Solids can be classified into two types: crystalline and amorphous. Crystalline solids are the most common type of solid. They are characterized by a regular crystalline organization of atoms that confer a long-range order. Amorphous, or non-crystalline, solids lack this long-range order.

Explanation:

• A solid has a definite shape and volume.
• Solids in general have higher density.
• In solids, intermolecular forces are strong.
• Diffusion of a solid into another solid is extremely slow.
• Solids have high melting points.

Solids have many different properties, including conductivity, malleability, density, hardness, and optical transmission, to name a few.

Covalent bonds are very strong, so covalent network solids typically have the highest melting points out of all four types of solids. They usually don’t conduct electricity because valence electrons are localized within covalent bonds.

There are four types of crystalline solids: ionic solids, molecular solids, network covalent solids and metallic solids.

hydrogen bonding

ionic interactions

The dipole-dipole attractions between CO molecules are comparably stronger than the dispersion forces between nonpolar N2 molecules, so CO is expected to have the higher boiling point.

The only intermolecular forces in methane are London dispersion forces. The major intermolecular forces would be dipole-dipole forces and London dispersion forces. The electronegativities of C and H are so close that C-H bonds are nonpolar. There are no bond dipoles and no dipole-dipole interactions.

The London Dispersion Forces in I2 are strong enough to keep I2 solid at room temperature; where as, F2 is a gas at room temperature. In general London Dispersion Forces are considered to be the weakest intermolecular force; however, London Dispersion Forces become very important for larger molecules.

Dipole-dipole interactions are the strongest intermolecular force of attraction.

The van der Waals forces are stronger in hexane than in pentane because hexane has a larger surface area to interact with neighboring molecules. The stronger intermolecular attraction holds molecules together more tightly, decreasing the vapor pressure of hexane and giving it a higher boiling point than pentane.

Terms in this set (6)

• Ionic Bonds. – is the strongest bonds – when one atom takes the electrons of another atoms.
• Covalent Bonds. when there is a charging of the electrons between two atoms.
• Van der Waals.
• London Dispersion Force.
• Dipole-Dipole interactions.
• Hydrogen Bonding.

Ionic bonds are stronger than covalent bonds, but when dissolved in water, they become much weaker because ions separate and are surrounded by water molecules.

Question: When Two Atoms Are Equally Electronegative, They Will Interact To Form Ionic Bonds Equal Numbers Of Isotopes. Nonpolar Covalent Bonds. Polar Covalent Bonds. Oions Atoms W, X, Y & Z Have Atomic Numbers Of 9, 10, 11 & 12 Respectively.