109年 - 109 台灣聯合大學系統_學士班轉學生考試試題_A1：普通化學#99762

科目：轉學考-普通化學 | 年份：109年 | 選擇題數：50 | 申論題數：0

試卷資訊

所屬科目：轉學考-普通化學

選擇題 (50)

1. How many unpaired electrons are found in Mn60ed2081ad011.jpg? (A) 4 (B) 5 (C) 1 (D)0 (E) 2
2. Which of the following is polar? (A) PBr3 (B) SiF4 (C) SBr6 (D) KrF2(E) BF3
3. Which of the following bonds would be the most polar without being considered ionic? (A) C-O (B) Mg-O (C) 0-0 (D) Si-O (E) N-O
4. In a 0.1 molar solution of NaCl in water, which of the following will be closest to 0.1? (A) the molality of NaCI (B) the mass percent of NaCI (C) the mole fraction of NaCl (D) the mass fraction of NaCl (E) all of these are about 0.1.

5. How many electrons are transferred in the following reaction? 60ed20c6d497b.jpg) (A) 4 (B) 10 (C) 3 (D)2(E) 6

6. Ammonium metavanadate reacts with sulfur dioxide in acidic solution as follows (hydrogen ions and H2O omitted): 60ed20fa05b3f.jpg(A) 1:3(B)1:2 (C) 2:1(D) 3:1(E) 1:1

7. When the equation 60ed2122cfe81.jpg (basic solution) is balanced using the smallest whole- number coefficients, what is the coefficient of OH-? (A)1 (B) 2(C) 3 (D) 4 (E)6
8. Which of the following is(are) oxidation-reduction reactions? I: PCl3 + Cl2→ PCI5； ll: Cu + 2AgNO3→Cu(NO3)2 + 2Ag； IIl；CO2+2LiOH→Li2CO3+H2O；IV:FeCl2+ 2NaOH → Fe(OH)2+2NaCl (A) l, ll, lll, and IV (B) I and II only (C) I, II, and Ill only (D) IV only (E) Ill only
9. An aqueous solution of silver nitrate is added to an aqueous solution of potassium chromate, and this reaction produces a solid. What is the formula for the solid? (A) AgCrO4 (B) KNO3 (C) AgK(D) K2NO3(E) Ag2CrO4

10. Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0℃ and 1 atm pressure. Which gas has the highest density? (A) NH3 (B) CH4 (C) CI2 (D) He (E) all the gases have the same density.
複選題

11. Consider the equation 60ed225f4fedf.jpg. At a particular temperature, K = 1.6 x 104. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will (A) have no effect (B) cause [X] to increase (C) cause (Y] to increase (D) cannot be determined (E) none of these

12. Calculate the percentage of pyridine (CsHsN) that forms pyridinium ion, C5H5NH+, in a 0.10 M aqueous solution of pyridine 60ed22b31e60f.jpg, (A) 0.77% (B) 0.060% (C) 0.0060%(D) 1.6%(E)0.013%

13. Identify the strongest base. (A) CH3OH (B) CH3O-(C) H2O(D) 60ed22fcb2592.jpg(E) CN-

14. The acids HC2H3O2 and HF are both weak, but HF is a stronger acid than HC2H3O2. HCI is a strong acid. Order the following according to base strength. (A) 60ed237b1d621.jpg(B)60ed2399f3397.jpg(C)60ed23bbe2ad3.jpg(D)60ed23dadcd0d.jpg60ed23fe7d9ee.jpg(E) none of these
15. A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a phenolphthalein endpoint. The formula of the acid is (A) H3A (B) H2A (C) H4A (D) HA(E) not enough information given

16. Calculate the solubility of Ag2SO460ed24504678d.jpgin a 2.0 M AgNO3 solution. (A) 60ed248b5b8c9.jpgmol/L (B)60ed24a7e32b8.jpgmol/L (C) 60ed24c4532dc.jpgmol/L (D) 60ed24e40c4cf.jpg mol/L(E) none of these

17. Given the equation S(s) + O2(g) → SO2(g), △H = -296 kIJ, which of the following statements is(are) true? I: The reaction is exothermic； Il: When 0.500 mol of sulfur is reacted, 148 kJ of energy is released. III: When 32.0 g of sulfur is burned, 2.96 x 105 J of energy is released. (A) I and Ill are true (B) only II is true (C) all are true (D) I and II are true (E) none is true.

