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Questions and Answers
What property allows ionic compounds to conduct electricity in certain states?
What property allows ionic compounds to conduct electricity in certain states?
Which characteristic is true regarding covalent compounds?
Which characteristic is true regarding covalent compounds?
In a polar covalent bond, what effect does the higher electronegativity of one atom have?
In a polar covalent bond, what effect does the higher electronegativity of one atom have?
Which of the following compounds is an example of a nonpolar covalent bond?
Which of the following compounds is an example of a nonpolar covalent bond?
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What factor primarily determines the solubility of ionic compounds in water?
What factor primarily determines the solubility of ionic compounds in water?
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What type of bond involves the transfer of electrons?
What type of bond involves the transfer of electrons?
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Which statement describes the typical structure of ionic compounds?
Which statement describes the typical structure of ionic compounds?
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Which of the following compounds is an example of a covalent compound?
Which of the following compounds is an example of a covalent compound?
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How do ionic compounds behave when they are dissolved in water?
How do ionic compounds behave when they are dissolved in water?
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What is the primary reason ionic compounds have high melting and boiling points?
What is the primary reason ionic compounds have high melting and boiling points?
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What characteristic is generally true of covalent compounds compared to ionic compounds?
What characteristic is generally true of covalent compounds compared to ionic compounds?
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Which of the following is a characteristic of ionic bonds?
Which of the following is a characteristic of ionic bonds?
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What is a common misconception about ionic compounds?
What is a common misconception about ionic compounds?
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Flashcards
Ionic Bond Formation
Ionic Bond Formation
Metals lose electrons, forming positive ions (cations), while nonmetals gain electrons, forming negative ions (anions). The attraction between these oppositely charged ions creates the bond.
Covalent Bond Formation
Covalent Bond Formation
Nonmetals share electrons to achieve a stable electron configuration (often the octet rule).
Ionic Compound Properties
Ionic Compound Properties
High melting/boiling points, typically solid at room temp, conduct electricity when dissolved or molten. Form crystals with repeating patterns of ions.
Covalent Compound Properties
Covalent Compound Properties
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Ionic vs. Covalent: Formation
Ionic vs. Covalent: Formation
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Ionic vs. Covalent: Participants
Ionic vs. Covalent: Participants
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Ionic Compounds and Hardness
Ionic Compounds and Hardness
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Covalent vs Ionic MP/BP
Covalent vs Ionic MP/BP
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High Melting/Boiling Points of Ionic Compounds
High Melting/Boiling Points of Ionic Compounds
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Solubility of Ionic Compounds
Solubility of Ionic Compounds
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Conductivity of Ionic Compounds
Conductivity of Ionic Compounds
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Low Melting/Boiling Points of Covalent Compounds
Low Melting/Boiling Points of Covalent Compounds
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Non-Conductivity of Covalent Compounds
Non-Conductivity of Covalent Compounds
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Study Notes
Ionic Bonds
- Ionic bonds form between metals and nonmetals.
- Metals lose electrons to become positively charged ions (cations).
- Nonmetals gain electrons to become negatively charged ions (anions).
- The electrostatic attraction between these oppositely charged ions forms the ionic bond.
- Ionic compounds typically have high melting and boiling points due to the strong electrostatic forces between ions.
- Ionic compounds are usually solid at room temperature.
- Ionic compounds are often crystalline solids with a regular, repeating arrangement of ions.
- Ionic compounds conduct electricity when molten or dissolved in water because the ions are free to move.
- Examples of ionic compounds include sodium chloride (NaCl) and magnesium oxide (MgO).
Covalent Bonds
- Covalent bonds form between nonmetals.
- Nonmetals share electrons to achieve a stable electron configuration, often the octet rule.
- Shared electrons are attracted to the nuclei of both atoms, creating a bond.
- Covalent bonds can be single, double, or triple bonds depending on the number of electron pairs shared.
- Covalent compounds generally have lower melting and boiling points compared to ionic compounds.
- Covalent compounds can exist as gases, liquids, or solids at room temperature.
- Covalent bonds can form between the same atom (e.g., O2) or different atoms (e.g., H2O).
- Their properties depend significantly on the types and number of atoms involved.
- Examples of covalent compounds include water (H2O) and carbon dioxide (CO2).
Differences between Ionic and Covalent Bonds
- Formation: Ionic bonds involve the transfer of electrons, whereas covalent bonds involve the sharing of electrons.
- Participants: Ionic bonds typically involve a metal and a nonmetal. Covalent bonds typically involve two nonmetals.
- Melting and Boiling Points: Ionic bonds generally have higher melting and boiling points. Covalent bonds typically have much lower melting and boiling points.
- Conduction: Ionic compounds conduct electricity in the molten or aqueous state, while covalent compounds generally do not.
- Structure: Ionic compounds form crystalline structures. Covalent compounds can form various structures, including molecules.
Properties of Ionic and Covalent Compounds
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Ionic Compounds:
- Hard and Brittle: The strong forces between ions make them hard. If stressed, ions of like charge can line up, leading to repulsion and breakage.
- High Melting and Boiling Points: Significant energy is required to overcome the strong electrostatic forces.
- Solubility: Many ionic compounds are soluble in water, where the polar water molecules surround and separate the ions.
- Conductivity: Conduct electricity in molten or aqueous solutions because ions are free to move.
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Covalent Compounds:
- Varying Hardness: Can range from soft (like wax) to hard (like diamond).
- Low to Med Melting and Boiling Points: Less energy is needed to overcome the intermolecular forces between molecules.
- Varying Solubility: Some are soluble in water (e.g., sugar and ethanol), while others are not.
- Non-Conductivity: Typically do not conduct electricity because electrons are not mobile.
Polar and Nonpolar Covalent Bonds
- Polar Covalent Bonds: Occur when atoms of different electronegativity share electrons. The more electronegative atom attracts the shared electrons more strongly, creating a partial negative charge (δ-) and a partial positive charge (δ+).
- Nonpolar Covalent Bonds: Form when atoms of similar electronegativity share electrons equally. There is no significant difference in charge distribution.
- Example of Polar Bond: The bond in water (H₂O). Oxygen is more electronegative than hydrogen, leading to a polar bond.
- Example of Nonpolar Bond: The bond in methane (CH₄). Carbon and hydrogen have similar electronegativities, resulting in a nonpolar bond.
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Description
Test your knowledge on ionic and covalent bonds with this quiz. Learn how these bonds form between metals and nonmetals, the properties of ionic compounds, and the sharing of electrons in covalent bonds. Perfect for students in chemistry classes!