each type of substance to its structure and bonding

• Which types of atoms are involved in ionic bonding?

  Metal and non-metal atoms
• Why are the electrons unequally distributed in the second diagram?

  Because some electrons have a slightly positive charge, while others have a slightly negative charge
• What forms as a result of ionic bonding?

  Charged ions held by electrostatic attraction
• How do Van der Waals forces compare to ionic and covalent bonds?

  They are much weaker and only temporary
• What are the key properties of covalent bonds?

  • Formed by sharing of electrons
  • Result in distinct molecules with a definite number of atoms
  • Create strong bonds between atoms
  • Require a specific number of shared electrons to achieve stability
• How do Van der Waals forces change with molecular size and surface area?

  They increase with size and surface area
• How does the sharing of electrons in a covalent bond create a strong bond between atoms?

  The shared electrons are attracted to the nuclei of both atoms
• How do ionic bonds differ from covalent bonds?

  Ionic bonds involve electron transfer, covalent bonds involve sharing
• What are the key properties of ionic bonding?

  • Formed by electron transfer
  • Involves metal and non-metal atoms
  • Charged ions are created
  • Held together by electrostatic attraction
• What is the appearance of Buckminsterfullerene?

  Grey/black solid
• Why are metallic bonds conductive?

  They have free-flowing electrons that can conduct electricity
• Which specific ionic compound is represented by all the models shown?

  Sodium Chloride (NaCl)
• How do hydrogen bonds compare to covalent bonds?

  Hydrogen bonds are weaker than covalent bonds
• What is the role of electrostatic attraction in ionic bonding?

  It holds the charged ions together
• What are the limitations of using models to represent ionic compounds?

  Models have limitations:

  • Chemical Formula: Lacks charge and structure details.
  • Dot and Cross: No lattice shown.
  • 2D: No ion formation or multiple layers shown.
  • 3D: No charges or spaces shown.
• What is the special characteristic of silicon dioxide?

  Piezoelectric - produces electric charge from mechanical stress
• How do hydrogen bonds compare to Van der Waals forces?

  Hydrogen bonds are much stronger than Van der Waals forces
• What is the conductivity of covalent bonding?


  i
• What is the boiling point of covalent substances compared to metallic and ionic substances?

  Covalent substances have low boiling points
• How do the bonding characteristics differ between simple covalent and giant covalent structures?

  Simple has weak Van der Waals, giant has strong covalent bonds
• What type of bonding is a good conductor in solid form?

  Metallic
• What information is missing from the chemical formula model of NaCl?

  Charges and lattice structure
• How do ionic compounds behave in water regarding solubility?

  They are soluble
• What is a hydrogen bond?

  An extra strong intermolecular force
• What is a covalent bond?

  A bond formed when atoms share electrons in their outer shells
• How do the melting and boiling points differ between the three types of bonding?

  • Metallic: High melting and boiling points
  • Ionic: High melting and boiling points
  • Covalent: Low melting and boiling points
• What is the electrical conductivity of graphene?

  Very good conductor
• What is the result of covalent bonding between atoms?

  Formation of distinct molecules with a definite number of atoms
• What is the conductivity of metallic bonding?

  C
• How do different bonding types affect physical properties?

  • Metallic: Good conductors, high melting/boiling points, insoluble in water
  • Ionic: Conductors in liquid, high melting/boiling points, soluble in water
  • Covalent: Poor conductors, low melting/boiling points, insoluble in water
• How does the conductivity of each type of bonding vary?

  • Metallic: Conductive (c = conductor)
  • Ionic: Conductive (c = conductor)
  • Covalent: Insulating (i = insulator)
• What are the properties of graphene?

  • Very high melting and boiling point
  • Very good conductor
  • Transparent sheets
  • Very strong and flexible; 100 times stronger than steel
• What is the electrical conductivity of Buckminsterfullerene?

  Good
• In which metal does delocalized electron movement enable conductivity?

  Copper ($Cu$)
• What are the structural differences between ionic lattices and metallic lattices?

  • Ionic lattice:
  • Forms from alternating positive and negative ions
  • Regular 3D pattern
  • Metallic lattice:
  • Metal atoms in a regular array
  • Delocalized electrons move freely
• What is the special characteristic of diamond?

  Hardest known naturally occurring substance
• What type of forces exist between molecules in simple covalent structures?

  Weak Van der Waals forces
• What are the different types of bonds present in this molecule?

  • Covalent bonds between hydrogen (H) and oxygen (O) atoms
  • Polar bonds due to the difference in electronegativity between H and O
  • Hydrogen bonds between the partially positive H atoms and the partially negative O atoms
• What is the solubility of metallic substances in water?

  Insoluble
• What is the melting point of metallic bonding?

  High