Ionic Compounds
Covalent Compounds
Molecular Geometry
Metallic Bonding
Intermolecular Forces
HL Topics
100
What is the formula of copper (I) sulfide?
Cu2S
100
Draw the lewis formula for : Ammonia , Carbon monoxide and Butane
100
Draw the Lewis diagram of CO2
State its molecular geomtery
State whether is is polar or non-polar
Linear
Non-Polar
100
How can the electrons in a metallic bond be described?
"Sea of elestrons" "Free floating" "Delocalized"
100
List the intermolecular forces in order of increasing strength
London dispersion forces < dipole induced dipole < dipole-dipole < hydrogen bonding
100
Draw a sketch of a sigma and pi bond.
200
Name two physical properties of solid ionic compounds
Poor electrical conductivity, Good solubility in water, High boiling point
200
Draw any polar covalent compound, indicate the dipole or partial positive / negative charges
Examples: water, ammonia, sulfur dioxide, etc.
200
What is the molecular geometry and bond angle in methane (CH₄)?
Tetrahedral
109.3º
200
Why does adding small amounts of carbon to iron make the metal harder? What is the resulting substance called?
Disrupts the regular arrangement of iron atoms/ions, reduces ability for atoms to slide over one another.
Called Steel / Aloy
200
What is the main interaction between ethanol molecules (C2H5OH)
Hydrogen bonding
200
What is the formal charge of the carbon atom
zero 0
300
Which two factors impact the relative strength of an ionic bond and how?
Difference in ionic radius (small = stronger) Difference in charge (bigger = stronger)
300
Draw an ozone molecule (O3) and describe the bond lengths and strengths
Single bond: Longer and weaker
Double bond: shorter and stronger
300
Draw a molecule where its molecular geometry is different to its electron geometry.
Name the molecular geometry and electron geometry.
Example:
300
Describe malleability
The ability of a metal or metal alloy to be formed into a variety of shapes by hammering it or rolling it into thin sheets.
300
How does increasing the amount of carbons in an alkane impact their boiling point?
Boiling point increases
Molecule gets longer, more points of contact for intermolecular forces, stronger intermolecular forces.
300
List 3 pieces of evidence disproving the kekulé structure of benzene
Same bond length and strength,
Bond length and strength halves,
enthalpy of hydrogenation halves,
undergoes substitution reactions,
only one isomer of benzene exists
400
Write the equation for the lattice enthalpy of magnesium sulfide including state symbols
MgS (s) → Mg2+ (g) + S2– (g)
400
State which allotrope(s) of carbon do not conduct electricity. Explain why.
diamond, no delocalized electrons (carbon has 4 covalent bonds)
400
Draw the 3 dimentional Lewis diagram and identify the molecular geometry of PCl3
Trigonal pyramidal
400
Place the following in order from weakest to strongest metallic bond: Mg, Na, K, Ca
K<Na<Ca<Mg
400
List 3 effects of hydrogen bonding in water
Cohesion, adhesion, surface tension, low density of solid water, high specific heat capacity, etc.
400
Count the number of sigma and pi bonds in the molecule below:
Sigma bonds: 4
Pi bonds: 1
500
Which has a more exothermic lattice enthalpy: NaBr or NaF ?
NaF (same cation (Na), Fluorine ion is smaller than brom
500
Draw and name 2 covalent molecules that are exceptions to the octet rule
(2 molecules)
500
Rank these molecules in order of increasing bond angle;
Ammonia, Boron trifluoride, Water
Water (104.5º)<Ammonia(107º)<Boron trifluoride(120º)
500
Which metal has the weakest metallic bonds?
Mercury (Hg)
500
What are the strongest intermolecular forces between molecules of propanone, CH3COCH3, in the liquid phase? (drawing recommended)
Dipole–dipole forces
500
Describe the type of hybridization of the oxygen atom in 
sp2 hybridization