WorksheetsChemistry Semester Exam
Total questions: 93
Worksheet time: 47mins
Experimental evidence was a critical factor in developing the atomic model. What is an example of evidence that helped develop the Dalton atomic model?
The path of cathode rays is affected by a magnet.
Alpha particles are deflected at large angles.
Elements give off specific colors of light when heated in a flame.
Elements combine in simple whole-number ratios to form compounds.
The periodic table
permits the properties of an element to be predicted before the element is discovered.
will be completed with element 118.
has been of little use to chemists since the early 1900s.
was completed with the discovery of the noble gases.
Rutherford expected alpha particles to travel almost straight through a target of gold foil. Which concept was not supported by his experimental results and research?
Millikan’s measurement of electrical charge
Thomson’s plum pudding model of the atom
the existence of electrons as particles
the planetary model of the atom
An atom has an atomic number of 26 and a mass number of 56. What is the composition of the atom?
26 protons, 56 neutrons, 26 electrons
30 protons, 26 neutrons, 30 electrons
26 protons, 30 neutrons, 26 electrons
30 protons, 30 neutrons, 26 electrons
The mass of the ashes left from burning a log is less than the mass of the log. Which explains why this is not a violation of the law of conservation of mass?
Some of the mass of the log is converted into energy.
The ashes are made of simpler compounds than were in the log.
New lighter atoms are produced during combustion.
Much of the mass of the log escapes as gases.
An atom has 23 protons and 28 neutrons. Which is the correct chemical symbol for this atom?
5123V
126C
6429Cu
5224Cr
The following symbols represent isotopes of four fictitious elements, W, X, Y, and Z.
Which isotope contains the most neutrons?
Y
W
Z
X
What of the following isotopes have the same number of neutrons?
silver-108, palladium-107, cadmium-109, indium-108, rhodium-108
silver-108, palladium-107, cadmium-109, indium-108
silver-108, indium-108, rhodium-108
silver-108, palladium-107, cadmium-109, indium-108, rhodium-106
silver-108, palladium-107, cadmium-109
A lead atom contains 82 protons and 125 neutrons. Which is the correct notation for this isotope of lead?
What many electrons can a each p-orbital accommodate?
4
6
2
10
The image below shows the order of filling sublevels in the atom. An atom of the element phosphorus contains 15 electrons. Which sublevel is partially filled?
3p
4p
2s
4d
Which is the correct ground state electron configuration for the element arsenic?
1s22s22p63s23p64s24d104p3
1s22s22p63s23p64s23d104p4
1s22s22p63s23p64s23d104p3
1s22s22p63s23p64s23d104p1
How many valence electrons does the element sulfur have?
4
2
14
6
The image below shows an orbital diagram for magnesium.
Which rule for filling orbital diagrams is violated in this diagram?
Heisenberg uncertainty principle
Pauli exclusion principle
Hund's rule
Aufbau principle
Which set of elements is in order from least to most valence electrons?
Ca, K, Cl, Ar
Ne, F, O, B
K, As, Br, Kr
C, B, Be, Li
Which is the ground state electronic configuration of an alkaline earth metal?
1s2 2s2 2p6 3s2 3p6 4s2
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
1s2 2s2 2p6 3s2 3p6 4s2 3d2
1s2 2s2 2p6 3s2 3p6 4s1
The image below shows the order of filling sublevels in the atom.
Which sublevels must be filled before the 3d sublevel will accept an electron?
1s, 2s
1s, 2s, 2p, 3s, 3p, 4s
1s, 2s, 2p, 3s
1s, 2s, 2p, 3s, 3p
Which best explains how the Heisenberg uncertainty principle helped make the Bohr model of the atom incorrect?
The Bohr model did not allow for sublevels of energy.
Assigning the electron to a fixed path around the nucleus is impossible.
The interaction of an electron and a photon of light changes the speed and position of the electron.
The electron's velocity at any given moment cannot be determined.
The Bohr model of the atom was replaced by the quantum mechanical model in which electrons occupy orbitals like the one shown in the image below. What is NOT true about this orbital?
There is a 90% probability of finding the electron within the orbital.
The electron follows specific paths within the orbital.
Spherical orbitals, like this one exist in every energy level in the atom.
The probability of finding the electron close to the nucleus is high.
According to modern periodic law, what property is used as a basis to organize elements into a regular pattern?
atomic mass
atomic number
periodicity
density
What are the valence electrons in the electron configuration of tin, [Kr]4d105s25p2?
[Kr]
5s25p2
4d10
5p2
How many valence electrons does a silicon atom have?
6
2
1
4
In which region of the periodic table do all the elements have 3 electrons in the highest p orbital?
A
B
C
D
Which element has the following electron configuration?
