Chemical Bonding and Molecular Structure

Ionic bonds are generally considered stronger than covalent bonds due to the strong electrostatic attraction between the full charges of the ions.

Oxygen and bromine are both non-metals. When two non-metals bond, they typically form a covalent bond by sharing electrons.

Lithium is a metal and Chlorine is a non-metal. The transfer of electrons between a metal and a non-metal results in an ionic bond.

Covalent bonds occur when two non-metals share electrons to achieve a stable electron configuration.

Ionic bonds are characterized by the electrostatic attraction between oppositely charged ions, typically formed by the transfer of electrons from a metal to a non-metal.

Sulfur is in Group 16 and needs 2 more electrons to complete its octet, resulting in a -2 charge when it forms an ion.

Strontium is an alkaline earth metal in Group 2, so it loses 2 valence electrons to form a +2 ion.

Salts are ionic compounds, not covalent. Furthermore, the definition provided incorrectly swaps the roles of cations and anions.

NaOH, LiOH, and Ca(OH)2 are strong bases that dissociate completely in water. Ammonia (NH3) is a weak base because it only partially reacts with water to form hydroxide ions.

Strong bases, such as sodium hydroxide (NaOH) or potassium hydroxide (KOH), are ionic compounds that dissociate completely to release hydroxide ions in water.

Water molecules can self-ionize into hydronium ions (H3O+) and hydroxide ions (OH-).

Ionization is the process by which atoms or molecules acquire a negative or positive charge by gaining or losing electrons, often when dissolving in water.

C2H5OH is ethanol, which is an alcohol. It does not release hydroxide ions in aqueous solution and is not a base, whereas NaOH, KOH, and NH4OH are all bases.

Carbon has four valence electrons, meaning it can form up to four covalent bonds to achieve a stable octet of electrons.

NH3 is the chemical formula for ammonia, a common household chemical compound.