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Matter and Energy Unit 2

Matter and Energy Unit 2. Matter. Matter is anything that occupies space and has mass. Mass – tha amount of matter in an object (measured in grams) Volume – the amount of space an object occupies (mL or L or cm^3) Weight – the amount of pull of gravity on an object (measured in Newtons).

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Matter and Energy Unit 2

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  1. Matter and Energy Unit 2

  2. Matter • Matter is anything that occupies space and has mass. • Mass – tha amount of matter in an object (measured in grams) • Volume – the amount of space an object occupies (mL or L or cm^3) • Weight – the amount of pull of gravity on an object (measured in Newtons)

  3. Physical Properties Properties - characteristics that identify an object: Physical properties: observed and measured without changing to something else Ex: State, Color, solubility and melting point Physical Change: Alters 1 or more physical properties without changing the chemical composition

  4. Chemical Properties Chemical Properties: formed when a substance reacts with another substance to form a different chemical composition Chemical Changes: cannot be observed without altering the chemical composition Ex: Na + Cl NaCl (Sodium Metal) + (Chlorine gas ) produces(Table Salt) Poisonous

  5. Elements The basic building blocks of matter: Elements are pure substance that can NOT be broken into simpler substances. Found on the Periodic Table. Ex: C, N, O… Each element has their own unique physical and chemical properties

  6. Compounds Compounds can be broken down into single elements by chemical changes Ex: H20 into 2 Hydrogens and 1 Oxygen NaCl into Sodium and Chlorine Binary compounds have only two elements. Ternary – compounds that have 2+ elements Diatomic compounds have only two elements that are the same. Diatomic elements include – H, N, O, F, Cl, Br and I

  7. Pure Substances and Mixtures Pure substances • Matter with fixed composition (can be elements or compounds) • Cannot be separated into any other form of matter by physical change (for compounds) Ex: He is an element (look on the Periodic Table) O2 (g) is a diatomic gas, Oxygen NaCl is table salt

  8. Pure Substances and Mixtures Mixtures 1. Combined 2 or more pure substances Ex: salt and sugar 2. Composition can vary 3. Can separate by physical means 4. Can be heterogeneous OR homogeneous

  9. Classification of Matter Homogenous matter • Same parts with same properties throughout Ex: Teaspoon of sugar, any element

  10. Classification of Matter Homogeneous mixture 1. Uniform blend of 2 or more substances 2. Can vary in proportion (like concentration) 3. Every part is exactly like every other part (think Kool-Aid) Ex: salt dissolved in water (a solution)

  11. Classification of Matter Heterogeneous matter 1. Different parts with different properties Ex: Salt and Pepper

  12. Classification of Matter Heterogeneous mixture 1. Different parts with different properties 2. Made of 2 or more substances with each retaining their unique properties (boiling point, solubility, etc.) 3. NOT the same composition or properties throughout 4. Composition can vary 5. Does NOT make a solution Ex: Salt and sand

  13. Separating Mixtures • With a magnet 1. Mixture of iron and sulfur 2. Separated by their physical properties • Distillation 1. Process in which a mixture can be separated by its boiling points 2. Ex: Petroleum (mixture of gas, kerosene and oil) when it boils the liquids separate with gas boiling first

  14. Separating Mixtures C. Filtration 1. Process that separates the solid and liquid parts 2. Use filter paper, funnel – the liquid part goes through the filter a. If solid is dissolved in liquid it will also go through paper Ex: Soda has carbon dioxide gas

  15. Separating Mixtures D. Chromatography 1. Way to separate different molecules in a mixture 2. Put drop from mixture near one end of chromatography paper – then put paper into the solvent and the mixture will move up so that molecules move different distances http://www.wooster.edu/chemistry/analytical/gc/default.html

  16. States of Matter Solid 1. Definite shape and definite volume 2. Particles stick rigidly together and vibrate – they don’t move position 3. Often crystalline structure – fixed, repeating internal structure 4. Amorphous solids – do NOT have a crystalline structure 5. Melting point – temperature at which a solid turns into a liquid (solid and liquid are in equilibrium 6. Sublimation – change from a solid to a gas ( skips the liquid stage

  17. States of Matter Liquid 1. No definite shape but has definite volume 2. Particles stick together but NOT rigidly and do NOT have a pattern. (more random) 3. Evaporation – when liquid changes into a gas 4. Vapor pressure – in closed containers some liquid changes to a gas which exerts pressure on the container walls a. Table H in reference tables.

  18. States of Matter 5. Boiling Point – when vapor pressure equals atmospheric pressure a. the atmospheric exerts a pressure on everything b. at the boiling point of water the vapor pressure is 101.3Kpa,(1atm.) and is equal to the atmospheric pressure

  19. States of Matter Gas 1. No fixed volume and no definite shape 2. Gas pressure is caused by particles move and collide with the walls of a container 3. Particles are far apart and move in all directions 4. Can be compressed or expanded

  20. States of Matter Plasma 1. Composed of electrically charged atomic particles 2. Examples: Stars including the our Sun 3. Made by heating gas to extremely high temperatures or or by passing a current though it

  21. States of Matter Entropy 1. As matter goes from a solid to a liquid and then a gas the entropy increases Note: Entropy is the randomness of a particle's energy and position

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