Use the method of Figure 11-18 to represent bonding in each of the following molecules: (a) CCl4

Use the method of Figure 11-18 to represent bonding in each...

Key Concepts

Resonance Structures

Resonance structures are multiple valid representations of a molecule’s bonding that illustrate electron delocalization when a single Lewis structure is insufficient. They collectively describe the distribution of electrons in cases where bonds or charges are spread out over two or more atoms, providing a more comprehensive understanding of the molecule’s electronic structure.

Orbital Hybridization

Orbital hybridization is the concept where atomic orbitals mix to form new, equivalent hybrid orbitals that dictate the geometry of molecular bonding. This concept explains how atoms adopt specific shapes (for example, tetrahedral, trigonal planar, or bent geometries) based on the number and type of bonds they form.

Lewis Structures

Lewis structures are diagrams that represent the bonds between atoms and the placement of electrons in a molecule. They use lines to indicate bonds and dots to show lone pairs, providing a simple way to visualize how atoms achieve stable electron configurations and satisfy the octet (or duplet) rule.

Valence Electron Counting

Valence electron counting is the process of determining the total number of electrons available for bonding in a molecule by summing the valence electrons of each atom. This fundamental step ensures that the constructed bonding diagram accurately reflects the electron distribution necessary for forming bonds and assigning lone pairs.

Transcript

00:01 Explanation for the question here here we have to represent bonding in each of the following modules part a is ccl 4 and part b is we have on c l c l then next we have part c is h o n o and part d is c l so here in tetrachlorate the total number of valence electrons in ccl4 is 32 valence electrons here total valence electrons are 32 valence electrons and the lavish structure can be written as we have lavish structure for this compound is your carbon centralitone chlorine having lawn pairs 1 2 3 4 5 6 7 8 and chlorine 1 2 3 4 5 6 7 8 and chlorine 1 2 3 4 5 6 7 8 so there are 4 electron groups around the central carbon atom all bond pairs and the electron group geometry according to whisper corresponding to tetrahedral tetrahedral geometry is from tetrahedal geometry according to valence cell electron pair calcium theory and this corresponds to sp3 hybridization and the hybridization is sp3 having four bonded atoms non -on pair hybridobuses are used to form sigma bond with carbon chlorine there is sigma bond and next we have the other compound is onco.

02:48 The total number of valence electrons in onco is 18 valence electrons.

02:57 So the lavish structure can be written as here.

03:00 Lovist structure for the given compound is oxygen, nitrogen, chlorine.

03:09 Then we have oxygen, double bond and then chlorine single one.

03:17 Loan pairs, long pair here, and long pair, chlorine, and this form, this structure.

03:34 And there are three electron groups around the central atom.

03:40 Around the central atom, there are three electrons group, central nitrogen atom, two bonded pairs and one lone pair of the electron.

03:53 One lone pair of the electron, and two bonded atoms.

03:58 Nitrogen group geometry according to whisper corresponding to trigonal planar geometry it is trigonal planar geometry trigonal planar geometry this correspond to sp2 hybridization and hybridization is sp2 of central carbon atom one sp2 hybrid orbital is used to form a sigma bond with chlorine atom sigma bond with chlorine atom the other sp2 hybrid orbital is used to form a sigma bond with oxygen atom.

04:41 The unhybridged p orbital of the carbon atom is used to form a pie bond here.

04:47 With oxygen for chlorine, the 3 p orbitals can be used for end -to -end overlap in the sigma bond to carbon...

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