Question

Interpret Data Could the following reaction occur? Explain your answer. $$3 \mathrm{Ni}+2 \mathrm{AuBr}_{3} \rightarrow 3 \mathrm{NiBr}_{2}+2 \mathrm{Au}$$

Short answer

The given reaction \(3 \mathrm{Ni}+2 \mathrm{AuBr}_{3} \rightarrow 3 \mathrm{NiBr}_{2}+2 \mathrm{Au}\) can occur as it follows the conservation of mass and adheres to the octet rule for all the elements involved. The number of atoms for each element is conserved, and the elements lose or gain electrons accordingly to achieve a stable electron configuration.

Step-by-step solution

Identify Elements and Compare the Number of Atoms on Both Sides of the Equation

First, we'll identify all the elements present in the given reaction and count the number of atoms for each element on both sides of the reaction: Left Side (Reactants) Ni: 3 atoms Au: 2 atoms Br: 6 atoms (2 * 3) Right Side (Products) Ni: 3 atoms Au: 2 atoms Br: 6 atoms (3 * 2) Now, let's compare the number of atoms for each element on both sides of the equation: Ni: 3 atoms (left side) = 3 atoms (right side) Au: 2 atoms (left side) = 2 atoms (right side) Br: 6 atoms (left side) = 6 atoms (right side)

Verify the Octet Rule for Each Element

We'll now verify the octet rule for each element in the reaction. Ni: Nickel has an electron configuration of [Ar] 3d^8 4s^2, and it can lose two electrons to form a stable +2 ion. This is because it will then have a filled 3d^10 configuration, which is a stable electron configuration. Au: Gold has an electron configuration of [Xe] 4f^14 5d^10 6s^1, and it can lose one electron or gain one electron to achieve a stable electron configuration with eight electrons in their outermost energy level. Br: Bromine has an electron configuration of [Ar] 3d^10 4s^2 4p^5, and it can gain one electron to form a stable -1 ion. This is because it will then have a filled 4p^6 configuration, which is a stable electron configuration.

Examine the Reaction for Conservation of Mass and Octet Rule Compliance

Now we will examine the reaction in terms of the conservation of mass and the octet rule: 3 Ni + 2 AuBr3 -> 3 NiBr2 + 2 Au - The number of atoms for each element is conserved. - Ni loses 2 electrons to form Ni^2+ ions, thus following the octet rule. - Br gains 1 electron to form Br^- ions, thus following the octet rule. - Au loses 1 electron when reacting with the Br ions, thus following the octet rule.

Conclusion

Based on the analysis above, we can conclude that the given reaction can indeed occur as it follows the conservation of mass and adheres to the octet rule for all the elements involved.

Key concepts

Conservation of Mass

The principle of conservation of mass is a fundamental concept in chemistry. During a chemical reaction, mass is neither created nor destroyed, meaning the mass of the reactants (substances you start with) must equal the mass of the products (substances you end with). This is why, in balancing chemical equations, it's crucial to ensure that the number of atoms for each element is the same on both sides of the equation.

In our example reaction, \(3 \mathrm{Ni} + 2 \mathrm{AuBr}_{3} \rightarrow 3 \mathrm{NiBr}_{2} + 2 \mathrm{Au}\), we verified that the number of atoms for each element is equal before and after the reaction occurs:

• Ni: 3 atoms on the left, 3 atoms on the right
• Au: 2 atoms on the left, 2 atoms on the right
• Br: 6 atoms on the left, 6 atoms on the right

This conservation proves the reaction can occur, as it follows this fundamental law of chemistry.

Octet Rule

The octet rule is a chemical principle that suggests atoms tend to bond in a way that each atom has eight electrons in its valence shell, resembling the electron configuration of a noble gas. This rule helps us understand how atoms will bond and is inherently related to an atom's electron configuration.

In our reaction:

• Nickel (Ni) has the electron configuration \([\text{Ar}] 3d^8 4s^2\). By losing two electrons, it achieves a stable \( 3d^{10} \) electron configuration, consistent with the octet rule.
• Gold (Au) with the electron configuration \([\text{Xe}] 4f^{14} 5d^{10} 6s^1\) can achieve stability by losing an electron.
• Bromine (Br) with \([\text{Ar}] 3d^{10} 4s^2 4p^5\), gains an electron, filling its \(4p\) orbital to satisfy the octet rule.

Each element in the reaction aligns its electron interaction according to the octet rule, ensuring that the reaction is feasible from a chemical bonding perspective.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It explains why atoms form certain types of ions to become electronically stable, often trying to resemble the electron configuration of noble gases.

Consider the elements involved in the given reaction:

• Nickel's electron configuration is \([\text{Ar}] 3d^8 4s^2\). By losing electrons from the \(4s\) orbital, it forms \(\text{Ni}^{2+}\), which is more stable due to the filled \(3d^{10}\).
• Gold's configuration is \([\text{Xe}] 4f^{14} 5d^{10} 6s^1\). It can lose its lone \(6s\) electron to reach a stable state.
• Bromine has \([\text{Ar}] 3d^{10} 4s^2 4p^5\). Adding one electron completes the \(4p\) orbital, leading to a more energetically favorable \(4p^6\) configuration.

Understanding these configurations is key to predicting how elements interact and form compounds, as seen in our balanced reaction.

Balancing Equations

Balancing chemical equations ensures that the principle of conservation of mass is met. It means adjusting the coefficients of reactants and products to have the same number of each type of atom on both sides of the equation.

In the reaction \(3 \mathrm{Ni} + 2 \mathrm{AuBr}_{3} \rightarrow 3 \mathrm{NiBr}_{2} + 2 \mathrm{Au}\), the coefficients applied to each compound reflect the need to keep the reaction balanced:

• 3 Ni atoms pair with the 2 AuBr₃ molecules on the left to generate 3 NiBr₂ and 2 Au atoms on the right.
• This ensures the conservation of each element's atom count across the reaction—critical for accurately depicting chemical change.

Balancing equations might seem challenging, but it's essential practice for mastering chemical reactions and preventing errors in representing reactions.