Podcast
Questions and Answers
Which molecular geometry is characterized by four bonding pairs of electrons around the central atom?
Which molecular geometry is characterized by four bonding pairs of electrons around the central atom?
- Trigonal Pyramidal
- Trigonal Planar
- Tetrahedral (correct)
- Bent
A molecule has a central atom with two bonded atoms and two lone pairs. What is its molecular shape?
A molecule has a central atom with two bonded atoms and two lone pairs. What is its molecular shape?
- Tetrahedral
- Trigonal Planar
- Linear
- Bent (correct)
Which of the following best describes the bond polarity in a molecule of $CO_2$?
Which of the following best describes the bond polarity in a molecule of $CO_2$?
- Polar bonds resulting in a polar molecule
- Non-polar bonds
- Polar bonds resulting in a non-polar molecule (correct)
- Ionic bonds
Which intermolecular force is primarily responsible for the relatively high boiling point of water?
Which intermolecular force is primarily responsible for the relatively high boiling point of water?
Which of the following compounds would likely dissolve in a non-polar solvent such as hexane ($C_6H_{14}$)?
Which of the following compounds would likely dissolve in a non-polar solvent such as hexane ($C_6H_{14}$)?
According to the Brønsted-Lowry definition, what characterizes a base?
According to the Brønsted-Lowry definition, what characterizes a base?
If a solution has a $pH$ of 3, what is the concentration of $H^+$ ions in the solution?
If a solution has a $pH$ of 3, what is the concentration of $H^+$ ions in the solution?
During a titration, what is the purpose of an indicator?
During a titration, what is the purpose of an indicator?
Which of the following molecules is nonpolar despite having polar bonds?
Which of the following molecules is nonpolar despite having polar bonds?
Which type of intermolecular force is present in all molecules, regardless of polarity?
Which type of intermolecular force is present in all molecules, regardless of polarity?
Which of the following aqueous solutions is considered acidic?
Which of the following aqueous solutions is considered acidic?
What is the $pOH$ of a solution with a $pH$ of 4.5 at 25°C?
What is the $pOH$ of a solution with a $pH$ of 4.5 at 25°C?
Which of these molecules can form hydrogen bonds with other identical molecules?
Which of these molecules can form hydrogen bonds with other identical molecules?
What is the molecular geometry of a molecule with a central atom, three bonding pairs, and one lone pair of electrons?
What is the molecular geometry of a molecule with a central atom, three bonding pairs, and one lone pair of electrons?
Which of the following statements accurately describes the relationship between intermolecular forces (IMFs) and boiling point?
Which of the following statements accurately describes the relationship between intermolecular forces (IMFs) and boiling point?
Which of the following is an Arrhenius base?
Which of the following is an Arrhenius base?
Consider a reaction between a strong acid and a strong base. Which of the following is true at the equivalence point of the titration?
Consider a reaction between a strong acid and a strong base. Which of the following is true at the equivalence point of the titration?
Which molecule is linear and nonpolar?
Which molecule is linear and nonpolar?
Which of the following compounds would you expect to have the highest melting point?
Which of the following compounds would you expect to have the highest melting point?
A solution has a hydroxide ion concentration of $1.0 \times 10^{-3}$ M. What is the $pH$ of this solution?
A solution has a hydroxide ion concentration of $1.0 \times 10^{-3}$ M. What is the $pH$ of this solution?
Flashcards
VSEPR Theory
VSEPR Theory
Predicts molecular shape based on minimizing electron pair repulsion around a central atom.
Polar Covalent Bond
Polar Covalent Bond
A covalent bond where electrons are unequally shared creating partial charges.
Polar Molecule
Polar Molecule
A molecule with unequally distributed electrons due to asymmetrical polar bonds or lone pairs.
Intermolecular Forces (IMFs)
Intermolecular Forces (IMFs)
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Dipole-Dipole Interactions
Dipole-Dipole Interactions
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London Dispersion Forces (LDF)
London Dispersion Forces (LDF)
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Hydrogen Bonding
Hydrogen Bonding
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"Like Dissolves Like"
"Like Dissolves Like"
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Arrhenius Acids
Arrhenius Acids
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Arrhenius Bases
Arrhenius Bases
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Brønsted-Lowry Acids
Brønsted-Lowry Acids
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Brønsted-Lowry Bases
Brønsted-Lowry Bases
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Water's Autoionization
Water's Autoionization
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pH Scale
pH Scale
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pH Equation
pH Equation
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pOH Equation
pOH Equation
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Titration
Titration
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Study Notes
- This study guide covers molecular geometry, intermolecular forces, and acids/bases.
Molecular Shape and Polarity
- VSEPR theory predicts molecular shape by minimizing electron pair repulsion around a central atom.
- Key molecular shapes include linear, trigonal planar, tetrahedral, trigonal pyramidal, and bent.
- Polar covalent bonds occur between atoms with differing electronegativities, resulting in partial charges (δ+ and δ-).
- Non-polar covalent bonds occur between atoms with similar electronegativities.
- Molecular polarity is determined by electron distribution.
- Polar molecules have unequally distributed electrons due to asymmetrical polar bonds or lone pairs, creating a dipole moment.
Intermolecular Forces (IMFs)
- IMFs are attractive forces between molecules.
- Dipole-dipole forces occur between polar molecules.
- London Dispersion Forces (LDF) are present in all molecules due to temporary electron distribution fluctuations.
- Hydrogen bonding is a strong dipole-dipole interaction between molecules with O-H, N-H, or F-H bonds.
- Stronger IMFs result in higher melting and boiling points.
- "Like dissolves like" dictates solubility: polar solvents dissolve polar solutes, and non-polar solvents dissolve non-polar solutes.
Acids and Bases
- Arrhenius acids increase the concentration of H+ in water, have a pH < 7, taste sour, and turn litmus red.
- Arrhenius bases increase the concentration of OH- in water, have a pH > 7, taste bitter, feel slippery, and turn litmus blue.
- Brønsted-Lowry acids are proton (H+) donors.
- Brønsted-Lowry bases are proton (H+) acceptors.
- Water autoionizes slightly, producing equal concentrations of H+ and OH-, resulting in a neutral pH of 7
- The autoionization reaction is H2O ⇄ H+ + OH- or 2H2O ⇄ H3O+ + OH-
- The pH scale ranges from 0 to 14, indicating acidity or basicity.
- pH = -log[H+]
- pOH = -log[OH-]
- pH + pOH = 14
- Higher [H3O+] corresponds to a lower pH, indicating a more acidic solution.
- Titration is a method to determine the concentration of an acid or base using a neutralization reaction.
- Indicators signal the titration endpoint with a color change at a specific pH.
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