CP CHEMISTRY HALF YEAR ASSESSMENT REVIEW TOPICS AND PROBLEMS
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Multiple Choice and Problems
STEPS OF SCIENTIFIC METHOD IN ORDER
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 1.
a. 2
b. 13
Group ____ in the figure above contains only metals.
c. 17
d. 18
____ 2.
Based on their location in the figure above, oxygen and selenium have
a. the same number of neutrons.
c. similar properties.
b. the same conductivity.
d. the same number of electron orbitals.
____ 3.
a. 13
b. 14
What is the atomic number for aluminum from the figure above?
c. 26.98
d. 26.9815
____ 4.
In the figure above, a neutral atom of silicon contains
a. 14 electrons.
c. 16 electrons.
b. 28.09 electrons.
d. 38 electrons.
____ 5.
The most useful source of chemical information about the elements is a
a. calculator.
c. periodic table.
b. table of metric equivalents.
d. table of isotopes.
____ 6.
a. group.
b. period.
A horizontal row of blocks in the periodic table is called a(n)
c. family.
d. octet.
____ 7.
a. group.
A vertical column of blocks in the periodic table is called a(n)
c. property.
b. period.
____ 8.
a. inactive.
b. metals.
d. octet.
The elements that border the zigzag line in the periodic table are
c. metalloids.
d. nonmetals.
____ 9.
Which is NOT a property of metals?
a. malleability
c. unreactivity
b. ability to conduct heat and electricity
d. tensile strength
____ 10.
Which statement is NOT true of nonmetals?
a. They have characteristics of both metals and nonmetals.
b. Many are gases at room temperature.
c. They have low conductivity.
d. There are fewer nonmetals than metals.
____ 11.
All of the following are steps in the scientific method EXCEPT
a. observing and recording data.
b. forming a hypothesis.
c. discarding data inconsistent with the hypothesis.
d. developing a model.
____ 18.
Who was the schoolmaster who studied chemistry and proposed an atomic theory?
a. John Dalton
c. Robert Brown
b. Jons Berzelius
d. Dmitri Mendeleev
____ 19.
Which of the following is NOT part of Dalton's atomic theory?
a. Atoms cannot be divided, created, or destroyed.
b. The number of protons in an atom is its atomic number.
c. In chemical reactions, atoms are combined, separated, or rearranged.
d. All matter is composed of extremely small particles called atoms.
____ 20.
Which of the following statements is true?
a. Atoms of the same element may have different masses.
b. Atoms may be divided in ordinary chemical reactions.
c. Atoms can never combine with any other atoms.
d. Matter is composed of large particles called atoms.
____ 21.
a. proton.
b. nucleus.
Experiments with cathode rays led to the discovery of the
c. neutron.
d. electron.
____
22.
Who discovered the nucleus by bombarding gold foil with positively charged particles and noting
that some particles were widely deflected?
a. Rutherford
c. Chadwick
b. Dalton
d. Bohr
____
23.
a(n)
a. nuclide.
b. neutron.
A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called
c. electron.
d. isotope.
____ 24.
The nucleus of an atom has all of the following characteristics EXCEPT that it
a. is positively charged.
c. contains nearly all of the atom's mass.
b. is very dense.
d. contains nearly all of the atom's volume.
____
25.
a. Nucleus
b. Electron
Which part of an atom has a mass approximately equal to 1/2000 of the mass of a common
hydrogen atom?
c. proton
d. electron cloud
____ 26.
The mass of a neutron is
a. about the same as that of a proton.
b. about the same as that of an electron.
c. double that of a proton.
d. double that of an electron.
____ 27.
The nucleus of most atoms is composed of
a. tightly packed protons.
c. tightly packed protons and neutrons.
b. tightly packed neutrons.
d. loosely connected protons and electrons.
____ 28.
Protons have
a. negative charges.
b. an attraction for neutrons.
c. no charges.
d. no mass.
____ 29.
An atom is electrically neutral because
a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.
____ 30.
a. nucleus.
b. nuclides.
Most of the volume of an atom is occupied by the
c. electron cloud.
d. protons.
