Date | May 2017 | Marks available | 1 | Reference code | 17M.1.sl.TZ2.6 |
Level | SL | Paper | 1 | Time zone | TZ2 |
Command term | Identify | Question number | 6 | Adapted from | N/A |
Question
Which electron transition emits radiation of the longest wavelength?
Markscheme
C
Examiners report
Syllabus sections
- 18M.1.sl.TZ1.6: Which are correct statements about the emission spectrum of hydrogen in the visible...
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18M.2.sl.TZ1.2b:
State the electron configuration of the Ca2+ ion.
- 22M.2.hl.TZ1.6a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
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18M.2.sl.TZ2.3c.i:
Copper is widely used as an electrical conductor.
Draw arrows in the boxes to represent the electronic configuration of copper in the 4s and 3d orbitals.
- 22M.2.sl.TZ2.2b(iii): Draw an arrow, labelled Z, to represent the lowest energy electron transition in the visible...
- 22M.2.sl.TZ1.2a: Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
- 19N.2.sl.TZ0.1c: Distinguish ultraviolet light from visible light in terms of wavelength and energy.
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22M.1.sl.TZ1.6:
What is the maximum number of electrons that can occupy a p-orbital?
A. 2
B. 3
C. 6
D. 8
- 17M.1.sl.TZ1.6: Which electron transition in the hydrogen atom emission spectrum emits radiation with...
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17M.2.sl.TZ2.1d:
Outline the model of electron configuration deduced from the hydrogen line emission spectrum (Bohr’s model).
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19N.2.sl.TZ0.5a(i):
State the electron configuration of the Cu+ ion.
- 22M.2.sl.TZ2.2b(ii): Draw an arrow, labelled X, to represent the electron transition for the ionization of a...
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18M.2.hl.TZ1.2c:
When calcium compounds are introduced into a gas flame a red colour is seen; sodium compounds give a yellow flame. Outline the source of the colours and why they are different.
-
22M.2.hl.TZ2.5a(i):
State the full electronic configuration of Fe2+.
- 16N.1.sl.TZ0.5: Which is correct for the line emission spectrum for hydrogen? A. Line M has a higher...
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18M.2.sl.TZ1.2c:
When calcium compounds are introduced into a gas flame a red colour is seen; sodium compounds give a yellow flame. Outline the source of the colours and why they are different.
- 18N.1.sl.TZ0.5: Which statements are correct for the emission spectrum of hydrogen? I. The lines converge at...
- 18N.2.hl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
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18N.2.hl.TZ0.3a.ii:
Sketch the orbital diagram of the valence shell of a bromine atom (ground state) on the energy axis provided. Use boxes to represent orbitals and arrows to represent electrons.
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18N.2.sl.TZ0.3a.ii:
Sketch the orbital diagram of the valence shell of a bromine atom (ground state) on the energy axis provided. Use boxes to represent orbitals and arrows to represent electrons.
- 17M.1.sl.TZ1.7: The full electron configuration of an element is: 1s22s22p63s23p2 To which group and period...
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18N.2.hl.TZ0.3a.i:
State the electron configuration of a bromine atom.
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18N.2.sl.TZ0.3a.i:
State the electron configuration of a bromine atom.
-
19M.1.hl.TZ1.4:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
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19M.2.hl.TZ1.6a:
Deduce the full electron configuration of Fe2+.
-
19M.1.sl.TZ2.6:
Which transition in the hydrogen atom emits visible light?
A. n = 1 to n = 2
B. n = 2 to n = 3
C. n = 2 to n = 1
D. n = 3 to n = 2
- 17N.2.hl.TZ0.2b: Outline how this spectrum is related to the energy levels in the hydrogen atom.
-
17N.1.sl.TZ0.6:
Which is the electron configuration of a chromium atom in the ground state?
A. [Ne]3s23p64s13d4
B. [Ar]3d3
C. 1s22s22p63s23p64s23d4
D. [Ar]4s13d5
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17M.2.sl.TZ1.2d.i:
State the full electron configuration of the 2+ ion.
- 19N.1.sl.TZ0.6: Which represents the shape of an s atomic orbital?
-
16N.1.sl.TZ0.6:
What is the condensed electron configuration of the Fe2+ ion?
A. [Ar]3d6
B. [Ar]3d44s2
C. [Ar]3d54s1
D. [Ar]3d64s2 - 16N.2.hl.TZ0.4c: Magnesium ions produce no emission or absorption lines in the visible region of the...
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16N.2.hl.TZ0.4d:
(i) Explain the convergence of lines in a hydrogen emission spectrum.
(ii) State what can be determined from the frequency of the convergence limit.
- 21N.1.sl.TZ0.6: How many p-orbitals are occupied in a phosphorus atom? A. 2 B. 3 C. 5 D. 6
- 17N.2.sl.TZ0.2d: Describe the emission spectrum of hydrogen.
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19M.1.sl.TZ1.6:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
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19N.2.hl.TZ0.6a(i):
State the electron configuration of the Cu+ ion.
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18M.2.sl.TZ2.3a.i:
Draw the first four energy levels of a hydrogen atom on the axis, labelling n = 1, 2, 3 and 4.
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21M.2.hl.TZ2.2b(iv):
[Cr(OH)6]3− forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.
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18M.2.sl.TZ2.3a.ii:
Draw the lines, on your diagram, that represent the electron transitions to n = 2 in the emission spectrum.
-
22M.1.sl.TZ1.8:
Which of the following is the electron configuration of a metallic element?
A. [Ne] 3s2 3p2
B. [Ne] 3s2 3p4
C. [Ne] 3s2 3p6 3d3 4s2
D. [Ne] 3s2 3p6 3d10 4s2 4p5
- 22M.1.sl.TZ2.5: Which experimental results support the theory that electrons exist in discrete energy...
- 21M.1.sl.TZ1.6: Which represents a p orbital?
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21N.2.hl.TZ0.9b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.
Sketch diagrams of 1s, 2s and 2p.
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21M.2.hl.TZ1.1d(iii):
State the full electron configuration of the sulfide ion.
- 21M.1.sl.TZ2.6: How are emission spectra formed? A. Photons are absorbed when promoted electrons return to...
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21M.2.sl.TZ1.1c(ii):
State the full electron configuration of the sulfide ion.
- 21M.2.hl.TZ1.7b: Explain why there are frequencies of UV light that will dissociate O3 but not O2.
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21M.2.sl.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3+.
-
21M.2.hl.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3+.
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20N.2.sl.TZ0.1a(i):
State the full electron configuration of the chlorine atom.
-
20N.1.sl.TZ0.6:
What is the maximum number of electrons that can occupy the 4th main energy level in an atom?
A.
B.
C.
D.
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20N.2.hl.TZ0.1a(i):
State the full electron configuration of the chlorine atom.
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18M.2.hl.TZ2.3a.iv:
Calculate the wavelength, in m, for the electron transition corresponding to the frequency in (a)(iii) using section 1 of the data booklet.
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21N.2.hl.TZ0.9b(ii):
State the electron configuration of copper.
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21N.2.sl.TZ0.8b(ii):
State the electron configuration of copper.
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21N.2.sl.TZ0.8b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.
Sketch diagrams of 1s, 2s and 2p.