Question

get it? explain what is the charge of an ionic compound?

compare ionic and covalent bonds in the venn diagram below with at least six facts.

ionic
both
covalent

get it? describe the atoms involved in a nonpolar bond.

evaluate your friend says that nonpolar molecules cannot contain polar bonds. do you agree? support your answer.

Explanation:

First Question: "What is the charge of an ionic compound?"

Ionic compounds are formed from the combination of positively charged ions (cations) and negatively charged ions (anions). The total positive charge from cations equals the total negative charge from anions, so the overall charge of an ionic compound is neutral (zero).

In a nonpolar bond, the atoms involved have the same (or very similar) electronegativities. This means that the electrons in the bond are shared equally between the atoms. Typically, nonpolar bonds form between atoms of the same element (e.g., H - H, O = O) or between atoms with very small electronegativity differences (e.g., C - H in some cases).

Disagree. A nonpolar molecule can contain polar bonds if the polar bonds are arranged symmetrically around the central atom, so that their dipole moments cancel out. For example, in CO₂, the C = O bonds are polar (oxygen is more electronegative than carbon). But the linear geometry of CO₂ (O = C = O) means that the dipole moments of the two C = O bonds are equal in magnitude and opposite in direction, resulting in a net dipole moment of zero for the molecule, making it nonpolar. Another example is CH₄, where the C - H bonds (slightly polar) are arranged in a tetrahedral geometry, and their dipole moments cancel out, resulting in a nonpolar molecule.

Answer:

The charge of an ionic compound is zero (neutral) because the positive charge of cations balances the negative charge of anions.

Second Task: "Compare ionic and covalent bonds in the Venn diagram"

Ionic (Left Circle):

• Formed by transfer of electrons.
• Occur between metal and non - metal.
• Result in ions (cations and anions).
• High melting/boiling points.
• Conduct electricity when dissolved/molten.
• Example: NaCl.

Both (Overlap):

• Involve atoms to achieve stable electron configuration.
• Result in stable compounds.
• Can form crystalline structures (in some cases for ionic; some covalent networks like diamond).

Covalent (Right Circle):

• Formed by sharing of electrons.
• Occur between non - metals (or metalloids and non - metals).
• Result in molecules (or covalent networks).
• Lower melting/boiling points (except network covalent).
• Do not conduct electricity (except in some special cases like graphite).
• Example: H₂O.

Third Question: "Describe the atoms involved in a nonpolar bond"