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Intermolecular Forces and Physical Properties

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Exploring the melting and boiling points of carbon and oxygen reveals how molecular structures and intermolecular forces dictate these physical properties. Carbon, with its network of covalent bonds, has a high sublimation point, while oxygen's diatomic molecules, held by weaker van der Waals forces, melt and boil at much lower temperatures. The text delves into the impact of intramolecular and intermolecular forces, bond polarity, and the resulting physical behaviors of various substances.

Comparative Analysis of Carbon and Oxygen's Melting and Boiling Points

Carbon and oxygen, elements with comparable atomic masses, exhibit starkly different melting and boiling points due to their distinct molecular structures. Carbon, particularly in its diamond form, is a network covalent solid with a robust three-dimensional lattice of covalent bonds, making it extremely difficult to melt; it sublimes directly into gas at about 3700°C under atmospheric pressure. Graphite, another form of carbon, also has a high melting point due to its strong covalent bonds within layers, although the forces between layers are weaker. Oxygen, in contrast, is a diatomic molecule (O2) with a relatively low melting point of -218.8°C, as it is held together by weaker intermolecular forces known as van der Waals forces.
Transparent glass beaker with water and ice cubes on reflective surface, surrounded by molecular models of O2 and CO2.

Intramolecular and Intermolecular Forces: A Contrast

Intramolecular forces are the strong bonds that hold atoms together within a molecule, including ionic, covalent, and metallic bonds. These forces are responsible for the chemical stability of compounds. Intermolecular forces, on the other hand, are the weaker forces that occur between molecules, such as London dispersion forces (a type of van der Waals force), dipole-dipole interactions, and hydrogen bonds. The melting and boiling points of substances are greatly influenced by these forces; materials with strong intramolecular bonds, like carbon in its diamond form, require substantial energy to change phases, whereas those with weaker intermolecular forces, like diatomic oxygen, require much less.

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00

______ in its diamond form sublimes at approximately ______°C, bypassing the liquid phase under normal atmospheric conditions.

Carbon

3700

01

Types of intramolecular forces

Ionic, covalent, metallic bonds.

02

Examples of intermolecular forces

London dispersion, dipole-dipole, hydrogen bonds.

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