Chemistry: Animation, Video, and Laboratory Activity

Power From the Nucleus

2011-01-28T22:30:00.001-08:00

Nuclear Fission

Some large radioactive atoms can be made to behave in a different way. For example, an atom of uranium-235 splits into two separate atoms when it is struck by neutron. The splitting of an atom is called nuclear fission. Fission of a uranum-235 atom produce a krypton atom, barium atom and three neutron, as well as gamma rays. It also gives out a huge amount of heat energy.

A Chain Reaction

When uranium-235 is struck by neutron, uranium split into barium and krypton and three neutron. Three neutron will be struck another uranium atom, to produce nine neutron and will be struck another uranium atom. A reaction that grows in this way called a chain reaction. This one is very fast. In only fraction of a second, enormous amounts of heat and radiation are produced.

The Atomic Bomb

The chain reaction above is the basis of the atomic bomb. In atomic bomb, the chain reaction builds up until its get out of control. Then the bomb explodes, giving out intense heat, a violent shock wave and deadly burst of radiation. The earth is scorched and burned for miles around, the air is poisoned, and the living thing are killed. The full effect of atomic bomb is not felt in a day, or even a week. The products of the explosion are radioactive, and some of them have long half-lives. They settle to the earth and slowly decay, causing radiation sickness, cancer and death.

The world's first atomic bomb was dropped on Hiroshima, in Japan, in August 1945. It probably contained about 10 kilograms of uranium. It killed 80 000 people within a day and 60 000 more died within a year. Nowadays, some countries possess bombs that are 5000 times more powerfull!!!

Electrochemical cells: Volta cells

2010-11-12T19:43:00.000-08:00

Oxidation-reduction involve the transfer of electrons. The transfer of electrons between metals and metal ions is a common type of redox reaction. It's illustrates what happened when a strip of zinc is placed in a solution of copper(II) sulfate.

In this reaction there is a transfer of electrons from the zinc metal to the copper(II) ions. The transfers of electrons from Zn to Cu2+ takes place on the surface of the zinc strip. As the reaction proceeds the zinc metal dissolves and copper metal is formed. As the Cu2+ ions are reduced to Cu metal the blue coloured solution fades, eventually becoming colourless. The Cu2+ ions have a greater tendency to gain electrons than Zn2+ ions. As a result, Cu2+ ions will accept electrons from atoms Zn metal, resulting in the formation of Cu atoms and Zn2+ ions.
This reaction illustrates how all redox reactions are the result of competition for electrons.
If a strip of copper is placed in a solution of zinc sulfate no reaction occurs. This is because Zn2+ ions have a lesser tendency to gain electrons than Cu2+ ions. As a result, Cu atoms will not give up electrons to Zn2+ ions.
Redox reactions can be used to generate electricity if the two half-reactions are
physically separated. The electrons which are transferred can then pass through an external wire or circuit rather than being transferred through direct contact. A redox reaction in which the reactants are physically separated so that the transferred electrons can be directed through an external circuit is called an electrochemical cell.
One of the earliest electrochemical cell was the Daniel cell, developed in 1835. This
cell was based on the reactions between metallic zinc and copper(II) sulfate reviously described. The only difference is that half-reactions are physically separated so that the transferred electrons can be directed through an external circuit. In this way usable electrical energy can be degenerated.
The Daniel cell was extensively used for many years in telegraph and telephone work
as a reliable source of electricity. This electrochemical cell can be demonstrated by partly immersing zinc and copper strips in 1 mol L-1 solutions of zinc sulfate and copper(II) sulfatemrespectively in separate containers. The solutions are joined by a salt bridge which consists of U-tube filled with an electrolyte solution such as potassium nitrate. Each of two parts, consisting of a metal strip in an electrolyte solution, is called a half-cell.
When the metal strips are connected with a piece of wire an electric current flows
through the circuit. If a voltmeter is connected across the metal strips the voltmeter should read 1.1 volts. As the cell operates, the zinc strip dissolves slowly, while the copper strip becomes coated with more copper. The blue colour of the copper(II) sulfate solution fades and the voltage gradually falls.
These observations can be explained in terms of oxidation and reduction processes. The zinc loses electrons to form zinc ions according to the following equation.
Zn(s) --> Zn2+(aq) + 2e-
The zinc ions go into solution and hence the zinc strip gradually dissolves. The electrons given up by the zinc pass through the external circuit to the copper strip. There they are accepted by copper(II) ions in the solution surrounding the copper strip. The copper(II) ions are reduced to copper atoms which deposit on the strip forming a copper layer. The equation is as follows.
Cu2+(aq) + 2e- --> Cu(s)
The removal of Cu2+ ions from the solution causes the blue colour of the solution to fade.
Each time two electrons are released by a zinc atom in the left-hand half-cell, two
electrons are accepted by copper(II) ion in the other half-cell. Thus, for each zinc ion produced, a copper(II) ion is removed from solution. Electrical neutrality in the half-cell solutions is maintained by the migration of positive ions towards the copper half-cell and negative ions towards the zinc half cell. Thus Zn2+ ions move into the salt bridge and K+ ions move into the copper half-cell. At the same time, SO4 2h ions from the copper half-cell move into the salt bridge while NO3 ions move into the zinc half-cell. Thus, the flow of current through the external circuit is by movement of electrons through a metallic wire conductor and the flow of current in the internal circuit is by movement of ions.
The cell will continue to generate an electric current until chemical equilibrium is
reached. In this reaction the reactants are almost completely converted to products before equilibrium is achieved. At equilibrium most of the copper(II) ions will have been lost from the solution and the concentration of the zinc ions will be nearly double the original 1 mol L-1. The voltage, ore.m.f., drops to zero at equilibrium.
Any electrochemical cell consists of two half-cells. Each half-cell consists of an
electrode, which is a conductive metal or graphite strip in contact with an electrolyte solution.
The electrode at which oxidation takes place is called the anode. As electrons are generated by oxidation, the terminal of the anode is marked as the negative (-). The electrode at which reduction takes place is called the cathode. Because electrons are accepted in reduction, the terminal of the cathode is marked as the positive (+).
When the anode and cathode are connected, an electric current flows through the
external circuit. This electron flow can be used as source of energy to heat a lamp filament, run a motor, operate a transistor radio and so on. In other words, chemical energy is being used to generate electrical energy. Electrochemical cells, in which chemical change is used to generate electrical energy, are also called galvanic or voltaic cells.
An electrochemical cell does not necessarily have reactive metal electrodes. Consider
the cell in Figure 19.5 in which the platinum electrodes are chemically inert. hydrogen and chlorine gases are bubbled over the surfaces of the platinum electrodes as shown. In this cell the half-cells share a common electrolyte which is 1 mol L-1 hydrochloric acid. When the external circuit is connected by a voltmeter an e.m.f. of 1.36 V register on the voltmeter.

