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Ch.6 - Electronic Structure of Atoms
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.6 - Electronic Structure of AtomsProblema 65
Capitolo 6, Problema 65

(b) In what sense does a 2p orbital have directional character? Compare the 'directional' characteristics of the px and dx² - y² orbitals. (That is, in what direction or region of space is the electron density concentrated?)

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Understand the concept of atomic orbitals: Atomic orbitals are regions in space where there is a high probability of finding an electron. Each type of orbital (s, p, d, f) has a unique shape and orientation.
Describe the 2p orbital: The 2p orbitals are dumbbell-shaped and have directional character because they are oriented along the x, y, or z axes. This means that the electron density is concentrated along these axes, giving them a specific direction in space.
Explain the px orbital: The px orbital is one of the three 2p orbitals, and it is oriented along the x-axis. The electron density is concentrated in two lobes on either side of the nucleus along the x-axis, indicating its directional character.
Describe the dx² - y² orbital: The dx² - y² orbital is one of the five d orbitals. It has a cloverleaf shape with lobes lying along the x and y axes. The electron density is concentrated in these lobes, making it directional, but in a different way compared to the p orbitals.
Compare the directional characteristics: While the px orbital has electron density concentrated along the x-axis, the dx² - y² orbital has electron density concentrated along both the x and y axes. This means the dx² - y² orbital has a more complex directional character, with electron density in regions between the axes as well.

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Orbital Shapes and Orientation

Orbitals are regions in an atom where there is a high probability of finding electrons. The 2p orbitals, which include px, py, and pz, have distinct shapes and orientations in three-dimensional space. The px orbital, for example, is oriented along the x-axis, while the py and pz orbitals are oriented along the y and z axes, respectively. This directional character influences how atoms interact and bond with one another.
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d Orbital Orientations

Electron Density Distribution

Electron density refers to the probability of finding an electron in a particular region of space around the nucleus. In the case of the px orbital, the electron density is concentrated along the x-axis, while the dx² - y² orbital has a unique shape that focuses electron density along the x and y axes, forming lobes in the quadrants of the xy-plane. Understanding these distributions is crucial for predicting chemical bonding and molecular geometry.
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Velocity Distributions

Comparison of Orbital Characteristics

When comparing the px and dx² - y² orbitals, it is important to note their different shapes and electron density distributions. The px orbital has a simple lobular shape along the x-axis, while the dx² - y² orbital has a more complex shape with four lobes oriented towards the corners of the xy-plane. This difference in orientation and shape affects how these orbitals overlap with others during chemical bonding, influencing molecular structure and reactivity.
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Molecular Orbital Theory
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(d) For the hydrogen atom, list the following orbitals in order of increasing energy (that is, most stable ones first): 4f, 6s, 3d, 1s, 2p.

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(c) What can you say about the average distance from the nucleus of an electron in a 2s orbital as compared with a 3s orbital?

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(a) With reference to Figure 6.19, what is the relationship between the number of nodes in an s orbital and the value of the principal quantum number?

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For the table that follows, write which orbital goes with the quantum numbers. Don't worry about x, y, z subscripts. If the quantum numbers are not allowed, write 'not allowed.' n l ml Orbital 2 1 -1 2p (example) 1 0 0 3 -3 2 3 2 -2 2 0 -1 0 0 0 4 2 1 5 3 0

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Sketch the shape and orientation of the following types of orbitals: (a) px, (b) dz2, (c) dx2 - y2.

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Sketch the shape and orientation of the following types of orbitals: (a) s, (b) pz, (c) dxy.

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