Question

question 4 of 10
which of the following examples is a molecule with a covalent bond? (use
the electronegativity values from the periodic table link to help you answer
this question.)

a. co

b. beo

c. rbbr

d. kcl

Explanation:

To determine a covalent bond, we check the electronegativity difference (ΔEN) between atoms. Covalent bonds typically form between non - metals (ΔEN < 1.7, often < 2.0 for polar covalent; pure covalent when ΔEN = 0).

• For option A (CO): Carbon (C) and Oxygen (O) are both non - metals. The electronegativity of C is ~2.5 and O is ~3.5, so ΔEN = 3.5 - 2.5 = 1.0, which is within the range for covalent (polar covalent) bonding.
• For option B (BeO): Beryllium (Be) is a metal and Oxygen (O) is a non - metal. This is an ionic bond (metal - non - metal combination).
• For option C (RbBr): Rubidium (Rb) is a metal and Bromine (Br) is a non - metal, forming an ionic bond.
• For option D (KCl): Potassium (K) is a metal and Chlorine (Cl) is a non - metal, forming an ionic bond.

So, only CO has a covalent bond.

Answer:

A. CO