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Review for Benchmark Obj. 3 chemistry Obj. 4 Physics

Review for Benchmark Obj. 3 chemistry Obj. 4 Physics. Nov. 22-23. Obj. 3 Chemistry. Structure of an atom:. +. +. +. The Atom’s “Center”. Protons and neutrons are grouped together to form the “center” or nucleus of an atom. Notice that the electrons are not apart of the nucleus. -. -.

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Review for Benchmark Obj. 3 chemistry Obj. 4 Physics

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  1. Review for BenchmarkObj. 3 chemistryObj. 4 Physics Nov. 22-23

  2. Obj. 3 Chemistry • Structure of an atom:

  3. + + + The Atom’s “Center” • Protons and neutrons are grouped together to form the “center” or nucleus of an atom. Notice that the electrons are not apart of the nucleus - - -

  4. Obj. 3 Chemistry • Protons: Positive Charge(+) • Neutrons: Neutral Charge(o) • Electrons: Negative Charge (-) • 1st shell- 2 electrons • 2nd shell- 8 electrons • 3rd shell- 8 electrons

  5. = 1 = 0 = 1 + - Hydrogen (H) Atom • Notice the one electron in the first orbital - + Even though there are no neutrons present, Hydrogen is still considered an atom

  6. + = 8 = 8 = 8 + + + - Oxygen (O) Atom • Notice the two electrons in the first orbital/level and the six in the second How many more electrons can fit in the 2nd orbital/ level? - - - + + + - - + + - - -

  7. + = 11 = 12 = 11 + + + - Sodium (Na) Atom • Notice the two electrons in the first orbital/level, eight in the second, and one in the third - - - How many more electrons can fit in the 3rd orbital/ level? - + + + - - - + + - - - -

  8. Obj. 3 Chemistry • Proton- identifies the element • Gives the name of the element ex. Hydrogen • Atomic Number- tell the number of protons in an atom Atomic number

  9. Obj. 3 Chemistry • Atomic Mass: Add Protons and Neutrons in the nucleus

  10. Obj.3 Chemistry • To find neutrons: Subtract atomic mass- atomic number Atomic number Atomic mass

  11. Obj. 3 Chemistry • Element: • A pure substance made up of one kind of atom that cannot be broken down into simpler substances by physical or chemical means • 90 occur naturally on earth • 25 were synthesized (made) by scientists

  12. Dmitri Mendeleev • In the 1860’s he devised a periodic table where the elements were ordered by their atomic masses • He did this by grouping elements together according to their similarities Image taken from: http://jscms.jrn.columbia.edu/cns/2006-04-18/fido-luxuriantflowinghair/mendeleev/

  13. Metals Location • Found on the left of the zigzag line/staircase on the periodic table (exception  Hydrogen) Chemical Properties • Have few electrons in their outer energy level, thus lose electrons easily Physical Properties • ductile, good conductors, malleable, shiny, most are solid @ room temperature Image taken from: http://chemistry.about.com/od/periodictableelements/ig/Element-Photo-Gallery.--98/Sodium.htm

  14. Non-Metals Location • Most found to the right of the zigzag line/staircase on the periodic table Chemical Properties • Most have almost full outer energy levels, thus they tend to gain electrons; some have completely full outer level Physical Properties • not ductile or malleable, not shiny, poor conductors, most are solid, but some are gas at room temperature Image taken from: http://nobel.scas.bcit.ca/resource/ptable/cl.htm Image taken from: https://www.dmr.nd.gov/ndgs/rockandmineral/sulfur.asp

  15. Metalloids Location • Border the zigzag line/staircase on the periodic table Chemical Properties • Most atoms have ½ (≈) complete set of electrons in outer level Physical Properties • have properties of both metals and non-metals Image taken from: http://library.thinkquest.org/C0113863/bios.shtml Image taken from: http://library.thinkquest.org/C0113863/bios.shtml

  16. Period (Row) Properties • Seven periods on a periodic table • Atomic numbers and atomic masses increase as you move from the left to the right in a period • All atoms of the elements in the same period have the same number of orbitals/levels/shells • Example Period 1 = 1 orbital • Period 2 = 2 orbitals • Period 3 = 3 orbitals • Etc…

  17. Group (Family) Properties • Eighteen groups on the periodic table (numbered from left to right) • Atomic numbers and atomic masses increase as you move from the top down in a group (family) • Atoms of elements in the same group have the same number of electrons in the outer orbitals/levels of their atoms (known as valence electrons) • Exceptions: • Transition elements (3-12) • Hydrogen (could be 1 or 17) • Helium (actually has 2 valence electrons) • Elements in groups usually have similar physical and chemical properties

  18. Group (Family) Names Alkali Metals Alkaline Earth Metals Noble Gases Boron Group Nitrogen Group Carbon Group Oxygen Group Halogens Transition Metals Periods

  19. Using the Periodic Table • The following is important information found on the periodic table. Atomic Number (Number of protons) Element Symbol (Written with a capital letter or a capital followed by a lower case if two letters ) Element Name Atomic Mass (Rounded to a whole number, equals the number of protons and neutrons)

  20. October 10, 2006 Changing Matter • Matter can be changed two ways: • Physically • Physical reaction • Physical change • Chemically • Chemical reaction • Chemical change

  21. Physical Changes • DoNOT CHANGE THE TYPE OF MATTER • Nothing new or different is formed • Could be a change in: • Mass • Volume • Density • Change in state • Color • Shape Size

  22. Examples of Physical Changes • Boiling • Freezing • Dissolving • Breaking • Making a mixture • 2 or more types of matter (substances) mixed together • Not in specific amounts • Can be separated physically

  23. Chemical Changes • Evidence of a chemical reaction • Formation of gas • Formation of precipitate • Change in color • Change in energy

  24. Chemical Changes • Chemical reactions can be represented by equations CaCO3 CaO + CO2 Reactants Products

  25. Balancing Equations • The equation for the burning of methane gas in oxygen is: • CH4 + 2 O2 → CO2 + 2 H2O Subscript Shows # of atoms Coefficient Shows # of molecules

  26. Chemical Changes • Atoms are re-arranged, NOT created or destroyed • Law of Conservation of Matter • Law of Conservation of Mass

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