Chemical Bonds and Ionic Compounds Quiz

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Questions and Answers

Which type of bond involves the sharing of electrons between non-metals?

Metallic bond

Ionic bond

Covalent bond (correct)

Polar bond

What indicates a covalent compound when naming?

They end with 'ate'

The ending changes to 'ide' (correct)

They use Roman numerals

Prefixes indicate the number of molecules (correct)

Which of the following is NOT a diatomic element?

Oxygen

Carbon (correct)

Hydrogen

Chlorine

What is a characteristic of ionic bonds?

They can conduct electricity in solution. Signup and view all the answers

What kind of intermolecular forces do giant covalent compounds have?

Strong intermolecular forces Signup and view all the answers

How do metallic structures differ from covalent compounds in terms of electron behavior?

Electrons can roam freely and are delocalized. Signup and view all the answers

What describes a polar covalent bond?

Electrons are shared unevenly. Signup and view all the answers

Which statement about electrolytes is true?

Ionic compounds dissociate in water to conduct electricity. Signup and view all the answers

What type of bond is formed through the sharing of electrons between atoms?

Covalent bond Signup and view all the answers

What is the charge of a calcium ion when it forms an ionic bond?

2+ Signup and view all the answers

Which of the following statements accurately describes ionic compounds?

They have high melting points and are brittle. Signup and view all the answers

How do ionic compounds achieve electrical neutrality?

By balancing the total positive and negative charges. Signup and view all the answers

Which of the following compounds is an example of an ionic binary compound?

Sodium Chloride Signup and view all the answers

What is the formula for Calcium Fluoride?

CaF2 Signup and view all the answers

Which of the following is a polyatomic ion?

Hydroxide Signup and view all the answers

Which statement correctly describes the alignment of charges in ionic bonds?

Opposite charges attract each other. Signup and view all the answers

What characterizes a polar covalent bond compared to a pure covalent bond?

Electronegativity difference is greater than 0.4 but less than 1.8 Signup and view all the answers

Which bond is likely to form between a metal and a non-metal?

Ionic bond Signup and view all the answers

What is a characteristic property of ionic compounds?

Good electrical conductors when dissolved in water Signup and view all the answers

What happens to valence electrons in an ionic bond?

One atom donates electrons to another Signup and view all the answers

Which of the following statements about non-polar covalent bonds is true?

They form between atoms of the same element or similar electronegativity Signup and view all the answers

Why do ionic compounds have high melting and boiling points?

Because of the electrostatic forces between oppositely charged ions Signup and view all the answers

Which type of bond is characterized by an electronegativity difference of less than 0.4?

Non-polar covalent bond Signup and view all the answers

What term is used to describe the Greek letter that indicates partial positive and negative charges in a molecule?

Delta (δ) Signup and view all the answers

Study Notes

Chemical Bonds

Elements are typically found in compounds, not by themselves
A compound is a substance composed of different elements (a mixture)
Bonds are a persistent attraction between two or more atoms
Ionic bonds: Electrostatic forces between oppositely charged ions (crystalline)
Covalent bonds: Sharing of electrons
Like charges repel, opposite charges attract

Ionic Bonds

Ions are charged (+ or -)
Ions attract each other (Coulomb's Law)
Atoms gain or lose electrons to achieve a full valence shell
Stable ionic structures form when charges balance
Ionic crystals: Regular arrangements of atoms held together by attraction between ion pairs
Properties: hard, brittle, crystalline, high melting point
Exist as crystals
Simple ions: Single atoms that have become charged
Naming ionic compounds: Write the metal first, then the non-metal, and change the non-metal ending to "ide" (e.g., sodium chloride).

Ratios

Compounds must be electrically neutral overall
Balancing ratios neutralize the compound
Example: Calcium fluoride (CaF₂) needs two fluoride ions to balance the positive charge of one calcium ion.
Ionic compounds are stable only when neutral (zero-sum rule).

Polyatomic Ions

Polyatomic ions are ions comprised of multiple atoms acting as a single ion
Atoms are covalently bonded within the ion
Naming compounds with polyatomic ions: Polyatomic ions are written as a group behind the positive ion

Multivalent Ions

Some ions have varying charges (multivalent). Their charges are indicated with Roman numerals using parentheses (e.g, iron (II), iron (III)).
Multivalent atoms are often transition metals.
Use roman numerals in parenthesis when naming.

Covalent Bonds

Covalent bonds are formed by nonmetals
Covalent compounds form molecules
Molecules make up larger structures
Sharing electrons enables atoms to achieve a full outer shell
Lewis dot diagrams: Show the arrangement of valence electrons
Naming covalent compounds: Written left to right based on position on the periodic table. Prefixes indicate the number of atoms of each type in the molecule.

Diatomic Elements

Some elements exist in nature as single bonded pairs (diatomic elements)

Video: Chemical Bonds

Metals usually have 1-3 valence electrons; nonmetals usually have 4-8 valence electrons
Ionic bonds have high melting points because a lot of energy is needed to break them apart
Covalent bonds also require energy to break apart
Covalent compounds come in three forms:
- Simple covalent: weak intermolecular forces, low boiling points.
- Giant covalent: Strong intermolecular forces, high boiling points
- Polymers: Complex long chains connecting similar units.

Other Information

Electrolytes: Compounds that conduct electricity
Ionic compounds separate into ions in water, a process called dissociation
Covalent compounds do not conduct electricity because they aren't charged
Molecular shape: 3D arrangement of atoms to show molecules

Polarity and Electronegativity

Polarity: How unevenly electrons are distributed in a covalent bond
Polar covalent bond: Uneven electron sharing
Non-polar covalent bond: Even electron sharing
Electronegativity: Atoms' ability to attract electrons in a bond
A high electronegativity difference between atoms indicates a polar bond; a low electronegativity difference between atoms indicates a non-polar bond.

Difference in Ionic and Covalent Compounds

Ionic bonds form crystalline solids; high melting and boiling points, hard, soluble in water. Conducts electricity when dissolved or is a liquid; no odor, definite shape, not crushable, strong interparticle attractions.
Covalent bonds form gases, solids, and liquids; low melting and boiling points; soft, some soluble in water, some not; poor electrical conductors, often odor-bearing + definite shape, crushable, weak interparticle attractions

Covalent: Polar vs Non-polar

Polar covalent bonds: The electronegativity difference is greater than 0.4- 0.5, electrons are unequally shared
Non-polar covalent bonds: The electronegativity difference is smaller than 0.4 -0.5, Electrons are shared equally.

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Description

Test your knowledge on chemical bonds, especially ionic bonds and their properties. This quiz covers the basics of compounds, how ions interact, and the rules for naming ionic compounds. See how well you understand the fundamental concepts of chemistry.