Choose the larger atom in each pair. a. Al or In b. Si or N c. P or Pb d. C or F

Name: Problem 71, Chapter 3: Chemistry: Structure and Properties
Uploaded: 2019-09-07T03:58:59-08:00
Duration: 2 min 47 s
Channel: Kevin Chimex
Description: Choose the larger atom in each pair. a. Al or In b. Si or N c. P or Pb d. C or F

step 1 So in this question we have to choose the larger atom from the pair. The first pair is halenium

Choose the larger atom in each pair. a. Al or In b. Si or N...

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Key Concepts

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by electrons in an atom, calculated by subtracting the shielding effect of inner electrons from the total nuclear charge. This concept explains why atomic radius decreases across a period and affects other atomic properties such as ionization energy and electronegativity.

Electron Shielding

Electron shielding is the phenomenon where inner electron layers partially block the attractive force of the nucleus on outer electrons. This reduced effective nuclear charge results in a larger atomic radius as electrons are held less tightly, especially in atoms with many electron shells.

Atomic Radius

Atomic radius is a measure of the overall size of an atom, typically defined as the distance from the nucleus to the boundary of the surrounding cloud of electrons. It is a key factor in determining how atoms interact and bond with one another.

Periodic Trends

Periodic trends refer to predictable patterns in the properties of elements across periods and groups in the periodic table. Atomic radius, for instance, generally decreases from left to right across a period due to increasing effective nuclear charge, and increases down a group as additional electron shells are added.

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