Ionic, covalent, metallic structures,

• What are the three types of bonding that need to be known?

  Ionic, covalent, and metallic
• What happens to a metal atom when it reacts with a non-metal?

  The metal atom loses electrons to form a positively charged ion (cation)
• What do non-metal atoms do when they react with metals?

  They gain electrons to form negatively charged ions (anions)
• What is the structure of ionic compounds called?

  • Giant ionic lattice
  • Closely packed arrangement
  • Strong electrostatic forces of attraction between oppositely charged ions
• What is a single crystal of sodium chloride an example of?

  A giant ionic lattice
• What are the properties of ionic compounds?

  They have high melting points
• What is the process of covalent bonding?

  Atoms share electrons to achieve full outer shells
• What do non-metal atoms do to form covalent bonds?

  They share pairs of electrons
• What are some examples of simple molecular substances?

  • Hydrogen (H₂)
  • Oxygen (O₂)
  • Methane (CH₄)
  • Chlorine (Cl₂)
  • Nitrogen (N₂)
  • Water (H₂O)
  • Hydrogen Chloride (HCl)
• How does hydrogen form covalent bonds?

  Hydrogen atoms form single covalent bonds by sharing one electron
• How do oxygen atoms bond in O₂?

  Two oxygen atoms share two pairs of electrons to form a double covalent bond
• How does carbon bond in methane (CH₄)?

  Carbon forms four covalent bonds with hydrogen atoms
• How do chlorine atoms bond in Cl₂?

  Two chlorine atoms share one pair of electrons to form a single covalent bond
• How do nitrogen atoms bond in N₂?

  Two nitrogen atoms share three pairs of electrons to form a triple bond
• How does water (H₂O) form covalent bonds?

  Oxygen shares a pair of electrons with two hydrogen atoms
• Why do simple molecular substances have low melting and boiling points?

  Weak intermolecular forces need to be broken, not covalent bonds
• What state are most molecular substances in at room temperature?

  Gases or liquids
• How does the size of molecules affect their melting and boiling points?

  Larger molecules have stronger intermolecular forces, requiring more energy to break them
• Why don't molecular compounds conduct electricity?

  They aren't charged and have no free electrons or ions
• What are the characteristics of polymers?

  • Long chains of repeating units
  • Strong covalent bonds between atoms
  • Higher intermolecular forces than simple covalent molecules
  • Generally solid at room temperature
• How do giant covalent structures differ from simple molecular substances?

  Giant covalent structures have all atoms bonded by strong covalent bonds
• What are the properties of giant covalent structures?

  They have very high melting and boiling points
• Why don't giant covalent structures conduct electricity?

  They don't contain charged particles
• What are the main examples of giant covalent structures?

  • Diamond
  • Graphite
  • Silicon dioxide (silica)
• How does diamond's structure contribute to its hardness?

  Each carbon atom forms four covalent bonds in a strong structure
• What is the structure of graphite?

  Graphite has sheets of carbon atoms arranged in hexagons
• Why is graphite soft and slippery?

  There are weak forces between the layers, allowing them to move over each other
• What are the characteristics of metallic bonding?

  • Involves delocalised electrons
  • Strong electrostatic attraction between electrons and positive metal ions
  • Forms a regular structure
• Why are most metals solid at room temperature?

  They have high melting and boiling points due to strong forces between atoms
• How do delocalised electrons contribute to the properties of metals?

  They carry electrical current and thermal energy
• What does it mean for metals to be malleable?

  They can be bent or hammered into flat sheets
• Why are alloys harder than pure metals?

  Alloying distorts the layers of metal atoms, making them harder to slide over each other
• What is an example of a metallic element?

  Copper
• What is the significance of delocalised electrons in metallic bonding?

  They allow metals to conduct electricity and heat
• What is the role of electrostatic forces in metallic bonding?

  They hold the metal atoms together in a regular structure
• How do the properties of metals relate to their structure?

  The structure allows for delocalised electrons, contributing to conductivity and malleability
• What are the differences between ionic, covalent, and metallic bonding?

  • Ionic bonding: Transfer of electrons, forms ions
  • Covalent bonding: Sharing of electrons, forms molecules
  • Metallic bonding: Delocalised electrons, forms a regular structure