[Ne] 3s2 3p6 4s2 3d1
titanium
calcium
yttrium
scandium
Which entity does NOT have the electron configuration [Ar]4s23d104p6
As3+
Br−
Kr
Sr2+
How do ionic radii compare from top to bottom in a group of the periodic table.
decrease
increase
stay the same
follow no pattern
Which diagram correctly depicts the general trend in first ionization energy?
Identify the element the highest electronegativity from the list of electron configurations given below:
[Ne] 3s23p4
[Ne] 3s23p5
[Ne] 3s23p3
[Ar] 4s2
Which of these is true about the oxidation numbers (charges) of transition metals, such as chromium?
oxidation number always equals to 2+
can have multiple positive oxidation numbers
can have multiple negative oxidation numbers
oxidation number always equals to 1+
The electron structure of a neutral atom is shown below. Which notation correctly labels an ion that would form from this atom?
Mg+
Na-
Ne−
Na+
The image below shows an orbital diagram for phosphorus. Which rule for filling orbital diagrams is violated in this diagram?
Aufbau principle
Paul exclusion principle
Hund's rule
Heisenberg uncertainty principle
What is the formula for the compound consisting of cesium and sulfate ions?
Cs2SO4
CsSO
Cs2SO
Cs4SO2
An atom of magnesium has two valence electrons. An atom of magnesium will most likely react with exactly one atom of which element?
carbon
chlorine
oxygen
nitrogen
To achieve a noble gas configuration, how many electrons does Fluorine need to gain?
1
2
3
0
1A : 2G
1A : 1G
No likely combination
2A : 1G
Which of these formulas is written incorrectly?
Aluminum Hydroxide
AlOH3
Calcium Hydroxide
Ca(OH)2
Ammonium Sulfide
(NH4)2S
Aluminum Sulfate
Al2(SO4)3
What is the name of the compound Be(NO3)2?
beryllium dinitrate
beryllium(II) nitrate
beryllium(II) dinitrate
beryllium nitrate
Which is the correct formula for the compound, manganese(III) fluoride?
MnF3
MnF
Mn3F3
Mn3F
What is the name of the compound whose formula is Na3P?
sodium phosphide
sodium(III) phosphide
sodium phosphite
sodium phosphate
What is the formula of calcium bromide?
Ca2Br2
Ca2Br
CaBr
CaBr2
What is the formula for the compound formed by calcium ions and chloride ions?
CaCl
Ca2Cl
CaCl3
CaCl2
What is the formula for the compound formed by lead(II) ions and chromate ions?
PbCrO4
Pb2CrO4
Pb2(CrO4)3
Pb(CrO4)2
What is the formula for aluminum sulfate?
AlSO4
Al2SO4
Al2(SO4)3
Al(SO4)3
What is the formula for barium hydroxide?
BaOH
BaOH2
Ba(OH)2
Ba(OH)
Name the compound Ni(ClO3)2
nickel(II) chlorate
nickel(II) chloride
nickel(II) chlorite
nickel(II) peroxide
Name the compound Zn3(PO4)2
zinc potassium oxide
trizinc polyoxide
zinc phosphate
zinc phosphite
What charge do Group 13 elements tend to acquire when they form ions?
3−
5−
5+
3+
In groups 13 through 18, valence electrons may be in sublevels
s and d.
s and p.
d and f.
p and d.
Among the d-block elements, as atomic radii decrease, electronegativity values
remain constant.
increase.
decrease.
drop to zero.
The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to
Mendeleev.
Moseley.
Bohr
Ramsay
What is the formula for sulfur dichloride?
SCl
SCl2
S2Cl
S2Cl2
What is the formula for dinitrogen trioxide?
Ni2O3
NO3
N2O6
N2O3
Name the compound N2O3
dinitrogen oxide
nitrogen trioxide
nitric oxide
dinitrogen trioxide
The electron configurations of the noble gases from neon to radon in the periodic table make these elements part of the
f block.
d block.
s block.
p block.
Elements in which the d-sublevel is being filled have the properties of
metals.
nonmetals.
metalloids.
gases
Name the compound SiO2
silver oxide
silicon oxide
silicon dioxide
monosilver dioxide
Name the compound CF4
calcium fluoride
carbon fluoride
carbon tetrafluoride
monocalcium quadrafluoride
Name the compound Al2S3
aluminum sulfate
aluminum sulfur
aluminum(II) sulfate
aluminum sulfide
Name the compound Fe(NO3)2
iron(II) nitrate
iron(II) nitrite
iron(III) nitrate
iron(III) nitride
What is the formula for zinc fluoride?
ZnF
ZnF2
Zn2F
Zn2F3
Name the compound KClO3
potassium chloride
potassium trioxychlorite
potassium chlorate
hypochlorite
Argon, krypton, and xenon are
alkaline earth metals.
noble gases.
actinides.
lanthanides.
Chlorine has atomic number 17 and mass number 35. It has
17 protons, 17 electrons, and 18 neutrons.
35 protons, 35 electrons, and 17 neutrons.
