The atomic radius is the distance from the atomic nucleus to the outermost stable electron orbital in an atom that is at equilibrium. The atomic radius tends to decrease as one progresses across a period from left to right because the effective nuclear charge increases, thereby attracting the orbiting electrons and lessening the radius. The atomic radius usually increases while going down a group due to the addition of a new energy level (shell). However, diagonally, the number of electrons has a larger effect than the sizeable radiu

1. REACTIONS IN SOLUTION
by Dr. Robert D. Craig, Ph.D.
Part I: REACTIONS IN SOLUTION: Chlorine & Potassium Bromide
Oxidation Reaction
Part II -Oxides of Elements
Part III-Evidence for the Presence of ion in Aqueous Solution

2. REACTIONS IN SOLUTION
students do this part
• Add 3 M sodium hydroxide dropwise to 5 Ml
of 0.1 M solutions of AlCl3, FeCl3, CdCl2, NiCl2
and CuCl2
• Each contained in a separate test tube, until a
precipitate forms.

3. AlCl3, FeCl3, CdCl2, NiCl2 and CuCl2
• .

4. .
• Stir the solution well. Write equations for the
reactions (68)
• What ions are reacting in each case? (69)
• Write the net ionic equations for the reactions
(70)

5. Part 2
• Place 5 mL of 0.1 M CuCl2, HgCl2, FeCl3, Pb(NO3)
2 and AgNO3, in indivdual test tube
Drop a piece of steel wool into each tube. Warm each
test tube and its contents slightly in a water bath on
a hot plate and observe what happens

6. Part 2 .what exactly is steel???

7. Part 2
• Record the observations (71)
What ions are reacting in each case (72)?
Write net ionic equations for the reactions (73)

8. Part 3
• Place 5 mL of 0.1 M CuCl2, HgCl2, FeCl2, NiCl2,
Pb(NO3) 2 and AgNO3 in individual test tubes.
Drop a piece of copper into each of the test
tubes. Record the observations (74)

9. What conclusions???
• Recall what happened when each of these
metals was place in hydrochloric acid.
• What conclusions can be drawn from these
experiments and those experiments and those
involving the addition of some of these metals
to 6M HCl (75)

10. What conclusions???
• What ions are reacting in each case?
• Write the net ionic equations for the reactions
(76).

11. Part I
H. Group VIIA Chlorine, bromine, iodine, and
fluorine
• (46) Location on the periodic table
• (47) Physical Properties of elements

12. Part I
• (48) Observations for addition of methylene
chloride to a reaction mixture chlorine water
and 0.1 M potassium bromide (KBr)
• (49) Account for the color changes that are
observed

13. Used in decaffienation process

14. Chlorine & Potassium Bromide
Oxidation Reaction
• (51) Observation for addition of methylene
chloride to a reaction mixture chlorine water
and 0.1 M potassium iodide (KI)
• (52) Account for the color changes that are
observed

15. Chlorine & Potassium Bromide
Oxidation Reaction
• (50) Equation for the reaction
• Cl2 (aq) + KBr(aq) -

16. Chlorine & Potassium Bromide
Oxidation Reaction
• http://www.ehow.com/facts_6915632_chlori
ne-potassium-bromide-oxidation-
reaction.html

17. .
• (54) Observation for addition of methylene
chloride to a reaction mixture chlorine water
and 0.1 M potassium iodide (KI)
• (55) Account for the color changes that are
observed

18. Chlorine & Potassium Bromide
Oxidation Reaction
Chlorine is more electronegative than bromine, meaning
that it has a greater affinity for electrons, so it's able to
steal an electron from its less fortunate neighbor or
oxidize it. A chlorine that has gained an electron has a
negative 1 charge and an oxidation number of -1, so it
has become reduced or gained electrons
•
Read more: Chlorine & Potassium Bromide Oxidation
Reaction | eHow.com
http://www.ehow.com/facts_6915632_chlorine-
potassium-bromide-oxidation-
reaction.html#ixzz1ecUKoPl8

