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2-1 The Nature of Matter
Pages 34 – 39
(2 Goals)
Goal 1
Review basic chemistry concepts
• Atoms– Basic unit of matter– Made up of 3 subatomic particles– Atoms have a net neutral charge
– Proton• Large particle• + charge
– Neutron• Large particle• No charge
– Electron• Small particle• - charge
• Element– Specific # of protons– Unique properties
• Reading Periodic table– Atomic # number of
protons or electrons
– Mass number total number of protons + neutrons
– Right column number of electrons, bottom number indicates valence electrons
6 24
carbon12
35 28
187
bromine80
• Isotopes– Same number of protons– Different number of neutrons– Chemical properties remain same– Mass number changes– Mass changes
• Example – One atom of “Carbon”
• 6 protons• 6 neutrons• Atomic mass ~ 12
– One isotope of “Carbon – 14” • 6 protons• 8 neutrons !!!• Atomic mass ~ 14
• How many neutrons are in the following isotopes?– Nitrogen -15– Sulfur – 35– Calcium – 45– Iodine - 131
• Radioactive isotopes– Nuclei fall apart– Unstable
• Radioactive tracers– Short-lived– Medicine
• Tumor location• Treatment• Drug path
PD-gov NIH
Goal 2
Review covalent and ionic bonding and compounds
• Compound
– Two or more different elements chemically combined
O2 H2
H2O HNO3 CO2
C6H12O6
• Covalent bonding– Forms covalent compounds– Molecules– Share electrons
– Memorize the following molecules and their chemical formulas:
• Water H2O
• Ammonia NH3
• Methane CH4
• Carbon dioxide CO2
• Ionic bonding– Forms ionic compounds– Transfer of electrons– + and – charges attract each other
– Memorize the following ions and their chemical formulas:
• Sodium chloride NaCl• Potassium chloride KCl
• Calcium carbonate CaCO3
• Magnesium sulfate MgSO4