Question

All chemical bonds are the result of (1) interaction of nuclei (2) interaction of electrons (3) difference in electronegativity (4) interaction of electron and nuclei

Short answer

Chemical bonds are the result of the interaction of electrons.

Step-by-step solution

Understand the Nature of Chemical Bonds

Chemical bonds are formed when atoms interact to achieve a stable electron configuration.

Focus on Electron Involvement

The interaction of electrons primarily contributes to the formation of different types of bonds such as ionic, covalent, and metallic bonds.

Compare Different Interactions

Analyze other options: nuclei interactions and nuclei-electron interactions can influence bonds but they are not the primary cause. Electronegativity differences can drive bond formation (e.g., ionic bonds) but also relate back to electron behavior.

Select the Correct Answer

The primary cause of chemical bond formation is the interaction of electrons, making option (2) the correct choice.

Key concepts

Electron Interaction

Chemical bonds are primarily formed through the interaction of electrons. Electrons are subatomic particles that orbit the nucleus of an atom in various energy levels or shells. When atoms come close to each other, their electrons start interacting. This interaction can lead to the formation of different types of bonds, depending on the behavior and sharing of these electrons. For instance, in a covalent bond, atoms share electrons to achieve a stable electron configuration. Ionic bonds, however, form when one atom donates an electron to another, creating charged ions that attract each other. Metallic bonds, on the other hand, involve a 'sea' of free-moving electrons around metal ions.

Bond Formation

The concept of bond formation is deeply tied to the principle of achieving stability. Atoms aim to reach a stable electron configuration, often resembling the nearest noble gas. There are three primary types of bonds:

• Covalent Bonds: Atoms share electrons to fill their outer shells. This is common in molecules like water (H₂O).
• Ionic Bonds: One atom donates an electron to another, creating positively and negatively charged ions. These opposite charges attract, forming a bond. Table salt (NaCl) is a classic example.
• Metallic Bonds: In metals, atoms release some of their electrons, creating a pool of free-moving electrons. This electron sea facilitates properties like malleability and electrical conductivity.

The type of bond formed depends on the atoms' tendency to either share, donate, or pool electrons.

Electronegativity

Electronegativity is a measure of an atom's ability to attract shared electrons in a chemical bond. Different atoms have varying electronegativities, which can influence the type of bond formed. Here’s how:

• High Electronegativity Difference: When there is a significant difference in electronegativity between two atoms, an ionic bond is likely to form. The atom with higher electronegativity will attract electrons more strongly, resulting in one atom donating an electron to the other.
• Moderate Electronegativity Difference: If the difference is moderate, a polar covalent bond may form. In this case, electrons are shared unevenly, creating partial positive and negative charges.
• Low Electronegativity Difference: When two atoms have a low difference in electronegativity, they share electrons equally, resulting in a nonpolar covalent bond.

Understanding electronegativity helps to predict how atoms will interact and the type of bond they will form.