Chapter 2: Inorganic Chemistry - PowerPoint PPT Presentation

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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 – PowerPoint PPT presentation

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Title: Chapter 2: Inorganic Chemistry


1
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

2
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

3
(No Transcript)
4
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

5
Covalent and Ionic bonds
6
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

7
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

8
H2O is a polar molecule, covalently bonded but
with an unequal distribution of shared electrons
9
Water is the versatile solvent
The hydrogen bonds between hydrogen and oxygen
cause unique properties of water
10
Polar solvents dissolve polar solutes
  • Sugar dissolves in water
  • Salt dissolves in water
  • Only ionic compounds form electrolytes in water

11
Nonpolar solutes do not dissolve in polar
solvents (water)
  • Salad oil
  • Oil
  • Gasoline
  • Vegetable shortening
  • butter

12
Acids, Bases, Buffers
pHyrion paper
  • Acids release H in solution
  • Bases release OH- in solution
  • Buffers resist changes in pH

13
pH scale
14
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
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