1301 TEST 1 – REVIEW SHEET
You need to read chapters 1 through 4 All is fair game unless I announce otherwise on Wednesday before the test.
Introductory Stuff
Know history, types of matter
Scientific Method
Know terms
Atoms and Molecules;
elements and compounds – know the definitions. Understand formulas
Dalton’s Theory
Know the parts of it and the laws it explained
1.
Which of the following is an example of heterogeneous matter?
(A)
Coffee
2.
(B)
Diamond
(C)
Wood
(D)
Air
Which of the following is an example of homogeneous matter?
(A)
(C)
Seawater (assume no particulates)
Earth's atmosphere (assume no particulates)
3.
Which of the following Greek philosophers developed a theory of matter based upon small, but indivisible,
pieces?
(A)
Socrates
4.
Which assumption of Dalton’s atomic theory had to be revised or discarded because of the existence of
stable isotopes?
(A)
(B)
(C)
(D)
The ultimate particles of matter are the atoms of elements, which are indivisible and indestructible.
All the atoms of a given element are alike in all respects.
The atoms of different elements differ in one or more properties.
Compounds are formed by combination of different kinds of atoms.
5.
Which of the following is a pure, elemental substance?
(A)
Br2
(B)
(B)
Democritus
SO2
(B)
(D)
(C)
(C)
Bronze (an alloy of copper and tin)
All of the above are homogeneous mixtures
Aristotle
H2O
(D)
(D)
Plato
H2O2
Structure of an atom:
Protons, neutrons and electrons:
protons same as atomic number (from Periodic Table)
Electrons same as protons in neutral atom
Mass (written in top left hand corner) – protons + neutrons
Isotopes
General structure:
Protons and Neutrons in nucleus (Rutherford’s expt.)
Electrons round outside
6.
The first scientist to propose that the atom had a dense nucleus which occupied only a small fraction of the
volume of the atom was
(A)
Heisenberg
(B)
Bohr.
(C)
De Broglie
1
(D)
Rutherford.
7.
When alpha particles were shot at a gold foil target, most of the particles were undeflected. This indicated
to Rutherford that
(A)
(C)
(E)
the gold foil was continuous matter.
(B)
the mass of the gold atoms was spread out thinly.
the atoms of gold were mostly empty space.
(D)
the alpha particles had great penetrating power.
the alpha particles had charges opposite to those on the nuclei
8.
According to the experiments of Ernest Rutherford, where can a majority of a given atom's mass be found?
(A)
(B)
(C)
(D)
Scattered randomly throughout an approximately cube-shaped atom
At the center of an approximately spherical atom
In concentric layers of spherical shape
As small pieces orbiting a common center in circular paths
9.
The structure of individual atoms can roughly be described as:
(A)
(B)
(C)
(D)
A massive, positively charged center and mostly empty space
An even mixture of mass and charge scattered throughout a spherical shape
Positively charged, low-mass pieces in orbit around a massive, negatively charged center
Massive, positively charged pieces in orbit around a low-mass, negatively charged center
10.
The number of neutrons in the nucleus of a specific atom is equal to its
(A) atomic mass.
(B) mass number.
(C) atomic number.
(D)
mass number - atomic number.
11.
In all neutral atoms, there are equal numbers of
(A)
(B)
protons and neutrons.
positrons and electrons.
12.
Which statement concerning the structure of the atom is correct?
(A)
(B)
(C)
(D)
Protons and neutrons have most of the mass and occupy most of the volume of the atom.
Electrons have most of the mass and occupy most of the volume of the atom.
Electrons have most of the mass but occupy very little of the volume of the atom.
Protons and neutrons have most of the mass but occupy very little of the volume of the atom.
13.
Which statement is true?
(A)
(B)
(C)
(D)
The nucleus of an atom contains neutrons and electrons.
The atomic number of an element is the number of protons in one atom.
The mass number of an atom is the number of protons in the nucleus plus the number of electrons.
The number of electrons outside the nucleus is the same as the number of neutrons in the nucleus.
14.
How is the term "mass number" defined for a given atom or isotope?
(A)
(B)
(C)
(D)
As the mass of one mole of that element or isotope
As the sum of the protons, neutrons, and electrons it contains
As the sum of the protons and neutrons its nucleus contains
As the number of protons its nucleus contains
(C)
(D)
neutrons and electrons.
electrons and protons.
2
15.
