In Table 7.8, the bonding atomic radius of neon is listed as58 pm, whereas that for xenon is listed as 140 pm. A classmateof yours states that the value for Xe is more realisticthan the one for Ne. Is she correct? If so, what is the basisfor her statement?

Verified step by step guidance

Understand the concept of atomic radius: Atomic radius is the measure of the size of an atom, typically the distance from the center of the nucleus to the boundary of the surrounding cloud of electrons.

Recognize the trend in atomic radii across the periodic table: Generally, atomic radii increase down a group due to the addition of electron shells.

Compare the positions of Neon (Ne) and Xenon (Xe) in the periodic table: Neon is in the second period and Xenon is in the fifth period, both in Group 18 (noble gases).

Consider the effect of increased electron shells: As you move from Neon to Xenon down Group 18, the number of electron shells increases, which generally leads to an increase in the atomic radius despite the increase in nuclear charge.

Evaluate the statement based on periodic trends: Given that Xenon has more electron shells than Neon, it is expected to have a larger atomic radius, making the larger value for Xenon more consistent with periodic trends.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

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

Atomic Radius

The atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electron shell. It varies across the periodic table, generally increasing down a group due to the addition of electron shells and decreasing across a period due to increased nuclear charge, which pulls electrons closer to the nucleus.

Noble Gases and Their Properties

Noble gases, such as neon and xenon, are characterized by their complete valence electron shells, making them largely unreactive. However, their atomic radii differ significantly due to their position in the periodic table, with xenon being larger than neon. This difference is important when discussing bonding atomic radii, as it reflects the effective size of the atoms in various contexts.

Bonding Atomic Radius vs. Van der Waals Radius

The bonding atomic radius refers to the size of an atom when it forms a bond with another atom, while the Van der Waals radius describes the size of an atom when it is not bonded but is in close proximity to another atom. The discrepancy in the atomic radii of neon and xenon can be attributed to their different bonding behaviors and the types of interactions they typically engage in, which can influence the perceived 'realism' of their atomic sizes.

Recommended video:

Guided course

01:40

Van der Waals Equation

Related Practice

Textbook Question

(c) Detailed calculations indicate that the effective nuclear charge is 5.6+ for the 3s electrons and 4.9+ for the 3p electrons. Why are the values for the 3s and 3p electrons different?

Textbook Question

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

Textbook Question

The As ¬ As bond length in elemental arsenic is 2.48 Å. The Cl ¬ Cl bond length in Cl2 is 1.99 Å. (a) Based on these data, what is the predicted As ¬ Cl bond length in arsenic trichlo- ride, AsCl₃, in which each of the three Cl atoms is bonded to the As atom?

Textbook Question

The As ¬ As bond length in elemental arsenic is 2.48 Å. The Cl ¬ Cl bond length in Cl2 is 1.99 Å. (b) What bond length is predicted for AsCl₃, using the atomic radii in Figure 7.7?

Textbook Question

The following observations are made about two hypotheticalelements A and B: The A¬A and B¬B bond lengths in theelemental forms of A and B are 236 and 194 pm, respectively.A and B react to form the binary compound AB2, which hasa linear structure (that is B-A-B = 180°). Based on thesestatements, predict the separation between the two B nucleiin a molecule of AB2.