CHEMICAL BONDING L.docx

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I. Experiment :Chemical BondingII. Starting of Experiment : Wednesday, November 2, 2011at 1 p.m.III. Finishing of Experiment : Wednesday, November 2, 2011at 3.30 p.m.IV. Purpose : To compare covalence bonding and ionic bonding

To observe the changing of Chlor unsure in

compound, from covalence to ionic.

V. Theoretical Background :A chemical bond is an attraction between atoms that allows the formation

ofchemical substances that contain two or more atoms. The bond is caused by

the electromagnetic forceattraction between opposite charges, either

between electrons and nuclei, or as the result of a dipole attraction. The strength of

chemical bonds varies considerably; there are "strong bonds" such as covalent orionic

bonds and "weak bonds" such as dipole-dipole interactions, the London dispersion

force and hydrogen bonding.

Ionic bonding

In ionic bonding, electrons are completely transferred from one atom to

another. In the process of either losing or gaining negatively charged electrons, the

reacting atoms form ions. The oppositely charged ions are attracted to each other by

electrostatic forces, which are the basis of theionic bond.

Ionic compounds share many features in common:

Ionic bonds form between metals and nonmetals. In naming simple ionic compounds, the metal is always first, the nonmetal

second (e.g., sodium chloride).

Ionic compounds dissolve easily in water and other polarsolvents. In solution, ionic compounds easily conduct electricity. Ionic compounds tend to form crystalline solids with high melting

temperatures.

Covalent bonding

The second major type of atomic bonding occurs

when atoms shareelectrons. As opposed to ionic bonding in which a complete transfer

of electrons occurs, covalent bonding occurs when two (or more) elementsshare

electrons. Covalent bonding occurs because the atoms in thecompound have a similar

tendency for electrons (generally to gain electrons). This most commonly occurs when

two nonmetals bond together. Because both of the nonmetals will want to gain
http://en.wikipedia.org/wiki/Atomhttp://en.wikipedia.org/wiki/Chemical_substancehttp://en.wikipedia.org/wiki/Electromagnetic_forcehttp://en.wikipedia.org/wiki/Electronshttp://en.wikipedia.org/wiki/Atomic_nucleushttp://en.wikipedia.org/wiki/Dipolehttp://en.wikipedia.org/wiki/Covalent_bondhttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Intermolecular_force#Dipole-dipole_interationshttp://en.wikipedia.org/wiki/London_dispersion_forcehttp://en.wikipedia.org/wiki/London_dispersion_forcehttp://en.wikipedia.org/wiki/Hydrogen_bondinghttp://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=853&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=883&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1545&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1546&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1546&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1517&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1565&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1571&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1510&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1517&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1517&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1510&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1571&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1565&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1517&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1546&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1546&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1545&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=883&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=853&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://en.wikipedia.org/wiki/Hydrogen_bondinghttp://en.wikipedia.org/wiki/London_dispersion_forcehttp://en.wikipedia.org/wiki/London_dispersion_forcehttp://en.wikipedia.org/wiki/Intermolecular_force#Dipole-dipole_interationshttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Covalent_bondhttp://en.wikipedia.org/wiki/Dipolehttp://en.wikipedia.org/wiki/Atomic_nucleushttp://en.wikipedia.org/wiki/Electronshttp://en.wikipedia.org/wiki/Electromagnetic_forcehttp://en.wikipedia.org/wiki/Chemical_substancehttp://en.wikipedia.org/wiki/Atom


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electrons, the elements involved will share electrons in an effort to fill their valence

shells. A good example of a covalent bond is that which occurs between two hydrogen

atoms. Atoms of hydrogen (H) have one valence electron in their firstelectron shell.

Since the capacity of this shell is two electrons, each hydrogen atom will "want" to

pick up a second electron. In an effort to pick up a second electron, hydrogen atoms

will react with nearby hydrogen (H) atoms to form the compound H2. Because the

hydrogen compound is a combination of equally matched atoms, the atoms will share

each other's single electron, forming one covalent bond. In this way, both atoms share

the stability of a full valence shell.

