S1.3 - electronic configuration

Question 1

What is an emission spectra?

Question 2

What is the line emission spectrum of hydrogen?

Question 3

What is an absorption spectra?

Question 4

How do atoms give out different colors?

Question 5

What is frequency?

Question 6

How do you work out wave speed?

Question 7

What is the electromagnetic spectrum?

Question 8

What is the order of the electromagnetic spectrum?

Question 9

What is the difference between a continuous and a line spectrum?

Question 10

What is the ground and excited state of an atom?

Question 11

What is a photon?

Question 12

What are the Paschen, Balmer and Lyman series?

Question 13

Why do lines converge at higher energies?

Question 14

What is the uncertainty principle?

Question 15

What is an energy level?

Question 16

What is a shell and sub-shell?

Question 17

What are orbitals?

Question 18

How many electrons can each energy level hold?

Question 19

What is the first energy level made out of?

Question 20

What is the second energy level made out of?

Question 21

What is the third energy level made out of?

Question 22

What is Hund’s third rule?

Question 23

What is the Aufbau principle?

Question 24

What is the Pauli-exclusion principle?

Question 25

What is the electronic configuration of Cu and Cr?

Question 26

What are valence electrons?

Question 27

What does the limit of convergence in an emission spectra correspond to?

Question 28

What happens when electrons fall back to lower energy levels?

Answer 28

gives out energy, which depends on the level it falls on

Question 29

What happens when electrons are excited?

Answer 29

they jump up to higher energy levels

Question 30

What is ionization energy?

Question 31

How can we work out ionization energy using a graph?

Answer 31

f - convergence, which occurs when the line intercepts the x-axis
h - Planck’s constant (6.63 x 10^-34)

Question 32

What equation do we use to work out ionization energy?

Answer 32

E = hf

Question 33

How do we work out ionization energy for 1 mole?

Answer 33

E = hf x Avogadro’s constant (6.02 x 10^23)

Question 34

What is successive ionization energy?

Answer 34

energy needed to remove an extra electron, from a positive ion.

Question 35

What are key observations from successive ionization graphs?

Answer 35

1) There is an increase in successive ionization energies.
2) There are big jumps in ionization energies?

Question 36

Why is there an increase in successive ionization energies?

Answer 36

As more and more electrons are removed from the atom, the atom itself becomes more charged, making it more difficult to remove.

Question 37

Why are there big jumps in ionization energy?

Answer 37

There are jumps when electrons are removed from increasingly closer shells to the nucleus, where it will be harder to remove the electrons as the electrons are closer to the + charge in the nucleus.

Question 38

Why is there a big jump between 9th and 10th ionization energy of Aluminium?

Answer 38

Jump between 9th and 10th ionization energies in Al shows that the 10th electron is more difficult to remove than expected, suggesting that the energy level is divided into 2 sub-levels, providing evidence of the existence of sub-shells.

Question 39

What is first ionization energy dependent on?

Answer 39

1) Charge on the nucleus
2) Distance of the outer electron from the nucleus
3) Electrons between outer electron and nucleus

Question 40

Why does 1st ionization energy increase across a period?

Answer 40

Across the period, ENC increases as proton number increases, and the electrons in the valence shell are more strongly attracted to the positive nucleus, and therefore requires more energy to overcome.

Question 41

Why does 1st ionization energy decrease down a group?

Answer 41

Down the group, more shells are added, increasing the shielding between the valence electrons and the nucleus, leading to less attraction between the electrons and nucleus so less energy is required too remove the electron.

Question 42

Why does B have a lower 1st IE than Be, despite having a higher nuclear charge?

Answer 42

The electron removed from B is in a partially filled 2p orbital, which requires less energy than removing an electron from the full and stable 2s orbital in Be.

Question 43

Why does O have a lower 1st IE than N, despite having a higher nuclear charge?

Answer 43

The electron removed from O is in a partially filled 2p orbital, where the electrons are starting to experience a repulsion from paired electrons in this orbital. This requires less energy than removing it from the half-full and semi-stable 2p orbital that the electron is being removed from in N.