The following questions relate to the bonding in the OH-1 ion. (16 points)

Write the electron configuration for H. (1 point)

Write the electron configuration for O. (1 point)

Draw the molecular orbital diagram for OH-1. (5 points)

Draw the Lewis Structure for OH-1. (3 points)

Which orbitals in the molecular orbital diagram contain the lone pair electrons around O? (2 points)

What is the bond order for OH-1? (2 points)

Predict the bond order for OH+1. (2 points)

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To answer these questions, we need to have a basic understanding of electron configurations, molecular orbital diagrams, Lewis structures, and bond order calculations. Let's start with the first question.

1. Write the electron configuration for H. (1 point)
The electron configuration of hydrogen (H) is simply 1s^1. In the first energy level (shell), there is only one subshell, labeled 1s, and it can hold a maximum of 2 electrons. Hydrogen has only one electron, so it occupies the 1s^1 orbital.

2. Write the electron configuration for O. (1 point)
Oxygen (O) has atomic number 8, meaning it has 8 electrons. The electron configuration for oxygen is 1s^2 2s^2 2p^4. In the first energy level, there is the 1s subshell with 2 electrons. In the second energy level, there are the 2s and 2p subshells, each with 2 electrons.

3. Draw the molecular orbital diagram for OH-1. (5 points)
To draw the molecular orbital (MO) diagram for OH-1, we start by combining the atomic orbitals (AOs) of the hydrogen and oxygen atoms. The hydrogen atom has only one electron and one atomic orbital (1s), while the oxygen atom has 8 electrons and several atomic orbitals (1s, 2s, 2px, 2py, 2pz). We need to fill up the MOs in order of increasing energy, following the Pauli exclusion principle, Aufbau principle, and Hund's rule.

4. Draw the Lewis Structure for OH-1. (3 points)
In the Lewis structure of OH-1, we represent the atoms and their valence electrons using symbols and dots, where each dot represents one valence electron. Oxygen (O) has 6 valence electrons, while hydrogen (H) has 1 valence electron. We place a lone pair of electrons on the oxygen atom and bond the oxygen atom with the hydrogen atom using a single bond.

5. Which orbitals in the molecular orbital diagram contain the lone pair electrons around O? (2 points)
In the molecular orbital diagram of OH-1, the lone pair electrons around O are located in the highest energy occupied orbitals. Specifically, the highest energy occupied molecular orbitals are the antibonding orbitals, which are derived from the oxygen 2pz atomic orbitals. Therefore, the 2pz atomic orbitals contain the lone pair electrons.

6. What is the bond order for OH-1? (2 points)
The bond order is a measure of the strength and stability of a covalent bond. It is calculated by taking the difference between the number of bonding electrons and the number of antibonding electrons and dividing it by 2. In the case of OH-1, the bond order can be calculated as [(number of bonding electrons) - (number of antibonding electrons)] / 2. Counting the electrons in these orbitals in the MO diagram can help determine the bond order.

7. Predict the bond order for OH+1. (2 points)
To predict the bond order for OH+1, we need to consider how the change in charge affects the number of electrons. In OH+1, the positive charge means one electron is lost compared to OH-1. By calculating the bond order using the same method as before, the bond order for OH+1 can be obtained.