Propertry of matter


Published on

It s very nice

Published in: Education, Technology
  • Be the first to comment

  • Be the first to like this

No Downloads
Total views
On SlideShare
From Embeds
Number of Embeds
Embeds 0
No embeds

No notes for slide

Propertry of matter

  1. 1. Properties of matter<br />- Shitanshu Desai<br />
  2. 2.
  3. 3. Classification of Matter<br />
  4. 4.
  5. 5. Matter exists in three states - Solids, Liquids and Gases<br />
  6. 6. Solids : A solid   has a definite characteristic shape   tends to resist deformation of its shape   is relatively non compressible   For example, diamond   Solids can be classified as:   Crystalline   Amorphous  <br />
  7. 7. liquid : Has a definite volume   no characteristic shape   takes the shape of the container   is fluid - is able to flow and change shape without separation   is essentially non compressible .<br />
  8. 8. Gas  : has no definite volume or shape   is fluid   is very compressible. It takes the volume and shape of the vessel in which it is kept. <br /> <br />  <br />
  9. 9. All the three states of matter are inter-convertible.<br />  When water is cooled to 0oC, it transforms into ice (solid). On heating, at 100oC, it begins to boil and gets converted into vapor (gas).<br />On cooling, water vapor gradually converts back into water (liquid).    <br />
  10. 10. Effect of heat and temperature on matter <br />
  11. 11. Elements compounds and mixture<br />Element : A group of same type of atoms is known as an element .<br />Compound : When two or more elements combine chemically with one another a compound is formed <br />Mixture : A mixture is a material consisting of two or more kinds of matter each retaining its own characteristic properties .<br />
  12. 12.
  13. 13. Typesof mixture<br /><ul><li>Homogeneous Mixture : Solution is a homogeneous mixture of a solvent .
  14. 14. Heterogeneous Mixture : Physical states of components is different in heterogeneous mixture .</li></li></ul><li>Difference between solute and solvent<br />
  15. 15. Solutions<br />Solution is defined as a homogeneous mixture of two or more chemical substances. The state of matter of a solution may be solid, liquid or gaseous. <br />  For example, common salt in water (liquid solution), air (gaseous solution), alloys (solid solution), etc.   <br />The components of a solution may be classified as: <br /> 1. Solute <br /> 2. Solvent  <br />
  16. 16. True Solutions<br />A true solution is a homogeneous solution in which the solute particles have diameters less than 10-7cm. i.e., the solute particles are of molecular dimensions.<br /> The particles are invisible even under powerful microscopes.   For example, sodium chloride in water is a true solution. Most ionic compounds form true solutions in water. Organic compounds like sugar and urea also form true solutions in water.<br />
  17. 17. Suspensions Solutions<br />A suspension is a heterogeneous mixture in which one or more components have a particle size greater than 10-5cm. Very often these particles are visible to the naked eye.<br />For example, sand in water, sodium chloride in benzene, turmeric in water etc.  <br />
  18. 18. Colloids Solutions<br />A colloid is a solution in which the particle size ranges between 10-7 and 10-5 cm.  <br />For example, milk, blood, honey, smoke, ink, gum, starch solution etc.<br />
  19. 19.
  20. 20. Atoms and Molecules<br />. Atom : Atom is the smallest particle of an element, which may or may not have independent existence. It is made up of subatomic particles like electrons, protons and neutrons. Atoms of one type of element differ from those of the other due to different number of subatomic particles.<br />Molecule : It is smallest particle (of an element or compound), which is capable of independent existence. Molecules are formed by combination of atoms.<br />
  21. 21. Dalton&apos;s Atomic Theory<br />John Dalton, a British school teacher, published his theory about atoms in the year 1808. His findings were based on experiments and also from laws of chemical combination.  <br />
  22. 22. Main assumptions or postulates of Dalton<br />- All matter consists of indivisible particles called atoms.<br />- Atoms of the same element are similar in shape and mass, but differ from the atoms of other elements.<br />- Atoms cannot be created or destroyed.<br />- Atoms of different elements may combine with each other in a fixed, simple, whole number ratio to form compound atoms.<br />- Atoms of same element can combine in more than one ratio to form two or more compounds.<br />- Atoms are the smallest unit of matter that can take part in a chemical reaction.<br />
  23. 23. Drawbacks of Dalton&apos;s atomic theory of matter<br /><ul><li>The indivisibility of an atom was proved wrong, for, an atom can be further subdivided into protons, neutrons and electrons. However an atom is the smallest particle, which takes part in chemical reactions.</li></ul>-According to Dalton, the atoms of same element are similar in all respects. This is wrong because atoms of some elements vary in their mass and density. Such atoms of the same element having different masses are called isotopes. For example, chlorine has two isotopes having mass numbers 35 a.m.u and 37 a.m.u. <br />
  24. 24. -Dalton also said atoms of different elements are different in all respects. This has been proved wrong in certain cases like argon and calcium atoms, which have the same atomic mass of 40. Such atoms of different elements that have the same atomic mass are called isobar.<br />-According to Dalton atoms of different elements combine in simple whole number ratio to form compounds. This is not seen in complex organic compounds like sugar C12H22O11.<br />-The theory completely fails to explain the existence of allotropes. The difference in properties of charcoal, graphite, diamond went unexplained in spite of being made up of same kind of atoms.<br />
  25. 25. Merits of Dalton&apos;s atomic theory <br />-It has enabled us to explain the laws of chemical combination.<br />-Dalton was the first person to recognize a workable distinction between the ultimate particle of an element (atom) and that of a compound (molecule).<br />
  26. 26. Mole Concept<br />Since it is not possible to calculate the weight of particles individually, a collection of such particles called mole is taken for all practical purposes. Avogadro discovered that under standard conditions of temperature and pressure, (1atm and 273K) a sample of gas occupies a volume of 22.4 L.  <br />
  27. 27. -It was discovered that the number of atoms present in 12g of carbon is 6.023 x 1023 atoms.<br />-This is referred to as Avogadro number.<br />-A mole of a gas is the amount of a substance containing 6.023 x 1023 particles.<br />-Avogadro&apos;s number is the number of atoms present in C12 isotope = 12g of C.<br />-One mole of any gas at STP will have a volume of 22.4 L. <br />
  28. 28. Thank You<br />