Lesson Notes By Weeks and Term - Senior Secondary 1

Particulate nature of matter II

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  4. Particulate nature of matter II

Term: 1st Term

Week: 9

Class: Senior Secondary School 1

Age: 15 years

Duration: 40 minutes of 5 periods each

Date:       

Subject:      Chemistry

Topic:-       Particulate nature of matter II

SPECIFIC OBJECTIVES: At the end of the lesson, pupils should be able to

  1. Discuss the constituents of atoms
  2. Use diagrams to illustrate the arrangement of electrons around the nucleus

INSTRUCTIONAL TECHNIQUES: Identification, explanation, questions and answers, demonstration, videos from source

INSTRUCTIONAL MATERIALS: Videos, loud speaker, textbook, pictures

INSTRUCTIONAL PROCEDURES

PERIOD 1-2

PRESENTATION

TEACHER’S ACTIVITY

STUDENT’S ACTIVITY

STEP 1

INTRODUCTION

The teacher reviews the previous lesson on particulate nature of matter

Students pay attention

STEP 2

EXPLANATION

He discusses the constituents of atoms

 

Students pay attention and participates

STEP 3

DEMONSTRATION

Using diagrams, he illustrates the arrangement of electrons around the nucleus

Students pay attention and participate

STEP 4

NOTE TAKING

The teacher writes a summarized note on the board

The students copy the note in their books

 

NOTE

PARTICULATE NATURE OF MATTER

Atom

An atom is the smallest particle of an element which can take part in a chemical reaction. It is the smallest unit of matter that uniquely defines an element

An atom consists of a neutron, a proton and an electron.

The nucleus of an atom lies at its center and consists of protons and neutrons, which are collectively called the nucleons.

Electrons found in a space around the nucleus are known as orbitals.

A neutral atom has equal number of protons and electrons. The positive charge of a proton equals the negative charge of an electron. The charges cancel each other out and the atom is neutral. The volume of the atom is determined by the space that the electrons occupy.

The properties of the three sub atomic particles are as follows

 

Particle

Relative mass

Relative charge

Location

 

Proton, p

1

+1

Nucleus

 

Neutron, n

1

No charge (0)

Nucleus

 

Electron, e

1/1840 (negligible)

-1

Shells/orbitals

 

Atomic Structure

Electrons hold the key to almost all chemistry. Protons and neutrons give atoms their mass but electrons make up the outer part and are able to interact with one another. The arrangement of electrons determines the chemical property of the element.

The electrons move round the nucleus in clearly defined regions called shells. Electrons closest to the nucleus have the lowest energy while electrons that are further away from the nucleus have higher energies

An atoms shell can hold 2n2 electrons where n is the electron shell level; represented as K, L, M, N, O

EVALUATION:    1. Define atom

  1. List and explain the constituents of an atom
  2. Using diagrams illustrate the arrangement of electrons                    around a nucleus
  3. What is the maximum number of electrons per shell?

CLASSWORK: As in evaluation

CONCLUSION: The teacher commends the students positively