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Magazine Chapter 1: Problem 2
Write out and compare an orbital diagram for a neutral oxygen \((\mathrm{O})\) atom and an \(\mathrm{O}^{2-}\) ion.
Short Answer
Expert verified
Neutral O has 8 electrons (2 unpaired in 2p), while \(\text{O}^{2-}\) has 10 electrons (all paired in 2p).
Step by step solution
01
Identify the number of electrons
A neutral oxygen atom has 8 electrons (because its atomic number is 8). For the \(\text{O}^{2-}\) ion, add 2 more electrons to the neutral atom鈥檚 electron count, giving a total of 10 electrons.
02
Determine the electron configuration for neutral oxygen
The neutral oxygen atom鈥檚 electron configuration is 1s虏 2s虏 2p鈦�. This is determined by filling orbitals in the order of increasing energy levels: \[1s^2\] two electrons in the 1s orbital, \[2s^2\] two electrons in the 2s orbital, and \[2p^4\] four electrons in the 2p orbital.
03
Draw the orbital diagram for neutral oxygen
The orbital diagram for a neutral oxygen atom is as follows:1s: \[ \uparrow \downarrow \] 2s: \[ \uparrow \downarrow \] 2p: \[ \uparrow \uparrow \uparrow \downarrow \]
04
Determine the electron configuration for \(\text{O}^{2-}\) ion
The \( \text{O}^{2-} \) ion has a total of 10 electrons. The electron configuration is: 1s虏 2s虏 2p鈦�.
05
Draw the orbital diagram for \( \text{O}^{2-} \) ion
The orbital diagram for the \( \text{O}^{2-} \) ion is as follows:1s: \[ \uparrow \downarrow \] 2s: \[ \uparrow \downarrow \] 2p: \[ \uparrow \downarrow \uparrow \downarrow \uparrow \downarrow \]
06
Compare the two diagrams
In the neutral oxygen atom, the 2p orbital has four electrons with two of them paired and two unpaired. In the \( \text{O}^{2-} \) ion, the 2p orbital is fully filled with six electrons, all paired.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Electron Configuration
Electron configuration is the arrangement of electrons in an atom or ion. It follows a specific order based on the increasing energy levels of orbitals. For example, in the case of a neutral oxygen atom, the configuration is written as 1s虏 2s虏 2p鈦�. This means:
- Two electrons in the 1s orbital
- Two electrons in the 2s orbital
- Four electrons in the 2p orbital
Neutral Oxygen Atom
A neutral oxygen atom has an atomic number of 8, which means it has 8 protons and an equal number of electrons. The electron configuration of a neutral oxygen atom is 1s虏 2s虏 2p鈦�. To visualize this:
1s: \([]\)
2s: \([]\)
2p: \( \)to further display how the zero charge of the atom is retained by having an equal number of protons and electrons.
- 1s orbital has two electrons, both paired
- 2s orbital also has two electrons, both paired
- 2p orbital has four electrons; two are paired, and two remain unpaired
1s: \([]\)
2s: \([]\)
2p: \( \)to further display how the zero charge of the atom is retained by having an equal number of protons and electrons.
Oxygen Ion
When an oxygen atom gains electrons and becomes an \( \text{O}^{2-} \) ion, it means two additional electrons are added. This gives it a total of 10 electrons since:1. Neutral oxygen = 8 electrons2. \(\text{O}^{2-}\) ion adds 2 electronsThis changes the electron configuration to 1s虏 2s虏 2p鈦�, filling up the 2p orbital completely. Each energy level in orbitals can now be visualized like this:
1s: \([]\)
2s: \([]\)
2p: \( \)
- 1s: two electrons, both paired
- 2s: two electrons, both paired
- 2p: six electrons, all paired
1s: \([]\)
2s: \([]\)
2p: \( \)
Orbital Filling
Orbital filling follows specific rules to ensure electrons are placed in the lowest energy position. These rules include the Aufbau principle, which states electrons fill lower-energy orbitals first, Hund's rule that requires electrons to occupy every orbital singly before pairing up, and the Pauli exclusion principle, asserting no two electrons can have the same set of quantum numbers. For instance:
- Neutral Oxygen (1s虏 2s虏 2p鈦�) - filled as 1s, followed by 2s, then partially filled 2p orbitals
- Oxygen Ion \(\text{O}^{2-}\) (1s虏 2s虏 2p鈦�) - 1s and 2s filled first, followed by completely filled 2p
