Lecture 6

Question 1

d orbitals vs. s orbitals

Answer 1

d orbitals have fewer lobes close to the nucleus than (n+1)s

Question 2

electronic configuration pattern

Answer 2

(n+1)s orbital is lower in E than nd orbital (general observation)

Question 3

exceptions of pattern

Answer 3

• due to the energy of 4s orbital and 3d orbitals being very similar

Question 4

chromium exception

Answer 4

adopts electron configuration: 4s1 3d5 ; all electrons in d orbital are 1/2 filled in the same direction

Question 5

copper exception

Answer 5

adopts electron configuration: 4s1 3d10 ; all electrons in d orbital are filled

Question 6

energies in poly electron atoms

Answer 6

energy comes from core electrons as well as electrons in the same orbital shielding the positive nuclear charge

Question 7

valence electrons

Answer 7

largely determines chemistry of an atom

Question 8

ionization energy (IE)

Answer 8

• the energy needed to remove the highest energy electron from an atom in gas phase.
• indicates the electron electron repulsion and screening in poly electron atoms

Question 9

IE trends

Answer 9

1. IE increases from left to right

2. IE decreases down a group

Question 10

types of bonds used to find radii

Answer 10

• single (covalent) bond
• Van der Waals interaction
• ionic radii

Question 11

single (covalent) bonds

Answer 11

divide distance between the two nuclei by 2

Question 12

Van der Waals interaction

Answer 12

divide distance between the two nuclei by 2

Question 13

ionic radii

Answer 13

distance in a solid lattice measured by X-ray diffraction