Concept explainers
(a)
Interpretation:
The polar nature of
Concept Introduction:
Polarity results from the uneven partial charge distribution between various atoms in a compound. Atoms, such as nitrogen, oxygen, and halogens that are more electronegative have a tendency to have partial negative charges. Atoms, such as carbon and hydrogen, have a tendency to be more neutral or have partial positive charges.
Polar nature of the molecules can be measured by the dipole moment. If a molecule has zero dipole moment then it is a non polar molecule. If a molecule has a net dipole moment then it is a polar molecule.
(b)
Interpretation:
The polar nature of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The polar nature of
Concept Introduction:
Refer to part (a).
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Chemistry Principles And Practice
- Which of the following is a polar molecule? (A) All of them are (B) SO2 (C) PCl3 (D) CH3Cl (E) O3arrow_forwardWhich of the following molecules does not have a dipole moment? (a) CH3Cl (b) CH2Cl2 (c) CFCl3 (d) CHCl3arrow_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_forward
- The structure of caffeine is shown below. (a) Complete the Lewis structure. (b) How many pi bonds are present in caffeine? How many sigma bonds? (c) Identify the hybridization of the carbon atoms. (d) What is the value of the O-C-N angle?arrow_forwardWhich of these molecules has a linear molecular geometry and the molecule is polar? (A) CO2 (B) Cl2O (C) N2O (D) SO2arrow_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
- 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 (c) PCI (b) AsF3 (d) XeFarrow_forwardNitrogen trifluoride (NF3) is used in the electronics industry to clean surfaces. NF3 is also a potent greenhouse gas. (A) Draw the Lewis structure of NF3 and determine its molecular geometry. (B) BF3 and NF3 both have three covalently bonded fluorine atoms around a central atom. Do they have the same dipole moment? (C) Could BF3 also behave as a greenhouse gas? Explain why or why not.arrow_forwardAre the following molecules polar or nonpolar? (a) CH2Cl2 (b) SO3 (c) SO2 (d) NH3arrow_forward
- a) Methane 1CH42 and the perchlorate ion 1ClO4- 2 are both described as tetrahedral. What does this indicate about their bond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forwardDraw the Lewis structures for CO2 and CO, and predict the number of σ and π bonds for each molecule.(a) CO2(b) COarrow_forwardWhich of the following molecules or ions contain polar bonds?(a) O3(b) S8(c) O22−(d) NO3−(e) CO2(f) H2S(g) BH4−arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning