Chemical Bonding and Structure

• ionic bond

  electrostatic attraction between oppositely charged ions in a lattice structure
• What is the attraction between positive and negative ions that forms an ionic bond called?

  electrostatic attraction
• What is the electronegativity difference for ionic bonds?

  x>=1.8
• What is the structure of ionic compounds like?

  crystalline lattice structure
• What is the state of ionic compounds under standard conditions?

  solids
• what is the melting point for ionic compounds like?

  melting point

  - greater ionic charge and smaller ionic radius means a higher melting point
• what is the volatility like for ionic compounds?

  volatility

  - strong forces of attraction between ions in ionic compounds cause low volatility
• how do ionic compounds dissolve in water?

  1. lattice structure breakdown

  2. ion separation
• what is the solubility of ionic compounds in nonpolar solutions like?

  nonpolar solvents cannot disrupt the lattice in the same manner
• what is the electrical conductivity of ionic compounds like?

  depends on the presence of mobile ions

  
  

  when ionic compounds are molten the ions are free to move and carry an electric current
• what is the brittleness like for ionic compounds?

  fracture across a plane when layers of ions become incorrectly aligned
• what are the properties of silicon dioxide? (MP/BP, volatility, conductivity, solubility)

  - high melting point

  - poor conductor

  - insoluble in water
• what is the vsepr distribution of silicon dioxide?

  tetrahedral - 109.5
• what are the properties of a diamond? (MP/BP, volatility, conductivity, heat, solubility)

  - high melting point

  - poor conductor (no delocalized electrons)

  - good heat

  - involatile

  - not soluble
• what is the vsepr distribution of diamond?

  tetrahedral - 109.5
• what are the properties of graphite? (MP/BP, volatility, conductivity, solubility)

  - soft

  - LDFs hold layers together making it soft

  - good electrical conductor due to delocalized 4th electron
• what is the bonding like in graphite?

  each carbon is bonded to 3 other atoms
• how are layers of graphene held together?

  LDF
• what are the properties of fullerene? (MP/BP, volatility, conductivity, solubility)

  - poor conductor due to having delocalized electrons that are unable to jump between individual fullerenes

  - high melting points
• what is the bonding like in fullerene?

  each bonded to 3 other atoms
• what 2 factors affects the melting point of a pure metal?

  charge and ionic radius
• what happens to the melting point trend down the halogen group?

  increases due to increased van der waals
• what happens to the melting point trend down the group 1 metals?

  decreases due to increased ionic radius
• why does reactivity increase down group 1?

  The number of electron shells increases down the group so there is more electron shielding. As a result, there is weaker attraction between the positive nucleus and outer shell electron. This means it is easier to remove an outer shell electron to form a positive metal ion.
• Why does reactivity increase as you go up group 17?

  atomic radius increases in size with an increase of electronic energy levels metal vs non metal behavior