Question 4 The two Group VB elements niobium and tantalum have the same atomic radii. This is because of.. O A Lanthanide contraction; the filling of 4f orbitals through the lanthanide elements causing a steady increase in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. OB. Scandide contraction; the filling of 4f orbitals through the Scandide elements causing a steady increase in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. OC. Lanthanide contraction; the filling of 4f orbitals through the lanthanide elements causing a steady decrease in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. orhitals through the Scandide elements causing a steady decrease in the effective nuclear charge. This contraction offsets the expected decrease of

Question 4 The two Group VB elements niobium and tantalum have the same atomic radii. This is because of.. O A Lanthanide contraction; the filling of 4f orbitals through the lanthanide elements causing a steady increase in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. OB. Scandide contraction; the filling of 4f orbitals through the Scandide elements causing a steady increase in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. OC. Lanthanide contraction; the filling of 4f orbitals through the lanthanide elements causing a steady decrease in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. orhitals through the Scandide elements causing a steady decrease in the effective nuclear charge. This contraction offsets the expected decrease of

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 95AP

See similar textbooks

Similar questions

Consider the following ionization energies for aluminum: Al(g)Al+(g)+eI1=580kJ/molAl+(g)Al2+(g)+eI2=1815kJ/molAl2+(g)Al3+(g)+eI3=2740kJ/molAl3+(g)Al4+(g)+eI4=11,600kJ/mol a. Account for the trend in the values of tbe ionization energies. b. Explain the large increase between I3 and I4
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L Martin, S. P. Kowalczyk. F. R. McFeely, and L. Ley: Core-electron binding energies of the first thirty elements, Physical Review B, Vol. 15, pp. 544-552, 1977.) (a) There are peaks at energies of 64.8 and 5.4 eV, corresponding to 2 and 1 electrons, respectively. (b) There are peaks at energies of 3614, 384, 301, 40.9, 24.7, and 4.34 eV, corresponding to 2, 2, 6, 2, 6, and 1 electrons, respectively. (c) There are peaks at energies of 4494, 503, 404, 56.4, 33.6, 8.01, and 6.65 eV, corresponding to 2, 2, 6, 2, 6, 1, and 2 electrons, respectively.
We expect the atomic radius to increase going down a group in the periodic table. Can you suggest why the atomic radius of hafnium breaks this rule? (See data below.)
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L. Martin, S. P. Kowalczyk. F. R. McFeely, and L Ley: Core-electron binding energies of the first thirty elements Physical Review B, Vol. 15, pp. 544-552, 1977.) (a) There are peaks at energies corresponding to 1079, 70.8, 38.0, 5.14 eV, corresponding to 2, 2, 6, and 1 electrons, respectively. (b) There are peaks at energies corresponding to 4043, 443, 351, 48.4, 30.1, and 6.11 eV, corresponding to 2, 2, 6, 2, 6, and 2 electrons, respectively. (c) There are peaks at energies corresponding to 5475, 638, 524, 77, 47, 12. and 7.3 eV, corresponding to 2, 2, 6, 2, 6, 3, and 2 electrons, respectively.
Spectroscopic studies show that Na can have electrons in its 1s, 2s, 2p, and 3s Hartree orbitals, and that Zeff(3s)=1.84 . Using data from Problem 13, compare the energies of the Na 3s orbital, the Li 2s orbital, and the H 1s orbital.
The radius trend and the ionization energy trend are exact opposites. Does this make sense?
From Figure 8.18, predict the first ionization energy of francium (Z = 87).
Predict the larger ion in each of the following pairs. Give reasons for your answers. (a) O,S2 (b) Co2+,Ti2+ (c) Mn2+,Mn4+ (d) Ca2+,Sr2+
Cesium is used extensively in photocells and in television cameras because it has the lowest ionization energy of all the stable elements. (a) What is the maximum kinetic energy of a photoelectron ejected from cesium by 520 nm light? Note that if the wavelength of the light used to irradiate the cesium surface becomes longer than 660 nm, no photoelectrons are emitted. (b) Use the rest mass of the electron to calculate the velocity of the photoelectron in (a).
(a) Predict the atomic number of the (as yet undiscovered) alkali-metal element in the eighth period. (b) Suppose the eighth-period alkali-metal atom turned out to have atomic number 137. What explanation would you give for such a high atomic number (recall that the atomic number of francium is only 87)?