Carole Bennett, Tampa FL
I always wanted the students to think, “What in the world isn’t chemistry?” Try to help them see that chemistry is everywhere.
I love chemistry and want students to see how wonderful and important chemistry is. Do whatever it takes to help them
visualize what is happening because chemistry is so abstract. That means doing demonstrations to illustrate concepts. Let
them ponder a while, see the wonder of it all, and still enjoy. Guide them and try to pull the explanations of the demonstration
out of them. Demonstrations must have a goal of students learning.
Scavenger hunt
Reprinted from pages 4-5, November 1992
Introduction
I find that this is an excellent activity to use for review at the end
of the year. It illustrates how chemistry is ubiquitous in our lives.
Students work in groups of 2-3. Tags are required on each item
indicating what category it represents. One material
(e.g., water) may represent several categories. Chemistry
laboratories or chemistry kits may not be the sources of chemicals,
but students may measure the materials using lab equipment
where required. The major stress is on how many household
products they can identify. Of course, you may select from this
list only those items that are appropriate to your situation.
Materials
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
Two liquids demonstrating the Law of Multiple Proportions
Element famous for great conductivity and malleability
One mole of something
A mixture
5% solution of HC2H3O2
Compound formed by an alkali and a halogen
Solid that is 100% carbohydrate
Element whose atoms contain 3 electrons in the third
energy level
Unstable acid (Not explosively unstable, please)
Compound whose specific heat is 4.18 J g-1 oC-1
Non-polar compound
Element whose density is 7.86 g/cm3
An ‘acid’ salt
Alcohol solution of a halogen
Alloy of elements #29 and #30
Polymer formed by hexamethylenediamine and hexanedioic
acid (adipic acid)
Solution of isomer of CH3-CH2-CH2OH
5% solution of NaClO
A mild laxative/water solution formed by adding a basic
anhydride to water
Macromolecule that is planar
Pieces of a three dimensional network solid
Acid anhydride that makes a refreshing drink
Ternary compound of an alkaline earth
Substance always produced in neutralization
Substance with specific gravity <1
Salt produced by mixing one mole of NaOH and one mole
of H2CO3
Glass container with metal that can form amalgams
Any organic compound famous for its “fruity” smell.
(You must know its chemical name)
Substance formed by heating Na2CO3
Hydrated ternary salt of element 16. (Most common)
Colloid
10 Chem 13 News/ February 2009
32. Emulsifying agent
33-34. Two transition elements other than Fe, Cu, Ag, Au or Hg
35. Inert gas
36. Metalloid
37. Amount of water whose temperature would rise by 15 ºC
when it absorbs 2646 J
38. Most common ternary salt of element 16 and element 12
39. A solution with a pH above 7
40. Ionic substance whose lattice energy is greater than its
hydration energy
41. A system at physical equilibrium
42. An element or alloy of an element whose electron
shorthand is d4
43. Something that would lower the freezing point of water to
-3.7oC if one mole were placed in 1000 g of water
44. An element whose common oxidation numbers in
compounds are +2 and +3
45. A metal whose 2+ ions form blue aqueous solutions
46. A substance that gets less soluble in water when heated
47. An example of chemical equilibrium
48. An ethyl alcohol solution of 4-hydroxy-3-methoxybenzaldehyde
49. A solution that is about 20 molal
50. An example of Le Chatelier’s Principle
51. A slightly polar nonelectrolyte
52. A strong electrolyte
53. A weak electrolyte
54. Salt produced by mixing two moles of NaOH and one mole
of H2CO3
55. Compound of a halogen other than chlorine
56. Transition element that does not usually form colored
compounds
57. Salt of H2C4H4O6
58. Liquid that exhibits abnormal behaviour when it solidifies
59. Solution that produces hydrogen and chlorine gases when
electrolyzed and yields a very basic end product
60. A liquid with higher vapor pressure than water
61. Substance whose heat of fusion is 335 J/g
62. Source of lime
63. Substance that boils at 70oC at 30 kPa
64. Substance that has a negative heat of solution
For the following find MATERIALS
that contain the following chemicals.
65. Lye (careful with this one — it
is very caustic)
66. Deliquescent salt
67. C12H22O11
68. Dissociated ions
69.
70.
71.
72.
