Activity 01
Hydride Property Sorting Challenge
Students in small groups receive cards with names of hydrides (e.g., LiH, CH4, H2S, TiH1.7) and property descriptions (e.g., 'gas at room temperature', 'conducts electricity in molten state'). They must match the properties to the correct hydride and then sort them into the three categories: ionic, covalent, and metallic.
Compare the properties of ionic hydrides like NaH and covalent hydrides like CH4.
Facilitation TipEncourage groups to justify their sorting using the periodic table and electronegativity trends.
What to look forUse an 'exit slip' where students must classify LiH, SiH4, and VH0.56 into their respective hydride types and list one defining property for each.
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Activity 02
Plot the Boiling Point Anomaly
Provide students with a data table of the boiling points for Group 15 and 16 hydrides. In pairs, they plot this data on a graph. The visual anomaly of NH3 and H2O leads to a guided discussion about hydrogen bonding.
Explain why metallic hydrides are often non-stoichiometric.
Facilitation TipAsk probing questions like, 'What force must be responsible for water's unusually high boiling point?'
What to look forA section in a unit test could ask students to draw and explain a graph of the boiling points of Group 16 hydrides, and to write the reaction for calcium hydride with water, identifying the products.
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Activity 03
Predict the Reaction
Present students with reaction scenarios, such as 'What happens when CaH2 is added to water?' or 'What happens when methane is burned in air?'. Students predict the products and write balanced chemical equations, reinforcing the chemical properties of different hydride types.
Analyse the trend in the boiling points of Group 16 hydrides (H2O, H2S, H2Se).
Facilitation TipStart with a demonstration of a safe reaction, like adding a metal to acid to produce hydrogen, to engage students.
What to look forStudents complete a 'Know-Want to know-Learned' (KWL) chart for the topic of hydrides before and after the lesson to reflect on their learning journey.
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Generate Complete Lesson→A few notes on teaching this unit
Use the periodic table as a visual guide throughout the lesson. Colour-code the s-block, p-block, and d/f-blocks to show where each type of hydride comes from. Use simple analogies: ionic hydrides are like 'salty' crystals, covalent hydrides are like individual 'molecular' families, and metallic hydrides are like a metal 'sponge' soaking up hydrogen. When discussing boiling points, have students first predict the trend based on size, then reveal the actual data to create a 'puzzle' that hydrogen bonding solves.
By the end of this lesson, your students will be able to look at a hydride's formula, predict its type, and describe its likely properties, such as its physical state and how it reacts with water.
Watch Out for These Misconceptions
All compounds with hydrogen are acids.
Hydrogen's chemical nature depends on the element it is bonded to. In ionic hydrides like NaH, hydrogen exists as the hydride ion (H-), which is a strong base and reacts with water to produce H2 gas and a basic solution.
Boiling points of hydrides must always increase down the group.
While boiling points generally increase down a group due to stronger van der Waals forces from more electrons, the hydrides of N, O, and F (NH3, H2O, HF) have exceptionally high boiling points for their size. This is due to strong intermolecular hydrogen bonding, which is much stronger than the van der Waals forces in the hydrides below them.
Metallic hydrides are just simple mixtures of a metal and hydrogen.
Metallic hydrides are interstitial compounds where hydrogen atoms occupy the empty spaces (interstices) in a metal's crystal lattice. They are not true compounds with fixed ratios, which is why they are often non-stoichiometric, like PdH0.6, and can alter the properties of the parent metal.
Methods used in this brief