Concept explainers
(a)
Interpretation:
The arrangement of electron pairs around the central atom in the given molecule or ion is to be predicted. The sketch and name of the molecular structure for the given molecule or ion are to be stated.
Concept Introduction:
The geometry of the molecule is determined by electron pairs present around the central atom.
The formula to calculate number of electron pairs in compound is,
If electron pairs are
Similarly, if electron pairs are
(b)
Interpretation:
The arrangement of electron pairs around the central atom in the given molecule or ion is to be predicted. The sketch and name of the molecular structure for the given molecule or ion are to be stated.
Concept Introduction:
The geometry of the molecule is determined by electron pairs present around the central atom.
The formula to calculate number of electron pairs in compound is,
If electron pairs are
Similarly, if electron pairs are
(c)
Interpretation:
The arrangement of electron pairs around the central atom in the given molecule or ion is to be predicted. The sketch and name of the molecular structure for the given molecule or ion are to be stated.
Concept Introduction:
The geometry of the molecule is determined by electron pairs present around the central atom.
The formula to calculate number of electron pairs in compound is,
If electron pairs are
Similarly, if electron pairs are
(d)
Interpretation:
The arrangement of electron pairs around the central atom in the given molecule or ion is to be predicted. The sketch and name of the molecular structure for the given molecule or ion are to be stated.
Concept Introduction:
The geometry of the molecule is determined by electron pairs present around the central atom.
The formula to calculate number of electron pairs in compound is,
If electron pairs are
Similarly, if electron pairs are
(e)
Interpretation:
The arrangement of electron pairs around the central atom in the given molecule or ion is to be predicted. The sketch and name of the molecular structure for the given molecule or ion are to be stated.
Concept Introduction:
The geometry of the molecule is determined by electron pairs present around the central atom.
The formula to calculate number of electron pairs in compound is,
If electron pairs are
Similarly, if electron pairs are
(f)
Interpretation:
The arrangement of electron pairs around the central atom in the given molecule or ion is to be predicted. The sketch and name of the molecular structure for the given molecule or ion are to be stated.
Concept Introduction:
The geometry of the molecule is determined by electron pairs present around the central atom.
The formula to calculate number of electron pairs in compound is,
If electron pairs are
Similarly, if electron pairs are
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Introductory Chemistry: A Foundation
- For each of the following molecules or molecular ions, give the steric number, sketch and name the approximate molecular geometry, and describe the direction of any distortions from the approximate geometry due to lone pairs. In each case, the central atom is listed first and the other atoms are all bonded directly to it. (a) TeH2 (b) AsF3 (c) PCl4+ (d) XeF5+arrow_forwardUse the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3 Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.arrow_forwardThe antibiotic thiarubin-A was discovered by studying the feeding habits of wild chimpanzees in Tanzania. The structure for thiarubin-A is a. Complete the Lewis structure, showing all lone pairs of electrons. b. Indicate the hybrid orbitals used by the carbon and sulfur atoms in thiarubin-A. c. How many and bonds are present in this molecule?arrow_forward
- A paper published in the research Journal Science in 2007 (S. Vallina and R. Simo, Science, Vol. 315, p. 506, January 26, 2007) reported studies of dimethylsulfide (DMS), an important green-house gas that is released by marine phytoplankton. This gas represents the largest natural source of atmospheric sulfur and a major precursor of hygroscopic (i.e., cloud-forming) particles in clean air over the remote oceans, thereby acting to reduce the amount of solar radiation that crosses the atmosphere and is absorbed by the ocean. (a) Sketch the Lewis structure of dimethylsulfide, CH3SCH3, and list the bond angles in the molecule. (b) Use electronegativities to decide where the positive and negative charges lie in the molecule. Is the molecule polar? (c) The mean seawater concentration of DMS in the ocean in the region between 15 north latitude and 15 south latitude is 2.7 nM (nanomolar). How many molecules of DMS are present in 1.0 m3 of seawater?arrow_forwardThe strucrure of TeF5 is Draw a complete Lewis structure for TeF5, and explain the distortion from the ideal square pyramidal structure. (See Exercise 26.)arrow_forwardDraw the Lewis electron dot structures for these molecules, including resonance structures where appropriate: (a) CS32 (b) CS2 (c) CS (d) predict the molecular shapes for CS32 and CS2 and explain how you arrived at your predictionsarrow_forward
- 7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?arrow_forward7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?arrow_forward7.13 Figure 7-2 depicts the interactions of an ion with its first nearest neighbors, second nearest neighbors, and third nearest neighbors in a lattice, (a) Would the interactions with the fourth nearest neighbors be attractive or repulsive? (b) Based on Coulomb's law, how would the relative sizes of the terms compare if the potential energy were expressed as V=V1st+V2nd+V3rd+V4th ?arrow_forward
- Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. In an N—O bond. electron density is greater near the O atom. An N—O bond is an example of a polar covalent band. In general, chemical bonds form to minimize energy. The bond in KBr is formed by sharing electrons.arrow_forwardWhich of the molecules in Exercises 21 and 22 have net dipole moments (are polar)?arrow_forward7.84 Which of the following molecules is least likely to actually exist OF4,SF4,SeF4 , or TeF4 ? Why?arrow_forward
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