WorksheetsBasic Chem Final Review
Total questions: 74
Worksheet time: 19hrs 30mins
Name
Class
Date
1.
The nucleus of an atom has all of the following characteristics except that it
a)
is very dense.
b)
contains protons and neutrons.
c)
is positively charged.
d)
contains almost all of the atom’s volume.
2.
What makes an atom electrically neutral?
a)
The neutrons balance out the protons and electrons.
b)
The nuclear forces contained in the atom neutralize the atom.
c)
The number of protons is equal to the number of electrons.
d)
The number of protons is equal to the number of neutrons.
3.
The smallest particle of an element that retains the properties of that element is a(n)
a)
electron
b)
atom
c)
proton
d)
quark
4.
What does the number 91 represent in the name zirconium-91?
a)
the atomic number
b)
the number of protons
c)
the mass number
d)
the sum of protons and electrons
5.
An element has an atomic number of 72. The number of protons and electrons in a neutral atom of this element is
a)
72 protons and 72 electrons
b)
72 protons and 0 electrons
c)
36 protons and 36 electrons
d)
none of the above
6.
Which of the following sets is correct?
a)
Zn-65, 65 protons, 65 electrons
b)
Mg-24, 12 protons, 12 neutrons
c)
U-238, 92 protons, 92 neutrons
d)
Pb-207, 207 protons, 207 electrons
7.
An atom has an atomic number of 32 and a mass number of 73. How many protons, neutrons, and electrons does
this atom contain?
a)
32 protons, 73 neutrons, 32 electrons
b)
73 protons, 73 neutrons, 41 electrons
c)
32 protons, 41 neutrons, 32 electrons
d)
41 protons, 32 neutrons, 41 electrons
8.
Identify the element that has 31 neutrons and a mass of 59.
a)
gallium
b)
praseodymium
c)
thorium
d)
nickel
9.
Isotopes of the same element have different
a)
chemical properties.
b)
masses.
c)
atomic numbers.
d)
number of protons.
10.
All atoms of the same element have the same
a)
number of protons.
b)
mass number.
c)
number of neutrons.
d)
protons and neutrons.
11.
Determine the number of neutrons in 119/50 Sn
a)
119
b)
50
c)
169
d)
69
12.
How does the isotopes carbon-12 and carbon-14 differ?
a)
Carbon-12 has 12 neutrons; carbon-14 has 14 neutrons
b)
Carbon-12 has 6 protons; carbon-14 has 8 protons
c)
Carbon-12 has 6 neutrons; carbon-14 has 8 neutrons
d)
Carbon-12 has 6 protons; carbon-14 has 6 protons
13.
Which of the following equals one atomic mass unit (amu)?
a)
the mass of protons plus neutrons
b)
1/12 the mass of one carbon-12 atom
c)
mass of one electron
d)
the mass of one atom of carbon-12
14.
Bohr’s model of the atom shows the electrons
a)
are mixed evenly with the positive charge.
b)
are found orbiting a positively charged nucleus.
c)
are found orbiting a positively charged nucleus in energy levels he called orbits.
d)
are found in regions of probability around the nucleus called orbitals.
15.
Which of these answers would apply to Thomson’s model?
a)
are mixed evenly with the positive charge.
b)
are found orbiting a positively charged nucleus.
c)
are found orbiting a positively charged nucleus in energy levels he called orbits.
d)
are found in regions of probability around the nucleus called orbitals.
16.
Which of these answers would apply to Rutherford’s model?
a)
are mixed evenly with the positive charge.
b)
are found orbiting a positively charged nucleus.
c)
are found orbiting a positively charged nucleus in energy levels he called orbits.
d)
are found in regions of probability around the nucleus called orbitals.
17.
Which subatomic particles have approximately the same mass?
a)
electrons and protons
b)
electrons and neutrons
c)
protons and neutrons
d)
protons and quarks
18.
An atom that has 15 protons and 16 neutrons is an isotope of what element?
a)
copper
b)
phosphorus
c)
gallium
d)
sulfur
19.
Which quantity can vary among neutral atoms of the same element?
a)
mass number
b)
atomic number
c)
number of protons
d)
number of electrons
20.
Which element on the periodic table has a total of 40 protons?
a)
calcium
b)
potassium
c)
chromium
d)
zirconium
21.
Which statement best describes the Quantum Mechanical model of the atom?
a)
Electrons are arranged on a large, solid, positive center.
b)
Electrons have properties similar to waves
c)
Electrons orbit around the nucleus in set paths.
d)
Electrons make up most of the mass of an atom
22.
