1. By: Rafal Grabowski CHEMISTRY

2. WHAT IS MATTER? Matter is it is any substance which has mass and occupies space. All physical objects are composed of matter, in the form of atoms, which are in turn composed of protons, neutrons, and electrons.

3. WHAT ARE THE STATES OF MATTER? The States of Matter are Gas, Liquid and Solid. Gas assumes the shape and volume of its container, it’s compressible, it flows easily, the particles are well separated with no regular arrangement and the particles vibrate and move freely at high speeds. Liquid assumes the shape of the part of the container which it occupies, it’s not easily compressible, it flows easily, particles are close together with no regular arrangement and particles vibrate, move about and slide past each other. Solid retains a fixed volume and shape, it’s not easily compressed, does not flow easily, particles are tightly packed usually in a regular pattern and particles vibrate but generally do not move from place to place.

4. WHAT ARE THE PHYSICAL AND CHEMICAL PROPERTIES OF MATTER? A Physical property is a quality or condition of a substance that can be observed or measured without changing the substance’s condition. A Chemical property is how a substance reacts to other substances. Some physical properties are state at room temperature, melting point, freezing point, color, conductivity. Some chemical properties are oxidation which is rusting and burning, flammability, color change, gas given off, temperature change.

5. PHYSICAL AND CHEMICAL CHANGES. A chemical change is the change of one or more substances into other substances. Physical change is when the appearance or shape of a substance is changed. Physical changes do not change the chemical make up of the substance. A chemical change cannot be reversed..Examples of chemical changes: burning wood, cooking rice, frying an egg, explosion of fire works - examples of physical changes: crumbling paper, breaking glass, cutting wood, boiling water, melting ice.

6. SOLUBILITY Solubility is the property of a solid, liquid, or gaseous chemical substance called solute to dissolve in a solid, liquid, or gaseous solvent to form a homogeneous solution of the solute in the solvent. The solubility of a substance fundamentally depends on the used solvent as well as on temperature and pressure. The extent of the solubility of a substance in a specific solvent is measured as the concentration where adding more solute does not increase the concentration of the solution.

7. ELEMENTS 1.A element is on the periodic table 2. each element has a limit of atoms,electrons,protrons 3.There are so far 103 elements but more can be found 4. a element can be solid,liqiud or gas 5. a element can be found all around you A element is a natural thing found in nature and you can fund in nature

8. ATOM A atom is a circle that goes on a shell but on each shell only a sertian number of atoms can be on one shell. On the first shell there can be only 2 and the seconded be only 8 3 18 4 32.

9. SUBSTANCE AND MIXTURE The difference between a pure substance and a mixture is that a pure substance such as aluminum and sugar has one type of particle in it and mixture such as salt has two or more particles within it or two pure substances. Sugar is not a pure substance. It is comprised of carbon, hydrogen, and oxygen. But when you see co2 or h2o these are compounds because they have different molecules. what ever the number follows is how molecules are in it.

10. PERIODIC TABLE Each element has a number and that number stands for electrons and there are atoms witch are on the shells and the protons are how much.there are

11. COUMPOUNDS Compounds are groups of two or more elements that are bonded together. There are two main types of bonds that hold those atoms together, covalent and electrovalent/ionic bonds. Covalent compounds happen when the atoms share the electrons, and ionic compounds happen when electrons are donated from one atom to another. 1 water is h20 2 hydroxide NaOH NaOH 3 nitrate NaNO 3NaNO 4 The salt is prepared by treating sodium hydroxide with mixtures of nitrogen dioxide and nitric 2 NaOH + NO 2 + NO → 2 NaNO 2 + H 2 O 5 sulphate Na 2 SO 4

12. SOLUTION A solution is a homogeneous mixture of one or more solutes dissolved in a solvent. 1.Microscopic view of Br 2 gas (solute) dissolved in Ar gas (solvent). 2. Microscopic view of Br 2 liquid (solute) dissolved in liquid H 2 O (solvent) 3Microscopic view of Ar gas (solute) dissolved in liquid H 2 O (solvent). 4. Microscopic view of solid NaCl (solute) dissolved in liquid H 2 O (solvent). Note that the ionic solid, NaCl, produces Na + ions (blue) and Cl - ions (green) when dissolved in water 5. Microscopic view of solid Kr (solute, blue ) dissolved in solid Xe (solvent, red ).

13. HETEROGENEOUS AND HOMOGENOUS MIXTURES A homogeneous mixture is a mixture where the components that make up the mixture are uniformly distributed throughout the mixture. A heterogeneous mixture is a mixture where the components of the mixture are not uniform or have localized regions with different properties. Examples of heterogeneous: sand and iron filings, water and oil, salad, trail mix, concrete Examples of homogeneous mixtures: blood, sugar water, salt water, soapy water, wine