____ 31.
The charge on the electron cloud
a. prevents compounds from forming.
b. balances the charge on the nucleus.
c. attracts electron clouds in other atoms to form compounds.
d. does not exist.
____
32.
The smallest unit of an element that can exist either alone or in combination with other such
particles of the same or different elements is the
a. electron.
c. neutron.
b. proton.
d. atom.
____ 33.
Isotopes are atoms of the same element that have different
a. principal chemical properties.
c. numbers of protons.
b. masses.
d. numbers of electrons.
____ 34.
a. moles.
b. isotopes.
Atoms of the same element that have different masses are called
c. nuclides.
d. neutrons.
____ 35.
a. electrons.
b. protons.
Isotopes of an element contain different numbers of
c. neutrons.
d. nuclides.
____ 36.
Helium-4 and helium-3 are
a. isotopes.
b. different elements.
c. compounds.
d. nuclei.
____ 37.
Isotopes of each element differ in
a. the number of neutrons in the nucleus.
b. atomic number.
c. the number of electrons in the highest energy level.
d. the total number of electrons.
____ 38.
The atomic number of oxygen, 8, indicates that there are eight
a. protons in the nucleus of an oxygen atom.
b. oxygen nuclides.
c. neutrons outside the oxygen atom's nucleus.
d. energy levels in the oxygen atom's nucleus.
____ 39.
In determining atomic mass units, the standard is the
a. C-12 atom.
c. H-1 atom.
b. C-14 atom.
d. O-16 atom.
____ 40.
The atomic mass listed in the periodic table is the
a. average atomic mass.
b. relative atomic mass of the most abundant isotope.
c. relative atomic mass of the most stable radioactive isotope.
d. mass number of the most abundant isotope.
____ 41.
A neutral carbon atom (atomic number 6) has
a. 3 electrons and 3 neutrons.
c. 3 protons and 3 electrons.
b. 6 protons.
d. 3 protons and 3 neutrons.
____ 42.
Chlorine has atomic number 17 and mass number 35. It has
a. 17 protons, 17 electrons, and 18 neutrons.
b. 35 protons, 35 electrons, and 17 neutrons.
c. 17 protons, 17 electrons, and 52 neutrons.
d. 18 protons, 18 electrons, and 17 neutrons.
____ 43.
Nickel-60 (atomic number 28) has
a. 28 neutrons.
c. 60 neutrons.
b. 32 neutrons.
d. 88 neutrons.
____ 44.
Silicon-30 contains 14 protons. It also contains
a. 16 electrons.
c. 30 neutrons.
b. 16 neutrons.
d. 44 neutrons.
____ 45.
Neon-22 contains 12 neutrons. It also contains
a. 12 protons.
c. 22 electrons.
b. 22 protons.
d. 10 protons.
____ 46.
One of the wave properties of electromagnetic radiation, such as light, is
a. volume.
c. mass.
b. frequency.
d. weight.
____ 48.
A line spectrum is produced when an electron moves from one energy level
a. to a higher energy level.
b. to a lower energy level.
c. into the nucleus.
d. to another position in the same sublevel.
____ 49.
For an electron in an atom to change from the ground state to an excited state,
a. energy must be released.
b. energy must be absorbed.
c. radiation must be emitted.
d. the electron must make a transition from a higher to a lower energy level.
____ 50.
If electrons in an atom have the lowest possible energies, the atom is in the
a. ground state.
c. excited state.
b. inert state.
d. radiation-emitting state.
____ 51.
The part of the atom where the electrons CANNOT be found is the
a. area surrounding the nucleus.
c. electron cloud.
b. nucleus.
d. orbitals.
____ 52.
a. charge.
b. mass.
The size and shape of an electron cloud are most closely related to the electron's
c. spin.
d. energy.
____
a.
b.
c.
d.
53.
With the quantum model of the atom, scientists have come to believe that determining an electron's
exact location around the nucleus
is impossible.
can be done before 2005.
can be done easily.
can be done only with specialized equipment.