Collision theory and activation energy

2010-11-08T18:12:00.000-08:00

Although the factors affecting rates were discussed in the previous section, no consideration was given to what was actually happening at a molecular level during a reaction. The chemical equation for a reaction indicates the nature of the reactants and products but provides no information about the way in which thereactants are converted to products. For example, the decomposition of hydrogen iodide is represented by the following equation.

2HI → H2 + I2

This equation indicates that for every two molecules of HI which decompose, one molecule of H2 and one molecule of I2 are produced. However, the equation does not indicate how HI molecules are converted to H2 and I2. The first step in a chemical reaction is thought to involve a collision between the reactant particles. This idea is part of the collision theory of reaction undergo an
appropriate collision.
From the kinetic theory, the particles in a gas are in a continuous state of random straight-line motion. While most of the particles have energies that are close to the average for all the particles in the system, a small fraction have energies much lower or much higher than the average. Because of this range of kinetic energies, collision between HI molecules will occur with differing energies. A collision between reactant molecules does not necessarily mean that a
reaction will take place. In fact, most collisions do not bring about a reaction. The collision theory requires that for a collision between reactant particles to lead to a chemical reaction the following conditions must be fulfilled.
1. The molecules must collide with sufficient energy to disrupt the bonds of the reactant molecules.
2. The molecules must collide with an orientation that is suitable for the breaking
For a reaction to occur between reactant molecules they must collide with a certain minimum energy. Unless this minimum collision energy is exceeded, the colliding molecules will simply rebound and move away from each other. The minimum energy that is required for a collision to result in a reaction is known as the activation energy for the particular reaction. Some reactions have relatively low activation energies and so react at a significant rate at room temperature. For these reactions, a noticeable reaction occurs as soon as the reactants are mixed. For example, a piece of sodium metal placed in water at room temperature produces a violent reaction almost instantaneously. Other reactions occur to an almost insignificant extent at room temperature. In such reactions the activation energy is so high that it is very unlikely that reactant molecules will collide with sufficient energy to undergo reaction. For example, methane will not react with oxygen unless the mixture is ignited. There is a relatively high activation energy for the reactions there would be in the order of 1010 collisions per second between
reactant molecules, virtually none of these would have sufficient energy for a reaction to take place.
As well as needing a minimum amount of energy, successful collisions also often have an orientation requirement. The relative orientations of the reactant molecules during a collision must be favorable for the breaking of particular bonds in the reactants and the formation of new bonds in the products. This factor also contributes to the fact that many collisions between reactants are unsuccessful in producing a reaction.

The Effect of ChangingThe Temperature of Equilibrium System

2010-11-04T20:09:00.000-07:00

The effect of changing the temperature of equilibrium system can be predicted from a knowledge of the heats of reaction. If the temperature of a system is lowered, the exothermic reaction is favoured. If the temperature isincreased, the endhotermic reaction is favoured.

For the N2O4/NO2 system the forward reaction is endothermic.

N2O4 + 57 kJ <===> NO2

The forward reaction therefore absorbs heat from the surroundings and the reverse reaction releases heat to the surroundings. According to Le Chatelier’s principle, if the temperature of an equilibrium system is increased the system will adjust to re-establish equilibrium in such a way as to decrease the temperature. Therefore in re-establishing equilibrium the endothermic reaction is favoured as this absorbs heat from the surroundings and would tend to decrease the temperature. In the N2O4/NO2 system this would result in an increase in the concentration of NO2 and a decrease in the cpncentration of N2O4.
If the temperature of the equilibrium system was reduced the system would re-establish equilibrium by favouring the exothermic reaction. This would tend to increase the temperature of the surroundings, partially counteracting the change. In the N2O4/NO2 system, more N2O4 and less NO2 would be present when equilibriuym was re-established.

