all of the possible halogen–
sodium halide combinations in bottles 2–6.
XII.
Record detailed observations as each solution is added. Complete Data Table B.
Test Tube
1
2
3
4
5
6
Halogen
Cl2
Cl2
Br2
Br2
I2
I2
Sodium Halide Solution
NaBr NaI NaCl NaI NaCl NaBr
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5.2. Based upon your observations, where there any patterns that emerged between the VIIA
elements.
5.3. What do you think might account for those differences?