Download All of these can affect the rate at which a

Matter Test
6. Rust (Fe2O3) forms on an iron (Fe) pipe after prolonged
exposure to humid air. What type of change does this
illustrate?
A mechanical
B nuclear
C chemical
D physical
1. What can be concluded from the relationships described
above?
A Gas molecules travel longer distances at greater speeds
when the volume of the gas is decreased.
B A gas is more likely to lose kinetic energy when its
volume is reduced.
C Gas molecules collide less frequently when the volume
of the gas is increased.
D A gas is more likely to increase in momentum when its
volume is increased.
7. Knowing the chemical properties of a substance will tell
you how the substance…
A looks
B smells
C can be broken down into atoms
D reacts with other substances
2. Sheets of ice containing mostly pure water can be formed by
decreasing the temperature of saltwater. Which of these best
describes this change?
A Chemical change
B Physical change
C Nuclear change
D Atomic change
3. What classification of matter is a ring that is 14-karat
gold? (Pure gold is 24 karat.)
A
B
C
D
compound
element
heterogeneous mixture
homogeneous mixture
4. The properties of a compound are ___________ the
properties of the elements making up the compound.
A
B
C
D
the same as
different from
the same as or different from, depending on the
compound
always similar to
5. A ____ is NOT a mixture.
A
B
C
D
colloid
compound
suspension
solution
8. Some types of weathering involve breaking up rock by
agents such as roots or ice. What type of change is
involved in this type of weathering?
A a physical change
B a chemical change
C both a chemical change and a physical change
D neither a chemical nor a physical change
9. Other types of weathering involve the breaking down of
rock by agents such as acids in rain, in groundwater, or
released by certain plants. What type of change is
involved in this type of weathering?
A a physical change
B a chemical change
C both a chemical change and a physical change
D neither a chemical nor a physical change
10. Which of these are composed of two or more different
substances that are chemically combined in a definite
ratio?
A
B
C
D
compounds
mixtures
elements
solutions
Matter Test
11.
A
B
C
D
Almost all matter ____ when heated.
condenses
contracts
expands
solidifies
12. The diagram above shows an example of which of the
following?
A element
B compound
C heterogeneous mixture
D homogeneous mixture
13. Compared to most substances, water is unusual because
it ____ when it goes from the liquid to solid state.
A contracts
B expands
C melts
D diffuses
14. When two or more substances are combined so each
substance can be separated by physical means, the result
is a(n)____.
A
B
C
D
chemical change
compound
mixture
element
15. Which of the following is a chemical property of the
element hydrogen?
A
B
C
D
18. Three examples of physical change would be the…
A boiling of water, the bursting of a balloon and the
crumpling of a piece of paper
B burning of gasoline, the rotting of an egg and the
exploding of fireworks
C freezing of water, the evaporation of gasoline and the
rusting of a nail
D sawing of wood, the crushing of a can and the toasting
of a marshmallow
The following items are characteristic properties of the
element Gadolinium:
I.
II.
III.
IV.
V.
melts at –259 C
density of 70.6g/ml at –262oC
colorless, odorless gas
reacts with Cl to form HCl
o
16. Which of the following best describes the air that we
breathe?
A
B
C
D
17. What type of change is shown in the diagram above,
which shows a distillation setup?
A a physical change
B a chemical change
C both a chemical and a physical change
D neither a chemical nor a physical change
rigid, compressible, definite volume
no definite shape, fluid, malleable
no definite volume, incompressible, no definite shape
particles in constant motion, compressible, no definite
shape
discovered in 1880
used in alloys and in making CD’s
silvery-white solid
density of 7.886g/ml
reacts vigorously with air
19. Which of the above properties describe physical
properties of Gadolinium?
A
B
C
D
I, II, III
III, IV, V
III, IV
all are physical properties
Matter Test
27. A horizontal row of blocks in the periodic table is called
a(n)
A. group
B. period
C. family
D. octet
Consider the following list of materials to answer the
question which follows.
I.
II.
III.
IV.
brass
oxygen
copper sulphate solution
solid sodium hydroxide
20. Which of the following statements is correct?
A
B
C
D
I, II and III are pure substances
II and III are pure substances
II and IV are pure substances
II, III and IV are pure substances
A. group
28. Which groups in the periodic table have lower
electronegativity than transition metals?
A. Groups 1 and 2
B. Groups 13 through 18
C. Groups 17 and 18
D. Groups 13 through 17
21. A physical property may be observed by
A melting ice
B letting milk turn sour
C allowing silver to tarnish
D burning wood
30. The idea of arranging the elements in the periodic table
according to their chemical and physical properties is
attributed to
A. Mendeleev.
B. Moseley.
C. Bohr.
D. Ramsay.
22. A physical change occurs when a
A peach spoils.
B copper bowl tarnishes.
C glue gun melts a glue stick.
