Bonding Flashcards
Define ionic bonding
Strong electrostatic FOA btw oppositely charged ions
Why do ionic compounds have a high melting point?
- Lots of strong electrostatic FOA btw oppositely charged ions
- Forming giant ionic lattice
- Needs alot of energy to overcome bonds
When can ionic compounds conduct electricity?
- Molten/ dissolved
- Ions are free to move + carry a charge
Why do ionic compounds dissolve in water?
- Water molecules = polar (parts of molecule has small -ve charge + +ve charge)
- Charged parts pull ions away from lattice
Sulfate
SO4 2-
Hydroxide
OH-
Nitrate
NO3 -
Carbonate
CO3 2-
Ammonium
NH4+
Define covelant bond
Shared pair of e-
What are the 2 types of covelant structures?
- Molecular
- Giant covelant
Define dative covelant
When 1 atom donates a shared pair of e-
Describe the structure of graphite + its properties
- Giant covelant
- High MP + insoluble - lots of strong covelant bonds need to be broken
- VDW btw layers allow layers to slide past each other
- Conducts electricity - delocalised e- are free to move + carry charge
- Low density - layers are far apart
Describe the structure of diamond + its properties
- Giant covelant
- Shape: tetrahedral, C bonded to 4 C
- High MP, hard + insoluble - lots of strong covelant bonds
- Good thermal conducter - vibrations travel easily
- Can’t conduct electricity - outer e- held in localised bonds
Which type of bonding pair has the biggest angle?
- LP to LP
- Repel more than BP
Define electronegativity
Power of an atom to attract pair of e- in a covelant bond
Define dipole
Diff in charge btw 2 atoms caused by shift in electron density in bond
Explain why some molecules w/ polar bonds don’t have a permanent dipole
If polar bonds are arranged symmetrically, charges cancel out
Explain how a permanent dipole occurs
E- distribution in covelant bond btw elements w/ diff. electronegativities will be unsymmetrical, produces polar bond
Outline how Van der Waals are formed
- e- movement in first molecule
- Induces dipole in another molecule
- δ+ attracts δ- in adjacent molecules
What affects the strength of VDW?
- Longer chain - more e- so stronger VDW
- Straight chain - lie closer together so stronger forces
Outline how H bonds are formed
- F, N + O are v electronegative so draw bonding e- away from H
- Bond is polarised + H has high charge density
- Causes H atoms to form weak bonds w/ LP on F, O + N
Define metallic bonding
Electrostatic FOA btw the +ve metal ions and the delocalised electrons
Outline the properties of metals
- High MP - lots of electrostatic FOA btw +ve metal + sea of delocalised e- - more DE, stronger the bond
- Good thermal conducter - DE pass kinetic energy
- Good electrical conducter - DE move + carry current
- Insoluble
Outline the factors affecting the strength of metallic bonding
- No. protons - more protons = stronger bond
- No. DE per atom - more DE = stronger bond
- Size of ions - smaller ion = stronger bond
Why do simple covelant molecules have low MP + BP?
Only have to break IMF BTM, not covelant bonds
Ionic
Eg.
MP + BP
State at room temp
Does solid conduct electricity
Does liquid conduct electricity
Is it soluble in water
- NaCl
- High
- Solid
- No
- Yes
- Yes
Simple covelant
Eg.
MP + BP
State at room temp
Does solid conduct electricity
Does liquid conduct electricity
Is it soluble in water
- CO2, I2
- Low
- I2 is solid but usually liquid + gas
- No
- No
- Depends on polarity
Giant covelant
Eg.
MP + BP
State at room temp
Does solid conduct electricity
Does liquid conduct electricity
Is it soluble in water
- Diamond, graphite
- High
- Solid
- No exp. graphite
- Sublimes, doesn’t melt
- No
Metallic
Eg.
MP + BP
State at room temp
Does solid conduct electricity
Does liquid conduct electricity
Is it soluble in water
- Fe, Mg
- High
- Solid
- Yes
- Yes
- No