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Questions and Answers
What percentage of a human's mass is approximately carbon?
Which chemical element has the strongest tendency to attract electrons based on electronegativity?
Which type of bond involves the sharing of electron pairs between atoms?
What type of noncovalent interaction occurs between a charged group on one molecule and an oppositely charged group on another molecule?
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Which interaction is largely associated with the attraction of a partially positively charged hydrogen atom to a partially negatively charged atom?
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Which arrangement minimizes electron pair repulsion in hydrogen bonding?
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What element is least likely to have a significant role in forming biological compounds based on covalent bonding?
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The stability of hydrogen bonds can be enhanced by which of the following factors?
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Which of the following interactions is weakest among noncovalent interactions?
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What structural feature gives rise to resonance structures?
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Which type of interaction is primarily responsible for the attractive forces between water molecules?
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What characterizes Van der Waals interactions?
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What happens to the pH when strong acids are added to a solution?
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Which of the following interactions involves the formation of water molecule 'cages'?
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How can the concentration of an acid and its conjugate base be described when pH is equal to pKa?
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Which type of interaction is considered the weakest according to the strength hierarchy?
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How would the dielectric constant of water be described?
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What effect does increasing hydrogen ion concentration have on pH?
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What separates a dipole within a molecule?
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What role do nonpolar molecules play in aqueous solutions?
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What is indicated by a pH that is smaller than the pKa value of a weak acid?
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Which statement about weak acids and weak bases functioning as buffers is true?
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What occurs to bicarbonate concentration when carbon dioxide removal is increased during ventilation?
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Why do strong acids and bases form poor buffers?
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What is the primary function of a buffer system involving carbonic acid (H2CO3) and bicarbonate anion (HCO3-)?
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When considering buffer systems, what occurs if there is an excess of hydrogen ions (H+) in the solution?
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Which amino acid is represented as a diprotic acid with more than one dissociable hydrogen ion?
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The dynamic equilibrium of a buffer system allows which of the following?
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What happens if the concentration of hydroxide ions (OH-) increases significantly in a buffered solution?
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How does hyperventilation affect the balance of bicarbonate in the blood?
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What is the primary role of the carbonic acid-bicarbonate buffer in the blood?
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According to the Le Bel–Van 't Hoff rule, how many stereoisomers can a compound with 3 asymmetric carbon atoms have?
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Which statement correctly summarizes the concept of entropy in living systems?
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What stabilizes the tertiary structure of proteins?
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Which of these statements is true regarding myoglobin?
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Which of the following describes the quaternary structure of proteins?
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In the context of thermodynamics, what does enthalpy refer to?
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Which type of amino acids carries a positive charge?
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What is the main factor that governs the stability of the carbonic acid-bicarbonate buffer system?
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Which of the following statements about isomers is correct?
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Study Notes
Biochemistry of Life Processes
- Life on Earth is carbon-based
- 18.5% of human mass is carbon
- Key elements in biological compounds: C, H, O, N, P, S
Covalent Bonds
- Strongest bonds
- Involve electron pair sharing between atoms
Electronegativity
- Property describing an atom's electron attraction
- Trend: O > N > S > C > P > H
Resonance Structures
- Double bonds cause resonance structures
- Not static bonds
Noncovalent Interactions
- Ionic Interactions: Oppositely charged groups attract
- Hydrogen Bonds: Partially positive hydrogen atoms attract partially negative acceptor atoms
- 180° angle in hydrogen bonds minimizes electron pair repulsion, optimizes interaction and increases stability
- Van der Waals Interactions: Weak, temporary attractive forces between molecules
Molecules in Aqueous Solutions
- Interact with water through hydrogen bonding and ionic interactions
- Water is a versatile solvent, especially for polar and charged compounds
Water (H₂O)
- Highly cohesive due to strong hydrogen bonding
- High dielectric constant (80)
Acids and Bases
- Acids: Proton donors
- Bases: Proton acceptors
- pH = -log[H+]
- Buffers help maintain stable pH
Amino Acids
- Peptide Bond Formation: Forms between amino acids
- Hydrophobic Amino Acids: (e.g. Glycine, Alanine, Valine - hydrophobic, less attraction to water molecules)
- Polar Amino Acids: (e.g. Serine, Threonine, Tyrosine - polar, more attraction to water molecules)
- Positively charged: (e.g., Arginine, Histidine, Lysine)
- Negatively charged: (e.g. Aspartate, Glutamate)
Stereoisomers
- Different spatial arrangement of atoms
- Le Bel-Van 't Hoff rule (2n)
Living Systems and Disorder
- Entropy: Measure of disorder in a system
- Enthalpy: Total heat content in a process
- 2nd law of thermodynamics: Natural processes tend to increase disorder
Proteins
- Primary Structure: Amino acid sequence
- Secondary Structure: Hydrogen bonding patterns (alpha helix, beta sheet)
- Tertiary Structure: 3D folding of a protein
- Quaternary Structure: Multiple polypeptide chains
Myoglobin and Hemoglobin
- Myoglobin: Heme protein for oxygen storage, single polypeptide chain
- Hemoglobin: Heme protein for oxygen transport, 4 polypeptide chains (2 alpha, 2 beta)
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Description
Explore the fundamental principles of biochemistry that govern life processes. This quiz covers topics such as covalent bonds, electronegativity, resonance structures, and noncovalent interactions. Test your understanding of how molecules interact in aqueous solutions and the significance of carbon in biological compounds.