View the demonstration video

The History of Chemistry

2010-11-04T15:58:00.000-07:00

Chemistry has evolved over thousands of years to become the sophisticated science it is today. As long ago as 3500 B.C., the early Egyptians were skilled in the production of wine and had discovered that certain metals such as copper and tin could be obtained by roasting metal ores in a fire with charcoal.
By about 1500 B.C., the Hittites discovered that when iron and charcoal are heated a much harder from of iron is produced. This material, which is today called steel, was used to produce a range of tools and weapons.
The Greek philosophers, including Democritus and Aristotle, were the first to attempt to understand the nature of matter. In fact, Democritus proposed the existence of atoms. He believed that the universe consisted of one kind of atom of varying sizes and shapes. About 350 B.C., Aristotle rejected the idea of atoms. He considered that the matter consisted of different proportions of four elements – earth, water, air and fire. Thisview of ma tter dominated Western scientific thought for about 2000 years until the development of modern chemistry.
In the period A.D. 500 – 1600 attention shifted from an interest in the nature of matter to more practical concerns. The ‘chemists’ of that time, better known as the alchemists, had two main aims. The first was to find a method of converting metals such as iron, zinc and copper into gold. The second aim was to discover an ‘elixir of life’ which would prolong life indefinitely. The alchemists relied heavily on experimentation but their activities were not guided by the development of scientific theories. As well, much of their work was done in secret and their findings were not subject to the opendebate which is characteristic of science today.
Despite the limitations of the alchemists’ approach, many important chemical substances were produced in this period. These included alcohol, arsenic, zinc, and hydrochloric, sulfuric and nitric acid.

Rutherford Atomic Model

2010-11-04T15:28:00.000-07:00

By the early 1900s, it was clear that each atom contains regions of both positive and negative charge. The question was, how are these charges distributed? The dominant view of that time was summarized in J. J. Thomson’s model of the atom; the positive charge was assumed to be distributed evenly throughout the atom. The negative charges were pictured as being imbedded in the atom like plums in a pudding (the “plum pudding model”). Soon after Thomson developed his model, tremendous insight into atomic structure was provided by one of Thomson’s former students, Ernest Rutherford (1871–1937), who was the outstanding experimental physicist of his time.

By 1909, Ernest Rutherford had established that alpha particles are positively charged particles. They are emitted at high kinetic energies by some radioactive atoms, that is, atoms that disintegrate spontaneously. In 1910, Rutherford’s research group carried out a series of experiments that had an enormous impact on the scientific world. They bombarded a very thin piece of gold foil with alpha-particles from a radioactive source. A fluorescent zinc sulfide screen was placed behind the foil to indicate the scattering of the alpha-particles by the gold foil (Figure 5-4). Scintillations (flashes) on the screen, caused by the individual alpha-particles, were counted to determine the relative numbers of alpha-particles deflected at various angles. Alpha particles were known to be extremely dense, much denser than gold.
If the Thomson model of the atom were correct, any alpha-particles passing through the foil would have been deflected by very small angles. Quite unexpectedly, nearly all of the alpha-particles passed through the foil with little or no deflection. A few, however, were deflected through large angles, and a very few -particles even returned from the gold foil in the direction from which they had come! Rutherford was astounded. In his own words, It was quite the most incredible event that has ever happened to me in my life. It was almost as if you fired a 15-inch shell into a piece of tissue paper and it came back and hit you.
Rutherford’s mathematical analysis of his results showed that the scattering of positively charged alpha-particles was caused by repulsion from very dense regions of positive charge in the gold foil. He concluded that the mass of one of these regions is nearly equal to that of a gold atom, but that the diameter is no more than 1/10,000 that of an atom. Many experiments with foils of different metals yielded similar results. Realizing that these observations were inconsistent with previous theories about atomic structure, Rutherford discarded the old theory and proposed a better one. He suggested that each atom contains a tiny, positively charged, massive center that he called an atomic nucleus. Most alpha-particles pass through metal foils undeflected because atoms are primarily empty space populated only by the very light electrons. The few particles that are deflected are the ones thatcome close to the heavy, highly charged metal nuclei.
Rutherford was able to determine the magnitudes of the positive charges on the atomic nuclei. The picture of atomic structure that he developed is called the Rutherford model of the atom.

"Atoms consist of very small, very dense positively charged nuclei surrounded by clouds of electrons at relatively great distances from the nuclei".

To download animation of Rutherford experiment click here

Milikan Experiment Animation

2010-11-03T01:42:00.000-07:00

Once the charge-to-mass ratio for the electron had been determined, additional experiments were necessary to determine the value of either its mass or its charge, so that the other could be calculated. In 1909, Robert Millikan (1868–1953) solved this dilemma with the famous “oil-drop experiment,” in which he determined the charge of the electron.

