Unit 2 Exam CP » Form D
Directions: Please choose the best answer choice for each of the following questions.
1.
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.
2.
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?
A. Salt does not dissolve in water.
B. Salt has a higher melting point than water.
3.
C.
Salt forms covalent bonds with the water
molecules.
D.
Salt separates into positive and negative
ions in the water.
Atoms with high ionization energies
A. easily lose electrons.
B. easily form positive ions.
C.
have weaker attractions for their
electrons.
D. hold their valence electrons tightly.
Why does the bulb in Solution A glow?
4.
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.
The Lewis dot structure of methane (CH4) is
shown below.
What is the geometric shape of the molecule
based on this diagram?
A. cubic
B. square
C. octahedral
D. tetrahedral
Go on to the next page »
DataDirector Assessment ID: 90097
Page 1 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
5.
Compounds that are formed by ionic bonds
separate into ions when dissolved in water.
These ions are able to carry electrical
current.
Which tool would be most useful in
determining whether a dissolved compound
was ionic?
A. conductivity meter
9.
A. linear.
B. bent.
C. trigonal planar.
D. tetrahedral.
10. How are salt crystals of sodium chloride
(NaCl) formed?
A.
Sodium forms a positive ion that is
attracted to chlorine's negative ion.
D. temperature meter
B.
Sodium forms a negative ion that is
attracted to chlorine's positive ion.
The elements in the periodic table are
arranged in order of increasing
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.
B. pH meter
C. pressure meter
6.
A. reactivity.
B. atomic radii.
C. number of ions.
11.
D. number of protons.
7.
The shape of the water molecule (H2O) is
Why is carbon able to form very large organic
molecules?
A. Electrons are lost to form ionic bonds.
In which substance are the atoms connected
by covalent bonds?
B. Electrons are gained to form ionic bonds.
A. NH3
C.
Four covalent bonds can be formed by
sharing electrons.
D.
Covalent bonds can be formed that have
unshared electrons.
B. NaF
C. CaO
D. CaCl2
8.
12. The more electronegative an atom is
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
A. the less protons it has.
A. gaining; fill
D. the greater its tendency to lose electrons.
B. losing; empty
B. the more protons it has.
C. the greater its tendency to gain electrons.
13. Annie is reading about the formation of ions.
+
C. sharing; fill
How does a potassium (K) atom become a K
ion?
D. sharing; empty
A. Potassium gains a proton.
B. Potassium increases in size.
C. Potassium loses an electron.
D. Potassium becomes an isotope.
Go on to the next page »
DataDirector Assessment ID: 90097
Page 2 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
14. An ionic bond involves
19. Which pair of elements typically combines
with each other by forming covalent bonds?
A. sharing of electrons.
A. copper and zinc
B. exchange of electrons.
B. argon and oxygen
C. sharing of metallic bonds.
C. calcium and chlorine
D. exchange of protons.
15. Which compound is held together by ionic
bonds?
D. hydrogen and nitrogen
20. Often atoms join so that each atom will have
A.
A. an even number of electrons.
B.
C.
D.
16. Which BEST describes the type of bonding
that occurs in potassium chloride (KCl)?
A. mostly ionic
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.
21. An ionic compound consists of
B. mostly covalent
cations
C. metallic and ionic
and
anions. What is the formula for this
ionic compound?
D. metallic and covalent
A.
B.
17. Which element would form covalent bonds
with sulfur?
C.
A. sodium (Na)
D.
B. nitrogen (N)
22. Ionic bonds form when two atoms
C. iron (Fe)
A. exchange outer shell electrons.
D. lead (Pb)
B. exchange inner shell electrons.
18. Carbon (C) and hydrogen (H) have
electronegativities that are similar. Which
type of bonding occurs between atoms in
methane (CH4)?
C. share inner shell electrons.
D. share outer shell electrons.
A. covalent
B. ionic
C. magnetic
D. metallic
Go on to the next page »
DataDirector Assessment ID: 90097
Page 3 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
23. The diagram below shows a cubic crystal of
salt (NaCl).
24. A water molecule is made up of 1 oxygen
atom and 2 hydrogen atoms. Which diagram
shows the correct Lewis dot structure for
water?
A.
B.
C.
D.
25. The shape of the carbon dioxide molecule
(CO2) is
A. linear.
B. bent.
What do the two arrows indicate?
A.
electrons and protons held together by
interatomic forces
B.
sodium and chlorine ions held together by
covalent bonds
C.
water and salt molecules held together by
intermolecular forces
D.
sodium and chlorine ions held together by
electrostatic attraction
C. trigonal planar.
D. tetrahedral.
26. 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.
D. the electrons of two different atoms.
27. When the difference in electronegativity
between two atoms is large, the atoms can
bond by transferring electrons. Which type of
bonding occurs when this happens?
