Question

During the bond formation normally all the elements in their outermost shell acquire (1) 2 electrons (2) 4 electrons (3) 8 electrons (4) 10 electrons

Short answer

8 electrons.

Step-by-step solution

Understanding the Question

The question is about the number of electrons elements typically acquire in their outermost shell during bond formation to achieve a stable structure.

Introduce the Octet Rule

During bond formation, elements tend to follow the octet rule, aiming to have 8 electrons in their outermost shell. This creates a stable electron configuration similar to noble gases.

Evaluate the Options

Examine each option: (1) 2 electrons, (2) 4 electrons, (3) 8 electrons, (4) 10 electrons. Based on the octet rule, the correct answer is 8 electrons.

Conclusion

Conclude that the number of electrons elements generally acquire in their outermost shell during bond formation is 8.

Key concepts

bond formation

Bond formation is a fundamental process in chemistry where atoms join together to form molecules. This occurs because atoms seek stability, which they achieve by having a full outer electron shell. During bond formation:

• Atoms can either share, donate, or receive electrons.
• The type of bond (covalent, ionic, or metallic) depends on how the electrons are arranged between the atoms.
• For example, in covalent bonds, atoms share electrons to fill their outer shells. In ionic bonds, one atom donates electrons to another, leading to attraction between the resulting ions.

Ultimately, bond formation results in a stable electron configuration for the participating atoms, mirroring the electronic arrangements of noble gases.

stable electron configuration

A stable electron configuration is crucial for an atom's stability. Atoms are naturally inclined to achieve this state, which often means having eight electrons in their outer shell, known as the octet rule. Key points include:

• The octet rule states that atoms are most stable when they have eight electrons in their valence shell.
• There are some exceptions, such as hydrogen and helium, which are stable with just two electrons in their only shell.
• Atoms achieve this configuration by losing, gaining, or sharing electrons through bonds.

For instance, in a molecule of water (H₂O), the oxygen atom shares electrons with two hydrogen atoms, filling its outer shell and stabilizing the molecule.

noble gases

Noble gases are a group of elements found in Group 18 of the periodic table. These elements include helium, neon, argon, krypton, xenon, and radon. Noble gases are characterized by their extremely stable electron configurations:

• They have complete outer electron shells, with helium having two and the others having eight electrons.
• This stability makes noble gases highly unreactive under normal conditions.
• Because of their stable configurations, other elements in the periodic table often try to emulate noble gases during bond formation.

For instance, when a sodium atom loses one electron, it attains the same electron configuration as neon, which is a noble gas, thus becoming more stable.