USING ENGLISH TO REPORT

I. TITLE            : UNITS AND IDENTIFICATION OF ELEMENTS

II. DAY/DATE   : Friday,27 May 2017

III. PURPOSE

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

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

3. Recognize the reaction of chlorine and halide air.

4. Analyzing an anu solution containing alkaline and alkaline earth elements and halides.

IV. PRACTICE QUESTIONS
1. Write down the elements that belong to the alkaline and alkaline classes

     Answer:

     IA (alkali) class: H (Hydrogen), Li (Lithium), Na (Sodium), Kr (Chromine),Group IIA (alkaline earth):          Be (Belrilium), Mg (Magnesium), Ca (Calcium), Sr (Strontium), Ba (Barium), Ra (Radium).
2. Complete the following reaction equation:

     CaCl2 + (NH4) 2CO3 → CaCO3 + 2NH4Cl

     BaCl2 + (NH4) 2CO3 → BaCo3 + 2NH4Cl

     2NaCl + (NH4) 2CO3 → Na2CO3 + 2NH4Cl

     2NaCl + Cl → TR

     2NaBr + 2Cl → 2NaCl2 + Br2

     2NaI + Cl2 → 2NaCl + I2
3. What is the function of adding CCl4 in experiment c?

     Answer: function at this time with iodine lar, the solution will be lit. As an identifier in an object, because        CCl4 is non polar.

V THEORY OF THEORY

       In this experiment will be tested flame of alkaline and alkaline earth solution. Flame test can be observed from very small amount of solution by using nichrome wire. By dipping the nichrome wire into the solution and then inflaming it in the blue flame will be observed the flame color of the element. The solution used is the salt solution of the element. Each element gives a different flame color. Example: barium solution gives yellow flame, green copper solution, red lithium solution.

      The flame becomes the hallmark of each of the elements. The sharp yellow flame color is a practical way to determine the element of sodium. This is why flame testing can be used to determine unknown solutions.

The halide salt of alkali and alkaline earth reacts to a more oxidizing halogen, thus forming a halogen of the halide. The order of oxidizing forces is: F2> Cl2> Br2> I2.F2 can oxidize Cl- to Cl2 and Cl2 can oxidize Br- to Br2 and so on (lecturer chemistry, 2013).

       The elements in one group have many chemical properties, the chemical properties are determined by the valence electrons, the electrons in the outer shell of the skin. Because the valence electrons of the same group of elements are themselves the same (Sukardjo 1985) .

Elements of alkaline groups are very elecrophositive and reactive. This element is because the reactive is not present in a state free in nature. Franium is a radioactive element. All elements of this class is a good conductor of heat and electricity. Because soft metal can be cut with a knife,

Reducers are strong and have a low heat type (Sukardjo, 1985: 373).

          The alkali metal in the IA family of the periodic table and the alkaline earth metal in the IIA family is so named because most of the oxides and their hydroxides are among the most powerful alkalies known (http://www.google.com/url? -and-elements-of-testing-qualitative-analysis-types).

The most striking feature of alkali and alkaline earth metals is

Its activity is enormous. Because these metals are so active that they do not exist as an element, when in contact with air or water. None of the IA and IIA elements exist in nature in its elemental state. All elements of alkali are present in natural compounds As a unipositive ion (positive-one), all the alkaline earth elements are present as positive (positive-two) ions (Sixth, 1980).

              Alkali and alkaline earth metals are very powerful reducing agents, because they are so easy to lose electrons. They are easy to join with most non-metallic elements, forming ionic compounds such as halides, hydrides, oxides and sulfides (https://www.google.com/search? Q = report + class + and + identification + element).

            Anhydrous halides can be made with dehydration from hydrate salts. Magnesium and calcium halides readily absorb water. The ability to form hydrates as well as their solubility in water decreases with increasing size and halides of Sr., Bad an Ra is usually anhydrous. This complements the fact that Energy decreases more rapidly than lattice energy with increasing M2 + size (Cotton, 1989).

For the purpose of qualitative analysis systematic cations are classified into 5 classes based on the cation's properties on reagents.

The five categories of cations and the characteristics of these factions are as follows:

1) Group I: this class cation forms a precipitate with dilute hydrochloric acid. These group ions are lead, mercury (I), and silver.

2) Group II: this group cation does not react with hydrochloric acid, but forms a precipitate with hydrogen sulfide in a dilute mineral acid atmosphere. These ionic ions are mercurium (II), copper, bismuth, cadmium, arsenic (III), arsenic (V), stibium (III), stibium (V), tin (II), and tin (III) (IV) .

