how do you find the bond order of OH- and OH+?
I know bond order = #bonded e- - #antibonding electron/2
im not sure how to find Oh- and Oh+
To find the bond order of OH- and OH+, you need to know the Lewis structures of these molecules or ions. Here's how you can determine the bond order step by step:
1. Draw the Lewis structure: Start by determining the arrangement of atoms and the number of valence electrons for each molecule or ion. For OH-, the Lewis structure can be represented as H-O- with three lone pairs on the oxygen atom, while OH+ can be represented as H-O with two lone pairs on the oxygen atom.
2. Count the total number of valence electrons: Add up the valence electrons for all the atoms. For OH-, you have 1 (from hydrogen) + 6 (from oxygen) + 1 (from the negative charge) = 8 valence electrons. For OH+, you have 1 (from hydrogen) + 6 (from oxygen) - 1 (from the positive charge) = 6 valence electrons.
3. Determine the number of bonding and antibonding electrons: Look at the Lewis structure and identify the number of shared electron pairs (bonding electrons) and the number of lone pairs on the central atom (antibonding electrons). In both OH- and OH+, there is only one bond between the oxygen atom and the hydrogen atom.
4. Calculate the bond order: The bond order is the difference between the number of bonding electrons and the number of antibonding electrons, divided by 2. So, for OH-, the bond order would be (2 - 6) / 2 = -2 / 2 = -1. For OH+, the bond order would be (2 - 4) / 2 = -2 / 2 = -1.
In this case, both OH- and OH+ have bond orders of -1. Note that negative bond orders represent unstable molecules, indicating that they are more likely to dissociate rather than exist as stable entities.
To find the bond order of OH- and OH+, you would need to follow these steps:
1. Determine the Lewis structure of OH- and OH+:
OH-: Oxygen (O) is the central atom, bonded to a hydrogen (H) atom. There is also an extra electron, giving OH- a negative charge.
OH+: Oxygen (O) is the central atom, bonded to a hydrogen (H) atom. There is one electron missing, giving OH+ a positive charge.
2. Calculate the number of valence electrons for each species:
OH-: Oxygen has 6 valence electrons, hydrogen has 1 valence electron, and there is an extra electron, bringing the total to (6 + 1 + 1) = 8 valence electrons.
OH+: Oxygen has 6 valence electrons, hydrogen has 1 valence electron, and there is a missing electron, bringing the total to (6 + 1 - 1) = 6 valence electrons.
3. Assign the electrons to bonding and antibonding orbitals:
For OH-, you will have 8 electrons to distribute. Place 2 electrons in the bonding orbital (σ) between oxygen and hydrogen, and the remaining 6 electrons in nonbonding or lone pairs on the oxygen atom.
For OH+, you will also have 6 electrons to distribute. Place 2 electrons in the bonding orbital (σ) between oxygen and hydrogen, and the remaining 4 electrons in nonbonding or lone pairs on the oxygen atom.
4. Determine the number of bonding and antibonding electrons:
OH- has 2 bonding electrons and 6 nonbonding electrons.
OH+ has 2 bonding electrons and 4 nonbonding electrons.
5. Calculate the bond order:
Bond order = (number of bonding electrons - number of antibonding electrons) / 2.
For OH-, the bond order would be:
(2 - 6) / 2 = -4 / 2 = -2
For OH+, the bond order would be:
(2 - 4) / 2 = -2 / 2 = -1
So the bond order of OH- is -2, and the bond order of OH+ is -1.