Two ions isoelectronic with carbon suboxide,
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Inorganic Chemistry
- (a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .arrow_forwardNitrogen exists as a diatomic molecule with a triple bond between the twoatoms, whereas the heavier elements of the group do not exist as E2at room temperature. Assign a reason.arrow_forwardIf an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? I know that group 3A atoms are elctron deficient, and that period 3 elements and below, except for group 3A elements like Aluminum, can expand their octet because of their available d-orbital, which may not be relevant to this problem. I don't understand this question, or why the answer would be 5A. Is it because 5A have odd valence electrons, and can form free radicals, like NO?arrow_forward
- ( ME 213: Properties of Material) Calculate the force of attraction between a K+ and an O2- ion the centers of whichare separated by a distance of 1.5 nm. My understanding is that in ionic bonds all atoms acquire stable configuration. Here potassium gives oxygen one electron. But oxygen needs two electrons to be stable. Hence it will not be stable.arrow_forward(a) Draw the best Lewis structure(s) for the nitrite ion, NO2-.(b) With what allotrope of oxygen is it isoelectronic?(c) What would you predict for the lengths of the bondsin NO2- relative to N¬O single bonds and doublebonds?arrow_forwardIn the series of group 5A hydrides, of general formulaMH3, the measured bond distances are P¬H, 1.419 Å;As¬H, 1.519 Å; Sb¬H, 1.707 Å. (a) Compare these valueswith those estimated by use of the atomic radii inFigure 7.7. (b) Explain the steady increase in M¬H bonddistance in this series in terms of the electron configurationsof the M atoms.arrow_forward
- 16. What is the molecular geometry of PH3? (A) Trigonal planar (B) T-shaped (C) Trigonal pyramidal (D) Tetrahedral 17. The correct Lewis structure for BF3 would have exactly: (A) 1 double bond (B) 2 double bonds (C) No double bonds (D) 1 triple bond 18. Nitrogen has a greater first ionization energy than phosphorus. What is the best evidence to support this observation? (A) Nitrogen has a greater effective nuclear charge. (B) A nitrogen atom is larger than a phosphorus atom. (C) The electron ionized from nitrogen is in a lower energy level closer to the nucleus. (D) The electron ionized from nitrogen is not from a valence energy level.arrow_forwardThe sulfate ion can be represented with four S-O bonds or with two S-O and two So=O bonds.(a) Which representation is better from the standpoint of formal charges?(b) What is the shape of the sulfate ion, and what hybrid orbitals of S are postulated for the σ bonding?(c) In view of the answer to part (b), what orbitals of S must be used for the π bonds? What orbitals of O?(d) Draw a diagram to show how one atomic orbital from S and one from O overlap to form a π bond.arrow_forward(i) What is the covalency of N in N2O5 ?(ii) Explain why phosphorus forms pentachloride whereas nitrogen andbismuth do not?arrow_forward
- (a) Construct a molecular orbital energy diagram of N₂. (b) Use this diagram to explain why the first ionization of N₂ is greater than that of N. (b) Use this diagram to predict which is more favorable: the first electron affinity of N₂ or that of N.arrow_forwardUse the following data to estimate AH; for potassium bromide. K(s) + Br2 (9) - KBr(a) Lattice energy -671 kJ/mol Ionization energy for K 419 kJ/mol Electron affinity of Br -325 kJ/mol Bond energy of Br2 Enthalpy of sublimation for K 193 kJ/mol 90. kJ/mol AH = kJ/molarrow_forwardWrite the electronic configuration of 3 Li and 26Fe and explain the possible valency they can exhibit.arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning