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- s Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species. O CN O N2 O CN OCN+ 02 A. (025)?(02s*)?(n2p)* B. (025)?(025*)?(02p)?(n2p)*(n2p*)3 c. (025) (02s*)?(n2p)*(02p)²(n2p*)! D. (025)?(02s*)?(n2p)*(02p)! E. (025)?(025*)?(n2p)*(02p)? F. (02s)2(02s*)?(02p)?(n2p)*(n2p*)? G. (025)?(02s*)?(02p)²(n2p)ª(n2p*)* 1 ar ecUse the molecular orbital energy diagram below to answer the questions about bond order for the negative ionBe2−. Number of BondingValence Electrons? Number of AntibondingValence Electrons? Be2−Bond Orderfill in the blank 3 This corresponds to: fill in the blank 4 ...... A. Single bond E. Between a single and double bond B. Double bond F. Between a double and a triple bond C. Triple bond G. No bond, Be2− does not form. D. Half of a bondUse the molecular orbital energy diagram below to answer the questions about bond order for the positive ion H₂*. Number of Number of Bonding Electrons Antibonding Electrons | This corresponds to: A. Single bond B. Double bond C. Triple bond Half of a bond D. E hydrogen 1s Submit Answer A MO's 0* 1s 01s H₂+ Bond Order E. Between a single and double bond F. Between a double and a triple bond G. No bond, H₂+ does not form. + hydrogen * Retry Entire Group 1s 7 more group attempts remaining Previous Next
- For each of the following molecules, give the bond order, and describe them as paramagnetic or diamagnetic a. O2 b. N2 c. F2 d. N2- e. C2^(2-)3. In a pi bond, A. electron density lies along the internuclear axis. B. electron density lies above and below the internuclear axis. C. electrons are more dense than they are in sigma bonds. D. more than two electrons are involved in the bond. 4. The hybridization of the central atom in CIF3 is A. sp? B. sp C. sp'd D. sp?d? 5. Determine the formal charge on the nitrogen in the Lewis structure shown below. A. +1 В. -2 C.0 D. +2 : s=C-N:This question is related to valence bond theory. a. Explain the assumptions made in bonding models under valence bond theory. What best describes bonding under these models? b. Draw the Lewis structure of SO2. Identify bonds in the moldule as either sigma or pi bonds. Draw orbital diagrams for ground state S and O atoms. Use these orbital diagrams determine the geometry of SO2 using valence bond theory (hint: SO2 must be descried using hybrid atomic orbitals. In other words, which orbitals on which atoms overlap to give rise to which bonds? C. d. Explain why valence bond theory does not adequately describe the bonding in SO2, even though it accurately predicts the geometry/bond angle.
- 31. TRUE or FALSE: The orbital energy diagram represents a molecule in its ground state electron configuration? o u2s Energy g2p A. TRUE B. FALSE 11 2px 2py 2pz 2px 2py 2pz 1 Og2p Tu2p 32. TRUE or FALSE: The molecular orbital energy diagram describes the bonding in the diatomic molecule B21-? u2s A. TRUE B. FALSE 2s 2s Og2s 33. TRUE or FALSE: The molecular orbital energy diagram is representative of a paramagnetic molecule? A. TRUE B. FALSE 34. According to the molecular orbital energy diagram, the bond order of the molecule described is...? А. 1.0 В. 1.5 С. 2.0 D. 2.5 E. None of the above 35. Of the following molecular orbitals of this molecule that do NOT have cylindrical symmetry, which is the highest in energy...? A. oʻu2p В. п'92p C. Og2p D. πυ2p E. None of the aboveConsider a NF molecule a. Draw orbitals of each atorn and find possible interactions among them. b. Draw atomic orbitals. using the potential energy information c. Draw molecular orbitals from the atomic orbitals of N and F. d. What is the band order of this molecule? e. Specify the types of molecular orbitals, or (NF,NF? Which of the three has the longest bond length -NF, NF, and NF ? Explain your answer.Use the molecular orbital energy diagram below to answer the questions about bond order for the negative ion H2. Number of Number of H, Bond Order Bonding Electrons Antibonding Electrons This corresponds to: A. Single bond E. Between a single and double bond B. Double bond F. Between a double and a triple bond С. Triple bond G. No bond, H, does not form. D. Half of a bond hydrogen A MO's hydrogenB o 1s 1s - 1s
- One of the first drugs to be approved for use in treatment of acquired immune deficiency syndrome (AIDS) was azidothymidine (AZT). Complete the Lewis structure for AZT. a. How many carbon atoms are sp3 hybridized? b. How many carbon atoms are sp2 hybridized? c. Which atom is sp hybridized? d. How many σ bonds are in the molecule? e. How many π bonds are in the molecule? f. Wnat isthe N9N9N bond angle inthe azide (-N3) group? g. What is the H-Q-C bond angle in the side group attached to the five membered ring? h. What is the hybridization of the oxygen atom in the -CH2OH group?Consider the following molecule: d. b. c. a. What is the hybridization at each of the labeled carbon atoms? b. What is the electron-pair geometry at each of the labeled carbon atoms? c. Which orbitals are responsible for the following bonds? Indicate which types of orbitals are used (i.e. s, p, sp?, etc.) and which types of bonds are formed (o or T). i. Bond a-b ii. Bond b-c iii. Bond d-e iv. Bond between carbon b and a hydrogen bound to it.4. For each of the following hypothetical diatomic species: i. Draw the molecular orbital diagram ii. Calculate the bond order of the molecule iii. Predict whether or not the molecule is stable iv. State whether the molecule is paramagnetic or diamagnetic a. O22- b. Be2 c. F2 d. NO+