Atomic Structure Flashcards
State the meaning of isoelectronic.
same number of electrons
State the meaning of isotopic.
same number of protons
State the meaning of isotonic.
same number of neutrons
Define isotopes.
Isotopes are atoms with the same proton number but different neutron numbers. They have similar chemical properties but different physical properties.
What is the unit for relative atomic mass?
There are no units for relative atomic mass.
What is an electric field made up of?
It is set up by oppositely-charged electrodes.
What is the reaction between electric fields and the charged particles?
The electric field exerts a force on charged particles and accelerates them towards the oppositely charged electrode and away from the similarly charged electrode.
State the behaviour of uncharged particles in the electric field.
They are not attracted to any charged electrodes.
What is the formula of angle of deflection?
k ✖ charge/mass, where k is a constant
Define angle of deflection.
The angle between the undeflected path and the deflected path
What happens to the angle of deflection when the charge of a particle increases? Explain.
The angle of deflection increases. An increased charge increases the attraction to the oppositely charged electrode.
What happens to the angle of deflection when the mass of a particle increases? Explain.
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.
State the Heisenberg Uncertainty Principle.
The more accurate the position of an electron is measured, the less accurate the momentum of the electron can be measured.
State the Aufbau Principle.
Electrons occupy orbitals in terms of increasing energy level, with the lowest energy levels being filled first.
State the Pauli Exclusion Principle.
An orbital cannot hold more than 2 electrons, and these 2 electrons must have opposite spins.
State the Hund’s rule.
The orbitals of a subshell must be occupied singly with parallel spins before they can be occupied in pairs.
Describe orbitals.
A region of space where electrons are likely to be found.
State the relationship between the type of subshell and their energy levels.
Later subshells have greater energy per electron than earlier subshells. (e.g. 2p electron is more energetic than a 2s electron)
State the relationship between the principle quantum number of subshells and their energy levels.
The subshell with higher principle quantum number has greater energy.
State the maximum number of electrons that can be filled in each:
1) s subshell
2) p subshell
1) 2
A s subshell has 1 orbital
2) 6
A p subshell has 3 orbitals
Write the electronic configuration of a potassium atom.
1s^2 2s^2 2p^6 3s^2 3p^6 4s^1
1s^2 2s^3
State which of the rules of electronic configuration is violated, and write the correct configuration.
1s^2 2s^2 2p^1
Pauli Exclusion Principle
