Flashcards
Atomic Structure
Cards in this deck (23)
- 1Which 4 factors affect ionisation energy?Nuclear charge, shielding, atomic radius, repulsion due to spin
- 2How does Nuclear Charge affect ionisation energy?If there are more protons, ionisation energy will be increased due to greater pull on electrons.
- 3How does shielding affect ionisation energy?The more shielding, the more repulsion and thus the lower ionisation energy.
- 4How does atomic radius affect ionisation energy?Larger atomic radius means lower ionisation energy, as they feel the electrostatic force less strongly.
- 5How 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.
- 6What is ionisation energy?The energy required to remove an outer electron.
- 7How 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.
- 8How does ionisation energy change going down the group?Ionisation energy decreases due to greater atomic radius and more shielding.
- 9What are the 6 stages in the mass spectrometer?Vaporisation, ionisation, acceleration, deflection, detection and recording.
- 10What is the definition of isotope?Atoms of an element with a different number of neutrons. They are chemically identical.
- 11Define atomic number.Proton number, Z. The number of protons that one atom of an element contains, and therefore the number of electrons it has.
- 12Define Mass number.A. The number of protons and neutrons an atom of an element contains.
- 13Define atom.The smallest component of an element showing the chemical properties of that element.
- 14Define relative atomic mass.The average mass of an atom relative to 1/12th the mass of a C12 atom.
- 15Define relative molecular mass.The average mass of a molecule relative to 1/12th the mass of a C12 atom.
- 16Define relative isotopic mass.The average mass of an isotope relative to 1/12th the mass of a C12 atom.
- 17What is first ionisation energy?The minimum energy required to remove an ourter electron from one mole of gaseous atoms to form gaseous 1+ atoms.
- 18What 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.
- 19What is the Aufbau principle?Electrons fill orbitals in order of increasing energy.
- 20What are the four orbitals?S, P, D and F
- 21What is an S sublevel like?It is spherical and can hold 2 electrons.
- 22What is a P orbital like?It holds 6 electrons and is comprised of 3 dumbbells which each hold 2 electrons.
- 23What 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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- Chemistry (Atomic Structure) Flashcards on Atomic Structure, created by Beth Ritchie on 13/11/2013.
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- Beth Ritchie
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