Bonding, Structure and the Properties of Matter Flashcards
What type of ion does a group 1 element form?
+ (positive)
What type of ion does a group 7 element form?
- (negative)
Describe how an ionic bond forms.
A metal loses electrons to form a positive ion and the non-metal gains these electrons to form a negative ion. These ion are strongly attracted to each other by electrostatic force.
Describe the structure of a crystal of sodium chloride.
A giant ionic lattice.
List the main properties of ionic compounds.
High melting/boiling point (due to strong bonds)
Can’t conduct electricity.
Can dissolve easily in water.
Describe how covalent bonds form.
Non-metal atoms bond by sharing pairs of electrons
Explain why simple molecular compounds typically have low melting and boiling points.
You don’t have to break the covalent bonds, only the weak intermolecular forces.
Describe the structure of a polymer.
Lots of small units covalently bonded together to form a long molecule.
Give three examples of giant covalent substances.
Diamond
Graphite
Buckministerfullerene
Explain why graphite can conduct electricity.
It has one delocalised electron per atom, allowing it to carry charge.
Explain how fullerenes could be used to deliever drugs into the body.
They are a hollow ball shape, which can be used to cage other molecules.
What is metallic bonding?
Strong forces of electrostatic attraction between the positive metal ions and the shared negative electrons.
List three properties of metals and explain how metallic structure causes each property.
Solid at room temperature - strong bonds that require a lot of energy to break
Good conductors of heat/electricity - sea of delocalised electrons to carry energy
Malleable - layers of atoms can slide over each other easily.
Explain why alloys are harder than pure metals.
Differently sized atoms bonded together are more difficult to slide over each other.
Name the three states of matter.
Solid
Liquid
Gas
