Chemistry Chapter 2: Chemical Organization
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Questions and Answers

Which of the following elements constitutes the majority of body weight?

  • Sodium
  • Sulfur
  • Chlorine
  • Carbon (correct)
  • How many of the naturally occurring elements have a biological role?

  • 24 (correct)
  • 92
  • 6
  • 12
  • Which of the following is NOT classified as a major element in living organisms?

  • Nitrogen
  • Oxygen
  • Calcium
  • Iron (correct)
  • What percentage of the body's weight is constituted by minerals?

    <p>4%</p> Signup and view all the answers

    Which of the following functions is associated with electrolytes?

    <p>Promoting muscular contraction</p> Signup and view all the answers

    What does the atomic number of an element represent?

    <p>Number of protons in its nucleus</p> Signup and view all the answers

    What is the primary reason elements are organized by atomic number in the periodic table?

    <p>To indicate the number of protons</p> Signup and view all the answers

    How is the atomic mass of an element determined?

    <p>Approximation of protons and neutrons in an atom</p> Signup and view all the answers

    What characterizes a nonpolar covalent bond?

    <p>Shared electrons spend approximately equal time around each nucleus.</p> Signup and view all the answers

    What happens in a polar covalent bond?

    <p>Electrons spend more time orbiting one nucleus than the other.</p> Signup and view all the answers

    What characterizes isotopes of an element?

    <p>Same number of protons but different neutrons</p> Signup and view all the answers

    What is the nature of a hydrogen bond?

    <p>It is a weak attraction between a slightly positive hydrogen atom and a slightly negative atom.</p> Signup and view all the answers

    What can radioactive isotopes potentially cause when they decay?

    <p>Generation of free radicals</p> Signup and view all the answers

    Which of the following isotopes is radioactive?

    <p>Carbon-14</p> Signup and view all the answers

    Why are hydrogen bonds significant in physiology?

    <p>They help maintain the structure of proteins and DNA.</p> Signup and view all the answers

    Which of the following statements is true about nonpolar covalent bonds?

    <p>They occur when atoms are of similar electronegativity.</p> Signup and view all the answers

    What type of radiation can radioactive isotopes emit?

    <p>All of the above</p> Signup and view all the answers

    What is one medical application of radioactive isotopes?

    <p>Nuclear medicine for organ function imaging</p> Signup and view all the answers

    How do hydrogen bonds affect water molecules?

    <p>They enable water to form a cohesive liquid.</p> Signup and view all the answers

    What is true about the stable isotopes of an element?

    <p>They always have the same number of protons and neutrons</p> Signup and view all the answers

    Which of the following is NOT a characteristic of a polar covalent bond?

    <p>It is the strongest type of bond.</p> Signup and view all the answers

    What role do hydrogen bonds play in the structure of DNA?

    <p>They connect complementary base pairs in the double helix.</p> Signup and view all the answers

    Which of the following describes ionizing radiation?

    <p>Ejects electrons from atoms</p> Signup and view all the answers

    What role does water play in chemical reactions?

    <p>It ionizes into H+ and OH- ions.</p> Signup and view all the answers

    How does water's high specific heat benefit the human body?

    <p>It maintains a stable internal temperature.</p> Signup and view all the answers

    What does a pH of 4.0 indicate about a solution's acidity?

    <p>It is 10 times more acidic than a solution with pH 5.0.</p> Signup and view all the answers

    What is true about the pH scale?

    <p>The scale is logarithmic regarding hydrogen ion concentration.</p> Signup and view all the answers

    What happens to water molecules in terms of temperature stability?

    <p>Hydrogen bonds allow them to resist temperature changes.</p> Signup and view all the answers

    What is the primary function of buffers in the body?

    <p>Resist changes in pH</p> Signup and view all the answers

    Which compound acts as a weak base in the carbonic acid-bicarbonate buffer system?

    <p>Bicarbonate ion</p> Signup and view all the answers

    What type of reaction is characterized by the formation of a more complex chemical structure?

    <p>Synthesis reaction</p> Signup and view all the answers

    Which process involves breaking complex substances into simpler components?

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

    Which of the following correctly represents a decomposition reaction?

    <p>AB → A + B</p> Signup and view all the answers

    In reversible reactions, which factor determines the direction of the reaction?

    <p>Concentration of reactants and products</p> Signup and view all the answers

    What happens during dehydration reactions?

