Quiz 1 cards

Lewis Dot Structure

Represents valence electrons of an atom using dots.

Valence Electrons

Electrons in the outermost shell or highest energy level of an atom.

Octet Rule

Atoms prefer to have eight electrons in their valence shell for stability.

Noble Gases

Elements with high ionization energy that are non-reactive due to a complete valence shell.

Duet Rule

H and He are stable with only two valence electrons.

Chemical Bonding

The process by which atoms combine to form compounds through interactions of valence electrons.

Ionic Bonding

Occurs when electrons are transferred between atoms, forming charged ions.

Cation

A positively charged ion formed when a metal atom loses electrons.

Anion

A negatively charged ion formed when a nonmetal atom gains electrons.

Sodium Chloride (NaCl)

An example of an ionic compound formed from sodium and chlorine.

Crystalline Structure

Regular arrangement of ions in ionic compounds for stability.

Electrical Conductivity

Ionic compounds conduct electricity when molten or in solution due to mobile ions.

Covalent Bonding

Occurs when two nonmetal atoms share pairs of electrons to achieve stable configurations.

Electronegativity

The tendency of an atom to attract shared electrons in a chemical bond.

Nonpolar Covalent Bonds

Bonds formed between atoms with similar electronegativities where electrons are shared equally.

Polar Covalent Bonds

Bonds formed between atoms with moderate electronegativity differences where electrons are shared unequally.

Shared Pair

A pair of electrons shared between two atoms, represented by a single line in Lewis structures.

Lewis Structures

Diagrams that represent the arrangement of electrons in covalent compounds.