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Chapter 10: Problem 131

In your own words, define the following terms: (a) valence electrons; (b) electronegativity; (c) bonddissociation energy; (d) double covalent bond;(e) coordinate covalent bond.

Short Answer

Expert verified
Valence electrons are those in an atom's outermost shell involved in bonding. Electronegativity reflects an atom's tendency to attract shared electrons. Bond dissociation energy is the energy needed to break a bond in a molecule, indicating bond strength. A double covalent bond involves sharing two electron pairs, and a coordinate covalent bond consists of shared electrons from only one atom.

Step by step solution

01

Defining Valence Electrons

Valence electrons are the electrons that reside in the outermost shell of an atom and are involved in bonding with other atoms. They determine the chemical properties of an atom.
02

Defining Electronegativity

Electronegativity refers to a measure of the tendency of an atom to attract a shared pair of electrons (or electron density). More electronegative atoms attract electrons more than less electronegative atoms.
03

Defining Bond Dissociation Energy

Bond dissociation energy is the energy required to break one mole of a bond in a diatomic molecule in the gaseous state into two free atoms. It is a measure of the strength of a chemical bond. The higher the bond dissociation energy, the stronger the bond.
04

Defining Double Covalent Bond

A double covalent bond refers to a type of bond where two pairs of electrons are shared between atoms. An example is the bond between two oxygen atoms in the oxygen molecule.
05

Defining Coordinate Covalent Bond

A coordinate covalent bond (also known as a dative bond) is a kind of covalent bond in which the two shared bonding electrons are supplied by one of the bonding atoms only.

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Most popular questions from this chapter

Predict the shapes of the following sulfur-containing species. (a) \(\mathrm{SO}_{2} ;\) (b) \(\mathrm{SO}_{3}^{2-} ;\) (c) \(\mathrm{SO}_{4}^{2-}\).

Of the following species, the one with a triple covalent bond is (a) \(\mathrm{NO}_{3}^{-} ;\) (b) \(\mathrm{CN}^{-} ;\) (c) \(\mathrm{CO}_{2} ;\) (d) \(\mathrm{AlCl}_{3}\).

Briefly describe each of the following ideas: (a) formal charge; (b) resonance; (c) expanded valence shell; (d) bond energy.

A \(1.24 \mathrm{g}\) sample of a hydrocarbon, when completely burned in an excess of \(\mathrm{O}_{2}(\mathrm{g}),\) yields \(4.04 \mathrm{g} \mathrm{CO}_{2}\) and \(1.24 \mathrm{g} \mathrm{H}_{2} \mathrm{O} .\) Draw a plausible structural formula for the hydrocarbon molecule. [Hint: There is more than one possible arrangement of the C and H atoms.]

Under appropriate conditions, both hydrogen and nitrogen can form monatomic anions. What are the Lewis symbols for these ions? What are the Lewis structures of the compounds (a) lithium hydride; (b) calcium hydride; (c) magnesium nitride?
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