Question

What types of atoms tend to form the following types of bonding? a. ionic b. covalent c. metallic

Short answer

a. Metals and non-metals, b. Non-metals, c. Metals

Step-by-step solution

Identify Atoms that Form Ionic Bonds

Ionic bonds typically form between atoms with a large difference in electronegativity. This usually involves a metal and a non-metal. Metals tend to lose electrons to form positive ions (cations), while non-metals tend to gain electrons to form negative ions (anions).

Identify Atoms that Form Covalent Bonds

Covalent bonds generally form between non-metal atoms that have similar electronegativity values. These atoms share pairs of electrons to attain a stable electron configuration.

Identify Atoms that Form Metallic Bonds

Metallic bonds occur between metal atoms. These atoms release some of their electrons to form a 'sea of electrons' that are free to move throughout the structure. This delocalized electron cloud allows metals to conduct electricity and heat, as well as to be malleable and ductile.

Key concepts

Ionic Bonds

Ionic bonds form due to the electrostatic attraction between positive and negative ions.

These bonds typically occur between:

• Metals: Elements that tend to lose electrons and form positive ions, known as cations.
• Non-metals: Elements that tend to gain electrons and form negative ions, known as anions.

The difference in electronegativity between the two atoms needs to be large enough to result in electron transfer from the metal to the non-metal.

After the electron transfer, the metal becomes a positively charged ion, while the non-metal becomes a negatively charged ion. These opposite charges attract each other, forming a strong bond. Examples of compounds with ionic bonds include sodium chloride (NaCl) and magnesium oxide (MgO).

Covalent Bonds

Covalent bonds involve the sharing of electrons between atoms. These bonds form mainly between non-metal atoms with similar electronegativity values.

Here’s how covalent bonding works:

• Non-metal atoms share pairs of valence electrons.
• This sharing allows each atom to attain a stable electron configuration, similar to that of noble gases.

There are various types of covalent bonds based on the number of shared electron pairs:

• Single bonds: Involve one pair of shared electrons (e.g., H₂).
• Double bonds: Involve two pairs of shared electrons (e.g., O₂).
• Triple bonds: Involve three pairs of shared electrons (e.g., N₂).

Examples of compounds with covalent bonds include water (H₂O) and carbon dioxide (CO₂).

Metallic Bonds

Metallic bonds occur between metal atoms. These bonds involve a unique sharing of free electrons among a lattice of metal cations.

The characteristics of metallic bonds include:

• Delocalized electrons: Metal atoms release some of their electrons to create a 'sea of electrons' that are free to move throughout the metallic structure.
• Formation of a lattice: Positively charged metal ions are arranged in a structured lattice immersed within the electron sea.

These properties give metals their distinctive characteristics:

• Electrical conductivity: The free electrons allow metals to conduct electricity efficiently.
• Thermal conductivity: The same free electrons also help in conducting heat.
• Malleability and ductility: Metals can be easily shaped and stretched without breaking due to the flexibility of the electron sea.

Examples of metallic bonding can be seen in pure metals such as aluminum (Al), gold (Au), and iron (Fe).