Quarterly 1 Review
Name:
1. Base your answer to the following question on the information below.
Two isotopes of potassium are K-37 and K-42.
What is the total number of neutrons in the nucleus of a K-37 atom?
2. Base your answer to the following question on the table below.
On the same grid, plot the data from the table. Circle and connect the points.

Quarterly 1 Review
3. Base your answer to the following question on the information and diagram below.
One model of the atom states that atoms are tiny particles composed of a uniform mixture of positive and negative charges. Scientists conducted an experiment where alpha particles were aimed at a thin layer of gold atoms.
Most of the alpha particles passed directly through the gold atoms. A few alpha particles were deflected from their straight-line paths. An illustration of the experiment is shown below.
A few of the alpha particles were deflected.
What does this evidence suggest about the structure of the gold atoms?
4. Base your answer to the following question on the information below.
The accepted values for the atomic mass and percent natural abundance of each naturally occurring isotope of silicon are given in the data table below.
Determine the total number of neutrons in an atom of Si-29.

Quarterly 1 Review
5. Naturally occurring boron is composed of two isotopes. The percent abundance and the mass of each isotope are listed below.
• 19.9% of the boron atoms have a mass of 10.013 atomic mass units.
• 80.1% of the boron atoms have a mass of 11.009 atomic mass units.
Calculate the atomic mass of boron. Your response must include both a correct numerical setup and the calculated result.
__________________ atomic mass units
6. What is the total number of neutrons in an atom of aluminum-27?
7. Describe the electrons in an atom of carbon in the ground state. Your response must include:
• the charge of an electron
• the location of electrons based on the wave-mechanical model
• the total number of electrons in a carbon atom
8. 40% of the isotopes of an element have a mass of 16 amu. 60% of the isotopes have a mass of
18 amu. Calculate the average atomic mass.
Show all work.

Quarterly 1 Review
9. The table below shows the electronegativity of selected elements of the Periodic Table.
a On the grid set up a scale for electronegativity on the y-axis. Plot the data by drawing a best-fit line.
b Using the graph, predict the electronegativity of nitrogen. _________________ c For these elements, state the trend in electronegativity in terms of atomic number.
10. Base your answer to the following question on the information below.
State, in terms of the number of subatomic particles, one similarity and one difference between the atoms of these isotopes of sulfur.

Quarterly 1 Review
11. Base your answer to the following question on the data table provided.
Record the electronegativity for the elements with atomic numbers 11 through 17.
12. Base your answer to the following question on the information below.
Elements with atomic numbers 112 and
114 have been produced and their
IUPAC names are pending approval.
However, an element that would be put between these two elements on the
Periodic Table has not yet been produced. If produced, this element will be identified by the symbol Uut until an
IUPAC name is approved.
Identify one element that would be chemically similar to Uut.

Quarterly 1 Review
13. Base your answer to the following question on the information below.
Arsenic is often obtained by heating the ore arsenopyrite, FeAsS. The decomposition of FeAsS is represented by the balanced equation below.
In the solid phase, arsenic occurs in two forms. One form, yellow arsenic, has a density of 1.97 g/cm
3
at
STP. The other form, gray arsenic, has a density of 5.78 g/cm
3
at STP. When arsenic is heated rapidly in air, arsenic(III) oxide is formed.
Although arsenic is toxic, it is needed by the human body in very small amounts. The body of a healthy human adult contains approximately 5 milligrams of arsenic.
Convert the mass of arsenic found in the body of a healthy human adult to grams.
14. A knowledge of the ionization energies of elements can be very useful in predicting the activity and type of reaction an element will have.
a What does the ionization energy quantitatively measure about an atom?
b Why do ionization energies decrease from the top to the bottom of a group on the periodic table of elements?
c Why do ionization energies increase from left to right across any period?
15. Base your answer to the following question on the information below.
A metal, M , was obtained from a compound in a rock sample.
Experiments have determined that the element is a member of Group 2 on the
Periodic Table of the Elements.
Explain, in terms of electrons, why element M is a good conductor of electricity.