____ 54
All of the following describe the Heisenberg uncertainly principle EXCEPT
a. it states that it is impossible to determine simultaneously both the position and velocity of
an electron or any other particle.
b. it is one of the fundamental principles of our present understanding of light and matter.
c. it helped lay the foundation for the modern quantum theory.
d. it helps to locate an electron in an atom.
____ 55.
A three-dimensional region around a nucleus where an electron may be found is called a(n)
a. spectral line.
c. orbital.
b. electron path.
d. orbit.
____ 56.
Unlike in an orbit, in an orbital
a. an electron's position cannot be known precisely.
b. an electron has no energy.
c. electrons cannot be found.
d. protons cannot be found.
____
a. 1
b. 2
57.
How many quantum numbers are needed to describe the energy state of an electron in an atom?
c. 3
d. 4
____ 58.
Quantum numbers are sets of numbers that describe the properties of
a. the atomic nucleus.
c. atoms.
b. atomic orbitals.
d. molecules.
____ 59.
The spin quantum number of an electron can be thought of as describing
a. the direction of electron spin.
b. whether the electron's charge is positive or negative.
c. the electron's exact location in orbit.
d. the number of revolutions the electron makes about the nucleus per second.
____ 60.
a. Spin
b. Stability
An electron for which n = 4 has more ____ than an electron for which n = 2.
c. energy
d. wave nature
____ 61.
a. 3d.
b. 8s.
An orbital that could never exist according to the quantum description of the atom is
c. 6d.
d. 3f.
____ 62.
The letter designations for the first four sublevels with the number of electrons that can be
accommodated in each sublevel are
a. s:1, p:3, d:10, and f:14.
c. s:2, p:6, d:10, and f:14.
b. s:1, p:3, d:5, and f:7.
d. s:1, p:2, d:3, and f:4.
____ 63.
The statement that an electron occupies the lowest available energy orbital is
a. Hund's rule.
c. Bohr's law.
b. the Aufbau principle.
d. the Pauli exclusion principle.
____ 64.
The Aufbau principle states that an electron
a. can have only one spin number.
b. occupies the lowest available energy level.
c. must be paired with another electron.
d. must enter an s orbital.
____ 65.
The Pauli exclusion principle states that no two electrons in the same atom can
a. occupy the same orbital.
c. have the same set of quantum numbers.
b. have the same spin quantum numbers.
d. be at the same main energy level.
____ 66.
The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a. Mg (Z = 12).
c. S (Z = 16).
b. C (Z = 6).
d. Si (Z = 14).
____ 67.
What is the electron configuration for nitrogen, atomic number 7?
a. 1s2 2s2 2p3
c. 1s2 2s3 2p1
2
3
2
b. 1s 2s 2p
d. 1s2 2s2 2p2 3s1
____ 68.
An element with 8 electrons in its highest main energy level is a(n)
a. octet element.
c. Aufbau element.
b. third period element.
d. noble gas.
____
69.
The idea of arranging the elements in the periodic table according to their chemical and physical
properties is attributed to
a. Mendeleev.
c. Bohr.
b. Moseley.
d. Ramsay.
____ 70.
Mendeleev left spaces in his periodic table and predicted several elements and their
a. atomic numbers.
c. properties.
b. colors.
d. radioactivity.
____ 71.
Mendeleev's table was called periodic because the properties of the elements
a. showed no pattern.
b. occurred at repeated intervals called periods.
c. occurred at regular time intervals called periods.
d. were identical.
____ 76.
Argon, krypton, and xenon are
a. alkaline earth metals.
c. actinides.
b. noble gases.
d. lanthanides.
___
77.
In the modern periodic table, elements are ordered according to
a. decreasing atomic mass.
c. increasing atomic number.
b. Mendeleev's original design.
d. the date of their discovery.
____ 79.
a. group.
b. period.
A horizontal row of blocks in the periodic table is called a(n)
c. family.
d. octet.
____ 82.
Elements in which the d-sublevel is being filled have the properties of
a. metals.
c. metalloids.
b. nonmetals.
d. gases.
