Srinivas Chemistry: 2013-03-03

Chemical Compounds -Most Important

Chemical Compounds -Most Important
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Inorganic Chemistry - IITJEE

Inorganic Chemistry - IITJEE

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Solids are usually hard because their molecules have been packed together. The closer your molecules are, the harder you are. Solids also can hold their own shape. A rock will always look like a rock unless something happens to it. The same goes for a diamond. Even when you grind up a solid into a powder, you will see little tiny pieces of that solid under a microscope. Liquids will move and fill up any container. Solids like their shape.
In the same way that a solid holds its shape, the atoms inside of a solid are not allowed to move around too much. This is one of the physical characteristics of solids. Atoms and molecules in liquids and gases are bouncing and floating around, free to move where they want. The molecules in a solid are stuck. The atoms still spin and the electrons fly around, but the entire atom will not change position.
Solids can be made up of many things. They can have pure elements or a variety of compounds inside. When you get more than one type of compound in a solid it is called a mixture. Most rocks are mixtures of many different compounds. Concrete is a good example of a manmade mixture

Q2 what is crystalline?

Ans A crystal or crystalline solid is a solid material whose constituent atoms, molecules, or ions are arranged in an orderly repeating pattern extending in all three spatial dimensions

Interactive Periodic Table

In this interactive periodic table animation you can view details of all elements by clicking on it. You can select the colored by option at bottom left to view the corresponding categories. By clicking the test yourselves option (checkmark )you can test your knowledge of elements.

Hookies Law Simulation

Hookes Law simulation. See how changing the bond strength or the masses attached to a bond influences the frequency of the vibration

Conformation Energy Profile for Butane C2-C3 Bond Rotation

Conformation energy profile for butane C2-C3 bond rotation. See how the energy of an butane molecule varies as the groups rotate around the C2-C3 bond

Conformation Energy Profile For Ethane

Conformation energy profile for ethane. See how the energy of an ethane molecule varies as the groups rotate around the C-C bond

Visualisation Of Hybrid Orbitals From C Atom

Visualisation of hybrid orbitals from C atomic orbitals . See the relationship of atomic orbitals in sp3, sp2 and sp hybrid sets

Electron Density Vs Internuclear Distance

Electron density vs internuclear distance for the formation of H2 from 2 H atoms. See how the electron density varies as two H atoms approach each other.

Milikan Oil Drop Experiment

The purpose of Robert Millikan and Harvey Fletcher's oil-drop experiment (1909) was to measure the electric charge of the electron. They did this by carefully balancing the gravitational and electric forces on tiny charged droplets of oil suspended between two metal electrodes. Knowing the electric field, the charge on the oil droplet could be determined. Repeating the experiment for many droplets, they found that the values measured were always multiples of the same number. They interpreted this as the charge on a single electron: 1.602 × 10−19 coulomb (SI unit for electric charge).

Decomposition Metal Hydrogen Carbonate

This animation shows the decomposition of a metal hydrogen carbonate upon heating.

Chemistry Line Spectra

At the end of 19th century, physicists knew there were electrons inside atoms, and that the wiggling of these electrons gave off light and other electromagnetic radiation. Each type of atom gives off a unique set of colors. The colored lines (or Spectral Lines) are a kind of "signature" for the atoms. This technique is so reliable that scientists can tell what elements they are looking at just by reading the lines. Spectroscopy is the science of using spectral lines to figure out what something is made of. That's how we know the composition of distant stars, for instance.

Chemistry Properties Of Gases

This animation demonstrates the properties of gases. Try increasing pressure at constant temperature, Increase temperature at constant volume, Increase temperature at constant pressure, Increase number of gas particles..

Chemistry Molecular View Of Solutions Formations

Molecular View of Solution Formation.Click the Zoom button after animation finishes...

Chemistry Rutherford's Experiment

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.

Chemistry Le Chatliers principle animates

In chemistry, Le Chatelier's principle, also called the Le Chatelier-Braun principle, can be used to predict the effect of a change in conditions on a chemical equilibrium. Changing the concentration of an ingredient will shift the equilibrium to the side that would reduce that change in concentration. The principle is used by chemists in order to manipulate the outcomes of reversible reactions, often to increase the yield of reactions.

Wednesday 6 March 2013