CHAPTER 8: BASIC CONCEPTS OF CHEMICAL BONDING

Atoms

Atoms

________ tend to gain, lose, or share electrons until they are surrounded by eight valence electrons.

electrons

The ________ are shared unequally- the bond is polar.

Polarity

________ affects several macroscopic properties in the lab and in life.

electrical charges of equal

Whenever two ________ magnitude but opposite signs are separated by a distance, a dipole is established.

Molecules

________ and ions with more than an octet of electrons around the central atom are often called hypervalent.

nonmetal gains

When a(n) ________ an electron, the process is generally exothermic, as seen from the negative electron affinities of the elements.

Resonance

________ is an important concept in describing the bonding in organic molecules, particularly aromatic organic molecules, a category that includes the hydrocarbon benzene.

Benzene

________ is commonly represented by omitting the hydrogen atoms and showing only the carbon- carbon framework with the vertices unlabeled.

American chemist Linus Pauling

The ________ (1901- 1994) developed the first and most widely used electronegativity scale, which is based on thermochemical data.

Electronegativity

________ is defined as the ability of an atom in a molecule to attract electrons to itself.

Lewis structures

________ can help us understand the bonding in many compounds and are frequently used when discussing the properties of molecules.

low melting

Covalent bonding causes compounds to behave like molecules, with ________ and boiling temperatures and nonelectrolyte behavior in water.

number of valence

For nonmetals, the ________ electrons in a neutral atom is the same as the group number.

chemical bond

A(n) ________ formed by sharing a pair of electrons is a covalent bond.

Polar molecules

________ attract positive and negative ions.

polar covalent bond

In a(n) ________, one of the atoms exerts a greater attraction for the bonding electrons than the other.

Ionic bonding

________ produces brittle, high- melting solids with extended lattice structures that behave strongly as electrolytes in water.

nitrogen atom

Because each ________ has five valence electrons, three electron pairs must be shared to achieve the octet configuration.

two electrons

The dots are placed on the four sides of the symbol- top, bottom, left, and right- and each side can accommodate up to ________.

Nitrogen

________ is a diatomic gas with exceptionally low reactivity that results from the very stable nitrogen- nitrogen bond.

formation of sodium

The ________ chloride from sodium and chlorine is very exothermic.

Lewis structures

There are ________ where you might have to choose between satisfying the octet rule and obtaining the most favorable formal charges by using more than an octet of electrons.

Polar molecules

________ attract each other at their negative and positive ends.

Lewis structure

A(n) ________ in which any negative charges reside on the more electronegative atoms is generally more dominant than one that has negative charges on the less electronegative atoms.

Electron Configurations of Ions of the s

and p-Block Elements