chem review

• Which intermolecular force is the strongest?

  Hydrogen bonding
• London dispersion forces


  Weak forces between non-polar molecules
• Dipole-dipole forces


  polar molecules place themselves so opposite charged ends are close to each other
• Hydrogen bonding

  polar molecule has H+ N,F, or O and other molecule has N,F or O
• what affects the rates of reaction

  
  

  1. Rate of reaction can be increased by increasing the temp.
  2. Increasing concentration of reactants usually increases rate of reaction
  3. Catalyst increases the rate or reaction.
  4. Increasing available surface area of reactant increases rate of reaction
  5. The rate of chemical reaction depends on what reactants are.
• acids have:

  sour taste and produce H+ ions when dissolved in water.

  bases have:

  bitter taste and produce OH- ions when dissolved in water
• acid theories:

  Arrhenius: acids increase concentration of H+

  bronsted Lowry: acids are proton donors must have a removable proton

  lewis: acids can accept pair of electrons to form covalent bonds
• bases theories:

  Arrhenius: bases increase concentration of OH-

  bronsted lowry: bases are proton acceptors, must have non bonding electrons

  lewis: can donate pair of electrons to form covalent bonds
• primary alcohols

  oxidize to form aldehydes which oxidize to form carboxylic acids
• secondary alcohols

  oxidize to form ketones
• tertiary alcohol

  do not oxidize
• indicators

  1. Ph meter: uses electrical properties of solution to determine PH. 
  2. Litmus paper: red litmus paper turns blue in presence of a base, blue litmus paper turns red in presence of acid. 
  3. Universal Indicator: mixture of several indicators that show different colours at different PH levels
• primary battery


  single use

  example: alkaline battery
• alkaline battery


  3-5x more energy, poses a chemical hazard is they leak 

  example: A AA or AAA batteries
• secondary battery


  rechargeable 

  example: nicd or lithium ion battery
• NiCd battery (nickel cadmium)


  can be charged 1000 times + has 1.2-1.25V 

  example: power tools
• Lithium ion battery

  
  

  provides 3.7V + holds charge well and are lightweight 

  example: cell phone battery
• Safe Li ion battery


  the Ni conducts electricity at normal temperatures  
• Lead acid battery

  used in cars and are an old secondary battery, 12V 

  example: car battery
• Anode:

  electrode where oxidation occurs
• cathode:

  electrode where reduction occurs
• salt bridge:

  tube that only ions can flow through. Equalizes charge of half cells, maintains redox
• Anions:

  flows to anode
• cations:

  flows to cathode
• inert electrodes:

  do not participate in reactions
• electrolytic cells:

  uses electricity to drive non spontaneous redox reactions
• Markovnikovs rule:

  1 major + 1 minor product formed, to break double bonds
• Condensation:

  carboxylic acid + amine = amide + h2o
• Estérification:

  carboxylic acid + alcohol = ester + h20
• hydrolysis:

  ester or amide react to for carboxylic acid + alcohol
• Heisenberg Uncertainty principle:

  impossible to know where electron is
• Paulis exclusion principle:

  each orbital can max occupy 2 electrons of opposite spin
• Aufbau principle:

  start with 1st atom in periodic table + build up
• Hunds rule:

  every orbital is single occupied before double
• Corrosion:

  degration of metals due to electrochemical reaction
• Fuel battery:

  converts chemical energy into electrical energy without combustion. Only by product is water
• how to prevent corrosion:

  paint: works but must be kept intact

  alloys: prevent corrosion from within.

  galvanization: coats metals with more easily oxidized metals

  sacrificial anode: oxidizes + protects coated metal
• Resonance:

  same formula but different placements of lone and bonding pairs
• who created quantum mechanics?

  Erwin Schrödinger
• Ground state:

  most stable energy state