REPORT

UNITS AND IDENTIFICATION OF ELEMENTS

OBJECTIVES OF EXPERIMENT

1. Assess the similarity of the properties of the elements in the periodic table

2. Observe flame and reaction test of some alkaline and alkaline earth elements

3. Recognize the reaction of chlorine and halide water

4. Analyzing an aqueous solution containing alkaline or alkaline earth elements and halides

THEORETICAL BASIS

The halogen elements in the periodic system are included in the VIA class. Making
these elements can be done dilaboratrium in a way that is not too difficult.
Chlorine preparation based on chloride ion oxidation:

2Cl + + Conductor à
Cl2 + reduction result

Oxidizerswhich may be used in acidic solutions, such as MnO2, MnO4-, Cr2O7-2, PbO2. The
preparation of bromine is also based on the oxidation of Br-ions by
oxidizing-oxidizing agents as used in chlorine preparation. Apart from that,
bromine can also be prepared by oxidizing bromide ions with chlorine.

Cl2 + 2Br- à 2Cl- +Br2

Whereas Yod, I2,can be prepared by oxidizing I ions

Cl2 + 2I¬- à 2Cl- +I2

Alkaline andalkaline earth metals are called light metals, therefore their density is
small. All of these metals react strongly with water, liberating hydrogen and
producing strong bases. This element has the valence electrons 1 compared
between the elements in 1 period, then the radius of the largest alkali metal
atom. The valence electrons are easily removed so that the alkali metals are
among the most electropositive elements. In this class, the more downward the
relative.The alkaline earthmetals, having 2 valence electrons whose oxidation rate is only 1 is +2

This element can also be known by examining the flame color of the salt changes

(Ahmad Hiskia 1993: 119-126).

Elements in 1 group have many chemical properties. The chemical properties are determined 

by the valenceelectrons, the electrons in the outer shell of the passageway, since the valence

electrons of elements belonging to one another are of the same chemical nature.

A.  Group IA

Elements of this class are highlyelectropositive and reactive. Because of this element its reactivity 

is notavailable in the free state of the dialam. Franogen is a radioactive element.
All elements of this class are powerful reducers and have low density. In
bunsen flame red lithium ions, yellow sodium, purple potassium, red rubidium
and cesium blue. 

B.  Group VIIA 

Elements of this classis very electronegative, it means easy to form nesotif ion x1. This element
forms the diatomic molecules F2, Cl2, Br2, and I2. At a chlorine temperature of gas Greenish

yellow, bromine is brownish red liquid. Iod is a black solid and flor is a yellowish gas. 

C.  Gas Noble 

The class consists of elements of helium, neon, argon, krypton, ksenon, and radon.
Some properties of this element of the class. The atoms of this noble gas all
have a full electron array of 8 electrons. In the outer shell of the electron
configuration such a configuration is so stable, therefore for years the
compounds of the noble gas element have not known. It was not until 1962 that
Bartlet discovered that the ksenon could react with Pt. F6 formed XePtF6 since
the ksenon compound was obtained so many experts investigate about noble gas
compounds. Of the ksenon has been known many compounds such as: XeF2, XeF6,
XeOF4, XeO2F2 and XeO3. 

B.  Transitional Elements 

In each long period between groups IIA and IIIA there are elements called
transition elements. These elements are elements with atomic numbers = 21-30,
34-48, 57-78, and 89-120. All transition elements are metal, except gold
(yellow) and copper (red). These elements resemble iron or lead. The chemical
equations appear more in one period than in one class. Especially the elements
in class VIIIB are very similar to each other. In general these metals: 1. The
number of electrons in the outer shell remains 2. Melting point and high
boiling point 3. The radius of the atom is almost the same 4. The potential
energy is only slightly increased with the increasing number of atoms
(Sukardjo.1990: 375-377).

The alkali metal group is a group of the most active active

metals. The metals exhibit low ionisation energies, large and negative
electrode potentials. The conclusion that in general the diversity of traits in
this class is easily predicted in terms of sustainability. Some deviations are
mainly shown by the main members of Li. Some of the material of Lithium and its
compounds compared to alkali metals: 1. The solubility of carbon, fluoride,
hydroxide, and phosphate compounds is low. 2. Ability to form Nitride (LI3N).
3. Normal oxide formers (LI2O), Not peroxides or superoxides. 4. When heated,
the carbonate and hydroxide compounds are to be oxidized. In the alkali
metal group, this difference is caused by the high charge density (ie the ratio
of cation charge to the cation radius) to Li + compared to other alkali metal
ions. IIA metal ion, the suit is reduced to free metal, because the
potential price of the reduction is large and negative. The alkaline earth
metal compounds as described above are alkaline earth cations having high
positive charge density. When dependent on a particular anion, the cation will
give high lattice energy and the salts may be slightly soluble or insoluble in
water (Raip H Pertucci.1993: 51-53, 96-106).

