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1Define isotope
- AA positively or negatively charged atom
- BDifferent forms of the same element with a different number of protons
- CDifferent forms of the same element with a different number of neutrons
- DA positively and negatively charged group of atoms
2Isotopes have different physical properties
- ATrue
- BFalse
3What did J. J. Thomson discover?
- AProtons
- BElectrons
- CNeutrons
- DIons
- EAtoms weren't solid
- FAtoms are solid spheres
- GShells
- HPlum pudding model
- ITiny positively charged nucleus surrounded by a 'cloud' of negative electrons
4What did Rutherford discover?
- AProtons
- BElectrons
- CNeutrons
- DIons
- EAtoms aren't solid
- FAtoms are solid spheres
- GShells
- HPlum pudding model
- ITiny positively charged nucleus surrounded by a 'cloud' of negative electrons
5The relative atomic mass is the [blank_start]weighted[blank_end] mean mass of an atom of an element, compared to 1/12 of the mass of an atom of [blank_start]carbon-12[blank_end].
- Acarbon-12
- Bweighted
6Define relative molecular mass
- AThe average mass of a molecule compared to 1/12 of the mass of an atom of carbon-12
- BThe weighted mean mass of an atom of an element, compared to 1/12 of the mass of an atom of carbon-12
- CThe average mass of a formula unit, compared to 1/12 of the mass of an atom of carbon-12
- DThe mass of an atom of an isotope of an element compared to 1/12 of the mass of an atom of carbon-12
7What is the difference between relative formula mass and relative molecular mass?
- ARelative molecular mass is compared to 1/12 of the mass of an atom of carbon-12, whist formula is compared to the whole atom
- BRelative formula mass is used for charged molecules
- CRelative formula mass is used for compounds that are ionic or giant covalent
- DRelative formula mass is used for metallic compounds
8How many particles are in one mole?
- A6.02 x 10²⁴
- B6.02 x 10²³
- C6.02 x 10²⁶
- D6.02 x 10²¹
9What is the ideal gas equation?
- ApR = nVT
- Bp = nRT
- CpT = nRV
- DpV = nRT
10What is the equation that links concentration with moles and volume?
- AMoles = Concentration x Volume
- BMoles = Concentration / Volume
- CMoles = Volume/ Concentration
11The empirical formula is the [blank_start]smallest[blank_end] whole number [blank_start]ratio[blank_end] of atoms of each element in a compound.
- Asmallest
- Bratio
12The molecular formula is the actual numbers of [blank_start]atoms[blank_end] of each type of [blank_start]element[blank_end] in a molecule.
- Aatoms
- Belement
13When 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?
- ACH₄
- BC₂H₄
- CCH
- DCH₂
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- User has deleted their subject information Quiz on Half-way quiz, created by Deleted user on 12/03/2018.
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- Deleted user
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- History
- Created on 12 Mar 2018 · updated on 4 Dec 2019
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