Questions and Answers
A chemical bond between atoms results from the attraction between the valence electrons and _______ of different atoms.
nuclei
What does a covalent bond consist of?
a shared electron pair
If two covalently bonded atoms are identical, how is the bond identified?
nonpolar covalent
What is a covalent bond in which there is an unequal attraction for the shared electrons?
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Atoms with a strong attraction for the electrons they share with another atom exhibit what characteristic?
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What type of bonds possess between 5% and 50% ionic character?
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What happens to the percentage of ionic character as the electronegativity difference between two atoms increases?
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What are the electrons involved in the formation of a chemical bond called?
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What is a chemical bond that results from the electrostatic attraction between positive and negative ions called?
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If electrons involved in bonding spend most of the time closer to one atom rather than the other, what type of bond is it?
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If a bond has more than 50% ionic character, what is it called?
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A bond characterized by more than 50% ionic character occurs when the electronegativity difference between the two atoms is greater than _______.
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Give an example of a nonpolar covalent compound.
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Provide an example of a polar covalent compound.
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What is an example of an ionic compound?
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Describe how a covalent bond holds two atoms together.
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What property of the two atoms in a covalent bond determines whether the bond will be polar?
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How can electronegativity be used to distinguish between an ionic bond and a covalent bond?
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Describe the electron distribution in a polar covalent bond and its effects on the partial charges of the compound.
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Use the concept of potential energy to describe how a covalent bond forms between two atoms.
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Name two elements that form compounds that can be exceptions to the octet rule.
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Explain why resonance structures are used instead of Lewis structures to correctly model certain molecules.
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Identify the major assumption of the VSEPR theory, which is used to predict the shape of atoms.
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In water, two hydrogen atoms are bonded to one oxygen atom. Why isn't water a linear molecule?
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What orbitals combine together to form sp3 hybrid orbitals around a carbon atom?
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What two factors determine whether or not a molecule is polar?
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How are dipole-dipole attractions, London dispersion forces, and hydrogen bonding similar?
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Is H-F nonpolar covalent, polar covalent, or ionic?
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Is Na-Cl nonpolar covalent, polar covalent, or ionic?
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Is H-O nonpolar covalent, polar covalent, or ionic?
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Is H-H nonpolar covalent, polar covalent, or ionic?
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Is H-C nonpolar covalent, polar covalent, or ionic?
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Is H-N nonpolar covalent, polar covalent, or ionic?
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How is a hydrogen bond different from an ionic or covalent bond?
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H2S and H2O have similar structures, and their central atoms belong to the same group. Yet H2S is a gas at room temperature, and H2O is a liquid. Use bonding principles to explain why this is.
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In what way is a polar covalent bond similar to an ionic bond?
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Is H2S polar or nonpolar?
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Is COCl2 polar or nonpolar?
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Is PCl3 polar or nonpolar?
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Is CH2O polar or nonpolar?
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Study Notes
Chemical Bonding Overview
- Chemical bonds form due to attraction between valence electrons and nuclei of different atoms.
- Valence electrons are crucial in bond formation.
Types of Chemical Bonds
- Covalent Bond: Formed by a shared electron pair between atoms.
- Nonpolar Covalent Bond: Occurs between identical atoms with equal sharing of electrons.
- Polar Covalent Bond: Unequal attraction for shared electrons leads to partial charges.
- Ionic Bond: Formed through electrostatic attraction between positive and negative ions.
Electronegativity
- High electronegativity indicates strong attraction for electrons in a bond.
- Differences in electronegativity determine bond type:
- Less than 1.7 indicates covalent bond.
- Greater than 1.7 indicates ionic bond.
Characteristics of Bonds
- Bonds with 5% to 50% ionic character are polar covalent.
- Greater electronegativity difference correlates with increased ionic character.
Examples of Bonds
- Nonpolar Covalent Compound Example: H2
- Polar Covalent Compound Example: HCl
- Ionic Compound Example: NaCl
Bonding Mechanics
- Covalent bonds hold two atoms through shared electron attraction towards both nuclei.
- Electron distribution in polar covalent bonds results in partial positive and negative charges on the molecule.
Resonance and Structure
- Resonance structures illustrate delocalized electrons, unlike fixed positions in Lewis structures.
- VSEPR theory states that pairs of valence electrons repel, affecting molecule shape.
Molecular Geometry & Polarity
- Water's non-linear shape results from non-bonding electron pairs creating a tetrahedral arrangement.
- Factors determining molecular polarity include electronegativity difference and molecular geometry.
Intermolecular Forces
- Dipole-dipole attractions, London dispersion forces, and hydrogen bonding all represent intermolecular attractions based on charge differences within molecules.
- Hydrogen bonds are distinct from ionic and covalent bonds as they are weaker and involve interactions between polar molecules.
State of Matter Comparisons
- H2S is a gas due to weaker intermolecular forces, while H2O is a liquid due to stronger hydrogen bonding from higher electronegativity of oxygen.
Summary of Polar and Nonpolar Bonds
- Polar covalent bonds have unequal sharing of electrons, leading to partial charges.
- Nonpolar covalent bonds feature equal sharing, resulting in no charges.
- Various compounds (like H2S, COCl2, PCl3, CH2O) exhibit different polarities based on their molecular structure and electronegativity differences.
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Description
Test your knowledge of chemical bonding with this review quiz. Explore key concepts like covalent bonds, nonpolar covalent bonds, and the role of valence electrons. Perfect for reinforcing your understanding of Chapter 6 in chemistry.