2.2 How bonding and structure are related to the properties of substances

• A chemical bond is the force that holds atoms together to form molecules
• The three main types of chemical bonding are ionic, covalent, and metallic
• Giant covalent structures have high melting points and hardness.


  True
• Metallic bonds involve the complete transfer of electrons from one atom to another.

  False
• What is the role of electrons in metallic bonding?

  Shared electron sea
• Explain why ionic compounds are brittle when distorted:

  1️⃣ Distortion of the lattice

  2️⃣ Like-charged ions come closer

  3️⃣ Repulsion between ions

  4️⃣ Breaking of the lattice
• Metallic bonding involves a shared sea of delocalized electrons among metal atoms.


  True
• Which type of covalent structure is non-conductive?

  Simple molecular structure
• The malleability and ductility of metals are due to the ability of atoms to slide past each other without breaking bonds
• The luster of metals is due to delocalized electrons reflecting light
• Ionic bonds involve the sharing of electrons between two nonmetal atoms.

  False
• The arrangement of ions in ionic compounds forms a giant ionic lattice
• Water (H₂O) and methane (CH₄) are examples of simple molecular structures.


  True
• The delocalized electrons in metals allow atoms to slide past each other, contributing to malleability and ductility.


  True
• What determines the properties of covalent compounds?

  Their structure
• Ionic compounds conduct electricity only when molten or in solution
• Simple molecular structures are generally non-conductive.


  True
• The structural differences between simple molecular and giant covalent structures directly impact their properties.


  True
• What property of metals allows them to reflect light and appear shiny?

  Luster
• Match the covalent structure with its property:

  Simple molecular ↔️ Low melting point

  Giant covalent ↔️ High hardness
• Water has a high boiling point of 100°C due to strong hydrogen bonding
• Metallic bonds consist of a sea of shared electrons
• Ionic compounds have low melting points due to strong electrostatic forces.

  False
• Malleability in metals is due to the ability of atoms to slide past each other without breaking bonds.


  True
• In ionic bonding, there is a complete transfer of electrons
• Match the type of chemical bond with its key feature:

  Ionic ↔️ Electron transfer

  Covalent ↔️ Electron sharing

  Metallic ↔️ Shared electron sea
• Ions in ionic compounds arrange themselves in a giant ionic lattice
• What type of covalent structure has weak intermolecular forces?

  Simple molecular structure
• The strong electrostatic forces in ionic compounds require a large amount of energy
• Delocalized electrons in metals enable electrical conduction
• A chemical bond is the force that holds atoms together to form molecules
• Water (H₂O) is an example of a covalent compound formed by electron sharing.


  True
• Covalent compounds are formed when two nonmetal atoms share electrons
• Graphene is an exception to the poor electrical conductivity of giant covalent structures.


  True
• The strong electrostatic forces in ionic compounds require significant energy to break, resulting in high melting and boiling points
• High melting and boiling points in ionic compounds are due to strong electrostatic forces in the giant ionic lattice
• What type of melting and boiling points do simple molecular structures have?

  Low
• What type of melting and boiling points do giant covalent structures have?

  High
• Delocalized electrons in metallic compounds allow for high electrical conductivity
• Metallic bonding involves the sharing of electrons in a "sea" rather than the complete transfer or sharing between specific atoms.


  True