Question

Which of the following statement is correct for \(\mathrm{CsBr}_{3} ?\) (a) It is a covalent compound (b) It contains \(\mathrm{Cs}^{3+}\) and \(\mathrm{Br}^{-}\) ions (c) It contains \(\mathrm{Cs}^{+}\) and \(\mathrm{Br}_{3}^{-}\) ions (d) It contains \(\mathrm{Cs}^{+}, \mathrm{Br}^{-}\) and lattice \(\mathrm{Br}_{2}\) molecule

Short answer

Option C is correct: \( \mathrm{CsBr}_3 \) contains \( \mathrm{Cs}^{+} \) and \( \mathrm{Br}_3^{-} \) ions.

Step-by-step solution

Understand the Formula

The compound given is \( \mathrm{CsBr}_3 \). Understanding the compound formula is crucial. \( \mathrm{Cs} \) represents Cesium and \( \mathrm{Br} \) represents Bromine. \( \mathrm{CsBr}_3 \) suggests a compound formed with Cesium and three Bromine atoms.

Analyze the Options

Examine each option:- **Option A:** Suggests covalent nature. Cesium is an alkali metal and typically forms ionic compounds.- **Option B:** Suggests \( \mathrm{Cs}^{3+} \). Typically, \( \mathrm{Cs} \) forms \( \mathrm{Cs}^+ \) ions, not \( \mathrm{Cs}^{3+} \).- **Option C:** Suggests \( \mathrm{Cs}^{+} \) and \( \mathrm{Br}_3^{-} \) ions. This matches the number of atoms in \( \mathrm{CsBr}_3 \) and the usual oxidation states.- **Option D:** Implies the existence of \( \mathrm{Br}_2 \), which doesn't correspond to the formula provided.

Determine the Correct Option

Given the typical ionic character of cesium compounds and the formula \( \mathrm{CsBr}_3 \), the compound likely involves cesium ions \( \mathrm{Cs}^{+} \) and a complex anion \( \mathrm{Br}_3^{-} \). Therefore, Option C accurately describes the compound.

Key concepts

Cesium Chemistry

Cesium is an alkali metal found in Group 1 of the periodic table. Known for its distinct properties, cesium is the most electropositive and alkaline element. This means that it has a very strong tendency to donate its one valence electron to achieve a stable electronic configuration. As a result, cesium typically forms the ion \( \text{Cs}^+ \).
Chemically, cesium is highly reactive. It reacts explosively with water to form cesium hydroxide and hydrogen gas. Because of its reactivity, cesium is often stored in non-reactive environments.
- **Highly reactive alkali metal**: Part of the Group 1 elements- **Forms \( \text{Cs}^+ \) ions**: Loses one electron to form stable ionic compounds- **Uses**: Cesium's properties make it valuable in applications like atomic clocks and in oil drilling fluids due to its ability to form dense solutions.

Oxidation States

Oxidation state refers to the degree of oxidation of an atom, essentially indicating how many electrons are gained, lost, or shared. For cesium, the oxidation state is typically \( +1 \) because it tends to lose its single outer electron easily to achieve a noble gas configuration. This results in the ion \( \text{Cs}^+ \).
In the context of \( \text{CsBr}_3 \), understanding oxidation states helps determine the correct formulation of ions. Bromine can have various oxidation states, but within the context of \( \text{Br}_3^- \), it behaves as a polyatomic ion where the combined oxidation states balance the positive charge of \( \text{Cs}^+ \).
- **Cesium's common oxidation state**: +1 due to loss of its outer electron- **Interpretation of \( \text{CsBr}_3 \)**: Balancing positive cesium with negative bromine ions

Chemical Formula Analysis

Analyzing chemical formulas involves determining the types of ions present and how they are arranged. The formula \( \text{CsBr}_3 \) indicates a compound composed of cesium and bromine.
Understanding the formula also helps in determining the charge balance within the compound. Here, one cesium ion typically carries a \( +1 \) charge, and the compound suggests the presence of a polyatomic bromine ion that could balance this charge as \( \text{Br}_3^- \).
- **\( \text{Cs}^+ \) and \( \text{Br}_3^- \)**: Represents a stable ionic compound- **Formulation insights**: The analysis leads to the correct balance of charges and understanding of the ions involved in \( \text{CsBr}_3 \)