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Matter Unit Vocabulary

Matter Unit Vocabulary. Physical change Chemical change Demoritus John Dalton JJ Thomson Ernest Rutherford Niels Bohr Atomos Bohr Model Cloud Model Valence Electrons Energy Levels Shells Properties of Water Universal solvent Adhesion Cohesion High specific heat

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Matter Unit Vocabulary

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  1. Matter Unit Vocabulary

  2. Physical change • Chemical change • Demoritus • John Dalton • JJ Thomson • Ernest Rutherford • Niels Bohr • Atomos • Bohr Model • Cloud Model • Valence Electrons • Energy Levels • Shells • Properties of Water • Universal solvent • Adhesion • Cohesion • High specific heat • Capillary action • Surface tension • Polarity • States of matter • Heat of vaporization • pH • Matter • Kinetic Theory • Solid • Liquid • Gas • Plasma • Phase change • Freezing • Melting • Deposition • Sublimation • Condenstation • Vaporization • Physical properties • Ducility • Malleability • Melting point • Boiling point • Freezing point • Solubility • Reaction to light • Electrical conductivity • Chemical properties • Flammability • Oxidation • decomposition

  3. Matter • Anything that has mass and occupies space • The materials or “stuff” that all objects and substances in the universe are made of • 4 States of Matter = Solid, liquid, gas, and plasma

  4. Matter • Because all matter takes up space (has volume) and contains a certain amount of material (has mass), all matter can be detected and measured

  5. Examples of Matter • Rocks, water, trees, bicycles, lighting, animals, stars, smoke, are all easily seen and observed • Dust mites that live in your furniture and rugs you may need a microscope to view • Air maybe invisible but we can feel it when the wind blows and see it bend the branches of trees (oxygen, nitrogen, hydrogen, CO2)

  6. What is not matter? • Light • Sound • Gravity • Friction

  7. Matter • Atoms are the building blocks of matter • The elements in our periodic table make up all matter

  8. Kinetic Theory All matter consists of tiny particles that are in constant motion.

  9. Kinetic Theory 1. All matter is composed of small particles (atoms, molecules, or ions). There is an attractive force between them. 2. They are in constant, random motion. The particles may collide with one another or the sides of their container. 3. As the temperature increases the speed of the particles increases. As the temperature decreases the speed of the particles decreases.

  10. SOLIDS • State of matter that has a definite shape and a definite volume. • Particles of solids are tightly packed, vibrating about a fixed position. • Particles are strongly attracted to each other

  11. LIQUID • A state of matter that has a definite volume but takes the shape of its container • Liquids do not have a definite shape • Particles of liquids are tightly packed, but are far enough apart to slide over one another, allowing it to flow

  12. GAS • A state of matter that has no definite shape and no definite volume; expands to fill the shape of its container • Particles of gases are very far apart and move freely. • Attractive forces are very weak • Contain mostly empty space – because the particles are so far apart • Particles spread throughout a given volume until distributed equally – diffusion

  13. Gas vs. Vapor • Gas – a substance that is naturally in the gaseous state at room temperature • EXAMPLE: Helium • Vapor – the gaseous state of a substance that is a solid or liquid at room temperature • EXAMPLE: Steam

  14. PLASMA • A state of matter that does not have a definite shape or volume and whose particles have broken apart • Consists of + and – charged particles (electrons are knocked off due to collisions) • A plasma is a very good conductor of electricity and is affected by magnetic fields. • Plasma is the most common state of matter in the universe

  15. STATES OF MATTER SOLID LIQUID GAS PLASMA Tightly packed, in a regular pattern Vibrate, but do not move from place to place, definite shape and volume Close together with no regular arrangement. Move about, flow and slide past each other. Definite volume, no definite shape takes shape of its container. Well separated with no regular arrangement. Move freely at high speeds. No definite shape or volume. Easily compressible. Has no definite volume or shape and is composed of electrical charged particles PLC-Unit 1B

  16. STATES OF MATTER LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

  17. Phase Change A transition of matter from one state to another.

  18. Some phase changes are more common and easier for us to visualize. For example, you have probably witnessed freezing, melting, and vaporization just by making ice, melting ice, and boiling water.

  19. Condensation often occurs on the outside of cold beverage containers. This is when the humid air changes directly to a liquid on the surface of the container.

