Sketch, on paper, the Lewis structure of I2, remembering to:Step 1: Arrange the atomsStep 2: Count the number of valence electrons.Step 3: Allocate two electrons between each pair of atoms which are assumed to be covalently bound.Step 4: Use the remaining valence electrons to form lone pairs, and/or double and triple bonds.What is the total number of valence electrons in I2?What type of bond exists between the iodine atoms?How many lone pairs are there on the each iodine atom?
Question
Sketch, on paper, the Lewis structure of I2, remembering to:Step 1: Arrange the atomsStep 2: Count the number of valence electrons.Step 3: Allocate two electrons between each pair of atoms which are assumed to be covalently bound.Step 4: Use the remaining valence electrons to form lone pairs, and/or double and triple bonds.What is the total number of valence electrons in I2?What type of bond exists between the iodine atoms?How many lone pairs are there on the each iodine atom?
Solution
Step 1: Arrange the atoms In I2, there are two iodine atoms. So, arrange them side by side.
Step 2: Count the number of valence electrons. Iodine is in Group 17 (also known as Group 7A) of the periodic table, which means it has 7 valence electrons. Since there are two iodine atoms, the total number of valence electrons in I2 is 7*2 = 14.
Step 3: Allocate two electrons between each pair of atoms which are assumed to be covalently bound. Allocate two of the 14 valence electrons to form a bond between the two iodine atoms. This leaves 12 electrons.
Step 4: Use the remaining valence electrons to form lone pairs, and/or double and triple bonds. The remaining 12 electrons will be distributed as lone pairs around the two iodine atoms. Each iodine atom will have 6 lone pairs.
The total number of valence electrons in I2 is 14.
The type of bond that exists between the iodine atoms is a single covalent bond.
Each iodine atom has 3 lone pairs.
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