1 / 65

Chemistry : Chemical Processes

Chemistry : Chemical Processes. WHMIS. Workplace Hazardous Materials Information System Why is it important? . WHMIS Symbols. CLASS A: COMPRESSED GAS This class includes compressed gases, dissolved gases, and gases liquefied by compression or refrigeration. .

adeola
Download Presentation

Chemistry : Chemical Processes

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemistry : Chemical Processes

  2. WHMIS • Workplace Hazardous Materials Information System • Why is it important?

  3. WHMIS Symbols CLASS A: COMPRESSED GAS This class includes compressed gases, dissolved gases, and gases liquefied by compression or refrigeration. CLASS B: FLAMMABLE AND COMBUSTIBLE MATERIAL This class includes solids, liquids, and gases capable of catching fire in the presence of a spark or open flame under normal working conditions. CLASS C: OXIDIZING MATERIAL These materials increase the risk of fire if they come in contact with flammable or combustible materials.

  4. WHMIS Symbols CLASS D: POISONOUS AND INFECTIOUS MATERIALDivision 1: Materials Causing Immediate and Serious Toxic Effects These materials can cause death or immediate injury when a person is exposed to small amounts. Examples: sodium cyanide, hydrogen sulphide CLASS D: POISONOUS AND INFECTIOUS MATERIALDivision 2: Materials Causing Other Toxic EFFECTS These materials can cause life-threatening and serious long-term health problems as well as less severe but immediate reactions in a person who is repeatedly exposed to small amounts. CLASS D: POISONOUS AND INFECTIOUS MATERIALDivision 3: Biohazardous Infectious MATERIAL These materials contain an organism that has been shown to cause disease or to be a probable cause of disease in persons or animals.

  5. WHMIS Symbols CLASS E: CORROSIVE MATERIAL This class includes caustic and acid materials that can destroy the skin or eat through metals. Examples: sodium hydroxide, hydrochloric acid, nitric acid CLASS F: DANGEROUSLY REACTIVE MATERIAL These products may self-react dangerously (for example, they may explode) upon standing or when exposed to physical shock or to increased pressure or temperature, or they emit toxic gases when exposed to water.

  6. What is Chemistry and Matter? Chemistry is the study of matter, its properties and its changes or transformations. Matter is anything that has mass and takes up space.

  7. Classification of Matter

  8. Mixtures • A mixture is a substance made by combining two or more different materials in such a way that no chemical reaction occurs. • Mixtures can be separated by physical means. • Ex. Party Mix, boiling Kool Aid

  9. Homogenous Mixture (Solution) • Mixture where the two different substances that are combined together are mixed very well. • Any portion of the sample has the same properties and composition. • Example: Salt Water Milk

  10. Heterogeneous Mixture • Mixture where the different parts or each substance can be separated physically. • Different parts are visible. • Example: Toppings on a Pizza Chocolate chip cookie Salad

  11. Pure Substances • How do we know that a sample of matter is a pure substance? • A pure substance is made up of all the same particles. • A pure substance also has constant properties. Example: pure water, aluminum foil. • Pure substances can be either elements or compounds.

  12. Compounds • Compounds are pure substances that contain two or more different elements in a fixed proportion. • Example: Water H2O = 2 parts hydrogen to 1 part oxygen. SaltNaCl = 1 sodium to 1 clorine

  13. Elements • Elements are pure substances that cannot be broken down into simpler substances. • Elements contain only one kind of atom. • Example: Oxygen, hydrogen, iron, etc. ( anything on the periodic table )

  14. Review • Homogeneous Mixture • Heterogeneous Mixture • Element • Compound • Pure Substance • Mixture

  15. Classify the following as:a) pure or mixtureb)element, compound, heterogeneous or homogeneous mixture • Salt • Sugar • Wood • Rock • Water • Milk • Plastic • Glass • Mercury • Apple Juice • Syrup • Gold • Air • Oxygen • Silver • Cookies • Cake • Sand

  16. States of Matter • http://www.harcourtschool.com/activity/states_of_matter/ There are 3 states of matter: Solid, Liquid and Gas.

  17. Properties of Matter: Physical and Chemical • A Physical Property is a characteristic of a substance. Usually these are properties that we can detect with our senses. • Changing the size or amount of the substance does not change the physical properties.

  18. Physical Properties • Color – red, green, white, etc. • Texture – smooth, fine, coarse. • Taste – sour, sweet, salty. • Odour – what smell does the substance have? • States of matter at room temperature: - solid, liquid, gas.

  19. Physical Properties • Malleable is the ability of a solid to be hammered or bent into different shapes. Aluminum foil is malleable. Gold is malleable since it can be hammered into thin sheets. • Hardness – the measure of the resistance of a solid to being scratched or dented

  20. Physical Properties • Ductility – The ability to stretch a substance into a wire. • Viscosity – the ability of a substance to flow or pour. • Luster – How shiny is the substance?

  21. Physical Properties • Boiling Point – the temperature at which a liquid changes state and becomes a gas. • Melting Point – the temperature at which a solid changes state and becomes liquid.

  22. List the Physical Properties Baking soda is: • solid at room temperature • white in color • crystal form • dissolves easily in water.

  23. Chemical Properties • A chemical property is a behaviour that occurs when a substance changes to a new substance. • For example: Is the substance combustible? Does the substance have a reaction with acid? Does the substance react with water?

  24. Physical Changes • In a physical change, the substance involved remains the same substance, even though it may change state or form. • Can be undone quite easily. Key: No new substance is created. • Examples: melting ice, freezing water, dissolving salt into water, breaking a stick.

  25. Chemical Changes • In a chemical change, the original substance is changed into one or more different substances that have different properties. • Not easily undone – almost impossible Key: New substance almost always formed. • Examples: burning wood, baking a cake, digesting food

  26. Clues that a chemical change has occurred • A new color appears. • Heat or light is given off. • Bubbles of gas are formed. • The change is difficult to reverse.

  27. Physical Changes • Here are some examples of physical changes:

  28. Melting popsicle

  29. Broken Twig

  30. Here are some other examples of chemical changes:

  31. Raw egg becomes cooked egg

  32. Cake mix becomes cake

  33. Steel becomes rust

  34. Your Turn Chemical or Physical Changes

  35. Chemical or Physical ? Cutting a piece of wood.

  36. Chemical or Physical ? Chewing of food

  37. Chemical or Physical ? Rusting Nail

  38. Chemical or Physical ? Ice Melting

  39. Chemical or Physical ? Burning a Match

  40. Chemical or Physical ? Stretching a Rubber Band

  41. Chemical or Physical ? Breaking a Stick

  42. Chemical or Physical ? Tarnishing Silver

  43. Chemical or Physical ? Ripening Tomatoes

  44. Chemical or Physical ? Water Boiling

  45. The Atom

  46. taken from: http//:education.jlab.org/atomtour/listofparticles.html

  47. Electrons • Negatively charged ( - ) • Almost have no mass • Located around the outside of the nucleus

  48. Proton • Same mass as neutrons • Positively charged (+) • Located in center of atom (nucleus) • Number of protons in an atom is equal to the elements atomic number.

  49. Neutron • Same mass as proton • No charge • Located in nucleus • Number per atom is based on the following formula: • #Neutrons = Atomic Mass – Atomic Number

More Related