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Description
Flashcards by Beth Ritchie, updated more than 1 year ago
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Created by Beth Ritchie
about 11 years ago
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| Question | Answer |
| Which 4 factors affect ionisation energy? | Nuclear charge, shielding, atomic radius, repulsion due to spin |
| How does Nuclear Charge affect ionisation energy? | If there are more protons, ionisation energy will be increased due to greater pull on electrons. |
| How does shielding affect ionisation energy? | The more shielding, the more repulsion and thus the lower ionisation energy. |
| How does atomic radius affect ionisation energy? | Larger atomic radius means lower ionisation energy, as they feel the electrostatic force less strongly. |
| How does repulsion due to spin affect ionisation energy? | If the outer electron is paired in a partially filled shell, it is unstable and will be repelled by the other electron in it's pair due to opposite spins. In this case, ionisation energy will decrease. |
| What is ionisation energy? | The energy required to remove an outer electron. |
| How does ionisation energy change across the period? | Ionisation energy increases due to increasing nuclear charge. There will be drops (ie. P - S) where shells are partially filled. |
| How does ionisation energy change going down the group? | Ionisation energy decreases due to greater atomic radius and more shielding. |
| What are the 6 stages in the mass spectrometer? | Vaporisation, ionisation, acceleration, deflection, detection and recording. |
| What is the definition of isotope? | Atoms of an element with a different number of neutrons. They are chemically identical. |
| Define atomic number. | Proton number, Z. The number of protons that one atom of an element contains, and therefore the number of electrons it has. |
| Define Mass number. | A. The number of protons and neutrons an atom of an element contains. |
| Define atom. | The smallest component of an element showing the chemical properties of that element. |
| Define relative atomic mass. | The average mass of an atom relative to 1/12th the mass of a C12 atom. |
| Define relative molecular mass. | The average mass of a molecule relative to 1/12th the mass of a C12 atom. |
| Define relative isotopic mass. | The average mass of an isotope relative to 1/12th the mass of a C12 atom. |
| What is first ionisation energy? | The minimum energy required to remove an ourter electron from one mole of gaseous atoms to form gaseous 1+ atoms. |
| What is second ionisation energy? | The minimum energy required to remove an outer electron from one mole of gaseous 1+ ions to form gaseous 2+ ions. |
| What is the Aufbau principle? | Electrons fill orbitals in order of increasing energy. |
| What are the four orbitals? | S, P, D and F |
| What is an S sublevel like? | It is spherical and can hold 2 electrons. |
| What is a P orbital like? | It holds 6 electrons and is comprised of 3 dumbbells which each hold 2 electrons. |
| What is hunts rule? | Electrons have a property called spin, and they spin in one of two directions. They will always arrange themselves so the number of opposite spins is minimised. |
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