chem exams 2
If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 7.00 g of K3PO4 in enough water to make 350. mL of solution
0.377 M
How many milliliters of 0.260 M Na2S are needed to react with 45.00 mL of 0.315 M AgNO3? Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s) A) 27.3 mL B) 54.5 mL C) 74.3 mL D) 109 mL
A) 27.3 mL
Assume that an aqueous solution of a cation, represented by shaded spheres, is allowed to mix with a solution of an anion, represented by unshaded spheres. Three possible outcomes are represented by boxes (a)-(c). Which outcome corresponds to the combination of calcium and carbonate ions shown in the following equation? Ca2+(aq) + CO 2-(aq) → ? 3 A) box (a) B) box (b) C) box (c) D) None of these
B) box (b)
The spheres below represent atoms of Li, Be, B, and F (not necessarily in that order). Which one of these spheres represents an atom of Li? A) sphere (a) B) sphere (b) C) sphere (c) D) sphere (d)
D) sphere (d)
What is the oxidation number of the sulfur atom in SO2? A) -2 B) +2 C) -4 D) +4
D) +4
How many milliliters of 0.458 M Pb(NO3)2 are needed to react with 0.200L of 0.885M K3PO4? 2 K3PO4 (aq) + 3 Pb(NO3)3 (aq) → 6 KNO3 (aq) + Pb3(PO4)2 (s)A) 153 mL B) 258 mL C) 386 mL D) 580 mL
D) 580 mL
6) Write a balanced net ionic equation for the reaction of AgNO3(aq) with Li Cl(aq).
D) Ag+(aq)) + Cl-(aq) → AgCl(s)
Using the following portion of the activity series for oxidation half reactions Mg(s) → Mg2+(aq) + 2e- Co(s) → Co2+(aq) + 2e- Cu(s) → Cu2+(aq) + 2e- indicate which pairs of reactions will occur.A) Cu(s) with Co2+(aq) and Co(s) with Mg2+(aq) B) Mg(s) with Cu2+(aq) and Co2+(aq) with Mg2+(aq) C) Mg(s) with Cu(s) and Co(s) with Cu(s) D) Mg(s) with Co2+(aq) and Co(s) with Cu2+(aq)
D) Mg(s) with Co2+(aq) and Co(s) with Cu2+(aq)
Which species functions as the oxidizing agent in the following reduction-oxidation reaction? 5 Fe2+(aq) + MnO -(aq) + 8 H+(aq) → Mn2+(aq) + 5 Fe3+(aq) + 4 H O(l) 42 A) Fe2+(aq) B) H+(aq) C) Mn2+(aq) D) MnO -(aq) 4
D) MnO -(aq) 4
Write a balanced net ionic equation for the reaction of Pb(NO3)2(aq) with NaI(aq). A) Pb(NO3)2(aq) + 2 NaI(aq) → PbI2(s) + 2 NaNO3(aq)
D) Pb2+(aq) + 2 I-(aq) → PbI2(s)
Which pair of compounds is insoluble in water?A) AgNO3 and KNO3 B) Na2S and CuSC) (NH4)2SO4 and AgI D) PbSO4 and Pb3(PO4)2
D) PbSO4 and Pb3(PO4)2
5) When K2SO4(aq) and Pb(NO3)2(aq) are mixed, a white colored precipitate forms which is A) KNO3. B) K2SO3. C) Pb. D) PbSO4.
D) PbSO4.
What are the possible values of n and ml for an electron in a 6d orbital? A)n=1,2,3,4,or5andml =2B)n=1,2,3,4,or5andml =-2,-1,0,+1,or+2C)n=6andml =2 D) n = 6 and ml = -2, -1, 0, +1, or +2
D) n = 6 and ml = -2, -1, 0, +1, or +2
Light can be made to have a higher intensity by raising its
amplitude
Which of the compounds H3PO4, Mg(OH)2, LiOH, and HCl, behave as bases when they are dissolved in water?A) Mg(OH)2 and LiOH B) H3PO4 and HCl C) only HCl D) only LiOH
A) Mg(OH)2 and LiOH
The ground state electron configuration for silver (anomalous) is A) [Kr]4d10 5s1. B) [Kr] 4d9 5s2.C) [Xe] 4f14 5d10 6s1. D) [Xe] 4f14 5d9 6s2.
A) [Kr]4d10 5s1.
Which have the largest number of unpaired electrons in p orbitals in their ground-state electron configurations?A)N, As,Bi B)F, At, BrC)Ne, Ar, Xe D)B, Ga,Tl
A)N, As,Bi
The ground state electron configuration for silver (anomalous) is 10 1 A)[Kr]4d 5s. 14 10 1 C)[Xe]4f 5d 6s. 9 2 B)[Kr]4d 5s. 14 9 2 D)[Xe]4f 5d 6s.
