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Atomic Structure

Kirsten Rowland 11 preguntas

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Preguntas del test (11)

  1. 1Define relative atomic mass.
    1. AThe weighted mass of one mole of an atom compared to 1/12th of an atom of carbon-12.
    2. BThe average weighted mass of one mole of an atom compared to 1/12th of an atom of carbon-12.
    3. CThe number of protons found in the nucleus of an atom.
    4. DThe sum of protons and neutrons found in the nucleus of an atom.
  2. 2What are the features of isotopes?
    1. AThey have the same number of protons but a different number of neutrons as its standard element.
    2. BThey have the same number of neutrons but a different number of protons as its standard element.
    3. CThey have the same number of electrons as its standard element.
    4. DThey have a different number of electrons as its standard element.
  3. 3Bromine's atomic number is 79 and its atomic mass is 35. Use the periodic table to help you.
    1. AVerdadero
    2. BFalso
  4. 4Electron configuration of bromine = 1s2 [blank_start]2s[blank_end]2 2p[blank_start]6[blank_end] 3[blank_start]s[blank_end]2 3p6 4s[blank_start]2[blank_end] [blank_start]3d10[blank_end] [blank_start]4p[blank_end]5
    1. A3d10
    2. B4p
    3. C2
    4. Ds
    5. E6
    6. F2s
  5. 5First ionisation energy is the [blank_start]amount of energy[blank_end] it take to remove the [blank_start]most loosely held[blank_end] electron from the outer shells of [blank_start]one mole[blank_end] of a gaseous atom to produce one mole of [blank_start]gaseous ions[blank_end] with a charge of [blank_start]1+[blank_end].
    1. Aamount of energy
    2. Bnumber of electrons
    3. Cnumber of ions
    4. Dmost loosely held
    5. Einnermost
    6. Fvalence
    7. Gone mole
    8. Hone iota
    9. Ione gram
    10. Jgaseous ions
    11. Ksolid ions
    12. Lelectronic energy
    13. M1+
    14. N2-
    15. O1-
  6. 6The [blank_start]first[blank_end] ionisation energy of [blank_start]sodium[blank_end] = [blank_start]Na[blank_end](g) -------> Na+[blank_start](g)[blank_end] + [blank_start]e-[blank_end]
    1. Afirst
    2. Bsecond
    3. Csodium
    4. Dnickel
    5. ENa
    6. FNi
    7. G(g)
    8. H(aq)
    9. Ie-
    10. Jheat
  7. 7What happens at the ionisation stage of mass spectrometry?
    1. AAn electron gun fires high energy electrons at the atoms of the vaporised sample, removing the most loosely held electron in each one so they become positively charged.
    2. BAn electron gun fires high energy electrons at the atoms of the vaporised sample, attaching to the outer shell of each one so they become negatively charged.
    3. CThe ions are accelerated so they all have the same kinetic energy.
    4. DThe ions a decelerated so they all have the same kinetic energy.
  8. 8What two things does the m/z ratio show?
    1. AThe mass of the ion
    2. BThe number of protons the ion contains
    3. CThe charge of the ion
    4. DThe weight of the ion
  9. 93 s.f. means exactly the same as 3 d.p.
    1. AVerdadero
    2. BFalso
  10. 10Generally ionisation energy [blank_start]increases[blank_end] across period 3. The dip between Mg and Al occurs because Al has a [blank_start]3p[blank_end] electron orbital which increases the distance between the [blank_start]outer electron[blank_end] and the nucleus and reduces the pull of the [blank_start]nucleus[blank_end]. The drop between P and Si occurs because P has a [blank_start]balanced[blank_end] set of electron orbitals whereas Si has one paired and two [blank_start]singular[blank_end] meaning there is slightly more [blank_start]repulsion[blank_end] so [blank_start]less[blank_end] energy.
    1. Aincreases
    2. B3p
    3. Couter electron
    4. Dnucleus
    5. Ebalanced
    6. Fsingular
    7. Grepulsion
    8. Hless

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Descripción
(Atomic Structure and The Periodic Table) Chemistry Test sobre Atomic Structure, creado por Kirsten Rowland el 23/01/2017.
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