Chemistry I Summative #4 Study Guide
Matching
Match the following terms with the correct definition. There is one extra term that will not match any of the
definitions.
a. alpha particles
b. nucleons
c. gamma rays
d. isotopes
e. beta particles
f. half-life
____
____
____
____
____
1. Negatively charged particles (electrons) emitted from the nucleus of a radioactive element
2. Positively charged particles emitted from the nucleus of an atom during radioactive decay; also called a
helium nucleus
3. Atoms of the same element that have different numbers of neutrons and different mass numbers
4. Photons emitted spontaneously by a radioactive substance
5. Collectively, the protons and neutrons in the nucleus
Match the following terms with the correct definition. There is one extra term that will not match any of the
definitions.
a. valence electrons
b. energy levels
c. ions
d. oxidation number
e. electronegativity
f. octet rule
____ 6.
____ 7.
____ 8.
____ 9.
____ 10.
The location of electrons around the nucleus of an atom
The electrons involved in chemical bonding
The number of electrons which are lost, gained, or shared when bonding occurs
Atoms that are positively or negatively charged
Most atoms need eight electrons to be stable
Match each item with the correct statement below.
a. atomic orbital
d. ground state
b. aufbau principle
e. Pauli exclusion principle
c. electron configuration
f. Heisenberg uncertainty principle
____
____
____
____
____
____
11.
12.
13.
14.
15.
16.
region of high probability of finding an electron
states the impossibility of knowing both velocity and position of a moving particle at the same time
lowest energy level
tendency of electrons to enter orbitals of lowest energy first
arrangement of electrons around atomic nucleus
each orbital has at most two electrons
Match each item with the correct statement below.
a. electronegativity
f. periodic law
b. ionization energy
g. cation
c. atomic radius
d. metal
e. transition metal
____
____
____
____
____
____
____
____
____
____
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
h. period
i. group
j. electrons
horizontal row in the periodic table
vertical column in the periodic table
A repetition of properties occurs when elements are arranged in order of increasing atomic number.
type of element that is a good conductor of heat and electric current
type of element characterized by the presence of electrons in the d orbital
one-half the distance between the nuclei of two atoms when the atoms are joined
type of ion formed by Group 2A elements
subatomic particles that are transferred to form positive and negative ions
ability of an atom to attract electrons when the atom is in a compound
energy required to remove an electron from an atom
Problem
27. Calculate the maximum number of electrons that can exist in the n = 4 level. Account for the
numbers of electrons within each sublevel of the principal level.
28. List the number of protons, neutrons, and electrons in
C.
29. Write the electron configuration for chromium.
30. How many energy levels would be completely filled by a neutral atom of fluorine? How many
electrons would be left over?
31. Explain Louis de Broglie's contribution to the quantum model of the atom.
32. How does the figure below illustrate Hund's rule?
33. How does the figure above illustrate the Pauli exclusion principle?
34. Determine the number of electrons in an atom of iridium.
35. What is the atomic number for an element with 41 neutrons and a mass number of 80?
36. What is the mass number for an oxygen atom that has 10 neutrons in its nucleus?
37. How many protons are present in the nuclei of the three known isotopes of hydrogen?
38. How many electrons are in the highest occupied energy level of a neutral chlorine atom?
39. How many electrons are in the highest occupied energy level of a neutral strontium atom?
40. How many electrons are in the highest occupied energy level of copper?
41. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5?
42. Explain how Dalton improved upon atomic theory more than 2000 years after Democritus’s hypotheses about
atoms.
43. What observations by Rutherford led to the hypothesis that atoms are mostly empty space, and that almost all
of the mass of the atom is contained in an atomic nucleus?
44. Explain how the atoms of one element differ from those of another element.
45. In what way are two isotopes of the same element different? Explain why isotopes of the same element have
the same chemical behavior.
46. Explain why the 4s sublevel fills before the 3d sublevel begins to fill as electrons are added.
47. Describe the different principles that govern the building of an electron configuration.
48. What is the quantum mechanical model?
49. Explain what is meant by the Heisenberg uncertainty principle.
50. Describe the trends in the atomic size of elements within groups and across periods in the periodic table.
Provide examples.
51. Describe the trends in first ionization energy within groups and across periods in the periodic table. Provide
examples.
52. Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the
atoms from which they are formed. Explain why this is so.
53. Describe the trends in electronegativity within groups and across periods in the periodic table. Provide
examples.
Chemistry I Summative #4 Study Guide
Answer Section
MATCHING
1.
2.
3.
4.
5.
ANS:
ANS:
ANS:
ANS:
ANS:
E
A
D
C
B
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
DIF:
DIF:
DIF:
DIF:
DIF:
basic
basic
basic
basic
basic
REF:
REF:
REF:
REF:
REF:
chapter 22 | section 22.1
chapter 22 | section 22.1
chapter 22 | section 22.1
chapter 22 | section 22.1
chapter 22 | section 22.1
6.
7.
8.
9.
10.
