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General Chemistry for Health Sciences
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General Chemistry for Health Sciences

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What is the ratio of chlorine-35 to chlorine-37 in naturally occurring chlorine?

  • 3:1 (correct)
  • 2:3
  • 4:1
  • 1:2

    • What does the atomic mass represent?

  • The weighted average of the masses of all isotopes present (correct)
  • The combined mass of all isotopes in equal proportions
  • The total mass of all atoms in a compound
  • The mass number of the most abundant isotope

    • If 75.77% of chlorine atoms are chlorine-35, what is the decimal equivalent of this percentage?

  • 0.757
  • 0.7577 (correct)
  • 0.7757
  • 0.0777

    • Which of the following calculations would be used to find the contribution of chlorine-37 to the atomic mass of chlorine?

    <p>0.2423 × 37</p> Signup and view all the answers

    What is the atomic mass of chlorine if it contains 75.77% of chlorine-35 and 24.23% of chlorine-37?

    <p>35.34</p> Signup and view all the answers

    What is the primary characteristic of metals in terms of electron behavior?

    <p>They lose electrons.</p> Signup and view all the answers

    Where are nonmetals primarily located on the periodic table?

    <p>Right 1/3</p> Signup and view all the answers

    Which of the following properties is NOT typical of metals?

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

    What does the atomic number of an element represent?

    <p>The number of protons in the nucleus.</p> Signup and view all the answers

    Which of the following describes metalloids?

    <p>Substances with properties intermediate between metals and nonmetals.</p> Signup and view all the answers

    What are the typical states of nonmetals at room temperature?

    <p>Solid, liquid, or gas.</p> Signup and view all the answers

    What is the relationship between atomic mass and atomic number?

    <p>Atomic mass is always greater than atomic number.</p> Signup and view all the answers

    Which of the following is NOT a property of metals?

    <p>Powdery solids</p> Signup and view all the answers

    What is the weighted average atomic mass of chlorine based on isotopes 35Cl and 37Cl?

    <p>35.5 amu</p> Signup and view all the answers

    Which of the following isotopes of neon has the highest natural abundance?

    <p>20Ne</p> Signup and view all the answers

    According to the periodic law, how are the physical and chemical properties of elements organized?

    <p>Periodically with respect to their atomic numbers</p> Signup and view all the answers

    What characterizes a 'group' in the periodic table?

    <p>Columns that share similar properties</p> Signup and view all the answers

    Which trend regarding metals is mentioned in the content?

    <p>Metals form positive ions by losing electrons</p> Signup and view all the answers

    What is the combined atomic mass contribution of the isotopes 20Ne and 21Ne considering their abundances?

    <p>$20.0 amu imes 0.9048 + 21.0 amu imes 0.0027$</p> Signup and view all the answers

    What distinguishes a period in the periodic table?

    <p>A sequential arrangement of elements based on their atomic number</p> Signup and view all the answers

    Which two scientists contributed to the development of the modern Periodic Table?

    <p>Dmitri Mendeleev and Lothar Meyer</p> Signup and view all the answers

    What does electron configuration describe?

    <p>The arrangement of electrons in atoms</p> Signup and view all the answers

    What are valence electrons?

    <p>The electrons involved in chemical bonding</p> Signup and view all the answers

    How many principal energy levels are there in an atom?

    <p>Counted as n=1, n=2, n=3, ...</p> Signup and view all the answers

    Which of the following is true regarding the capacity of a principal energy level?

    <p>The formula to calculate is 2(n)²</p> Signup and view all the answers

    What did Schrödinger contribute to the understanding of electron arrangement?

    <p>Introduced quantum mechanics to determine electron probability</p> Signup and view all the answers

    Which sublevels exist within the principal energy level n=3?

    <p>s, p, and d</p> Signup and view all the answers

    What occurs as the value of n increases?

    <p>Energy levels are farther from the nucleus</p> Signup and view all the answers

    How many electrons can the n=3 level hold?

    <p>18</p> Signup and view all the answers

    Which model failed to adequately explain the electron structure of atoms apart from hydrogen?