TOOLS AND MATERIALS

1.Flame test for alkaline and alkaline earth elements

A. Tool

Ø Reaction tube 6 pieces

Ø Nichrome wire

Ø On bunsen

Ø Shelf

B. material

Ø Solution BaCl2 0.5 M

Ø CaCl2 0.5 M solution

Ø LiCl 0.5 M solution

Ø 0.5 M KCl solution

Ø 0.5 M NaCl solution

Ø Solution SrCl 0.5 M

Ø HCl 12 M concentrated solution

2. Reactions of alkaline and alkaline earth elements

A. Tool

Ø Tubes

Ø Report sheets

B. material

Ø 1 ml of 0.5 M ammonium carbonate solution

Ø 2 ml barium solution, calcium, lithium, potassium, sodium and strontium

Ø1 ml of 0.5 M ammonium phosphate solution

Ø Distilled water

3. Halide reactions

A. Tool

Ø Reaction tube 3 pieces

B. material

Ø NaCl 0.5M, NaBr 0.5M, NaI 0.5M

Ø 1 ml of carbon tetrachloride

Ø 1 ml of chlorine water

Ø 5 drops of dilute nitric acid

4. Analysis of this solution

A. Tool

Ø Reaction tube 3 pieces

B. material

Ø Solution anu (x)

Ø 1 ml of ammonium carbonate

Ø 1 ml of ammonium sulphate

Ø 1 ml of ammonium phosphate

Ø 1 ml of anu solution (y)

Ø 1 ml of carbon tetrachloride

Ø 1 ml of chlorine water

Ø A drop of nitric acid

WORK PROCEDURES
A) Flame test for alkaline and alkaline earth elements
1. Place six test tubes on the rack. Add each of them 2 ml of BaCl2 solution 0.5 M, CaCl2 0.5 M, 
KCl 0.5 M, NaCl 0.5 M.
2. Take the nichrome wire, heat it on the blue part of Bunsen flame. Heat it until there is no more 
color on the flame. To prevent contamination, do not touch the clean nikrom wire.
3. Dip the wire into the tube containing the barium solution, then heat the wire tip on the flame. 
Record your observation. Clean the wire and repeat the flame test for a solution containing calcium 
and sodium. Note: to wire the used wire dip the wire into a concentrated HCl solution (12 M) and 
heat it to red. If necessary repeat this procedure.
B) Reactions of alkaline and alkaline earth elements
1. Add 1 ml of solution (NH4) 2CO3 0.5 M into each tube if formed precipitate, write EDP in report 
sheet, if no reaction write TR.
2. Clean the test tube and rinse with distilled water. Put 2 ml of barium, calcium, lithium, sodium and 
strontium solution, respectively into the test tube. Add 1 ml of solution (NH4) 2PO4 0.5 M into each 
tube. Record your observations. 3. Clean the tube and insert 1ml of barium, calcium, lithium, 
potassium, sodium and strontium solution into separate tubes. Add 1 ml of solution (NH4) 2SO4 
into each tube and record your observations.
C) Halide Reactions 
1. Place the three test tubes on the rack. Put 1 ml of the following solution into each tube: NaCl 
0.5 M, NaBr 0.5 M, NaI 0.5 M. 2. In each tube add 1 ml CCl4.1 ml of water chlorine and 5 drops 
of dilute HNO3 (6M). 3. Shake each tube and observe the color of the CCl4 layer at the bottom 
(Note: dispose of this solution into a special container for disposal of organic waste).

D) Analysis of such solutions

1. Ask a number of solutions anu (x) to asisiten.Lakukan flame test and record your observations.

2. Enter 1 ml of each anu solution into the first tube, 1 ml (NH4) 2PO4 into the second tube and 1 ml 

(NH4) 2SO4 into the third tube. Note your observations.

3. Place 1 ml of solution (y) into the test tube. Add 1 ml CCl4,1 ml of chlorine water and a drop 

of HNO3. Mix the test tube and note the color of the CCl4 coating.

4. Compare the flame test and the reaction of solution X with the six known solutions 

(procedures A and B), state what alkaline elements are present in solution X. 5. Compare the 

test of halide from solution Y with the three known halide solutions (procedure C). 

State what halides are in solution Y.

OBSERVATION DATA

A. Flame Test Alkali and Alkali Elements

 


  

  

No.

