Atomic Structure Flashcards
What are the 2 factors affecting the ionisation energy?
- nuclear charge
- shielding effect
Explain the trend in ionisation energy across the period
-As number of protons increases, nuclear charge increases.
-As successive electrons are added to the same outermost electron shell, the shielding
effect is approximately the same
-Effective nuclear charge increases.
-Forces of attraction between the nucleus and the outermost electron increases.
-More energy is needed to remove the outermost electron.
-Thus first IE generally increases across a period
Explain the trend in ionisation energy down the group.
- As number of protons increases, nuclear charge increases
- As number of principal quantum shell increases, shielding effect increases significantly.
-the outermost electron is further away from the nucleus
- attraction between the nucleus and the outermost electron decreases.
-less energy is needed to remove the outermost electron
- the first IE decreases down a group.
Explain for the decrease in IE between elements with ns^2 and ns^2np^1 configurations
-write down the electronic configuration of both elements
- less energy is needed to remove the 2p electron from a higher energy 2p subshell.
Explain the decrease in IE between group 15 and 16 elements
- group 15 elements have an electronic configuration of ns2 npx1 npy1 npz1
- group 16 elememts have an electronic configuration of ns2 npx2 npy1 npz1
- less energy is required to remove the paried npx electron as it experiences inter electronic repulsion.
Explain the IE between periods.
(take example to be Na and Ne)
- As Na has one more proton than Ne, nuclear charge increases
- As Na has one more principal quantum shell than Ne, shielding effect increases significantly.
- The outermost electron is further away from the nucleus in Na.
- Attraction between the nucleus and the outermost electron decreases in Na
- Less energy is required to remove the 3s electron in Na.
- The first IE decreases significantly from Ne to Na
Why do anions have a larger radii than their respective atoms?
- There are more electrons than protons in the anion
- The net attractive force on the valence lectrons by the nucleus decreases
How does id-id attraction come about?
-In an atom or molecule, the elctrons are constantly moving.
- At any moment, there can be an asymmertrical electron desnsity around a molecule.
- this results in an instantaneous dipole formed.
- this instantaneous dipole will induce another dipole on its neighbouring molecule.
- the electrostatic attraction between these fluctuating dipoles are known as id-id attraction.
How does pd-pd attraction arise?
- Polar molecules have a permamenent net dipole.
- The oppositely charged ends of the dipoles attract each other.
- This attraction is known as the pd-pd attraction.