Define isotope
A positively or negatively charged atom
Different forms of the same element with a different number of protons
Different forms of the same element with a different number of neutrons
A positively and negatively charged group of atoms
Isotopes have different physical properties
What did J. J. Thomson discover?
Protons
Electrons
Neutrons
Ions
Atoms weren't solid
Atoms are solid spheres
Shells
Plum pudding model
Tiny positively charged nucleus surrounded by a 'cloud' of negative electrons
What did Rutherford discover?
Atoms aren't solid
The relative atomic mass is the mean mass of an atom of an element, compared to 1/12 of the mass of an atom of .
Define relative molecular mass
The average mass of a molecule compared to 1/12 of the mass of an atom of carbon-12
The weighted mean mass of an atom of an element, compared to 1/12 of the mass of an atom of carbon-12
The average mass of a formula unit, compared to 1/12 of the mass of an atom of carbon-12
The mass of an atom of an isotope of an element compared to 1/12 of the mass of an atom of carbon-12
What is the difference between relative formula mass and relative molecular mass?
Relative molecular mass is compared to 1/12 of the mass of an atom of carbon-12, whist formula is compared to the whole atom
Relative formula mass is used for charged molecules
Relative formula mass is used for compounds that are ionic or giant covalent
Relative formula mass is used for metallic compounds
How many particles are in one mole?
6.02 x 10²⁴
6.02 x 10²³
6.02 x 10²⁶
6.02 x 10²¹
What is the ideal gas equation?
pR = nVT
p = nRT
pT = nRV
pV = nRT
What is the equation that links concentration with moles and volume?
Moles = Concentration x Volume
Moles = Concentration / Volume
Moles = Volume/ Concentration
The empirical formula is the whole number of atoms of each element in a compound.
The molecular formula is the actual numbers of of each type of in a molecule.
When a hydrocarbon is burnt in excess oxygen, 8.8g of CO₂ and 3.6g of H₂O are made. What is the empirical formula of the hydrocarbon?
CH₄
C₂H₄
CH
CH₂
