1.7: Metallic Bonding and Interpreting Properties of Substances Flashcards
Q: What is metallic bonding?
A: Metallic bonding is the attraction between positive metal ions and a sea of delocalized electrons.
Q: Why are metals good conductors of electricity?
A: Delocalized electrons in metals can move freely, carrying electric charge.
Q: Why are metals good conductors of heat?
A: The free-moving electrons transfer thermal energy efficiently through the metal.
Q: Why are metals malleable?
A: Metal ions in the lattice can slide over each other without breaking the metallic bonds.
Q: Why do metals have high melting and boiling points?
A: Strong metallic bonds require a lot of energy to break.
Q: What type of bonding is present in ionic compounds?
A: Ionic bonding involves electrostatic attraction between oppositely charged ions.
Q: How can solubility help determine the type of bonding?
A: Ionic compounds dissolve well in water, while non-polar covalent compounds are often insoluble.
Q: Why do covalent compounds have low melting points?
A: Covalent compounds have weak intermolecular forces, requiring little energy to break.
Q: How do the properties of ionic and metallic compounds differ?
A: Ionic compounds are brittle and conduct electricity when molten or dissolved, while metals are malleable and conduct electricity as solids.
Q: How can melting/boiling points indicate the type of bonding?
A: High melting/boiling points suggest strong bonds (ionic, metallic, or giant covalent), while low points suggest weak bonds (simple covalent).