A)[Kr]4d 5s. 1
What is the oxidation number change (final - initial) for the chromium atom in the following unbalanced reduction half reaction? Cr O 2-(aq) + H+(aq) → Cr3+(aq) + H O(l) 272 A) -7 B) -3 C) +3 D) +6
B) -3
What is the oxidation number change (final - initial) for the manganese atom in the following unbalanced reduction half reaction? MnO -(aq) + H+(aq) → Mn2+(aq) + H O(l) 42 A) -7 B) -5 C) +5 D) +7
B) -5
4) What is the concentration of of NO3 ions in a solution prepared by dissolving 20.0 g of Ca(no3) in enough water to produce 300.0 mL of solution
B) 0.406 M
Three different substances, A2X, A2Y, and A2Z, were dissolved in water with the following results. (Water molecules are omitted for clarity.) Which of the substances is the strongest electrolyte, and which is the weakest? A) A2X is the strongest electrolyte and A2Y is the weakest electrolyte. B) A2Y is the strongest electrolyte and A2X is the weakest electrolyte. C) A2Y is the strongest electrolyte and A2Z is the weakest electrolyte. D) A2Z is the strongest electrolyte and A2Y is the weakest electrolyte.
B) A2Y is the strongest electrolyte and A2X is the weakest electrolyte
Using the following portion of the activity series for oxidation half-reactions, determine which combination of reactants will result in a reaction. Li(s) → Li+(aq) + e- Al(s) → Al3+(aq) + 3e- A) Li(s) with Al(s) B) Li(s) with Al3+(aq) C) Li+(aq) with Al3+(aq) D) Li+(aq) with Al(s)
B) Li(s) with Al3+(aq)
Assume that an aqueous solution of a cation, represented by shaded spheres, is allowed to mix with a solution of an anion, represented by unshaded spheres. Three possible outcomes are represented by boxes (a)-(c). Which outcome corresponds to the combination of copper(II) and sulfide ions shown in the following equation? Cu2+(aq) + S2-(aq) → ?A) box (a) B) box (b) C) box (c) D) None of these
B) box (b)
For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0 B) n = 4 and l = 1 C) n = 4 and l = 2 D) n = 4 and l = 3
B) n = 4 and l = 1
Water (H2O), methyl alcohol (CH3OH), ethyl alcohol (CH3CH2OH), ethylene glycol (HOCH2CH2OH), and sucrose (C12H22O11) are commonly classified as A) bases. B) nonelectrolytes. C) strong electrolytes. D) weak electrolytes.
B) nonelectrolytes
Which of the above fourth-shell orbitals is a 4pz orbital? A) orbital (a) B) orbital (b) C) orbital (c) D) orbital (d)
B) orbital (b
What is the concentration of HNO3 in the final solution when 70.0 mL of a 6.00 M HNO3 solution is diluted with pure water to a total volume of 0.15 L? A)3.57×10-2 M B)2.80M C) 12.6 M D) 1.75 M
B)2.80M
What is the oxidation number of the sulfur atom in Cs2SO3? A) -2 B) +2 C) +4 D) +6
C) +4
How many orbitals are represented by the set of quantum numbers n = 8 and l = 2? A) 0 B) 1 C) 5 D) 8
C) 5
Which pair of compounds is soluble in water? A) AgCl and AgBrC) KClO4 and Ba(ClO4)2 B) CdS and (NH4)2S D) K2SO4 and BaSO4
C) KClO4 and Ba(ClO4)2
Which species functions as the reducing agent in the following reduction-oxidation reaction? 2 P(s) + 3 Br2(l) → 2 PBr3(l) A) Br-(aq) B) Br2(l) C) P(s) D) P3+(aq)
C) P(s)
Which one of the following compounds is soluble in water? A) BaSO4 B) AgClC) Pb(ClO4)2 D) Mg(OH)2
C) Pb(ClO4)2
Electromagnetic radiation with the shortest wavelength will be emitted when an electron undergoes which of the following transitions?A) m = 1 → n = 2 B) m = 2 → n = 3C) n = 2 → m = 1 D) n = 3 → m = 2
C) n = 2 → m = 1
The reaction CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) can be classified as a(n)
C) oxidation-reduction reaction.
The reaction Sr(NO3)2(aq) + Cs2SO4(aq) → SrSO4(s) + 2 CsNO3(aq) is best classified as a(n) A) acid-base neutralization reaction. B) oxidation-reduction reaction.C) precipitation reaction. D) single replacement reaction.
C) precipitation reaction.
The spheres below represent atoms of Li, Be, B, and F (not necessarily in that order). Which one of these spheres represents an atom of Be? A) sphere (a) B) sphere (b) C) sphere (c) D) sphere (d)
C) sphere (c)
Which have the largest number of unpaired electrons in p orbitals in their ground-state electron configurations?A)Ne, Ar, Xe B)F, At, BrC)N,As,Bi D)B, Ga,Tl
C)N,As,Bi
Arrange the following spectral regions in order of increasing wavelength: infrared, microwave, ultraviolet, visible.A) microwave < infrared < visible < ultravioletB) microwave < visible < infrared < ultraviolet C) ultraviolet < infrared < visible < microwave D) ultraviolet < visible < infrared < microwave
D) ultraviolet < visible < infrared < microwave