State what is meant by the term orbital.
Draw the shapes of the s, px, py and pz orbitals.
State the maximum number of orbitals in the n = 4 energy level.
State the d, f, p and s orbitals in order of decreasing energies.
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Write the condensed electronic configurations for the following species
i) Na
[1]
ii) Al3+
[1]
Complete the orbital diagrams of phosphorus and fluorine as shown in the diagram below.
Give the number of each type of orbital in the first four energy levels.
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Using sections 1 and 5 of the data booklet describe how the following change in moving from the infrared region of the electromagnetic spectrum to the radio region of the electromagnetic spectrum.
i) Wavelength
[1]
ii) Frequency
[1]
iii) Energy
[1]
Describe the process occurring in an atom to produce a single line on an emission spectrum.
Distinguish between a continuous spectrum and a line spectrum.
Describe the emission spectrum of hydrogen. Outline how this spectrum is related to the energy levels in the hydrogen atom.
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The element chromium has several naturally occurring isotopes whose abundances are shown below.
Mass number | % abundance |
50 | 4.345 |
52 | 83.789 |
53 | 9.501 |
54 | 2.365 |
Calculate the relative atomic mass of chromium to two decimal places.
State the full electron configuration for chromium.
State the meaning of [Ar] and complete the orbital diagram shown below for chromium.
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This question is about line emission spectra of elements.
i) Explain the difference between a continuous spectrum and a line spectrum.
[2]
ii) Draw a labelled diagram that shows electron transitions in a hydrogen atom in the ultraviolet and visible regions of the electromagnetic spectrum. Include three electron transitions for each region.
[4]
The visible line emission spectrum of hydrogen is shown below in the diagram, and the wavelengths of the first four lines are listed in the table.
i) Use the information provided and Sections 1 and 2 of the IB data booklet to determine the frequency of the red line.
[1]
The visible line emission spectrum hydrogen
Table 1
Balmer spectral line | Wavelength in nm | Colour |
Hα | 656 | Red |
Hβ | 486 | Blue(cyan) |
Hγ | 434 | Blue |
Hδ | 410 | Violet |
ii) Which spectral line carries more energy, Hα or Hδ?
[1]
Draw the shape of a 1s atomic orbital and 2p atomic orbital.
Describe the relationship between colour, energy, frequency, and wavelength in the visible spectrum.
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The element rubidium has two naturally occurring isotopes of 85Rb and 87Rb. The relative atomic mass of rubidium is 85.47. Calculate the percentage abundance of each isotope.
Rubidium forms an ionic compound with selenium, Rb2Se.
Using boxes to represent orbitals and arrows to represent electrons, sketch the orbital diagram of the valence shell of selenium on the axis provided.
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The diagram below shows electron transitions in a hydrogen atom in two regions of the electromagnetic spectrum.
Using section 5 of the data booklet, predict which electron transition is most likely to correspond to the emission of red light.
Using sections 1 and 5 of the data booklet, predict which electron transition will correspond to the greatest frequency of light emitted.
The wavelengths of the first four lines for the Balmer series are shown below.
Balmer spectral line | Wavelength in nm | Colour |
Hα | 656 | red |
Hβ | 486 | cyan(blue) |
Hγ | 434 | blue |
Hδ | 410 | violet |
Using section 1 of the Data booklet, determine the ratio of the frequencies Hα to Hγ to 2 decimal places.
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