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Unit 2 Exam HP » Form B
Directions: Please choose the best answer choice for each of the following questions.
1.
Kevin is listing the similarities between
metallic and ionic bonds for a laboratory
project. Which similarity regarding the
properties of bonds is true?
3.
Hydrogen cyanide is a molecule that is
both linear and polar. Which diagram
represents the correct Lewis dot structure of
hydrogen cyanide?
A.
Metallic and ionic bonds account for
electrical conductivity.
A.
B.
Metallic and ionic bonds are formed due
to the sharing of electrons.
B.
Compounds containing metallic bonds
C. and compounds containing ionic bonds
have low melting and boiling points.
Compounds containing metallic bonds
and compounds containing ionic bonds
D.
have electrostatic repulsion between their
atoms or ions.
2.
C.
Which of the following ion pairs would be
held together by electrostatic attractions?
A. carbon and hydrogen
B. nitrogen and hydrogen
D.
C. sodium and oxygen
D. sodium and magnesium
4.
Which element has the lowest ionization
energy (energy need to remove an electron)?
A. boron (B)
B. carbon (C)
C. nitrogen (N)
D. fluorine (F)
5.
In which substance is the chemical
bonding BEST described as covalent?
A.
B.
C.
D. NaCl
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Unit 2 Exam HP » Form B
6.
A compound containing carbon (C), oxygen
(O), hydrogen (H), and nitrogen (N) would be
bonded together by _____ electrons in order
to _____ their outer energy levels
9.
The diagram below shows the Lewis dot
structure of carbon tetrafluoride.
A. gaining; fill
B. losing; empty
C. sharing; fill
D. sharing; empty
7.
Which statement BEST explains why this
molecule is nonpolar?
The fusion reaction of boron-11 and a proton
(hydrogen atom) is shown below. Three
atoms of an unknown element are formed in
the reaction.
A.
The bonds between carbon and fluorine
are covalent.
B.
The electronegativities of carbon and
fluorine are different.
C.
The molecule has nonbonded electrons
on the fluorine atoms.
D.
The molecule has a symmetrical
distribution of electron clouds.
10. The shape of the water molecule (H2O) is
A. linear.
B. bent.
C. trigonal planar.
D. tetrahedral.
Which element is formed?
11.
C. helium
Substances that are good conductors of heat
and electricity at room temperature usually
have delocalized electrons moving freely
from atom to atom. Which type of bonding
occurs in these substances?
D. magnesium
A. covalent
How are salt crystals of sodium chloride
(NaCl) formed?
B. electric
A. beryllium
B. carbon
8.
A.
Sodium forms a positive ion that is
attracted to chlorine's negative ion.
B.
Sodium forms a negative ion that is
attracted to chlorine's positive ion.
C.
Sodium forms a positive ion that is
attracted to chlorine's positive ion.
D.
Sodium forms a negative ion that is
attracted to chlorine's negative ion.
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C. ionic
D. metallic
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Unit 2 Exam HP » Form B
12. Which statement BEST describes how
transuranium elements were discovered?
A.
Transuranium elements were discovered
synthetically, using particle accelerators.
16. A water molecule is made up of 1 oxygen
atom and 2 hydrogen atoms. Which diagram
shows the correct Lewis dot structure for
water?
Transuranium elements were discovered
B. naturally, through mining rare earth
metals.
A.
Transuranium elements were discovered
C. by chemically reacting heavy elements
together.
B.
Transuranium elements were discovered
D. by adding electrons to the nuclei of larger
elements.
C.
13. How is the Lewis dot structure of
different from the Lewis dot structure for
?
D.
A.
There is a lone pair on the central atom in
.
B.
There is a lone pair on the central atom in
.
17. Which compound is held together by ionic
bonds?
A.
B.
has more electrons around the central
C.
atom than
.
D.
has more Fluorine atoms around the
central atom than
.
14. Which of these elements would have the
greatest electronegativity?
A. nitrogen (N)
B. oxygen (O)
C.
D.
18. Chlorine (Cl) and iodine (I) both react
with sodium (Na) to form sodium chloride
(NaCl) and sodium iodide (NaI). Which of
these BEST explains why chlorine reacts with
sodium more readily than does iodine?
