79) Which one of the following compounds produces a basic solution when dissolved in water?
A) SO2
B) Na2O
C) CO2
D) OF2
E) O2
80) Element M reacts with oxygen to form an oxide with the formula MO. When MO is dissolved in
water, the resulting solution is basic. Element M could be __________.
A) Na
B) Ba
C) S
D) N
E) C
81) Which alkaline earth metal will not react with liquid water or with steam?
A) Be
B) Mg
C) Ca
D) Ba
E) They all react with liquid water and with steam.
82) Which element is solid at room temperature?
A) Cl2
B) F2
C) Br2
D) I2
E) H2
83) __________ is a unique element and does not truly belong to any family.
A) Nitrogen
B) Radium
C) Hydrogen
D) Uranium
E) Helium
84) Of the following statements, __________ is not true for oxygen.
A) The most stable allotrope of oxygen is O2.
B) The chemical formula of ozone is O3.
C) Dry air is about 79% oxygen.
D) Oxygen forms peroxide and superoxide anions.
E) Oxygen is a colorless gas at room temperature.
85) Which one of the following elements has an allotrope that is produced in the upper atmosphere by
lightning?
A) N
B) O
C) S
D) Cl
E) He
86) In nature, sulfur is most commonly found in __________.
A) pure elemental sulfur
B) sulfur oxides
C) metal sulfides
D) sulfuric acid
E) H2S
87) All of the halogens __________.
A) exist under ambient conditions as diatomic gases
B) tend to form positive ions of several different charges
C) tend to form negative ions of several different charges
D) exhibit metallic character
E) form salts with alkali metals with the formula MX
88) This element reacts with hydrogen to produce a gas with the formula HX. When dissolved in water,
HX forms an acidic solution. X is __________,
A) Na
B) H
C) C
D) Br
E) O
89) The noble gases were, until relatively recently, thought to be entirely unreactive. Experiments in the
early 1960s showed that Xe could, in fact, form compounds with fluorine. The formation of compounds
consisting of Xe is made possible by __________.
A) the availability of xenon atoms
B) xenon’s noble gas electron configuration
C) the stability of xenon atoms
D) xenon’s relatively low ionization energy
E) xenon’s relatively low electron affinity
90) Of the following elements, which have been shown to form compounds?
helium neon argon krypton xenon
A) xenon and argon
B) xenon only
C) xenon, krypton, and argon
D) xenon and krypton
E) None of the above can form compounds.
91) In nature, the noble gases exist as
A) monatomic gaseous atoms
B) the gaseous fluorides
C) solids in rocks and in minerals
D) alkali metal salts
E) the sulfides
92) Hydrogen is unique among the elements because __________.
1. It is not really a member of any particular group.
2. Its electron is not at all shielded from its nucleus.
3. It is the lightest element.
4. It is the only element to exist at room temperature as a diatomic gas.
5. It exhibits some chemical properties similar to those of groups 1A and 7A.
A) 1, 2, 3, 5
B) 1, 2, 3, 4, 5
C) 1, 4, 5
D) 3, 4
E) 2, 3, 4, 5
93) Hydrogen is unique among the elements because __________.
1. It has only one valence electron.
2. It is the only element that can emit an atomic spectrum.
3. Its electron is not at all shielded from its nucleus.
4. It is the lightest element.
5. It is the only element to exist at room temperature as a diatomic gas.
A) 1, 2, 3, 4, 5
B) 1, 3, 4
C) 1, 2, 3, 4
D) 2, 3, 4
E) 3, 4
94) Ozone is a (an) __________ of oxygen.
A) isotope
B) allotrope
C) precursor
D) peroxide
E) free radical
95) Astatine has a __________ density and a __________ atomic radius compared to iodine.
A) greater; greater
B) smaller; greater
C) smaller; smaller
D) greater; smaller
E) equal; equal
96) Xenon has been shown to form compounds only when it is combined with __________.
A) something with a tremendous ability to remove electrons from other substances
B) another noble gas
C) something with a tremendous ability to donate electrons to other substances
D) an alkali metal
E) an alkaline earth metal
7.2 Bimodal Questions
1) __________ is credited with developing the concept of atomic numbers.
A) Dmitri Mendeleev
B) Lothar Meyer
C) Henry Moseley
D) Ernest Rutherford
E) Michael Faraday
2) Elements in the modern version of the periodic table are arranged in order of increasing __________.
A) oxidation number
B) atomic mass
C) average atomic mass
D) atomic number
E) number of isotopes
3) An electron in a(n) __________ subshell experiences the greatest effective nuclear charge in a many-
electron atom.
A) 3f
B) 3p
C) 3d
D) 3s
E) 4s
4) A tin atom has 50 electrons. Electrons in the __________ subshell experience the lowest effective
nuclear charge.