ANS:
ANS:
ANS:
ANS:
ANS:
B
A
D
C
F
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
DIF:
DIF:
DIF:
DIF:
basic
basic
basic
basic
REF:
REF:
REF:
REF:
chapter 19 | section 19.1
chapter 19 | section 19.1
chapter 19 | section 19.1
chapter 19 | section 19.1
11. ANS:
OBJ:
12. ANS:
OBJ:
13. ANS:
OBJ:
14. ANS:
OBJ:
15. ANS:
OBJ:
16. ANS:
OBJ:
A
5.1.2
F
5.1.3
D
5.1.3
B
5.1.3 | 5.2.1
C
5.2.1
E
5.2.1
PTS: 1
DIF: L1
REF: p. 130 | p. 131
PTS: 1
DIF: L1
REF: p. 145
PTS: 1
DIF: L1
REF: p. 142
PTS:
STA:
PTS:
STA:
PTS:
STA:
1
SC.HS.1.1.1
1
SC.HS.1.1.1
1
SC.HS.1.1.1
DIF: L1
REF: p. 133
DIF: L1
REF: p. 133
DIF: L1
REF: p. 134
17. ANS:
OBJ:
18. ANS:
OBJ:
19. ANS:
OBJ:
20. ANS:
OBJ:
21. ANS:
OBJ:
22. ANS:
OBJ:
23. ANS:
OBJ:
24. ANS:
OBJ:
25. ANS:
H
6.1.1
I
6.1.1
F
6.1.1
D
6.1.3
E
6.2.2
C
6.3.1
G
6.3.2
J
6.3.2
A
PTS:
STA:
PTS:
STA:
PTS:
STA:
PTS:
1
DIF: L1
SC.HS.1.1.1| SC.HS.1.1.4
1
DIF: L1
SC.HS.1.1.1| SC.HS.1.1.4
1
DIF: L1
SC.HS.1.1.1| SC.HS.1.1.4
1
DIF: L1
PTS: 1
DIF: L1
REF: p. 157
REF: p. 157
REF: p. 157
REF: p. 158
REF: p. 166
PTS: 1
DIF: L1
STA: SC.HS.1.1.1| SC.HS.1.1.5
PTS: 1
DIF: L1
REF: p. 170
PTS: 1
DIF: L1
REF: p. 172
PTS: 1
DIF: L1
REF: p. 177
REF: p. 172
OBJ: 6.3.3
26. ANS: B
OBJ: 6.3.3
PTS: 1
DIF: L1
REF: p. 173
PROBLEM
27. ANS:
For n = 4, there are four sublevels: s, p, d, and f, with one s orbital, three p orbitals, five d orbitals,
and seven f orbitals, for a total of 1 + 3 + 5 + 7 = 16 orbitals. Each orbital can hold a maximum of
two electrons, so the maximum total number of electrons is 16  2 = 32 electrons.
PTS: 1
OBJ: 4D 4.g
28. ANS:
protons: 6; neutrons: 7; electrons: 6
PTS: 1
DIF: L2
OBJ: 4.3.1 | 4.3.2
29. ANS:
1s 2s 2p 3s 3p 3d 4s
REF: p. 110 | p. 111
PTS: 1
OBJ: 5.2.2
30. ANS:
REF: p. 134 | p. 135 | p. 136
DIF: L3
The neutral fluorine atom has one filled energy level and seven electrons left over.
PTS: 1
DIF: advanced
REF: chapter 18 | section 18.3
31. ANS:
If light has a particle nature, de Broglie reasoned, could particles have a wave nature? He compared the
behavior of Bohr's quantized electron orbits to the known behavior of waves. Finally, he hypothesized that
electrons are confined to the space around an atomic nucleus and that electron waves exist only at specific
energies.
PTS: 1
DIF: II
REF: 2
OBJ: 1
32. ANS:
According to Hund's rule, the arrangement of electrons with the maximum number of unpaired electrons is
the most stable arrangement.
PTS: 1
DIF: III
REF: 3
OBJ: 2
33. ANS:
According to the Pauli exclusion principle, no two electrons can have the same set of four quantum numbers.
Therefore, no more than two electrons can occupy an orbital, and these two must have opposite spins.
PTS: 1
34. ANS:
77
DIF: III
PTS: 1
DIF: L1
STA: SC.HS.1.1.1| SC.HS.1.1.2
35. ANS:
REF: 3
OBJ: 2
REF: p. 112
OBJ: 4.3.1
39
PTS: 1
OBJ: 4.3.1
36. ANS:
18
DIF: L2
REF: p. 110 | p. 111
STA: SC.HS.1.1.1| SC.HS.1.1.2
PTS: 1
DIF: L2
STA: SC.HS.1.1.1| SC.HS.1.1.2
37. ANS:
1
REF: p. 111
OBJ: 4.3.1
PTS: 1
DIF: L2
STA: SC.HS.1.1.1| SC.HS.1.1.2
38. ANS:
7
REF: p. 113
OBJ: 4.3.1
PTS: 1
STA: SC.HS.1.1.1
39. ANS:
2
DIF: L3
REF: p. 131
OBJ: 5.1.3 | 5.2.1
PTS: 1
OBJ: 5.2.1
40. ANS:
1
DIF: L3
STA: SC.HS.1.1.1
REF: p. 134 | p. 135 | p. 136
PTS: 1
41. ANS:
bromine
DIF: L2
REF: p. 136
OBJ: 5.2.2
PTS: 1
DIF: III
REF: 3
OBJ: 3
42. ANS:
John Dalton used experimental methods to hypothesize that atoms of the same element are identical, and that
they differ from atoms of other elements. Dalton also noted that atoms of different elements can form
compounds in which the elements combine in whole-number ratios. He noted that individual atoms are not
transformed into different atoms as a result of a chemical reaction. What Dalton did not contribute was the
fact that individual atoms are divisible into subatomic particles, which came from the discovery of the
electron and the atomic nucleus by Thomson and Rutherford, respectively.