The ions in most ionic compounds are organized into a
a)
molecule
b)
crystal lattice
c)
Lewis Structure
d)
polyatomic ion
23.
Ionic compounds are formed by ionic bonds between
a)
metals and metals
b)
transition metals
c)
nonmetals and nonmetals
d)
metals and nonmetals
24.
Malleability and ductility are characteristics of substances with
a)
metallic bonds
b)
ionic bonds
c)
covalent bonds
d)
polyatomic ions
25.
Which of the following atom’s Lewis dot notation shows six valence electrons?
a)
nitrogen
b)
magnesium
c)
sulfur
d)
iodine
26.
How many electrons do strontium atoms generally lose?
a)
0
b)
1
c)
2
d)
3
27.
Cesium has an electronegativity value of 0.7 and fluorine has and electronegativity value of 4.0. Which of the following statements is true?
a)
Cesium has less of a tendency to attract electrons than fluorine.
b)
Fluorine repels electrons more than cesium.
c)
Cesium attracts electrons easier than fluorine.
d)
Fluorine has less of a tendency to attract electrons than cesium.
28.
If atoms that share electrons, have an unequal attraction for the electrons, the bond is called
a)
ionic
b)
polar
c)
nonpolar
d)
metallic
29.
The melting points of ionic compounds are higher than the melting points of molecular compounds because
a)
ionic compounds are brittle.
b)
attractive forces between ions are stronger than the attractive forces between molecules.
c)
Ionic substances are all flammable.
d)
none of the above
30.
Which of these compounds would have the highest melting point?
a)
NH3
b)
OF2
c)
H2O
d)
NaCl
31.
The chemical formula for water is H2O. This formula is an example of a(n)
a)
Lewis Structure
b)
formula unit
c)
molecular formula
d)
ionic formula
32.
Which of the following molecules has a single covalent bond?
a)
F2
b)
CO2
c)
N2
d)
NO
33.
Which of the following molecules has a single lone pair of electrons?
a)
HCl
b)
CH4
c)
H2O
d)
NH3
34.
Which of the properties listed below is not a property of ionic compounds?
a)
hardness
b)
brittle
c)
low melting point
d)
high melting point
35.
A covalent bond between two different atoms in which the bonding electrons are not shared equally is a
a)
polar bond
b)
nonpolar bond
c)
ionic bond
d)
hydrogen bond
36.
The Russian scientist, Dmitri Mendeleev, noticed that by arranging the elements known at his time in order of increasing _______________, similarities in the chemical properties appeared at regular intervals.
a)
atomic number
b)
atomic mass
c)
group number
d)
period number
37.
Mendeleev predicted that spaces left in his periodic table represented
a)
isotopes.
b)
radioactive elements.
c)
undiscovered elements.
d)
noble gases.
38.
Based on evidence collected since Mendeleev’s time, elements on the modern periodic table are arranged in order of _____________.
a)
mass number
b)
average atomic mass
c)
group number
d)
atomic number
39.
The periodic law states that the physical and chemical properties of elements are periodic functions of their
a)
atomic masses.
b)
atomic numbers.
c)
atomic radii.
d)
ionic charges.
40.
What periodic group includes argon, krypton, and xenon?
a)
noble gases
b)
halogens
c)
alkaline earth metals
d)
actinides
41.
Elements in a group on the periodic table can be expected to have similar
a)
atomic masses.
b)
number of neutrons.
c)
properties.
d)
atomic numbers.
42.
Each period on the periodic table corresponds to
a)
an energy level.
b)
a sublevel.
c)
atomic mass.
d)
atomic number.
43.
The horizontal rows on the periodic table are called
a)
groups.
b)
families
c)
an octet.
d)
periods.
44.
Calcium, Ca, and arsenic, As, belong to
a)
Group 17.
b)
Period 4.
c)
Group 2.
d)
Period 3.
45.
The electron configuration for phosphorus is [Ne]3s23p3. Phosphorus is in period
a)
2.
b)
3.
c)
5.
d)
15.
46.
Identify the sublevels in a period that contains 18 elements.
a)
s, f
b)
s, p
c)
s, p, d
d)
s, p, d, f
47.
Elements in which the d-sublevel is being filled have properties of
a)
metalloids.
b)
nonmetals.
c)
metals.
d)
actinides.
48.
The group of 14, f-block elements, in the sixth period are called the
a)
actinides.
b)
lanthanides.
c)
transition elements.
d)
metalloids.
49.