The Millikan oil-drop experiment. Tiny spherical oil droplets are produced by an atomizer. The mass of the spherical drop can be calculated from its volume (obtained from a measurement of the radius of the drop with a microscope) and the known density of the oil. A few droplets fall through the hole in the upper plate. Irradiation with X-rays gives some of these oil droplets a negative charge. When the voltage between the plates is increased, a negatively charged drop falls more slowly because it is attracted by the positively charged upper plate and repelled by the negatively charged lower plate. At one particular voltage, the electrical force (up) and the gravitational force (down) on the drop are exactly balanced, and the drop remains stationary. Knowing this voltage and the mass of the drop, we can calculate the charge on the drop.

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Limiting Reagent

2010-11-03T01:05:00.001-07:00

From the balanced equation for a chemical reaction it is possible to calculate the exact quantities of reactants which are consumed and products which are formed. For example, consider the reaction between nitrogen momooxide gas and oxygen gas to form nitrogen dioxide. The equation for the reaction is :

3 NO (g) + O2 (g) → 3 NO2 (g)

From the equation it is evident that every mole of O2 which reacts, three moles of NO are needed and three moles of NO2 will be produced. However, consider the situation where the ratio of coefficients in the balanced chemical equation. In this situation, one of the reactants will be the limiting reagent and the other will be present in excess.

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The Hydrogen Spectrum

2010-11-03T00:43:00.000-07:00

If electricity is passed through a discharge tube containing hydrogen gas at very low pressure, the hydrogen molecules are split into individual atoms.these excited hydrogen emit a violet light which, when passed through a prism, produces a specrtum consisting of a series of bright lines separated by dark spaces.

The spectrum produces is called a line emission spectrum and indicates that excited atoms emit light of certain frequencies only. The occurrence of line emission spectra for hydrogen and other elements could not be satisfactorily explained in terms of classical physics at the beginning of the twentieth century. To account for these observations a radical revision of the laws and theories of physics was required.

To Download The Hydrogen Spectrum click here

Source of animation from Learnestv.com

Formation of Solution

2010-11-03T00:29:00.000-07:00

An electrolyte is a substance that produces ions in solution. For example, when sodium chloride is dissolved in water the ionic lattice of Na+ and Cl- ions breaks up to form separate Na+ and Cl- ions which are surrounded by water molecules. This can be represented as follows.

NaCl (s) → Na+(aq) + Cl-(aq)

This process is known as dissociation. The ions in the ionic solid have been separated in the solution process.

Download Free Formation of Solution

Properties Of Gasses Animation

2010-11-03T00:17:00.000-07:00

In gases the particles are widely spaced and move virtually independently of one another. Because of this a gas will become dispersed throughout any container into which it is placed. Also diffusion can occur rapidly. Gases are very compressible because the particles are relatively widely spaced compared with the size of the particles.

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Rutherford Experiment Animation

2010-11-02T23:55:00.000-07:00

The Geiger-Marsden experiment (also called the Gold foil experiment or the Rutherford experiment) was an experiment done by Hans Geiger and Ernest Marsden in 1909, under the direction of Ernest Rutherford at the Physical Laboratories of the University of Manchester which led to the downfall of the plum pudding model of the atom. They measured the deflection of alpha particles (helium ions with a positive charge) directed normally onto a sheet of very thin gold foil. Under the prevailing plum pudding model, the alpha particles should all have been deflected by, at most, a few degrees. However they observed that a very small percentage of particles were deflected through angles much larger than 90 degrees; some were even scattered back toward the source. From this observation Rutherford concluded that the atom contained a very physically-small (as compared with the size of the atom) positive charge, which could repel the alpha particles if they came close enough, subsequently developed into the Bohr model.

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Source: Learnestv.com

Le Chatelier’s Principle Animation

2010-11-02T23:35:00.000-07:00

The effect of various changes on equilibrium systems can be predicted using the principle developed by the French chemist Henri Le Chatekier. Le Chatelier’s principle can be stated as follows.

‘If a chemical system at equilibrium is subjected to a change in conditions, the system will adjust to re-establish equilibrium in such a way as to partially counteract the imposed change.’

To download this Le Chatelier’s Principle Animation click here

Animation source from Learnestv.com

Development of Atomic Theory

2010-03-31T10:55:00.001-07:00

Development of Atomic Theory
1. Democritus (440 B.C)
  Atom – came from the word "atomos" which means small, indivisible particles
1. Antoine Lavoisier (1774)
  Law of Conservation of Mass – mass can neither be created nor destroyed in chemical reactions
  Example :
  3.25 g + 3.32 g = 6.57 g
Hg(NO₃)_2(aq) + 2KI_(aq)
à HgI_2(s) + 2KNO_3(aq)

4.55 g + 2.02 g = 6.57 g
1. Joseph Proust (1799)
  Law of Constant Composition – Different samples of a pure chemical substance always contain the same proportion of elements by mass.
  By mass, water is: 88.8 % oxygen
  11,2 % hydrogen
1. John Dalton (1808)
  Dalton's Atomic Theory
  1. All matter consists of tiny particles called atoms.
  2. An atom cannot be created, divided, destroyed, or converted to any other type of atom.
  3. Atoms of a particular element have identical properties
  4. Atoms of different elements have different properties
  5. Atoms of different elements combine in simple whole-number ratios to produce compounds.
  6. Chemical change involves joining, separating, or rearranging
  Law of Multiple Proportions - Elements can combine in different ways to form different substances, whose mass ratios are small whole-number multiples of each other.
To download complete the development of atomic structure please click here!!!

