Untitled Flashcards Set

What is the main similarity among ionic, covalent, and metallic bonds?

They all occur to satisfy the octet rule or fulfill the outer shell.

What occurs in ionic bonds?

Metals (cations) give up valence electrons to non-metals (anions) which receive the valence electrons.

What characterizes covalent bonds?

Non-metals (anions) bond with each other by sharing valence electrons.

What is the nature of metallic bonds?

Metals (cations) are attracted to delocalized valence electrons shared in a sea of electrons among surrounding metal atoms.

What are some properties of ionic compounds?

They form crystal lattices, are hard and brittle, conduct electricity when dissolved in water, and have high melting and boiling points.

What are the properties of covalent compounds?

They form non-uniform crystal structures, do not conduct electricity if dissolved, have low melting and boiling points, are soft as solids, and can be flammable.

What characterizes metallic compounds?

They are durable, ductile, malleable, conduct electricity and heat, and have moderate to high melting and boiling points.

What is lattice energy?

The energy required to break an ionic bond.

What is bond dissociation?

The energy required to break a covalent bond.

How many valence electrons are required for a single bond?

2 valence electrons.

What distinguishes a double bond from a single bond?

A double bond requires 4 valence electrons and consists of one sigma bond and one pi bond.

What characterizes a triple bond?

A triple bond requires 6 valence electrons, is short in length, and is the strongest bond, consisting of one sigma and two pi bonds.

What is a polar covalent bond?

An unequal sharing of valence electrons.

What is a non-polar covalent bond?

An equal sharing of valence electrons.

What is the London dispersion force?

The weakest intermolecular force; a temporary attractive force resulting from temporary dipoles in adjacent atoms.

What are dipole-dipole forces?

Attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

What defines a hydrogen bond?

The attractive force between hydrogen attached to an electronegative atom in one molecule and an electronegative atom in a different molecule, usually O, N, or F.