Question

for each row in the table below, decide whether the pair of elements will form a molecular or ionic compound. if they will, then enter the chemical formula of the compound. if the elements will form more than one compound, enter the compound with the fewest total number of atoms. you may assume all chemical bonds are single bonds, not double or triple bonds.
table with columns: element #1, element #2, compound formed? (ionic, molecular, neither), chemical formula; rows: xenon & krypton, hydrogen & fluorine, oxygen & fluorine

Explanation:

Row 1: Element #1 = Xenon, Element #2 = Krypton

Step1: Determine Bonding Type

Xenon and krypton are both noble gases (Group 18 elements). Noble gases are inert and do not typically form compounds with each other or most other elements under normal conditions. So, they form neither ionic nor molecular compounds.

Step2: Chemical Formula

Since they don't form a compound, there's no chemical formula.

Row 2: Element #1 = Hydrogen, Element #2 = Fluorine

Step1: Determine Bonding Type

Hydrogen (non - metal) and fluorine (non - metal) will form a molecular compound. They share electrons to form covalent bonds.

Step2: Determine Chemical Formula

Hydrogen has a valency of 1, and fluorine has a valency of 1. To form a stable compound, one hydrogen atom combines with one fluorine atom. So the chemical formula is $HF$.

Row 3: Element #1 = Oxygen, Element #2 = Fluorine

Step1: Determine Bonding Type

Oxygen and fluorine are both non - metals. They will form a molecular compound through covalent bonding.

Step2: Determine Chemical Formula

Oxygen has a valency of 2, and fluorine has a valency of 1. To satisfy the valency, two fluorine atoms combine with one oxygen atom. The chemical formula is $OF_2$.

Row 1:

Answer:

compound formed: neither; chemical formula: (no compound)

Row 2: