S3.1 The periodic table: classification of elements questions for IB Chemistry
189 questions on The periodic table: classification of elements, written by Augment in the style of IB exam papers. Six of them are below in full, to answer on paper.
- IB Chemistry
- Part of S3 Classification of matter
- SL and HL
Questions by paper and level
SL and HL questions are for students at either level. HL only questions cover what only HL students study.
| Paper | SL and HL | HL only | All |
|---|---|---|---|
| Paper 1A | 57 | 31 | 88 |
| Paper 1B | 15 | 10 | 25 |
| Paper 2 | 44 | 32 | 76 |
| Every paper | 116 | 73 | 189 |
Counted on
Questions to try
Written by Augment in the style of IB exams, not past papers. Answer them on paper, then check each one against its markscheme with a free account.
Element X is in group 2 and element Y is in group 15 of the periodic table.
What is the formula of the ionic compound formed between X and Y?
A student used a database to investigate whether the melting points of s-block metals depend on the charge-to-radius ratio of their cations. The ratio was calculated as (charge on ion ÷ ionic radius in 10−12 m) × 100.
Metal | Ion | Ionic radius / × 10−12 m | Charge-to-radius ratio | Melting point / °C |
|---|---|---|---|---|
Cs | Cs+ | 167 | 0.60 | 28.44 |
Rb | Rb+ | 152 | 0.66 | 39.30 |
K | K+ | 138 | 0.72 | 63.38 |
Na | Na+ | 102 | 97.79 | |
Li | Li+ | 76 | 1.32 | 180.5 |
Ba | Ba2+ | 135 | 1.48 | 725.0 |
Sr | Sr2+ | 118 | 1.69 | 768.8 |
Ca | Ca2+ | 100 | 2.00 | 842.0 |
Mg | Mg2+ | 72 | 2.78 | 650.0 |
Be | Be2+ | 45 | 4.44 | 1287 |
The group 1 data were plotted with a linear trend line (y = 205.8x − 94.2, R2 = 0.988). The group 2 points for Ba, Sr and Ca are also shown.
- group 1 trend line
- (a)
Calculate the missing charge-to-radius ratio for Na+.
1 mark
- (b)
Describe the relationship for the group 1 metals and comment on the value of R2.
2 marks
- (c)
Explain, in terms of metallic bonding, why the melting point increases as the charge-to-radius ratio of the cation increases.
2 marks
- (d)
Ca, Sr and Ba lie well above the group 1 trend line. Suggest a reason, other than the charge-to-radius ratio, for their higher melting points.
1 mark
- (e)
Magnesium and beryllium do not follow the trend shown by Ca, Sr and Ba. The student suggests that boiling points would be a better test of the hypothesis. Explain why.
2 marks
- (f)
Suggest one reason for using database values rather than measuring these melting points in the laboratory.
1 mark
The boiling points of the hydrogen halides are shown.
Hydrogen halide | HF | HCl | HBr | HI |
|---|---|---|---|---|
Boiling point / °C | 20 | −85 | −67 | −35 |
- (a)
State the types of intermolecular force present in liquid hydrogen chloride.
1 mark
- (b)
Explain the increase in boiling point from HCl to HI.
2 marks
- (c)
Explain why the boiling point of HF is much higher than that of HCl.
2 marks
- (d)
Using section 9 of the data booklet, calculate the electronegativity difference in the H–F and H–I bonds and deduce which bond is more polar.
2 marks
- (e)
Suggest how the data for HCl, HBr and HI show that London forces, rather than dipole–dipole forces, dominate the intermolecular attraction in these compounds.
1 mark
What is the name of ?
A student used a database to investigate the strength of metallic bonding across period 4, using the enthalpy of atomization, ΔHat (the enthalpy change to form one mole of gaseous atoms from the element in its standard state).
Element | K | Ca | Sc | Ti | V | Cr | Mn | Fe | Co | Ni | Cu | Zn |
|---|---|---|---|---|---|---|---|---|---|---|---|---|
Number of 3d + 4s electrons | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 |
ΔHat / kJ mol−1 | 89 | 178 | 378 | 470 | 514 | 397 | 281 | 416 | 425 | 430 | 338 | 131 |
The student drew a straight line through the points for K and Ca and extended it.
- line through K and Ca
- (a)
Suggest why the enthalpy of atomization is a better measure of the strength of metallic bonding than the melting point.
1 mark
- (b)
Use the line to predict ΔHat for scandium and calculate the percentage error of this prediction, taking the database value as correct.
2 marks
- (c)
Suggest why scandium's actual value is higher than the line predicts, although the line already allows for its extra delocalized electron.
2 marks
- (d)
From chromium onwards, the values lie well below the line. Suggest a reason, with reference to the electron configurations.
2 marks
- (e)
Identify the element in the series Ti to Ni that does not follow the general pattern of its neighbours.
1 mark
At room temperature and pressure, fluorine and chlorine are gases, bromine is a liquid and iodine is a solid.
- (a)
Draw the Lewis (electron dot) formula of a chlorine molecule, Cl2.
1 mark
- (b)
Explain the change in physical state down group 17.
2 marks
- (c)
Iodine dissolves readily in hexane but only very slightly in water. Explain this difference.
2 marks
- (d)
Iodine sublimes on gentle warming. State what is overcome when iodine sublimes.
1 mark
- (e)
Using section 12 of the data booklet, identify the halogen molecule with the strongest covalent bond.
1 mark
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The notes on S3.1 The periodic table: classification of elements
More questions in Classification of matter
- S3.1The periodic table: classification of elementsThis page
- S3.2Functional groups: classification of organic compounds
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