75) 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
76) Ozone is a a(n) ________ of oxygen.
A) isotope
B) allotrope
C) precursor
D) peroxide
E) free radical
77) Astatine has a(n) ________ density and a(n) ________ atomic radius compared to iodine.
A) greater; greater
B) smaller; greater
C) smaller; smaller
D) greater; smaller
E) equal; equal
78) 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 ________ 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) The first ionization energies of the elements 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.
31
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) 2F2 (g) + 2H2O (l) → ________
A) 2HF (aq) + 2HFO (aq)
B) 2F– (aq) + 2H+ (aq) + H2O2 (aq)
C) 4HF (aq) + O2 (g)
D) 2HF2 (aq) + 2OH– (aq)
E) 4HF (aq) + 2O2- (aq)
39) Cl2 (g) + H2O (l) → ________
A) HCl (aq) + HOCl (aq)
B) 2Cl– (aq) + H2O (l)
C) 2HCl (aq) + O2 (g)
D) 2HCl (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
rubidium?
A) Cu
B) Fe
C) S
D) Ca
E) K
2) In which orbital does an electron in a nitrogen atom experience the greatest shielding?
A) 3p
B) 3s
C) 2p
D) 2s
E) 1s
3) In which orbital does an electron in a copper atom experience the greatest effective nuclear charge?
A) 1s
B) 4s
C) 4p
D) 4d
E) 3d
4) In which of the following atoms is the 3s orbital closest to the nucleus?
A) S
B) Po
C) Te
D) Se
E) P