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Chapter #2

Chapter #2. Matter. Notes 2.1. Chemistry : is the branch of science that studies composition of matter and how it changes. Matter : is anything that has mass and occupies space. Examples air, water, you… Light, sound, and electricity are not matter. They have no mass or volume.

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Chapter #2

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  1. Chapter #2 Matter

  2. Notes 2.1 • Chemistry: is the branch of science that studies composition of matter and how it changes. • Matter: is anything that has mass and occupies space. Examples air, water, you… • Light, sound, and electricity are not matter. They have no mass or volume.

  3. Element: is a substance that cannot be broken down into simpler substances. • Atom: is the smallest particle that has the properties of an element. 1 square on the periodic table 2 or more squares on the periodic table

  4. Compound: is a substance made of atoms of more than one element chemically bound together. • Molecule: is the smallest unit of a substance that exhibits all the properties characteristic of that substance.

  5. Chemical Formula is used to show how many atoms of each element are present. • Subscripts little numbers. Represent # of atoms Examples CH4 C6H12O6 C16H10N2O2 H2O

  6. A pure substance is any matter that has a fixed composition and definite properties. • Amixture is a combination of more than one pure substance. They are physically mixed.

  7. Miscible describes two or more liquids that are able to dissolve into each other in various proportions. • Immiscible describes two or more liquids that do not mix into each other.

  8. A heterogeneous mixture is a combination of substances that are not uniformly mixed. Ex.. Italian Dressing • In a homogeneous mixture the substances are uniformly mixed throughout the compound. Ex.. Salt water

  9. Hetero

  10. Chapter 2.2 Notes Kinetic Theory • All Matter is made of atoms and molecules that act like tiny particles. • These particles are always in motion. • The higher the temp the faster they move • At the same temp heavy gases are slower than lighter gases.

  11. 3 States of matter • Solid particles have a rigid structure and a definite shape and volume • Liquid particles are fluids the particles can slide past one another. No definite shape but a definite volume • Gas particles are fluid. No definite shape or volume.

  12. Viscosity- the resistance of liquid to flow… • The thicker it is the higher the viscosity.

  13. Evaporate- changing from a liquid to a gas. • Condenses- changing from a gas to a liquid. • Melting- changing from a solid to a liquid. • Freezing- changing from a liquid to a solid • Sublimation- changing from a solid to a gas

  14. Evaporation

  15. The law of conservation of mass- Mass cannot be created or destroyed. • The law of conservation of energy- Energy cannot be created or destroyed.

  16. Chapter 2.3 Notes Chemical Properties – the way a substance reacts to form new substance with different properties • Reactivity – the ability to combine chemically with another substance • Flammability – is the ability of a substance to burn when reacting with oxygen and being exposed to a flame

  17. Physical property – a characteristic of a substance that can be observed or measured without changing the composition of the substance • Melting point – the temperature in which a substance turn from a solid to a liquid • Boiling point – the temperature at which a substance turn from a liquid to a gas

  18. Density – the mass per unit volume of a substance • Density equation D=m/V Density=mass/volume • Buoyancy-the force with which a more dense fluid pushes a less dense substance upward

  19. Chemical change- a change that occurs when a substance changes composition by forming one or more new substances • Odor, fire, light, rusting

  20. Physical change- a change in the physical form or properties of a substance that occurs without a change in composition Changes in state from solid to liquid to gas are physical changes it is still the same substance…

  21. Work cited • “Cartoon”. Dec. 12, 2007. http://www.mpch-mainz.mpg.de/~sander/lecture.gif • “Pure Substances Diagram”. Dec. 12, 2007. http://faculty.colostate-pueblo.edu/linda.wilkes/111/2a.4.gif • “Matter Diagram”. Dec. 12, 2007. http://www.personal.kent.edu/~cearley/ChemWrld/compounds/matter.gif • “Heterogeneous Mixture.” Dec. 12, 2007. http://www.arborsci.com/CoolStuff/magnetic_seperation.jpg • “Homogeneous Mixture.” Dec. 12, 2007. http://content.answers.com/main/content/wp/en-commons/thumb/7/77/180px-SaltInWaterSolutionLiquid.jpg • “Immiscible”. Dec. 12, 2007. http://www.csiro.au/helix/sciencemail/activities/images/EmulsionStepOne.jpg • “Miscible”. Dec. 12, 2007. http://employees.csbsju.edu/hjakubowski/classes/ch111/olsg-ch111/solutions/animliqsat.gif • States of Matter. Dec. 14, 2007. http://www.ilpi.com/msds/ref/gifs/statesofmatter.gif • “Motor oil viscosity”. Dec. 14, 2007. http://www.smartsynthetics.com/images/cold-temp-hot-temp-viscosity.jpg • “Pouring Motor oil”. Dec. 14, 2007. http://www.trucktestdigest.com/images/Oil%20wrong%20viscosity.jpg • “Change of state flow chart”. Dec. 14, 2007. http://resources.yesican-science.ca/lpdd/g07/lp/nelson/states.gif • “Fireplace”. Dec. 18, 2007. http://z.about.com/d/chemistry/1/8/W/P/fireplace.jpg • “Flask on fire”. Dec. 18, 2007. http://htdconnect.com/~chargers/chem/Image3.jpg • “Chemical change pictures”. Dec. 18, 2007. http://www.ric.edu/faculty/ptiskus/chemical/index_files/mcmcb3fe%5B1%5D.gif • “Physical changes chart”. Dec. 18, 2007. http://www.schools.pinellas.k12.fl.us/educators/tec/Davis2/matter.ppt/img008.gif • “Change in state”. Dec. 18, 2007. http://www.windows.ucar.edu/earth/geology/images/change_state_sm.gif

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