Inorganic Chemistry Notes

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Inorganic Chemistry Notes
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Physical Chemical Changes
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Phases of Matter
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Structure of an atom
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Chemical Bonding
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• Chemical bond force that joins atoms to form a
  stable substance
• Compound substance made of the joined atoms of
  two or more different elements
• identified by a chemical formula Ex. CO2, H2O,
  C6H12O6, NaCl

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• Types of Chemical Bonds
• Covalent bonds when atoms share electrons to
  form molecules Ex. H2O
• Ionic bond formed when ions of opposite charge
  interact (are attracted to each other) Ex. NaCl
• Ion atom or molecule that has gained or lost
  one or more electrons
• Cation (aka. positive ion) has lost electrons,
  i.e. K, Na, Ca2
• Anion (aka negative ion) has gained electrons,
  i.e. Cl, F, O2

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• Types of Chemical Bonds
• Hydrogen bonds Weak attractions between polar
  molecules (i.e. water)

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Mixtures
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• Mixtures
• Mixtures - combination of substances that can be
  separated into its individual substances by
  appropriate physical changes
• Homogenous mixture completely uniform in
  composition, its components are not
  distinguishable
• Heterogenous mixture - not uniform in
  composition, its components are distinguishable
  Ex. Salad dressing, concrete

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• Mixtures
• Homogenous mixture completely uniform in
  composition, its components are not
  distinguishable
• Solution - type of homogeneous mixture in which
  solutes are dissolved in a solvent Ex. Air,
  seawater
• Suspension type of homogenous mixture in which
  particles are suspended in another substance ex.
  blood, river water

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SECTION 2 WATER AND SOLUTIONS
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• Water in Living Things
• 70 of your body is made of water
• 2/3 of the molecules in your body are water
  molecules
• cells are filled with water and surrounded by
  water
• water is known as the universal solvent
• Solvent - the substance that dissolves the solute
  when making a solution
• Solute - the substance that is being dissolved
  when making a solution

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10 Properties of Water
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• Water is inorganicbecause it does not contain
  carbon, H2O
• Water has a set molecular
• structure H2O
• 3. A Water molecule is held
• together by covalent bonds
• 4. Water molecules are held to
• each other by hydrogen bonds

/- charge
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• 5. Water is polar - because of its uneven
  distribution of charge results in most of the
  other unique properties of water
• Polar molecules (like water) dissolve polar and
  ionic molecules
• (like dissolves like)
• Nonpolar molecules do not dissolve well in water
• Important in membrane structure and function
• Water has a high specific heat
• Water heats slowly and retains heat longer than
  many other substances
• Important in helping organisms maintain body
  temperature through evaporation of water, which
  carries the heat away

O
_
H
H


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• 7. Cohesion and adhesion
• Waters polar nature makes it exhibit both
  cohesion and adhesion
• Cohesion attraction between water molecules
  (hydrogen bonds)
• causes surface tension
• causes drops of water to form
• Adhesion attraction between a water molecule
  and another substance
• causes substances to get wet
• causes capillary action

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Adhesion things get wet
Cohesion surface tension
Adhesion capillary action
Cohesion
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1. liquid water has a density of 1 g/ml - In
   general, solid water is less dense than liquid
   water

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Periodic Table
Number of Protons? Number of Neutrons? Atomic
Mass? Atomic Number?
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Acids and Bases
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• Acid compound that forms hydrogen ions in water
• Base compound that forms hydroxide ions in
  water, or removes hydrogen ions from water
• pH(stands for pondus hydrogenii meaning
  potential hydrogen) a value used to express the
  acidity or alkalinity of a solution

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• pH scale measures the concentration of hydrogen
  ions in solutions scale of 0 to 14
• 0 to 6.9 is acidic
• 7.0 is neutral
• 7.1 to 14 is basic or alkaline
• a solution of pH of 3 has 10 times more hydrogen
  ions than one with a pH of 4

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• Neutralization - the reaction of an acid with a
  base, so called because the properties of both
  the acid and base are diminished or neutralized.
• Buffer - a solution that resists changes in pH
  when moderate amounts of acids or bases are added
  to it.
• Is your whole body at a pH of 7, or does the pH
  change from one place to another? What do you
  think is the purpose of this arrangement?
• Answer It changes, not just within a body
  but within a cell, too. The purpose is to create
  unique environments, each with a specific
  purpose. For example, enzymes in the stomach are
  only functional at a pH between 1 and 2 to
  prevent them from digesting the body.