ch 5 1 review and 5 2 n.
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Ch 5-1 review and 5-2. Physical Sci. Which are compounds which are mixtures. SO 2 Air in a scuba tank Distilled water Oxygen gas Carbon monoxide. Structure of compounds. Three different types Network of bonded atoms Bonded positive and negative ions

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which are compounds which are mixtures
Which are compounds which are mixtures
  • SO2
  • Air in a scuba tank
  • Distilled water
  • Oxygen gas
  • Carbon monoxide
structure of compounds
Structure of compounds
  • Three different types
    • Network of bonded atoms
      • Bonded positive and negative ions
    • Separate molecules weakly attracted to each other
structure properties
Structure properties
  • Network of bonded atoms
    • Very strong solids
    • Takes a lot of energy to break the bonds
    • Very high melting and boiling points
    • Salt (NaCl)
    • Sand (SiO2)
    • Magnesium Fluoride (MgF2)

Some compounds are made of separate molecules weakly attracted to each other

    • The atoms within the molecule are strongly bonded together but they are not greatly attracted to other molecules
    • Low boiling points
    • Low melting points (can be solid but often liquid or gas at room temperature)
hydrogen bonds
Hydrogen bonds
  • Water molecules (and other polar molecules containing hydrogen) are polar
    • Polar means they have a negative end and a positive end
    • The hydrogen bond is not as strong as the bonds that make a water molecule
review questions
Review Questions
  • Why does AgI have a higher melting point than vanillin (a compound used for flavoring) C8H8O3
  • Which molecules have a greater attraction for each other, C3H8O rubbing alcohol, or CH4 molecules of methane gas
  • O-H bonds in water are 95.8 pm long while S-H bonds in dihydrogen sulfide are 135 pm. Why are S-H bonds longer?
5 2 ionic and covalent bonds
5-2 Ionic and Covalent Bonds
  • Three types of bonds exist
    • Ionic
    • Metallic
    • Covalent
  • Why do atoms bond
    • To obtain a full outer shell of electrons (stable electron configuration)
  • When do atoms bond
    • When valence electrons interact
what is a bond
What is a bond
  • Bonds are somewhat flexible
    • Think of them like stiff springs, they can bend, vibrate, move slightly back and forth
  • Bonds hold atoms together
electron configuration
Electron configuration
  • Bonding example 2 H come together to form H2
    • One valance electron (wants 2) so it shares with another hydrogen
ionic bonds
Ionic bonds
  • Form between oppositely charged ions
    • Metals bonding to nonmetals
  • Electrons are lost by one atom and gained by another atom to achieve stable electron configuration
  • Result is positive ion and negative ion
    • Opposites attract and from ionic bond
ionic bonds cont
Ionic Bonds cont.
  • Sodium ion Na+
  • Chlorine ion Cl-
  • Ionic bond NaCl
  • Net zero charge
  • Ionic bonds form networks
    • One salt molecule
    • But due to charges they form a network
ionic bonds conduct electricity
Ionic bonds conduct electricity
  • Solid ionic compounds do not conduct electricity because the ions are locked in place
  • But if they are dissolved in water or melted they will conduct electricity!