3) Group III: this class of cations does not react with dilute HCl, nor with H2S in a dilute mineral acid atmosphere. These cations are cobalt (II), nickel (II), iron (II), iron (III), chromium (III), aluminum, zinc, and manganese (II).

4) Group IV: this group cation does not react with reagents of classes I, II, and III. These cations are calcium, strontium and barium.

5) Group V: common cations, which do not react with group I, II, III and IV reagents, are the last cationic groups, including magnesium, sodium, potassium, ammonium, lithium and hydrogen ions.

(Petrucci, 1997).

VI TOOLS AND MATERIALS

6.1 tools

• Test tube

• Reaction tube shelf

• Nichrome wire

• Drop pipette

• Bunsen

• Brace

6.2 Material

• BaC l2

• CaCl2

• NaCl

• KCl

• Dense HCl

• NaBr

• NaCl

• (NH4) 2PO4

VII WORK PROCEDURES

A. Flame test for alkaline and alkaline earth elements

1. Reaction Tubes

-2 ml bacl2 0.5 M solution, CaCl2 0.5 M, LiCl 0.5 M, KCl 0.5 M, NaCl 0.5 M, Srcl 0.5M, inserted into 6 test tubes.

2. Nichrome wire

- Heated on blue agian until no color that comes on the flame

- Dipped into a tube containing a Barium solution

- Heated wire tip on flame

- Heated wire tip on flame

-In observed and recorded observations

3. The reaction tube

-Cleaned

- Repeated flame test for a solution containing Ca, Li, K, and s

-Result

B. Reactions of alkaline and alkaline earth elements

1. Ammonium carbonate

-Added into each tube

-Well, write EDP if settled, write TR if there is no reaction

2. Test tube

-Cleaned

-Enter each into 2ml tube Ba, Ca, li, Na, Sr.

-Equipped each tube with 1 ml of ammonium phosphst .5 M

-In observe

 - Recorded observations

3. The reaction tube

-Cleaned

-Enter each 1 ml of ammonium sulphate larvae

- Observed, recorded observations.

-Result

C. Halide reactions

1. Three test tubes

-Laid on the shelf

-Include each NaCl 0.5M, NaBr 0.5M, Na 0.5 MIml CCl4, 1ml chlorine water, 5 drops of dilute acid 6M

-Added to the tube stack

-Matches

- Observed, recorded observations

-Result

D. Analysis of such solutions

1. Test the flame of the anu solution

- Inserted into the test tube

-Laid on the shelf

-Nikrom wire in the heat tip

- Dip it in an anu x solution

- Heated on the flame tip

- Observed, recorded observations

-Result

2. Solution Anu

-1 ml of the anu solution x is inserted into 3 test tubes

-Added ammonium carbonate pd tube 1, ammonium phosphate tube 2, ammonium sulfate tube 3

- Recorded observations

-Result

3. Solution anu y

-Ented into 1 ml CCl4, 1 ml water chlorine, 5 drops of dilute nitric acid 6 M

- Included into the test tube

-Matches

-Described CCl4 layer color

-Result

VIII. OBSERVATION DATA
A. Flame test for alkaline and alkaline earth elements

No	Substance	Color Is on	Information
1	CaCl2	Red Brick	-
2	BaCl2	Yellow	-
3	SiCl2	Red	-
4	KCl2	Purple	-
5	NaCl2	Yellow	-
6	LiCl2	Red	-

    B. Reactions of alkaline and alkaline earth elements

No	Substance	Pereaksi	EDP	TR
1	CaCl2	(NH4)2CO3	EDP	-
2	BaCl2		-	-
3	SiCl2		EDP	-
4	KCl2		-	TR
5	NaCl2		-	TR
6	LiCl2		-	TR

No	Substance	Reactor	EDP	TR
1	CaCl2	(NH4)2PO4	EDP	-
2	BaCl2		-	-
3	SiCl2		EDP	-
4	KCl2		-	TR
5	NaCl2		-	TR
6	LiCl2		-	TR

No	Substance	Reaactor	EDP	TR
1	CaCl2	(NH4)2SO4	-	TR
2	BaCl2		-	-
3	SiCl2		-	TR
4	KCl2		-	TR
5	NaCl2		-	TR
6	LiCl2		-	TR

C.Halide Reactions

No	Substance	Color is on
1	NaCl + Cl2	Clear
2	NaBr + Cl2	Yellow
3	NaI    + Cl2	Purple

D. Analysis of such solutions

A. Substance x

- Color of the substance x: red

- X + (NH4) 2CO3: TR

- X + (NH4) 2PO4: TR

- X + (NH4) 2PO4: TR

B. Substance y

- Substance y + CCl4 + HNO3 TR

- Color of yellow CCl4 layer

IX POST-FACTORY QUESTIONS

1. Will the flame test alone be used to identify the element?

Explain !

