(b) How many bonding electrons are in the structure?

Verified step by step guidance

Step 1: Understand the concept of bonding electrons. Bonding electrons are the electrons that are shared between atoms in a molecule, forming covalent bonds.

Step 2: Identify the molecule or compound in question. Without this information, we cannot proceed further.

Step 3: Draw the Lewis structure of the molecule. This will help visualize the arrangement of atoms and the distribution of electrons.

Step 4: Count the number of covalent bonds in the Lewis structure. Each covalent bond consists of two bonding electrons.

Step 5: Multiply the number of covalent bonds by two to find the total number of bonding electrons in the structure.

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Key Concepts

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

Bonding Electrons

Bonding electrons are the electrons that are involved in the formation of chemical bonds between atoms. These electrons are typically found in pairs and are shared between atoms in covalent bonds or transferred in ionic bonds. Understanding the number of bonding electrons is crucial for determining the stability and reactivity of a molecule.

Lewis Structures

Lewis structures are diagrams that represent the arrangement of atoms and the distribution of electrons in a molecule. They illustrate how bonding and lone pairs of electrons are organized, allowing chemists to visualize the connectivity and electron sharing between atoms. Analyzing a Lewis structure helps identify the number of bonding electrons present.

Valence Electrons

Valence electrons are the outermost electrons of an atom that are involved in chemical bonding. The number of valence electrons determines how an atom interacts with others, influencing its ability to form bonds. Knowing the valence electron count is essential for constructing Lewis structures and understanding the bonding characteristics of a molecule.

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Textbook Question

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?

Textbook Question

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?

Textbook Question

Use Lewis symbols and Lewis structures to diagram the formation of PF3 from P and F atoms, showing valence-shell electrons. e. How many bonding pairs of electrons are in the PF3 molecule?

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.

Textbook Question

Place the following pairs of elements in order from smallest to largest difference in electronegativity: K and F, S and O, Br and I, Ca and Se, Li and Cl.