Lesson Plan. Lesson: Shape of Molecules. Aim: To investigate the shapes of molecules and ions. Learning Outcomes :
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1 Lesson Plan Lesson: Shape of Molecules Aim: To investigate the shapes of molecules and ions Learning Outcomes : At the end of the lesson, students will be able to : 1. explain the Valence Shell Electron Pair Repulsion Theory that governs the shape of molecules and ions. 2. predict and describe the shapes and bond angles of some covalent molecules and ions. Assumed prior knowledge : Students should already : 1. be able to draw Lewis structures of covalent molecules and ions. 2. be familiar with the concept of lone pairs and bonding pairs of electrons. Underlying Principles 1. Making the invisible, visible. 2. Enabling students to know what to look for. Time taken to complete the activities : 80 minutes Differentiation Questions in the student notes are designed to enable all students to complete the activity. The pop-up answers are provided for the students to view when they have considered their responses. Worksheet questions include questions that require recall, understanding and application of the new concepts learned Ministry Of Education Malaysia. All Rights Reserved. 1
2 Development of Lesson : No. Steps Strategy Resources 1 Set Induction. (Ascertaining prior Teacher to quiz students on the Lewis knowledge and symbols of some elements. Teacher to introducing lesson get students to suggest shapes of some topic for the day). simple molecules. Teacher to point out the role of electron pairs in determining molecular shapes and to introduce lesson objectives. 2 Student Activity Teacher to go through Activities 1-3 with the students. Courseware Activity 1 : Valence Shell Electron Pair Repulsion Students learn how the repulsion of electron pairs results in the shapes of CH 4, NH 3 and H 2 O. Activity 2 : More molecular shapes Students get to investigate the shapes of molecules of BeH 2, BF 3, PCl 5 and SF 6. Activity 3 : Shapes of ions Students get to investigate the shapes of the following ions : NH 4 + and H 3 O +. 3 Evaluation Students to answer questions in the student worksheet on their own. 4 Extension activity Students to go through the extension activities on their own. Worksheet Website and References Ministry Of Education Malaysia. All Rights Reserved. 2
3 Worksheet Answers 1. Valence Shell Electron Pair Repulsion Model 1.1 Bonding pair are two electrons of opposite spin localised between two atoms, and non-bonding pair are two electrons of opposite spin found in an orbital of an atom not bonded to another atom. 1.2 a. The central atoms of both haloalkanes have 4 bonding pairs of electrons. There are no non-bonding pairs of electrons on their central atoms. b. Both molecules are tetrahedral with a bond angle of o. This is because the four bonding pairs of electrons will repel each other, and the position of minimum repulsion is when they occupy the four corners of a tetrahedron. Thus, the bond angle corresponds to the angle of a tetrahedron, that is o. c. CH 3 Cl, CH 2 Cl 2, etc. 1.3 The Lewis structures of CCl 4 The central atom of CCl 4 has four bonding pairs of electrons. Thus, its molecular shape is tetrahedral. The Lewis structures of NCl 3 is The central atom of NCl 3 has three bonding pairs and one non-bonding pair of electron. Thus, its molecular shape is trigonal pyramid. The Lewis structures of OCl 2 is The central atom of OCl 2 has two bonding pairs and two non-bonding pairs of electrons. Thus, its molecular shape is V Ministry Of Education Malaysia. All Rights Reserved. 3
4 1.4 PCl 3 has similar molecular shape as ammonia. The central atom of NH 3 has three bonding pairs and one non-bonding pair of electrons. Thus, its molecular shape is trigonal pyramid. The central atoms of BCl 3 and AlCl 3 have three bonding pairs of electrons. Their molecular shape is trigonal planar. The central atom of PCl 3 has tree bonding pairs and one non-bonding pair of electrons. Thus, its molecular shape is the same as that of ammonia. The central atom of ICl 3 has three bonding pairs and two non-bonding pairs of electrons. Its molecular shape is known as distorted T-shape. 2. More Molecular Shapes 2.1 Bonding pair Non-bonding pair Molecular shape Bond angle 2 0 linear 180 o 2 1 V-shape Slightly less than 120 o 2 2 V-shape Slightly less than 109 o 3 0 Trigonal planar 120 o 3 1 Trigonal pyramid Slightly less than 109 o 3 2 T-shape ~180 o and ~90 o 2.2 The Lewis structures of PCl 3 and PCl 5 are The central atom of PCl 3 has three bonding pairs and one non-bonding pair of electrons. Thus, its molecular shape is trigonal pyramid with a bond angle of slightly less than o. The central atom of PCl 5 has five bonding pairs and no non-bonding pair of electrons. Thus, its molecular shape is trigonal bipyramid with a bond angle of 120 o and 90 o Ministry Of Education Malaysia. All Rights Reserved. 4
5 2.3 The Lewis structures of aluminium chloride and its dimer are The central atom of AlCl 3 has three bonding pairs and no lone pair of electrons. Thus, its molecular shape is trigonal planar with a bond angle of 120 o. The central atoms of Al 2 Cl 6 have four bonding pairs and no lone pair of electrons. Thus, the molecular shape at each centre is tetrahedral with a bond angle of o. 2.4 The molecular shapes of carbon dioxide and sulphur dioxide are different. The Lewis structures of carbon dioxide and sulphur dioxide are The central atom of CO 2 has two ( bonding pairs and no lone pair of electrons. Thus, its molecular shape is linear with a bond angle of 180 o. The central atom of SO 2 has two ( bonding pairs and one lone pair. Thus, its molecule is V-shaped. 3. Shapes of Ions 3.1 a. The central atom of NH 4 + is N. The Lewis structure is Shape : tetrahedral 2003 Ministry Of Education Malaysia. All Rights Reserved. 5
6 b. The central atom of NO 3 - is N. The Lewis structure is Shape : trigonal planar c. The central atom of CO 3 2- is C.The Lewis structure is Shape : trigonal planar d. The central atom of I 3 - is I. The Lewis structure is Shape : linear e. The central atom of SO 4 2- is S. The Lewis structure is Shape : tetrahedral 2003 Ministry Of Education Malaysia. All Rights Reserved. 6
7 3.2 The Lewis structure of NO 3 - ion is The central atom has three ( ) bonding pairs and no non-bonding pair. Thus, the molecular shape is trigonal planar. 3.3 The Lewis structure of (C 6 H 5 ) 3 C + is The central atom has three bonding pairs and no non-bonding pairs of electrons. Thus, the molecular shape is expected to be trigonal planar with a bond angle of 120 o Ministry Of Education Malaysia. All Rights Reserved. 7
At the end of this lesson, students should be able to :
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