A. Chlorine is more volatile than iodine.
C. phosphorous (P)
D. sulfur (S)
15. What is the element that has the ground state
2
14
6
B.
Chlorine is more electronegative than
iodine.
C.
Chlorine has a lower atomic mass than
iodine.
D.
Chlorine and sodium have the same
number of electron shells.
electron configuration [Xe]6s 4f 5d ?
A. La
B. Ti
C. W
D. Os
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Unit 2 Exam HP » Form B
19. Atoms with high ionization energies
23. The diagram below shows the structure that
results when sodium and chlorine combine to
form table salt (NaCl).
A. easily lose electrons.
B. easily form positive ions.
C.
have weaker attractions for their
electrons.
D. hold their valence electrons tightly.
20. When two atoms which both have high
electronegativity values combine, they form
________bonds.
A. ionic
B. covalent
C. metallic
D. hydrogen
21. Large biological molecules such as proteins
and carbohydrates, are held together by
What is the name of this type of structure?
A. ionic bonds.
A. crystal
B. metallic bonds.
B. polymer
C. covalent bonds.
C. Bohr model
D. hydrogen bonds.
D. Lewis dot diagram
22. A chemist was doing research on halogens.
Which elements could be included in her
work?
24. A molecule of silicon dioxide is overall ____
because it ____
A. neon, krypton, xenon
A. polar; has polar covalent bonds.
B. fluorine, chlorine, iodine
B. polar; is symmetrical in shape.
C. carbon, nitrogen, oxygen
C. nonpolar; has nonpolar covalent bonds.
D. thorium, plutonium, uranium
D. nonpolar; is symmetrical in shape.
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Unit 2 Exam HP » Form B
25. Ionic compounds, such as sodium chloride,
form crystals that have a regular, repeating
pattern of positive and negative ions, as
shown in the diagram below.
28. The shape of the carbon dioxide molecule
(CO2) is
A. linear.
B. bent.
C. trigonal planar.
D. tetrahedral.
29. An element belongs to group 17 (VIIA) of the
periodic table. Which type of ion will it MOST
LIKELY form?
What determines these patterns?
A. the geometrical shape of each ion
B. the number of isotopes in each ion
C. the magnetic forces between the ions
D. the electrostatic forces between the ions
26. Which statement BEST describes the
nucleus of an atom?
A.
most of the volume and contains most of
the mass
B.
most of the volume but contains very little
of the mass
A. an ion with a
charge
B. an ion with a
charge
C. an ion with a
charge
D. an ion with a
charge
30. The Lewis dot structure for a carbon
tetrachloride molecule is shown below.
very little of the volume but contains most
C.
of the mass
very little of the volume and contains very
D.
little of the mass
27. A chromium ion (Cr3+) combines with
Which statement is true about carbon
tetrachloride?
A. The carbon atom has eight bonds.
B. Each chlorine atom has four bonds.
C.
The carbon atom has four unshared
electrons.
D.
Each chlorine atom has six unshared
electrons.
2–
an oxygen ion (O ) to form an ionic
compound. Which formula represents the
ionic compound formed by these two ions?
A. CrO
B. CrO2
C. Cr2O3
D. Cr3O2
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Unit 2 Exam HP » Form B
31. The diagram below shows an incorrect Lewis
dot structure for carbon dioxide.
34. Two atoms which have large differences in
electronegativity would form a(n)
A. ionic bond.
B. nonpolar covalent bond.
C. polar covalent bond.
What is needed to make this Lewis dot
structure correct?
D. metallic bond.
A. two triple bonds
, oxygen
, and water
35. Methane
have similar bonding. Which statement
correctly describes each of these molecules?
B. two double bonds
C. two shared electrons
A. The molecules are all polar.
D. two unshared electrons
B. The molecules are all very reactive.
32. The Lewis dot structure of methane (CH4) is
shown below.
C.
Electrons are shared by the atoms of the
molecules.
D.
Electrons are transferred between the
atoms of the molecules.
36. Two potassium atoms will each transfer an
electron to a sulfur atom to form potassium
sulfide. What is the formula of potassium
sulfide?
A. KS
B. K2S
What is the geometric shape of the molecule
based on this diagram?
C. 2KS
D. KS2
A. cubic
B. square
37. Often atoms join so that each atom will have
C. octahedral
A. an even number of electrons.
D. tetrahedral
33. Which statement about noble gases is
correct?