18. Given the following two reactions at 298 K and 1 atm, which of the statements is true?60ed255593fe4.jpg(A) △Hf for NO2(g) =△H2+(1/2)△H1(B) △H1 = △H2 (C)△Hf for NO(g) = △H1 (D) △Hf for NO2(g) = △H2)(E) none of these

19. A 100-mL sample of water is placed in a coffee cup calorimeter. When 1.0 g of an ionic solid is added, the temperature decreases from 21.5℃ to 20.8℃ as the solid dissolves. Which of the following is true for the dissolving of the solid? (A) AH ＜O (B) 60ed25ebaa51a.jpg

(C) 60ed261029c97.jpg (D) 60ed263c5a3d7.jpg (E) none of these
複選題

20. For a spontaneous endothermic process, which conditions must hold? 60ed268d50451.jpgcannot be negative； IV △S is positive. (A) all (B) none (C) I and IIll only (D) I, I, and IV only (E) IIl and IV only
21. At constant pressure, the reaction； 2NO2(g) → N2O4(g) is exothermic. The reaction (as written) (A) spontaneous at low temperatures but not at high temperatures (B) spontaneous at high temperatures but not at low temperatures (C) always spontaneous (D) never spontaneous (E) none of these

22. The reaction below occurs in basic solution. In the balanced equation, what is the sum of the coefficients?60ed26e6c0d24.jpg(A) 27 (B) 19 (C) 23 (D) 12 (E) 15
23. How many unpaired electrons are there in an atom of sulfur in its ground state? (A) 1(B) 2 (C) 4 (D)0(E)3

24. The valence electron configuration of an element is60ed272d09b81.jpg . To which group does X belong? (A) Group 3A (B) Group 4A (C) Group 6A (D) Group 5A (E) Group 7A
25. The_______ states that in a given atom no two electrons can have the same set of four quantum numbers (n, I, mI, ms). (A) Pauli exclusion principle (B) Huygens-Fresnel principle (C) Cauchy's argument principle (D) Heisenberg uncertainty principle(E) Le Chatelier's principle
26. Of the following, which molecule has the smallest bond angle? (A)CO2(B) H2O (C) SCI2 (D) SO3 (E) NF3
27. What type of structure does the XeOF2 molecule have? (A) trigonal planar (B) octahedral (C) pyramidal (D) T-shaped (E) tetrahedral

28. Which of the following statements is false? (A) The carbon-carbon bond in60ed279d41041.jpgis shorter than the one in CH3CH3 (B) the carbon-carbon bond in 60ed279d41041.jpgis stronger than the one in CH3CH3 (C) C2 is diamagnetic (D) C2 is paramagnetic (E) two of these statements are false.
29. Consider the molecular-orbital energy-level diagrams for O2 and NO. Which of the following is true?I : Both molecules are paramagnetic； II: The bond strength of O2 is greater than the bond strength of NO； III: NO is an example of a homonuclear diatomic molecule； IV: The ionization energy of NO is smaller than the ionization energy of NO+ . (A) I and II only (B)I, II, and IV (C) I and IV (D) II and III (E) I only

30. How many ofthe following are paramagnetic?60ed283570427.jpg(A) 3 (B) 2 (C) 4 (D) 5(E) 0
31. Doping Se with As would produce a(n)_____semiconductor with_____conductivity compared to pure Se. (A) n-type, increased (B) p-type, increased (C) n-type, decreased (D) intrinsic, identical (E) p-type, decreased
32. Which of the following statements is incorrect? (A) ionic solids have high melting points (B) the binding forces in a molecular solid include London dispersion forces (C) ionic solids are insulators (D) molecular solids have high metting points (E) all of these statements are correct.
33. A liquid placed in a closed container will evaporate until equilibrium is reached. At equilibrium, which of the following statements is not true? (A) liquid molecules are still evaporating (B) the number of vapor molecules remains essentially constant (C) the partial pressure exerted by the vapor molecules is called the vapor pressure of the liquid (D) the boundary (meniscus) between the liquid and the vapor disappears (E) all of these statements are true.
34. How many different possible tetramethylbenzenes exist? (A) 6 (B)2 (C) 5 (D)3(E)4
35. Oxidation of a primary alcohol results in a(n)_____， and oxidation of a secondary alcohol results in a(n)_____. (A) ester, ether (B) ketone, aldehyde (C) amine, carboxylic acid (D) carboxylic acid, amine (E) aldehyde, ketone

