a. How many molecular orbitals will be formed by combination of the 28 and 2p atomic orbitals in 3.00 mol of Be atoms? molecular orbitals b. At OK, what fraction of molecular orbitals, formed by combination of the 2s and 2p atomic orbitals of Be atoms, will be occupied by electron pairs (all orbitals filled up to the Fermi level)? 01 01/4 03/8 01/22 03/4 01/8

a. How many molecular orbitals will be formed by combination of the 28 and 2p atomic orbitals in 3.00 mol of Be atoms? molecular orbitals b. At OK, what fraction of molecular orbitals, formed by combination of the 2s and 2p atomic orbitals of Be atoms, will be occupied by electron pairs (all orbitals filled up to the Fermi level)? 01 01/4 03/8 01/22 03/4 01/8

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

Chapter12: The Solid State

Section: Chapter Questions

Problem 20PS

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wich conjugate pir would be the best amortiguator a. HCI, NaCl ОБ. СНЗСООН, СНЗСОONa О с. НЗРО4, Na3PО3 O d. HNO3, NaNO3 O e. H2CO3, NaNO2
11. Based on application of the VSEPR theory, which molecule is trigonal bipyramidal? А. ВF, B. ASF. C. SF4 D. XEOF. E. SÞC1, Use the diagram below to answer the following question # 12-15: B 1 atm 0.5 stm A 50 150 250 350 T, "C+ 12. Melting occurs along the: А. АC ine B. CB line C. CD line D. All of the choices are possible. 13.The temperature and pressure at which all three phases can coexist in equilibrium is: B. 1.0 atm and 140°c D. 0.45 atm and 130°C. A. 0.25 atm and 110°C C. 1.25 atm and 300°C 14.The nomal boiling point of this substance is approximately: A.25'C В. 140 "с C. 300 "C D. 350'C 15. What phases can be present at 200°C and 0.75 atm pressure? A.Only the vapor phase C. Only the solid phase B. Only the liquid phase D. Both solid & vapor phases
The features of polar bonds can be illustrated by considering HF. The general form of the molecular orbital is y = GHY + GỰF, where y, is an H1s orbital and ựe is an F2p, orbital (with z along the internuclear axis, the convention for linear mol- ecules). The relevant data are leV Egglev H 13.6 0.75 F 17.4 3.40 Calculate the energies and coefficients of the bonding and antibonding orbitals made from this combination of atomic orbitals in HF.
The picture below shows two atomic orbitals on two neighboring atoms. The orbitals have the specific phases and orientation pictured. Use this picture to answer the questions in the table below. If the orbitals come together as shown in the picture, can a molecular orbital (MO) be formed? JT O yes If you answered yes write the type of orbital formed using the buttons in the palette. O no Tf the atomic orbitale can intoract to makoa molocular orhital 回品回白

Please help me understand this. The geometry of the CS2 molecule is best described asA. linear.B. trigonal planar.C. tetrahedral.D. trigonal pyramidal.
Which linear combination of H and F atomic orbitals, f;, forms the bonding molecular orbital, y, in HF? Notes: The coefficient, c, represents the fractional contribution of f to y. Assume the z axis is the internuclear axis. y = -CHỘHIS – CPOFIS, CH CP y = CHYHIS + CrOF2pr, has cH = CH y = CHVHIS - CrOF2px, has CH < CF y = CHOHIS + CrộF2pz, has CH < CF
The diagram below shows the molecular orbital energy levels for valence electrons of the S2 molecule, which forms when sulphur is vapourised at high temperatures. 1. How many valence electrons are there in S2? 2. Identify the HOMO for each of the three species S2, S22-, S2+ 3. Calculate the bond order for each of the three species S2, S22-, S2+ 4. List the three species in order of predicted increasing bond energy. 5. Identify which, if any, of the three species S2, S22-, S2+ is paramagnetic, and briefly explain your answer.
Which of the following molecules is non-polar? KCI O A. NaCl В. Al P C. OD. F2 CaO E.
In the construction of molecular orbital diagram involving a hypervalence system of hexafluoro sulphur, only 12 valence electrons are distributed across the molecular orbitals. Explain why this is so?
a.An s orbital and a p orbital can combine to form molecular orbitals in a couple different ways. Draw a sketch of the overlap between these two atomic orbitals that would produce each of the following molecular orbitals. A. a sigma bonding MO B. a sigma antibonding MO b. For each of the following molecules, make a list of the molecules that are (i) polar, (ii) nonpolar and (iii) ionic. A. NH 3 B. H2 O C. CH3 CH2 CH3 D. NH4 Cl E. Na2 SO 4 F. CH3 Cl G. C6H6OH H. CH3COOH I. LiNO3
2. It has been reported that 3-electron bonds may be possible. These bonds would be similar to "normal" two-electron bonds, except that three electrons would be required for each bond. I was curious as to what might happen to molecular geometries if ALL bonds involved three electrons and ALL lone pairs were actually lone triplets. Under this system, and using the VSETR (Valence Shell Electron Triplet Repulsion) Model, predict the ideal molecular geometries of the following molecules. (NOTES: The number of valence electrons for each atom remains the same; only worry about VSE Triplets around the central atom; electron triplets would still want to position themselves around the atom just like doublets.) a. FH;2 b. ХеН c. FH2 d. H30
40. Buckminsterfullerene, C60, is an allotrope of carbon. Examine its structure below, and predict how many unhybridized p orbitals there are in a С6⁰ molecule. a. 10 b. 20 c. 30 d. 60 e. 120