Chemistry Chapter 6: Chemical Bonds Quiz

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Questions and Answers

List 3 differences between ionic bonds and covalent bonds.

C: share electrons, prefixes (di), Hydrogen w/ nonmetal or 2 nonmetals (medium force of attraction). I: transfers electrons, Roman Numerals (II), metal (other than Hydrogen) & nonmetal (strong force of attraction).

Define electronegativity.

Attraction an atom has for a shared pair of electrons.

What does electronegativity have to do with bond polarity?

The type of bond can usually be calculated by finding the difference in electronegativity (∆EN) of the two atoms that are bonding.

Explain why ionic compounds are formed when a metal bonds with a nonmetal.

Electrons are transferred from the metal to the nonmetal because metals have low electronegativities and nonmetals have high electronegativities. Signup and view all the answers

A triple bond is where _ pairs of electrons (a total of _ electrons) is shared between two different atoms. It is usually ____ in strength than a double or single bond.

3, 6, greater Signup and view all the answers

What other name is sometimes given to ionic bonds?

Electrovalent bond. Signup and view all the answers

What type of bond will usually be formed between hydrogen and nonmetals or between two nonmetals?

Covalent bonds. Signup and view all the answers

What type of bond will usually be formed between a metal (other than hydrogen) and a nonmetal?

Ionic bonds. Signup and view all the answers

What type of bonding will always be present between two nonmetals?

Covalent. Signup and view all the answers

A molecule refers SPECIFICALLY to substances that have ____ type of bond.

Covalent Signup and view all the answers

The type of bond that holds together a diatomic molecule of fluorine is called ____.

Nonpolar Covalent Signup and view all the answers

Define ionic bond.

A force of attraction that results when electrons are transferred from one atom to another. Signup and view all the answers

Define covalent bond.

Force of attraction between atoms that results when electrons are shared. Signup and view all the answers

What is the reason atoms bond with each other?

To form an octet and decrease potential energy. Signup and view all the answers

List 2 rules used to determine which atom will be the central atom of the dot diagram of a chemical formula.

<ol> <li>The atom with the lowest subscript. 2. The atom that forms the most bonds.</li> </ol> Signup and view all the answers

Define polyatomic.

A covalently bonded group of atoms with a charge. Signup and view all the answers

What is a nonpolar covalent bond?

Even sharing of electrons, symmetrical electron density, and identical atoms. Signup and view all the answers

What is a polar covalent bond?

Uneven sharing of electrons, asymmetrical electron density, partial charges. Signup and view all the answers

What are the properties of ionic compounds?

Hard, brittle, high melting and boiling points, conduct electricity only when dissolved in water. Signup and view all the answers

What are the properties of covalent compounds?

Soft, liquid, flammable, low melting and boiling points, don't conduct electricity. Signup and view all the answers

Is Concrete made primarily of ionic compounds?

True Signup and view all the answers

Is Gasoline made primarily of ionic compounds?

False Signup and view all the answers

Is Candy Corn made primarily of ionic compounds?

False Signup and view all the answers

How can you determine the number of bonds an atom will form?

Use Roman numeral for metals; for nonmetals, use δ-. Signup and view all the answers

Explain how a molecule with polar bonds can be nonpolar.

If the polar bonds are symmetrically arranged around the central atom, the molecule will be nonpolar. Signup and view all the answers

Why can water dissolve many ionic compounds?

The δ+ ends of H2O are attracted to the negative ion, while the δ- end is attracted to the positive ion. Signup and view all the answers

What are partial charges?

Partial charges are created due to the asymmetric distribution of electrons in chemical bonds. Signup and view all the answers

Where are the s & p electrons located on an atom with a Lewis dot diagram?

On the right of an atom is the S section, and on the left is the P section. Signup and view all the answers

Study Notes

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.

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Description

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.