Download Free Lesson Plan (RPP verswi bahasa inggris) untuk SMA

2010-03-27T21:11:00.000-07:00

Download free Lesson plan for High School:
1. Acid and Base
2. Solubility and Solubility product (Ksp)
3. Atomic Structure
4. Colloid
5. Hydrolysis
6. Chemical Equilibrium
7. Thermochemistry
8. Reaction Rate

9. Chemical bond

10. Chemical periodicity

11. Hydrocarbon

12. Management of laboratory

13. Reduction and oxidation (redox) reaction

14. stoichiometry

15. stoichiometry (II)

Chemical Equation

2010-01-06T00:49:00.000-08:00

Why reactant can be change into product ? It can be explained by CHEMICAL REACTION

When atoms, molecules, or ions regroups to form the other substances, chemist use a shorthand type expression. The expression is called Chemical Equation

Chemical equation can describe the chemical change. Formulas indicate all substances involved and their composition.

For example, the equation for the reaction of Hydrogen with oxygen to form water.
2H2 + O2 -> 2H2O
The formula for the reactants are written to the left arrow, and the formulas for the products are written to the right.
The arrow is read as “gives”, “produces”, “yields”, or “ forms”.
A plus sign on the left side of an equation means ‘reacts with’.
Coefficient of reaction is the ratio between a substances involved in the reaction.
Look at this reaction :
2H2 + 1 O2 -> 2H2O
For example above, coefficient reaction shows that 2 molecules of Hydrogen react with one molecule of oxygen to form 2 molecules of water.
Since matter cannot be created or destroyed in a chemical reaction, a chemical equation must have the same number of atoms in the products as there are in the reactants.
From the example above, we can look that the number of hydrogen atom in the left side is same as the right one, is 4. Either, the number of oxygen atom in the left side is same as the right one, is 2. This equation is called balanced equation
For balancing the chemical equation, can’t determine by change index number.
Index number determines the formula of substances, so that if we change index number as like as we change the kind of substances.
Coefficient number related with a number of substances, so if we change coefficient number that we only change the number of substances.
2H2 + O2 -> 2H2O
This reaction can’t be balanced by change index O in H2O become 2, so the reaction :
2H2 + O2 -> H2O2

There are 3 steps to write a balanced equation, they are:
• Write the word equation consist of name and the form of reactants and products.
• Write the formula equation consists of a chemical formula of reactants and products complete with the phase.
• Balancing, gives a correct coefficient so that it has the same number of atoms in the products and reactants.
Example :
a. Aluminum reacts with sulfuric acid solution to form aluminum sulfate solution and hydrogen gases. Balanced the reaction!
Answer :
Step 1 : write the word equation
aluminum + sulphuric acid solution à aluminum sulphate solution + hydrogen gases
Step 2 : write the formula equation
Al(s) + H2SO4(aq) ->à Al2(SO4)3(aq)+ H2(g)
Step 3 : balancing
2Al(s) + 3H2SO4(aq) -> Al2(SO4)3(aq)+ 3H2(g) Balance

Balancing the chemical equation
1 Determine one of substances (a substances which has a complex chemical formula). Give assign 1 in it. And the other, you can give assign with other characters.
2 Balance a substances related with a substances which given assign 1 first.
3 Balance the other substances. It will easier if oxygen atom is balanced first.
Example :
b. The reaction of aluminum and hydrochloric acid solution to form aluminum chloride solution and hydrogen gases
Al(s) + HCl(aq) -> AlCl3(aq)+ H2(g) not balanced
Step 1 : determine coefficient of AlCl3 = 1, and letter for the other
aAl(s) + bHCl(aq) -> 1AlCl3(aq)+ cH2(g)
Step 2 : balance aluminum and chlorine atom
The number of Al atom in the left side = a, while in the right side = 1, so a = 1
The number of Cl atom in the left side = b, while in the right side = 3, so b = 3
1Al(s) + 3HCl(aq) ->à 1AlCl3(aq)+ cH2(g)
Step 3 : balance Hydrogen atom
The number of hydrogen atom in the left side =3
In the right side = 2c, so c = 1,5
1Al(s) + 3HCl(aq) -> 1AlCl3(aq)+ 1,5H2(g)
Final balance equation : 2Al(s) + 6HCl(aq) -> 2AlCl3(aq)+ 3H2(g)

Doubled Multiple Law (Dalton’s Law)

2010-01-06T00:48:00.000-08:00

Doubled multiple law related to a pair of element can form more than one compound.

Example : Carbon atom and Oxygen atom can form CO2 and CO.

If the mass one of the element in two compounds is same, so that differing masses in other element in this compound is a simple integer. It’s call Doubled Multiple Law ( Dalton’s Law)

Example Problem 1 :

a. Sulfur (S) and Oxygen (O) form two kinds of compounds. The percent of mass in two compounds is 50 % and 40 %. Is this statement appropriate with Dalton’s Law ?