Quarterly 1 Review
16. Base your answer to the following question on the Reference Tables for Physical Setting/Chemistry.
a Complete the data table provided for the following Group 18 elements: He, Ne, Ar, Kr, Xe b Using information from your data table in part a , construct a line graph on the grid provided , following the directions below.
• Mark an appropriate scale on the axis labeled “First Ionization Energy (kJ/mol). ”
• Plot the data from your data table. Circle each point and connect the points.
c Based on your graph in part c , describe the trend in first ionization energy of Group 18 elements as the atomic number increases.
17. A student determines the density of zinc to be
7.56 grams per milliliter. If the accepted density is 7.14 grams per milliliter, what is the student’s percent error?
• Show a correct numerical setup.
• Record your answer.

Quarterly 1 Review
18. Base your answer to the following question on the information below.
A hydrate is a compound that has water molecules within its crystal structure. The formula for the hydrate CuSO
CuSO
4
•5H
4
•5H
2
O(s) shows that there are five moles of water for every one mole of CuSO
2
O(s) is heated, the water within the crystals is released, as represented by the balanced equation below.
4
(s). When
CuSO
4
•5H
2
O(s) —> CuSO
4
(s) + 5H
2
O(g)
A student first masses an empty crucible (a heat-resistant container). The student then masses the crucible containing a sample of CuSO
4
•5H
2
O(s). The student repeatedly heats and masses the crucible and its contents until the mass is constant. The student’s recorded experimental data and calculations are shown below.
Use the student’s data to show a correct numerical setup for calculating the percent composition by mass of water in the hydrate.

Quarterly 1 Review
19. Base your answer to the following question on the information below.
Archimedes (287–212 BC), a Greek inventor and mathematician, made several discoveries important to science today. According to legend, Hiero, the king of Syracuse, commanded
Archimedes to find out if the royal crown was made of gold, only. The king suspected that the crown consisted of a mixture of gold, tin and copper.
Archimedes measured the mass of the crown and the total amount of water displaced by the crown when it was completely submerged. He repeated the procedure using individual samples, one of gold, one of tin, and one of copper. Archimedes was able to determine that the crown was not made entirely of gold without damaging it.
Determine the volume of a 75-gram sample of gold at STP.
20. Using a triple beam balance and a graduated cylinder, a student collected data on a sample of an element:
Mass of sample – 10.9 g
Volume of water – 30.0 ml
Volume of water and sample – 34.0 ml a) Calculate the density of the sample. Show all work and use significant figures and units.
b) Based on Reference Table S, what element might the sample be?

1. 18.
probable location. • a carbon atom has six electrons.
13. 5 x 10
-3 g or 0.005 g
2.
8. 17.2 amu
9.
14. a) The ionization energy is the amount of energy needed to remove the most loosely bound electron from an atom. b) The electrons are farther away in the lower periods so there is less pull from the nucleus.
Also, there is shielding from the electrons that are closer to the nucleus. c)
Allow credit for plotting all the points correctly
(±0.3 grid space). Plotted points do not need to be circled or connected.
Electrons are held tighter to an atom because of the increase in nuclear charge.
15. Examples: – Metals have freely moving valence electrons. – mobile valence electrons
3. Examples:
– Alpha particles were
4. 15 deflected by the positively charged nucleus.
– nucleus — charged b The electonegativity of nitrogen is 3.0 (
)
0.2).
c Example: -Atomic
– sea of mobile electrons
– Electrons are delocalized.
number increases—electronegativit
16. y increases.
5. • Correct Numerical Setup
Examples: 10. Similarity: All atoms of
–– (10.013)(0.199) + these isotopes have the
(11.009)(0.801) same number of protons;
––
100 100
–– (10.013)(19.9%) +
Every sulfur atom has 16 protons; Difference: An S-
(11.009)(80.1%) 32 atom has 16 neutrons,
• Calculated Result an S-33 atom has 17
Examples: ––10.8 atomic mass units; ––10.81 neutrons, an s-34 atom has 18 neutrons, and an satomic mass units; 36 atom has 20 neutrons.
––10.8108 atomic mass units 11.
18.
19. 3.9 cm
3
20. a) 2.7 g/ml b) Al
6. 14
7. Answer: • an electron has a negative charge. • electrons are located in orbitals or regions of most
Examples: – Ti – boron
17.
7.14
7.14
Examples: 5.88 or 5.9 or 6