(b) The anion IO₄^- has a tetrahedral structure: three oxygen atoms form double bonds with the central iodine atom and one oxygen atom which carries a negative charge forms a single bond. Predict the molecular geometry of IO₆^5-.

검증된 단계별 안내

Identify the central atom in the IO6^5- ion, which is iodine (I).

Determine the total number of valence electrons available. Iodine has 7 valence electrons, and each oxygen has 6 valence electrons. Since there are 6 oxygen atoms, calculate the total valence electrons from oxygen and iodine, and account for the 5- charge by adding 5 more electrons.

Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. Count the number of electron pairs around the central iodine atom, including both bonding pairs and lone pairs.

Assign the electron pairs to positions around the iodine atom to minimize repulsion, considering that the IO6^5- ion has 6 bonding pairs and no lone pairs on the central atom.

Based on the arrangement of electron pairs, determine the molecular geometry. For 6 bonding pairs and no lone pairs, the geometry is expected to be octahedral.

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Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the shape according to VSEPR (Valence Shell Electron Pair Repulsion) theory. Understanding molecular geometry is crucial for predicting the behavior and reactivity of molecules.

VSEPR Theory

VSEPR theory posits that electron pairs around a central atom will arrange themselves to minimize repulsion, leading to specific molecular shapes. This theory helps predict the geometry of molecules based on the number of bonding and non-bonding electron pairs. For example, a tetrahedral arrangement occurs when there are four regions of electron density around a central atom.

Oxidation States

Oxidation states indicate the degree of oxidation of an atom in a compound, reflecting the number of electrons lost or gained. In the case of IO<sub>6</sub><sup>5-</sup>, understanding the oxidation states of iodine and oxygen is essential for determining the overall charge and the bonding characteristics of the molecule. This knowledge aids in predicting the molecular structure and stability.

(b) The anion IO4- has a tetrahedral structure: three oxygen atoms form double bonds with the central iodine atom and one oxygen atom which carries a negative charge forms a single bond. Predict the molecular geometry of IO65-.