D bracelet turns your wrist green.
31. The most reactive group of the nonmetals are the
A. lanthanides.
B. transition elements
C. halogens.
D. rare-earth elements.
23. The state of matter in which a material has neither a
definite shape nor a definite volume is the
A gaseous state..
B liquid state.
C elemental state.
D solid state
32. As you move down the periodic table from carbon
through lead, atomic radii
A generally increase.
B generally decrease
C do not change.
D vary unpredictably.
24. A substance classified as a fluid contains particles that
A may slide past each other.
B are held in fixed position.
C quickly expand into any available space.
D are very far from each other.
33. The energy required to remove an electron from an atom
is the atom's
A electron affinity.
B electron attraction.
C electronegativity.
D ionization energy
25. Physical means can be used to separate
A elements.
B pure substances.
C mixtures.
D compounds
34. Elements in a group or column in the periodic table can
be expected to have similar
A atomic masses.
B atomic numbers..
C numbers of neutrons.
D properties.
26. The electrons involved in the formation of a
chemical bond are called
A. valence electrons.
B. dipoles.
C. s electrons
D. Lewis electrons
35. The discovery of the noble gases changed Mendeleev's
periodic table by adding a new
A energy level.
B series.
C group.
D sublevel block
Matter Test
36. The elements in Group 1 are also known as the
A alkali metals
B rare-earth series
C period 1 elements.
D actinide series.
37. Which is the best reason that the atomic radius generally
increases with atomic number in each group of elements?
A The nuclear charge increases.
B The number of neutrons increases.
C The number of energy levels increases
D A new octet forms.
38. The person whose work led to a periodic table based on
increasing atomic number was
A Moseley..
B Mendeleev.
C Rutherford.
D Cannizzaro.
44. The electrons available to be lost, gained, or
shared when atoms form bonds are called…
A ions.
B valence electrons.
C d electrons
D electron clouds
45. How many electrons are in the outer energy
level of all halogens?
A 1
B 6
C 7
D 8
46. Noble gases do not form compounds because ______.
A they do not have any electrons
B they have empty outer energy levels
C they have seven valence electrons
D their valence shells are filled
39. The property most unique to the noble gases is that they
A have low boiling points.
B are radioactive.
C are gases at ordinary temperatures.
D are largely unreactive
40. The principle that states that the physical and chemical
properties of the elements are periodic functions of their
atomic numbers is
A the periodic table.
B the periodic law.
C the law of properties.
D Mendeleev's law.
41. Mendeleev predicted that the spaces in his periodic table
represented
A isotopes.
B radioactive elements
C permanent gaps.
D undiscovered elements.
42. The element that has the greatest electronegativity is
A oxygen.
B sodium.
C. chlorine.
D fluorine.
43. In a row in the periodic table, as the atomic number
increases, the atomic radius generally
A decreases.
B remains constant.
C. increases.
D becomes unmeasurable.
47. According to Bohr, electrons cannot reside at which
location in the figure above?
A point A
B point B
C point C
D point D
48. The family of elements that has two electrons in
its outer energy level is the __________.
A actinides
B alkaline earth metals
C alkali metals
D halogens
49. Consider the following orbital diagram:
__ __ __ __ __
1s 2s
2p
Which rule does this arrangement violate?
A the Aufbau principle
B the Pauli exclusion principle
C Bohr’s postulate
D Hund’s rule
Matter Test
50. Which of the following groups contains
members with similar chemical reactivity?
A Li, Be, C
B Be, Mg, Sr
C Sc, Y, Zr
D C, N, O
56. Atoms are ____ when they are combined.
A at a high potential energy
B more stable
C less stable
D not bound together.
57. A chemical bond resulting from the electrostatic
attraction between positive and negative ions is called a(n)
A dipole bond
B covalent bond.
C ionic bond.
D charged bond.
51. According to the periodic table and the information
above, which element has this electron configuration?
A sodium
B neon
C magnesium
D argon
52. Which of the following is the electron-configuration of
aluminum?
A 1s22s22p63s23p1
B 1s22s22p63s3
C 1s22s23s23p64s1
D 1s22s22p63s23d1
53. A spherical electron cloud surrounding an atomic
nucleus would best represent…
A an s orbital
B a p orbital
C a combination of two different p orbitals
D a combination of an s and a p orbital
54. The principal difference between Bohr's model of the
atom and the quantum model of the atom is that electrons in
the Bohr model…
A move in orbitals of various shapes and energies
B travel around the nucleus of the atom
C move in specific orbits
D exist in a series of spherical orbits of different
energies
55. In a chemical bond, the link between atoms results from
the attraction between electrons and
A isotopes.
B Lewis structures
C nuclei
D van der Waals forces.
58. If two covalently bonded atoms are identical, the bond is
A coordinate covalent
B nonpolar covalent.
C polar covalent.
