Properties of Metallic, Ionic, and Covalent Substances

The different types of chemical bonding result in distinct properties for metallic, ionic, and covalent substances.

Metallic substances exhibit several characteristic properties due to their unique bonding structure:

• High melting and boiling points, attributed to the strong metallic bonds in their giant structures.
• Malleability and ductility, as the atoms are arranged in layers that can slide over each other.
• Excellent conductivity of electricity and thermal energy, due to the presence of free electrons.

Highlight: Alloys, which are mixtures of two or more elements with at least one being a metal, are harder than pure metals because the layers are distorted and cannot slide easily over each other.

Ionic substances also have distinctive properties:

• High melting and boiling points, due to the strong electrostatic forces between oppositely charged ions in all directions within the giant ionic lattice.
• Conductivity of electricity only when melted or dissolved in water, as the ions become free to move and carry charge.

Example: An ionic compound must be molten (at high temperatures) or dissolved in water to conduct electricity, as this allows the ions to move freely.

Covalent substances can be categorized into small molecules and giant structures, each with unique properties:

Small molecules:

• Relatively low melting and boiling points, as only weak intermolecular forces need to be overcome.
• Increasing melting and boiling points with molecule size, due to stronger intermolecular forces.
• Non-conductive of electricity, as the molecules have no overall electric charge.

Giant structures:

• High melting and boiling points, due to strong covalent bonds between all atoms.
• Varied conductivity and hardness, depending on the specific structure.

Example: Diamond is very hard and has a high melting point due to strong covalent bonds between carbon atoms, while graphite conducts electricity due to free electrons between its layers.

Highlight: Graphene, a single layer of graphite, and fullerenes like carbon nanotubes exhibit exceptional strength and conductivity due to their unique structures and free electrons.

Understanding these properties and the limitations of covalent bonding models is crucial for predicting and explaining the behavior of different materials in various applications.

Metallic Bonding and Ionic Bonding

Metallic bonding and ionic bonding are two distinct types of chemical bonding that play crucial roles in determining the properties of metals and ionic compounds.

In metallic bonding, metals lose electrons to form positive ions arranged in a giant, regular structure. The resulting delocalized electrons are free to move, contributing to the unique properties of metals.

Highlight: Metallic bonding involves strong bonds formed by sharing delocalized electrons.

Ionic bonding, on the other hand, occurs between metals and non-metals. In this process, metals lose electrons to form positive ions, while non-metals gain electrons to form negative ions.

Definition: An ionic bond is a strong electrostatic force of attraction between oppositely charged ions.

The charges on ions can be quickly determined based on the number of electrons in the outer shell of the atom. For example, Group 1 elements form +1 ions, while Group 7 elements form -1 ions.

Example: Sodium (Na) loses one electron to form Na+, while chlorine (Cl) gains one electron to form Cl-.

Covalent bonding, which occurs between non-metals, involves the sharing of electron pairs. This can result in small molecules or giant structures, depending on the atoms involved.

Vocabulary: A covalent bond is a strong bond formed when two non-metals share pairs of electrons.

Various models are used to represent covalent bonding, including ball and stick models, dot and cross diagrams, and displayed formulas. However, these models have limitations in accurately representing the true nature of chemical bonds.

Highlight: Models of covalent bonding have limitations, such as not showing the true shape of molecules or the identical nature of electrons.