front 1 Which of the following does not have eight valence electrons? Cl- Xe Ti+4 Rb+ Sr+ | back 1 Answer: Sr+ |
front 2 How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? 1 2 3 4 5 | back 2 Answer: 4 |
front 3 How many equivalent resonance forms can be drawn for SO2 without expanding octet on the sulfur atom? (Sulfur is the central atom.) 0 2 3 4 1 | back 3 Answer: 2 |
front 4 consider the BEST Lewis structures of the following oxyanions: (i) NO2- (ii) NO3- (iii) SO32- (iv) SO42- (v) BrO3- In which of the ions do all X-O bonds (X indicates the central atom) have the same length? none all (i) and (ii) (iii) and (v) (iii), (iv), and (v) | back 4 Answer: all |
front 5 Electropositivity ________ from left to right within a period and ________ from top to bottom within a group. decreases, increases increases, increases increases, decreases stays the same, increases increases, stays the same | back 5 Answer: decreases, increases |
front 6 The ion PO43- has ________ valence electrons. 14 24 27 29 32 | back 6 Answer: 32 |
front 7 Of the possible bonds between carbon atoms (single, double, and triple), ________. a triple bond is longer than a single bond a double bond is stronger than a triple bond a single bond is stronger than a triple bond a double bond is longer than a triple bond a single bond is stronger than a double bond | back 7 Answer: a double bond is longer than a triple bond |
front 8 Using the table of average bond energies below, the △H for the reaction is ________ kJ. C≡O (g) + 2H2 (g) → H3C-O-H (g) Bond: C-O C=O C≡O C-H H-H O-H ΔH (kJ/mol): 358 799 1072 413 436 463 +276 -276 +735 -735 -116 | back 8 Answer: -116 |
front 9 The oxidation number of phosphorus in PF5 is ________. 5 3 1 -5 0 | back 9 Answer: 5 |
front 10 Which of the following would have to lose three electrons in order to achieve a noble gas electron configuration? Si Mg Al Cl P Si, P Al P Cl Mg, Al, P | back 10 Answer: Al |
front 11 What is the electron configuration for the Fe3+ ion? [Ar]4s13d6 [Ar]4s03d7 [Ar]4s03d5 [Ar]4s23d9 [Ne]3s23p10 | back 11 Answer: [Ar]4s03d5 |
front 12 The formula of palladium (IV) sulfide is ________. Pd2S4 PdS4 Pd4S PdS2 Pd2S2 | back 12 Answer: PdS2 |
front 13 The oxidation number of phosphorus in PF5 is ________. 5 3 1 -5 0 | back 13 Answer: 5 |
front 14 Resonance structures differ by ________. number and placement of electrons number of electrons only placement of atoms only number of atoms only placement of electrons only | back 14 Answer: placement of electrons only |
front 15 Determining lattice energy from Born-Haber cycle data requires the use of ________. the octet rule Coulomb's law Periodic law Hess's law Avogadro's number | back 15 Answer: Hess's law |
front 16 In the Lewis structure of ClF, the formal charge on Cl is ________, and the formal charge on F is ________. Answers: -1, -1 0, 0 0, -1 +1, -1 -1, +1 | back 16 Answer: 0, 0 |
front 17 There are ________ valence electrons in the Lewis structure of CH3OCH3 20 16 18 24 22 | back 17 Answer: 20 |
front 18 There are ________ valence electrons in the Lewis structure of CH3Cl. 14 16 18 20 22 | back 18 Answer: 14 |
front 19 For a given arrangement of ions, the lattice energy increases as ionic radius ________ and as ionic charge ________. decreases, increases increases, decreases increases, increases decreases, decreases This cannot be predicted. | back 19 Answer: decreases, increases |
front 20 The electron configuration of the S2- ion is ________. [Ar]3s23p6 [Ar]3s23p2 [Ne]3s23p2 [Ne]3s23p6 [Kr]3s22p6 | back 20 Answer: [Ne]3s23p6 |
front 21 A valid Lewis structure of ________ cannot be drawn without violating the octet rule. PO43- SiF4 CF4 SeF4 NF3 | back 21 Answer: SeF4 |
