Some review
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What term best describes the relation of hydrogen (1H) to deuterium (2H)?
C
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How many neutrons are in carbon–14?
C
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What pair of particles has the same number of electrons?
A
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Which group contains nonmetals, metalloids, and metals?
C
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What group contains halogens?
C
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What is the wavelength (in nm) of a photon with an energy of 6.51×10–19 J?
B
\(E = \dfrac{hc}{\lambda}\)
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Which ground state electron configuration is possible for an atom in the second period?
C
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Which of these species is/are paramagnetic?
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The size of metal atoms
A
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Which of these elements has the smallest atomic radius?
A
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Which ion is the smallest?
A
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Which ion has the largest radius?
Note: For those that were present in the 9AM class, I’ve changed this question since ionic radii of transition metals is not mentioned in your textbook.
A
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Which sample has the largest mass?
A
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A 10 gram sample of which substance contains the greatest number of hydrogen atoms?
C
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A 3.41×10–6 g sample is known to contain 4.67×1016 molecules. What is this compound?
B
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What is the mass (in g) of 1.75 moles of Zn?
D
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What is the mass (in g) of 1.75 moles of Zn?
D
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What mass (in g) of oxygen does 25.5 g of aluminum carbonate, Al2(CO3)3, contain? (Molar mass of Al2(CO3)3 = 233.99 g mol–1)
D
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Which compound contains the largest percent by mass of oxygen?
A
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The limiting reagent for a given reaction can be recognized because it is the reagent that
D
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How many moles of water are necessary to react completely with 8.0 mol PCl5?
\[\mathrm{PCl_5} + 4~\mathrm{H_2O} \longrightarrow \mathrm{H_3PO_4} + 5~\mathrm{HCl}\]
D
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If 365.5 g H2O(l) is combined with excess KO2, what mass of O2(g) (in g), is expected to be produced?
\[2~\mathrm{KO_2(s)} + 2~\mathrm{H_2O} \longrightarrow 2~\mathrm{KOH(s)} + \mathrm{O_2(g)} + \mathrm{H_2O_2(l)}\]
C
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What mass (in g) of FeS is necessary to form 1.08 g Fe2O3 with excess O2?
\[4~\mathrm{FeS} + 7~\mathrm{O_2} \longrightarrow 2~\mathrm{Fe_2O_3} + 4~\mathrm{SO_2}\] (Molar mass FeS = 87.92 g mol–1; Molar mass Fe2O3 = 159.7 g mol–1)
C
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A mixture of 9 mol F2 and 4 mol S are allowed to react. \[3~\mathrm{F_2} + \mathrm{S} \longrightarrow \mathrm{SF_6}\] How many moles of F2 remain after 3 mol of S have reacted?
D
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What is the molar concentration of a solution when 7.00 mL of a 3.25 M aqueous solution is diluted to 25.00 mL?
B
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What is a weak acid in water?
C
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What is the oxidation number of chlorine in NaClO2?
C
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What is the oxidation number of chromium in Na2Cr2O7?
B
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Which combination will result in a precipitate forming?
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What volume (in mL) of a 0.0557 M Sr(OH)2 solution is needed to neutralize 36.4 mL of a 0.0750 M HNO3 solution?
A
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