How many neutrons does the nucleus of the phosphorus-32 isotope have?
(A)
15
16.
An atom of strontium–90 (90Sr) contains
(B)
16
(C)
(A) 38 electrons, 38 protons, 52 neutrons.
(C) 52 electrons, 52 protons, 38 neutrons.
17.
17
(D)
32
(B) 38 electrons, 38 protons, 90 neutrons.
(D) 52 electrons, 38 protons, 38 neutrons.
Select the answer that lists the correct atomic number, number of neutrons and mass number for 80Br
(A) 45, 80, 35
(B) 80, 46, 35
(C) 35, 45, 80
18.
1 2
3
The species 1H, 1H, and 1H represent three
(A)
allotropes.
19.
Elemental tin has several isotopes. All of them have the same:
(A)
(D)
number of protons
number of neutrons
(B)
isomers.
(B)
(E)
(C)
(D) 35, 80, 45
homologs.
(D)
total number of neutrons and protons
total number of neutrons and electrons
(E) 35, 46, 81
isotopes.
(C)
mass number
Periodic Table
Atom types arranged by order of atomic number
Things in groups have similar properties
Mass is weighted related mass = [(mass of isotope 1 x % of 1) + (mass of 2 x % of 2)… ] /100
Know first 36 names/symbols. Know special groups:
1st = alkali metals (e. g. Na)
last = noble gases (e. g. He)
4th to last = pnictogens (e. g. N)
2nd = alkaline earth metals (e. g. Mg)
2nd to last = halogens (e. g. Cl)
20.
What is the name given to the element with the symbol "P"?
(A)
Polonium
21.
What is the name of the element whose symbol is "Co" ?
(A)
Carbon
22.
By what chemical symbol do we know the element chromium?
(A)
Cr
23.
What chemical symbol has been given to the element sodium?
(A)
S
(B)
(B)
(B)
(B)
Protactinium
Chromium
Co
K
(C)
(C)
(C)
(C)
Phosphorus
Coal
C
Na
3
middle block = transition metals
3rd to last = chalcogens (e. g. O)
(D)
Palladium
(D)
Cobalt
(D)
Cs
(D)
Sr
24.
Which of the following elements are largely unreactive substances?
(A)
alkali metals
25.
Which of the following is a non-metal?
(A)
lithium
26.
Which of the following is a metal?
(A)
nitrogen
27.
Which of the following is a metalloid?
(A)
carbon
28.
A column of the periodic table is called a
(A)
group
29.
A row of the periodic table is called a
(A)
group
30.
What name is commonly given to the elements of Group IA of the periodic table?
(A)
Alkaline earth metals
31.
Lithium forms compounds which are used in dry cells and storage batteries and in high-temperature
lubricants. It has two naturally occurring isotopes, 6Li (isotopic mass = 6.015121 amu) and 7Li (isotopic
mass = 7.016003 amu). Lithium has an atomic mass of 6.9409 amu. What is the percent abundance of
lithium-6?
(A)
86.66%
32.
Silicon, which makes up about 25% of Earth’s crust by mass, is used widely in the modern electronics
industry. It has three naturally occurring isotopes, 28Si, 29Si, and 30Si. Calculate the atomic mass of silicon.
Isotope
28
Si
29
Si
30
Si
(A)
(B)
(B)
(B)
(B)
(B)
(B)
(B)
noble gases
bromine
phosphorus
sulfur
period
period
(B)
29.2252 amu
(B)
halogens
(D)
alkaline earth metals
(C)
mercury, Hg
(D)
bismuth, Bi
(C)
arsenic
(D)
thallium, Tl
(C)
germanium
(D)
iridium, Ir
(C)
isotopic mixture
(D)
pillar
(C)
isotopic mixture
(D)
family
Transition metals
46.16%
Isotopic Mass (amu)
27.976927
28.976495
29.973770
(C)
(C)
(C)
7.503%
halogens
(D)
(D)
Alkali metals
6.080%
Abundance %
92.23
4.67
3.10
28.9757 amu
(C)
28.7260 amu
(D)
28.0855 amu
Stuff about light:
33
Select the arrangement of electromagnetic radiation which goes from lowest energy to greatest energy.
(A)
(C)
radio, visible, infrared, ultraviolet
visible, ultraviolet, infrared, gamma rays
(B)
(D)
4
microwave, infrared, visible, ultraviolet
X-radiation, visible, infrared, microwave
34.