front 22 There are ________ unpaired electrons in the Lewis symbol for an oxygen atom 0 1 2 4 3 | back 22 Answer: 2 |
front 23 The ion ICl4- has ________ valence electrons. 34 35 36 28 8 | back 23 Answer: 36 |
front 24 A valid Lewis structure of ________ cannot be drawn without violating the octet rule. NF3 IF3 PF3 SbF3 NH3 | back 24 Answer: IF3 |
front 25 What is the electron configuration for the Co2+ ion? [Ar]4s13d6 [Ar]3d7 [Ar]3d5 [Ar]4s23d9 [Ne]3s23p10 | back 25 Answer: [Ar]3d7 |
front 26 The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e) of the negative charge on I in HI? (1 debye = 3.34 × 10-30 coulomb-meters; e = 1.6 × 10-19 coulombs) 1.6 × 10-19 0.057 9.1 1 0.22 | back 26 Answer: 0.057 |
front 27 The oxide of which of the following metals should have the greatest lattice energy? calcium strontium magnesium beryllium barium | back 27 Answer: beryllium |
front 28 How many equivalent resonance forms can be drawn for CO32-? (Carbon is the central atom.) 1 2 3 4 0 | back 28 Answer: 3 |
front 29 Given the electronegativities below, which covalent single bond is most polar? Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5 C—H N—H O—H O—C O—N | back 29 Answer: O—H |
front 30 What species has the electron configuration [Ar]3d2? Mn2+ Cr2+ V3+ Fe3+ K+ | back 30 Answer: V3+ |
front 31 The electron configuration of the S2- ion is ________. [Ar]3s23p6 [Ar]3s23p2 [Ne]3s23p2 [Ne]3s23p6 [Kr]3s22p6 | back 31 Answer: [Ne]3s23p6 |
front 32 The ________ ion has a noble gas electron configuration. Be2+ Li2+ LiMg2- Al2+ | back 32 Answer: Be2+ |
front 33 n the resonance form of ozone shown below, the formal charge on the central oxygen atom is ________. +1 -1 +2 -2 | back 33 Answer: +1 |
front 34 What is the electron configuration for the Fe2+ ion? [Ar]4s03d6 [Ar]4s23d4 [Ar]4s03d8 [Ar]4s23d8 [Ar]4s63d2 | back 34 Answer: [Ar]4s03d6 |
front 35 Which of the following does not have eight valence electrons? Ca+ Rb+ Xe Br- All of the above have eight valence electrons. | back 35 Answer: Ca+ |
front 36 Based on the octet rule, boron will most likely form a ________ ion. B3- B+ B3+ B2+ B2 | back 36 Answer: B3+ |
front 37 What is the electron configuration for the Co2+ ion? [Ar]4s13d6 [Ar]3d7 [Ar]3d5 [Ar]4s23d9 [Ne]3s23p10 | back 37 Answer: [Ar]3d7 |
front 38 The central atom in ________ does not violate the octet rule. SF4 KrF2 CF4 XeF4 ICl4- | back 38 Answer: CF4 |
front 39 Given the electronegativities below, which covalent single bond is most polar? Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5 C—H N—H O—H O—C O—N | back 39 Answer: O—H |
front 40 Which of the following does not have eight valence electrons? Ca+ Rb+ Xe Br- All of the above have eight valence electrons. | back 40 Answer: Ca+ |
front 41 here are ______ covalent bonds in the Lewis Structure of CH3CHCl2. 7 6 8 5 4 | back 41 Answer: 7 |
front 42 How many single covalent bonds must a chlorine atom form to have a complete octet in its valence shell? 0 1 2 3 4 | back 42 Answer: 1 |
front 43 Using the table of bond dissociation energies, the ΔH for the following reaction is ________ kJ. 2HCl (g) + F2 (g) → 2HF (g) + Cl2 (g) Bonds: H-Cl 431 F-F 155 H-F 567 Cl-Cl 242 Answers: -359 -223 359 223 208 | back 43 Answer: -359 |
front 44 The Lewis structure of N2H2 shows ________. a nitrogen-nitrogen triple bond a nitrogen-nitrogen single bond each nitrogen has one nonbonding electron pair each nitrogen has two nonbonding electron pairs each hydrogen has one nonbonding electron pair | back 44 Answer: each nitrogen has one nonbonding electron pair |
front 45 The electron configuration of the S2- ion is ________. [Ar]3s23p6 [Ar]3s23p2 [Ne]3s23p2 [Ne]3s23p6 [Kr]3s22p6 | back 45 Answer: [Ne]3s23p6 |
