Flashcards
Electronic structure and ionisation energy
Cards in this deck (26)
- 1What do electrons have in the currently accepted model of the atom?Fixed energy levels.
- 2How does a shell’s energy and principal quantum number change the further it is from the nucleus?Its energy and principal quantum number increase.
- 3What do experiments show about electrons energy levels in a shell?Not all the electrons in a shell have exactly the same energy.
- 4Which model explains why not all electrons in a shell have exactly the same energy? How?The atomic model explains that the shells are divided into sub-shells. Different electron shells have different numbers of sub-shells, which each have a different energy.
- 5What are the types of sub-shells?s sub-shells, p sub-shells, d sub-shells or f sub-shells.
- 6What do sub-shells contain?Orbitals.
- 7How many orbitals does each sub-shell have? What is the maximum number of electrons each sub-shell can hold?
- 8• For the first four shells, what are the sub-shells and the total number of electrons it can hold?
- 9What is electron configuration?The number of electrons an atom or ion has and how they’re arranged.
- 10What are the three ways that electron configuration can be shown?Sub-shell notation, arrows in boxes or energy level diagrams.
- 11What does each part represent in the sub-shell notation 1s^2?1 = Energy level / shell (principal quantum number)
s = sub-shell
2 = number of electrons - 12When representing electron configuration using boxes, what does each box represent?An orbital.
- 13When representing electron configuration using boxes, what does each arrow represent?An electron.
- 14What must two electrons in the same orbital have?Opposite spin.
- 15What do energy level diagrams show?The energy of the electrons in different orbitals as well as the number of electrons in their arrangement.
- 16What do energy levels look like?
- 17What is an exception to the energy of the electrons increasing as the principal quantum number increases?The 4s sub-shell has a lower energy level than the 3d sub-shell.
- 18What are the three rules when working out electron configurations?1. Electrons fill the lowest energy sub-shells first.
2. Electrons fill orbitals in a sub-shell singly before they start sharing.
3. For the configuration of ions from the s and p blocks of the periodic table, just add or remove the electrons to or from the highest energy occupied sub-shell. - 19How are electron configurations shortened?Noble gas symbols in square brackets are sometimes used as shorthand in electron configurations.
- 20How would calcium be written in shorthand?[Ar]4s2
- 21What are the two elements that don’t follow the usual rules for electron configuration? What do they do differently in terms of their electron configuration and why?Chromium and copper. They donate one of their 4s electrons to 3d sub-shell because they are more stable with a full or half-full d sub-shell.
- 22What is the electron configuration of a Chromium atom?1s2 2s2 2p6 3s2 3p6 3d5 4s1.
- 23What do transition metals do differently when they become ions?They lose their 4s electrons before their 3d electrons.
- 24check computercheck computer
- 25Define first ionisation energy?The energy needed to remove 1 electron from each atom in 1 moles of gaseous atoms to form 1 mole of gaseous 1+ atoms.
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- A2 Chemistry Flashcards on Electronic structure and ionisation energy, created by Jasmine Bayliss-Dagg on 21/09/2017.
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- Jasmine Bayliss-Dagg
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