Concept explainers
(a)
Interpretation:
Whether
Concept Introduction:
VSEPR model is useful tool to determine shapes as well as properties such as polarity of molecules.
The extent of polarity is quantitatively expressed as dipole moment. It is defined as product of charges of two bonded atoms and the separation between them.
The electronegativity difference decides the direction of dipole moment. It is indicated by an arrow head from positive end towards negative end.
For complex molecules, the shape must be determined prior to determination of individual dipoles. Thus shape is governed by the VSEPR model.
(b)
Interpretation:
Whether
Concept Introduction:
Refer to part (a).
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CHEM PRINCIPLES LL W/ACHIEVE ONE-SEM
- Consider the molecules SCl₂, F₂, CS₂, CF₄, and BrCl.(a) Which has bonds that are the most polar?(b) Which have a molecular dipole moment?arrow_forward1. Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central atom. (a) POF3 (b) XeO₂F3+ (c) BrCl₂ (d) N3 (the central atom is N; two other N's are bonded to it) (e) PF3arrow_forwardWhat are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(a) ClF5(b) ClO2−(c) TeCl42−(d) PCl3(e) SeF4(f) PH2−arrow_forward
- The Lewis structure of BH2Cl (a) Is the molecule polar or nonpolar? (b) What is the hybridization of the carbon atom? (c) What is the geometric shape of the molecule?arrow_forward(a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forwardAn important starting material for the manufacture ofpolyphosphazenes is the cyclic molecule (NPCl₂)₃. The mol-ecule has a symmetrical six-membered ring of alternating N and P atoms, with the Cl atoms bonded to the P atoms. The nitrogen-phosphorus bond length is significantly less than that expectedfor an N−P single bond.(a) Draw a likely Lewis structure for the molecule.(b) How many lone pairs of electrons do the ring atoms have?(c) What is the order of the nitrogen-phosphorus bond?arrow_forward
- . Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?arrow_forwardA common form of elemental phosphorus is the tetrahedralP4 molecule, where all four phosphorus atoms areequivalent: At room temperature phosphorus is a solid. (a) Are there anylone pairs of electrons in the P4 molecule? (b) How manyP¬P bonds are there in the molecule? (c) Draw a Lewisstructure for a linear P4 molecule that satisfies the octet rule.Does this molecule have resonance structures? (d) On thebasis of formal charges, which is more stable, the linear moleculeor the tetrahedral molecule?arrow_forwardA common form of elemental phosphorus is the tetrahedralP4 molecule, where all four phosphorus atoms areequivalent:At room temperature phosphorus is a solid. (a) Are there anylone pairs of electrons in the P4 molecule? (b) How manyP¬P bonds are there in the molecule? (c) Draw a Lewisstructure for a linear P4 molecule that satisfies the octet rule.Does this molecule have resonance structures? (d) On thebasis of formal charges, which is more stable, the linear moleculeor the tetrahedral molecule?arrow_forward
- 15. Which of the following species is not likely to have a tetrahedral shape? (a) SiBr4 (b) NF4+, (c) SF4, (d) BeCl4–2, (e) BF4–, (f) AlCl4–arrow_forwardWhich statement is always true according to VSEPR theory?(a) The shape of a molecule is determined only by repulsions among bonding electron groups.(b) The shape of a molecule is determined only by repulsions among nonbonding electron groups.(c) The shape of a molecule is determined by the polarity of its bonds.(d) The shape of a molecule is determined by repulsions among all electron groups on the central atom (or interior atoms, if there is more than one).arrow_forwardCommon exceptions to the octet rule are compounds and polyatomic ions with central atoms having more than 8 electrons around them. Phosphorus pentafluoride, PF5; sulfur tetrafluoride, SF4; xenon tetrafluoride, XeF4; and tri-iodide ion, I3, are all examples of exceptions to the octet rule. (a) Draw the Lewis structures of these substances.(b) For which elements in these substances can theatoms have more than 8 electrons around them?(c) How can the atoms of the elements youidentified in Part (b) be surrounded by morethan 8 electrons?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning