 The relationship between the electronic configuration and the chemical properties of elements is most readily expressed in terms of the periodic table. The elements are arranged in the table in the order of increasing atomic numbers in horizontal rows, called periods of such length that elements with similar properties recur periodically.
 The elements with similar chemical properties are arranged in vertical columns called groups or families and they have the same number of valence electrons. Elements found in the same horizontal rows have the same number of energy levels but cannot be expected to behave in similar ways.

1.) To examine the properties of elements in various group.
2.) To observe the reactions of compounds of elements that belong to the same group in the periodic table.

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Beaker
Blue & red litmus papers
Bunsen burner
Corks
Crucible tong
Evaporating dish
Glass tubing
Graduated Cylinder
Pipette
Rubber aspirator
Sand paper/Triangular file
Test tubes
Tripod
Wire gauze

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0.1M AlCl
3
１ M HCl
1M NaOH
BaCO
3
CaCO
3
CaO
Concentrated HNO
3
Copper wire
Distilled wire
K
2
CO
3
Magnesium ribbon
Na
2
CO
3
Phenolphthalein
Sulfur Powder

A.) 1.) Place 3mL of CuSO
4 solution in a test tube. Take note of its color.
2.) Add 1mL of NH
4
OH solution to the CuSO
4 solution.
Observe and record what happens.
B.) 1.) Clean a 2-cm piece of Cu wire and a 2-cm piece of Mg ribbon with sand paper. Get a small pinch each of Al metal turning and iron filings.
2.) Place 5mL HCl in each of four test tubes. *CAUTION! HCl can damage skin, eyes, and clothes. Pour carefully*
3.) Add the metals separately to the test tubes. Label each test tube with the name of the metal added.
4.) Observe what happens in each tube. Record any change in the color or appearance of the metal pieces. Record observations on the data chart.
C.) 1.) Place 3mL of ZnSO
4 in a test tube. Add 1mL of BaCl
2 to it.
Describe and record what happens.

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Group IA metal + water →Base + Hydrogen ions
1.) Group I - 2Na + H
2
O → 2NaOH + H
2
↑ = More
- 2 K +H
2
O → 2KOH +H
2
↑ = reactive because rxn occurs at RT only.
›
Group IIA metal + water → Base
Mg + O
2
→ MgO heat
2.) Group 2 – MgO + H
2
O → Mg[OH]
2
+ H
2
↑(occurs at high
Boiling temp.) turns to fuschia solution w/ phenolphthalein.

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Group I-A Carbonates are soluble in water.
Na
2
Co
3
+ H
2
O → soluble Group IA elements – more reactive
K
2
Co
3
+ H
2
O → Soluble
›
Group II-A Carbonates are insoluble in water.
CaCo
3
+ H
2
O → insoluble Group IIA elements – less reactive
BaCO
3
+ H
2
O → insoluble

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Group IIA Metallic + Water → Base
Mg + O
2
→ MgO + H
2
O → Mg [OH]
2
+ H
2
↑ + phenolphthalein
↓
Colorless to fuschia pink – Base
CaO + H
2
O → Ca[OH]
2
+H
2
↑ + Phenolphthalein
↓ fuschia pink – Base

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Group V-A and VI-A Non – metallic oxides + water → Acid
S + O
2
→ SO
2
+ H
2
O → H
2
SO
3
+ pH(BLP to RLP)→pink – Acid
Burning (Yellow Gas) (Sulfurous acid)
HNO
3
+ Cu → HNO
2
+ CuO + pH (moist BLP to RLP) → pink – Acid
(nitrous acid (Copper oxide
*green*) *brown*)

AlCl
3
+ 6H
2
O → Al(H
2
O)
6
+
3
+ 3CL hydrated
Aluminum ion
Al(H
2
O)
6
+
3
+ H
2
O → Al(H
2
O)
5
OH+ 2 + H
3
O(hydronium)
Acid Base Base Acid
(hydrated hydrated
Aluminum ion) Aluminum ion
BLP
AlCl
3
→ BLP – Acidic + HCl → – Acidic
RLP
AlCl
3
→ RLP – No change + NaOH → - Basic
Metalloid elements such as that of aluminum when combined with other compounds can act both as an acid and as a base.

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