____ 83.
1) 1
2) 2
3) 3
4) 4
For the next 3 questions: An atom has 16 electrons and 19 neutrons.
____ 137. What is the atomic number of this atom?
1) 3
2) 16
3) 17
4) 19
5) 5
5) 35
____ 138. How many energy levels contain one or more electrons in this atom?
1) 3
2) 5
3) 8
4) 9
____ 139. Find the number of orbitals that contain one or more electrons in this atom.
1) 5
2) 7
3) 9
4) 16
140.What is the wavelength of electromagnetic radiation which has a frequency of 4.464 x 1014 s-1?
a. 1.338 x 1023 m
b. 1.489 x 10-6 m
c. 6.716 x 10-7 nm
d. 671.6 nm
e. 7.472 x 10-15 nm
____
____
141. What is the wavelength of electromagnetic radiation which has a frequency of 5.732 x 1014 s-
?
a. 1.718 x 1023 m
b. 1.912 x 106 m
c. 5.230 x 10-7 m
d. 523.0 m
e. 5.819 x 10-15 nm
1
142. Calculate the frequency of visible light having a wavelength of 464.1 nm
a. 139.1 s-1
b. 1.548 x 10-6 s-1
c. 1.548 x 10-15 s-1
d. 6.460 x 1014 s-1
e. 6.460 x 105 s-1
____
143. A police radar unit is operating on a frequency of 9.527 Gigahertz. What is the wavelength of
the radiation being employed?
a. 314.7 nm
b. 314.7 m
c. 3.147 cm
d. 314.7 cm
e. 31.78 m
____
144. Which one of the following types of radiation has the lowest frequency?
a. FM radio waves
b. infrared radiation
c. microwave radiation
d. x-rays
e. ultraviolet rays
____
145. Which one of the following types of radiation has the highest frequency?
a. blue visible light
b. FM radio
c. infrared radiation
d. microwave radiation
e. short wave radio waves
____
146. Which one of the following types of radiation has the highest frequency?
a. x-rays
b. ultraviolet rays
c. FM radio waves
d. microwave radiation
e. infrared radiation
____
147. Which one of the following types of radiation has the shortest wavelength?
a. FM radio waves
b. infrared radiation
c. microwave radiation
d. ultraviolet rays
e. x-rays
____
148. Which one of the following types of radiation has the longest wavelength?
a. gamma rays
b. green colored visible light rays
c. red colored visible light rays
____
d. ultraviolet rays
e. x-rays
149. What is the energy, in joules, of one photon of microwave radiation with a wavelength of
0.158 m?
a. 1.26 x 10-24 J
b. 3.14 x 10-26 J
c. 3.19 x 1025 J
d. 3.49 x 10-43 J
e. 7.15 x 1040 J
____
____
150. What is the energy, in joules, of one photon of visible radiation with a wavelength of 464.1
nm?
a. 1.026 x 10-48 J
b. 2.100 x 1035 J
c. 2.341 x 1011 J
d. 4.280 x 10-19 J
e. 4.280 x 10-12 J
151. What is the wavelength, in nm, of radiation which has an energy of 3.371 x 10-19 joules per
photon?
a. 655.9 nm
b. 152.5 nm
c. 170.0 nm
. 589.3 nm
e. 745.1 nm
____
152. What is the frequency, in sec-1, of radiation which has an energy of 219.1 kJ per mole (of
these photons)?
a. 615.9 x 1014 sec-1
b. 1.624 x 1014 sec-1
c. 1.058 x 10-10 sec-1
d. 5.491 x 1014 sec-1
e. 3.588 x 10-19 sec-1
____
153. The definite energies associated with specific wavelengths in the emission spectrum of
atomic hydrogen suggest that
a. electrons have a smaller rest mass than photons
b. photons have a smaller rest mass than electrons
c. energy states in the hydrogen atom are quantized
d. atomic hydrogen is more stable and has a lower potential energy than molecular hydrogen
e. the potential energy of electrons in the atom can have any arbitrary value over a period of time, but the
kinetic energy may only have certain specific values
____