Chemistry Course Overview and Lewis Structures

These flashcards cover essential concepts from the chemistry lecture, focusing on clicker courses, Lewis structures, formal charges, electronegativity, bonding types, and bond line structures.

The key rule to keep in mind when drawing Lewis structures is the __ rule.

octet

Hydrogen follows a __ instead of an octet rule.

duet

Atoms can occasionally have a __ charge, which means they may be cations or anions.

formal

If an atom has a formal charge that is negative, it is called an __.

anion

To calculate the formal charge, use the formula: valence electrons minus lines and dots around the atom, which can be summarized as __.

Valence - Lines - Dots

Electronegativity is the ability of an atom to __ electron density towards itself.

attract

A bond is classified as __ if the electronegativity difference between two atoms is less than 0.5.

nonpolar covalent

If the electronegativity difference is between 0.5 and 1.7, the bond is classified as __.

polar covalent

An ionic bond occurs when the electronegativity difference is greater than __.

1.7

Formal charges greater than __ are considered unstable and generally do not exist for long periods.

one

In bond line structures, each and each represents a carbon atom.

corner; endpoint

In determining the number of implicit hydrogens, complete each carbon to __ bonds.

four

Electronegativity is the ability of an atom to __ electron density towards itself.\n\n

attract\n\n

A bond is classified as __ if the electronegativity difference between two atoms is less than 0.5

nonpolar covalent

If the electronegativity difference is between 0.5 and 1.7, the bond is classified as __.

polar covalent

Formal charges greater than __ are considered unstable and generally do not exist for long periods.

1

In determining the number of implicit hydrogens, complete each carbon to __ bonds.

4 to satisfy the tetravalency of carbon.

The process of mixing atomic orbitals to generate new, equivalent bonding orbitals is called __.

hybridization

The steric number involves the sum of the number of bonded atoms and the number of __.

lone pairs

An atom with a steric number of 4 typically exhibits __ hybridization.\n\n

sp^3

An atom with a steric number of 3 typically exhibits __ hybridization.

sp^2

The bond angle associated with sp^2 hybridization in a trigonal planar geometry is __.

120^{\circ}

The bond angle associated with sp^3 hybridization in a tetrahedral geometry is __.\n\n

109.5^{\circ}

An atom with a steric number of 2 exhibits __ hybridization and a linear geometry.

sp

A double bond is composed of one \sigma bond and one __ bond.

\pi