  

  

Substance

  

  

Flame color

  

  

Information

 

  

  

1.

  

  

CaCl2

  

  

Red

  

  

Alkaline
  earth

 

  

  

2.

  

  

BaCl2

  

  

Yellow

  

  

Alkaline
  earth

 

  

  

3.

  

  

SrCl2

  

  

Red

  

  

Alkaline
  earth

 

  

  

4.

  

  

KCl

  

  

Purple

  

  

Alkali

 

  

  

5.

  

  

NaCl

  

  

Orange

  

  

Alkali

 

  

  

6.

  

  

LiCl

  

  

-

  

  

-

B. Reactions of Alkaline and Alkaline Soil Elements

 


  

  

No.

  

  

Subtance

  

  

Reactor

  

  

EDP

  

  

TR

 

  

  

1.

2.

3.

4.

5.

6.

  

  

CaCl2

BaCl2

SrCl2

KCl

NaCl

LiCl

  

  

(NH4)2CO3­

  

  

  

  

  

-

 

  

  

  

  

  

-

 

  

  

  

  

  

-

 

  

  

-

  

  

  

 

  

  

-

  

  

  

 

  

  

-

  

  

-

 

  

  

No.

  

  

Subtance

  

  

Reactor

  

  

EDP

  

  

TR

 

  

  

1.

2.

3.

4.

5.

6.

  

  

CaCl2

BaCl2

SrCl2

KCl

NaCl

LiCl

  

  

(NH4­)3PO4

  

  

  

  

  

-

 

  

  

  

  

  

-

 

  

  

  

  

  

-

 

  

  

-

  

  

  

 

  

  

-

  

  

  

 

  

  

-

  

  

-

 

  

  

No.

  

  

Subtance

  

  

Reactor

  

  

EDP

  

  

TR

 

  

  

1.

  

  

CaCl2

  

  

(NH4)2SO4

  

  

  

  

  

-

 

  

  

2.

  

  

BaCl2

  

  

  

  

  

-

 

  

  

3.

  

  

SrCl2

  

  

  

  

  

-

 

  

  

4.

  

  

KCl

  

  

-

  

  

  

 

  

  

5.

  

  

NaCl

  

  

-

  

  

  

 

  

  

6.

  

  

LiCl

  

  

-

  

  

-

 

C. Halide Reactions

 


  

  

No.

  

  

Subtance

  

  

Flame color

 

  

  

1.

  

  

NaCl + Cl2

  

  

Clear

 

  

  

2.

  

  

NaBr + Cl2

  

  

Orange
  yellowish

 

  

  

3.

  

  

NaI + Cl2

  

  

Red

D. Analysis of Anu

A. Substance X

• The color of the substance X = purple

• X + (NH4) 2CO3 à TR

• X + (NH4 ) 3PO4 à TR

• X + (NH4) 2SO4 à TR

Conclusion: This substance is KCl

B. Substance Y

Substance Y + CCl4 + HNO3 à There is Sludge

Layer Color CCl4 = red brick

Conclusion: This substance is NaI

DISCUSSION

A. Flame Test for Alkaline and Alkaline Soil Elements 

The elements of the alkaline and alkaline earth classes are highly reactive elements. 

The alkaline and alkaline earth elements also give different colors to the flame. Flame 

tests are usually used to identify alkaline and alkaline earth elements. Electrons in atoms 

can move from one skin to another. When electrons move from lower skin there will be 

release of energy in the form of electromagnetic radiation with a certain wavelength. If the 

radiation is in visible light, it will be visible color. Here are the results of the color test on 

the elements alkaline and alkaline earth elements that have been done. 

• Alkaline and flame colors

1. KCl: Purple

2. NaCl: Orange

3. LiCl: Not practiced

• Ground alkaline and flame color

1. CaCl2: Red

2. BaCl2: Yellow

3. SrCl2 ¬: Red

B. Reactions of Soil Alkaline Elements 

From the experiments of alkaline earth reactions with (NH4) 2CO3, (NH4,) 3PO4, and (NH4) 2SO4. 