Solution :
Compound I contain 50 % sulfur, so the mass of oxygen is 50 %
Compound II contain 40 % sulfur, so the mass of oxygen is 60 %
Differing mass between S : O in compound I = 50 : 50 = 1 : 1
Differing mass between S : O in compound II = 40 : 60 = 1 : 1,5
Differing mass between S : O in compound II = 40 : 60 = 1 : 1,5
The compound appropriate with Dalton’s Law

Halloween Reaction or Old Nassau Reaction

2009-09-30T20:32:00.000-07:00

Halloween Reaction or Old Nassau Reaction
Orange and Black Clock Reaction

By Anne Marie Helmenstine, Ph.D., About.com

The Old Nassau or Halloween reaction is a clock reaction in which the color of a chemical solution changes from orange to black. Here's how you can do this reaction as a chemistry demonstration and a look at the chemical reactions that are involved.

Halloween Reaction Materials

* water
* soluble starch
* sodium metabisulphite (Na2S2O5)
* mercury(II) chloride
* potassium iodate (KIO3)

Prepare the Solutions

* Solution A: Mix 4 g soluble starch in a couple milliliters of water. Stir the starch paste into 500 ml boiling water. Allow the mixture to cool to room temperature. Add 13.7 g of sodium metabisulphite. Add water to make 1 liter of solution.

* Solution B: Dissolve 3 g mercury(II) chloride in water. Add water to make 1 liter of solution.

* Solution C: Dissolve 15 g potassium iodate in water. Add water to make 1 liter of solution.

Perform the Demonstration

1. Mix 50 ml solution A with 50 ml of solution B.

2. Pour this mixture into 50 ml of solution C.

The color of the mixture will change to an opaque orange color after a few seconds as the mercury iodide precipitates. After another few seconds the mixture will turn blue-black as the starch-iodine complex forms.

If you dilute the solutions by a factor of two then it takes longer for the color changes to occur. If you use a smaller volume of solution B the reaction will proceed more rapidly.

Chemical Reactions

1. Sodium metabisulfite and water react to form sodium hydrogen sulfite:

Na2S2O5 + H2O --> 2 NaHSO3

2. Iodate(V) ions are reduced to iodide ions by the hydrogen sulfite ions:

IO3- + 3 HSO3- --> I- + 3 SO42- + 3 H+

3. When the concentration of iodide ions becomes sufficent for the solubility product of the HgI2 to exceed 4.5 x 10-29 mol3 dm-9, then orange mercury(II) iodide precipitates until the Hg2+ ions are consumed (assuming an excess of I- ions):

Hg2+ + 2 I- --> HgI2 (orange or yellow)

4. If I- and IO3- ions remain, then an iodide-iodate reaction takes place:

IO3- + 5 I- + 6 H+ --> 3 I2 + 3 H2O

5. The resulting statch-iodine complex is black to blue-black:

I2 + starch --> a blue/black complex

Make Fake Blood

2009-09-30T20:28:00.000-07:00

What You Need:

* 1 c (250mL) peanut butter
* 1 qt. (1 L) corn syrup
* 1/2 cup (125mL) soap
* 1 oz (30mL) red color
* 15 drops blue food color

Here's How:
1. Mix creamy peanut butter with a sufficient amount of white corn syrup to make a runny mixture.
2. Add (non-sudsy) soap and food colors and mix well.
3. Stir more corn syrup in until the desired consistency is reached.
4. Refrigerate unused blood in an airtight container.

Tips:

1. Inexpensive white corn syrup is said to be thicker and more suitable for the fake blood than its costlier relatives.

Absorb Chemistry

2009-09-30T08:42:00.000-07:00

Absorb Chemistry is an interactive course written by Lawrie Ryan, the best selling author of 'Chemistry for You'. It's ideal for use on a whiteboard in front of a whole class or by students by themselves.

Absorb Chemistry is divided into units, so you can follow the course all the way through, or use the units individually. Each unit provides a compelling narrative supported by interactive animations, our unique simulations, videos of key experiments, and exercises to ensure concepts have been understood.
Try the free sample units in your class. Also try downloading SCORM-compliant sample units for use in your VLE or learning management system.
Absorb Chemistry Resources

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Colored Fire - Where to Find Metal Salts

2009-07-10T21:30:00.000-07:00

Fire Color - Source

Green - Boric acid is probably your best source of "green". Boric acid most commonly is sold as a disinfectant in the pharmacy section of a store. Copper sulfate is another metal salt that produces green fire. You can find copper sulfate, usually diluted in liquid form, in products used to control algae in pools or ponds.

White - Magnesium compounds can lighten a flame color to white. You can add Epsom salts, which are used for a variety of household purposes. I usually see Epsom salts sold in the pharmacy section of stores for use as a bath soak.
Yellow - Your usual fire will be yellow already, but if you are burning a fuel that produces a blue flame, for example, you can turn it from green to yellow by adding sodium salt, such as common table salt.

Orange - Calcium chloride produces orange fire. Calcium chloride is sold as a dessicant and as a road de-icing agent. Just be sure the calcium chloride isn't mixed with sodium chloride or else the yellow from the sodium will overpower the orange from the calcium.

