Number 2 only d. n=3m = 1m; = +½Corrected value:2. Without looking at the periodic table write the generic valence electron configuration for the first threeperiods of group 4A (14).3. Give the symbol for the ion that would be formed if cadmium (Cd) gained 2 electrons:Explain briefly why the answer for this question cannot be Sn2.4. Discuss the trend in atomic radius across a period. Explain why the general trend is that radius increasesacross the period from left to right, but in the d-block (transition metals) the atomic radius stays relativelyconstant.5. You and a friend went out for Silas and Maddy's ice cream and are enjoying your treat outside. Apedestrian, who is COVID positive, passes by you (not wearing a mask) and sneezes in your direction. Tdroplets from their uncovered sneeze travel at a velocity of 35.0 m/s ± 1%, what is the uncertainty inposition of the coronavirus from their sneeze if the virus mass is 2.14 × 10-14 g?

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Answered: 2. Without looking at the periodic…

2. Without looking at the periodic table write the generic valence electron configuration for the first three periods of group 4A (14).

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter7: The Structure Of Atoms And Periodic Trends

Section: Chapter Questions

Problem 64GQ: Answer the questions below concerning ground state electron configurations. (a) What element has the...

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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.)
The radius trend and the ionization energy trend are exact opposites. Does this make sense?
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.
Cerium, as noted in Applying Chemical Principles: 22.3 The Rare Earths, is a relatively abundant lanthanide element that has some important uses. Cerium(IV) oxide. CeO2, is widely used as a polishing agent for glass. Cerium(III) sulfide, Ce2S3, is becoming more widely used as a red pigment to replace cadmium pigments, which are environmentally less desirable. (a) Give the electron configurations (using the noble gas notation) for Ce, Ce3+, and Ce4+. (b) Is either Ce3+ or Ce4+ paramagnetic? If so, how many unpaired electrons does each have? (c) The solid state structure for CeO2 is shown below. Describe the unit cell of the compound. How is this structure related to the formula?
Answer the questions below concerning ground state electron configurations. (a) What element has the electron configuration [Ar]3d64s2? (b) What element has a 2+ ion with the configuration [Ar]3d5? Is the ion paramagnetic or diamagnetic? (c) Mow many unpaired electrons are in a Ni2+ ion? (d) The configuration for an element is given here. What is the identity of the element? Is a sample of the element paramagnetic or diamagnetic? How many unpaired electrons does a 3 ion of this element have? (e) What element has the following electron configuration? Write a complete set of quantum numbers for electrons 1-3.
The electron affinity of the lutetium atom (element 71) was measured using the technique of photoelectron spectroscopy with an infrared laser (the essay on p. 310 describes this instrumental method, using X rays). In this experiment, a beam of lutetium negative ions, Lu, was prepared and irradiated with a laser beam having a wavelength at 1064 nm. The energy supplied by a photon in this laser beam removes an electron from a negative ion, leaving the neutral atom. The energy needed to remove the electron from the negative ion to give the neutral atom (both in their ground states) is the electron affinity of lutetium. Any excess energy of the photon shows up as kinetic energy of the emitted electron. If the emitted electron in this experiment has a kinetic energy of 0.825 eV, what is the electron affinity of lutetium?
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.
Thallium has the ground-state configuration [Xe]4f145d106s26p1. Give the group and period for this element. Classify it as a main-group, a d-transition, or an f-transition element.
The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.
Which of the following statements correctly describes the value of the effective nuclear charge. Z, felt by (a) the 2s electron at a large distance from a Li atom? (i) Z equals 1. (ii) Z is between 1 and 3. (iii) Z equals 3. (b) the 2s electron at its most probable distance from the nucleus of a Li atom? (i) Z equals 1. (ii) Z is between 1 and 3. (iii) Z equals 3.
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?