bonding and physical properties

• How many main types of crystal lattice structure are there?

  Four
• What is an example of a metallic crystal lattice structure?

  Mg
• What is an example of a simple molecular crystal lattice structure?

  I2
• What is an example of a giant covalent crystal lattice structure?

  Diamond
• What are the four types of crystal lattice structures and their bonding types?

  • Ionic: Ionic bonding
  • Metallic: Metallic bonding
  • Simple molecular: Covalent bonding
  • Giant covalent: Covalent bonding
• What are the physical properties of the four crystal types?

  • Ionic: High melting/boiling points, solid at room temperature, conductive when molten or in solution, soluble in water.
  • Metallic: High melting/boiling points, solid at room temperature, high conductivity, insoluble in water.
  • Simple molecular: Low melting/boiling points, usually liquid or gas at room temperature, non-conductive, solubility depends on polarity.
  • Giant covalent: Very high melting/boiling points, solid at room temperature, non-conductive, insoluble in water.
• Why do ionic compounds have high melting and boiling points?

  Strong electrostatic forces between ions
• How do ionic compounds conduct electricity?

  Charged ions move when molten or dissolved
• Why are ionic compounds soluble in water?

  Charged ions interact with polar water molecules
• Why do metals have high melting points?

  Strong forces between positive ions and electrons
• How do metals conduct thermal energy?

  Delocalised electrons conduct thermal energy
• Why do metals conduct electricity?

  Delocalised electrons carry charge through metals
• Why are metals insoluble in water?

  Strong metallic bonds prevent dissolution
• Why do simple molecules have low melting and boiling points?

  Weak intermolecular forces require little energy
• What is a peculiar property of ice compared to water?

  Ice is less dense than water
• Why do simple molecules have poor electrical conductivity?

  Absence of charged particles prevents conduction
• How does molecular polarity affect solubility?

  Polar molecules can form hydrogen bonds with water
• Why do giant covalent substances have very high melting and boiling points?

  Many strong covalent bonds require significant energy
• How does graphite conduct electricity?

  Delocalised electrons between carbon layers allow conduction
• Why do diamond and silicon(IV) oxide not conduct electricity?

  Localized electrons prevent electrical conduction
• Why are giant covalent substances insoluble in water?

  Strong covalent bonds prevent interaction with water
• What does a high melting point and electrical conductivity when molten indicate about a substance?

  It likely has an ionic crystal lattice structure