Learning objectives
By the end of the lesson, students should be able to:
-
identify where metals and non-metals are found in the periodic table
-
describe typical physical properties of metals and non-metals
-
use practical evidence to classify unknown samples
-
explain why metals form positive ions
Using the interactive lesson
Booklet page 17 – Introduce the pattern
Begin with the retrieval questions on groups, outer-shell electrons and positive ions. Use the interactive periodic table to establish that most metals are found towards the left and bottom, while non-metals are mainly towards the right and top. Draw attention to hydrogen as a non-metal despite its position above Group 1.
Students then predict whether properties such as conductivity, shininess, brittleness and malleability are more typical of metals or non-metals before seeing experimental evidence.
Booklet page 18 – Virtual practical investigation
Use the virtual laboratory to investigate copper, sulfur, aluminium, graphite and iron.
Students can test each specimen for:
Encourage students to predict before testing. The animation can be played, paused, stepped through, replayed or explored using the progress control, making it useful for whole-class questioning as well as independent use.
Observations are added to the results area as tests are completed. Students can then select individual specimens, classify them as a metal or non-metal and justify their decision using evidence.
Emphasise precise observations such as “the bulb lit, so the sample conducted electricity” rather than vague descriptions such as “it worked”.
Booklet page 19 – Identify patterns and exceptions
Use the property comparison to establish the typical patterns:
-
metals are generally shiny, malleable and good electrical conductors
-
solid non-metals are generally dull, brittle and poor electrical conductors
The graphite example is particularly important. Graphite is a form of the non-metal carbon but conducts electricity, demonstrating why students should say usually, generally or typically rather than always.
Students then apply the evidence to the mystery samples and construct a scientific conclusion.
Booklet page 20 – From properties to chemical behaviour
Move from physical properties to the specification statement that metals react to form positive ions.
Use the animated atomic model to show that:
metal atom → loses electron(s) → positive ion
The animation keeps the nucleus and proton number unchanged while an electron leaves the atom. Use the proton and electron counts to make the origin of the positive charge explicit.
The sodium example develops this as:
2,8,1 → loses 1 electron → Na⁺ with 2,8
Students then compare lithium, sodium and potassium and connect their similar reactions to each having one electron in the outer shell.
Booklet pages 21–22 – Check and apply
Finish with the 12-question Quick Check. Students receive explanatory feedback and can revise their answers.
The exam-practice section follows the booklet questions and includes selected-response checking, suggested answers and self-assessment support for the longer responses. Use these questions to identify whether students need to revisit periodic-table position, practical evidence or electron loss.
Teaching tips and common misconceptions
Encourage students to describe properties as typical patterns rather than absolute rules. Graphite is deliberately included because it challenges the idea that all non-metals are electrical insulators.
Students may incorrectly think that an atom becomes positive by gaining protons. Reinforce that the number of protons does not change during an ordinary chemical reaction. A metal ion becomes positive because electrons have been lost.
Students may also assume that all metals are solids or all non-metals are gases. The five practical specimens are all solids, so remind students that this investigation alone cannot establish the states of every metal and non-metal.
Hydrogen is useful for reinforcing that position and properties should both be considered: it is a non-metal despite appearing above Group 1.
At this level, the important chemical pattern is that metals form positive ions by losing electrons. Detailed metalloid classification and the bonding explanation for graphite are not required for this lesson.
Practical safety
The virtual experiment can be used instead of, before or alongside a teacher demonstration or practical investigation.
If carrying out the real practical, follow the school's risk assessment and normal laboratory procedures. Use an appropriate low-voltage conductivity circuit, handle samples carefully and test brittle specimens gently over a tray. Eye protection should be worn where required by the practical procedure.
The simulation supports observation and scientific reasoning but does not replace the development of hands-on practical skills.
Display and independent use
For whole-class teaching, use Focus view to maximise the teaching area and make the visualisations easier to see on a projector. Full-screen viewing is also available where supported by the browser.
The interface includes Teal & Cream, Ocean, Plum and Slate colour schemes, allowing the display to be adjusted to suit the classroom or personal preference.
Students can also work through the lesson independently using the section navigation, Lesson Map and Previous/Next controls. Answers and explanations remain hidden until requested, allowing prediction and discussion before feedback is revealed.
The virtual practical and ion animations include stepped controls so teachers can pause at key points for questioning rather than allowing the complete process to run automatically.