Chapter 2: Inorganic Chemistry

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Chapter 2 Inorganic Chemistry

• Atomic structure and the periodic table
• Bonds ionic, covalent (and hydrogen)
• Solubility and polarity, electrolytic properties
• Properties of water, hydrogen bonding
• Acids, bases and buffers

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Atomic structure

• Number of protons
• Number of protons number of neutrons
• (isotopes vary in neutrons)
• Equal to of protons
• Row on periodic table
• Group (1-8)
• (active bonding electrons)

• Atomic number
• Atomic mass
• Number of electrons
• Electron energy levels
• valence electrons

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Bonds involve valence electrons

• Metals tend to transfer electrons
• Nonmetals tend to take electrons when bonding
  with metals
• Nonmetals tend to share electrons when bonding to
  other non-metals

• Ions charged atoms due to the gain or loss of
  electrons
• Ionic bonds cations and anions
• Covalent bonds shared electrons

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Covalent and Ionic bonds
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Ionic bonds

• Metals form cations when they lose valence
  electrons
• Nonmetals form anions when they gain valence
  electrons
• Generally are hydrophilic, dissolve in water,
  form electrolytes
• Ionic equations show the ions into which they
  separate

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Covalent bonds

• Shared electrons
• Non-metals to non-metals
• Do not form ions in solution
• May be polar or non-polar covalent
• Covalent bonds are stronger than ionic bonds
• CHNOPS compounds of living things (organic) are
  covalently bonded

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H2O is a polar molecule, covalently bonded but
with an unequal distribution of shared electrons
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Water is the versatile solvent
The hydrogen bonds between hydrogen and oxygen
cause unique properties of water
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Polar solvents dissolve polar solutes

• Sugar dissolves in water
• Salt dissolves in water
• Only ionic compounds form electrolytes in water

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Nonpolar solutes do not dissolve in polar
solvents (water)

• Salad oil
• Oil
• Gasoline
• Vegetable shortening
• butter

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Acids, Bases, Buffers
pHyrion paper

• Acids release H in solution
• Bases release OH- in solution
• Buffers resist changes in pH

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pH scale
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Biological systems depend on buffers

• Narrow tolerances to changes in pH
• Acid rain alters pH of soils and aquatic
  ecosystems
• Limestone is used as a buffer in acidified lakes