Structure 1

• Why are metals never gases?

  Metals have too high an atomic mass to be stable in gas form
• Combination reaction

  Reaction of COMPOUNDS to form new products (usually an aqueous reaction)
• Combustion reaction

  Any molecule/element/compound reacting with sole O2 in any quantity (when reacting with organic compounds, forming H2O and CO2)
• Single displacement reactions


  Switching the compositions between the elements for one of them (often seen with metals)

  ex. A + BC -> B + AC
• Double displacement reactions

  The dual switching of elemental compounds (usually seen with acids and bases)

  ex. AB + CD -> AD + CB
• Decomposition reaction

  The breaking of compounds into their separate elements

  ex. 2H2O -> O2 + 2H2
• Synthesis reaction


  The "normal" reaction- combining elements/molecules to create a final product/compound

  ex. O2 + 2H2 -> 2H2O
• An emission line spectrum proves the existence of discrete energy levels in an atom
• Matter

  Pure substances:

  Compounds

  Elements:

  Atoms:

  Electrons

  Nucleus:

  Protons

  Neutrons

  
  

  Mixtures:

  Homogenous

  Heterogenous
• Mass spectrometer

  Upon injecting a substance, it can either

  a ) detect a positive charge and identify composition by mass : charge ratio

  b ) detect more than one positive charge, and identify composition by mass only
• Radioactive elements

  Unstable, bigger masses that give off radiation due the their imbalance between negative and positive charges and their electrons consistently being excited. An example: Uranium 255
• Matter with uniform composition throughout

  Elements, Compounds, Homogenous mixtures
• Matter that retain their individual properties

  Homogenous mixtures, Heterogenous mixtures, elements
• Matter than has exact melting and boiling points

  Elements and Compounds
• Collisions between matter

  They are elastic, causing no loss in kinetic energy.
• Matter structure and attraction

  Solids have strong attraction and a clearly defined shape while gas molecules have a low attraction to each other and no clear shape
• Celsius to Kelvin

  + 273
• Ideal gases

  Exist when pressure is low, temperature is high, energy is high, gas particles are far apart and hold weak Van der Waal forces between them
• Real gases

  Exist when temperature is low, pressure is high, energy is low, particles have intermolecular attraction and are close together
• Relative atomic mass

  Average mass of naturally occurring isotope of an element compared with 1/12 of an atom of Carbon-12
• Filtration

  Insoluable solid separated from a solution
• Evaporation


  Soluable solid separated from a solution
• Solvation

  Soluble liquid separated from insoluble solid
• Distillation


  Separation of liquids based on boiling points
• Paper chromatography


  Separation of a mix of solutes based on their affinity for mobile of stationary movement
• Re-crystallization

  Separation of impurities from a solid
• Pure substances have definite compositions throughout
• Homogenous mixtures are uniform throughout and have a distinct, same boiling point
• Heterogenous mixtures are not uniform with distinct pieces from each material mixed- have different boiling points
• Compounds are chemical fusing of two or more substances, mixture is physical combination of two or more substances
• Solid to gas is sublimation
• Gas to solid is deposition
• solid to liquid is melting
• liquid to solid is freezing
• liquid to gas is boiling
• gas to liquid is condensation
• A lattice is a 3 dimensional arrangement of ions, atoms, and electrons
• In matter, collisions between particles are elastic
• the s-orbital can hold 2 electrons (1 spin)
• the p-orbital can hold 6 electrons (3 spins)