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Chapter 8 Grade 12 SABIS Chemistry Atomic Structure and Periodicity

Hisham Mahmoud 11 preguntas

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Preguntas del test (11)

  1. 1First ionization energy of sodium causes an [blank_start]......[blank_end] to be changed to an [blank_start].......[blank_end]
    1. AAtom
    2. BIon
    3. CIon
    4. DAtom
  2. 2First ionization energy of sodium causes an electron to be [blank_start]gained[blank_end]
    1. Agained
    2. Blost
  3. 3Ionization energy is [blank_start]added[blank_end] as it [blank_start]creates[blank_end] a bond between electron and atom
    1. Aadded
    2. Bremoved
    3. Ccreates
    4. Dbreaks
  4. 4Write equations to illustrate the first and second ionisation energies of sodium.

    Na([blank_start]g[blank_end]) --> Na[blank_start]+[blank_end](g) + [blank_start]1 e-[blank_end]
    Na+([blank_start]g[blank_end])--> Na[blank_start]2[blank_end]+(g) + [blank_start]1e-[blank_end]
    1. Ag
    2. Bg
    3. C+
    4. D2
    5. E1e-
    6. F1 e-
  5. 5Explain why the second ionization energy of any atom is always larger
    than its first
    The 1st e- is being removed from a [blank_start]neutral atom[blank_end] whereas the second electron is being
    removed from a [blank_start]+1 ion[blank_end], the same nuclear charge is attracting a smaller number of
    electrons, so the electrons are held [blank_start]more firmly[blank_end].
    1. Aneutral atom
    2. Bpositive 1 ion
    3. C+1 ion
    4. Dneutral atom
    5. Emore firmly
    6. Fmore weakly
  6. 6
    The second ionisation energy of sodium is around 9 times larger than its first, while the
    third is only around 1.5 times larger than its second. Suggest why this is so.
    The electron being removed from Na+ is from [blank_start]2p[blank_end] orbitals which are [blank_start]closer[blank_end] to the
    nucleus, shielded less, so more closely attracted to the nucleus. This makes them
    [blank_start]harder[blank_end] to be removed.
    The electron being removed from Na+2 is also from 2p orbitals which are relatively the
    same distance from the nucleus, same shielding, so attracted to the nucleus slightly
    more. This makes them only a little [blank_start]harder[blank_end] to be removed.
    1. A2p
    2. B2s
    3. Ccloser
    4. Dfarther away
    5. Eeasier
    6. Fharder
    7. Gharder
    8. Heasier
  7. 7Na is larger ⇒more [blank_start]shielding[blank_end]
    The electron being removed in Li is the [blank_start]2s[blank_end] and the electron being removed in Na is the
    [blank_start]3s[blank_end]. The electron in 3s is [blank_start]further away[blank_end] from the nucleus
    1. Ashielding
    2. B2s
    3. C3s
    4. Dfurther away
  8. 8Why is the ionisation energy of sodium less than that of magnesium?
    For the same shielding Mg has [blank_start]higher[blank_end] nuclear charge.
    1. Ahigher
    2. Bless
  9. 9Why is the ionisation energy of aluminium less than that of magnesium?
    Al: 1s2 2s2 2p6 3s23p1
    Mg: 1s2 2s2 2p6 3s2
    Removing [blank_start]3p[blank_end] electrons is easier than removing [blank_start]3s[blank_end] electrons because [blank_start]3p[blank_end] are more
    energetic.
    1. A3s
    2. B3p
    3. C3s
    4. D3p
    5. E3p
    6. F3s
  10. 10 IE [blank_start]decreases[blank_end] down a group
    1. Adecreases
    2. Bincreases

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Chapter 8 Grade 12 SABIS Chemistry Atomic Structure and Periodicity
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