Ch.5 - Periodicity & Electronic Structure of Atoms

McMurry8th EditionChemistryISBN: 9781292336145Non è quello che usi tu?Cambia libro di testo

McMurry 8th Edition

Ch.5 - Periodicity & Electronic Structure of Atoms

Problema 121

Capitolo 5, Problema 121

Order the following atoms according to increasing atomic radius: Rb, Cl, As, K.

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Identify the periodic trend for atomic radius: Atomic radius generally increases as you move down a group and decreases as you move across a period from left to right.

Locate each element on the periodic table: Rb (Rubidium) and K (Potassium) are in Group 1, Cl (Chlorine) is in Group 17, and As (Arsenic) is in Group 15.

Compare elements within the same group: Rb and K are in the same group, with Rb below K, so Rb has a larger atomic radius than K.

Compare elements across periods: Cl is in Period 3, As is in Period 4, K is in Period 4, and Rb is in Period 5. Elements in higher periods generally have larger atomic radii.

Order the elements by increasing atomic radius: Start with the smallest atomic radius and proceed to the largest based on their positions in the periodic table.

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Atomic Radius

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.

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02:02

Atomic Radius

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. For atomic radius, the trend shows that elements in the same group have larger radii as you go down, while elements in the same period have smaller radii as you move from left to right due to effective nuclear charge.

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00:38

Periodic Trends

Group and Period Positioning

The position of an element in the periodic table, defined by its group (vertical column) and period (horizontal row), significantly influences its atomic radius. For instance, rubidium (Rb) and potassium (K) are in Group 1 and have larger atomic radii compared to chlorine (Cl) and arsenic (As), which are in Groups 17 and 15, respectively, leading to a clear ordering based on their positions.

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Lone Pair Positions

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Why do atomic radii decrease from left to right across a period of the periodic table?

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Orbital energies in single-electron atoms or ions, such as He+, can be described with an equation similar to the Balmer–Rydberg equation:

where Z is the atomic number. What wavelength of light in nanometers is emitted when the electron in He+ falls from n = 3 to n = 2?

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Why do the Earth and Sun have different emission spectra?

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