36. Choose the correct molecular structure for 60ed28a44f540.jpg.(A) octahedral (B) tetrahedral (C) trigonal planar (D) trigonal bipyramidal (E) linear
37. What Group 6A elements are semiconductors? (A) selenium and polonium (B) sulfur and tellurium (C) sulfur and selenium (D) selenium and tellurium (E) tellurium and polonium
38. Which is the most reactive form of phosphorus? (A) white phosphorus (B) red phosphorus (C) black phosphorus (D) two of these forms of phosphorus are equally reactive (E) all of these forms of phosphorus are equally reactive
39. When a non volatile solute is added to a volatile solvent, the solution vapor pressure________ ， the  boiling point ________ , the  freezing point________，and the osmotic pressure across a  semipermeable membrane_________. (A) decreases, decreases, increases, decreases (B)J increases, decreases, increases, decreases (C) decreases, increases, decreases, increases (D) increases, increases, decreases, increases (E) decreases, increases, decreases, decreases
40. Which of the following statements is(are) true? (A) the rate of dissolution of a solid in a liquid always increases with incr reasing temperature (B) the solubility of a solid in a liquid always increases with increasing temperature (C) according to Henry's law, the amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the liquid (D) two of these statements are true (E) all of these statements are true.
41. Which statement regarding water is true? (A) liquid water is less dense than solid water.(B) only covalent bonds are broken when ice melts (C) hydrogen bonds are stronger than covalent bonds (D) energy must be given off in order to break down the crystal lattice of ice to a liquid (E) all of these statements are false.
42. Which of the following is the smallest hole in a closest-packed lattice of spheres? (A) trigonal (B) cubic (C) tetrahedral (D) octahedral (E) none of these
43. The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. The unit cell contains a net (A) 2 anions and 3 cations (B) 2 anions and 2 cations (C) 5 anions and 3 cations (D) 3 anions and 4 cations (E) 5 anions and 6 cations.
44.How many of the following compounds exhibit geometric isomers? I: Pd(NHa3)2Br2 (square planar)； Il:[Co(H2O)2]Br3； I1:[Ni(H2O)4(NO2)2]； lV:K2[CoCl4] (A) 2(B) 3 (C) 1 (D) 4(E)0

45. For which of the following metal ions would there be no distinction between low spin and high spin in octahedral complexes? (A)60ed2ae5f259f.jpg(B)60ed2b0ac7de0.jpg(C) 60ed2b39b0362.jpg(D) 60ed2b59eaf6d.jpg(E)60ed2b79e90d5.jpg
46. Which of the following stateme ents is true of the crystal field model? (A) the electrons are assumed to be localized (B) the metal ion-ligand bonds are considered completely ionic (C) the ligands are treated as negative point charges (D) the interaction between metal ion and ligand is treated as a Lewis acid-base interaction (E) none of these statements is true

47. A d6 ion 60ed2bbb65a9f.jpg is complexed with six strong-field ligands (for example, SCN-). What is the number of unpaired electrons in this complex? (A) 3(B) 2 (C)0(D) 1(E) 4
48. Which of the following state nts are true about starch? I: the mono omers are fructose and Rlucose； Il: the mon onomer is glucose； Ill: it is the main carbohydrate reservoir in plants； IV: It is the main carbohydrate reservoir in animals； V: It is an addition polymer； VI. It is a condensation polymer. (A) II, III, VI (B) I, IV, V (C) I, II, IV, V (D) I, II, V (E) II, IV, VI
49. Which of the following pairs of substances could form an addition copolymer? (A) HOCH2CH2OH + HOOCH2COOH(B) HOOC(CH2)3COOH + HOCH2CH2CHANH2 (C) HOOCCH2CH2COOH + HOCH2OCH2 OH (D) H2C=CHCH=CH2 +H2CCH=CHCH3 (E) H2NCH2 COOH + H2NCH2CH2COOH
50. Which of the following statements is/are true of benzene? I: Benzene belongs to a class of cyclic unsaturated hydrocarbons known as the aromatic hydrocarbons；II : Benzene undergoes substitution reaction in which hydrogen atoms are replaced by other atoms； Ill: sp2 hybrid orbitals on each carbon of a benzene molecule are used to form the H-H and H-C a bonds. (A) IIl only (B) II only (C) I only (D) I and Il (E) I and Ill

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