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ESUHSD Chemistry Benchmark Assessment #2
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
1. Alkali metals, alkaline-earth metals and halogens are found respectively in groups
a. 1, 2, 18
c. 1, 2, 17
b. 1,2, 14
d. 2, 13, 17
____
2. Which element do you expect to have similar chemical properties as sulfur?
a. carbon
c. nitrogen
b. magnesium
d. oxygen
____
3. Which of these ions has the same electron configuration as Ar?
a. Na+
c. S–
b. Ca+
d. Cl–
____
4. Which of the following is the Lewis dot diagram of the element fluorine (F)?
a.
c.
b.
____
d.
5. Which element in Period 2 of the Periodic Table is the most reactive non-metal?
a. nitrogen
c. carbon
b. oxygen
d. fluorine
____
6. Which of these elements achieves a noble gas (stable) electron configuration by forming four
covalent bonds?
a. oxygen
b. nitrogen
c. carbon
d. chlorine
____
7. The force of attraction that holds ions together in salts like KCl is ___________.
a. electrostatic
c. magnetic
b. nuclear
d. gravitational
____
8. :X X:
In the Lewis dot structure shown above, X is most likely _______.
a. fluorine
b. neon
c. nitrogen
d. oxygen
____
9.
Above is the Lewis dot structure of ammonia, NH3. Which molecule or ion has a similar Lewis dot
structure and geometric shape as ammonia?
a. BF3
c. O3
b. PCl3
d. NH4+
____ 10. Atoms of metallic elements tend to
a. lose electrons and form negative ions
b. gain electrons and form positive ions
c. lose electrons and form positive ions
d. gain electrons and form negative ions
____ 11. Which statement best describes the bond in BaO?
a. It is ionic because valence electrons
c. It is covalent because valence electrons
are transferred from barium to oxygen.
are transferred from barium to oxygen.
b. It is ionic because valence electrons
are shared between barium and
oxygen.
____
12. Where are valence electrons located?
a. inside the nucleus
b. in the innermost shell
d. It is covalent because valence electrons
are shared between barium and
oxygen.
c. in the outermost shell
d. in the s orbitals
____
13. As you move down a group of the periodic table, the atomic radii of the elements
a. increase.
c. remain constant.
b. decrease.
d. show no pattern.
____
14. When a sodium atom loses an electron,
a. it collapses.
b. it becomes negatively charged.
____
c. it becomes bigger.
d. it becomes smaller.
15. What is the number of shared electrons in a double covalent bond?
a. 2
c. 6
b. 4
d. 8
Ionization Energy
Atomic Number
____
16. Based on the graph shown above, what general trend exists for first ionization energy across a
period, from left to right?
a. Ionization energy increases.
b. Ionization energy decreases.
c. Ionization energy remains fairly constant.
d. Ionization energy first increases, then decreases.
____ 17. Which of the following factors does NOT contribute to the decrease in ionization energy within a
group on the periodic table as the atomic number increases?
a. Increase in atomic size
b. Increase in nuclear charge
c. Increase in number of protons
d. Fewer electrons in the highest occupied energy level
____ 18. Which of the following elements has the smallest first ionization energy?
a. sodium
c. lithium
b. calcium
d. magnesium
____ 19. Which statement is true about electronegativity?
a. Electronegativity is the ability of an anion to attract another anion.
b. Electronegativity generally increases as you move from top to bottom within a
group.
c. Electronegativity generally is higher for metals than for nonmetals.
d. Electronegativity generally increases from left to right across a period.
TABLE OF COMMON IONS
H1+
Ca2+
Zn2+
Cu2+
Al3+
Fe3+
Cl1–
OH1–
P3–
NO31–
SO42–
CO32–
PO43–
Figure 1
____
20. Using Figure 1, determine the formula of the compound formed between calcium and hydroxide
ions.
a. CaOH
c. CaOH2
b. Ca(OH)2
d. Ca2OH
____ 21. What type of bond do the following molecules have in common: H2, C6H12O6, NH3?
a. hydrogen bond
b. covalent
c. ionic
d. metallic
____ 22. Which element do you expect to have the same number of valence electrons as phosphorus?
a. sodium
b. argon
c. nitrogen
d. sulfur
____ 23. Which of the following is a characteristic of most ionic compounds?
a. They are mostly liquids at room temperature.
b. They have low melting points.
c. When melted, they conduct an electric current.
d. They are composed of nonmetallic elements.
____ 24. Which of the following covalent bonds is the most polar?
a. H—F
c. H—H
b. H—C
d. H—N
____ 25. Which of these changes does NOT involve the breaking of hydrogen bonds?
a. boiling water
b. electrolysis of water into hydrogen gas and oxygen gas
c. decomposition of hydrogen peroxide(H2O2) into water and hydrogen gas
d. dissociation of hydrogen chloride (HCl) into hydrogen ion (H+) and chloride ion
(Cl-)
____
26. What is the name of the compound whose formula is (NH4)3PO4?
a. triammonium quatrophosphate
c. ammonium phosphate
b. polyammonium phosphate
d. ammonium phosphide
____ 27. In which of the following is the name and formula given correctly?
a. sodium oxide, NaO
c. copper(II) chloride, CuCl2
b. barium nitride, Ba(NO3)2
d. iron(II) oxide, Fe2O3
____ 28. An element with an electronegativity of 0.9 bonds with an element with an electronegativity of 3.1.
Which of the following phrases best describes the bond between these elements?
a. mostly covalent in character and formed between a metal and a non-metal
b. mostly covalent in character and formed between two non-metals
c. mostly ionic in character and formed between a metal and a non-metal
d. mostly ionic in character and formed between two non-metals
____ 29. Conductivity in metals results from metal atoms having
a. high electronegativity
c. highly mobile protons in the nucleus
b. highly mobile electrons in the valence d. high ionization energy
shell
____ 30. Which of the following is the correct name for N2O5?
a. nitrous oxide
c. nitrogen dioxide
b. dinitrogen pentoxide
d. nitrate oxide
GP#2: ESUHSD Chemistry Benchmark Test
Answer Section
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