A. covalent
B. ionic
C. metallic
D. nuclear
Go on to the next page »
DataDirector Assessment ID: 90097
Page 4 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
28. The diagram below shows the structure that
results when sodium and chlorine combine to
form table salt (NaCl).
31. Covalent bonds are formed between
A. ions.
B. metal atoms.
C. nonmetal atoms.
D. compounds.
32. The diagram below shows two different
versions of ethane
.
Why are there different versions of the same
molecule?
A. The bonding is different.
What is the name of this type of structure?
B. The molecular weights are different.
A. crystal
C. The bonds are shown in different ways.
B. polymer
D.
C. Bohr model
D. Lewis dot diagram
29. An ionic compound consists of positive and
negative ions which
The different numbers of electrons are
shown.
33. 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.
A. form individual molecules.
B. alternate in a crystal lattice.
C. are embedded in a sea of electrons.
D.
are held together by intermolecular
forces.
30. 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?
What determines these patterns?
A. the geometrical shape of each ion
B. the number of isotopes in each ion
A. covalent
C. the magnetic forces between the ions
B. electric
D. the electrostatic forces between the ions
C. ionic
D. metallic
Go on to the next page »
DataDirector Assessment ID: 90097
Page 5 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
34. Covalent bonds involve the
38. 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. sharing of electrons.
B. exchange of electrons.
C. sharing of metallic bonds.
D. exchange of protons.
35. In which substance are all the bonds MOST
LIKELY covalent?
A.
B.
C.
D.
36. The Lewis dot structure for a carbon
tetrachloride molecule is shown below.
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.
39. The diagram below shows an incorrect Lewis
dot structure for carbon dioxide.
What is needed to make this Lewis dot
structure correct?
Which statement is true about carbon
tetrachloride?
A. two triple bonds
A. The carbon atom has eight bonds.
C. two shared electrons
B. two double bonds
B. Each chlorine atom has four bonds.
C.
The carbon atom has four unshared
electrons.
D.
Each chlorine atom has six unshared
electrons.
D. two unshared electrons
40. Copper is a good conductor of electricity
because its electrons
A. are positively charged.
B. are free to move from atom to atom.
37. Which element has twelve protons in its
nucleus?
C.
can take on either positive or negative
charges.
D.
are shared between neighboring
compounds.
A. carbon
B. chromium
C. magnesium
D. sodium
41. How many nonbonding electrons are present
in the Lewis dot structure of ammonia
?
A. 2
B. 3
C. 5
DataDirector Assessment ID: 90097
Page 6 of 9
Go on to the next page »
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
42. Metallic bonds form when atoms
A. exchange outer shell electrons.
B. share inner shell electrons.
C. share outer shell electrons.
D. exchange multiple electrons.
Go on to the next page »
DataDirector Assessment ID: 90097
Page 7 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
Directions: Review the content below and answer the questions that follow
Periodic Table
43. Below is a list of seven different elements.
B, Si, Ge, As, Sb, Te, Po
44. Which statement BEST explains the
elements found in group 17 of the periodic
table?
Which statement BEST explains the general
nature of these elements?
A.
Elements of a metallic nature are in this
group.
These are metals, with nonmetals located
A. toward the right and metalloids located
toward the left.
B.
Elements with the same valence are in
this group.
C.
Elements with the same atomic number
are in this group.
D.
Elements with the same atomic mass
number are in this group.
These are nonmetals, with metals located
B. toward the right and metalloids located
toward the left.
These are metalloids, with metals located
C. toward the right and nonmetals located
toward the left.
These are metalloids, with nonmetals
D. located toward the right and metals
located toward the left.
Go on to the next page »
DataDirector Assessment ID: 90097
Page 8 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.
Unit 2 Exam CP » Form D
Directions: Please choose the best answer choice for each of the following questions.
45. In relation to the atom, the nucleus has the
50. Which set of elements are halogens?
A. most mass and least volume.
A. helium (He), neon (Ne), argon (Ar)
B. most mass and most volume.
B. lithium (Li), sodium (Na), potassium (K)
C. least mass and most volume.
C. bromine (Br), iodine (I), chlorine (Cl)
D. least mass and least volume.
D. boron (B), aluminum (Al), gallium (Ga)
46. Which of the following would you expect to
have the largest atomic radius?
A. calcium (Ca)
B. iodine (I)
C. potassium (K)
D. cesium (Cs)
47. 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)
48. Aluminum, magnesium, silicon, and sodium
are elements that can be found in the
periodic table. Based on their position in the
periodic table, which element has the highest
electronegativity?
A. aluminum
B. magnesium
C. silicon
D. sodium
49. Which of these is the correct number of
electrons that boron (B) has available for
bonding?
A. 1
B. 3
C. 5
D. 8
Stop! You Go
have
onfinished
to the next
thispage
exam.
»
DataDirector Assessment ID: 90097
Page 9 of 9
© 2011 Houghton Mifflin Harcourt. All rights reserved.