Question

The clements of IVA group have 4 clectrons in their outermost orbit. They (1) form \(\mathrm{M}^{4+}\) ions (2) form \(\mathrm{M}^{4+}\) and \(\mathrm{M}^{4}\) ions. (3) exhibit oxidation states of \(+4\) and \(+2\). (4) exhibit oxidation states of \(+4\).

Short answer

Option (3): Exhibit oxidation states of +4 and +2.

Step-by-step solution

Identify Key Information

The elements of group IVA have 4 electrons in their outermost orbit.

Understand Ion Formation

These elements can form different ions such as \( \text{M}^{4+} \) and undergo various oxidation states.

Determine Oxidation States

The commonly exhibited oxidation states for group IVA elements are \( +4 \) and \( +2 \).

Match with Given Options

Compare the information with the provided options: 1. Form \( \text{M}^{4+} \) ions. 2. Form \( \text{M}^{4+} \) and \( \text{M}^{4} \) ions. 3. Exhibit oxidation states of \( +4 \) and \( +2 \). 4. Exhibit oxidation states of \( +4 \). The correct statement is option (3): 'Exhibit oxidation states of \( +4 \) and \( +2 \).' as it accurately describes the oxidation behaviors of group IVA elements.

Key concepts

outermost electrons

Group IVA elements, also known as Group 14 of the periodic table, have 4 electrons in their outermost electron shell. This group includes elements like carbon (C), silicon (Si), germanium (Ge), tin (Sn), and lead (Pb). These four electrons play a crucial role in determining the chemical behavior and bonding properties of these elements.
Because these electrons are in the outermost shell, they are the most accessible for chemical reactions. For example, in carbon, the 4 outermost electrons can form up to four covalent bonds, which allows it to create a vast array of compounds.
This characteristic makes Group IVA elements versatile in forming different kinds of chemical bonds, which is essential for understanding their reactivity and applications.

ion formation

Ion formation for Group IVA elements involves either losing or gaining electrons to achieve a more stable electron configuration.
More commonly, these elements tend to share electrons through covalent bonding rather than forming ions. However, they can form cations like \(\text{M}^{4+}\) (where M represents the element) by losing all four outermost electrons. This is less common due to the high energy required to remove four electrons.
In the context of simpler compounds, they might not fully ionize, but rather, they share electrons to form complex structures. For example, silicon forms a vast number of silicates by sharing its four outer electrons with oxygen atoms.

oxidation states

The oxidation states of Group IVA elements typically include +4 and +2. These states describe the number of electrons an atom gains, loses, or shares in forming chemical bonds.
When Group IVA elements exhibit a +4 oxidation state, they share all four of their outermost electrons in bonding. For example, carbon in methane \(\text{CH}_4\) has an oxidation state of +4 because it shares its four outermost electrons.
In some cases, these elements can also exhibit a +2 oxidation state, particularly in heavier elements like lead (Pb). In lead (II) chloride (PbCl_2), lead exhibits a +2 oxidation state, indicating it has lost two electrons.

group IVA elements

Group IVA elements are diverse and play significant roles in various fields. Each element has distinct properties, but they share the common feature of having four electrons in the outermost shell.
- **Carbon (C):** An essential element for life, forming the backbone of organic molecules.
- **Silicon (Si):** Widely used in electronics as a key component of semiconductors.
- **Germanium (Ge):** Also used in electronics and fiber optics.
- **Tin (Sn):** Used in alloys and coatings to prevent corrosion.
- **Lead (Pb):** Historically used in pipes and paints, now limited due to its toxicity.
The study of these elements and their properties is crucial for advancements in technology, chemistry, and materials science.