Atomic Structure

Question 1

State the meaning of isoelectronic.

Answer 1

same number of electrons

Question 2

State the meaning of isotopic.

Answer 2

same number of protons

Question 3

State the meaning of isotonic.

Answer 3

same number of neutrons

Question 4

Define isotopes.

Answer 4

Isotopes are atoms with the same proton number but different neutron numbers. They have similar chemical properties but different physical properties.

Question 5

What is the unit for relative atomic mass?

Answer 5

There are no units for relative atomic mass.

Question 6

What is an electric field made up of?

Answer 6

It is set up by oppositely-charged electrodes.

Question 7

What is the reaction between electric fields and the charged particles?

Answer 7

The electric field exerts a force on charged particles and accelerates them towards the oppositely charged electrode and away from the similarly charged electrode.

Question 8

State the behaviour of uncharged particles in the electric field.

Answer 8

They are not attracted to any charged electrodes.

Question 9

What is the formula of angle of deflection?

Answer 9

k ✖ charge/mass, where k is a constant

Question 10

Define angle of deflection.

Answer 10

The angle between the undeflected path and the deflected path

Question 11

What happens to the angle of deflection when the charge of a particle increases? Explain.

Answer 11

The angle of deflection increases. An increased charge increases the attraction to the oppositely charged electrode.

Question 12

What happens to the angle of deflection when the mass of a particle increases? Explain.

Answer 12

The angle of deflection decreases. If all particles are travelling at the same speed, then particles with larger mass have higher momentum and undergo less deflection.

Question 13

State the Heisenberg Uncertainty Principle.

Answer 13

The more accurate the position of an electron is measured, the less accurate the momentum of the electron can be measured.

Question 14

State the Aufbau Principle.

Answer 14

Electrons occupy orbitals in terms of increasing energy level, with the lowest energy levels being filled first.

Question 15

State the Pauli Exclusion Principle.

Answer 15

An orbital cannot hold more than 2 electrons, and these 2 electrons must have opposite spins.

Question 16

State the Hund’s rule.

Answer 16

The orbitals of a subshell must be occupied singly with parallel spins before they can be occupied in pairs.

Question 17

Describe orbitals.

Answer 17

A region of space where electrons are likely to be found.

Question 18

State the relationship between the type of subshell and their energy levels.

Answer 18

Later subshells have greater energy per electron than earlier subshells. (e.g. 2p electron is more energetic than a 2s electron)

Question 19

State the relationship between the principle quantum number of subshells and their energy levels.

Answer 19

The subshell with higher principle quantum number has greater energy.

Question 20

State the maximum number of electrons that can be filled in each:
1) s subshell
2) p subshell

Answer 20

1) 2
A s subshell has 1 orbital
2) 6
A p subshell has 3 orbitals

Question 21

Write the electronic configuration of a potassium atom.

Answer 21

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1

Question 22

1s^2 2s^3
State which of the rules of electronic configuration is violated, and write the correct configuration.

Answer 22

1s^2 2s^2 2p^1
Pauli Exclusion Principle