  20. SublimationDry ice is actually solid carbon dioxide. When it sits in the open or is placed in water it rapidly changes directly from solid to gas creating a foggy cloud.

  21. DepositionFrozen patterns of ice on your car windshield is an example. Deposition involves a gas changing to a solid. This occurs during winter months when the humid air directly freezes into solid ice.

  22. Physical properties • Characteristics that can be observed without changing the makeup or identity of the matter • Examples: color, size, state of matter, density, ductility, malleability, boiling point, melting point, freezing point, electrical conductivity, solubility, reaction to light

  23. Density • The ratio of the mass of an object to its volume • Formula: d = m/V • Units: g/mL or g/cm3

  24. Ductility • The ability to be pulled into a thin strand • EX: wire

  25. Malleability • The ability to be pressed or pounded into a thin sheet • EX: aluminum foil, sheet metal

  26. Boiling Point • The temp at which a substance changes from a liquid to a gas • EX: the boiling point of water = 1000C

  27. Melting Point • The temp at which a substance changes from a solid to a liquid • EX: the melting point of chocolate is 340C

  28. Freezing Point • The temp at which a substance changes from a liquid to a solid • EX: the freezing point of water = 00C

  29. Electrical Conductivity • How well a substance allows electricity to flow through it • EX: copper wires, electrical lines

  30. Solubility • The ability to dissolve in another substance • EX: sugar in water

  31. Reaction to Light • Reflection – to bounce off ( mirror) • Refraction – to bend (water) • Absorption – to take in (leaf)

  32. Reaction to Light • Transmission – allow to pass through • Opaque – little to no light passes through (blanket) • Translucent – some light passes through (sunglasses) • Transparent- most light passes through ( glass window)

  33. Chemical properties • The ability of matter to undergo a specific chemical change, creating a different type of matter with new properties • Examples: flammability, decomposition, oxidation

  34. Flammibility • To burn • Must occur in the presence of oxygen • EX: Flame tests help to identify metals by their characteristic flame color

  35. Decomposition • To rot or breakdown • Complex compounds breakdown to simpler substances • EX: CO2 breaks down to Carbon and Oxygen

  36. Oxidation • The process of losing electrons • EX: iron rusts when exposed to oxygen

  37. Physical Changes • A process where a substance’s chemical properties have not changed • Can be a change in size, color, shape, state of matter • EX: ice melting, salt dissolving in water, glass breaking

  38. Chemical Change • Occurs when new substances or materials are produced to have different chemical properties from the reactants • EX: rust is the product of iron and oxygen, wood burning

  39. Democritus Greek philosopher in 440 bc Was the first to proposed the existence of atoms “Atomos” meaning “not to be cut”

  40. John Dalton British chemist 1803 Atomic Theory – He came up with the theory that all substances were made of atoms Atoms were small, hard, dense spheres that could not be created, destroyed, or altered

  41. Dmitri Mendeleev Known as the father of the present day periodic table Organized the elements (each type of atom) by similar properties in 1869

  42. J. J. Thomson British scientist 1898 Proposed that atoms themselves were made of smaller particles . He discovered that atoms contained negatively charged particles, but did not know their location

  43. J. J. Thomson • Theorized the negatively charged particles were spread evenly throughout the positively charged material • Thomson’s model of the atom was called the “plum-pudding” model

  44. Ernest Rutherford • 1911 a former student of Thomson's • Proposed that atoms had a dense, positively charged nucleus surrounded by electrons

  45. Niels Bohr • 1913 Danish scientist • Said that electrons revolve around the nucleus in circular paths, called orbits • And that electrons could only exist in certain orbits and at certain energy levels http://youtu.be/wCCz20JOXXk

  46. Today’s modelelectron cloud model • Bohr’s model was an important stepping stone to today’s, which was developed in the 1920’s • Electrons surround the nucleus, traveling not in prescribed paths but in regions of various thicknesses called clouds http://youtu.be/kYkD-dcupAU

  47. Bohr Model • Electrons orbit the nucleus of an atom in set energy levels P = 20 N = 20

  48. Energy Level • The specific energies an electron in an atom can have • In the Bohr model used to describe the different orbits or shells that the electrons travel in around the nucleus

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