IB Chemistry Paper 2 SL - Mistakes I've Made

Deduce the Lewis (electron dot) structure for the nitrate anion.

always include state symbols

what equation other than moles/mr would you use here to find the answer

n=cv

Deduce the Lewis (electron dot) structure and shape for dinitrogen monoxide showing nitrogen as the central atom.

State the ground-state electron configuration for copper.

State the ground-state electron configuration for Fe2+

Explain, with reference to Le Châtelier’s principle, the effect of using dilute rather than concentrated sulfuric acid as the catalyst on the yield of the reaction.

dilute adds «excess»

water OR water is a product ✔

shift left AND decreases yield

Explain, with reference to intermolecular forces, why B is more volatile than A

B = C3H5O

A has hydrogen bonding/bonds AND B does not ✔

hydrogen bonding/bonds stronger «than dipole-dipole»

brown/orange/red/yellow to colourless ✔

Write an equation that shows how sulfur dioxide can produce acid rain.

Suggest two variables, other than concentration, that should be controlled when comparing relative rates at different temperatures.

Any two of: depth/volume «of solution» ✔ colour/darkness/thickness/size/background of mark ✔ intensity of lighting in the lab ✔

Discuss two different ways to reduce the environmental impact of energy production from coal.

add lime during combustion ✔

not allow sulfur oxides to be released into the environment ✔

reduce proportion/percentage of energy/power produced by «the combustion of» coal ✔

What is the electronic configuration of chromium?

[Ar] 3d⁵ 4s¹

What is the electronic configuration of copper

[Ar] 3d¹⁰ 4s¹

Compare and contrast the combustion of an s-block metal and a p-block non-metal.

1. both are oxidation reactions ✓

2. s-block metals produce ionic oxides AND p-block non-metals produce covalent oxides✓

Suggest why water was chosen to extract ascorbic acid from the spinach leaves with reference to its structure.

«ascorbic acid» has multiple −OH/hydroxyl groups ✔

can H-bond with water ✔

Suggest a reason why the volume of hydrogen gas collected was smaller than predicted.

gas leaked/ignited ✔

Describe two observations that indicate the reaction of lithium with water is exothermic

temperature of the water increases ✔ lithium melts ✔ pop sound is heard ✔

Explain why the first ionization energy of calcium is greater than that of potassium

increasing number of protons/nuclear charge/Zeff ✔

similar shielding «by inner electrons» ✔

Define first ionisation energy

The first ionisation energy is the energy required to remove one mole of the most loosely held electrons from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+

All models have limitations. Suggest two limitations to this model of the electron energy levels

does not represent sub-levels/orbitals ✔

only applies to atoms with one electron/hydrogen ✔

does not take into account the interactions between atoms/molecules/external fields ✔

does not consider the number of electrons the energy level can fit ✔

Draw an arrow, labelled X, to represent the electron transition for the ionization of a hydrogen atom in the ground state.

upward arrow X AND starting at n = 1 extending to n = ∞ ✔

Draw an arrow, labelled Z, to represent the lowest energy electron transition in the visible spectrum

downward or upward arrow between n = 3 and n = 2 ✔

State the meaning of a strong Brønsted–Lowry acid.

fully ionizes/dissociates ✔ proton/H+ «donor »✔

C60 and diamond are allotropes of carbon. (i) Outline one difference between the bonding of carbon atoms in C60 and diamond.

C60 fullerene: «each carbon is» bonded to 3 C AND diamond: bonded to 4 C

Explain why C60 and diamond sublime at different temperatures and pressures.

diamond giant/network covalent AND sublimes at higher temperature ✔ C60 molecular/London/dispersion/intermolecular «forces» ✔

State two features showing that propane and butane are members of the same homologous series.

C4H8 (g) + HBr (g) → C4H9Br (l)

what equation would you use for this

«ΔH = bond breaking – bond forming = 656 kJ – 755 kJ» = –99 «kJ» ✔

what is the lewis diagram for oxygen, O2

what does this make the average bond enthalpy

498 kJ mol−1

what is the lewis diagram for carbon dioxide

what does this make the average bond enthalpy

804 kJ mol−1

The data booklet value for enthalpy of combustino of methanol is -726 kJ mol ^ -1

Suggest why this differs from values calculated in part a/b

bond enthalpies are averages

Give examples of weak acids accoording to bronsted lowry theory

Hydrogen Sulfide (H₂S)

Carbonic Acid (H₂CO₃)

Phosphoric Acid (H₃PO₄)

Give examples of strong acids accoording to bronsted lowry theory

Hydrochloric Acid (HCl)

Nitric Acid (HNO₃)

Sulfuric Acid (H₂SO₄)

Hydrobromic Acid (HBr)

Give examples of weak bases accoording to bronsted lowry theory

Ammonia (NH₃)

Aluminium hydroxide( Al(OH)₃)

Lead hydroxide (Pb(OH)₂)

Give examples of strong bases accoording to bronsted lowry theory

Sodium Hydroxide (NaOH)

Potassium Hydroxide (KOH)

Lithium Hydroxide (LiOH)

Explain the differences in boiling point in butane, propanal and propan - 1 - ol

Butane has the lowest boiling point due to its nonpolar nature and weak London dispersion forces.

While propanal has a higher boiling point due to the presence of polar dipole-dipole interactions.

Propan-1-ol has the highest boiling point among the three due to the additional formation of strong hydrogen bonds between its molecules.

State the half equations occuring at the cathode in a hydrogen oxygen fuel cell in an alkaline medium

O₂​ + 2H₂​O + 4e⁻ → 4OH⁻

State the half equations occuring at the anode in a hydrogen oxygen fuel cell in an alkaline medium

2H₂​ + 4OH⁻ → 4H₂O + 4e⁻

Draw and label an energy level diagram for the hydrogen atom