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Chemistry Review

Chemistry Review. Things you should already know. Elements http:// creationwiki.org/Periodic_table http://www.universetoday.com/56747/atom-structure /. Nucleus: proton (p+) = 1 a.m.u . Neutron (N) = 1 a.m.u . Orbiting: Electron (e-) = negligible The periodic table:

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Chemistry Review

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  1. Chemistry Review Things you should already know

  2. Elementshttp://creationwiki.org/Periodic_tablehttp://www.universetoday.com/56747/atom-structure/Elementshttp://creationwiki.org/Periodic_tablehttp://www.universetoday.com/56747/atom-structure/ Nucleus: proton (p+) = 1 a.m.u. Neutron (N) = 1 a.m.u. Orbiting: Electron (e-) = negligible The periodic table: Symbol: ex. Carbon = C Atomic # = number of protons Atomic mass = #P + #N

  3. Other Important Element Stuff Electrons are arranged in energy levels (2 electrons in the first, 8 in the rest [ish]) Valence electrons are the ones in the outermost energy level (corresponds to periodic table group #) Isotopes are different forms of the same element with different atomic masses due to different # of neutrons Isotopes tend to be radioactive http://factspage.blogspot.ca/2011/06/facts-what-is-isotope.html http://wordpress.mrreid.org/2011/03/23/potassium-iodide-pills-are-radioactive/

  4. Ions http://www.healingfabrics.com/Q_A.html http://crescentok.com/staff/jaskew/isr/tigerchem/oxidation/numbers3.htm Ions are charged atoms Atoms that gain electrons become negatively charged Atoms that lose electrons become positively charged This transfer of electrons can lead to the formation of an ionic bond

  5. Chemical Bonds Intra-molecular forces holding atoms together (very strong) Ionic bonds involve transfer of electrons Covalent bonds involve sharing of electrons http://www.homework-help-secrets.com/electronegativity.html

  6. Electronegativity Aproperty of an atom which increases with its tendency to attract the electrons of a bond. If the electronegativity difference between atoms in a bond is ≥ 1.7 the bond is considered ionic (http://www.f.u-tokyo.ac.jp/~fukuyama/interactive_trial/virtual%20textbook/electronegativity/electronegativity.html)

  7. Non-Polar Covalent Bonds Happens between atoms of equal electronegativities A molecule as a whole may be non-polar due to a symetrical shape, regardless of its bonds http://spcproom5.blogspot.ca/2010/09/ionic-bonding-chemical-bond-formed.html https://vinstan.wikispaces.com/chapter+two+chemical+bonding http://www.bbc.co.uk/bitesize/higher/chemistry/energy/bsp/revision/2/

  8. Polar Covalent Bonds Happen between atoms of unequal electronegativities The result of this pattern of unequal electron association is a charge separation in the molecule, where one part of the molecule has a partial negative charge and the other a partial positive charge http://www.geo.arizona.edu/xtal/nats101/s04-18.html

  9. Physical Bonds http://www.glogster.com/arooke2/hydrogen-bonds/g-6m99vd692fc7hgidt985ta0?old_view=True Intermolecular forces holding molecules together Weaker than chemical bonds Strongest physical bond is a hydrogen bond

  10. Molecular Structure Molecular Formula Structural Formula Shows # of atoms but not arrangement in space Ex. C2H6O or C2H5OHor CH3CH2OH Shows bonding arrangements between atoms (single, double, triple bonds etc.) http://www.scienceaid.co.uk/chemistry/organic/nomenclature.html

  11. Molecular Shape Important in most chemical reactions Important in biological action Ex. Tetrahedral, planar. linear

  12. ISOMERS StructuralIsomers Stereoisomers Two or more compounds with the same atoms bonded differently Ex. Glucose & fructose Two or more compounds with their atoms bonded in the same way but arranged differently in space Ex. Glucose and galactose http://bioweb.wku.edu/courses/biol115/wyatt/biochem/carbos.htm

  13. THE end

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