What element am I? period 4, group 4
a)
titanium
b)
scandium
c)
zirconium
d)
vanadium
50.
Iodine belongs to group 17. How many valence electrons does iodine have?
a)
17
b)
35
c)
7
d)
4
51.
The group 1 elements are known as the
a)
noble gases.
b)
alkaline earth metals.
c)
alkali metals.
d)
halogens.
52.
What group is the most reactive group of nonmetals?
a)
noble gases.
b)
transition metals.
c)
alkali metals.
d)
halogens.
53.
Identify the group of elements that are soft, silvery, reactive metals, and have one electron in an s orbital.
a)
noble gases
b)
alkali metals
c)
transition metals
d)
halogens
54.
Tellurium, atomic number 52, has the electron configuration [Kr]5s23d105p4. Tellurium is classified as a
a)
metal.
b)
transition metal.
c)
alkali metal.
d)
metalloid.
55.
To what period and group does nitrogen belong?
a)
period 15, group 2
b)
period 17, group 2
c)
period 2, group 17
d)
period 2, group 15
56.
In which set of elements below, would you expect to find similar chemical properties?
a)
N, O, F
b)
K, Rb, Cs
c)
Ne, Na, Ca
d)
S, Se, Si
57.
Of the following, which gives the correct order for atomic radius for Mg, Na, P, Cl, and Si?
a)
Na > Mg > Si > P > Cl
b)
b) Cl > Si > P > Na > Mg
c)
c) Na > Mg > Cl > P > Si
d)
d) Cl > P > Si > Mg > Na
58.
Within a group of elements, what is the trend for atomic radius moving down the group?
a)
increases
b)
decreases
c)
remains constant
d)
very irregular
59.
Which is the BEST explanation of the trend of decreasing atomic radius when moving across the period left to right?
a)
the number of neutrons increases
b)
the number of energy levels increases
c)
the nuclear charge increases
d)
the atomic number increases
60.
The energy required to remove an electron from an atom is called
a)
electron energy.
b)
electronegativity.
c)
ionization energy.
d)
valence energy.
61.
What is the term for electrons available to be lost, gained, or shared when atoms form compounds.
a)
ions
b)
s-block electrons
c)
valence electrons
d)
the electron cloud
62.
Which of the following factors contributes to the increase in ionization energy going across the period from left to right?
a)
an increase in the shielding effect
b)
an increase in the number of energy levels
c)
fewer electrons in the outermost energy level
d)
an increase in the number of protons, smaller atomic radius
63.
As you move across the second period of the periodic table,
a)
ionization energy decreases
b)
atomic radius decreases
c)
ionization energy increases
d)
both b and c
64.
Which of the following has the largest second ionization energy?
a)
magnesium, Mg
b)
sodium, Na
c)
phosphorus, P
d)
aluminum, Al
65.
If the first ionization energy for carbon is 1086 kJ/mol, then the first ionization energy for silicon will be
a)
1086 kJ/mol.
b)
close to zero.
c)
greater than 1086 kJ/mol.
d)
less than 1086 kJ/mol.
66.
A measure of the ability of an atom to attract electrons from another atom in a chemical compound is called
a)
ionization energy
b)
electronegativity
c)
electron configuration
d)
electron affinity
67.
Which element is the most electronegative?
a)
fluorine, F
b)
sodium, Na
c)
neon, Ne
d)
cesium, Cs
68.
Which of the following elements has the greatest electronegativity?
a)
chlorine, Cl
b)
sodium, Na
c)
magnesium, Mg
d)
bromine, Br
69.
How does an atom’s ability to attract electrons in a chemical compound change as you move left to right across period 4 from cobalt, Co, to bromine, Br?
a)
It does not change.
b)
It can’t be predicted.
c)
It increases.
d)
It decreases.
70.
Which of the following elements is the least electronegative?
a)
bromine, Br
b)
carbon, C
c)
sodium, Na
d)
lithium, Li
71.
What would an element with the electron configuration [Kr] 5s24d7 be classified as?
a)
halogen
b)
transition metal
c)
noble gas
d)
alkali metal
72.
In which of the following pairs will the ion formed be larger than the neutral atom?
a)
Ca & Ca2+
b)
K & K+
c)
F and F-
d)
Al and Al3+
73.
Which of the groups below contains elements that will form 2+ ions?
a)
alkaline earth metals
b)
alkali metals
c)
halogens
d)
noble gases
74.
What is the most active element in group 17?
a)
iodine, I
b)
chlorine, Cl
c)
bromine, Br
d)
fluorine, F
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