Complete the table below. Element Electronic Distribution Last sublevel Orbital Quantum numbers of last electron in the last sublevel Quantum numbers of specifie electron Orbital Electron Configuration Write the electronic of e- in the main configuration diagram of last (last written electronic diagram of specifie electron configuration of specific electron sublevel configuration in the format below: Is 2s 3s 4s 2p" 3p" 3d energy level configuration configuration) configuration K= 2 Electron #9 n=2 1= 1 Example: 1=2 ml =2 L=8 M = 13 N= 2 2p Mn 3d 25 ml = 0 Electron # 17 Cd 48 Electron # 53 Ir

Complete the table below. Element Electronic Distribution Last sublevel Orbital Quantum numbers of last electron in the last sublevel Quantum numbers of specifie electron Orbital Electron Configuration Write the electronic of e- in the main configuration diagram of last (last written electronic diagram of specifie electron configuration of specific electron sublevel configuration in the format below: Is 2s 3s 4s 2p" 3p" 3d energy level configuration configuration) configuration K= 2 Electron #9 n=2 1= 1 Example: 1=2 ml =2 L=8 M = 13 N= 2 2p Mn 3d 25 ml = 0 Electron # 17 Cd 48 Electron # 53 Ir

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 2P

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Givethreeexamplesofionsthatwouldbeisoelectronicwithneon1s 2 2s 2 2p 6
Many compounds of the transition-metal elements containdirect bonds between metal atoms. We will assumethat the z-axis is defined as the metal–metal bond axis.(a) Which of the 3d orbitals (Figure 6.23) is most likely tomake a σ bond between metal atoms? (b) Sketch the s3dbonding and σ*3d antibonding MOs. (c) With reference tothe “Closer Look” box on the phases of orbitals, explain whya node is generated in the σ*3d MO. (d) Sketch the energyleveldiagram for the Sc2 molecule, assuming that only the3d orbital from part (a) is important. (e) What is the bondorder in Sc2?
Many compounds of the transition-metal elements containdirect bonds between metal atoms. We will assumethat the z-axis is defined as the metal–metal bond axis.(a) Which of the 3d orbitals (Figure 6.23) is most likely tomake a s bond between metal atoms? (b) Sketch the s3dbonding and s*3d antibonding MOs. (c) With reference tothe “Closer Look” box on the phases of orbitals, explain whya node is generated in the s*3d MO. (d) Sketch the energyleveldiagram for the Sc2 molecule, assuming that only the3d orbital from part (a) is important. (e) What is the bondorder in Sc2?
the options for atom B are linear, tetrahedral, or trigonal planar. Betwwen those would it be tetrahedral or trigonal planar?
The compound gallium arsenide is a commonly used semiconductor,having an energy gap Eg of 1.43 eV. Its crystal structureis like that of silicon, except that half the silicon atoms are replacedby gallium atoms and half by arsenic atoms. Draw a flattened-outsketch of the gallium arsenide lattice, following the pattern.What is the net charge of the (a) gallium and (b) arsenic ioncore? (c) How many electrons per bond are there? (Hint: Consultthe periodic table in Appendix G.)
Why catenation property is most remarkable in the case of carbon?
7.84 Which of the following molecules is least likely to actually exist OF4,SF4,SeF4 , or TeF4 ? Why?
hy is the molecular structure of H2Ononlinear, whereas that of BeF2is linear, even though both molecules consist of three atoms?
Benzene is commonly regarded as a resonance hybrid ofthe two Kekule structures. but other possible structures canalso contribute. Draw three other structures in which thereare only covalent n bonds (al lowing for bonding betweensome non-adjacent C atoms) and two structures in whichthere is one ionic bond. Why may these structures be ignoredin simple descriptions of the molecule?
The main reason alkali metal dihalides (MX₂) do notformis the high IE₂ of the metal. (a) Why is IE₂ so high for alkalimetals? (b) The IE2for Cs is 2255 kJ/mol, low enough for CsF₂to form exothermically (ΔHf=-125 kJ/mol). This compoundcannot be synthesized, however, because CsF forms with a muchgreater release of heat (ΔHf=-530 kJ/mol). Thus, the break-down of CsF₂ to CsF happens readily. Write the equation for thisbreakdown, and calculate the heat of reaction per mole of CsF.
(a) The ionization energy of potassium (K) is 4.34 eV and the electron affinity of chlorine (Cl) is -3.61 eV. The Madelung constant for the KCl structure is 1.748 and the distance between ions of opposite sign is 0.314 nm. On the basis of these data only, compute the cohesive energy of KCl per ion pair. (b) The observed cohesive energy of KCl is 6.42 eV per ion pair. On theassumption that the difference between this figure and that obtained in (a) is due to the exclusion principle repulsion, find the exponent n in the formula Br^-n for the potential energy arising from this source.
From As to Bi only a small increase is observed in covalent radius why?