Question

For each of these nonmetals, write the chemical symbol for the corresponding monoatomic ion (with charge). (a) Nitrogen (b) Sulfur (c) Chlorine (d) Iodine

Short answer

(a) \( \text{N}^{3-} \), (b) \( \text{S}^{2-} \), (c) \( \text{Cl}^{-} \), (d) \( \text{I}^{-} \).

Step-by-step solution

Identify the Group in the Periodic Table

Determine the group number for each nonmetal atom. The group number helps determine the typical charge of the ions formed by these elements. - Nitrogen is in Group 15. - Sulfur is in Group 16. - Chlorine is in Group 17. - Iodine is in Group 17.

Determine the Typical Ionic Charge

Use the group number to find the charge of the monoatomic ion. - Elements in Group 15 typically form ions with a -3 charge. - Elements in Group 16 typically form ions with a -2 charge. - Elements in Group 17 typically form ions with a -1 charge.

Write the Ion Symbols with Charges

Combine the element symbol with its ionic charge to write the complete symbol for each ion.- (a) Nitrogen becomes the nitride ion, written as \( \text{N}^{3-} \).- (b) Sulfur becomes the sulfide ion, written as \( \text{S}^{2-} \).- (c) Chlorine becomes the chloride ion, written as \( \text{Cl}^{-} \).- (d) Iodine becomes the iodide ion, written as \( \text{I}^{-} \).

Key concepts

Nonmetals

Nonmetals are elements found on the right side of the periodic table. They are distinct from metals in several ways. Unlike metals, nonmetals are usually poor conductors of heat and electricity. They also appear in a variety of states at room temperature: some are gases (like oxygen), some are solids (like sulfur), and one is a liquid (bromine). Nonmetals are known for their high electronegativities, meaning they have a strong tendency to attract electrons.
Nonmetals commonly form anions when they gain electrons, as they tend to have higher electronegativities compared to their metallic counterparts. This is particularly evident in elements like nitrogen, sulfur, chlorine, and iodine, which are part of the exercise at hand. Understanding their position and properties is crucial to predicting their behavior in forming ions.

Ionic Charge

The ionic charge of an element refers to the electrical charge that an atom carries when it has gained or lost electrons to form an ion. For nonmetals, this charge is typically negative, as they tend to gain electrons. The magnitude of the ionic charge is largely determined by the group number in the periodic table.

• Elements in Group 15 typically form ions with a -3 charge, as they gain three electrons to achieve a stable noble gas electron configuration.
• Elements in Group 16 form ions with a -2 charge by gaining two electrons.
• Elements in Group 17 form ions with a -1 charge by gaining one electron to fill their valence shell.

This systematic determination of ionic charge helps in predicting the formulas of compounds and understanding the reactivity of the elements.

Periodic Table Groups

The periodic table is organized into groups and periods, with groups being the vertical columns. Elements in the same group have similar properties and often form ions with the same charge due to having the same number of valence electrons. This layout is useful for predicting the behavior of elements in chemical reactions.
For nonmetals, their group number (particularly groups 15 to 17) plays a pivotal role in determining their ionic charges when forming monoatomic ions:

• Group 15 nonmetals, such as nitrogen, form ions with a -3 charge.
• Group 16 nonmetals, like sulfur, typically have a -2 charge as ions.
• Group 17 nonmetals, including chlorine and iodine, carry a -1 charge in their ionic form.

This information is crucial for understanding chemical reactions and bonding patterns of the nonmetals.

Chemical Symbols

Chemical symbols are shorthand representations of elements. Each symbol consists of one or two letters, with the first letter always capitalized and, if there is a second letter, it is lowercase. These symbols are used to write chemical formulas and equations succinctly and are universal across languages.
In the exercise, we deal with monoatomic ions, where the chemical symbol is combined with the ionic charge to represent the ion.

• Nitrogen forms the ion symbolized as \( \text{N}^{3-} \), known as the nitride ion.
• Sulfur creates the sulfide ion, written as \( \text{S}^{2-} \).
• Chlorine becomes the chloride ion, represented as \( \text{Cl}^{-} \).
• Iodine converts into the iodide ion, shown as \( \text{I}^{-} \).

The ability to write and interpret these symbols is fundamental in chemistry, allowing for efficient communication of complex ideas.