C1 Key concepts in chemistry Flashcards
What is the formula for moles?
moles = mass/ molar mass
What is Avogadros constant?
6.02 x10^23
What is the order of prioritisation when balancing equations?
- metals
- non metals
- hydrogen
- oxygen
What is the test for hydrogen?
- lighted splint
- squeaky pop
What is the test for oxygen?
- glowing splint
- re ignites
How do you find the relative formula mass of compounds?
atomic mass x number of element
eg. CH4
1 carbon, atomic mass of 12
4 hydrogen, atomic mass of 1
(1x12) + (4x1) = 16
What is an ionic bond?
a bond that involves the electrostatic attraction between oppositely charged ions
between a none metal and metal
transfer of electrons
properties of ionic compounds:
- conduct electricity when molten/dissolved but NOT when solid
- very high melting/boiling point due to strong electrostatic forces
- metal and non metal
properties of simple covalent molecules:
- non metals
- joined by strong covalent bonds but weak intermolecular forces
- low melting and boiling points
- usually gas at room temperature
- do not conduct electricity
properties of diamond:
- giant covalent molecule
- giant 3D lattice
- each carbon atom bonded to 4 others
- very high boiling and melting point due to 4 strong covalent bonds on each carbon atom
- doesn’t conduct electricity due to no free electrons
properties of graphite:
- giant 3D covalent
- each carbon covalently
bonded to 3 others in layers - weak intermolecular forces hold the layers together
- high melting/boiling point
- conducts electricity due to delocalised pool of electrons which can carry charge
- layers slide over each other making a great lubricant
properties of fullerene:
- hollow molecules
- conducts electricity
- e.g. nanotubes, buckminsterfullerene
- used as catalysts due to large surface area
- used as medicine cages
- nanotubes strengthen other materials because they don’t break when stretched and add little weight
moles formula
moles = mass / Mr
atoms = moles x avogadro
how to use empirical formula to determine molecular formula:
1) find the Mr of the empirical formula by using the Ar values of the compound
2) divide the Mr of the empirical formula by the Mr of the actual compound
3) multiply everything in the empirical formula by the result from step 2
definition of empirical formula:
simplest ratio of atoms