Select the arrangement of electromagnetic radiation which goes from lowest to highest wavelength
(A)
(C)
radio, infrared, ultraviolet, gamma rays
gamma rays, infrared, radio, ultraviolet
35.
Calculate the energy in joules of microwave radiation of wavelength 12.7 centimeters (h = 6.63 x 10-34 J
sec; speed of light = 3 x 108 meters/sec.)
(A)
4.87 x 1019 J
(B)
(B)
(D)
7.30 x 10-19 J
(C)
radio, ultraviolet, infrared, gamma rays
gamma rays, ultraviolet, infrared, radio
3.61 x 10-18 J
(D)
1.56 x 10-24 J
Bohr Model for the Atom
Atomic Spectra only lines
Specific Energies
Quantized energy levels, explained by ORBITS. THINK OF ORBITS AS “SHELLS”with a maximum number of
electrons = 2n2
Quantum
Electrons considered waves or particles. DE BROGLIE.
Heisenberg – can’t know position and energy/velocity etc
ORBITALS – where electrons probably are
Defined by
SHELLS
split into n SUBSHELLS
which split into ORBITALS
SUBSHELLS
s
p
d
f
contain
contain
contain
contain
1 s orbital
3 p orbitals
5 d orbitals
7 f orbitals
36.
The scientist who was first to propose that electrons in an atom could have only certain energies was
(A)
Heisenberg
37.
The concept that particles of matter could have wave properties was proposed by
(A)
Heisenberg
38.
The principle which states that one cannot know the exact position and velocity of a particle simultaneously
was proposed by
(A)
Heisenberg
39.
Atomic orbitals developed using quantum mechanics
(A)
(B)
(C)
(D)
describe regions of space in which one is most likely to find an electron
describe exact paths for electron motion
give a description of the atomic structure which is essentially the same as the Bohr model
allow scientists to calculate an exact volume for the hydrogen atom
(B)
(B)
(B)
Bohr.
Bohr.
Bohr.
spherical
dumbbell shape
4-leaf clover shape
“double” 4-leaf clover shape
(C)
(C)
(C)
De Broglie
De Broglie
De Broglie
5
smallest = 1s
smallest = 2p
smallest = 3d
smallest = 4f
(D)
(D)
(D)
Rutherford.
Rutherford.
Rutherford.
40.
What is the main difference between "classical physics" and "quantum physics"?
(A)
(B)
(C)
(D)
Quantum physics requires the speed of light to be a constant value.
Classical physics requires that only certain, allowed values for energy be used.
Quantum physics requires that only certain, allowed values for energy be used.
Quantum physics can only describe the behavior of very small objects, like atoms and molecules.
41.
Which feature of Bohr's atomic model is no longer accepted as true by today's scientists?
(A)
(B)
(C)
(D)
That most of an atom's mass is located within the nucleus
That electrons have only certain, allowed energy values
That electrons orbit the nucleus in circular paths
That each principal quantum level can hold a maximum of 2n2 electrons
42.
The orbitals of 2p electrons are often represented as being
(A)
elliptical.
43.
How many electrons can be "stored" in a completely filled 4f sublevel?
(A)
14
44.
For any given value of n greater than or equal to 2, how many electrons can be "stored" in a completely
filled p-block of elements?
(A)
10
45.
Within a given n-level, which of the following is the correct order in which subshells become filled with
electrons?
(A)
s, p, d, f
(B)
(B)
(B)
(B)
Electron configuration
tetrahedral.
10
3
p, s, f, d
(C)
(C)
(C)
(C)
spherical.
7
6
s, p, f, d
(D)
(D)
(D)
(D)
dumbbell shaped
28
5
d, s, p, f
“fill in electrons” in order of energy orbitals
Max of 2 electrons per orbital
Use Periodic Table to determine order
Can shorthand as [previous noble gas] valence electrons
Members of same group have same number of valence electrons
46.
Which of the following is the correct electron configuration of rubidium (Note: Both the number of
electrons and the proper filling order in terms of energy must be present in the answer you select)?
(A)
(C)
1s22s22p63s23p63d104s24p64d1
1s22s22p62d103s23p63d103f1
47.
Which electron configuration is impossible?
(A)
1s22s22p63s2 (B)
48.
A bismuth (Bi) atom has one more electron than a lead atom. Into which energy sub–level does this added
electron go?
