Exam Practice
Structure 2: Comprehensive Review
Test your understanding of Bonding, Structure, and Material Properties (Topics 2.1 - 2.4).
Paper 1A|MCQ
Paper 1B|Data
Paper 2|Written
A
Paper 1A: Multiple Choice
Conditions: No Calculator. No Data Booklet. Average 1.5 mins per question.
Student Practice Set
1.
Which factor most significantly increases the lattice enthalpy of an ionic compound?
2.
What is the molecular geometry of the sulfite ion, ?
3.
(HL) Which statement about hybridization in ethyne () is correct?
4.
Why does Magnesium have a higher melting point than Sodium?
5.
Which distinct feature belongs to the bonding of Benzene ()?
6.
Which molecule contains a central atom with a non-zero formal charge?
7.
Why are alloys typically harder than their pure parent metals?
8.
How many (sigma) and (pi) bonds are in Propene ()?
B
Paper 1B: Data Analysis
Analysis Context
You are provided with the boiling points of Group 16 hydrides:
| Hydride | Boiling Point (K) |
|---|---|
| 373 | |
| 213 | |
| 232 | |
| 271 |
Intermolecular Forces Trends
Identify the anomaly in the trend and explain its high boiling point in terms of bonding.
Then, explain the general trend from to .
C
Paper 2: Extended Response (HL)
Expansion of the Octet
Consider the molecule Sulfur Tetrafluoride, .
- Deduce the Lewis (electron dot) structure.
- Predict the molecular geometry (shape) and bond angles.
- State the hybridization of the sulfur atom.
Organic Bonding & Hybridization
Consider the carbon-carbon bonds in Ethane (), Ethene (), and Ethyne ().
- Compare the bond lengths and bond enthalpies of the C-C bond in these three molecules.
- Explain the bond angle around the carbon atom in Ethene using hybridization.