Small amounts of hydrosulfuric acid from Florida aquifer
Starch, acid salt and sodium hydrogen carbonate
Base indicator used as a laxative
Liquid known for its high viscosity due to H bonds (not
water)
73.
CH3 C CH3
41.
O
74.
75.
42.
O
H
H
C
O
O
H
H
O
H
H
H
C
O
CH3
76. Any ionic fluoride
77. Two substances produced when Ca(OH)2 and NH4Cl are
heated
78. Tannic acid
Answers
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
36.
37.
38.
39.
40.
Water and hydrogen peroxide
Any metal
Usually 18 mL of water
Salt water, salt and pepper, etc.
Vinegar
Salt is most common possibility
Sugar, fructose, starch, etc.
Aluminum
Carbonic acid in sodas
Water
Oil, kerosene, gasoline, cooking oil, etc.
Iron
NaHCO3
Tincture of iodine
Brass
Nylon
Rubbing alcohol is isopropyl alcohol
Chlorine bleach, ‘Chlorox’
Mg(OH)2 is in Milk of Magnesia
Graphite in pencil ‘leads’
Sand or quartz
CO2 makes acid in sodas
Epsom salts, MgSO4; gypsum in wall board, CaSO4, or
chalk, CaCO3
24. Water
25. Cork, plastic, cooking oil, etc.
26. Baking soda, NaHCO3
27. Mercury fever thermometer
28. Ester such as ethyl acetate in fingernail polish, or amyl
acetate in banana flavoring
29. Carbon dioxide
30. Epsom salts, MgSO4•7H2O
31. Jell-O, whipping cream, etc.
32. Soap, detergent, egg yolks (lecithin)
33-34. Nickel 5 cent piece, chrome auto part, Ti earrings,
sunglasses coated with iridium, and tungsten light filament
are the most common examples
35. I planned on Ne, Ar or Kr in old ‘neon’ signs, but got He
balloons
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
71.
72.
73.
74.
75.
76.
77.
78.
Si or Ge from computer or calculator chip
42.2 mL water
Epsom salts, magnesium sulfate
Milk of Magnesia, lime water, bleach, etc.
Most ionic salts, e.g., NaCl. One brought ammonium nitrate
from a ‘cold pack’
Sealed container with liquid, e.g., the contents of a soda
can are in vapor-liquid equilibrium
Tungsten filament from light bulb — you decide whether to
accept a chrome plated auto part (Cr is 3d54s1)
NaCl is easiest choice. Any ionic salt with one cation and
one anion
Iron
Copper
Any gas, e.g., CO2 or NH3 from aqueous household
ammonia
H2CO3 ⇌ H2O + CO2 in a sealed soda can
Vanilla flavoring
‘Fudge’ is about 20 m when first cooked. (My students
make fudge to show colligative properties)
Soda can when first opened; relieve stress on gas and the
equilibrium shifts to right
Any alcohol, e.g., isopropyl; sucrose
NaCl is easiest
Vinegar
Washing soda, Na2CO3
Film has AgBr and Agl. Toothpaste has fluoride. Some
scrubbing powders have bromides for bleaching.
Zinc nails or ‘galvanized’ iron
‘Cream of tartar’ is KHC4H4O6
Water expands as it freezes
Solution of NaCl produces H2 at cathode, Cl2 at anode and
NaOH remains
Alcohol, gasoline, fingernail polish remover, etc.
Water
Limestone, chalk, marble, CaCO3
Water
Lye, NaOH; battery acid, H2SO4 is also possible
‘Red Devil’ brand lye is almost pure NaOH
CaCl2 used in closet dehumidifiers
Sucrose (table sugar)
Salt water or solution of any ionic salt
‘Sulfur’ water has H2 dissolved in it
Baking powder
Phenolphthalein is ingredient in ‘Ex-Lax’
Honey, syrup, etc. are easiest. Glycerin or ethylene glycol
would also work but are less common in a home
Acetone as solvent for glues, some cheap fingernail polish
removers
Phenol is in acne preparations like ‘Clear-a-Sil’
Aspirin, acetylsalicylic acid
Some toothpastes contain SnF2 or NaF
Ammonia and water in household ammonia
Tea
Reference
The original idea for this activity was published in an issue of
Chem 13 News in the 1970s. I have lost the reference and
author’s name. I have greatly expanded the material. ∎
February 2009/Chem 13 News 11