Red - Strontium salts produce red colored fire. The easiest way to get strontium is to break open a red emergency flare, which you can find in the automotive section of stores. Road flares contain their own fuel and oxidizer, so this material burned vigorously and very brightly.

Purple - Purple or violet flames may be produced by adding potassium chloride to the fire. Potassium chloride is sold as lite salt or salt substitute in the spice section of the grocery store.

Blue - You can get blue fire from copper chloride. I am not aware of a widely-available source of copper chloride. You can produce it by dissolving copper wire (easy to locate) in muriatic acid (sold in building supply stores). This would be an outdoors-only type of reaction and not something I really recommend doing unless you have a little chemistry experience... but if you're determined, dissolve a piece of copper in a solution of 3% hydrogen peroxide (sold as a disinfectant) to which you have added sufficient muriatic acid (hydrochloric acid) to make 5% HCl solution.

Do you know of other sources of metal salts that can be used to color fire? If so, please add your comments in response to this post.

Nanocrystalline Materials

2009-05-20T20:16:00.000-07:00

Included here are ceramics, metals, and metal oxide nanoparticles. In the last two decades a class of materials with a nanometer-sized microstructure have been synthesized and studied. These materials are assembled from nanometer-sized building blocks, mostly crystallites. The building blocks may differ in their atomic structure, crystallographic orientation, or chemical composition. In cases where the building blocks are crystallites, incoherent or coherent interfaces may be formed between them, depending on the atomic structure, the crystallographic orientation, and the chemical composition of adjacent crystallites.

In other words, materials assembled of nanometer-sized building blocks are microstructurally heterogeneous, consisting of the building blocks (e.g. crystallites) and the regions between adjacent building blocks (e.g. grain boundaries). It is this inherently heterogeneous structure on a nanometer scale that is crucial for many of their properties and distinguishes them from glasses, gels, etc. that are microstructurally homogeneous.3

Grain boundaries make up a major portion of the material at nanoscales, and strongly affect properties and processing. The properties of NsM deviate from those of single crystals (or coarsegrained polycrystals) and glasses with the same average chemical composition. This deviation results from the reduced size and dimensionality of the nanometer-sized crystallites as well as from the numerous interfaces between adjacent crystallites. An attempt is made to summarize the basic physical concepts and the microstructural features of equilibrium and non-equilibrium NsM.

Nanocrystallites of bulk inorganic solids have been shown to exhibit size dependent properties, such as lower melting points, higher energy gaps, and nonthermodynamic structures.4,5 In comparison to macro-scale powders, increased ductility has been observed in nanopowders of metal alloys.6,7 In addition, quantum effects from boundary values become significant leading to such phenomena as quantum dots lasers.

One of the primary applications of metals in chemistry is their use as heterogeneous catalysts in a variety of reactions. In general, heterogeneous catalyst activity is surface dependent. Due to their vastly increased surface area over macro-scale materials, nanometals and oxides are ultra-high activity catalysts. They are also used as desirable starting materials for a variety of reactions, especially solid-state routes. Nanometals and oxides are also widely used in the formation of nanocomposites. Aside from their synthetic utility, they have many useful and unique magnetic, electric, and optical properties.8,9

Transmutation of elements

2009-05-18T22:06:00.000-07:00

Transmutation of elements, conversion of one chemical element into another. The expression has both historical and contemporary significance. The transmutation of certain metals into gold by means of a substance called the philosopher's stone was one of the two most ambitious quests of the alchemists (see alchemy); the other was for the elixir of life that would cure all diseases, restore youth to the aged, and make youthfulness eternal. The possibility of finding the philosopher's stone harmonized with ideas long generally held, and honest and able men were hopeful of finding it. Now and then a charlatan professed to have found it.
In modern times it has been found that a transmutation from one element to another actually does occur in the process of natural radioactivity. Transmutation of elements can be achieved artificially by the bombardment of elements with high-speed particles by means of such machines as the cyclotron (see particle accelerator). Both artificial and natural transmutations involve changing the number of protons in the atomic nucleus. The transuranium elements are created in this manner. When a nucleus is bombarded with neutrons from an atomic pile or nuclear reactor, some of the neutrons will be absorbed, resulting in an unstable nucleus. The nucleus then becomes more stable by converting one of its neutrons into a proton by beta decay, becoming a nucleus of the next heavier element in the process.

Dalton's Atomic Theory

2009-05-17T20:29:00.000-07:00

It was in the early 1800s that John Dalton, an observer of weather and discoverer of color blindness among other things, came up with his atomic theory. Let's set the stage for Dalton's work. Less than twenty years earlier, in the 1780's, Lavoisier ushered in a new chemical era by making careful quantitative measurements which allowed the compositions of compounds to be determined with accuracy. By 1799 enough data had been accumulated for Proust to establish the Law of Constant Composition ( also called the Law of Definite Proportions). In 1803 Dalton noted that oxygen and carbon combined to make two compounds. Of course, each had its own particular weight ratio of oxygen to carbon (1.33:1 and 2.66:1), but also, for the same amount of carbon, one had exactly twice as much oxygen as the other. This led him to propose the Law of Simple Multiple Proportions, which was later verified by the Swedish chemist Berzelius. In an attempt to explain how and why elements would combine with one another in fixed ratios and sometimes also in multiples of those ratios, Dalton formulated his atomic theory.

