Chapter 8

Question 1

A property of an element that is predictable based on an element’s position in the periodic table

Answer 1

Periodic property

Question 2

A notation that shows the particular orbitals that are occupied by electrons in an atom

Answer 2

Electron configuration

Question 3

The lowest energy state for electron configuration

Answer 3

Ground state

Question 4

A diagram that gives information similar to an electron configuration but symbolizes an electron as an arrow in a box representing an orbital, with the arrow’s direction denoting the electron’s spin

Answer 4

Orbital diagram

Question 5

The principle that no two electrons in an atom can have the same for quantum numbers

Answer 5

Pauli exclusion principle

Question 6

A term describing two or more electron orbitals with the same value of n that have the same energy

Answer 6

Degenerate

Question 7

The potential energy of two charged particles depends on their charges (q1 and q2) and on their separation (r)

Answer 7

Coulomb’s law

Question 8

The effect on an electron of repulsion by electrons in lower-energy orbitals that screen it from the full effects of nuclear charge

Answer 8

Shielding

Question 9

The actual nuclear charge experienced by an electron, defied as the charge of the nucleus plus the charge of the shielding electrons

Answer 9

Effective nuclear charge (Zeff)

Question 10

The phenomenon of some higher-level atomic orbitals having significant amounts of probability within the space occupied by orbitals of lower energy level. For example: the 2s orbital penetrates into the 1s orbital.

Answer 10

Penetration

Question 11

The principle that indicates the pattern of orbital filling in an atom

Answer 11

Aufbau principle

Question 12

The principle stating that when electrons fill degenerate orbitals, they first fill them singly with parallel spins

Answer 12

Hund’s rule

Question 13

Those electrons that are important in chemical bonding. For main-group elements, the valence electrons are those in the outermost principle energy level

Answer 13

Valence electrons

Question 14

Those electrons in a complete principal energy level and those in complete d and f sublevels

Answer 14

Core electrons

Question 15

Defined as one-half the distance new\tween the centers of adjacent, nonbonding atoms in a crystal

Answer 15

van der Waals radius (nonbonding atomic radius)

Question 16

Defined in nonmetals as one-half the distance between two atoms bonded together, and in metals as one-half the distance between two adjacent atoms in a crystal of the metal

Answer 16

Covalent radius (bonding atomic radius)

Question 17

The radius of an atom when it is bonded to another atom and is always smaller than the van der Waals radius

Answer 17

Atomic radius

Question 18

The state of an atoms or ion that contains unpaired electrons and is, therefore, attracted by an external magnetic field.

Answer 18

Paramagnetic

Question 19

The state of an atom or ion that contains only paired electrons and is, therefore, slightly repelled by an external magnetic field.

Answer 19

Diamagnetic

Question 20

The energy required to remove an electron from an atom or ion in its gaseous state

Answer 20

Ionization energy

Question 21

The energy change associated with the gaining of an electron by an atom in its gaseous state

Answer 21

Affinity electron