Electronic Structure of Atoms

Question 1

Electron Configurations

Answer 1

Describe where electrons are located around the nucleus of an atom.

Question 2

s,p,d,f

Answer 2

Shows which block the atom is on, this depends on the angular momentum (l).

Question 3

n

Answer 3

Principal Number

Question 4

How many electrons can s hold?

Answer 4

2 Electrons

Question 5

How many electrons can p hold?

Answer 5

6 Electrons

Question 6

How many electrons can d hold?

Answer 6

10 Electrons

Question 7

How many electrons can f hold?

Answer 7

14 Electrons

Question 8

Orbital Diagrams

Answer 8

Electrons are represented with half arrows. One point up (+1/2) and one pointing down (-1/2). They are arranged in order of increasing energy.

Question 9

Aufbau Principal

Answer 9

Electrons should fill lower-energy orbitals before filling higher-energy ones.

Question 10

Hund’s Rule

Answer 10

Fill all empty orbitals with electrons before doubling the orbitals with a second electron.

Question 11

What are condensed electron configurations?

Answer 11

Taking the core electrons and using a stable atom to represent it with the valence electrons.

Question 12

Valence Electrons

Answer 12

Outer-shell (highest n) electrons.

Question 13

Core Electrons

Answer 13

Inner (lower n) electrons.

Question 14

How to determine number of valence electrons from group 1A and 2A?

Answer 14

Group # = # of valence electrons.

Question 15

Anions (-) for electron configuration?

Answer 15

To make anion add electrons using filling rules.

Question 16

Cation (+) for electron configuration?

Answer 16

To make cation take away electrons from highest n first. This is important for transition metals.

Question 17

Isoelectric Atoms and Ions

Answer 17

When they have the same number of electrons (same electron configuration).

Question 18

Z sub eff

Answer 18

Amount of positive charge from the nucleus that an electron “feels”.

Question 19

How to calculate Z sub eff

Answer 19

Z - Shielding