Name: ______________________________ Date: ____________________ Period: __________
CHAPTER 5 TEST REVIEW
1. Give the electron configurations for the following elements.
A.
B.
C.
D.
E.
F.
Mg 1s2 2s2 2p6 3s2
K 1s2 2s2 2p6 3s2 3p6 4s1
Ge 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
Fe 1s2 2s2 2p6 3s2 3p6 4s2 3d6
O 1s2 2s2 2p4
B 1s2 2s2 2p1
2. Give the orbital filling diagrams for the following elements.
Mg
A.
1s2 2s2 2p6 3s2
1s
B.
2s
C.
2s
D.
1s
2p
3s
3p
4s
1s2 2s2 2p4
O
1s
3s
1s2 2s2 2p6 3s2 3p6 4s1
K
1s
2p
2s
2p
1s2 2s2 2p1
B
2s
2p
3. Write the noble gas notation for the following elements.
Na: [Ne] 3s1
c)
V: [Ar] 4s2 3d3
b) F: [He] 2s2 2p5
d)
Mg: [Ne] 3s2
a)
4. Give the Lewis electron dot diagrams for the following elements.
A. Mg
Mg
D. He
He
B. K
K
E. O
O
C. Ge
Ge
F. B
B
5. Give the number of orbitals & maximum number of electrons in
each of the sublevels:
A. s sublevel
1 orbital
2 electrons
B. p sublevel
3 orbitals
6 electrons
C. d sublevel
5 orbitals
10 electrons
D. f sublevel
7 orbitals
14 electrons
6. How many valence for each of the following elements?
A. atomic number 7
Nitrogen (N) - 1s22s22p3 = 5 valence electrons
B. atomic number 17
Chlorine (Cl) - 1s22s22p63s23p5 = 7 valence electrons
C. atomic number 33
Arsenic (As) - 1s22s22p63s23p64s23d104p3 = 5 valence electrons
D. atomic number 5
Boron (B) - 1s22s22p1 = 3 valence electrons
7. Give the name of the element for each of the following electron
configurations.
A. 1s2 2s2 2p3
Nitrogen
B. 1s2 2s2 2p6 3s2 3p6 4s2 3d8 Nickel
C. 1s2 2s2 2p6 3s2 3p5
Chlorine
8. When given an orbital filling diagram for an element, be able to determine
which of the rules is violated: Example: What rule(s) are violated in the
following diagram?
1s
2s
2p
3s
3p
1s orbital should be filled before filling the 2s
(lower energy levels fill up first) Aufbau Principle is violated
- 2p orbital has two electrons with the same spin.
The two electrons should have opposite spins
(one up arrow and one down arrow) Pauli Exclusion Principle
violated
- In 3p orbital each orbital should get one electron
before a single orbital gets two Hund’s Rule is violated
9. How does light behave like a wave? How does light behave like a particle?
Light behaves like a wave: with a wavelength and frequency.
Electromagnetic waves have two fields: electric field and
magnetic field which are perpendicular (90 degrees) to each
other.
Light behaves like a particle: when high frequency light
encounters metal, a photon (particle of light) is released which
contains a specific quantity (quantum) of energy, calculated with
E = hʋ.
10. Sketch a beryllium-9 atom (Be) showing the proper number of p+, n0 and e-. Sketch
what happens to the electrons when the atom is energized (i.e., by electricity or flame).
Show where the photon is released.
A Be atom contains 4 protons (assume 5
neutrons) and 4 electrons.
When energized, electrons jump to higher
energy levels. When they jump back down,
they release energy in the form of a light
photon.
11. Define the following terms or equations:
a. wavelength, :
the distance between crests (or any two equivalent points) on
wave
b. atomic emission spectrum:
the set of frequencies of light emitted by the atoms of an
element
c. E = hʋ
Equation used to calculate the energy of a photon
developed by Planck
d. Electromagnetic Spectrum
The range of wavelengths of electromagnetic radiation
e. c = ʋ
Equation that relates the wavelength, frequency, and speed
of an electromagnetic wave
f. electromagnetic radiation:
a form of energy with wave-like behavior as it travels
through space
g. photon:
a particle of light energy that carries a quantum of energy
h. frequency
number of waves per second
i. the levels and sublevels of the electron cloud:
(1) Energy Level a 3-D region around
the nucleus of an atom
that describes an electrons probable location. There are 7
energy levels in an atom.
Each energy level can be broken down into
sublevels. The 4 sublevels are s, p, d, f
(2) Sublevel
Each sublevel contains orbitals. Each orbital can
only contain 2 electrons max.
(3) Orbital
12. When given an electromagnetic spectrum be able to identify which of a pair of waves
has a longer wavelength and a higher frequency.
a) Which waves have the longest wavelength?
Radio Waves: longer wavelength but lower frequency & energy.
b) Which waves have the shortest wavelength?
Gamma (Rays: shorter
wavelength, but higher frequency & energy.
c) Do visible light waves have a higher or lower frequency compared to ultraviolet?
ROYGBIV: Red has the lowest energy & frequency and longest
wavelength. Visible light has lower frequency compared to
ultraviolet.
d) Do x-rays have a longer or shorter wavelength compared to infrared waves?
X-rays have shorter wavelength compared to infrared.


 = wavelength;= frequency; = gamma
13. How are atomic emission spectra used to identify an element (think about how you
could identify the element lamps)?
Each element has its own unique emission spectra which can be used
like a “fingerprint” to identify the element.
14. Problem solving:
a. What is the wavelength of electromagnetic radiation having a frequency of
5.00×1012 Hz?
c = λѵ
Where c is speed of light (3.00×108 m/s) and
ѵ is frequency (5.00×1012 Hz)
λ = (3.00×108 m/s)  (5.00×1012 1/s)
λ = 6.00×10-5 m
b. What is the frequency of electromagnetic radiation having a wavelength of
3.33×10-8 m?
c = λѵ
Where c is speed of light (3.00×108 m/s) and
λ is wavelength (3.33×10-8 Hz)
c = λѵ
8
ѵ = (3.00×10 m/s)  (3.33×10-8 m)
ѵ = 9.00×1015 Hz or 9.00×1015 /s
c. Calculate the energy of a photon of violet light with a frequency of 6.8×1014 Hz.
E=hѵ
Where h is Planck’s Constant 6.626×10-34 J•s and
ѵ is frequency (6.8×1014 Hz)
E = (6.626×10-34 J•s) x (6.8×1014 Hz)
E= 4.5×10-19 J
d. Calculate the energy of a photon of ultraviolet light that has a frequency of
5.02×1020 Hz.
E=hѵ Where h is Planck’s Constant 6.626×10-34 J•s and
ѵ is frequency (5.02×1020 Hz)
E = (6.626×10-34 J•s) x (5.02×1020 Hz)
E= 3.33×10-13 J