Bonding, Structure and Properties of Matter

• Formation of ions
• Electrostatic forces between oppositely charged ions
• Ionic bonding is the strongest type of intermolecular force.
• The strength of ionic bonds depends on the size of the positive and negative charges involved.
• The strength of ionic bonds depends on the size of the positive and negative ions involved.
• Metals are good conductors because they have delocalized electrons that can move freely through the lattice structure.
• Metals are good conductors of electricity because they have delocalized electrons that can move freely through the lattice structure.
• Non-metals do not conduct electricity as their atoms are held together by covalent bonds.
• Covalent compounds can be polar or nonpolar depending on whether there is an uneven distribution of charge within the molecule.
• Non-metals do not form giant covalent structures due to their small atomic radii and high electronegativity differences.
• Covalent compounds are formed when two non-metal elements share one or more pairs of electrons to form molecules with strong covalent bonds.
• Ionic bonding is the electrostatic attraction between oppositely charged ions.
• The formation of ionic compounds involves the transfer of electrons from metal atoms to non-metal atoms.
• Ions are arranged in a regular pattern called a crystal lattice.
• In ionic compounds, metals lose electrons to become positive ions (cations) while non-metals gain electrons to become negative ions (anions).
• Metallic bonding occurs when positively charged metal ions are surrounded by delocalized sea of electrons.
• In metallic bonding, the positive charges attract the negative charges, resulting in strong forces of attraction that hold the lattice structure together.
• Metallic bonding occurs when positively charged metal ions attract delocalized electrons, resulting in metallic properties such as good conductivity and malleability.
• In metallic bonding, the positive ions attract the negatively charged electron cloud, resulting in strong forces of attraction that hold the structure together.
• Metals have high melting points due to the strength of metallic bonds.
• Hydrogen bonding is a type of intermolecular force where hydrogen atoms in certain molecules interact weakly with other nearby molecules containing highly electronegative atoms such as nitrogen, oxygen, or fluorine.
• Metallic solids have high melting points because they require a lot of energy to break the strong metallic bonds.
• Metals conduct electricity because they contain free electrons that can move through the structure.
• Covalent bonds form when two atoms share one or more pairs of valence electrons.
• Giant covalent lattices have very high melting and boiling points because they require breaking many strong covalent bonds.
• Molecular substances consist of molecules held together by covalent bonds.
• The strength of intermolecular forces depends on factors like polarity, shape, size, and charge distribution.
• Covalent bonds form between two non-metal atoms sharing one or more pairs of electrons.
• Metals are malleable and ductile as their layers slide over each other easily.
• Molecules formed through covalent bonding have low melting points due to weak intermolecular forces of attraction.
• Polymers are long chains made up of many repeating units joined by covalent bonds.
• The arrangement of atoms in solids can be regular or irregular.