Covalent Bonding and Lewis Structures (chapter 4 flashcards)

These flashcards cover key vocabulary and concepts related to covalent bonding and Lewis structures, crucial for understanding molecular chemistry.

Covalent Bond

A bond formed by the sharing of electrons between two atoms.

Molecule

A discrete group of atoms held together by covalent bonds.

Lone Pairs

Nonbonded electron pairs that are not involved in bonding.

Lewis Structure

An electron-dot structure that shows the location of all valence electrons in a molecule.

Octet Rule

Atoms tend to form bonds by sharing electrons to achieve an electron configuration resembling that of a noble gas with eight electrons in the outer shell.

Valence Electrons

Electrons in the outermost shell of an atom that are involved in forming bonds.

Multiple Bonds

When two atoms share more than one pair of electrons, resulting in double or triple bonds.

Electronegativity

A measure of an atom's ability to attract electrons in a bond.

Nonpolar Bond

A bond formed between two atoms with similar or equal electronegativities, resulting in equal sharing of electrons.

Polar Covalent Bond

A bond formed between two atoms with different electronegativities, resulting in unequal sharing of electrons.

Shapes based on number of groups, atoms, and lone pairs

Linear , Trigonal planar , Tetrahedral, Trigonal pyramid, and Bent

Linear

2 groups, 180 degrees

Trigonal planar

3 groups, 120 degrees

Tetrahedral

4 groups, 109.5 degrees

Trigonal pyramid 

1 lone pair, 107 degrees to 109.5 degrees 

Bent

2 lone pairs, 105 degrees to 109.5 degrees.