C2.3.1 Properties of Ionic Compounds

    Cards (49)

    • What type of particles are formed when electrons are transferred between metals and non-metals in ionic compounds?
      Ions
    • Electrostatic attraction is the bonding mechanism in ionic compounds.

      True
    • What does the coordination number in ionic compounds refer to?
      Nearest-neighbor ions
    • Ionic compounds have high melting and boiling points due to strong electrostatic forces.
      True
    • What type of energy is required to overcome the strong ionic bonds in ionic compounds?
      Electrostatic energy
    • The coordination number in ionic compounds influences the packing efficiency of the crystal structure.

      True
    • The crystal structure of ionic compounds is characterized by a regular, repeating arrangement of cations and anions
    • The coordination number in an ionic compound directly influences its packing efficiency.
      True
    • Two key factors affecting the melting and boiling points of ionic compounds are the charge and the size
    • Higher ion charges in ionic compounds result in stronger ionic bonds and higher melting points.

      True
    • How does the size of ions affect the melting and boiling points of ionic compounds?
      Larger ions lower melting points
    • Which type of ionic compounds are generally highly soluble in water?
      Small, highly charged ions
    • When are ionic compounds good conductors of electricity?
      Molten or in aqueous solution
    • Ionic compounds in the solid state are generally poor conductors of electricity.

      True
    • In an ionic compound, the metal becomes a cation by losing electrons
    • What type of ion does a metal form in an ionic compound?
      Cation
    • Ionic compounds are formed by the sharing of electrons between atoms.
      False
    • An example of an ionic compound is NaCl
    • Metals lose electrons to form cations in ionic compounds.
      True
    • Larger ions in ionic compounds have weaker ionic bonds and lower melting points.
    • What is the melting point of NaCl in degrees Celsius?
      801
    • Match the ion properties with their solubility in water:
      Small, highly charged ions ↔️ Highly soluble
      Large, low-charged ions ↔️ Poorly soluble
    • Which type of ions in ionic compounds are highly soluble in water?
      Small, highly charged ions
    • Why are metallic compounds good conductors of electricity?
      Delocalized electrons
    • Ionic compounds are formed by the transfer of electrons between metals and non-metals
    • Match the type of compound with its bonding mechanism:
      Ionic ↔️ Electrostatic attraction
      Covalent ↔️ Electron sharing
    • The coordination number in ionic compounds influences the degree to which ions are closely packed
    • Arrange the following factors affecting the melting point of ionic compounds in order of their effect, from strongest to weakest:
      1️⃣ Charge of the ions
      2️⃣ Size of the ions
    • The high melting and boiling points of ionic compounds are due to the strong ionic bonds
    • What is meant by the term "packing efficiency" in the context of ionic compounds?
      Degree ions are closely packed
    • What does the coordination number in an ionic compound's crystal structure refer to?
      Nearest-neighbor ions
    • Why are the melting and boiling points of ionic compounds generally high compared to covalent compounds?
      Strong electrostatic attractions
    • The solubility of ionic compounds in water depends on the strength of the ionic bonds and the size
    • Polar water molecules can overcome the strong electrostatic attractions in ionic compounds with small, highly charged ions, making them soluble.

      True
    • Covalent compounds are poor conductors of electricity because electrons are tightly bound between atoms
    • What type of crystal structure do ionic compounds have?
      Regular, repeating arrangement
    • Match the compound type with its bonding description:
      Ionic ↔️ Electrostatic attraction
      Covalent ↔️ Sharing of electrons
      Metallic ↔️ Delocalized electrons
    • Which of the following is an example of an ionic compound?
      NaCl
    • Oppositely charged ions in ionic compounds are held together by electrostatic attractions
    • What is the name given to the force that holds ions together in ionic compounds?
      Ionic bond