D nonionic.
59. A ____ shows the types and numbers of atoms joined in
a single molecule of a molecular compound.
A ionic bond
B molecular formula.
C chemical formula.
D covalent bond
60. In many compounds, atoms of main-group elements
form bonds so that the number of electrons in the outermost
energy levels of each atom is
A 10
B 8.
C 6.
D 2
61. What principle states that atoms tend to form
compounds so that each atom can have eight electrons in its
outermost energy level?
A octet rule
B rule of eights
C Avogadro principle
D configuration rule
62. To draw a Lewis structure, one must know the
A ionization energy of each atom.
B number of valence electrons in each atom.
C atomic mass of each atom.
D bond length of each atom.
63. The substance whose Lewis structure shows exactly
three covalent bonds is
A CCl4.
B H2O.
C CH2Cl2.
D NH3
Matter Test
70. Use VSEPR theory to predict the shape of the
hydrosulfuric acid molecule.
A tetrahedral
B linear
C bent
D trigonal planar
71. Predict the formula of the ionic compound formed from
magnesium and oxygen.
A Mg2O
B MgO
C Mg2O2
D MgO2
64. Which of the above is the Lewis structure for carbon
tetraiodide?
A A.
B B
C C
D D
72. Which of the following is the proper name for the
formula MgCl2?
A magnesium dichloride
B magnesium chlorine
C magnesium chloride
D magnesium chlorate
65. Which of the Lewis structures below represents
hydrochloric acid?
73. Which of the following is the proper name for the
formula H2CO3?
A carbonic acid
B carbonous acid
C dihydrogen carbonate
D dihydrogen monocarbon trioxide
66. The chemical formula for an ionic compound represents
the
A simplest ratio of the combined ions that balances total
charges..
B total number of ions in the crystal lattice.
C number of atoms in each molecule.
D number of ions in each molecule.
74. Which of the following is the proper chemical formula
for iron (III) bromide?
A FeBr3
B FeBr2
C IrBr3
D Fe3Br
67. The following molecules contain covalent bonds. The
only polar molecule is
A CH4.
B CCl4.
C CO2.
D NH3.
68. In the electron-sea model of a metallic bond,
A mobile electrons are shared by all the atoms.
B electrons are stationary.
C electrons are bonded to particular positive ions.
D some electrons are valence electrons and some are not.
69. Use VSEPR theory to predict the shape of the
hydrochloric acid molecule.
A tetrahedral
B linear
C bent
D trigonal planar
75. What type of bond is formed by a reaction between one
magnesium atom and two chlorine atoms?
A covalent
B ionic
C metallic
D polar covalent
Matter Test
76. Based on their location on the periodic table, which of
the following pairs of atoms would most likely share
electrons when bonding?
A Al and F
B Ca and I
C Na and Cl
D P and O
77. Based on their location on the periodic table, which of
the following pairs of atoms would most likely form ionic
bonds?
A B and N
B Li and O
C P and Br
D Sn and As
78.
A
B
C
D
Which of the following is a covalent compound?
CCl4
NaCl
Al2O3
AgNO3
79.Which two substances are covalent compounds?
A
B
C
D
KI and H2O
KCl and HCl
NO2 and C6H11O6
KBr and CaCl2
A. 4 bonding pairs, 0 lone pairs
B. 3 bonding pairs, 1 lone pair
C. 2 bonding pairs, 2 lone pairs
D. 1 bonding pair, 3 lone pairs
84. Which of the following does NOT represent a covalent
bond?
A BrCl
B LiCl
C HCl
D S2Cl2
85. Isotopes are atoms of the same element that have
different
A principal chemical properties
B masses.
C numbers of protons.
D numbers of electrons
86. Alpha particles are
A electrons..
B helium nuclei.
C electromagnetic waves.
D neutrons.
88. Balance the following equation:

+ _____
A.
C.
B.
D.
89. Which of the following forms of radiation has the
greatest penetrating power?
A alpha particles
B beta particles.
C gamma rays
D positrons
90. What does the 4 in
Match the molecule with the correct description.
80. ____ NH3
81. ____ H2O
82. ____ CH4
83. ____ HF
87. Gamma rays are
A electrons..
B helium nuclei.
C electromagnetic waves.
D neutrons.
A
B
C
D
represent?
the mass number
the atomic number.
the number of protons
the number of neutrons
91. Dalton's atomic theory helped to explain the law of
conservation of mass because it stated that atoms
A could not combine
B could not be created or destroyed.
C all had the same mass
D were invisible
92. The deflection of cathode rays in Thomson's
experiments was evidence of the ____ nature of electrons.
A wave
B charged
C particle
D spinning
93. Who discovered the nucleus by bombarding gold foil
with positively charged particles and noting that some
particles were widely deflected?
A Rutherford
B Dalton
C Chadwick
D Bohr