17 protons, 17 electrons, and 52 neutrons.
18 protons, 18 electrons, and 17 neutrons.
Identify the number of neutrons in one atom of sulfur with an atomic mass number of 34 amu.
16
18
32
34
Elaborate on the nuclear model of the atom.
The nuclear model describes the atom as protons and neutrons distributed throughout a sea of electrons.
The nuclear model describes the atom as electrons uniformly scattered in a positive cloud of protons.
The nuclear model describes the atom as a small, negative center enveloped by a cloud of positive particles.
The nuclear model describes the atom as a dense, positive nucleus surrounded by a cloud of negative electrons.
The atomic number of an element is
the mass of the element.
1 mol of the element.
the number of protons in each atom of the element.
the number of neutrons in each atom of the element.
Because a few alpha particles bounced back from the foil, Rutherford concluded that they were
striking electrons.
indivisible.
repelled by densely packed regions of positive charge.
magnetic.
In 1911, Ernest Rutherford conducted his now famous goldfoil experiment. During the experiment, alpha particles bombarded a thin piece of gold foil. The alpha particles were expected to pass easily through the gold foil. Every now and then, however, an alpha particle bounced back—an unexpected result. Rutherford concluded that these particles were striking....
a tiny region of positive charge.
a dense region of negative charge.
a dense region of neutrons.
a tiny region with a strong magnetic field.
The isotope uranium-235 has 92 protons and 143 neutrons. Therefore, its mass number is
92
235
143
Mass number is...
the average atomic mass of an element.
the total number of electrons in an atom of an element.
the total number of protons in an atom of an element.
the total number of protons and neutrons in an atom of an element.
Isotopes are atoms of the same element that have different
masses
charges
number of electrons
atomic numbers
The atomic number of an element is
the mass of the element.
1 mol of the element.
the number of protons in each atom of the element.
the number of neutrons in each atom of the element.
Which of the following states an important result of Rutherford’s gold-foil experiment?
Atoms have mass.
Electrons have a negative charge.
Neutrons are uncharged particles.
The atom has a nucleus
When an electrical current passed through a glass tube, it caused the surface of the tube directly across from the cathode to glow. Scientists concluded that
a magnetic field was produced.
the particles of the beam were negatively charged.
there was gas in the tube.
atoms were indivisible.
The principles of atomic theory recognized today were conceived by
Avogadro.
Bohr.
Dalton.
Rutherford
The electron notation for aluminum (atomic number 13) is
1s2 2s2 2p3 3s2 3p3 3d1
1s2 2s2 2p6 3s2 2d1
1s2 2s2 2p6 3s2 3p1
1s2 2s2 2p9
What is the electron configuration for nitrogen, atomic number 7?
1s2 2s2 2p3
1s2 2s3 2p2
1s2 2s3 2p1
1s2 2s2 2p2 3s1
The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
Mg (Z = 12).
C (Z = 6).
S (Z = 16).
Si (Z = 14).
In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?
3d1 4s2
4s3
3d3
4s2 4p1
The atomic sublevel with the next highest energy after 4p is
4d.
4f.
5p
5s.
How many electrons can occupy the s orbitals at each energy level?
two, if they have opposite spins
two, if they have the same spin
one
no more than eight
The number of orbitals for the d sublevel is
1.
3.
5.
7.
The letter designations for the first four sublevels with the maximum number of electrons that can be accommodated in each sublevel are
s:2, p:4, d:6, and f:8.
s:1, p:3, d:5, and f:7.
s:2, p:6, d:10, and f:14.
s:1, p:2, d:3, and f:4.
An orbital that can never exist according to the quantum description of the atom is
3d.
8s.
6d.
3f.
The major difference between a 1s orbital and a 2s orbital is that
the 2s orbital can hold more electrons.
the 2s orbital has a slightly different shape.
the 2s orbital is at a higher energy level.
the 1s orbital can have only one electron.
The discovery of what elements added a new column to Mendeleev's periodic table?
noble gases
radioactive elements
transition elements
metalloids
The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called
d orbitals.
f orbitals.
p orbitals.
s orbitals.
The change of an atom from an excited state to the ground state always requires
absorption of energy.
emission of electromagnetic radiation.
release of visible light.
an increase in electron energy.
The emission of electrons from metals that have absorbed photons is called the
interference effect.
photoelectric effect.
quantum effect.
dual effect.
The energy of a photon is related to its
mass.
speed.
frequency.
size.
The frequency of electromagnetic radiation is measured in waves/second, or
nanometers.
quanta.
hertz.
joules.
Match the model and the scientist.
Billiard ball model
John Dalton
Plum Pudding Model
J.J. Thomson
Nuclear model
Ernest Rutherford
Planetary model
Niels Bohr
Electron Cloud model
Einstein, Heisenburg, Hund
Which scientist developed this model?
Dalton
Thomson
Rutherford
Bohr
