Write a balanced chemical equation for everyreaction A. The Group I Elements: AlkaliMetals–Lithium, Sodium, and Potassium with 50mL distilled water

phenolphthalein indicator. he Group 2 Elements:Alkaline Earth Metals–Magnesium and Calcium 5 mL ofwater and a few drops of phenolphthaleinindicator and he Group 2 Elements: Alkaline EarthMetals–Magnesium and Calcium and 5 mL of 6 MHCl he Group 13 Elements–Aluminum with 5mL of 6 M HCl.

Aluminum with water

The purpose of this part of the experiment is to find out whichhalogen can oxidize which halide ions or ions. If such a reactionoccurs, the product halogen will be dissolved in the organicsolvent (hexane) and, from the color observed above, you can decideif the reaction occurred.

Reaction of Cl2 with Br-and Cl2 with I- Add a fewdrops of chlorine water (chlorine dissolved in water) to a cleantest tube containing 1 mL of 0.2 M NaBr and to a second test tubecontaining 1 mL of 0.2 M NaI.

Reaction of Br2 with Cl-and Br2 with I-

18. Add a few drops of bromine water (bromine dissolved inwater) to another test tube containing 1 mL of 0.2 M NaCl and to atest tube containing 1 mL of 0.2 M NaI.

Reaction of I2 with Cl-and I2 with Br-

19. Add a few drops of iodine water (iodine dissolved in a KIsolution) to a different test tube containing 1 mL of 0.2 M NaCland to a second test tube containing 1 mL of 0.2 NaBr.

Add hexane to each test tube above

20. Add 2 mL of hexane (C6H14) to each solution from steps 1 7through 19 and mix the contents thoroughly (by shaking or swirlingit carefully). Record your observation in the availabletable. In particular look for evidence of reaction byexamining the color of the hexane layer.

he Transition Elements–Iron, Copper, andZinc

21. Place a piece of iron (steel wool) in one test tube, copper(turnings) in a second, and zinc (turnings) in a third. Place 5 mLof water in each of t h e three test tubes. Tap each tube. Recordthe observations.

22. Repeat the experiment with 2 mL of 6 M HCl and a sample ofeach metal. Record the observations. 23. Repeat the experiment with2 mL of 6 M nitric acid, HNO3 and a sample of each metal. Recordthe

observations.

REPORT

The following tables are for your results section ofyour notebook. DO NOT RECORD these tables in your observationsection.

Write balanced equations for all reactions that you observed. Besure that you specify the state of matter for each reactant andproduct. Water is likely to be the only reagent to have a liquidstate (l). All species dissolved in a solution with water as thesolvent should be labeled as aqueous (aq). If no reaction wasobserved, write N.R. The following tables show the reactants forthe possible reactions. Please record these reactions inyour notebook.

A. The Group 1 Elements: Alkali Metals–Lithium andSodium

Element	Balanced Equation
Lithium, sodium, and potassium with oxygen(O2)
Li + O2
Na + O2
K + O2
Lithium, sodium, and potassium with water; phenolphthaleintest
Li + H2O	Example: 2Li(s) +2H2O(l) ?2Li+(aq) +2OH- (aq) +H2(g)
Na + H2O
K + H2O

B. The Group 2 Elements: Alkaline Earth Metal– Magnesiumand Calcium

Element	Balanced Equation
Magnesium and calcium with air (burning)(O2)
Mg + O2
Ca + O2
Magnesium and calcium with water; phenolphthalein.
Mg + H2O
Ca + H2O
Magnesium and calcium with hydrochloric acid
Mg + HCl
Ca + HCl

Periodic Properties of the Elements – Page- 4

C. The Group 13 Elements—Aluminum

Element	Balanced Equation
Al + O2
Al + H2O
Al + HCl

D. The Group 14 Elements–Carbon

E. The Group 17 Elements: the Halogens–Chlorine,Bromine, and Iodine

Element	Balanced Equation
C + H2O
C + HCl

Mixture	Balanced Net ionic Equation for ObservedReactions
Cl2 and NaBr
Cl2 and NaI
Br2 and NaCl
Br2 and NaI
I2 and NaCl
I2 and NaBr

F. The Transition Elements–Iron, Copper, andZinc

Element	Balanced Equation
Iron, copper, and zinc with water
Fe + H2O
Cu + H2O
Zn + H2O
Iron, copper, and zinc with hydrochloric acid
Fe + HCl
Cu + HCl
Zn + HCl
Iron, copper, and zinc with nitric acid
Fe + HNO3

Periodic Properties of the Elements – Page- 5

Cu + HNO3
Zn + HNO3

A note about the reactions with nitric acid:

a) In general you should see the brown gas NO2 evolved in thesereactions. However, other nitrogen oxides are also possible. Forthe sake of balancing the equation, however, assume NO2 is theproduct of the reaction with HNO3. b) Balance the equations as netionic equations. For example

Cu(s) + 4H+(aq) + 2 NO3 -(aq) ? Cu2+(aq) + 2 NO2 (g) + 2H2O(l)

Discussion

Compare the reactions of Group I metals with Group 2metals.
Compare the reactivity of C to Al.
Compare the reactivity of the transition metals
Explain how reactivity relates to an elements position in theperiodic table.

ADDITIONAL QUESTIONS

Answer the following questions using your lab observations,your knowledge of the reaction products, and the electronicstructure of each element. Keep in mind the relative position ofeach element that you investigated in the periodic table.

What trend can you note for the relative reactivities oflithium, sodium and potassium and their respective position in theperiodic table?

Compare, briefly, the similarities and differences in theproperties of the Group 2 elements with the Group 1 elements youinvestigated. Can you rationalize their contrasting behavior? Usethe position of the elements in the periodic table and, ifpossible, the electron configuration for each element.

How did the reactivities for the representative elements ofGroup 13 (Al) and Group 14 (C) compare to each other and to thereactivities of the elements you investigated in Group 1 and 2. Bespecific and give examples to illustrate your findings.

Compare the similarities and differences in the properties ofthe three transition elements you investigated in their combinationwith water, hydrochloric acid, and nitric acid. Is this behaviorconsistent with their relative position in the periodic table.

Halogen chemistry

a) Which halogen–C12, Br2, or I2 –is mostreactive? How do you conclude this?

b) Which halogen–C12, Br2, or I2 –isleast reactive? How do you conclude this?

c) Is there a trend you can note between the order ofreactivity of these Group 17 elements and their position with

respect to each other in the periodic table?

d) Is the trend in reactivity similar to any trend notedfor the Group1 or 2 elements you observed.