Chapter 3

Question 1

the quantization of the
energy levels in Bohr’s
model can be explained
by

Answer 1

the wavelike behavior
of the electrons

Question 2

The wavelike behavior of
electrons was confirmed
experimentally by the

Answer 2

double slit experiment

Question 3

An orbital is

Answer 3

a region where an
electron is most probable to
reside.

Question 4

An orbital is defined by

Answer 4

4 quantum numbers

Question 5

What are the 4 quantum numbers

Answer 5

n, l, ml, ms

Question 6

What is n

Answer 6

The principal quantum number n tells you the energy level of an electron

Question 7

1. If an electron transitions to a higher
   energy level (n)…
2. If an electron transitions to a lower
   energy level….

Answer 7

1. energy is absorbed
   in the form of a photon.
2. energy is released in the
   form of a photon.

Question 8

l specifies

Answer 8

the shape of the orbital
(0…n-1)

Question 9

l = 0 corresponds
l = 1 corresponds
l = 2 corresponds
l = 3 corresponds

Answer 9

to s orbitals (sphere)
to p orbitals (dumbells)
to d orbitals
to f orbitals

Question 10

A radial node is

Answer 10

a value where the odds of finding an electron is 0

Question 11

What is ml

Answer 11

specifies the spatial
orientation of a orbital.
(-l…l)

Question 12

The number of
possible orbitals in the same
subshell is

Answer 12

2l + 1.

Question 13

Ms is

Answer 13

Spin quantum number : its the direction of the quantum “spinning”
of the electron
(+1/2, -1/2)

Question 14

Electron configuration of ions

Main group elements:

Answer 14

the electrons that were added last are
the first electrons removed

Question 15

Electron configuration of ions

Transition metals:

Answer 15

The highest ns electrons are lost first, then the (n – 1)d or (n – 2)f electrons are removed.

Question 16

The electrons occupying the outermost shell orbital(s) are

Answer 16

valence electrons

Question 17

those occupying the inner shell orbitals are called

Answer 17

core electrons

Question 18

Electrons experience two conflicting
forces:

Answer 18

• Attraction to the nucleus
• Repulsion by other electron

Question 19

The repulsion by other electrons is
called

Answer 19

shielding

Question 20

Atoms and ions that have the same electronic configuration are said to be

Answer 20

isoelectronic

Question 21

The size of an atom can be defined by its

Answer 21

Covalent Radius

Question 22

More shielding means

Answer 22

the outer electrons are less tightly held by the nucleus, so the atom becomes bigger

Question 23

Fewer shields mean

Answer 23

the outer electrons are held tighter by the nucleus, so the atom becomes smaller

Question 24

Zeff =

Answer 24

= Z – shielding

Question 25

the atomic size

Answer 25

• increases down a group: there are more core electrons blocking the nucleus’s pull
• decreases across a period: the nucleus pulls more strongly on the outer electrons, without much extra shielding

Question 26

For atoms or ions that are isoelectronic the size is determined by

Answer 26

the number of protons
determines the size (more protons = smaller radius)

Question 27

The energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called

Answer 27

its first ionization energy (IE1)

Question 28

The energy required to remove the second most loosely bound electron is
called

Answer 28

the second ionization energy (IE2)

Question 29

Ionization energy:

Answer 29

• decreases down a
  group
• increases across a
  period

Question 30

Ionization energy: Deviation #1:

Answer 30

IE1 decreases when l
increases

Question 31

Ionization energy: Deviation #2:

Answer 31

IE1 decreases when a
subshell becomes more
than one-half filled

Question 32

The electron affinity (EA) is the

Answer 32

energy change for the process of adding an electron to a gaseous atom to form an anion

Question 33

EAs tend to become

Answer 33

more negative across a period (with increasing Zeff)

Question 34

EA Deviation #1:

Answer 34

group 2 (2A)
High positive energy

Question 35

EA Deviation #2:

Answer 35

group 15 (5A)
low negative energy

Question 36

EA Deviation #3:

Answer 36

noble gases
positive energy