Download Atomic Structure Test Review Answer Key - Unit 1

Chapter 4 and 5 Test Review
1) Define the following:
a. Proton- Positive charge particle
in nucleus
b. Neutron-neutral charge particle
in nucleus
c. Electron- negative charge
particle outside nucleus
d. Atom- the smallest particle of
an element that retains the
properties of that element
e. Ion- Atom with a different
number of protons and
electrons
f. Isotope- two atoms of same
element that have differing
number of neutrons.
g. Nucleus- Center of atom.
Contains the protons and
neutrons.
h. mass number- sum of the
protons and neutrons in an
atom.
i. atomic number- indicates the
number of protons in an atom.
j. atomic mass- weighted average
of all of the different isotopes
of an element.
k. atomic orbital- region of high
probability of finding an
electron
l. aufbau principle- tendency of
electrons to enter orbitals of
lowest energy first
m. Hund’s Rule- every orbital in
a subshell is singly occupied
with one electron before any
one orbital is doubly
occupied, and all electrons in
singly occupied orbitals have
the same spin.
n. electron configuration- the
arrangement of electrons in an
atom.
o. ground state electron- electron
in its lowest energy state
p. Pauli exclusion principle- no
two electrons can occupy the
same place in an atom (cannot
have the same 4 quantum
numbers.)
q. Heisenberg uncertainty
principle- you cannot know
the location and velocity of an
electron at same time.
r. atomic emission spectrumfrequencies of light emitted
by an element.
s. Frequency- number of wave
cycles per second (s-1)
t. Wavelength- distance from
equivalent points on two
different waves (m)
u. Photon- discrete bundled of
electromagnetic energy
2) Know the theories or models presented by the following scientists.
a. Democritus- coined the term atomos
b. Dalton- 4 theories of atom
i. Atoms cannot be broken down
ii. Different elements have different masses
iii. Elements combine to form compounds
iv. Chemical reaction rearranges atoms. Cannot form atoms with partial elements.
c. Thompson- found electron. Chocolate chip cookie model of atom.
d. Rutherford- found nucleus
e. Bohr- Planetary model of the atom. Rings are fixed energy levels.
f. (Know what the cloud model states)
3)
Using the periodic table fill in the spaces below.
Atomic #
Symbol
Mass #
Charge
# Protons
# Neutrons
# Electrons
7
+1
3
4
2
N
14
-3
7
7
10
Co
59
0
37
32
27
I
127
-1
53
74
54
Au
118
.
+3
79
118
76
3
7
7
14
27
53
79
Li
59
127
118
4) Explain what happens when an atom absorbs energy. Explain in terms of what the electrons do.
-
Electrons go from being in their ground state to being in their excited state. Immediately they
fall back down to their ground state and emit the energy they absorbed.
5) What is the speed of light? How does it compare with the speed of other electromagnetic waves?
-
3.00x108 m/s…all electromagnetic waves have the exact same speed.
6) What determines the color of light? How do the colors of light change with frequency and
wavelength?
-
Color of light is determined by either the frequency or the wavelength. As frequency of
wave goes up you move from red to violet. As wavelength goes up you move from violet to
red.
7) Describe what is meant by atomic emission spectrum. Draw a picture if necessary.
Energy given off by an atom as it releases absorbed energy.
8) What is the frequency of ultraviolet light with wavelength 2.94
-
10
m? (c = 3.00
10 m/s)
F= c ÷ λ= 3.00x108 ÷2.94 x10-8 = 1.02 x1016 Hz
9) What is the wavelength of gamma ray electromagnetic radiation with a frequency of 2.73
Hz? (c = 3.00 10 m/s)
10
-
λ= c ÷ F = 3.00x108 ÷ 2.74 x1020 = 1.09 x10-12 m
10) Consider an element Z that has two naturally occurring isotopes with the following percent
abundances: the isotope with a mass number of 16.0 is 35.0% abundant; the isotope with a mass
number of 21.5 is 65.0% abundant. What is the average atomic mass for element Z?
(16*.35) + (21.5*.65) = 19.6 amu
11) Write the full electron configuration for:
a. Potassium (K)
- 1s2 2s2 2p6 3s2 3p6 4s2
b. Cadmium (Cd)
- 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10
c. Phosphorous (P)
- 1s2 2s2 2p6 3s2 3p3
d. Zirconium (Zr)
- 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2
12) Write the abbreviated electron configuration for:
a. Cesium (Cs)
- [Xe] 6s1
b. Hafnium (Hf)
- [Xe] 6s2 4f14 5d2
c. Radium (Ra)
- [Rn] 7s2
d. Niobium (Nb)
- [Kr] 5s2 4d3
13) Determine the identity of the element using the electron configuration:
a. 1s2 2s2 2p6 3s2 3p6 4s2 3d7
- Nickel
b. [Kr] 5s2 4d10 5p3
- Antimony
c. [Ne] 3s2
- Magnesium
d. [Xe] 6s2 4f14 5d7
- Iridium
14) Determine the 4 quantum numbers for the outermost electrons for:
a. Cesium (Cs)
N=5
l=0
ml=0
ms=+1/2
b. Hafnium (Hf)
N=5
l=1
ml=0
ms=+1/2
Radium (Ra)
N=7
l=0
ml=0
ms=(-)1/2
Niobium (Nb)
N=4
l=1
ml=1
ms=+1/2
15) What is meant by the term atomic orbital?
a. What shape is an s orbital?
-Spherical
b. What shape is a p orbital?
- Pear or dumbbell
c. How many s orbitals are there?
-1
d. How many p orbitals are there?
-3
e. How many d orbitals are there?
-5
f. How many f orbitals are there?
-10