Honors Chemistry: Bonding, Polarity, and Lewis Structures
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Questions and Answers

Considering Coulomb's Law, which of the following ionic compounds would you predict to have the highest lattice energy?

  • NaCl
  • KBr
  • MgO (correct)
  • CsI

A molecule with polar bonds will always exhibit a dipole moment and be considered a polar molecule.

False (B)

Explain how the principles of formal charge can be utilized to determine the most plausible Lewis structure for the thiocyanate ion (SCN-).

To determine the most plausible Lewis structure for SCN-, one would look at the possible arrangements and calculate the formal charges on each atom for each structure. The most plausible structure would be the one that minimizes the formal charges on all atoms, and places any negative formal charge on the most electronegative atom (Nitrogen).

According to the Kinetic Molecular Theory, the average kinetic energy of gas molecules is directly proportional to the gas's ______ temperature.

<p>absolute</p> Signup and view all the answers

Match the following intermolecular forces with the molecular properties that influence their strength:

<p>Hydrogen Bonding = Presence of N-H, O-H, or F-H bonds Dipole Forces = Molecular polarity and dipole moment Dispersion Forces = Molecular size, shape, and surface area</p> Signup and view all the answers

Which of the following scenarios would result in a supersaturated solution?

<p>Cooling a saturated solution carefully without disturbance, causing it to hold more solute than it normally would at the lower temperature. (B)</p> Signup and view all the answers

For a given amount of gas at a constant temperature, if the volume is doubled, what happens to the pressure?

<p>The pressure is halved. (C)</p> Signup and view all the answers

Which of the following statements accurately describes the relationship between intermolecular forces (IMFs) and boiling point?

<p>Weaker IMFs generally lead to lower boiling points because less energy is needed to overcome the attractive forces. (D)</p> Signup and view all the answers

In VSEPR theory, what is the effect of nonbonding (lone pair) electrons on bond angles around a central atom?

<p>Lone pair electrons cause bond angles to decrease due to increased repulsion. (D)</p> Signup and view all the answers

Consider two ionic compounds, NaCl and MgO. According to Coulomb's Law, which factor most significantly contributes to MgO's substantially higher lattice energy compared to NaCl?

<p>The higher charges of Mg2+ and O2- (+2 and -2, respectively) compared to Na+ and Cl- (+1 and -1, respectively). (B)</p> Signup and view all the answers

Explain how the concept of formal charge can be used to determine the most stable resonance structure for the thiocyanate ion (SCN-).

<p>Formal charge helps determine the most stable resonance structure by favoring structures where atoms carry formal charges closest to zero and where negative formal charges are placed on more electronegative atoms.</p> Signup and view all the answers

Match the following intermolecular forces (IMFs) with their primary dependence on molecular properties:

<p>Hydrogen Bonding = Presence of H bonded to N, O, or F Dipole Forces = Presence of polar molecules Dispersion Forces = Molecular size and shape</p> Signup and view all the answers

A gas is collected over water at 22°C. The total pressure of the collected gas is 758 torr. Given that the vapor pressure of water at 22°C is 20 torr, what is the pressure of the dry gas?

<p>738 torr (C)</p> Signup and view all the answers

A supersaturated solution is unstable and contains more solute than it can theoretically hold at a given temperature.

<p>True (A)</p> Signup and view all the answers

Describe how an increase in temperature generally affects the solubility of solid solutes in liquid solvents and explain the underlying principle.

<p>Increasing temperature usually increases the solubility of solid solutes in liquid solvents because it provides more energy to break the solute-solute interactions in the solid, allowing it to dissolve more effectively in the solvent.</p> Signup and view all the answers

Determine the molecular geometry of $XeF_4$ using VSEPR theory.

<p>Square planar (D)</p> Signup and view all the answers

Flashcards

Ionic Bond

Attraction between oppositely charged ions that holds the compound together

Covalent Bond

Sharing of electrons between atoms

Metallic Bond

Attraction between metal atoms where electrons are delocalized

Lattice Energy

Energy required to separate one mole of an ionic compound into gaseous ions

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Dipole Moment

Unequal sharing of electrons in a bond, resulting in partial charges

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Electronegativity

Measure of an atom's ability to attract electrons in a chemical bond

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Lewis Symbol

Diagram showing valence electrons in an atom

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Molarity (M)

M = moles of solute / L of solution

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Intermolecular Forces (IMFs)

Attractive forces between molecules

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Lattice Energy Definition

Energy released when ions combine to form a solid.

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Lattice Energy Trends

As charge increases, lattice energy increases. As size increases, lattice energy decreases.

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Molecular Polarity

A measure of the polarity of a molecule.

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Lewis Structure

Diagram showing valence electrons and bonds in a molecule.

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Octet Rule

Atoms share electrons to achieve a full outer shell (8 electrons).

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Resonance

Multiple valid Lewis structures for one molecule.

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Formal Charge

A way to decide which lewis structure is best

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Ideal Gas Law

P = nRT/V - relates pressure, volume, moles, and temperature.

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VSEPR Theory

Arrangement of atoms in space to minimize electron repulsion.

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Study Notes

Bonding and Polarity

  • Lattice energy influences the melting point of ionic compounds.

Lewis Symbols, Structures, Octet Rule, Resonance, and Formal Charges

  • Includes Lewis symbols for hydrogen (H), beryllium (Be), helium (:He), and neon (:Ne).
  • The thiocyanate ion (SCN-) exhibits resonance, with formal charges of -1, 0, 0 or 0, 0, -1 or +1, 0, -2 on the S, C, and N atoms, respectively.
  • Carbon dioxide (CO₂) can be represented with formal charges of 0, 0, 0 or +1, 0, -1 or -1, 0, +1 on the O, C, and O atoms, respectively.
  • Lewis structures for covalent compounds also include hydrogen fluoride (H-F:), chlorine (:Cl:), formaldehyde (H₂CO), and ethene (H₂C=CH₂).

Gas and Pressure

  • Includes Boyle's Law (P₁V₁ = P₂V₂).
  • Incorporates Charles's Law (V₁/T₁ = V₂/T₂).
  • Lists Avogadro's Law as V₁/n₁ = V₂/n₂.
  • Includes Amonton's Law: P₁/T₁ = P₂/T₂.

VSEPR

  • Linear geometry has a bond angle of 180°.
  • Trigonal planar geometry has a bond angle of 120°.
  • If there are lone pairs on a trigonal planar molecule then it is Bent or Angular.
  • Tetrahedral geometry has a bond angle of 109°.
  • If there are lone pairs on a tetrahedral molecule then it is Trigonal Pyramidal or Angular.
  • Example of a linear molecule is CO₂
  • Example of a trigonal planar molecule is BCl₃ or SO₃
  • Example of a tetrahedral molecule is CH₄ or SO₄²⁻
  • Example of a trigonal bipyramidal molecule is PCl₅
  • Example of an octahedral molecule is SF₆
  • Axial chlorides are at 90° angle in trigonal bipyramidal molecules such as PCl₅
  • Equatorial chlorides are at 120° angle in trigonal bipyramidal molecules such as PCl₅

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Description

Study guide covering chemical bonding types, lattice energy, and polarity. Includes Lewis symbols and structures, the octet rule, resonance, and formal charges. Covers both ionic and covalent compounds with examples.

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