Predict the molecular and bond angle for each molecule or ion given below: SO3, ClO3-, NF3, SO42-
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To predict the molecular and bond angles for each molecule or ion, we need to follow a few steps:
Step 1: Determine the Lewis structure of the molecule or ion.
Step 2: Count the total number of electron domains (lone pairs + bonding pairs) around the central atom.
Step 3: Determine the molecular geometry based on the electron domain arrangement.
Step 4: Determine the bond angle based on the molecular geometry and any lone pairs.
Let's apply these steps to each molecule or ion:
1. SO3 (Sulfur trioxide):
Step 1: The Lewis structure of SO3 contains a central sulfur atom bonded to three oxygen atoms. The sulfur atom has three lone pairs.
Step 2: The total number of electron domains around sulfur is 3 (3 oxygen atoms).
Step 3: The electron domain arrangement is trigonal planar.
Step 4: Since there are no lone pairs on sulfur, the bond angles are approximately 120 degrees.
2. ClO3- (Chlorate ion):
Step 1: The Lewis structure of ClO3- shows a central chlorine atom bonded to three oxygen atoms. The chlorine atom has one lone pair.
Step 2: The total number of electron domains around chlorine is 4 (3 oxygen atoms + 1 lone pair).
Step 3: The electron domain arrangement is tetrahedral.
Step 4: The presence of a lone pair causes distortion, resulting in a pyramid-like shape. The bond angle is approximately 109.5 degrees.
3. NF3 (Nitrogen trifluoride):
Step 1: The Lewis structure of NF3 displays a central nitrogen atom bonded to three fluorine atoms. Nitrogen has one lone pair.
Step 2: The total number of electron domains around nitrogen is 4 (3 fluorine atoms + 1 lone pair).
Step 3: The electron domain arrangement is tetrahedral.
Step 4: With one lone pair, the molecular geometry becomes trigonal pyramidal, and the bond angle is approximately 107 degrees.
4. SO42- (Sulfate ion):
Step 1: The Lewis structure of SO42- exhibits a central sulfur atom bonded to four oxygen atoms. There are two additional oxygen atoms with a double bond.
Step 2: The total number of electron domains around sulfur is 6 (4 oxygen atoms and 2 double bonds).
Step 3: The electron domain arrangement is octahedral.
Step 4: However, one of the electron domains is a double bond, so the molecular geometry becomes tetrahedral, with bond angles of approximately 109.5 degrees.
Remember that these values are approximate and may vary slightly depending on factors such as lone pair repulsion and bond length.