Atomic Structure

Question 1

How does energy relate to shell number?

Answer 1

The further the energy level is from the nucleus, the higher its number (n) and the higher its energy

Question 2

Atomic orbital

Answer 2

An atomic orbital represents a region of space where there is a high probability of finding an electron

Question 3

Heisenberg’s uncertainty principle

Answer 3

Not possible to know, at the same time, the exact position and momentum of an electron

we can only state the probability that an electron will be somewhere in a given region of space.

For an atomic orbital, the probability stated is usually 95%.

Question 4

Pauli exclusion principle

Answer 4

Simply put, two electrons can only occupy the same atomic orbital if they have opposite spins

Question 5

In what way is an electron filled in the Aufbau principle

Answer 5

The 1s sub-level has the lowest energy, therefore, it is filled first.

Question 6

Which Orbitals have more energy, S or P?

Answer 6

Within a given main energy level, s orbitals are of lower energy than p orbitals and fill first

Question 7

What are the energy levels with a sub-level like?

Answer 7

The atomic orbitals within a sub-level are of equal energy (known as degenerate orbitals). This includes the three p orbitals in the 2p, 3p and 4p sub-levels and the five d orbitals in the 3d sub-level.

Question 8

Are there overlaps

in the Aufbau principle?

Answer 8

Yes,
There is an overlap between the 3d and 4s sub-levels. This means that the 4s sub-level is of lower energy and fills before the 3d sub-levels

Question 9

Order of the Aufbau principle?

Answer 9

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s

Question 10

Is there an overlap in the order of sub-levels?

Answer 10

Yes,
There is an overlap between the 3d and 4s sub-levels. This means that the 4s sub-level is of lower energy and fills before the 3d sub-levels

Question 11

Exceptions to the Aufbau Principle

Answer 11

Chromium: (24) 1s2 2s2 2p6 3s2 3p6 4s1 3d5

Copper: (29) 1s2 2s2 2p6 3s2 3p6 4s1 3d10

Question 12

Frequency and wavelength equation

Answer 12

c = vλ

Question 13

Explain why some elements have several isotopes and others like fluorine have only one isotope?

Answer 13

The other Isotopes of Monoisotopic elements are unstable

The large elements are unstable

An increasing number of neutrons is required to stabilize a nucleus that is packed with protons so heavier elements have more isotopes

Fluorine is not a large element

Question 14

What is the name of the instrument used to distinguish between 14N and 15N?

What are the two characteristic differences that we see?

Answer 14

The Mass Spectrometer

N14 AND N15 will have different abundances and different mass/charge ratios in the mass Spectrum of N.

Question 15

Predict and explain, giving two reasons, how the first ionization energy of 15N would be different to 14N?

Answer 15

The ionization energy of both Isotopes of N would be the same

Neutrons don’t affect Ionization energy

They still have the same electronic configuration

Question 16

Explain the difference between a continuous spectrum and a line spectrum?

Answer 16

A continuous wavelength shows all wavelengths in a spectrum

A line Spectrum doesn’t show all the wavelengths

Question 17

The shape of a 1S atomic orbital?

Answer 17

Circle

Question 18

The shape of a 2P atomic Orbital?

Answer 18

Infinity sign

Question 19

Describe the relationship between colour, energy, frequency and wavelength in the visible spectrum?

Answer 19

The Visible Spectrum ranges from Red to Blue/Violet Light

From Red to Blue, the energy and frequency increases but the wavelength decreases

Question 20

What are the four shell orbitals in order of increasing energy?

Answer 20

S,P,D,F

Question 21

What are the number of atomic orbitals in S,P,D,F?

Answer 21

4S = 1
4P = 3
4D= 5
4F = 7

Question 22

Relative Atomic Mass?

Answer 22

Average mean of masses of all isotopes of an element relative to the element

Question 23

Mass Spectrometry?

Answer 23

Ionization: sample bombarded with high-energy or high-speed electrons

Acceleration: electric fields/ oppositely charged plates

Deflection: magnet