CHEMISTRY

 types of materials:  atoms, elements, elemental formula, compounds, chemical formula;  mixtures, physical, heterogeneous, homogeneous, suspension, solution, solvent, solute, concentration = amount of solute/volume total solution;  molarity (M),  mole = 6.02 x 10 ²³ particles, Avogadro’s number

Chemical reactions: reactants >>> products, coefficient = # of particles of a compound, subscript = # atoms of an element in a compound, conservation of mass; balancing equations

Bonding:  valence shell, Lewis dot diagram, up to 8 valence electrons;

ionic bonding:  atoms form ions to get a filled valence shell, superscript gives charge of an ion, chemical attraction holds the two ions adjacent to each other, ionic compounds, charges must balance, usually clusters rather than distinct pairs

covalent bonding:  sharing of unpaired valence electrons, molecules are held together by covalent bonds, electronegativity, polar molecules, dipoles, induced dipoles

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 Analyze the differences between atoms, elements, compounds and mixtures.

 
Explain the differences between heterogeneous and homogeneous mixtures, and the differences between solutions and suspensions.  How is the concentration of a solution calculated?  Why do chemists often use molarities rather than g/liter?

 
Be prepared to balance chemical reactions.