Question

Predict the charges for monoatomic ions of these elements. (a) Gallium (b) Fluorine (c) Silver (d) Nitrogen

Short answer

(a) Ga³⁺; (b) F⁻; (c) Ag⁺; (d) N³⁻.

Step-by-step solution

Understanding Ion Formation

To predict the charges for monoatomic ions of elements, we need to understand how these ions are formed. Typically, elements form ions to achieve a stable electron configuration, often imitating the nearest noble gas in the periodic table.

Gallium: Losing Electrons

Gallium is located in Group 13 of the periodic table. Elements in this group typically lose three electrons to achieve the electron configuration of a noble gas. Thus, gallium forms a Ga³⁺ ion.

Fluorine: Gaining Electrons

Fluorine is in Group 17, known as the halogens. Elements in this family tend to gain one electron to form ions, achieving a noble gas configuration. Therefore, fluorine forms an F⁻ ion.

Silver: Transition Metals Behavior

Silver, found in the transition metals, most commonly forms a +1 oxidation state. This is due to the stability provided by the d10 electron configuration it achieves when it loses one electron. Thus, silver forms an Ag⁺ ion.

Nitrogen: Gaining Electrons for Stability

Nitrogen is in Group 15 and needs to gain three electrons to achieve the stable electron configuration of a noble gas. As a result, nitrogen forms an N³⁻ ion.

Key concepts

Ion Formation

Ion formation is a critical concept in chemistry where atoms gain or lose electrons to form ions. This process occurs so that elements can achieve a stable electron configuration, similar to the closest noble gas in the periodic table.

• Atoms with fewer than four electrons in their outer shell tend to lose electrons to achieve stability, forming positively charged ions called cations.
• Conversely, atoms with more than four electrons often gain electrons to fill their outer shell, forming negatively charged ions known as anions.

Ion formation is driven by the desire of atoms to be energetically stable by having a full outer electron shell. This is often achieved by achieving the electron configuration of a nearby noble gas, leading to predictable ion charges based on the element's position in the periodic table.

Electron Configuration

Electron configuration describes how electrons are distributed in an atom's orbitals. The way electrons fill these orbitals dictates the chemical properties and reactivity of elements.

• The configuration is guided by the Aufbau principle, which states that electrons fill orbitals starting from the lowest energy level and moving to higher levels.
• Electrons fill orbitals in a specific order: starting with the 1s orbital, followed by 2s, 2p, 3s, and so forth.

A complete outer shell achieves stability, often found in noble gases. For example, when elements form ions, they may lose or gain electrons to reach a stable electron configuration of a noble gas. Understanding electron configuration helps to predict the charge of an ion based on how many electrons must be lost or gained to achieve stability.

Periodic Table Groups

The periodic table is organized into groups (columns) and periods (rows), which help identify the properties and behaviors of different elements. Groups, in particular, are important for predicting ion charge and understanding element behavior during ion formation.

• Elements in the same group have the same number of electrons in their outer shell, leading to similar chemical properties.
• For instance, Group 1 elements tend to form +1 ions as they lose one electron to reach a stable configuration.
• Group 17 elements, like fluorine, tend to gain one electron forming -1 ions, aiming to fill their outer shell.

Each group has a characteristic electron configuration that influences how they react to form ions, which is why elements in a particular group often display similar behaviors.

Transition Metals

Transition metals, found in the center of the periodic table, exhibit unique electron configuring behavior due to their d subshells. This flexibility allows transition metals to adopt multiple oxidation states.

• Unlike main-group elements, transition metals can often lose different numbers of electrons without disrupting their electron shells.
• Silver, for instance, typically forms a +1 ion as it achieves a stable d10 electron configuration.
• This variable oxidation state gives transition metals a wide variety of uses in different chemical reactions and processes.

Transition metals' ability to form complex ion charges stems from the partially filled d orbitals. Understanding their variable oxidation states is crucial in predicting how they participate in chemical reactions.