Chemistry Chapter 6: Chemical Bonds Quiz

Differences Between Ionic and Covalent Bonds

• Ionic bonds involve the transfer of electrons from metal to nonmetal, creating a strong attraction.
• Covalent bonds involve the sharing of electrons, typically formed between nonmetals, with medium strength.
• Ionic compounds utilize Roman numerals for charge, while covalent compounds use prefixes like "di."

Electronegativity

• Electronegativity measures an atom's attraction for shared electrons in a bond.
• Higher electronegativity results in a partial negative charge (δ⁻), while lower electronegativity results in a partial positive charge (δ⁺).

Bond Polarity and Electronegativity

• Bond type (ionic or covalent) can be predicted by calculating the electronegativity difference (∆EN).
• A larger ∆EN indicates a more polar bond, with ionic bonds having the greatest differences.

Formation of Ionic vs. Covalent Compounds

• Ionic compounds form when metals (low electronegativity) bond with nonmetals (high electronegativity), leading to electron transfer.
• Covalent compounds form when two nonmetals (similar electronegativities) bond, leading to electron sharing.

Types of Bonds

• A triple bond consists of three shared pairs of electrons, totaling six electrons, and is stronger than double or single bonds.
• Ionic bonds are also known as electrovalent bonds.
• Covalent bonds are formed between hydrogen and nonmetals or between two nonmetals.

Molecular Bonding

• Molecules are specifically covalent compounds with shared electron pairs.
• Diatomic molecules, such as F₂, exhibit nonpolar covalent bonding.

Ionic and Covalent Bond Definitions

• An ionic bond is the attraction between oppositely charged ions resulting from electron transfer.
• A covalent bond occurs when two atoms share electrons, characterized as intramolecular forces.

Bonding Principles

• Atoms bond to achieve a stable octet of valence electrons and to minimize potential energy.
• The central atom in a chemical formula is often the one with the lowest subscript or the one that can form the most bonds.

Polyatomic Ions

• A polyatomic ion comprises a covalently bonded group of atoms with a net charge.

Characteristics of Bonds

• Nonpolar covalent bonds have even electron sharing with symmetrical distributions.
• Polar covalent bonds feature uneven electron sharing, leading to dipole moments and partial charges.

Properties of Ionic Compounds

• Ionic compounds are typically hard, brittle, have high melting and boiling points, and conduct electricity in solution.

Properties of Covalent Compounds

• Covalent compounds are generally soft, liquid at room temperature, flammable, with low melting and boiling points that do not conduct electricity well.

Examples of Compounds

• Concrete is primarily made of ionic compounds, being solid and brittle.
• Gasoline and candy corn are primarily covalent compounds, existing as liquids and soft solids, respectively.

Bond Formation Determinants

• The number of bonds an atom forms can be determined using Roman numerals for metals or by assessing the electronegativity of nonmetals.

Polar Molecules

• A molecule with polar bonds can be nonpolar if the bonds are symmetrically arranged, causing dipole moments to cancel out.

Solubility of Ionic Compounds in Water

• Water can dissolve many ionic compounds due to its polar nature, which facilitates attraction to positive and negative ions.

Partial Charges

• Partial charges arise from the asymmetric distribution of electrons in polar covalent bonds.

Test your knowledge on the key concepts of chemical bonds, focusing on the differences between ionic and covalent bonds. Additionally, explore the concept of electronegativity and its role in bonding. This quiz is perfect for reinforcing the material covered in Chapter 6.