A normal mode of vibration for H₂O is at 3650 cm Calculate the force constant, k, for H₂O. Assuming the force constant to be the same for H₂O and D₂O. Do you expect the corresponding D₂O wave number to be higher or lower? (Given: The atomic masses for H, D and O are 1.0, 2.0 and 16.0 respectively) (ii)

A normal mode of vibration for H₂O is at 3650 cm Calculate the force constant, k, for H₂O. Assuming the force constant to be the same for H₂O and D₂O. Do you expect the corresponding D₂O wave number to be higher or lower? (Given: The atomic masses for H, D and O are 1.0, 2.0 and 16.0 respectively) (ii)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?
Give the ground-state electron configu rations of (a) H2 - . (b) Li2, (c) Be2, (d) C2, (e) N2, and (f) O2 .
Photoelectron spectroscopy studies of silicon atoms excited by X-rays with wavelength 9.890 × 10-1º m show four peaks in which the electrons have speeds 2.097 × 107 m s-!, 2.093 x 107 m s-!, 2.014 × 107 m s', and 1.971 x 107 m s-1. (Recall that 1 J = 1 kg m² s-2.) (a) Calculate the ionization energy of the electrons in each peak. (b) Assign each peak to an orbital of the silicon atom.
Use the noble-gas notation and write the ground-state electronic configurations of the following ions:(a) O2- (b) Tl3+ (c) V3+
7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°
For each of the following pairs of atoms, state which youexpect to have the higher electron affinity: (a) Rb or Sr;(b) I or Rn; (c) Ba or Te; (d) Bi or C
2. Which one of each of the following pairs has the higher ionization energy? Explain in detail for each case. (a) Na or K (b) Ве or B (с) В or C (d) N or O F or Ne (f) Mg or Mg* Ne or Na
(v) n = 6, 1 = 3, ms = +½ (c) Give the ground-state electron configuration for each of following substances: (1) Phosphorus (ii) Cr(Il) ion (iii) Sulfide ion (iv) Ti(IV) ion DELL
Based on data in Table 8.1, estimate (within 30 kJ/mol) thelattice energy for (a) LiBr, (b) CsBr, (c) CaCl2.
Write the electronic configuration of:(i) Al3+ (ii)K+ (iii)O2-
The experimentally determinded Bi-Cl bond distance in bismuth trichloride is 2.48Å . Given the tablulated value of 0.99Å for the atomic radius of Cl, predict the atomic radius of Bi?
Use the periodic table to (i) predict electron configurations for the following species: Arsenic ion, As3– Magnesium ion, Mg2+ Vanadium(II) ion, V2+ (ii) Write the electron configurations of each species in the noble gas notation. (iii) Draw an orbital diagram to represent 1 c above. Draw the Lewis electron dot structures of the following chemical species. In each case you must say whether or not the central atom obeys the Octet Rule. CS2 and H2S CF4 and SiH4 NH2Cl CO32– and BF3 PCl5 ClF3, XeF2, Calculate the formal charge on the Sulphur atom in the Sulphate anion structure shown below(picture attatched) Give the electron-pair and molecular geometries for NF3 and XeF4.