Answer: No, since the flame test is only one feature of the excited elements because heating is one of the characteristics of an element that emits the observed emission spectrum as a beam of light with a certain color. So it can cause errors.

2. Why does the reaction of chlorine water with NaCl, NaBr and NaI give different results?

Answer: because every element of halogen has a different oxidizing rate. The oxidizing power of halogen elements from top to bottom is smaller. So the above halogen can oxidize the halides below but not vice versa.

3. Why do the elements of the IIA class give different results to the IIA groups in experiments B 1, 2 and 3?

Answer: because the solubility of the compound decreases from the top down on the table of the periodic system according to the increase of the atomic number. The alkaline element has a greater novelty than the alkaline earth.

XI DISCUSSION

A. Observation of flame test of alkaline and alkaline earth elements

Alkaline earth metals include Be, Mg, CR, Sr, Ba, Ra. This group is found in soil in the form of insoluble compounds. Flame color given: Be white, Mg white, Ca orange, Sr red, green Ba.

From the observation, the data obtained are as follows: CaCl red, SrCl red, Kcl purple, yellow Nacl, red Licl. The data obtained from the observations show that the resulting flame color is in accordance with the theory put forward by Suhardi. Our experiments are done very thoroughly.

B. Reactions of alkaline and alkaline earth elements

In the reaction, CaCl and SrCl solutions are deposited. As for the solution of KCl, NaCl and LiCl not formed precipitate. This occurs because the alkaline earth element has 2 electrons involved in the formation of metal bonds. The radius of the atom increases from the top down so that the distance to the core causes the reactivity to increase.

C. Halide reactions

Based on the experimental results, the data obtained are: is NaCl + Cl is yellow, NaBr + Cl is yellow, NaI + Cl2 is purple. The flame color difference is caused by a more oxidizing reaction of halide salts of alkali and alkaline earths. So at the time of nikro burning wire to give different flame color.

The halide salt of the alkaline earth may act with a more oxidizing halogen. The halogen element is the most reactive non-metallic group. From top to bottom, boiling point and melting titk increase. At room temperature (25oc, 1 atm) F2 and Cl2 are gases, Br2 is a volatile liquid and a solid, sublimate I2 is sublimable. The halda molecule has a color because it absorbs light as the result of excitation of electrons to a higher level.

D. Analysis of such solution

1. Substance x

- Color of the substance x: red

- X + (NH4) 2CO3: TR

- X + (NH4) 2PO4: TR

- X + (NH4) 2PO4: TR

From the data obtained can be concluded that the x is a NaCl that produces red.

2. Substance y

- Substance y + CCl4 + HNO3 TR

- Color of yellow CCl4 layer

From the datd it can be concluded that y is a yellow sodium.

XII.CONCLUSION

1) The alkaline and alkaline earth salts on the flame test can produce a color that is orange-red Ca, green Ba, K color Purple, Na color yellow. Alkali and alkaline earth salts in alkaline and alkaline earth reactions exist which can react (with the formation of the precipitate) and there is no reaction when mixed with a solution of the substance which can react with (NH4) 2CO3 are CaCl2 and BaCl2, whereas KCl and NaCl are unreacted, (NH4) 3PO4 is CaCl 2 and which is obtained or has been identified with the result of reacting the compound element with some solution.

2) The reaction of chlorine water with NaCl, NaBr and NaI gives different results, this is because each substance or compound has different halogen elements and has different reactivity, and at ordinary temperature has distinct distinct shapes and colors that is: chlorine (Cl ) Is a greenish yellow gas, brom (Br) is a brownish red liquid, iod (I) is a substance in black and flour (F) is a yellowish gas. Whereas chlorine water is useful to give color difference in each substance .

3) Group IA element gives different result with group IIA in experiments B 1,2 and 3 is because group IA when reacting will form strong and soluble base, while group IIA when react will form weak and difficult base, dissolved.

XIII. BIBLIOGRAPHY

Cotton, F Albert. (1989). Basic Inorganic Chemistry.Jakarta: University of Indonesia

Keenan.dkk. (1984) .Chemistry for the University.Jakatra: Erland

Petrucci, Ralph. (1985) .Kimia Dasar.Jakarta: Erland

Sukardjo. 1998. Inorganic chemistry. Jakarta: Erland

Sunardi. 2000. Chemistry. Bandung: Mas Bandung

Tajjudin. 1998. Chemical summary. Jakarta: Erland

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