Lecture 7

Question 1

d and f orbitals

Answer 1

less effective at screening nuclear charge

Question 2

B and Al orbitals

Answer 2

radius Al > radius of B

Question 3

Al and Ga orbitals

Answer 3

has d-orbital contraction, therefore radius of Al > radius of Ga

Question 4

d-orbital contraction

Answer 4

causes radii to decrease as an effect of having full d orbitals on period 4 elements

Question 5

f-orbita/lanthanide contraction

Answer 5

causes radii increase to be smaller as an effect of full f orbitals on lanthanides

Question 6

Mulliken electronegativity

Answer 6

ability of an atom to attract electrons, depending on IE and e- affinity

Question 7

Mulliken electronegativity trends

Answer 7

• elements to the left have low electronegativities, therefore elements will give up electrons in rxns
• electronegativity increases left to right
• electronegativity increases up a group, since valence e-‘s are in lower energy (less screened orbitals are above)

Question 8

noble gases

Answer 8

filled valence shells, therefore a high Zeff and will not want to react (extremely stable)

Question 9

reactivity

Answer 9

• can be predicted with electronegativity

- hydrogen can be acidic (protic) or basic (hydridic)

Question 10

radii of charged atoms

Answer 10

• halides will accept an e- to make anions, which have a larger radii than neutral atoms
• radii anions and dianions increase down a group
• single valence e-s in s orbital will donate an e- to make cations, which have a smaller radii than neutral atoms
• radii cations decrease from left to righ

Question 11

anions

Answer 11

adds e-s to the outer valence orbital (most favourable to elements on the rights) to form inert gas configuration

Question 12

cations

Answer 12

donates e-s from orbital (most favourable to elements on the left) to form inert gas configuration