Bonding, Structure and Properties of Matter Flashcards
Name the three States of matter, identify them from a simple model and state which changes of state
happen at melting and boiling points
Solid, liquid and gas.
Solid to liquid is melting and liquid to gas is boiling.
Explain changes of state using particle theory and describe factors that affect the melting and boiling point of a substance
Solid to liquid is melting and liquid to gas is boiling.
Gas to liquid is condensing and liquid to solid is freezing.
The amount of energy needed to change state depends on the strength between particles. Stronger forces have higher melting and boiling points.
HT ONLY: Discuss the limitations of particle theory
The particle theory doesn’t show the forces between particles and particles aren’t solid, inelastic spheres so it’s an inaccurate representation.
Recall what (s), (l), (g) and (aq) mean when used in chemical equations and be able to use them appropriately
(s) - solid
(l) - liquid
(g) - gas
(aq) - aqueous (dissolved in water)
2HCl(aq)+ CaCO3(s) → CaCl3(aq) + H2O(l) + CO2(g)
Explain how the structure of ionic compounds affects their properties, including melting and boiling points and conduction of electricity (sodium chloride structure only)
Giant ionic lattice - electrostatic forces of attraction between oppositely charged ions
High melting and boiling point - lots of energy needed to overcome strong bonds
Conduct electricity (when in molten/dissolved) - ions free to move and carry electric charge
Explain how the structure of small molecules affects their properties
Low melting + boiling points - weak intermolecular forces so they are mostly gas/liquid at room temperature
Don’t conduct electricity - no charged particle to carry charge
Explain how the structure of polymers affects their properties
Solid at room temperature they have relatively strong intermolecular forces.
Explain how the structure of giant covalent structures affects their properties
High melting + boiling points - lots of energy needed to overcome strong covalent bonds
Don’t conduct electricity - no charged particle to carry charge
Explain how the structure of metals and alloys affects their properties, including explaining why they are good conductors
High melting and boiling point - lots of energy needed to overcome strong metallic bonds
Thermal conductors - energy transferred by delocalised electrons
Electrical conductors - delocalised electrons carry charge
ONLY METAL: Soft and malleable - layers in metals slide over each other
Explain why alloys are harder than pure metals in terms of the layers of atoms
Alloys are harder than pure metals because the new element distorts the layer of metal atoms therefore they can’t slide past each other.
Explain the properties of graphite, diamond and graphene in terms of their structure and bonding
Graphite - soft & slippery = no bonds between layers, conducts electricity = one delocalised electron 3 C bonds, high melting point = lots of energy needed to break bonds
Diamond - very hard = 4 covalent bonds, high melting point = lots of energy needed to break bonds, doesn’t conduct electricity = no delocalised electron 4 C bonds
Graphene - conducts electricity = one delocalised electron 3 C bonds, strong and light = one layer of graphite
Describe the structure of fullerenes, and their uses, including Buckminsterfullerene and carbon nanotubes
Fullerenes - rings of 6 carbon atoms (sometimes 5 or 7)
They are used to cage other molecules. this could be used to deliver a drug into the body
Nanotubes - used in electronics or to strengethen material without adding weight e.g. tennis rackets frames