Multiple Bonds: For every pair ofelectrons shared between two atoms, a

single covalent bond is formed. Some atoms can share multiple pairs of electrons,

forming multiple covalent bonds. For example, oxygen (which has

six valence electrons) needs two electrons to complete its valence shell. When two

oxygen atoms form the compound O2, they share two pairs of electrons, forming two

covalent bonds.

Polar and nonpolar covalent bonding

There are, in fact, two subtypes ofcovalent bonds. The H2 molecule is a

good example of the first type of covalent bond, the nonpolar bond. Because

both atoms in the H2 molecule have an equal attraction (or affinity) forelectrons, the

bonding electrons are equally shared by the two atoms, and a nonpolar covalent bond

is formed. Whenever two atoms of the same elementbond together, a nonpolar bond

is formed.

A polar bond is formed when electrons are unequally shared between

twoatoms. Polar covalent bonding occurs because one atom has a stronger affinity for

electrons than the other (yet not enough to pull the electrons away completely and

form an ion). In a polar covalent bond, the bonding electrons will

spend a greater amount of time around the atom that has the stronger

affinity for electrons. A good example of a polarcovalent bond is the

hydrogen-oxygen bond in the watermolecule.

Watermolecules contain two hydrogen atoms (pictured in

red) bonded to one oxygen atom (blue). Oxygen, with six valence electrons, needs two

additional electrons to complete its valence shell. Each hydrogen contains one

electron. Thus oxygen shares the electrons from two hydrogen atoms to complete its
http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=851&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1540&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1563&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1563&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1517&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1518&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1510&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1552&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1518&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1518&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=851&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=851&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1518&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1518&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1552&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1510&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1518&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1517&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1563&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1509&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=852&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1563&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1540&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=851&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1550&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=http://www.visionlearning.com/library/pop_glossary_term.php?oid=1539&l=


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own valence shell, and in return shares two of its own electrons with each hydrogen,

completing the H valence shells.

From (online) http://www.visionlearning.com/library/module_viewer.php?mid=55accessed on October 22, 2011

VI. Procedures1. Comparing covalence and ion bonding

Test tube 1

5 drops of NaCl +

20 drops aquades

Test tube 2

20 drops CCl4

Added by 2 drops of AgNO3 Observe the changing and

note the time

Result
http://www.visionlearning.com/library/pop_glossary_term.php?oid=1563&l=http://www.visionlearning.com/library/module_viewer.php?mid=55http://www.visionlearning.com/library/module_viewer.php?mid=55http://www.visionlearning.com/library/pop_glossary_term.php?oid=1563&l=


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VII. Result of ObservingData of Experiment

No TreatmentResult

Before After1. a. Test Tube I colorless White dirty and theres

precipitate after adding AgNO3

b. Test Tube II colorless Colorless (no changing)2. a. when heated and adding the 2

drops of CCl4

White, solid Soluble into solution

b. Adding 3 drops of CCl4 Soluble into solution Theres precipitate (whitedirty)

c. Adding 20 drops of HNO3 White dirty Bright yellowd. Adding by 2 drops of AgNO3 Bright yellow White dirty, theres precipitate

3. a. Little pieces of C2H2O4 heated Solid, white, small Expand and has many fiber

b. Little pieces of C12H22O11 Solid, white, small Molten, changes into brown

VIII. AnalysisIn the first experiment, test tube I has precipitate in it because NaCl can

react with AgNO3. But in test tube II it doesnt. It show that ionic bonding react

faster than covalence. The color of test tube I is white dirty because there is

precipitate of AgCl. Test tube doesnt change because theres no reaction. The

reaction is:

NaCl + AgNO3 AgCl + NaNO3

CCl4 + AgNO3

So, NaCl is ionic bonding than CCl4 is covalence. Here we can notice that

ionic is more reactive than covalence. Ionic rearrange its structure easily but

covalence doesnt.

Second experiment, when CaO added by CCl4 there will be precipitate of

CaCO3. The reaction is:

3CaO + CCl4 2CaCl2 + CaCO3


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Then the adding of HNO3 will make the precipitate soluble. HNO3 will

make the gas evaporate and the color change into bright yellow. To check that it has

CaCl2 (ionic bonding), we drop AgNO3. Then the precipitate will form again. Thats

AgCl. The reaction is below.

