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| Question | Answer |
| Name the 3 subatomic particles that make up an atom | Proton Neutron Electron |
| What is the relative masses of the 3 subatomic particles? | PROTON = 1 NEUTRON = 1 ELECTRON = 1/2000 |
| What is the relative charge of the 3 subatomic particles? | PROTON = +1 NEUTRON = 0 ELECTRON = -1 |
| Complete the sentences: Ions have different numbers of protons and ___________. A negative charge means that there's more __________ than _________. A positive charge means that there are more ___________ than ___________. | Ions have different numbers of protons and ELECTRONS. A negative charge means that there's more ELECTRONS than PROTONS. A positive charge means that there are more PROTONS than ELECTRONS. |
| What are isotopes? | Isotopes of an element are atoms with the same number of protons but different number of neutrons |
| Why do isotopes have the same chemical properties but different physical properties? | CHEMICAL They have the same electron configuration PHYSICAL Physical properties tend to depend more on the mass of the atom |
| Name the 4 atomic models | Dalton's model Thomson's model Rutherford's model Bohr's model |
| Describe Dalton's model of atomic structure | Dalton described atoms as solid spheres, and that different types of sphere made up different elements |
| Describe Thomson's model of atomic structure | J.J. Thomson concluded that atoms weren't solid and indivisible. His measurements of charge and mass showed that an atom must contain negatively charged particles (electrons). The new model was known as the 'plum pudding model'. |
| Describe Rutherford's model of atomic structure | Rutherford and his students Geiger and Marsden conducted the gold foil experiment. Rutherford came up with the nuclear model of the atom, where there is a tiny positively charged nucleus surrounded by a 'cloud' of negative electrons. He then discovered that the nucleus contained protons, which led James Chadwick to discover the neutron. |
| Describe Bohr's model of atomic structure | Bohr proposed a new model with four basic principles: 1. Electrons can only exist in fixed orbits (shells) and not anywhere in between 2. Each shell has a fixed energy 3. When an electron moves between shells, electromagnetic radiation is emitted or absorbed 4. As the energy of shells is fixed, the radiation will have a fixed frequency The Bohr model also explained why noble gases are inert |
| Define relative atomic mass | The relative atomic mass (Aᵣ) is the weighted mean mass of an atom of an element, compared to 1/12th of the mass of an atom of carbon-12 |
| Define relative isotopic mass | Relative isotopic mass is the mass of an atom of an isotope of an element compared to 1/12th of the mass of an atom of carbon-12 |
| Define relative molecular mass | The relative molecular mass (Mr) is the average mass of a molecule compared to 1/12th of the mass of an atom of carbon-12. |
| How would you find the Mr of a molecule using Ar values? | Add up the Ar values of all atoms in the molecule |
| Define relative formula mass | Relative formula mass is the average mass of a formula unit, compared to 1/12th of the mass of an atom of carbon-12 |
| What is the difference between relative molecular mass and relative formula mass? | Relative formula mass is used for compounds that are ionic (or giant covalent, e.g. SiO₂) |
| Complete the sentence: Different isotopes of an element occur in different... | Quantities, or isotopic abundances |
| What is the equation for relative Ar, using isotopic masses? |
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| If the isotopic abundances are not given as percentages but as a relative abundance, how would you calculate relative Ar? | 1. Multiply each relative isotopic mass by its relative abundance and add up the results 2. Divide by the sum of the relative abundances |
| What is mass spectra used for in isotopes? | Determining the relative isotopic masses and relative abundances of the isotope Calculating the relative atomic mass of an element from the relative abundances of its isotopes |
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