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Review test #3 trends,bond,lewis,naming

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 

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.
 

 2. 

Mendeleev attempted to organize the chemical elements based on their
a.
symbols.
c.
atomic numbers.
b.
atomic mass and properties.
d.
electron configurations.
 

 3. 

Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing
a.
atomic number.
c.
reactivity.
b.
density.
d.
atomic mass.
 

 4. 

Mendeleev is credited with developing the first successful
a.
periodic table.
b.
method for determining atomic number.
c.
test for radioactivity.
d.
use of X rays.
 

 5. 

Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar
a.
properties.
c.
densities.
b.
atomic numbers.
d.
colors.
 

 6. 

Mendeleev predicted that the spaces in his periodic table represented
a.
isotopes.
c.
permanent gaps.
b.
radioactive elements.
d.
undiscovered elements.
 

 7. 

Argon, krypton, and xenon are
a.
alkaline earth metals.
c.
actinides.
b.
noble gases.
d.
lanthanides.
 

 8. 

Which two periods have the same number of elements?
a.
2 and 4
c.
4 and 5
b.
3 and 4
d.
5 and 6
 

 9. 

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.
c.
the law of properties.
b.
the periodic law.
d.
Mendeleev's law.
 

 10. 

Elements in a group or column in the periodic table can be expected to have similar
a.
atomic masses.
c.
numbers of neutrons.
b.
atomic numbers.
d.
properties.
 

 11. 

A horizontal row of blocks in the periodic table is called a(n)
a.
group.
c.
family.
b.
period.
d.
octet.
 
 
test_3_review_files/i0130000.jpg
 

 12. 

To which group do lithium and potassium belong? Refer to the figure above.
a.
alkali metals
c.
halogens
b.
transition metals
d.
noble gases
 

 13. 

Refer to the figure above. To which group do fluorine and chlorine belong?
a.
alkaline-earth metals
c.
halogens
b.
transition elements
d.
actinides
 

 14. 

Elements to the right side of the periodic table (p-block elements) have properties most associated with
a.
gases.
c.
metals.
b.
nonmetals.
d.
metalloids.
 

 15. 

The elements that border the zigzag line in the periodic table are
a.
inactive.
c.
metalloids.
b.
metals.
d.
nonmetals.
 

 16. 

The most characteristic property of the noble gases is that they
a.
have low boiling points.
c.
are gases at ordinary temperatures.
b.
are radioactive.
d.
are largely unreactive.
 

 17. 

The energy required to remove an electron from an atom is the atom's
a.
electron affinity.
c.
electronegativity.
b.
electron energy.
d.
ionization energy.
 

 18. 

A measure of the ability of an atom in a chemical compound to attract electrons is called
a.
electron affinity.
c.
electronegativity.
b.
electron configuration.
d.
ionization potential.
 

 19. 

The element that has the greatest electronegativity is
a.
oxygen.
c.
chlorine.
b.
sodium.
d.
fluorine.
 

 20. 

Ionization energy is the energy required to remove ____ from an atom of an element.
a.
the electron cloud
c.
an electron
b.
the nucleus
d.
an ion
 

 21. 

When an electron is acquired by a neutral atom, the energy change is called
a.
electron affinity.
c.
ionization energy.
b.
electronegativity.
d.
electron configuration.
 

 22. 

A positive ion is known as a(n)
a.
ionic radius.
c.
cation.
b.
valence electron.
d.
anion
 

 23. 

A negative ion is known as a(n)
a.
ionic radius.
c.
cation.
b.
valence electron.
d.
anion.
 

 24. 

In a row in the periodic table, as the atomic number increases, the atomic radius generally
a.
decreases.
c.
increases.
b.
remains constant.
d.
becomes unmeasurable.
 

 25. 

Within a group of elements, as the atomic number increases, the atomic radius
a.
increases.
c.
decreases regularly.
b.
remains approximately constant.
d.
decreases, but not regularly.
 

 26. 

In the alkaline-earth group, atoms with the smallest radii
a.
are the most reactive.
c.
are all gases.
b.
have the largest volume.
d.
have the highest ionization energies.
 

