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Victoria Robinson Englisch 41 Karten

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  1. 13 subatomic particlesprotons neutrons and electrons
  2. 2Mass number = ? Atomic number = ? Electrons = ?For a neutral atom, protons = electronsMass number = ? Atomic number = ? Electrons = ?
  3. 3Electrons of an ion = ?Electrons of an ion = ?
  4. 4Isotopes ? Atomic mass ?Isotopes: Atoms with same atomic number (number of protons) but different mass
    number (number of neutrons)
    Atomic Mass: weighted average mass of element’s naturally occurring isotopes    Isotopes ? Atomic mass ?
  5. 5Orbitals• A wave function, ψ, used to determine the volume of space around
    nucleus that an electron is most likely to occupy.
    • Atomic orbitals described by quantum numbers n, l, m
  6. 6s orbitalonly 1s orbital
  7. 7p orbitalsthere are 3p orbitals
  8. 8d orbitalsthere are 5d orbitals
  9. 9quantum numbers n, l, mn = energy level
    l = shape
    m = orientation
  10. 10Electron Configuration DiagramsOrganization of atomic orbitals in electron shells of increasing energy
    shells (n=1, n=2, n=3, ...)    Electron Configuration Diagrams
  11. 11SubshellsWithin a shell
    For example:
    Shell - n=2
    Subshell - 2s, 2p
  12. 12valence electrons- Electrons in outermost shell
    - participate in bonding
  13. 13Electron Configuration Aufbau Principle:lowest E orbitals fill-up first
    (1s, 2s, 2p, 3s, 3p…)
  14. 14Electron Configuration Pauli Exclusion Principle:2 e- max in each atomic orbital and those
    must have opposite spin
  15. 15Electron Configuration Hund’s rule:orbitals in a subshell must be singly occupied with same spin before doubly occupied (with opposite spin)
  16. 16Covalent- electron sharing
    - nonmetal and nonmetal    Covalent
  17. 17ionic- Forms ions
    - gain or lose electrons
    - metal and nonmetal    ionic
  18. 18Drawing Lewis structures streps1. Sum valence electrons of all atoms in molecule (1+4+5=10)
    2. Place least electronegative atom in center (except for H) and connect all
    atoms by single bonds
    3. Fill octets of all atoms (except for H) with lone pairs of e4. Count ein the structure; if more than count in step 1 then create multiple bonds    Drawing Lewis structures streps
  19. 19Non metals that we use in OrgoH, C, N , O, F, Cl, Br, I
    maybe P & S
  20. 20Electronegativy Trend- Everything points to Fluorine
    - O > N > C
  21. 21H in Lewis Structurescannot hold the center position
  22. 22Resonance structures for an ion OCN ^ -Resonance structures for an ion OCN ^ -
  23. 23Carbon in its neutral stateHas 4 bondsCarbon in its neutral state
  24. 24Nitrogen in its neutral stateHas 3 bonds
    and 1 lone pair    Nitrogen in its neutral state
  25. 25Oxygen in its neutral stateHas 2 bonds
    and 2 lone pairs    Oxygen in its neutral state
  26. 26X = F, Cl, Br, I in its neutral stateHas 1 bond
    and 3 lone pairs    X = F, Cl, Br, I in its neutral state
  27. 27Formal charge"every bond (line) counts as 1, every electron (dot) counts as 1!!"
    = # of valence electrons - (each dot + each line)
  28. 28Gaining a bond is (+) Losing a bond is (-)Example:
    Nitrogen in its neutral state has 3 bonds and one lone pair
    Now it has 4 bonds so the charge is (+)
    Why? - a lone pair is more negative than one bond    Gaining a bond is (+) Losing a bond is (-)
  29. 29Resonance structures and formal chargescalculate the formal charge for each atom in the resonance structuresResonance structures and formal charges
  30. 30Best to Worst Resonance Structure The rules.The best resonance contributors have:
    1. Maximum number of covalent bonds
    2. Least charge separation
    3. (-) charge on most electronegative atom and (+) charge on least electronegative atom
    *Electronegativity - O > N > C    Best to Worst Resonance Structure The rules.
  31. 31sp3 hybrid orbitalsTetrahedral Geometrysp3 hybrid orbitals
  32. 32sp2 hybrid orbitalsTrigonal Planar Geometrysp2 hybrid orbitals
  33. 33sp hybrid orbitalsLinear geometrysp hybrid orbitals
  34. 34Sigma bonds• Head to head orbital overlap
    • Cylindrical symmetry of electron density around internuclear axis    Sigma bonds
  35. 35Pi bonds• Side to side orbital overlap
    • Electron density above and below internuclear axis    Pi bonds
  36. 36Single vs double vs triple bondsSingle = 1 sigma bond
    Double = 1 sigma and 1 pi bond
    Triple = 1 sigma and 2 pi bonds    Single vs double vs triple bonds
  37. 37Electron promotion- allowing carbon to have 4 hybrid orbitals ready to bond
    - in between 2s and 2p energy levels    Electron promotion
  38. 38sp3 vs sp2 vs sp- depending on number of domains C has, circle 2, 3, or 4 sp orbitalssp3 vs sp2 vs sp
  39. 39This carbon has 3 domainsso, circle 3 sp orbitalsThis carbon has 3 domainsThis carbon has 3 domains
  40. 40Predicting Hybridization- Electron domains = single b., double b., triple b., lone pair (both dots together count as 1)
    1. Count electron domains around atom of interest
    2. 1 electron domain = 1 site of electron density
    4 domains = sp3
    3 domains = sp2
    2 domains = sp    Predicting Hybridization
  41. 41Predicting Hybridization when lone pairs are omitted in drawings- remember the octet rule. there should be a total of 8 electrons. add a lone pair if drawing has less than 8. then count it as a domainPredicting Hybridization when lone pairs are omitted in drawings

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Karteikarten am 330, erstellt von Victoria Robinson am 05/02/2020.
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Victoria Robinson
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