Electronic Configurations (DP IB Chemistry)
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What is the electromagnetic spectrum?
The electromagnetic spectrum is a range of frequencies that covers all electromagnetic radiation and their respective wavelengths and energy.
True or False?
The electromagnetic spectrum is divided into bands or regions.
True.
The electromagnetic spectrum is divided into bands or regions.
Define the term frequency, in relation to the electromagnetic spectrum.
Frequency is the number of waves per second.
What is the relationship between frequency and wavelength in the electromagnetic spectrum?
Frequency is inversely proportional to wavelength
What is the difference between a continuous and line spectrum?
A continuous spectrum is a spectrum that contains all frequencies of light whereas a line spectrum is a spectrum that only shows certain fixed frequencies of light.
True or False?
Gamma rays, X-rays, and UV radiation are considered safe forms of radiation.
False.
Gamma rays, X-rays, and UV radiation are all dangerous forms of radiation.
Describe what happens to energy moving from the UV region of the electromagnetic spectrum to the microwave region.
Moving from the UV region of the electromagnetic spectrum to the microwave region, energy decreases.
Describe what happens to frequency moving from the radio wave region of the electromagnetic spectrum to the infrared region.
Moving from the radio wave region of the electromagnetic spectrum to the infrared region, frequency will increase.
True or False?
The image below is an example of a continuous spectrum.
False.
The image is an example of a line spectrum.
Describe the frequency of a wave that has a long wavelength and low energy.
A wave that has a long wavelength and low energy wil have a low frequency.
What happens when electrons return to their original energy levels after being excited?
When electrons return to their original energy levels, they emit energy.
True or False?
The energy emitted by electrons falling back to lower energy levels is always in the visible spectrum.
False.
The energy emitted can be in the infrared, visible, or ultraviolet regions of the spectrum.
What region of the electromagnetic spectrum do electron jumps from n∞ to n1 correspond to?
Electron jumps from n∞ to n1 correspond to the ultraviolet region of the spectrum.
What region of the electromagnetic spectrum do electron jumps from n∞ to n2 correspond to?
Electron jumps from n∞ to n2 correspond to the visible region of the spectrum.
What region of the electromagnetic spectrum do electron jumps from n∞ to n3 correspond to?
Electron jumps from n∞ to n3 correspond to the infrared region of the spectrum.
Define convergence in relation to emission spectra.
Convergence is when the spectral lines get closer together towards the higher energy end of the spectrum.
True or False?
The emission spectrum of hydrogen in the visible region shows lines converge at a higher frequency.
True.
The emission spectrum of hydrogen in the visible region shows lines converge at a higher frequency.
What does the line emission spectrum of the hydrogen atom provide evidence for?
The line emission spectrum of the hydrogen atom provides evidence for the existence of electrons in discrete energy levels which converge at higher energies.
Define the term ionisation energy, in the context of emission spectra.
Ionisation energy is the maximum amount of energy an electron can reach, corresponding to the energy required for the electron to escape the atom.
Which letter represents the ionisation of hydrogen in the ground state?
A represents the ionisation of hydrogen in the ground state because the ionisation energy corresponds to a transition from the ground state to n=∞
True or False?
The higher the principal quantum number, the lower the energy of the electron within that shell.
False.
The higher the principal quantum number, the greater the energy of the electron within that shell.
Identify the following orbital.
The following orbital is the px orbital.
Identify the following orbital.
The following orbital is the pz orbital.
Identify the following orbital.
The following orbital is the pyorbital.
Identify the following orbital.
The following orbital is the s orbital.
True or False?
The subshells increase in energy as follows: s ＜ p ＜ d ＜ f
True.
The subshells increase in energy as follows: s ＜ p ＜ d ＜ f
What is the maximum number of electrons that can be held in the n=1 principal energy level?
The maximum number of electrons that can be held in the n=1 principal energy level is 2.
What is the maximum number of electrons that can be held in the n=2 principal energy level?
The maximum number of electrons that can be held in the n=2 principal energy level is 8.
What is the maximum number of electrons that can be held in the n=3 principal energy level?
The maximum number of electrons that can be held in the n=3 principal energy level is 18.
What is the maximum number of electrons that can be held in the n=4 principal energy level?
The maximum number of electrons that can be held in the n=4 principal energy level is 32.
True or False?
Each orbital can hold a maximum number of 4 electrons.
False.
Each orbital can hold a maximum number of 2 electrons.
How many electrons can the p subshell hold?
The p subshell hold 6 electrons.
Complete the full electron configuration for sodium.
1s2 2s2
The completed electron configuration for sodium is:
1s2 2s2 2p6 3s1
Complete the full electron configuration for aluminium.
1s2 2s2
The completed electron configuration for aluminium is:
1s2 2s2 2p6 3s2 3p1
Complete the full electron configuration for calcium.
1s2 2s2
The completed electron configuration for calcium is:
1s2 2s2 2p6 3s2 3p6 4s2
What is the condensed electronic configuration for gallium?