front 46 Which two bonds are most similar in polarity? O-F and Cl-F B-F and Cl-F Al-Cl and I-Br I-Br and Si-Cl C-Cl and Be-Cl | back 46 Answer: O-F and Cl-F |
front 47 What is the maximum number of double bonds that a hydrogen atom can form? 0 1 2 3 4 | back 47 Answer: 0 |
front 48 The formal charge on nitrogen in NO3- is ________, where the Lewis structure of the ion is: -1 0 +1 +2 -2 | back 48 Answer: +1 |
front 49 What species has the electron configuration [Ar]3d4? Mn2+ Cr2+ V3+ Fe3+ K+ | back 49 Answer: Cr2+ |
front 50 In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii ________. increases, decrease, increase increases, increase, increase decreases, increase, increase increases, increase, decrease increases, decrease, decrease | back 50 Answer: increases, increase, decrease |
front 51 Elements from opposite sides of the periodic table tend to form ________. covalent compound ionic compounds compounds that are gaseous at room temperature homonuclear diatomic compounds covalent compounds that are gaseous at room temperature | back 51 Answer: ionic compounds |
front 52 As the number of covalent bonds between two atoms increases, the distance between the atoms ________ and the strength of the bond between them ________. increases, increases decreases, decreases increases, decreases decreases, increases is unpredictable | back 52 Answer: decreases, increases |
front 53 Of the bonds C-C, C=C, and C≡C, the C-C bond is ________. strongest/shortest strongest/longest weakest/longest weakest/shortest intermediate in both strength and length | back 53 Answer: weakest/longest |
front 54 The ion ICl4- has ________ valence electrons. 34 35 36 28 8 | back 54 Answer: 36 |
front 55 The Lewis structure of HCN (H bonded to C) shows that ________ has ________ nonbonding electron pair(s) C, 1 N, 1 H, 1 N, 2 C, 2 | back 55 Answer: N, 1 |
front 56 Electronegativity ________ from left to right within a period and ________ from top to bottom within a group. decreases, increases increases, increases increases, decreases stays the same, increases increases, stays the same | back 56 Answer: increases, decreases |
front 57 Of the molecules below, the bond in ________ is the most polar. HBr HI HCl HF H2 | back 57 Answer: HF |
front 58 Which two bonds are most similar in polarity? O-F and Cl-F B-F and Cl-F Al-Cl and I-Br I-Br and Si-Cl C-Cl and Be-Cl | back 58 Answer: O-F and Cl-F |
front 59 Which of the following has eight valence electrons? Ti4+ Kr Cl- Na+ all of the above | back 59 Answer: all of the above |
front 60 The halogens, alkali metals, and alkaline earth metals have ________ valence electrons, respectively. 7, 4, and 6 1, 5, and 7 8, 2, and 3 7, 1, and 2 2, 7, and 4 | back 60 Answer: 7, 1, and 2 |
front 61 A ________ covalent bond between the same two atoms is the longest. single double triple strong They are all the same length. | back 61 Answer: single |
front 62 What is the electron configuration for the Fe2+ ion? [Ar]4s03d6 [Ar]4s23d4 [Ar]4s03d8 [Ar]4s23d8 [Ar]4s63d2 | back 62 Answer: [Ar]4s03d6 |
front 63 Of the atoms below, ________ is the most electronegative. Ba Sr Ca Mg Be | back 63 Answer: Be |
front 64 Of the possible bonds between carbon atoms (single, double, and triple), ________. a triple bond is longer than a single bond a double bond is stronger than a triple bond a single bond is stronger than a triple bond a double bond is longer than a triple bond a single bond is stronger than a double bond | back 64 Answer: a double bond is longer than a triple bond |
front 65 How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom? 5 2 1 4 3 | back 65 Answer: 3 |
front 66 A valid Lewis structure of ________ cannot be drawn without violating the octet rule. NI3 SO2 ICl5 SiF4 CO2 | back 66 Answer: ICl5 |