 27. 

As the atomic number of the metals of Group 1 increases, the ionic radius
a.
increases.
c.
remains the same.
b.
decreases.
d.
cannot be determined.
 

 28. 

Across a period in the periodic table, atomic radii
a.
gradually decrease.
b.
gradually decrease, then sharply increase.
c.
gradually increase.
d.
gradually increase, then sharply decrease.
 

 29. 

Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
a.
The nuclear charge increases.
c.
The number of energy levels increases.
b.
The number of neutrons increases.
d.
A new octet forms.
 

 30. 

For each successive electron removed from an atom, the ionization energy
a.
increases.
c.
remains the same.
b.
decreases.
d.
shows no pattern.
 

 31. 

As you move down the periodic table from carbon through lead, atomic radii
a.
generally increase.
c.
do not change.
b.
generally decrease.
d.
vary unpredictably.
 

 32. 

As you move left to right from gallium through bromine, atomic radii
a.
generally increase.
c.
do not change.
b.
generally decrease.
d.
vary unpredictably.
 

 33. 

The energy required to remove an electron from an atom ____ as you move left to right from potassium through iron.
a.
generally increases
c.
does not change
b.
generally decreases
d.
varies unpredictably
 

 34. 

The electrons available to be lost, gained, or shared when atoms form molecules are called
a.
ions.
c.
d electrons.
b.
valence electrons.
d.
electron clouds.
 

 35. 

Valence electrons are those
a.
closest to the nucleus.
c.
in the highest energy level.
b.
in the lowest energy level.
d.
combined with protons.
 

 36. 

The electrons involved in the formation of a chemical bond are called
a.
dipoles.
c.
Lewis electrons.
b.
s electrons.
d.
valence electrons.
 

 37. 

A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)
a.
covalent bond.
c.
charged bond.
b.
ionic bond.
d.
dipole bond.
 

 38. 

The chemical bond formed when two atoms share electrons is called a(n)
a.
ionic bond.
c.
Lewis structure.
b.
orbital bond.
d.
covalent bond.
 

 39. 

The electrostatic attraction between ____ forms an ionic bond.
a.
ions
c.
electrons
b.
dipoles
d.
orbitals
 

 40. 

A covalent bond results when ____ are shared.
a.
ions
c.
electrons
b.
Lewis structures
d.
dipoles
 

 41. 

The octet rule states that chemical compounds tend to form so that each atom has an octet of electrons in
a.
its highest occupied energy level.
c.
its d orbitals.
b.
the 1s orbital.
d.
its p orbitals.
 

 42. 

An octet is equal to
a.
2.
c.
5.
b.
4.
d.
8.
 

 43. 

What principle states that atoms tend to form compounds so that each atom can have eight electrons in its outermost energy level?
a.
rule of eights
c.
configuration rule
b.
Avogadro principle
d.
octet rule
 

 44. 

The electron configuration of nitrogen is 1s2 2s2 2p3. How many more electrons does nitrogen need to satisfy the octet rule?
a.
1
c.
5
b.
3
d.
8
 

 45. 

The elements of the ____ group satisfy the octet rule without forming compounds.
a.
main
c.
alkali metal
b.
noble gas
d.
alkaline-earth metal
 

 46. 

In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by
a.
2 electrons.
c.
8 electrons.
b.
4 electrons.
d.
10 electrons.
 

 47. 

To draw a Lewis structure, one must know the
a.
number of valence electrons in each atom.
b.
atomic mass of each atom.
c.
bond length of each atom.
d.
ionization energy of each atom.
 

 48. 

How many extra electrons are in the Lewis structure of the phosphate ion, PO43–?
a.
0
c.
3
b.
2
d.
4
 
 
test_3_review_files/i0510000.jpgtest_3_review_files/i0510001.jpg
 

 49. 

What is the Lewis structure for hydrogen chloride, HCl?
a.
A
c.
C
b.
B
d.
D
 

 50. 

What is the formula for zinc fluoride?
a.
ZnF
c.
Zn2F
b.
ZnF2
d.
Zn2F3
 

 51. 