The idea of atoms had been proposed much earlier. The ancient Greek philosophers had talked about atoms, but Dalton's theory was different in that it had the weight of careful chemical measurements behind it. It wasn't just a philosophical statement that there are atoms because there must be atoms. His atomic theory, stated that elements consisted of tiny particles called atoms. He said that the reason an element is pure is because all atoms of an element were identical and that in particular they had the same mass. He also said that the reason elements differed from one another was that atoms of each element were different from one another; in particular, they had different masses. He also said that compounds consisted of atoms of different elements combined together. Compounds are pure substances (remember they cannot be separated into elements by phase changes) because the atoms of different elements are bonded to one another somehow, perhaps by hooks, and are not easily separated from one another. Compounds have constant composition because they contain a fixed ratio of atoms and each atom has its own characteristic weight, thus fixing the weight ratio of one element to the other. In addition he said that chemical reactions involved the rearrangement of combinations of those atoms.

So that, briefly, is Dalton's theory. With modifications, it has stood up pretty well to the criteria that we talked about earlier. It did not convince everyone right away however. Although a number of chemists were quickly convinced of the truth of the theory, it took about a half century for the opposition to die down, or perhaps I should say die off.

Let me point out again the difference between a model of atoms and a theory of atoms. A model focuses on describing what the atoms are like, whereas the theory not only talks about what the atoms are like but how they interact with one another and so forth. Dalton's model was that the atoms were tiny, indivisible, indestructible particles and that each one had a certain mass, size, and chemical behavior that was determined by what kind of element they were. We will use that model of an atom for now, but we will modify it considerably in a later lesson.

Green Chemistry

2009-03-22T21:10:00.006-07:00

Green chemistry, also called sustainable chemistry, is a chemical philosophy encouraging the design of products and processes that reduce or eliminate the use and generation of hazardous substances. Whereas environmental chemistry is the chemistry of the natural environment, and of pollutant chemicals in nature, green chemistry seeks to reduce and prevent pollution at its source. In 1990 the Pollution Prevention Act was passed in the United States. This act helped create a modus operandi for dealing with pollution in an original and innovative way. It aims to avoid problems before they happen.

As a chemical philosophy, green chemistry derives from organic chemistry, inorganic chemistry, biochemistry, analytical chemistry, and even physical chemistry. However, the philosophy of green chemistry tends to focus on industrial applications. Click chemistry is often cited as a style of chemical synthesis that is consistent with the goals of green chemistry. The focus is on minimizing the hazard and maximizing the efficiency of any chemical choice. It is distinct from environmental chemistry which focuses on chemical phenomena in the environment.

In 2005 Ryoji Noyori identified three key developments in green chemistry: use of supercritical carbon dioxide as green solvent, aqueous hydrogen peroxide for clean oxidations and the use of hydrogen in asymmetric synthesis.[1] Examples of applied green chemistry are supercritical water oxidation, on water reactions and dry media reactions..

Bioengineering is also seen as a promising technique for achieving green chemistry goals. A number of important process chemicals can be synthesized in engineered organisms, such as shikimate, a Tamiflu precursor which is fermented by Roche in bacteria.

From: http://en.wikipedia.org/wiki/Green_chemistry

How does chemistry affect our daily lives?

2009-03-22T21:10:00.005-07:00

Chemistry is everywhere, and we use all the time in our daily lives, probably without knowing it.

Here are some things that wouldn't be possible without the field of chemistry.

No plastic. That's no plastic bags, no CDs or DVDs, no iPods, no plastic silverware or plastic cups and plates, no scotch tape, no styrofoam, no synthetic fabics (like nylon, fleece, rayon, and kevlar). Most of your car is made of plastic too.

No gasoline. No driving fancy cars!

No pharmaceuticals. Modern medicine wouldn't exist. No aspirin, no pain killers!

No water purification. Drinking water would make you sick half the time. Most of sewage treatment is done using chemistry.

No synthetic fertilizers. Farming and food production wouldn't be nearly as productive and starvation would be a massive problem. Insecticides are also made by chemists.

No paint. No cosmetics. No processed foods. No air conditioning. No refrigeration. No soap and cleaning products. No photography. No televisions. No radios. No computeres. No glue. No batteries. No electricity in your house.

There's probably nothing you've done today that wasn't made thanks to chemistry. You'd pretty much have to go back to living in a cave to get away from it!
From: http://wiki.answers.com/Q/How_does_chemistry_affect_our_daily_lives

Download Free Chemistry and Physics Books and Flash Animation

2009-03-16T07:51:00.002-07:00

Download Free Chemistry and Physics Books and Flash Animation...

You can download FREE chemistry and physics book in this blog. Beside e-book you also can download free animation flash. List of chemistry animation:

I wish, in the next future this blog can be usefull to all. Amin...

Selamat Datang

2009-03-13T00:44:00.001-07:00

Selamat datang di komunitas kimia unnes. Untuk yang berminat tinggalkan saja alamat e-mail, friendster, face book atau apalah lainnya. Semoga bermanfaat....