1.3 Electronic Configurations

Question 1

What is the electromagnetic spectrum?

Answer 1

The electromagnetic spectrum is a range of frequencies that covers all electromagnetic radiation and their respective wavelengths and energy.

Question 2

True or False?

The electromagnetic spectrum is divided into bands or regions.

Answer 2

True.

The electromagnetic spectrum is divided into bands or regions.

Question 3

Define the term frequency, in relation to the electromagnetic spectrum.

Answer 3

Frequency is the number of waves per second.

Question 4

What is the relationship between frequency and wavelength in the electromagnetic spectrum?

Answer 4

Frequency is inversely proportional to wavelength

Question 5

What is the difference between a continuous and line spectrum?

Answer 5

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.

Question 6

True or False?

Gamma rays, X-rays, and UV radiation are considered safe forms of radiation.

Answer 6

False.

Gamma rays, X-rays, and UV radiation are all dangerous forms of radiation.

Question 7

Describe what happens to energy moving from the UV region of the electromagnetic spectrum to the microwave region.

Answer 7

Moving from the UV region of the electromagnetic spectrum to the microwave region, energy decreases.

Question 8

Describe what happens to frequency moving from the radio wave region of the electromagnetic spectrum to the infrared region.

Answer 8

Moving from the radio wave region of the electromagnetic spectrum to the infrared region, frequency will increase.

Question 9

True or False?

The image below is an example of a continuous spectrum.

Answer 9

False.

The image is an example of a line spectrum.

Question 10

Describe the frequency of a wave that has a long wavelength and low energy.

Answer 10

A wave that has a long wavelength and low energy wil have a low frequency.

Question 11

What happens when electrons return to their original energy levels after being excited?

Answer 11

When electrons return to their original energy levels, they emit energy.

Question 12

True or False?

The energy emitted by electrons falling back to lower energy levels is always in the visible spectrum.

Answer 12

False.

The energy emitted can be in the infrared, visible, or ultraviolet regions of the spectrum.

Question 13

What region of the electromagnetic spectrum do electron jumps from n∞ to n1 correspond to?

Answer 13

Electron jumps from n∞ to n1 correspond to the ultraviolet region of the spectrum.

Question 14

What region of the electromagnetic spectrum do electron jumps from n∞ to n2 correspond to?

Answer 14

Electron jumps from n∞ to n2 correspond to the visible region of the spectrum.

Question 15

What region of the electromagnetic spectrum do electron jumps from n∞ to n3 correspond to?

Answer 15

Electron jumps from n∞ to n3 correspond to the infrared region of the spectrum.

Question 16

Define convergence in relation to emission spectra.

Answer 16

Convergence is when the spectral lines get closer together towards the higher energy end of the spectrum.

Question 17

True or False?

The emission spectrum of hydrogen in the visible region shows lines converge at a higher frequency.

Answer 17

True.

The emission spectrum of hydrogen in the visible region shows lines converge at a higher frequency.

Question 18

What does the line emission spectrum of the hydrogen atom provide evidence for?

Answer 18

The line emission spectrum of the hydrogen atom provides evidence for the existence of electrons in discrete energy levels which converge at higher energies.

Question 19

Define the term ionisation energy, in the context of emission spectra.

Answer 19

Ionisation energy is the maximum amount of energy an electron can reach, corresponding to the energy required for the electron to escape the atom.

Question 20

Which letter represents the ionisation of hydrogen in the ground state?

Answer 20

A represents the ionisation of hydrogen in the ground state because the ionisation energy corresponds to a transition from the ground state to n=∞

Question 21

True or False?

The higher the principal quantum number, the lower the energy of the electron within that shell.

Answer 21

False.

The higher the principal quantum number, the greater the energy of the electron within that shell.

Question 22

Identify the following orbital.

Answer 22

The following orbital is the px orbital.

Question 23

Identify the following orbital.

Answer 23

The following orbital is the pz orbital.

Question 24

Identify the following orbital.

Answer 24

The following orbital is the py orbital.

Question 25

Identify the following orbital.

Answer 25

The following orbital is the s orbital.

Question 26

True or False? The subshells increase in energy as follows: s ＜ p ＜ d ＜ f

Answer 26

True. The subshells increase in energy as follows: s ＜ p ＜ d ＜ f

Question 27

What is the maximum number of electrons that can be held in the n=1 principal energy level?

Answer 27

The maximum number of electrons that can be held in the n=1 principal energy level is 2.

Question 28

What is the maximum number of electrons that can be held in the n=2 principal energy level?

Answer 28

The maximum number of electrons that can be held in the n=2 principal energy level is 8.

Question 29

What is the maximum number of electrons that can be held in the n=3 principal energy level?

