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Concept explainers
(a)
Interpretation:
The hybridization of atomic orbitals should be described briefly.
Concept introduction:
When there is a formation of a new set of orbitals by overlapping of valence shell atomic orbitals, it is called as hybridization and the orbitals are known as hybridized orbitals.
These newly formed hybridized orbitals are present in equal number to the
(b)
Interpretation:
The
Concept introduction:
Hybridization resulted due to the formation of a new set of orbitals by overlapping of valence shell atomic orbitals and the orbitals are known as hybridized orbitals.
When hybridized orbitals are again overlapped with other hybridized orbitals or valence shell orbitals through the inter-nuclear axis, it is known as a sigma bond.
(c)
Interpretation:
The Kekule structure of benzene should be explained.
Concept introduction:
Kekule was the first scientist who had given the first stable structure of benzene in which six carbons of benzene are present in a hexagonal shape.
In this structure, each carbon contains one hydrogen atom with it and single and double bonds are present in between carbon-carbon atoms.
(d)
Interpretation:
Theband theory should be explained for metallic bonding.
Concept introduction:
Metallic bonding is a term used to represent the
This type of bonding is the strongest bonding as metals have strong attraction forces between them.
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Chapter 11 Solutions
General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)
- Aspirin, or acetylsalicylic acid, has the formula C9H8O4 and the skeleton structure (a) Complete the Lewis structure and give the number of bonds and bonds in aspirin. (b) What is the hybridization about the CO2H carbon atom (colored blue)? (c) What is the hybridization about the carbon atom in the benzene-like ring that is bonded to an oxygen atom (colored red)? Also, what is the hybridization of the oxygen atom bonded to this carbon atom?arrow_forwardAcrylonitrile, C3H3N is the building mer Orlon. Its Lewis structure is What is the hybridization of nitrogen and of the three numbered carbon atoms?arrow_forwardIt is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forward
- Consider the polyatomic ion IO65-. How many pairs of electrons are around the central iodine atom? What is its hybridization? Describe the geometry of the ion.arrow_forwardIn ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another. (a)What is the best choice of hybridization scheme for the atoms of ozone? (b) For one of the resonance forms of ozone, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons? (c) Which of the orbitals can be used to delocalize the π electrons? (d) How many electrons are delocalized in the π system of ozone?arrow_forward(a) Complete the Lewis structure for the molecule shown below. How many lone pairs are there? H-C H 1 H (b) Give the hybridizations of the following atoms in the structure: (i) Ca; (ii) Ob (c) Give approximate values of the following bond angles: (i) O a-Ca-Ob; (ii) С a -О b-Сbarrow_forward
- The drawing below shows the overlap of two hybrid orbitalsto form a bond in a hydrocarbon. (a) Which of the followingtypes of bonds is being formed: (i) C¬C σ, (ii) C¬C π,or (iii) C¬H σ? (b) Which of the following could be theidentity of the hydrocarbon: (i) CH4, (ii) C2H6, (iii) C2H4, or(iv) C2H2?arrow_forward(c) Describe the hybridization of sulfur in sulfur hexafluoride.arrow_forward(a) Write a single Lewis structure for SO3 , and determine the hybridization at the S atom. (b) Are there other equivalent Lewis structures for the molecule? (c) Would you expect SO3 to exhibit delocalized π bonding?arrow_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_forwardDraw the molecular orbital energy diagrams for the valence electrons in the following diatomic molecules. Calculate the bond order and indicate if each of them is diamagnetic or paramagnetic. (а) В> (b) С. (c) CO (d) NO (е) Оzarrow_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_forward
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