CHEMISTRY WKST KEY: CH. 11 REVIEW
1)
wavelength
crest
trough
node
amplitude
2)
a) λ → wavelength
3)
Frequency and wavelength of a wave are inversely proportional. For electromagnetic waves, the product of the
wavelength and frequency is equal to the speed of light (3.00 x 10 8 m/s).
4)
a) red
5)
The bright-line spectrum is produced by photons of different energies. These photons come from different
energies being emitted by the electrons within atoms when they go from a higher energy level to a lower energy
level.
6)
Bohr’s model only worked for hydrogen. Also, Bohr’s electron should end up in the nucleus but doesn’t.
7)
c= λν
λ=
b) red
b) ν → frequency
c) blue
3.00 x 108 ms
c
=
= 9.22 x 10-11 m
ν 3.253 x 1018 Hz
NOTE: If you need to get the wavelength in nm, then multiply the answer in meters by 10 9 nm:
9.22 x 10-11 m (
109 nm
) = 0.0922 nm
1m
8)
When an excited electron in an atom moves to a lower energy level, it releases energy in the form of photons.
These photons produce light of a specific energy and wavelength.
9)
-electrons travel in circular orbits
-energy levels increase in energy as they move farther away from the nucleus
-electrons gain energy to move to higher energy levels (they become excited)
-electrons lose energy in the form of a photon when moving to a lower energy level
-electrons are quantized
10)
Schrödinger postulated that if light can have dual properties of waves and particles, then why not electrons. He
stated that electrons travel in standing waves.
11)
Quantum mechanics is based on a 90% probability that electrons are in specific orbitals.
12)
Electrons being quantized means they exist only at discrete levels of energy.
CHEMISTRY WKST KEY: CH. 11 REVIEW
p. 2
13)
a) d
b) d
c) p
d) f
e) f
f) s
14)
a) 7
b) 4
c) 1
15)
a) 6
b) 18
c) 14
16)
2
17)
The two electrons have opposite spins to allow them to remain close to each other, such as in an orbital.
18)
The 2p and 4p orbitals have the same shape and each orbital can hold up to 2 electrons. The 2p and 4p orbitals
are different in that the 4p orbitals are larger and have more energy than the 2p orbitals.
19)
a)
C → [He]
↑↓
2s
↑
b)
Fe → [Ar]
↑↓
4s
↑↓ ↑
a)
Cu →
1s2 2s2 2p6 3s2 3p6 4s1 3d10
b)
Rb →
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
c)
Se2− →
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
d)
As5+ →
1s2 2s2 2p6 3s2 3p6 3d10
a)
Eu →
[Xe] 6s2 5d1 4f6
b)
Sb3+ →
[Kr] 5s2 4d10
c)
I− →
[Kr] 5s2 4d10 5p6
d)
W→
[Xe] 6s1 4f14 5d5
e)
In3+ →
[Kr] 4d10
f)
Hf →
[Xe] 6s2 4f14 5d2
a)
Se →
4s2 4p4
b)
Ba →
6s2
c)
Xe →
5s2 5p6
d)
Pb4+ →
5s2 5p6 5d10
e)
O2− →
2s2 2p6
20)
21)
22)
↑
2p
↑ ↑
3d
↑
CHEMISTRY WKST KEY: CH. 11 REVIEW
b) He → 2
c) K → 1
p. 3
23)
a) Ne → 8
d) Ge → 4
24)
The electrons in the valence shell are the electrons involved in chemical reactions. Electrons are lost and gained
through the valence shell.
25)
Elements form the ion they form to become like a noble gas. Metals will lose electrons to do this whereas
nonmetals will gain electrons. Those elements that are in the higher energy levels will instead generally end up
with filled sublevels rather than be exactly like a noble gas.
26)
The 4s sublevel fills before the 3d sublevel because the 4s has less energy than the 3d sublevel. The 4f sublevel
fills before the 5d sublevel because the 4f has less energy than the 5d sublevel.
27)
These elements have the given electron configuration rather than what we may think because this configuration is
more stable.
28)
a) S → ground
b) Sc → excited
c) Ne → excited
d) Ti → impossible; the 2d sublevel does not exist
e) Ge → impossible; the 3p sublevel can only hold up to 6 electrons
f)
I → ground
29)
Elements in the same group have similar properties because they have the same number of valence electrons.
30)
Atoms form ions to become more stable—they lose energy when becoming ions.
31)
a) O
e) Ca
b) F
f)
c) Br
g) Ba
d) Au
h) Clˉ
32)
33)
S2ˉ Cl1ˉ K1+ Ca2+
size increases
Rb
CHEMISTRY WKST KEY: CH. 11 REVIEW
34)
35)
a) 1
c) 3
e) 8
b) 5
d) 2
f)
p. 4
7
a) metals
b) nonmetals
c) nonmetals
d) nonmetals
36)
SeCl4 and SeCl6
37)
a)
The atoms get smaller going across the period left to right due to increased nuclear charge on electrons in
the same valence shell.
b)
Atoms get larger going down the groups due to electrons entering larger energy levels and increased
shielding effect by core electrons on the valence shell.
38)
Fluorine
39)
Chemical reactions take place in the valence shell.
40)
a) Fe → 26+
b) Xe → 54+
c) Lr → 103+