A) 1s
B) 3p
C) 3d
D) 5s
E) 5p
5) The first ionization energies of the elements __________ as you go from left to right across a period
of the periodic table, and __________ as you go from the bottom to the top of a group in the table.
A) increase, increase
B) increase, decrease
C) decrease, increase
D) decrease, decrease
E) are completely unpredictable
6) In general, as you go across a period in the periodic table from left to right:
(1) the atomic radius __________;
(2) the electron affinity becomes __________ negative; and
(3) the first ionization energy __________.
A) decreases, decreasingly, increases
B) increases, increasingly, decreases
C) increases, increasingly, increases
D) decreases, increasingly, increases
E) decreases, increasingly, decreases
7) The __________ have the most negative electron affinities.
A) alkaline earth metals
B) alkali metals
C) halogens
D) transition metals
E) chalcogens
8) Element M reacts with chlorine to form a compound with the formula MCl2. Element M is more
reactive than magnesium and has a smaller radius than barium. This element is __________.
A) Sr
B) K
C) Na
D) Ra
E) Be
9) Metals can be __________ at room temperature.
A) liquid only
B) solid only
C) solid or liquid
D) solid, liquid, or gas
E) liquid or gas
10) Most of the elements on the periodic table are __________.
A) gases
B) nonmetals
C) metalloids
D) liquids
E) metals
11) Na reacts with element X to form an ionic compound with the formula Na3X. Ca will react with X
to form __________.
A) CaX2
B) CaX
C) Ca2X3
D) Ca3X2
E) Ca3X
12) Ca reacts with element X to form an ionic compound with the formula CaX. Al will react with X to
form __________.
A) AlX2
B) AlX
C) Al2X3
D) Al3X2
E) Al3X
13) Oxides of the active metals combine with water to form __________.
A) metal hydroxides
B) metal hydrides
C) hydrogen gas
D) oxygen gas
E) water and a salt
14) Oxides of the active metals combine with acid to form __________.
A) hydrogen gas
B) metal hydrides
C) water and a salt
D) oxygen gas
E) metal hydroxides
15) Oxides of most nonmetals combine with water to form __________.
A) an acid
B) a base
C) water and a salt
D) water
E) hydrogen gas
16) Oxides of most nonmetals combine with base to form __________.
A) hydrogen gas
B) an acid
C) a base
D) water
E) water and a salt
17) An alkaline earth metal forms a compound with oxygen with the formula __________.
(The symbol M represents any one of the alkaline earth metals.)
A) MO
B) M2O
C) MO2
D) M2O2
E) MO3
18) An alkali metal forms a compound with chlorine with the formula __________.
(The symbol M represents any one of the alkali metals.)
A) M2Cl2
B) M2Cl
C) MCl2
D) MCl
E) MCl3
19) What is the coefficient of M when the following equation is completed and balanced if M is an
alkali metal?
M (s) + H2O (l) →
A) 1
B) 2
C) 3
D) 4
E) 0
20) The substance __________ is always produced when an active metal reacts with water.
A) NaOH
B) H2O
C) CO2
D) H2
E) O2
21) The reaction of potassium metal with elemental hydrogen produces __________.
A) KH
B) KH2
C) K2H
D) None of the above; potassium will not react directly with hydrogen.
E) KOH
22) What is the coefficient of H2O when the following equation is completed and balanced?
Ba (s) + H2O (l) →
A) 1
B) 2
C) 3
D) 5
E) Ba(s) does not react with H2O (l).
23) The element(s) __________ could be used to produce a red or crimson color in fireworks.
A) Mg or Ba
B) Sr
C) Ca, Sr, or Li
D) Ba
E) Na or K
24) Element X reacts with chlorine to form a compound with the formula XCl2. The oxide of element X
is basic. Element X is __________.
A) Rb
B) Ca
C) Al
D) P
E) H
25) The reaction of a metal with a nonmetal produces a(n) __________.
A) base
B) salt
C) acid
D) oxide
E) hydroxide
26) Which nonmetal exists as a diatomic solid?
A) bromine
B) antimony
C) phosphorus
D) iodine
E) boron
27) The most common and stable allotrope of sulfur is __________.
A) S
B) S2
C) S4
D) S8
E) Sulfur does not form allotropes.
28) Which group 6A element is a metal?
A) tellurium and polonium
B) sulfur
C) selenium
D) tellurium
E) polonium
29) The most common sulfur ion has a charge of __________.
A) 2-
B) 1-
C) 4+
D) 6+
E) Sulfur does not form ions.
30) The element phosphorus exists in two forms in nature called white phosphorus and red phosphorus.
These two forms are examples of __________.
A) isotopes
B) allotropes
C) oxidation
D) metalloids
E) noble gases
31) Which periodic table group contains only nonmetals?
A) 8A
B) 2A
C) 6A
D) 7A
E) 5A
32) Which periodic table group contains only metals?