What is the formula for the compound formed by calcium ions and chloride ions?
a.
CaCl
c.
CaCl3
b.
Ca2Cl
d.
CaCl2
 

 52. 

What is the formula for the compound formed by lead(II) ions and chromate ions?
a.
PbCrO4
c.
Pb2(CrO4)3
b.
Pb2CrO4
d.
Pb(CrO4)2
 

 53. 

What is the formula for aluminum sulfate?
a.
AlSO4
c.
Al2(SO4)3
b.
Al2SO4
d.
Al(SO4)3
 

 54. 

What is the formula for barium hydroxide?
a.
BaOH
c.
Ba(OH)2
b.
BaOH2
d.
Ba(OH)
 

 55. 

Name the compound Ni(ClO3)2.
a.
nickel chlorate
c.
nickel chlorite
b.
nickel chloride
d.
nickel peroxide
 

 56. 

Name the compound Zn3(PO4)2.
a.
zinc potassium oxide
c.
zinc phosphate
b.
trizinc polyoxide
d.
zinc phosphite
 

 57. 

Name the compound Hg2(NO3)2.
a.
mercury(II) nitrate
c.
mercury(I) nitrate
b.
dimercury dinitrate
d.
mercuric nitrate
 

 58. 

Name the compound KClO3.
a.
potassium chloride
c.
potassium chlorate
b.
potassium trioxychlorite
d.
hypochlorite
 

 59. 

Name the compound Fe(NO2)2.
a.
iron(II) nitrate
c.
ferric nitrate
b.
iron(II) nitrite
d.
ferrous nitride
 

 60. 

Name the compound CuCO3.
a.
copper(I) carbonate
c.
cuprous carbide
b.
cupric trioxycarbide
d.
copper(II) carbonate
 

 61. 

What is the metallic ion in copper(II) chloride?
a.
Co2+
c.
Cu2+
b.
Cl2–
d.
Cl
 

 62. 

Name the compound CF4.
a.
calcium fluoride
c.
carbon tetrafluoride
b.
carbon fluoride
d.
monocarbon quadrafluoride
 

 63. 

Name the compound SiO2.
a.
silver oxide
c.
silicon dioxide
b.
silicon oxide
d.
monosilicon dioxide
 

 64. 

Name the compound N2O4.
a.
sodium tetroxide
c.
nitrous oxide
b.
dinitrogen tetroxide
d.
binitrogen oxide
 

 65. 

Name the compound SO3.
a.
sulfur trioxide
c.
selenium trioxide
b.
silver trioxide
d.
sodium trioxide
 

 66. 

Name the compound N2O5.
a.
dinickel pentoxide
c.
neon oxide
b.
dinitrogen pentoxide
d.
nitric oxide
 

 67. 

Which compound's name includes the Greek numerical prefixes di- and tri-?
a.
Fe2O3
c.
N2O3
b.
Ca3(PO4)2
d.
Al2S3
 

 68. 

Name the compound N2O3.
a.
dinitrogen oxide
c.
nitric oxide
b.
nitrogen trioxide
d.
dinitrogen trioxide
 

 69. 

What is the formula for nitrogen monoxide?
a.
N2O
c.
NO
b.
NOO
d.
N2O2
 

 70. 

What is the formula for silicon dioxide?
a.
SO2
c.
Si2O
b.
SiO2
d.
S2O
 

 71. 

What is the formula for nitrogen trifluoride?
a.
NiF3
c.
N3F
b.
NF3
d.
Ni3F
 

 72. 

What is the formula for dinitrogen trioxide?
a.
Ni2O3
c.
N2O6
b.
NO3
d.
N2O3
 

 73. 

What is the formula for sulfur dichloride?
a.
NaCl2
c.
S2Cl
b.
SCl2
d.
S2Cl2
 

 74. 

What is the formula for diphosphorous pentoxide?
a.
P2PeO5
c.
P2O4
b.
PO5
d.
P2O5
 

 75. 

What is the formula for carbon disulfide?
a.
CaS2
c.
S2C
b.
CS2
d.
SC2
 



 
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