The Period Table/Periodic Chemistry

Grade 10 · Chemistry

Semester 1 | Period 3 | Week 15

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Subject: Chemistry

Semester: 1

Period: 3

Week: 15

School Name:
Teacher’s Name:
Subject: Chemistry
Grade Level: Grade 10
Week & Period: Week 15, Period III
Date:
Topic: The Periodic Table / Periodic Chemistry
Topic: Trends in Periodic Properties

  • Electronegativity
  • Ionization energy
  • Electron affinity
  • Atomic radius
  • Metallic and nonmetallic character
  • Ionic to covalent bonding in compounds
  • Lattice energy

Learning Objectives:

  • Discuss periodic trends: electronegativity, ionization energy, electron affinity, atomic radius, metallic and nonmetallic character
  • Explain ionic to covalent bonding in compounds
  • Understand lattice energy concept

Previous Knowledge:
Learners understand element placement on the periodic table.

Instructional Materials:

  • Charts of periodic trends
  • Visual aids for bonding types
  • Sample compounds for discussion

Anticipation (Warm-Up) – 5 minutes
Ask:

  • "Why do elements in the same group behave similarly?"
  • "What happens to the size of atoms as you move across a period?"

Building Knowledge (Main Lesson) – 25 minutes

  1. Trends in periodic properties
    • Electronegativity: ability to attract electrons
    • Ionization energy: energy to remove an electron
    • Electron affinity: energy change when gaining an electron
    • Atomic radius: size of atom
    • Metallic character and nonmetallic character
    • Explanation of ionic and covalent bonding
    • Lattice energy: energy to separate ions in ionic compound

Learners’ Activities:

  • Chart trends using example elements
  • Compare bonding types with sample compounds
  • Discuss trends in groups and present findings

Consolidation – 10 minutes
Questions:

  • What is electronegativity? Which element is most electronegative?
  • How does atomic radius change across a period?
  • What is lattice energy?

Homework / Assignment:

  • Create a chart showing 5 elements and their electronegativity, atomic radius, and ionization energy
  • Write short notes explaining ionic and covalent bonds

Notes – Detailed and Explained:

  • Electronegativity increases across a period and decreases down a group.
  • Ionization energy follows a similar trend to electronegativity.
  • Atomic radius decreases across a period and increases down a group.
  • Metallic character decreases across a period and increases down a group.
  • Ionic bonds form between metals and nonmetals; covalent bonds form between nonmetals.
  • Lattice energy reflects bond strength in ionic compounds.

Expanded Notes / Instructions:

  • Use visual diagrams for electron cloud size and bonding types.
  • Allow learners to use periodic table color codes for trends.
  • Offer guided questions to struggling learners.

Inclusive / Differentiation:

  • Use physical models of atoms and bonds for tactile learners.
  • Encourage peer tutoring during group work.

Teacher’s Reflection:

  • Did learners grasp periodic trends and their importance?
  • Were bonding concepts clear and linked to periodic table trends?