Answer 29

The maximum number of electrons that can be held in the n=3 principal energy level is 18.

Question 30

What is the maximum number of electrons that can be held in the n=4 principal energy level?

Answer 30

The maximum number of electrons that can be held in the n=4 principal energy level is 32.

Question 31

True or False? Each orbital can hold a maximum number of 4 electrons.

Answer 31

False. Each orbital can hold a maximum number of 2 electrons.

Question 32

How many electrons can the p subshell hold?

Answer 32

The p subshell hold 6 electrons.

Question 33

Complete the full electron configuration for sodium. 1s2 2s2 ‎________

Answer 33

The completed electron configuration for sodium is: 1s2 2s2 2p6 3s1

Question 34

Complete the full electron configuration for aluminium. 1s2 2s2 ‎________

Answer 34

The completed electron configuration for aluminium is: 1s2 2s2 2p6 3s2 3p1

Question 35

Complete the full electron configuration for calcium. 1s2 2s2 ‎________

Answer 35

The completed electron configuration for calcium is: 1s2 2s2 2p6 3s2 3p6 4s2

Question 36

What is the condensed electronic configuration for gallium?

Answer 36

The condensed electronic configuration for gallium is: [Ar] 4s2 3d10 4p1

Question 37

Which element has the following full electronic configuration of 1s2 2s2 2p6 3s2 3p5 ?

Answer 37

Chlorine has the full electronic configuration of 1s2 2s2 2p6 3s2 3p5 ?

Question 38

What is the condensed electronic configuration for copper?

Answer 38

The condensed electron configuration for copper is: [Ar] 4s1 3d10

Question 39

What is the condensed electronic configuration for chromium?

Answer 39

The condensed electron configuration for chromium is: [Ar] 4s1 3d5

Question 40

True or False? The 4s subshell fills first and empties before the 3d subshell.

Answer 40

True. The 4s subshell fills first and empties before the 3d subshell.

Question 41

True or False? [Ar] 4s2 3d4 is more energetically favourable than [Ar] 4s1 3d5

Answer 41

False. [Ar] 3d4 4s2 is less energetically favourable than [Ar] 3d5 4s1

Question 42

What is the full electronic configuration of Sr2+ ?

Answer 42

The full electronic configuration of Sr2+ is: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

Question 43

Complete the electronic configuration using box notion for silicon.

Answer 43

The electronic configuration silicon is:

Question 44

Complete the electronic configuration using box notion for vanadium.

Answer 44

The electronic configuration vanadium is:

Question 45

What is ΔE in the following equation? ΔE = h ν

Answer 45

ΔE is change in energy. ΔE = h ν

Question 46

What is h in the following equation? ΔE = h ν

Answer 46

h is Planck's constant. ΔE = h ν

Question 47

What is v in the following equation? ΔE = h ν

Answer 47

v is frequency. ΔE = h ν

Question 48

What is c in the following equation? c = ν λ

Answer 48

c is the speed of light. c = ν λ

Question 49

What is λ in the following equation? c = ν λ

Answer 49

λ is wavelength. c = ν λ

Question 50

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)

Answer 50

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)

Question 51

State the equation to calculate the frequency of the convergence limit.

Answer 51

The equation to calculate the frequency of the convergence limit is: ν = c ÷ λ

Question 52

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

Answer 52

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

Question 53

True or False? Down a group ionisation energy decreases as shielding effect increases, therefore, the attraction of outer electrons to the nucleus decreases.

Answer 53

True. Down a group ionisation energy decreases as shielding effect increases, therefore, the attraction of outer electrons to the nucleus decreases.

Question 54

Why does ionisation energy increase across a period?

Answer 54

Ionisation energy increase across a period because the nuclear charge increases and the shielding by inner shell electrons remains the same.

Question 55

Why do the successive ionisation energies of an element increase?

Answer 55

Successive ionisation energies increase because removing electrons from a positive ion becomes more difficult due to increasing attractive forces and decreasing shielding.

Question 56

Why is there a dip in first ionisation energy, IE1 , between Be and B?

Answer 56

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.

Question 57

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.

Answer 57

True. There is a slight decrease in IE1 between nitrogen and oxygen due to spin-pair repulsion in the 2px orbital of oxygen.

Question 58

True or False? The increase in successive ionisation energies is constant.

Answer 58

False. The increase in successive ionisation energies is not constant and depends on the atom's electronic configuration.

Question 59

The first five ionisation energies of an element are shown below. Which group of the Periodic Table is the element found in?

Answer 59

The element is located in Group 13.

Question 60

Why is there a large decrease in ionisation energy between the last element in one period and the first element in the next period?

Answer 60

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.

Question 61

What information can be derived from successive ionisation energy data?

Answer 61

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

Question 62

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?

Answer 62

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