CaCl2 + 2AgNO3 2AgCl + Ca(NO3)2

Third experiment, here we heat C2H2O4. This process will produce formic

acid. Formic acid has many fibers. The reaction can be notice by the smell that we

know from the experiment. It indicates theres reaction between C2H2O4 and O2. The

reaction is:

C2H2O4 CO2 + HCOOH

Then, when we heat sugar or sucrose (C12H22O11)we will produce caramel

or glucose (C6H12O6). We know that sugar is disaccharide than glucose is

monosaccharide. So, this reaction is dispersing the bonding from disaccharide into

monosaccharide. The reaction is below.

C12H22O11 + 6O2 5H2O + 6CO2 + C6H12O6

The color of sugar changes into brow and it liquids. This changing indicates

that theres reaction and the structure of it has rearange.

IX. DiscussionFrom our experiment we find the mistake especially in the second

experiment. Actually based on the theory, in the final result we will get precipitate

from the reaction between CaCl2 (aq) + 2 AgNO3 (aq) 2 AgCl(s) + Ca(NO3)2. AgNO3

is the precipitate that the color is white but in our experiment the precipitate is not so

visible. It case happened might be cause when we would give HNO3 to the test tube,

might be the test tube was still warm so that can be destroy the reaction and make it

does not react perfectly so finally the precipitate cannot be visible clearly. This might

also happen because the adding of AgNO3 is less. So, therere two possibility why

the precipitate doesnt visible perfectly.


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X. ConclusionBased the data that we have got from experiment, we can conclude some statements,

involves:

1. Ionic bonding reacts easily than covalence. Because ionic bonding disserve itsstructure easily. Covalence difficult to disserve its bonding.

2. Chlor is solid when it is in ionic bonding, but it is liquid or solution in covalencebonding. So in ionic, it will precipitate but in covalence its soluble. We can

dissolve the bonding by heating process, mixture the compound, etc. By dissolving

it, the new compound that formed is more simpler and has different kind of

bonding.

XI. Answer of Question1. Because ionic bonding can let go their electron easily and the ionization is easy

then on covalence bonding, they difficult to ionization and difficult to let go their

electron.

2. a. ocsalate acid = C2H2O4 b. sugar = C12H22O113. It will easily soluble in NH3. Because ethanol isnt good solvent. The result if we

put NaCl in NH3 will be ammonium chloride. But if we put NaCl in ethanol it will

be difficult to react.

XII. ReferencesVogel. 1990.Buku teks Analisis Kualitatif. Jakarta: PT Kalman Media Pustaka.

Tim Kimia Dasar. 2011.Petunjuk Praktikum Kimia Dasar. Surabaya: UNESAPress.

(online) http://id.wikipedia.org/wiki/Sukrosa accessed on October 22, 2011

(online) http://www.visionlearning.com/library/module_viewer.php?mid=55 accessed

on October 22, 2011

(online) http://rachmakimhunter.blogspot.com/p/kimia-organik.html accessed on

October 22, 2011

Surabaya, November 8, 2011

Known Student

Lecture/ Guidance Assistant

(..) (..)
http://id.wikipedia.org/wiki/Sukrosahttp://www.visionlearning.com/library/module_viewer.php?mid=55http://rachmakimhunter.blogspot.com/p/kimia-organik.htmlhttp://rachmakimhunter.blogspot.com/p/kimia-organik.htmlhttp://www.visionlearning.com/library/module_viewer.php?mid=55http://id.wikipedia.org/wiki/Sukrosa


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ATTACHMENT

First Experiment

a. Test Tube I = NaCl + AgNO3(White dirty) - left

b. Test Tube II CCl4 + AgNO3(colorless) - right

Second Experiment

1. Heated for 20 minutes = nochanging

2. Adding by CCl4 = white dirtyand precipitate

3. Heated and Adding HNO3 =bright yellow

4. Adding AgNO3 = white dirtyand precipitate again

1 2

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Third experiment

C2H2O4 heated

C2H2O4 heated

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