Models of Multielectron Atoms

Question 1

What is the size of an orbital equivalent to?

Answer 1

the average distance of an electron from the nucleus

Question 2

Quantum number n

Answer 2

principle quantum number; determines size; orbital size increases as n increases; impacts energy

Question 3

Quantum number l

Answer 3

orbital quantum number; number of angular nodes = l; determines the shape; values range from 0 to n-1; impacts energy when electron repulsion is present

Question 4

What l value does the p orbital correspond to?

Answer 4

1

Question 5

Quantum number ml

Answer 5

magnetic quantum number; specifies the spatial orientation of an orbital; does not affect E

Question 6

Subshell

Answer 6

Orbitals with the same value n and l

Question 7

Nodes

Answer 7

where a wave function changes signs; probability of finding electrons at nodes is zero; more nodes = higher energy

Question 8

Radial nodes

Answer 8

occur at specific values of r and are spherical

Question 9

Angular nodes

Answer 9

non spherical nodes (often planes or cones)

Question 10

Quantum number ms

Answer 10

spin quantum number; describes electrons magnetic field; either .5 or -.5

Question 11

Degenerate

Answer 11

orbitals with same energy levels

Question 12

Pauli exclusion principle

Answer 12

if electrons have the same n, l, and ms, then their ml must be different from each other (no 2 electrons in an atom can have the same quantum numbers)

Question 13

Hund’s rule

Answer 13

lowest energy configuration has max number of unpaired electrons with parallel spins

Question 14

Aufbau principle

Answer 14

process of filling electrons into orbitals from lowest E occupancy up

Question 15

Valence electrons

Answer 15

occupy the outermost orbitals

Question 16

Core electrons

Answer 16

occupy inner orbitals

Question 17

Shell

Answer 17

n value