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13- :Br :ö: :F-P. :O-As-O: Н-Se-H :Br Br: :0: II II IV

13- :Br :ö: :F-P. :O-As-O: Н-Se-H :Br Br: :0: II II IV

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Which statement is false given the following Lewis structures?

 

Structure III is a valid structure for PF4 because P can expand its octet.
Structure I is a valid structure for BBr3 because B (n=2) needs an octet of electrons.
Structure II is a valid structure for SeH2 because H needs a duet of electrons.
Structure IV is a valid structure for AsO43- because As can expand its octet.
 
 
The image consists of Lewis structures for four different chemical species. Each structure shows the arrangement of valence electrons around the central atoms and any associated bonding. I. **Bromine Trifluoride (BrF₃)**: A trigonal planar structure where a boron (B) atom is centrally located and bonded to three bromine (Br) atoms. Each bromine atom is depicted with lone pairs of electrons, represented by dots. II. **Hydrogen Selenide (H₂Se)**: A linear structure with a selenium (Se) atom centrally bonded to two hydrogen (H) atoms. Selenium is shown with two lone pairs of electrons. III. **Phosphorus Pentafluoride (PF₅)**: A trigonal bipyramidal structure with a phosphorus (P) atom centrally bonded to five fluorine (F) atoms. Each fluorine atom is shown with three lone pairs of electrons. IV. **Arsenate Ion (AsO₄³⁻)**: A tetrahedral structure showing an arsenic (As) atom centrally bonded to four oxygen (O) atoms. Three oxygen atoms are singly bonded to arsenic with a charge of -1 for the ion, each having three lone pairs. The fourth oxygen is double bonded with two lone pairs, depicted within brackets indicating the overall -3 charge of the ion. These diagrams provide visual guidance on how electrons are distributed in these molecules and ions, which is crucial for understanding their chemical behavior and bonding characteristics.
Transcribed Image Text:The image consists of Lewis structures for four different chemical species. Each structure shows the arrangement of valence electrons around the central atoms and any associated bonding. I. **Bromine Trifluoride (BrF₃)**: A trigonal planar structure where a boron (B) atom is centrally located and bonded to three bromine (Br) atoms. Each bromine atom is depicted with lone pairs of electrons, represented by dots. II. **Hydrogen Selenide (H₂Se)**: A linear structure with a selenium (Se) atom centrally bonded to two hydrogen (H) atoms. Selenium is shown with two lone pairs of electrons. III. **Phosphorus Pentafluoride (PF₅)**: A trigonal bipyramidal structure with a phosphorus (P) atom centrally bonded to five fluorine (F) atoms. Each fluorine atom is shown with three lone pairs of electrons. IV. **Arsenate Ion (AsO₄³⁻)**: A tetrahedral structure showing an arsenic (As) atom centrally bonded to four oxygen (O) atoms. Three oxygen atoms are singly bonded to arsenic with a charge of -1 for the ion, each having three lone pairs. The fourth oxygen is double bonded with two lone pairs, depicted within brackets indicating the overall -3 charge of the ion. These diagrams provide visual guidance on how electrons are distributed in these molecules and ions, which is crucial for understanding their chemical behavior and bonding characteristics.
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