19. Chlorine & Potassium Bromide
Oxidation Reaction
Chlorine and bromine are both halogens, elements under
group 17 of the periodic table. As a general rule, each
halogen can oxidize the halogens below it in the group.
Chlorine, for example, can oxidize bromine or iodine,
both of which are below it in the group, while bromine
can only oxidize iodine
•
Read more: Chlorine & Potassium Bromide Oxidation
Reaction | eHow.com
http://www.ehow.com/facts_6915632_chlorine-
potassium-bromide-oxidation-
reaction.html#ixzz1ecTs7woc

20. .Can use same web site
(56) Equation for the reaction
Br2 (aq) + KI (aq) -

21. Can use similar web site!!!.
• (57) What can be said about the chemical
reactivity of chlorine, bromine and iodine with
respect to one another?

22. .
• (58) Discussion of chemical and physical
properties of elements studied section A
through H
• Please comment on the way in which the
properties vary with position

23. Part II -Oxides of Elements
• (59) Please make observations for heating
oxides

24. Part II -Oxides of Elements
• (60) Produce the equations for the reactions
Al2O3 -
___________________________________
CaO ->
_____________________________________

25. Part II -Oxides of Elements
• Oxides of Elements
ZnO -
___________________________________
Ag2O ->
_____________________________________
HgO ->
_____________________________________

26. .
(61) Which of the tested oxides are most
thermally stable? Explain using the results

27. .
(62) Which of the tested oxides are least
thermally stable? Explain using your results

28. • (63) Equation of the reaction of Fe2O3 and
Mg
• Fe2O3 + Mg
• __________________________________

29. • (64) Equation for the reaction of calcium
oxide and water
• Ca0 + H20
• ____________________________________.

30. Need observations from last lab
• (65) Comparison of the results from Part II-D
with those of experiments for Part I-F(10 and
Part I-G (1). (Compare these results with
those of experiments with phosphorus
• And Sulfur, Part I-G(1)
• Video in portal!!!!!!

31. Part III-Evidence for the Presence of
ion in Aqueous Solution
(66) What can be concluded about the nature
of solutions of NaOH, HCL, NaCL, FeCl3 and
CH3COOH compared with pure water

32. .
(67) List the symbols for the ions that exist in
each of the following solutions:
NaOH__________
HCl____________
NaCl___________
FeCl3__________

33. .
(68) Equations for reactions of NaOH with
solutions of AlCl3, FeCl3, CdCl2, NiCl2, and CuCl2

34. .
AlCl3 + NaOH__________
FeCl3 + NaOH__________
CdCl2 + NaOH__________
NiCl2+ NaOH__________
CuCl2 + NaOH__________

35. .
• (69) What ions are reacting in each case in
question 68??

36. .
Al 3+ + OH-__________
Fe 3+ + OH-__________
Cd 3+ + OH-__________
Ni 2+ + OH-__________
Cu 2+ + OH-__________

37. .
• (71) observation for addition of Fe to
solutions of CuCl2C, HgCl2, FeCl3 , Pb (NO3) 2
and AgNO3

38. • (72) What ions are reacting in each case when
Fe is added to CuCl2, HgCl2, FeCl3, Pb(NO3)2
and AgNO3?

39. (73) Write net ionic equations for the
above reactions
Cu 3+ + Fe__________
Hg 2++ Fe__________
Fe 3+ + Fe-__________
Pb 2+ + Fe-__________
Ag++ + Fe-__________

40. .
• (74) Observations for addition to Cu to
solutions of CuCl2, HgCl2, FeCl2, Pb(NO3) 2and
AgNO3

41. (75) Same for Copper
Cu 3+ + Cu__________
Hg 2++ + Cu__________
Fe 3+ + Cu__________
Pb 2+ + Cu__________
Ag++ + Cu__________

42. .
• (76) What ions are reacting in each case?
Write the net ionic equations for the reactions