The condensed electronic configuration for gallium is:
[Ar] 4s2 3d10 4p1
Which element has the following full electronic configuration of 1s2 2s2 2p6 3s2 3p5?
Chlorine has the full electronic configuration of 1s2 2s2 2p6 3s2 3p5.
What is the condensed electronic configuration for copper?
The condensed electron configuration for copper is:
[Ar] 4s1 3d10
What is the condensed electronic configuration for chromium?
The condensed electronic configuration for chromium is:
[Ar] 4s1 3d5
True or False?
The 4s subshell fills first and empties before the 3d subshell.
True.
The 4s subshell fills first and empties before the 3d subshell.
True or False?
[Ar] 4s2 3d4 is more energetically favourable than [Ar] 4s1 3d5
False.
[Ar] 3d4 4s2 is less energetically favourable than [Ar] 3d5 4s1
What is the full electronic configuration of Sr2+ ?
The full electronic configuration of Sr2+ is:
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
Complete the electronic configuration using box notion for silicon.
The electronic configuration silicon is:
Complete the electronic configuration using box notion for vanadium.
The electronic configuration using box notion for vanadium is:
What is ΔE in the following equation?
ΔE = h ν
ΔE is change in energy.
ΔE = h ν
What is h in the following equation?
ΔE = h ν
h is Planck's constant.
ΔE = h ν
What is v in the following equation?
ΔE = h ν
v is frequency.
ΔE = h ν
What is c in the following equation?
c = ν λ
c is the speed of light.
c = ν λ
What is λ in the following equation?
c = ν λ
λ is wavelength.
c = ν λ
The frequency of the point of convergence on a hydrogen emission spectrum is 32.883 x 1014 s-1.
What is the ionisation energy for one atom of hydrogen?
(h = 6.63 x 10-34 J s)
The ionisation energy for one atom of hydrogen is:
ΔE = h ν
E = 32.883 x 1014 x 6.63 x 10-34 = 2.18 x 10-18 (J)
State the equation to calculate the frequency of the convergence limit.
The equation to calculate the frequency of the convergence limit is:
ν = c ÷ λ
The ionisation energy of a sodium atom is 8.22 × 10−19 J atom−1. Calculate the energy change per mole (kJ mol-1).
Avogadro's constant (NA) 6.02 × 1023
To calculate the energy change per mole (kJ mol-1):
IE1 = 8.22 × 10−19 × 6.02 × 1023
IE1 = 494 844 J mol−1
IE1 = 495 kJ mol−1
True or False?
Down a group ionisation energy decreases as shielding effect increases, therefore, the attraction of outer electrons to the nucleus decreases.
True.
Down a group ionisation energy decreases as shielding effect increases, therefore, the attraction of outer electrons to the nucleus decreases.
Why does ionisation energy increase across a period?
Ionisation energy increase across a period because the nuclear charge increases and the shielding by inner shell electrons remains the same.
Why do the successive ionisation energies of an element increase?
Successive ionisation energies increase because removing electrons from a positive ion becomes more difficult due to increasing attractive forces and decreasing shielding.
Why is there a dip in first ionisation energy, IE1 , between Be and B?
There is a slight decrease in IE1 between beryllium and boron as the fifth electron in boron is in the 2p subshell, which is further away from the nucleus than the 2s subshell of beryllium.
True or False?
There is a slight decrease in IE1 between nitrogen and oxygen due to spin-pair repulsion in the 2px orbital of oxygen.
True.
There is a slight decrease in IE1 between nitrogen and oxygen due to spin-pair repulsion in the 2px orbital of oxygen.
True or False?
The increase in successive ionisation energies is constant.
False.
The increase in successive ionisation energies is not constant and depends on the atom's electronic configuration.
The first five ionisation energies of an element are shown below.
Which group of the Periodic Table is the element found in?
The element is located in Group 13.
Why is there a large decrease in ionisation energy between the last element in one period and the first element in the next period?
There is a large decrease in ionisation energy between periods due to increased distance between the nucleus and outer electrons, and increased shielding by inner electrons in the new shell, which outweigh the increased nuclear charge.
What information can be derived from successive ionisation energy data?
Successive ionisation energy data can be used to:
Predict or confirm the simple electronic configuration of elements
Confirm the number of electrons in the outer shell
Deduce the group an element belongs to in the Periodic Table
Successive ionisation energies for an element are shown.
IE1 = 899 kJ mol-1,
IE2 = 1757 kJ mol-1,
IE3 = 14850 kJ mol-1,
IE4 = 21005 kJ mol-1
Which group of the Periodic Table is the element found in?
The element is found in Group 2 as the largest jump in energy is between Group 2 and Group 13.
IE1 = 899 kJ mol-1,
IE2 = 1757 kJ mol-1,
IE3 = 14850 kJ mol-1,
IE4 = 21005 kJ mol-1