    <p>Water is removed to form chemical bonds</p> Signup and view all the answers

    What characterizes an exchange reaction?

    <p>New bonds are formed and old bonds are broken</p> Signup and view all the answers

    How do buffers help maintain homeostasis?

    <p>By removing hydrogen ions when they are in excess</p> Signup and view all the answers

    What is a defining characteristic of metabolism?

    <p>It encompasses all chemical processes in the body</p> Signup and view all the answers

    Study Notes

    Atoms and Elements

    • Elements are pure substances that cannot be decomposed into simpler forms; they represent the smallest amount of matter.
    • The periodic table lists 92 naturally occurring elements; 24 of these have biological roles.
    • Six elements account for 98.5% of body weight: oxygen, carbon, hydrogen, nitrogen, calcium, and phosphorus.
    • Oxygen, carbon, hydrogen, and nitrogen alone represent 96% of body weight; remaining 4% includes trace elements.

    Major Elements in Living Organisms

    • Minerals are inorganic elements sourced from soil, essential for life, including calcium, phosphorus, chlorine, magnesium, potassium, sodium, and sulfur, making up about 4% of body weight.
    • Minerals play crucial roles in body structure, enzyme functions, and are vital electrolytes for nerve and muscle activities.

    Atomic Number and Mass

    • Atomic number indicates the number of protons in an element and determines its position in the periodic table.
    • Atomic mass is the sum of protons and neutrons in an atom.
    • Isotopes of an element differ in neutron count but have the same number of protons and electrons, reacting chemically in the same way.

    Radioactive Isotopes

    • Unstable isotopes can undergo decay, releasing energy and atomic fragments, posing risks such as genetic mutations and cancer.
    • However, radioactive isotopes have medical applications like imaging (MRI, CT scans) and targeted radiation therapy for tumors.

    Covalent Bonds

    • Covalent bonds can be nonpolar (equal electron sharing) or polar (unequal electron sharing).
    • Nonpolar bonds are the strongest and involve equal time spent by electrons around nuclei, while polar covalent bonds create slight charges in molecules.

    Hydrogen Bonds

    • Hydrogen bonds are weak attractions between a slightly positive hydrogen atom and a slightly negative atom (oxygen or nitrogen).
    • Essential in maintaining the structure of proteins and DNA, they influence the properties of water.

    Chemical Reactivity

    • Water's ability to ionize and participate in hydrolysis and dehydration synthesis is crucial for chemical reactivity.
    • Functions as a solvent for acids and salts, essential in biological processes.

    Thermal Stability of Water

    • Water has a high specific heat, allowing it to absorb and release substantial heat with little temperature change, facilitating temperature regulation in living organisms.

    Acids, Bases, and pH

    • The pH scale quantifies hydrogen ion concentration; 7.0 is neutral, values below indicate acidity, and above indicate basicity.
    • Each unit change in pH reflects a tenfold change in hydrogen ion concentration.

    Buffers

    • Buffers are compounds that help maintain pH homeostasis in body fluids, crucial for physiological functions.
    • For example, blood pH is tightly regulated between 7.35 and 7.45 to prevent severe health issues.

    Acid-Base Balance

    • The carbonic acid-bicarbonate buffer system stabilizes blood pH by balancing H⁺ and OH⁻ ion concentrations.
    • If pH falls, bicarbonate ions neutralize excess H⁺ to restore balance.

    Chemical Reactions

    • Chemical reactions involve the formation or breaking of bonds, categorized as reactants and products.
    • Types include synthesis (combination), decomposition (breaking down), exchange (swapping components), and reversible reactions.

    Metabolism

    • Metabolism encompasses all chemical processes in the body, with catabolism (breaking down molecules) and anabolism (building complex molecules) being critical functions.

    Types of Chemical Reactions

    • Synthesis reactions combine small molecules into larger ones, while decomposition reactions split larger molecules into smaller parts.
    • Exchange reactions exchange atoms or groups between molecules, reversible reactions can shift depending on reactant or product quantities.

    Dehydration and Hydrolysis Reactions

    • Dehydration reactions remove water to form bonds, while hydrolysis reactions add water to break bonds, integral for metabolic processes.

    Upcoming Topics

    • Future discussion will cover organic compounds, macromolecules, and biomolecules relevant to biological systems.

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