Benchmark #1 Review Guide
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Name:___________________________________ Period:______
Section 1 – Matter and Density
1. What is the definition of matter?
2. Which of the following is an example of matter?
a. Energy
b. An idea
c. Rain
d. A dream
3. What is the formula for density?
4. What is the density of an item that has a mass of 85 g and a volume of 15 mL?
5. The density of zinc is 7.1 g/cm3. How much would 20 cm3 of zinc weigh?
6. Why does a steel nail have the same density as a steel beam?
7. Which of these statements is true about two blocks of gold that are different shapes but have the
same mass?
a. They have the same volume, but different densities.
b. They have different volumes, but the same density.
c. They have different volumes and different densities.
d. They have the same volume and the same density.
8. Two objects both have a volume of 16 cm3. Object 1 has a mass of 10 g and object 2 has a mass of 8
g. Calculate the density of each object. Which is less dense?
Section 2 – Periodic Table
9. Most of the elements on the periodic table are:
a. Solid metals
b. Gaseous nonmetals
c. Liquid metals
d. Radioactive
10. Which of these describes bromine’s location on the periodic table?
a. Group 7A, Period 4
b. Group 4, Period 7A
c. Group 3A, Period 2
d. Group 2, Period 3A
11. Name three elements that are alkali metals.
12. What are the groups 2A, 7A, and 8A called?
13. Draw the box on the periodic table for one element. On the box, label the atomic number, average
atomic mass, element symbol, and element name.
14. Where can nonmetals be found on the periodic table?
15. Where are the transition metals located on the periodic table?
16. The most reactive elements on the periodic table are on the bottom of group 1A and the top of
group 7A. Name the most reactive metal and the most reactive nonmetal. Make sure to label which
is which.
17. Which of the following elements would you expect to be the most reactive?
a. Boron, B
b. Gold, Au
c. Argon, Ar
d. Barium, Ba
Section 3 – Isotopes and Nuclear Chemistry
Use the following information to answer questions 18, 19, and 20:
12
13
14
6𝐶
6𝐶
6𝐶
𝐶𝑎𝑟𝑏𝑜𝑛 − 12
𝐶𝑎𝑟𝑏𝑜𝑛 − 14
𝐶𝑎𝑟𝑏𝑜𝑛 − 13
18. In the isotope symbols shown above, what does the number on the upper left represent?
a. Atomic number
b. Number of protons
c. Number of neutrons
d. Mass number
19. Why do the isotopes above have a different atomic mass?
20. Why do all of the isotopes on the previous page have the number 6 in the lower left?
21. Lithium has an atomic number of 3 and an average atomic mass of 6.941 amu. Predict the isotope
you would find in the greatest abundance given a sample of lithium
a. Lithium-4
b. Lithium-6
c. Lithium-7
d. Lithium-6.9
22. The element gallium has two stable isotopes. About 60% of the gallium atoms found are gallium69, while the remaining 40% are gallium-71. The average atomic mass of gallium is about:
a. 69.6 amu
b. 69.8 amu
c. 70.2 amu
d. 70.4 amu
23. What are the two types of radioactive decay and what particles do they produce?
24. If potassium-40 undergoes beta decay, the result is?
a. Argon-40
b. Calcium-40
c. Chlorine-36
d. Scandium-44
25. What is the definition of fission and the definition of fusion?
26. In nuclear reactors uranium is bombarded with neutrons and the large isotope breaks apart into
smaller isotopes and releases energy. Is this fission or fusion?
Section 4 – Light, Valence Electrons, and Ions
27. Use the table to determine the color of the flame produced by a sample of potassium bromide
(KBr).
Compound
Flame Color
BaBr2
Green
NaBr
Yellow
K2SO4
Violet
a.
b.
c.
d.
Yellow
Green
Violet
Violet-green
28. Define absorption and emission. Draw a picture of each process.
29. Violet light has a wavelength of 410 nm. Which of the following energy differences (shell
transitions) would correspond to violet light? Show your work.
a. ∆E= 8.56 x 10-19 J
b. ∆E= 4.84 x 10-19 J
c. ∆E= 7.32 x 1014 J
d. ∆E= 2.56 x 1014 J
30. Calculate the wavelength (in m) of radio waves if they produce photons with an energy equal to
2.47 x 10-30 J.
31. An atom that has 7 valence electrons is in which group?
a. Alkali metals
b. Alkaline earth metals
c. Halogens
d. Noble gases
32. To create an ion from a neutral atom, which of these values is changed?
a. The number of electrons
b. The number of neutrons
c. The number of nuclei
d. The number of protons
33. Which of these are the correct labels for the two shell diagrams below?
a.
b.
c.
d.
a fluorine atom and a fluoride ion with a charge of –1
a fluorine atom and a fluoride ion with a charge of +1
a fluorine atom and a neon atom
a neon ion with a charge of +1 and a neon atom
34. Atoms in group 7A have 7 valence electrons and they need one more. Which group of atoms has
one valence electron on their outermost shell?
35. Name an atom on the periodic table that has three spaces available for bonding (i.e. needs 3 more
electrons in order to be stable).
36. Write out the full electron configuration for the following elements:
a. Mg
b. O
c. S
d. B
37. Write the noble gas short-hand for the following elements:
a. Tc
b. Sn
c. Pb
d. Pr