Complete the exercises below. Write the chemical formula for each of the following compounds, and indicate the oxidation state of the halogen or noble-gas atom in each: a. chlorate ion, b. hydroiodic acid, c. iodine trichloride, d. sodium hypochlorite, e. perchloric acid, f. xenon tetrafluoride.

Verified step by step guidance

Step 1: Identify the chemical formula for each compound. For example, the chlorate ion is ClO₃⁻.

Step 2: Determine the oxidation state of the halogen or noble-gas atom in each compound. For the chlorate ion, assign oxidation states to oxygen (-2 each) and solve for chlorine.

Step 3: Repeat the process for hydroiodic acid (HI), where iodine is the halogen. Assign hydrogen a +1 oxidation state and solve for iodine.

Step 4: For iodine trichloride (ICl₃), assign oxidation states to chlorine (-1 each) and solve for iodine.

Step 5: Continue this method for sodium hypochlorite (NaClO), perchloric acid (HClO₄), and xenon tetrafluoride (XeF₄), assigning known oxidation states to other elements and solving for the halogen or noble-gas atom.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Formulas

A chemical formula represents the composition of a compound, indicating the types and numbers of atoms present. For ionic compounds, the formula reflects the ratio of ions, while for covalent compounds, it shows the actual number of atoms. Understanding how to derive and write these formulas is essential for identifying compounds and their properties.

Oxidation States

The oxidation state (or oxidation number) of an atom in a compound indicates the degree of oxidation or reduction it has undergone. It helps in understanding electron transfer during chemical reactions. Assigning oxidation states involves rules, such as the oxidation state of elements in their elemental form being zero and the sum of oxidation states in a neutral compound being zero.

Halogens and Noble Gases

Halogens are a group of elements in Group 17 of the periodic table, known for their high reactivity and tendency to gain electrons, often resulting in negative oxidation states. Noble gases, found in Group 18, are generally inert and have a stable electron configuration, typically exhibiting a zero oxidation state. Understanding the behavior of these elements is crucial for predicting their chemical properties and reactions.