(A)
5p
(B)
(B)
(D)
1s22s22p63s23p6
6p
(C)
1s22s22p63s23p64s24d104p65s1
1s22s22p63s23p64s23d104p65s1
(C)
6s
6
1s22s22p62d2 (D)
(D) 7s
1s22s22p63s1
49.
The electronic configuration of the manganese (Mn) atom is
(A)
(C)
1s22s22p63s23p64s2 4d5
1s22s22p63s23p64s24p5
50.
What is the electronic configuration of Uranium?
(A)
[Rn]7s26d15f3
51.
Which represents the electronic structure of the element having the atomic number 17?
(A)
(D)
1s22p83d7
1s22s22p42d23s23p43d1
52.
The electron configuration of the two outer subshells of vanadium, element number 23, is
(A)
4s33d2
53.
In has the valence electron configuration
(A)
5s25p1
54.
An atom has a valence shell electron configuration of ns1. To which group of metals in the periodic table
does it belong?
(A)
transition
55.
How many valence electrons does an ordinary chlorine atom contain?
(A)
7
(B)
(B)
(B)
(B)
(B)
6
(B)
(D)
[Ra]7s27d17f3
(B)
(E)
4s24p3
3s23p5
alkaline earth
(C)
8
(C)
1s22s22p63s23p63d7
1s22s22p63s23p64s23d5
[Rn]7s26d16f3
(D)
1s22s22p63s23p5
1s22p22d63f7
[Rn]7s27d15f3
(C)
(C)
4s23d3
(D)
4s13d4
(C)
3s23p3
(D)
5s25p3
(C)
(D)
rare earths
(D)
1s22s83p7
alkali
5
Properties of Atoms
“Happy” Atoms
Only Noble gases are happy
All others want same electron configuration (same number of electrons as Noble gases)
Ionize:
metals lose electrons; gain positive charge; CATIONS
Non-metals lose electrons; gain negative charge; ANIONS
56.
How many protons are present in a 127I- ion?
(A)
72
57.
Which pair of particles has the same number of electrons?
(A)
Cl–, Ca2+
(B)
(B)
127
Br–, Se
(C)
(C)
54
Ne, Ar
7
(D)
53
(D)
Al3+, P3–
(E)
73
58.
In what respect does an atom of magnesium differ from a magnesium ion (Mg2+)?
(A)
(B)
(C)
(D)
The ion has a more stable electronic arrangement than the atom.
The positive charge on the nucleus of the ion is two units greater than the nuclear charge on the atom.
The ion has two more protons than the atom.
The ion has two more electrons than the atom.
59.
What do these have in common?
(A)
(C)
the same number of protons
the same number of electrons
60.
Which ion has twenty–six electrons?
(A)
Cr2+
61.
Which ion is not likely to form from its atoms?
(A)
Al3+
62.
What charge would you expect to find on a selenide ion?
(A)
0
63.
The ions most commonly formed by calcium, aluminum and bromine are:
(A)
(D)
Ca+, Al2+, BrCa2-, Al5-, Br+
64.
Which one of these has an electronic configuration different from the others?
(A)
Ar
65.
Which element, isotope, or ion listed below contains 16 protons, 17 neutrons, and 18 electrons?
(A)
33
66.
Which of the following atoms or ions is, as written, in violation of the "octet rule"?
(A)
O3-
67.
Which of the following atoms or ions complies with the "octet rule"?
(A)
Mg2+
(B)
(B)
(B)
Ar2-
Fe2+
S2-
+2
(B)
(E)
(B)
(B)
(B)
(B)
Mg2+
33 2-
S
Sr2+
Ar
20Ne
(C)
(C)
(C)
19F–
24Mg2+
(B)
(D)
the same number of neutrons
the same size
Ni2+
(D)
Cu2+
As3-
(D)
K+
(E)
Mg+
(D)
-2
(E)
-1
+1
Ca2+, Al5-, BrCa2+, Al3+, Br-
(C)
(C)
(C)
(C)
(C)
K+
33
Cl
P3P
Br-
Ca2-, Al3+, Br-
(D)
(D)
(D)
(D)
S2–
34 2-
S
Ne
All of the above
Answers: C D B B A | D C B A D | D D B C C | A C D A C | D A C B B | D C A B D | C D B D D |
BCAAC|CDACA|DCBDA|BCADA|DAACC|EDEBB|AD
8