A) 8A
B) 2A
C) 6A
D) 7A
E) 5A
33) Of the hydrogen halides, only __________ is a weak acid.
A) HCl (aq)
B) HBr (aq)
C) HF (aq)
D) HI (aq)
E) They are all weak acids.
34) All the elements in group 8A are gases at room temperature. Of all the groups in the periodic table,
only group __________ contains examples of elements that are gas, liquid, and solid at room
temperature.
A) 2A
B) 1A
C) 7A
D) 5A
E) 6A
35) The only noble gas that does not have the ns2np6 valence electron configuration is __________.
A) radon
B) neon
C) helium
D) krypton
E) All noble gases have the ns2np6 valence electron configuration.
36) The first noble gas to be incorporated into a compound was __________.
A) Ar
B) Kr
C) He
D) Ne
E) Xe
37) Of the halogens, which are gases at room temperature and atmospheric pressure?
A) fluorine, bromine, and iodine
B) fluorine, chlorine, and bromine
C) fluorine, chlorine, bromine, and iodine
D) fluorine, chlorine, and iodine
E) fluorine and chlorine
38) 2 F2 (g) + 2 H2O (l) → __________
A) 2 HF (aq) + 2 HFO (aq)
B) 2 F– (aq) + 2 H+ (aq) + H2O2 (aq)
C) 4 HF (aq) + O2 (g)
D) 2 HF2 (aq) + 2 OH– (aq)
E) 4 HF (aq) + 2 O2- (aq)
39) Cl2 (g) + H2O (l) → __________
A) HCl (aq) + HOCl (aq)
B) 2 Cl– (aq) + H2O (l)
C) 2 HCl (aq) + O2 (g)
D) 2 HCl (aq) + O2– (g)
E) Cl2 (aq) + H2O (l)
7.3 Algorithmic Questions
1) Which element would be expected to have chemical and physical properties closest to those of argon?
A) Cl
B) S
C) Fe
D) O
E) Kr
2) In which orbital does an electron in a phosphorus atom experience the greatest shielding?
A) 2p
B) 3s
C) 3p
D) 2s
E) 1s
3) In which orbital does an electron in a lead atom experience the greatest effective nuclear charge?
A) 1s
B) 4p
C) 5s
D) 6s
E) 5d
4) In which of the following atoms is the 3s orbital closest to the nucleus?
A) Se
B) Br
C) As
D) Ga
E) Ge
5) Which one of the following atoms has the largest radius?
A) Sr
B) Ca
C) K
D) Rb
E) Y
6) Which one of the following has the smallest radius?
A) K
B) Br
C) Fe
D) Sr
7) Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?
A) F < K < Ge < Br < Rb
B) F < Br < Ge < K < Rb
C) F < Ge < Br < K < Rb
D) F < K < Br < Ge < Rb
E) F < Br < Ge < Rb < K
8) Of the following atoms, which has the largest first ionization energy?
A) Sb
B) Se
C) As
D) S
E) Ge
9) Which of the following has the largest second ionization energy?
A) Ge
B) Ga
C) Ca
D) K
E) Se
7.4 Short Answer Questions
1) The degree of interaction between two electrical charges depends on the __________ and the
__________ of the charges and the distance between them.
2) As successive electrons are removed from an element, the ionization energy __________.
3) Which noble gas has the highest first ionization energy?
4) When electrons are removed from a lithium atom they are removed first from which orbital?
5) An added electron to the element bromine goes into which orbital?
6) Write the balanced reaction between zinc oxide and sulfuric acid.
7) What are the elements called that are located between the metals and non-metals?
8) Complete the following : P4O10 + 6 H2O
9) Which metal is a liquid at room temperature?
10) [Xe]6s2 is the electron configuration for __________.
11) [Kr]5s2 is the electron configuration for __________.
12) In their compounds, the charges on the alkali metals and the alkaline earth metals are __________
and __________, respectively.
13) Which alkali metals can react with oxygen to form either the peroxide or the superoxide?
14) Write the balanced equation for the reaction of potassium with water.
15) Of the alkaline earth metals, which two elements are the least reactive?
16) Write the balanced equation for the reaction of elemental fluorine with liquid water.
17) Write the balanced equation for the reaction of elemental chlorine with liquid water.
18) List seven nonmetals that exist as diatomic molecules in their elemental forms.
19) All of the group VIA elements are solids except __________.
20) Which noble gas has the lowest first ionization energy?
7.5 True/False Questions
1) The effective nuclear charge acting on an electron is larger than the actual nuclear charge.
2) The effective nuclear charge in an atom is proportional to the number of nuclear protons.
3) The atomic radius of iodine is one-half the distance separating the iodine nuclei.
4) A group of ions all containing the same number of electrons constitute an isoelectronic series.
5) Elements that readily conduct electricity are elements with low ionization energies.
6) Electron affinity measures how easily an atom gains an electron.
7) Xenon can form compounds with fluorine.