Ch. 2 - General Chemistry Translated: Finding the Electrons

Mullins - Organic Chemistry: A Learner Centered Approach 1st Edition

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Mullins 1st Edition

Ch. 2 - General Chemistry Translated: Finding the Electrons

Problem 72a,b

Chapter 1, Problem 72a,b

Refer to the following Lewis structures.
(a)
(b)
If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?

Verified step by step guidance

Step 1: Understand the concept of sp² hybridization. In sp² hybridization, one s orbital and two p orbitals mix to form three sp² hybrid orbitals. This leaves one unhybridized p orbital available for bonding or other interactions.

Step 2: Determine the number of sp²-hybridized orbitals. Since three orbitals (one s and two p) are hybridized, the atom will have three sp²-hybridized orbitals.

Step 3: Determine the number of unhybridized p orbitals. In sp² hybridization, one p orbital remains unhybridized. This unhybridized p orbital is perpendicular to the plane of the sp² orbitals and is often involved in π bonding.

Step 4: Summarize the findings. An atom with sp² hybridization uses three sp²-hybridized orbitals for bonding and has one unhybridized p orbital.

Step 5: Apply this understanding to specific molecules or Lewis structures as needed, identifying sp²-hybridized atoms and their bonding configurations.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is the concept in organic chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. In the case of sp² hybridization, one s orbital and two p orbitals combine to create three equivalent sp² hybrid orbitals, which are oriented in a trigonal planar geometry. This hybridization is crucial for understanding the bonding and geometry of molecules with double bonds or resonance structures.

Bonding Orbitals

Bonding orbitals are formed when atomic orbitals combine to create new orbitals that can accommodate electrons from two atoms. In sp² hybridization, the three sp² orbitals are used for sigma (σ) bonding with other atoms, while the remaining unhybridized p orbital can participate in pi (π) bonding, particularly in double bonds. This distinction is essential for predicting molecular shapes and reactivity.

Geometry of Molecules

The geometry of molecules refers to the three-dimensional arrangement of atoms within a molecule, which is influenced by the types of hybridization present. For sp² hybridized atoms, the geometry is trigonal planar, with bond angles of approximately 120 degrees. Understanding molecular geometry is vital for predicting the physical and chemical properties of compounds, including their reactivity and interaction with other molecules.

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Related Practice

Textbook Question

Predict the hybridization of all non-hydrogen atoms.

(c)

(d)

1020

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Textbook Question

Refer to the following Lewis structures.

(a)

(b)

Predict the hybridization of all non-hydrogen atoms.

962

views

Textbook Question

Refer to the following Lewis structures.

(c)

(d)

If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?

984

views

Textbook Question

For the following partial structures, the bond is shown. Add the indicated number of bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.

(c)

1443

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Textbook Question

Predict the hybridization of all non-hydrogen atoms.

(e)

(f)

(g)

1169

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Textbook Question

Connect the atoms using the indicated hybrid orbitals.