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Flashcards

Chemistry Module 2: Chapter 5.1

BUKDABOSS . Chemistry A level English 23 cards

Chemistry Module 2: Chapter 5.1

Cards in this deck (23)

  1. 1What are shells? What are they regarded as? What is the shell number know as? What are shells divided up into?-Shells are the storage of electrons which have fixed energy levels
    -Shells are regarded as energy levels.
    -It is known as the principal quantum number denoted (n)
    -Sub-shells (SUB SHELLS HAVE DIFFERENT ENERGY LEVELS DEPENDANT ON THE SUB SHELL)
  2. 2Why do shells have different energy levels? (SN:Turn over)-This is because they are comprised of different number of sub shells which all have different energy levels.
    For example a S sub shell has only 1 orbital, where as a P sub-shell has 3 orbitals
    ( Orbitals of the same sub shell have the same energy. )
  3. 3What is an atomic orbital? What is spin-pairing?-It is a portion of space that electrons move in.
    -Spin pairing is when within an orbital there are two electrons which spin in opposite directions
  4. 4What are the shape of S orbitals? And how many orbitals do S sub-shells have? What are the shape of P orbitals? And how many orbitals do P sub-shells have?-It is a region around the nucleus that can hold 2 electrons with opposite spins.
    -S-orbitals are sphere shaped and S-Subshells contain 1 orbital which holds 2 electrons
    -P-orbitals are dumbbell shaped and P-Subshells contain 3 orbitals (at right angles to eachother) which each contain 2 electrons.
  5. 5Draw an S orbital? Draw an P orbital?Draw an S orbital? Draw an P orbital?
  6. 6Draw a full P subshell.Draw a full P subshell.
  7. 7How many orbitals do: D-subshells contain? F-subshells contain?-D-subshells contain 5 d orbitals
    -F-subshells contain 7 f orbitals
  8. 8Shells, Sub-shells and Orbitals explanation (TURN OVER)Shells, Sub-shells and Orbitals explanation (TURN OVER)
  9. 9In the shell where n = 1 what orbitals are found and how many? In the shell where n = 2 what orbitals are found and how many? In the shell where n = 3 what orbitals are found and how many? In the shell where n = 4 what orbitals are found and how many?-1 S-orbital
    -1 S-orbital and 3 P-orbitals
    -1 S-orbital, 3 P-orbitals and 5 D-orbitals
    -1 S-orbital, 3 P-orbitals, 5 D-orbitals and 7 F-orbitals
  10. 10In the shell where n = 1 which sub-shells are present? In the shell where n = 2 which sub-shells are present? In the shell where n = 3 which sub-shells are present? In the shell where n = 4 which sub-shells are present?-1s
    -2s + 2p
    -3s + 3p + 3d
    -4s + 4p + 4d + 4f
  11. 11How many electrons are in each subshell when n=1? How many electrons are in each subshell when n=2? How many electrons are in each subshell when n=3? How many electrons are in each subshell when n=4?-2
    -2 + 6 = 8
    -2 + 6 + 10 = 18
    -2 + 6 + 10 + 14 = 32
  12. 12What are the rules for filling oribitals with electrons?-Orbitals fill in order of increasing energy, orbitals fill up singly before they start to pair (if they pair they spin in opposing directions)
  13. 13What are the ways of representing electron configuration?What are the ways of representing electron configuration?
  14. 14Why does the 3d subshell fill after the 4s subshell?-This is because electrons fill in order of energy, and because the 3d sub-shell has a higher energy level than the 4s sub-shell it fills after the 4s sub-shell
  15. 15Why do electron pairs have opposing spins? Why do electrons spin in orbitals?-Because they are negatively charged they will repel eachother, this causes them to spin up and spin down (In opposing directions).
    -The spinning helps counteract the repulsion of the electrons due to them being both negatively charged.
  16. 16Key information about the filling of orbitals.Key information about the filling of orbitals.
  17. 17Key information about the filling of orbitals.Key information about the filling of orbitals.
  18. 18Why do electrons fill singly first?-This is to prevent repulsion between electrons until there is no further orbitals to further fill singly and electron pairing is required.
  19. 19What does the sub-shell notation mean?What does the sub-shell notation mean?
  20. 20What is shorthand electron configuration? How do you do shorthand electron configuration?What is shorthand electron configuration? How do you do shorthand electron configuration?
  21. 21What is a anion? What is a cation?-A positively charged atom which has lost electrons
    -A negatively charged atom which has gained electrons
  22. 22Why does the 4s sub-shell fill up before the 3d subshell but empties before the 3d subshell when it becomes an ion?-This is because when the the 3d sub-shell has a higher energy than the 4s before they have both been filled. But once it has been filled it is at a lower level than the 4s sub-shell.
  23. 23[STUDY TIP BEHIND] Electron configuration examples for ions[STUDY TIP BEHIND] Electron configuration examples for ions

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A level Chemistry (Generals) Flashcards on Chemistry Module 2: Chapter 5.1, created by BUKDABOSS . on 15/11/2018.
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BUKDABOSS .
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