In general, the reaction with alkaline earth is deposited, this is due to the solubility of alkaline ion 

ions> alkali ions. While the elements of the alkaline group does not occur precipitate in the reaction. 

a. The reactions of alkaline and alkaline earth elements which are associated with (NH4) 2CO3 ¬

KCl + (NH4) 2CO3 à TR (Does not have precipitation or no reaction)

NaCl + (NH4) 2CO3 à TR (No deposition or no reaction)

LiCl + (NH4) 2CO3 à is not quoted

• Soil Alkaline Elements

CaCl2 + (NH4) 2CO3 à CaCO3 + 2NH4Cl (settles)

BaCl2 + (NH4) 2CO3 à BaCO3 + 2NH4Cl (settles)

SrCl2 + (NH4) 2CO3 à SrCO3 + 2NH4Cl (settles)

b. The reactions of alkaline and alkaline earth elements which are associated with (NH4 ·) 3PO4

• Alkali Elemental Elements

KCl + (NH4 ¬) 3PO4 à TR (Not subject to precipitation or no reaction)

NaCl + (NH4 ¬) 3PO4 à TR (Does not have precipitation or no reaction)

LiCl + (NH4¬) 3PO4 à is not practiced

• Soil Alkaline Elements

3CaCl2 + 2 (NH4 ¬) 3PO4 à Ca3 (PO4) 2 + 6NH4Cl (settles)

3BaCl2 + 2 (NH4 ¬) 3PO4 à Ba3 (PO4) 2 + 6NH4Cl (settles)

3SrCl2 + 2 (NH4¬) 3PO4 ¬à Sr3 (PO4) 2 + 6NH4Cl (settles)

C. Reactions of alkaline and alkaline earth elements which are associated with (NH4) 2SO4

• Alkali Elemental Elements

KCl + (NH4) 2SO4 à TR (Not subject to precipitation or no reaction)

NaCl + (NH4) 2SO4 à TR (Does not have precipitation or no reaction)

LiCl + (NH4) 2SO4 à is not practiced

• Soil Alkaline Elements

BaCl2 + (NH4) 2SO4 à BaSO4 + 2NH4Cl (settles)

CaCl2 + (NH4) 2SO4 à CaSO4 + 2NH4Cl (settles)

SrCl2 + (NH4) 2SO4 à SrSO4 + 2NH4Cl (settles)

Based on the observed table data, there is a similarity of the properties of the elements, namely the 

similarity of the properties of the elements of a group, for example: in the alkaline element, ie K, Na, 

and Li which are not reacted by solution (NH4) 2CO3¬, (NH4) 3PO4, and (NH4) 2SO4. And on 

alkaline earth elements, the elements reacted with (NH4) 2CO3, NH4, 3PO4 and NH4 2SO4 

produce precipitate and can react, except Be and Mg, react continuously in air until completely 

converted to oxide, Hydroxides, and carbonates. But K, Na, Li, Ba, Sr and Ca. After being put 

into practice, not all results are the same as theories, maybe here an error occurred during the 

experiment.

C. Halide Reactions

The halide reactions tested in this experiment are NaCl, NaBr, and NaI, before the compounds are 

converted into ions.

NaCl à Na + + Cl-

NaBr à Na + + Br-

NaI à Na + + I-

Br- and I- can be detected by reaction with Cl2 and Cl2 reducing to Cl-, while Br- or I-oxidized to 

Br2 or I2. Br2 or I2 is extracted from an aqueous solution with a solvent of nitric acid (HNO 3) so 

that Br2 is formed in a yellowish precipitate at the top and the nodes of the undercoat. The clear 

color of the lower layer is the reaction of CCl4. The top layer is a chlorine water reaction, while 

the bottom layer is the reaction of the halide.

• Halogen properties

From the top down the radius of the atom increases, the boiling and melting points increase.

• Properties of halide elements

A. Chlorine (Cl)

Chlorine in water is light green. Chlorine with hydrogen gas reacts quickly and if the ultraviolet 

element will blast due to a chain reaction, the chlorine in water is not completely dissolved and 

the reaction is slow.

B. Bromine (Br)

Bromine in reddish brown water. With hydrogen gas reacting slowly. Bromine in water does not 

dissolve completely and its reaction is slow.

C. Iodine (I)

Iodine in brown water. With hydrogen gas reacting slowl.

D. Solution Analysis of X and Y

In the X substance, the practicum states that the solution of X is a solution of Potassium Chloride 

(KCl), because no one is subjected to the precipitate. While on the substance Y, practicum states 

that the solution Y is a solution of NaI, Because the color layer CCl4 is red brick.

BIBLIOGRAPHY

Ahmad, Hiskia. 1993. Chemical Basics Guide. Jakarta: Depdikbud

Epinur et al. 2013. Basic Chemical Practicum Guide. Jambi: University of Jambi

Oxtoby, David. 2003. The Principles of Modern Chemistry. Jakarta: Erland

Petrucci, Raip. 1993. Applied Chemical Principles. Jakarta: Erland

Soetopo. 1990. Applied Chemical Principles. Jakarta: Yudhisthira

Sukardjo. 1990. Basic Chemistry. Jakarta: Erland