front 67 Based on the octet rule, iodine most likely forms an ________ ion. I2+ I4+ I4- I+ I- | back 67 Answer: I- |
front 68 A valid Lewis structure of ________ cannot be drawn without violating the octet rule. NF3 IF3 PF3 SbF3 NH3 | back 68 Answer: IF3 |
front 69 Of the bonds C-N, C=N, and C≡N, the C-N bond is ________. strongest/shortest strongest/longest weakest/shortest weakest/longest intermediate in both strength and length | back 69 Answer: weakest/longest |
front 70 n the Lewis symbol for a nitrogen atom, there are ________ paired and ________ unpaired electrons. two, three one, three three, two zero, five two, two | back 70 Answer: two, three |
front 71 Using the table of average bond energies below, the ΔH for the reaction is ________ kJ. Bond: C≡C C-C H-I C-I C-H ΔH (kJ/mol): 839 348 299 240 413 Answers: +160 -160 -217 -63 +63 | back 71 Answer: -217 |
front 72 The ________ ion has eight valence electrons. Sc3+ Ti3+ V3+ Cr3+ Mn3+ | back 72 Answer: Sc3+ |
front 73 How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? 1 2 3 4 5 | back 73 Answer: 4 |
front 74 Using the table of average bond energies below, the △H for the reaction is ________ kJ. C≡O (g) + 2H2 (g) → H3C-O-H (g) Bond: C-O C=O C≡O C-H H-H O-H ΔH (kJ/mol): 358 799 1072 413 436 463 Selected Answers: +276 -276 +735 -735 -116 | back 74 Answer: -116 |
front 75 The only noble gas without eight valence electrons is ________. Ar Ne He Kr All noble gases have eight valence electrons. | back 75 Answer: He |
front 76 How many equivalent resonance forms can be drawn for SO2 without expanding octet on the sulfur atom? (Sulfur is the central atom.) 0 2 3 4 1 | back 76 Answer: 2 |
front 77 The Lewis structure of AsH3 shows ________ nonbonding electron pair(s) on As. 0 1 2 3 This cannot be determined from the data given. | back 77 Answer: 1 |
front 78 What is the maximum number of triple bonds that a carbon atom can form? 4 1 0 2 3 | back 78 Answer: 1 |
front 79 As the number of covalent bonds between two atoms increases, the distance between the atoms ________ and the strength of the bond between them ________. increases, increases decreases, decreases increases, decreases decreases, increases is unpredictable | back 79 Answer: decreases, increases |
front 80 Lattice energy is ________. the energy required to convert a mole of ionic solid into its constituent ions in the gas phase the energy given off when gaseous ions combine to form one mole of an ionic solid the energy required to produce one mole of an ionic compound from its constituent elements in their standard states the sum of ionization energies of the components in an ionic solid the sum of electron affinities of the components in an ionic solid | back 80 Answer: the energy required to convert a mole of ionic solid into its constituent ions in the gas phase |
front 81 What is the electron configuration for the Fe2+ ion? [Ar]4s03d6 [Ar]4s23d4 [Ar]4s03d8 [Ar]4s23d8 [Ar]4s63d2 | back 81 Answer: [Ar]4s03d6 |
front 82 The ________ ion has eight valence electrons. Sc3+ Ti3+ V3+ Cr3+ Mn3 | back 82 Answer: Sc3+ |
front 83 How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? 1 2 3 4 5 | back 83 Answer: 4 |
front 84 n the nitrite ion (NO2-), ________. both bonds are single bonds both bonds are double bonds one bond is a double bond and the other is a single bond both bonds are the same there are 20 valence electrons | back 84 Answer: both bonds are the same |
front 85 The only noble gas without eight valence electrons is ________. Ar Ne He Kr All noble gases have eight valence electrons. | back 85 Answer: He |
front 86 Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet? N C H O B | back 86 Answer: B |