Name the proper three-dimensional molecular shapes for each of the following molecules or ions, showing lone pairs as needed: (a) ClO2- (b) SO4 2- (c) NF3 (d) CCl2Br2 (e) SF4 2+

Verified step by step guidance

Step 1: Determine the total number of valence electrons for each molecule or ion. For example, for ClO2-, count the valence electrons from Cl and O, and add one more for the negative charge.

Step 2: Draw the Lewis structure for each molecule or ion. Arrange the atoms to satisfy the octet rule, and place any extra electrons as lone pairs on the central atom.

Step 3: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to determine the electron pair geometry around the central atom. Consider both bonding pairs and lone pairs of electrons.

Step 4: Identify the molecular geometry by considering only the positions of the atoms (ignoring lone pairs). For example, if there are four electron pairs and one is a lone pair, the molecular shape is trigonal pyramidal.

Step 5: Name the molecular shape for each molecule or ion based on the arrangement of atoms. For example, a molecule with four bonding pairs and no lone pairs is tetrahedral.

Key Concepts

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

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) Theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to VSEPR, electron pairs, including lone pairs, will arrange themselves to minimize repulsion, leading to specific molecular shapes such as linear, trigonal planar, tetrahedral, and octahedral.

Lone Pairs and Bonding Pairs

In molecular geometry, lone pairs are pairs of valence electrons that are not involved in bonding, while bonding pairs are shared between atoms. Lone pairs occupy more space than bonding pairs, affecting the overall shape of the molecule. Understanding the distinction between these pairs is crucial for accurately predicting molecular geometry using VSEPR Theory.

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding and lone pairs in a molecule. This process helps explain the geometry of molecules by determining the types of bonds formed and the angles between them. For example, sp3 hybridization leads to tetrahedral shapes, while sp2 results in trigonal planar arrangements.

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Hybridization

Related Practice

Textbook Question

Consider the following XF₄ ions: PF₄^-, BrF₄^-, ClF₄⁺, and AlF₄^-. (a) Which of the ions have more than an octet of electrons around the central atom?

Textbook Question

Consider the following XF4 ions: PF4-, BrF4-, ClF4+, and AlF4-. (c) Which of the ions will have an octahedral electron-domain geometry?

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Textbook Question

Which of the following statements are true?

i. The overall dipole moment of a molecule is the vector sum of its individual bond dipoles.

ii. If atoms A and B in an AB𝑛 molecule have different electronegativities, then the AB𝑛 molecule must have a nonzero dipole moment.

iii. The bond dipoles in a tetrahedral AB4 molecule cancel one another.

Textbook Question

a. Does SCl2 have a nonzero dipole moment?