Ch.8 - Basic Concepts of Chemical Bonding

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 36a,c,d

Chapter 8, Problem 36a,c,d

Using Lewis symbols and Lewis structures, diagram the formation of PF₃ from P and F atoms, showing valence-shell electrons. (a) How many valence electrons does P have initially? (c) How many valence electrons surround the P in the PF₃ molecule? (d) How many valence electrons surround each P in the PF₃ molecule?

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Identify the number of valence electrons for each atom: Phosphorus (P) has 5 valence electrons, and each Fluorine (F) atom has 7 valence electrons.

Draw the Lewis symbol for Phosphorus (P) with 5 dots around it, representing its 5 valence electrons.

Draw the Lewis symbol for each Fluorine (F) atom with 7 dots around it, representing its 7 valence electrons.

Form bonds by pairing unpaired electrons: Phosphorus will share one of its unpaired electrons with an unpaired electron from each of the three Fluorine atoms, forming three P-F single bonds.

Count the total number of valence electrons around the Phosphorus atom in the PF_3 molecule: After forming the bonds, Phosphorus will have 8 electrons in its valence shell, satisfying the octet rule.

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Key Concepts

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

Lewis Symbols

Lewis symbols represent the valence electrons of an atom as dots surrounding the element's symbol. Each dot corresponds to a valence electron, allowing for a visual representation of how atoms bond and share electrons. This concept is crucial for understanding the formation of molecules, as it helps predict how atoms will interact based on their electron configurations.

Lewis Structures

Lewis structures are diagrams that depict the arrangement of atoms and the distribution of valence electrons in a molecule. They illustrate how atoms are bonded together and show lone pairs of electrons. By using Lewis structures, one can visualize the connectivity and electron sharing in molecules like PF3, which is essential for understanding molecular geometry and reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are involved in chemical bonding. The number of valence electrons determines how an atom can bond with others, influencing the molecule's structure and properties. In PF3, phosphorus has five valence electrons, and each fluorine contributes one, leading to a total of eight electrons around phosphorus in the molecule.

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Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons. e. How many bonding pairs of electrons are in the SiCl4 molecule?

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Textbook Question

Which of the following statements about electronegativity is or are true? i. The alkali metals are the family with the largest electronegativity values. ii. The numerical values for electronegativity have no units. iii. Electronegativity is the ability of an atom in a molecule to attract electron density toward itself.

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