Concept explainers
(a)
Interpretation:
Lewis structure for
Concept Introduction:
Lewis structures are diagrams that represent the
Electron geometry is the shape of a molecule predicted by considering both bond electron pairs and lone pair of electrons.
Molecular geometry is the shape of a molecule predicted by considering only bond pair of electrons
Geometry of different type of molecules with respect to the number of electron pairs are mentioned below,
(b)
Interpretation:
Hybridisation of each carbon atom in
Concept Introduction:
Refer to (a).
(c)
Interpretation:
Whether croconate ion is planar or not has to be determined.
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Chemistry: The Molecular Science
- 4. (a) Draw the shape of the atomic valence orbitals formed by the overlaping of two fluoride 2p atomic orbitals. (b) Draw the molecular orbital diagrams for F2 and F2*. Identify their bond order and magnetic properties. (c) An unstable nucleus exhibit radioactivity. (i) Explain how the number of protons and neutrons in a radioactive nucleus can be used to predict its probable mode decay. (ii) Illustrate your answer in (i) with a schematic graph.arrow_forwardConsider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product 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_forward
- Nitrogen 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_forward(a) Triazine, C3 H3 N3, is like benzene except that in triazineevery other C¬H group is replaced by a nitrogen atom.Draw the Lewis structure(s) for the triazine molecule. (b) Estimatethe carbon–nitrogen bond distances in the ring.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_forward
- For each of the following molecule: (i) draw the correct Lewis structure; (ii) determine the molecular geometry and the type of hybridization on the central atom, and (iii) predict whether the molecule is polar or nonpolar. (a) BrCl5arrow_forwardA useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers.(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds.(c) Describe the atomic orbitals that form the π bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.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
- Butadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths: (a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.arrow_forwardAmmonia, NH3, reacts with incredibly strong bases to producethe amide ion, NH2-. Ammonia can also react with acidsto produce the ammonium ion, NH4+. (a) Which species(amide ion, ammonia, or ammonium ion) has the largestH¬N¬H bond angle? (b) Which species has the smallestH¬N¬H bond angle?arrow_forward(a) Find the angle u between adjacent nearest-neighbor bonds in the silicon lattice. Recall that each silicon atom is bonded to four of its nearest neighbors.The four neighbors form a regular tetrahedron— a pyramid whose sides and base are equilateral triangles. (b) Find the bond length, given that the atoms at the corners of the tetrahedron are 388 pm apart.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning