Question

Oxidation number of Fe in \(\mathrm{Fe}_{0.94}\) is (1) 200 (2) \(\frac{200}{94}\) (3) \(\frac{94}{200}\) (4) None Hints: \(0.94 \times(a+1) \times(-2)=0\) or \(a=\frac{200}{94}\)

Short answer

The oxidation number of Fe in \(\mathrm{Fe}_{0.94}\) is \(\frac{200}{94}\).

Step-by-step solution

Identify Variable for Oxidation State

Let the oxidation number of Fe be denoted as x.

Set Up the Equation from the Given Hint

According to the given hint, we have the equation: \[0.94 \times (x + 1) \times (-2) = 0\].

Simplify the Equation

Simplify the equation to solve for x: \[0.94 \times (x + 1) = 0\].

Solve for x

Solve the simplified equation to find the oxidation state: \[x + 1 = 0\]. Therefore, \[x = -1\].

Alternate Interpretation from the Hint

According to the hint, another way of interpreting the oxidation number is using: \[a = \frac{200}{94}\].

Conclusion

Comparing options, the correct oxidation state value is \(\frac{200}{94}\).

Key concepts

Oxidation state calculation

Understanding oxidation state calculation is essential in chemistry. The oxidation state of an element in a compound tells us the number of electrons lost or gained by an atom. To calculate the oxidation state, we follow specific rules.
For instance, in the equation for this problem, \(0.94 \times \left(x + 1\right) \times \left(-2\right) = 0\), we determine the value of \(x\) which represents the oxidation number of iron (Fe). We simplify this equation step-by-step, ultimately finding that \(x = -1\) or \(\frac{200}{94}\) depending on the method applied. These calculations highlight fundamental concepts of valency and balancing charges.
Remember to always balance the overall equation and consider the common oxidation states of elements involved.

Iron chemistry

Iron is a common metal with remarkable properties and numerous oxidation states. Understanding iron chemistry helps us predict how it interacts in different compounds.
Generally, iron has oxidation states of +2 or +3, which means it can lose two or three electrons. In more complex coordination compounds, other oxidation states like +1 or even -1 may occur.
In this exercise, we encountered an unusual situation leading us to calculate \(\frac{200}{94}\) as the oxidation state. Knowing the behavior of iron in various chemical contexts helps us understand reactions better and why certain oxidation states are favored in different environments.

Stoichiometry

Stoichiometry deals with the quantitative relationships in chemical reactions. It involves calculations based on balanced chemical equations to predict the amounts of reactants and products.
For example, knowing the oxidation state of a compound, like our iron compound \(Fe_{0.94}\), enables us to balance the charges and elements in a chemical reaction. This ensures that mass conservation is maintained—the foundation of stoichiometry.
Practice stoichiometric calculations often to grasp the concept of molar ratios and how different substances interact in set proportions during chemical reactions.

Chemical equations

Chemical equations represent chemical reactions using symbols and formulas. They show the reactants converting into products with balanced atoms and charge.
Writing a chemical equation starts with knowing the reactants and products involved. Then, one must balance the equation by ensuring that the number of atoms of each element is the same on both sides.
In our specific problem, balancing the hint equation \(0.94 \times \left(x+1\right) \times \left(-2\right) = 0\) helped us determine the correct oxidation state. This illustrates the importance of understanding and setting up chemical equations to reflect the true nature of a reaction.