1) Answer the following questions by showing electron configuration (spdf notation). a) Identify which of the following is paramagnetic and which is diamagnetic:I, Na, K", Zn. b) Which of the following has the largest number of unpaired electrons.P, Cu, Ar, Cs. c) Which of the following has the smallest first ionization energy: Rb , N, Ne, Cu. d) List the following in order of increasing size: Na^+,K^+,Se^2-,Cl^- 2) Draw the Lewis structure of the following compounds and determine the formal charge of each element. a) HCSNH_(2) b) ClCH_(2)CH_(2)NH_(2) c) CH_(3)CH_(2)NH_(2) 3) Draw the Lewis structure of the following s species and show resonance structures where applicable. a) FSO_(3)^- b) H_(2)SO_(4) c) PO_(4)^3- 4) Given the below compounds, draw the appropriate Lewis structure, calculate the formal charge on each atom, indicate the VSEPR notation, determine the electron and molecular geometry using VSEPR theory, identify the hybridization of all interior atom(s), and make a sketch of the molecule based on the valence bond theory. a) S_(2)Cl_(2) b) COF_(2) c) CH_(3)SH 5) For CH_(3)CCCH_(2)CH_(2)COOH molecule, answer the questions that are listed below. a) Write correct Lewis structure and calculate the formal charge for atoms. b) Determine the number of electron groups for each interior atom, indicate the VSEPR notation and the bond angle.and draw the molecular shape using VSEPR theory. c) Identify hybridization of all carbons and shown the hybridization scheme for only the carbons indicated in blue (CH_(3)CCCH_(2)CH_(2)COOH) d) Make a sketch of the molecules according to valance bond theory by showing orbital overlap and specifically show the multiple bond formation e) Indicate the number of sigma and pi bonds in the structure. 6) a) Draw the molecular orbital diagram of the given compounds, predict the bond order, and comment on whether the molecule can exist or not. F2 Be_(2) b) Is C_(2)^2+ diamagnetic or paramagnetic? c) Would you expect the bond in F_(2) to be stronger or weaker than in the C_(2)^2+ molecule? why?

Question

1) Answer the following questions by showing electron configuration (spdf notation). a) Identify which of the following is paramagnetic and which is diamagnetic:I, Na, K", Zn. b) Which of the following has the largest number of unpaired electrons.P, Cu, Ar, Cs. c) Which of the following has the smallest first ionization energy: Rb , N, Ne, Cu. d) List the following in order of increasing size: Na^+,K^+,Se^2-,Cl^- 2) Draw the Lewis structure of the following compounds and determine the formal charge of each element. a) HCSNH_(2) b) ClCH_(2)CH_(2)NH_(2) c) CH_(3)CH_(2)NH_(2) 3) Draw the Lewis structure of the following s species and show resonance structures where applicable. a) FSO_(3)^- b) H_(2)SO_(4) c) PO_(4)^3- 4) Given the below compounds, draw the appropriate Lewis structure, calculate the formal charge on each atom, indicate the VSEPR notation, determine the electron and molecular geometry using VSEPR theory, identify the hybridization of all interior atom(s), and make a sketch of the molecule based on the valence bond theory. a) S_(2)Cl_(2) b) COF_(2) c) CH_(3)SH 5) For CH_(3)CCCH_(2)CH_(2)COOH molecule, answer the questions that are listed below. a) Write correct Lewis structure and calculate the formal charge for atoms. b) Determine the number of electron groups for each interior atom, indicate the VSEPR notation and the bond angle.and draw the molecular shape using VSEPR theory. c) Identify hybridization of all carbons and shown the hybridization scheme for only the carbons indicated in blue (CH_(3)CCCH_(2)CH_(2)COOH) d) Make a sketch of the molecules according to valance bond theory by showing orbital overlap and specifically show the multiple bond formation e) Indicate the number of sigma and pi bonds in the structure. 6) a) Draw the molecular orbital diagram of the given compounds, predict the bond order, and comment on whether the molecule can exist or not. F2 Be_(2) b) Is C_(2)^2+ diamagnetic or paramagnetic? c) Would you expect the bond in F_(2) to be stronger or weaker than in the C_(2)^2+ molecule? why?

Answer 1

1) a) Electron configurations:I: [Kr]4d10 5s2 5p5Na: [Ne]3s1K: [Ar]4s1Zn: [Ar]3d10 4s2Paramagnetic: I, KDiamagnetic: Na, Znb) Electron configurations:P: [Ne]3s2 3p3Cu: [Ar]3d10 4s1Ar: [Ne]3s2 3p6Cs: [Xe]6s1Largest number of unpaired electrons: Cuc) First ionization energy:Rb: 4.17 eVN: 14.53 eVNe: 21.56 eVCu: 7.73 eVSmallest first ionization energy: Cud) Order of increasing size:

2) a) Lewis structure of

:H-C≡N-HFormal charges: H: 0, C: 0, N: 0b) Lewis structure of

:Cl-CH2-CH2-NH2Formal charges: Cl: 0, C: 0, H: 0, N: 0c) Lewis structure of

:CH3-CH2-NH2Formal charges: C: 0, H: 0, N: 03) a) Lewis structure of

:F-O-S(=O)(-O)2-Resonance structures:F-O-S(=O)(-O)2-F-O-S(-O)(=O)2-b) Lewis structure of

:H2SO4Resonance structures:H2SO4c) Lewis structure of

:P(=O)(-O)2(O)3-Resonance structures:P(=O)(-O)2(O)3-4) a) Lewis structure of

:Cl-S-S-ClFormal charges: S: 0, Cl: 0VSEPR notation: AX2E2Electron geometry: TetrahedralMolecular geometry: LinearHybridization: sp3b) Lewis structure of

:F-C(=O)-FFormal charges: C: 0, O: 0, F: 0VSEPR notation: AX2E1Electron geometry: TetrahedralMolecular geometry: Trigonal planarHybridization: sp2c) Lewis structure of

:H3C-S-HFormal charges: C: 0, S: 0, H: 0VSEPR notation: AX2E2Electron geometry: TetrahedralMolecular geometry: BentHybridization: sp35) a) Lewis structure of

:CH3-C≡C-CH2-CH2-COOHFormal charges: C: 0, H: 0, O: 0b) VSEPR notation: AX4EBond angle: 109.5°Molecular shape: Tetrahedralc) Hybridization of all carbons: sp, sp2, sp3d) Sketch of the molecule according to valence bond theory:CH3-C≡C-CH2-CH2-COOHe) Number of sigma bonds: 9Number of pi bonds: 26) a) Molecular orbital diagram of F2:Bond order: 1F2 can existb)

is diamagneticc) The bond in F2 is stronger than in

because F2 has a higher bond order.

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