Problem 83 - Chemistry Matter and Change

Question

Write the electron configuration and draw the orbital notation for atoms of oxygen and sulfur.

Step-by-Step Solution

Answer

The electron configurations and orbital notations for oxygen and sulfur atoms are as follows: Oxygen (Z = 8): Electron configuration: \(1s^2 2s^2 2p^4\) Orbital notation: ``` 1s: [↑↓] 2s: [↑↓] 2p: [↑ ↑ ↑ ] [↓ ↓ (empty)] ``` Sulfur (Z = 16): Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^4\) Orbital notation: ``` 1s: [↑↓] 2s: [↑↓] 2p: [↑ ↑ ↑ ] [↓ ↓ ↓ ] 3s: [↑↓] 3p: [↑ ↑ ↑ ] [↓ ↓ (empty)] ```

Step 1: Identify atomic numbers of oxygen and sulfur

In order to write the electron configuration for each element, we have to first find their atomic numbers. The atomic number (Z) of an element is equal to the number of electrons in a neutral atom of that element. Oxygen has an atomic number (Z) of 8, which means it has 8 electrons. Sulfur has an atomic number (Z) of 16, which means it has 16 electrons. Now, we will write the electron configuration and orbital notation for these atoms.

Step 2: Write the electron configuration for oxygen and sulfur atoms

Using the Aufbau principle and remembering the Pauli Exclusion Principle, we will fill the orbitals in increasing order of energy. Oxygen (Z = 8): 1s^2 2s^2 2p^4 Sulfur (Z = 16): 1s^2 2s^2 2p^6 3s^2 3p^4

Step 3: Draw the orbital notation for oxygen and sulfur atoms

Keeping Hund's Rule in mind, which states that electrons will fill degenerate orbitals singly before pairing up, we will represent the electron configuration in the orbital notation. For Oxygen (Z = 8): ``` 1s: [↑↓] 2s: [↑↓] 2p: [↑ ↑ ↑ ] [↓ ↓ (empty)] ``` For Sulfur (Z = 16): ``` 1s: [↑↓] 2s: [↑↓] 2p: [↑ ↑ ↑ ] [↓ ↓ ↓ ] 3s: [↑↓] 3p: [↑ ↑ ↑ ] [↓ ↓ (empty)] ``` In conclusion, the electron configuration for oxygen is 1s^2 2s^2 2p^4, and its orbital notation is as shown above. The electron configuration for sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4, and its orbital notation is also shown above.

Key Concepts

Oxygen Atom

The oxygen atom is a fundamental element in chemistry with an atomic number of 8. This means it has 8 electrons when it's neutral. Understanding the electron configuration of oxygen helps in predicting how it interacts with other elements.

To describe its electrons, we use the order of filling these electrons into different shells and orbitals. The electronic configuration is written as \(1s^2 2s^2 2p^4\). This tells us that:

• The first two electrons fill the lowest energy 1s orbital.
• Next, two electrons fill the 2s orbital.
• The remaining four electrons are placed in the 2p orbital, which can hold up to six electrons in total.

Grasping this configuration gives insight into oxygen's chemical behavior, such as its tendency to form double bonds as it seeks to fill its p-orbital by sharing electrons.

Sulfur Atom

Sulfur, with an atomic number of 16, has a more complex electron configuration compared to oxygen. It holds 16 electrons when in a neutral state. Getting familiar with these configurations helps understand sulfur's interactions and chemical properties.

For sulfur, the electron configuration is written as \(1s^2 2s^2 2p^6 3s^2 3p^4\). Here's a breakdown:

• The first two electrons enter the 1s orbital.
• Next, the 2s orbital accommodates two electrons.
• Then, the 2p orbital is fully filled with six electrons.
• After the second energy level is filled, electrons fill the 3s orbital next with two electrons.
• The remaining four go into the 3p orbital.

Sulfur’s electron configuration explains its common oxidation states and its ability to form sulfide compounds by completing its p orbital.

Orbital Notation

Orbital notation provides a more detailed view of an atom’s electron arrangement. By using boxes and arrows, it visually represents where each electron resides within orbitals of a given energy level.

In orbital notation, each orbital is represented by a box:

• An arrow inside the box denotes an electron. The direction of the arrow (up or down) indicates the electron's spin, governed by the Pauli Exclusion Principle.
• Electrons fill available orbitals according to Hund's Rule: electrons must occupy every orbital in a sublevel singly before any orbital is doubly occupied.

This means that when filling the p-orbitals, each orbital gets one electron (all arrows pointing in the same direction) before any pairing begins. Understanding orbital notation is crucial for visualizing electron arrangements and their spin properties.

Aufbau Principle

The Aufbau Principle is key to predicting an atom's electronic structure. It states that electrons occupy orbitals of lower energy first before filling higher energy orbitals. This principle aids in understanding the systematic arrangement of electrons.

The order of filling typically starts from the lowest energy level moving to higher ones as follows:

• 1s, 2s, and then 2p
• 3s, 3p, 4s, and so forth

This order is sometimes visualized using the diagonal rule or through an energy-level diagram. Applying the Aufbau principle alongside Hund’s Rule and the Pauli Exclusion Principle effectively predicts electronic structures across the periodic table.