Ch.7 - Periodic Properties of the Elements

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.7 - Periodic Properties of the Elements

Problem 80a

Chapter 7, Problem 80a

Figure 7.4 shows the radial probability distribution functions for the 2s orbitals and 2p orbitals. (a) Which orbital, 2s or 2p, has more electron density close to the nucleus?

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Understand the concept of radial probability distribution: It describes the probability of finding an electron at a certain distance from the nucleus.

Identify the key difference between 2s and 2p orbitals: The 2s orbital has a spherical shape, while the 2p orbital has a dumbbell shape.

Consider the presence of nodes: The 2s orbital has a radial node, which affects electron density distribution.

Analyze the radial probability distribution functions: The 2s orbital typically shows a peak closer to the nucleus compared to the 2p orbital.

Conclude based on the analysis: The 2s orbital generally has more electron density close to the nucleus than the 2p orbital.

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Key Concepts

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

Radial Probability Distribution

The radial probability distribution function describes the likelihood of finding an electron at a certain distance from the nucleus in an atom. It is derived from the square of the wave function and provides insight into how electron density varies with distance. This concept is crucial for understanding where electrons are likely to be found in different orbitals.

Electron Density

Electron density refers to the probability of finding an electron in a given region of space around the nucleus. In the context of atomic orbitals, higher electron density indicates a greater likelihood of locating an electron near the nucleus. Comparing the electron densities of the 2s and 2p orbitals helps determine which orbital has more electrons concentrated close to the nucleus.

Orbital Shapes and Types

Orbitals are regions in an atom where electrons are likely to be found, and they come in different shapes and types, such as s and p orbitals. The 2s orbital is spherical, allowing for a higher probability of finding electrons near the nucleus, while the 2p orbital has a more complex shape with lobes extending further away. Understanding these shapes is essential for analyzing electron distribution in atoms.

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Textbook Question

(d) If you remove a single electron from a P atom, which orbital will it come from?

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Textbook Question

In Table 7.8, the bonding atomic radius of neon is listed as 0.58 Å, whereas that for xenon is listed as 1.40 Å. A classmate of yours states that the value for Xe is more realistic than the one for Ne. Is she correct? If so, what is the basis for her statement?

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Textbook Question

Consider the stable elements through lead (Z = 82). In how many instances are the atomic weights of the elements out of order relative to the atomic numbers of the elements?

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Textbook Question

(b) Repeat these calculations using Slater’s rules.

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Textbook Question

Write a balanced equation for the reaction that occurs in each of the following cases: (d) Fluorine reacts with water.

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