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Ch. 6-1 Chemical Bonding

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by

Allison Hill

on 29 April 2010

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Transcript of Ch. 6-1 Chemical Bonding

Chapter 6 Atomic Bonding Electron Theory Chemical Bonding JJ Thompson discovered
the electron in 1897 plum pudding model Neils Bohr theroized that
electrons occupy certain
energy levels certain
distances from atom's nucleus Electron Cloud Model electrons have properties similar to waves
which led scientistists to develop this model
to more accurately describe where electrons are
most likely to be found since exact path can't
be predicted the joining of atoms
to create a new substance chemical change= new substance created Electrons negatively charged particle atoms are neutral # of protons= # of electrons Remember that protons are positively charged Use models to help us
understand atoms although
they don't show the true
structure not all electrons create
the chemical bonds= only the
valence electrons valence electrons=
electrons in outermost energy level The Periodic Table Representative Elements Groups 1,2 & 13-18 the number in the ones place
of the group number tells
us the number of valence electrons EXCEPT Helium Transition Elements have no rule relating to valence electrons the number of electrons in the
atoms outermost shell lets us
know how likely it is to bond Noble gases rarely bond
because they already have
8 valence electrons in their
outer shell Helium has a completed
outer shell even with
only 2 electrons Remember: 2n
1st shell= 2 electrons
2nd shell= 8 electrons
3rd shell= 18 electrons
4th shell= 32 electrons atoms with less than 8 valence electrons are more likely to form bonds form bonds by
gaining, losing, or
sharing electrons atomic number= # of protons atomic mass= total # of protons and neutrons
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