A.
They form compounds with very bright
colors.
B.
They exist as single atoms rather than as
molecules.
C.
They are highly reactive with both metals
and nonmetals.
B.
an outermost energy level that is full of
electrons.
C.
an equal number of protons and
electrons.
D.
more electrons than either protons or
neutrons.
D. They are extremely rare in nature.
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Unit 2 Exam HP » Form B
38. An ionic bond is a bond that forms between
A. ions with opposite charges.
B. atoms with neutral charges.
C.
one atom´s nucleus and another atom´s
electrons.
40. In a lab activity, Susan fills Beaker A and
Beaker B with water. Susan adds an ionic
compound, magnesium chloride, to Beaker
A and a covalent compound, naphthalene, to
Beaker B.
D. the electrons of two different atoms.
39. Which type of bond occurs when atoms
complete their outermost electron shells by
sharing electrons?
A. ionic
B. covalent
C. hydrogen
D. van der Waals
What is the solubility behavior of the two
compounds?
A.
Both compounds have equal solubility in
water.
B.
Magnesium chloride has less solubility in
water than does naphthalene.
C.
Naphthalene has slightly less solubility in
water than does magnesium chloride.
D.
Naphthalene is insoluble in water, while
magnesium chloride is soluble in water.
41. Based on its dot structure dichloromethane,
CH2Cl2, is
A. polar because it is symmetrical.
B. nonpolar because it is symmetrical.
C. polar because it is asymmetrical.
D. nonpolar because it is asymmetrical.
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Unit 2 Exam HP » Form B
42. The formula unit for the ionic compound
sodium fluoride is NaF. What must occur
during bonding?
A. A catalyst helps form the bond.
B.
An electron transfers from one atom to
the other.
C.
The atoms repel each other by
electrostatic force.
D.
The outer orbitals of the two atoms join to
share electrons.
44. An electrical circuit is set up for Solution
A and Solution B as shown below. When
the electrodes are placed into the beakers,
the bulb in Solution A glows, but the bulb in
Solution B does not glow.
43. Cathy analyzes trends in the periodic table
by comparing oxygen and fluorine. Which
comparison is true based on the trends of the
periodic table?
A.
The ionic radius of fluorine is less than
that of oxygen.
B.
The atomic radius of oxygen is less than
that of fluorine.
C.
The electronegativity of oxygen is more
than that of fluorine.
D.
The ionization energy of fluorine is the
same as that of oxygen.
Why does the bulb in Solution A glow?
A.
Solution A is ionic and conducts
electricity.
B.
Solution A is covalent and conducts
electricity.
C.
Solution A has a low boiling point, which
makes it a good conductor of electricity.
D.
Solution A contains neutral atoms, which
makes it a good conductor of electricity.
45. The shape of the molecule BF3 is
A. linear.
B. bent.
C. trigonal planar.
D. tetrahedra.
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Unit 2 Exam HP » Form B
46. The more electronegative an atom is
A. the less protons it has.
B. the more protons it has.
C. the greater its tendency to gain electrons.
D. the greater its tendency to lose electrons.
50. Table salt crystals consist of a pattern
of alternating sodium ions and chloride
ions. When the salt is added to water, the
electrical conductivity of the water increases.
Which explanation BEST describes this
observation?
47. John is conducting a lab experiment to test
the melting points of an ionic and a covalent
compound. He uses sodium chloride, an
ionic compound, and cane sugar, a covalent
compound. What is true about the melting
points of the two compounds?
A.
Sodium chloride and cane sugar do not
melt.
B.
Sodium chloride and cane sugar have the
same melting points.
C.
Sodium chloride has a lower melting point
than does cane sugar.
D.
Sodium chloride has a higher melting
point than does cane sugar.
A. Salt does not dissolve in water.
B. Salt has a higher melting point than water.
C.
Salt forms covalent bonds with the water
molecules.
D.
Salt separates into positive and negative
ions in the water.
48. Copper is a good conductor of electricity
because its electrons
A. are positively charged.
B. are free to move from atom to atom.
C.
can take on either positive or negative
charges.
D.
are shared between neighboring
compounds.
49. How many nonbonding electrons are present
in the Lewis dot structure of ammonia
?
A. 2
B. 3
C. 5
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