Min. Exam 3

Question 1

Quantum numbers

Answer 1

Principal quantum number (n) - function of distance from nucleus, effective volume of electron orbital (any positive integer)
Orbital shape quantum number (l) - describes the general shape of the regions within which an electron moves (0 to n-1)
Magnetic quantum number (m) - restricts the orientation and shape of each type of orbital (-1 to +1)
Spin quantum number (s) - direction of spin of an electron in space (-1/2,+1/2)

Question 2

characteristic mass

Answer 2

sum of protons and neutrons in nucleus

Question 3

Coordination number

Answer 3

the number of closest neighbors that surround a specific ion in a crystal

Question 4

First ionization potential

Answer 4

the energy required to remove the most weakly held electron

Question 5

Metals/Nonmetals are:

Answer 5

metals are electron donors/Nonmetals are electron acceptors

Question 6

Elements want to reach a:

Answer 6

noble gas configuration

Question 7

Ionization potentials greatly increase when additional electrons need to be removed because:

Answer 7

there is greater pull per electron from the nucleus that needs to be overcome

Question 8

Energies of ionic bonds depend on:

Answer 8

1) Center to center spacing between ions 2) the product of their charges

Question 9

Bond strength is inversely proportional to:

Answer 9

its length. The stronger the bond, the harder the crystal.

Question 10

Ionic bonds are:

Answer 10

poor conductors of heat and electricity

Question 11

Covalent bonding is:

Answer 11

the sharing of electrons and the strongest of all chemical bonds

Question 12

Metallic bonding

Answer 12

electrons are shared and are to move through the metal

Question 13

Van der Waals bonding

Answer 13

a weak bond due to residual charges

Question 14

Hydrogen bonding

Answer 14

a weak, but numerous, dipole-dipole bond between hydrogen ion and a negatively charged ion