Chapter 4: Problem 45

Use the periodic table to describe the chemical properties of the following elements: $$\begin{array}{l}{\text { a. iodine, I }} \\ {\text { b. krypton, Kr }} \\\ {\text { c. rubidium, Rb }}\end{array}$$

Short Answer

Expert verified

Iodine, being a halogen, tends to gain an electron, is highly electronegative, and forms a negative ion. Krypton, a noble gas, has a full electron shell, is chemically unreactive with high ionization energy. Rubidium, an alkali metal, tends to lose its single valence electron, is highly reactive, and forms a positive ion.

Step by step solution

Iodine (I)

Iodine is in Group 17 (Halogen group) and Period 5 of the periodic table. It is a non-metal with seven valence electrons. It tends to gain an electron to achieve a stable configuration, thus forming a negative ion, I$^-$. Iodine typically forms one covalent bond, has a high electronegativity and a high ionization energy.

Krypton (Kr)

Krypton is located in group 18 (Noble gas group) and Period 4. As a noble gas, it has a complete electron shell with eight valence electrons. It is chemically unreactive due to its full valence shell and stable configuration. Krypton has a high ionization energy and a low electronegativity since it doesn't tend to accept or donate electrons.

Rubidium (Rb)

Rubidium is in Group 1 (Alkali Metal group) and Period 5. Being an alkali metal, it has a single valence electron. It tends to lose this electron easily to achieve a stable configuration, forming positive ions, Rb$^+$. Rubidium usually forms a single ionic bond, and it has a low electronegativity and low ionization energy.

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Use the periodic table to describe the chemical properties of the following elements: $$\begin{array}{l}{\text { a. iodine, I }} \\ {\text { b. krypton, Kr }} \\\ {\text { c. rubidium, Rb }}\end{array}$$

Short Answer

Step by step solution

Iodine (I)

Krypton (Kr)

Rubidium (Rb)

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