PTS: 1
DIF: L3
REF: p. 101 | p. 102
OBJ: 4.1.1 | 4.1.2
43. ANS:
Rutherford’s gold-foil experiment led to this hypothesis. Alpha particles were observed to mostly pass
through a gold foil, which suggests that the volume of individual gold atoms consists mainly of empty space.
The observation that some alpha particles were scattered at large angles led to the suggestion that the gold
atom has a central core, or nucleus, composed of a concentrated mass capable of deflecting the alpha
particles.
PTS: 1
DIF: L3
REF: p. 107
OBJ: 4.2.2
44. ANS:
Different elements have different numbers of protons in their nuclei. All atoms of the same element have the
same number of protons. Because atoms are neutral, the number of electrons in an atom equals the number of
protons.
PTS: 1
DIF: L2
REF: p. 110 | p. 111 | p. 112
OBJ: 4.3.1
STA: SC.HS.1.1.1| SC.HS.1.1.2
45. ANS:
Isotopes of the same element have different numbers of neutrons, and therefore, different mass numbers and
different atomic masses. Isotopes of the same element have the same number of protons and electrons. The
electrons, not the neutrons, are responsible for an element's chemical behavior.
PTS: 1
DIF: L3
REF: p. 112
OBJ: 4.3.1
STA: SC.HS.1.1.1| SC.HS.1.1.2
46. ANS:
Electrons occupy orbitals in a definite sequence, filling orbitals with lower energies first. Generally, orbitals
in a lower energy level have lower energies than those in a higher energy level. But, in the third level the
energy ranges of the principal energy levels begin to overlap. As a result, the 4s sublevel is lower in energy
than the 3d sublevel, so it fills first.
PTS: 1
DIF: L2
REF: p. 133
OBJ: 5.2.1
STA: SC.HS.1.1.1
47. ANS:
The aufbau principle states that electrons enter the orbitals of lowest energy first. The Pauli exclusion
principle states that each orbital can hold only two electrons. Hund's rule states that electrons first enter
separate orbitals of the same energy, with each electron having the same spin, before pairing with electrons
that have opposite spins.
PTS: 1
DIF: L3
REF: p. 133 | p. 134 | p. 135 | p. 136
OBJ: 5.2.1 | 5.2.2
48. ANS:
It is a model that describes subatomic particles and atoms as waves. Schrodinger applied a mathematical
model of the wave/particle nature of matter to hydrogen. Solutions to the Schrodinger equation determine the
energies an electron can have and how likely it is to find the electron in various locations.
PTS: 1
DIF: L3
REF: p. 130 | p. 145
OBJ: 5.1.3 | 5.3.4
49. ANS:
The measurement of the speed or position of a moving particle necessarily involves an interaction with the
particle. Therefore, the position or the speed of the particle is changed as a result of the measurement. As a
consequence, accurate measurements of both these variables cannot be made at the same time.
PTS: 1
DIF: L3
REF: p. 145
OBJ: 5.3.4
50. ANS:
Atomic size increases with increasing atomic number within a group. For example, sodium atoms are larger
than lithium atoms, and potassium atoms are larger than sodium atoms. Atomic size decreases with increasing
atomic number across a period. For example, lithium atoms are larger than beryllium atoms, and beryllium
atoms are larger than boron atoms.
PTS: 1
DIF: L2
REF: p. 171
OBJ: 6.3.1
STA: SC.HS.1.1.1| SC.HS.1.1.5
51. ANS:
First ionization energies decrease from top to bottom within a group and increase across a period from left to
right. For example, the first ionization energy of rubidium is less than that of lithium. The first ionization
energy of iodine is much greater than that of lithium.
PTS: 1
DIF: L2
REF: p. 174
OBJ: 6.3.3
52. ANS:
When an electron is added to an atom, the attraction of the nucleus for any one electron decreases and the size
of the ion’s radius increases. When an electron is removed from an atom, there is an increase in the nuclear
attraction experienced by the remaining electrons. Consequently, the remaining electrons are drawn closer to
the nucleus.
PTS: 1
DIF: L3
REF: p. 176
OBJ: 6.3.3
53. ANS:
Electronegativity values decrease from top to bottom within a group, and from right to left across a period.
For example, rubidium is less electronegative than lithium. Lithium is less electronegative than fluorine.
PTS: 1
DIF: L3
REF: p. 177
OBJ: 6.3.3