    <p>Bohr’s model</p> Signup and view all the answers

    What is the relationship between the number of sublevels and principal energy levels?

    <p>Equal to n</p> Signup and view all the answers

    What defines an atom as the basic structural unit of an element?

    <p>It retains the chemical properties of that element.</p> Signup and view all the answers

    Which of the following correctly describes the charge of protons and electrons?

    <p>Protons have a positive charge while electrons have a negative charge.</p> Signup and view all the answers

    What is the mass number of an atom, represented as A?

    <p>The sum of the number of protons and neutrons.</p> Signup and view all the answers

    How can the number of neutrons in an atom be calculated?

    <p>By subtracting the atomic number from the mass number.</p> Signup and view all the answers

    What characterizes isotopes of the same element?

    <p>They have the same number of protons but different masses.</p> Signup and view all the answers

    What is the charge and mass (in amu) of a neutron?

    <p>Charge: 0, Mass: 1.0 amu</p> Signup and view all the answers

    In a neutral atom, which of the following statements is true?

    <p>Number of protons equals the number of electrons.</p> Signup and view all the answers

    Which of the following is true regarding the nucleus of an atom?

    <p>It is positively charged and dense.</p> Signup and view all the answers

    What is represented by the atomic number (Z) of an atom?

    <p>The number of protons in the atom.</p> Signup and view all the answers

    Which statement about electrons is accurate?

    <p>Electrons have mass much smaller than protons.</p> Signup and view all the answers

    Which of the following is an accurate method to determine the composition of an atom?

    <p>Using the mass number and atomic number.</p> Signup and view all the answers

    What is the main feature of isotopes of hydrogen?

    <p>They contain the same number of protons but different numbers of neutrons.</p> Signup and view all the answers

    What is the approximate mass in grams of a proton?

    <p>1.6725 × 10^-24 grams</p> Signup and view all the answers

    Which of the following particles has a negative charge?

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

    Study Notes

    General Chemistry Overview

    • General Chemistry covers fundamental concepts crucial for health sciences.
    • Key chapters include: Methods and Measurements, Atomic Structure, States of Matter, and Nuclear Medicine.

    Composition of the Atom

    • Atoms consist of three subatomic particles: electrons, protons, and neutrons.
    • Nucleus contains protons (positive charge) and neutrons (no charge).
    • Electrons are negatively charged and located outside the nucleus, moving rapidly.

    Atomic Properties

    • Atomic number (Z) equals the number of protons.
    • Mass number (A) represents the sum of protons and neutrons.
    • For a neutral atom, the number of protons equals the number of electrons.

    Subatomic Particle Characteristics

    • Electrons: Charge of -1, mass of approximately 0.00055 amu.
    • Protons: Charge of +1, mass of about 1.0 amu.
    • Neutrons: No charge, mass of approximately 1.0 amu.

    Isotopes

    • Isotopes are variants of elements with the same number of protons but different neutrons.
    • Examples include Hydrogen, Deuterium, and Tritium.
    • Isotopes of the same element share identical chemical properties, but some can be radioactive.

    Atomic Mass Calculation

    • Atomic mass is the weighted average of isotopes' masses in nature.
    • For chlorine, atomic mass (35.34) derived from isotopes 35Cl and 37Cl with respective abundances of 75.77% and 24.23%.
    • Calculation involves converting percentages to decimal, multiplying by isotope mass, then summing contributions.

    Periodic Law and Table

    • Dmitri Mendeleev and Lothar Meyer developed the Periodic Table based on atomic mass and properties.
    • Periodic Law states properties of elements are periodic functions of their atomic numbers.
    • Periods are horizontal rows; groups (families) are vertical columns.

    Element Classification

    • Metals: Typically lose electrons, form positive ions, have high conductivity, malleability, and luster; primarily found in the left two-thirds of the periodic table.
    • Nonmetals: Gain electrons, form negative ions; appear in the right third of the table, often brittle and gaseous.
    • Metalloids: Exhibit properties of both metals and nonmetals.

    Electron Configuration

    • Electron configuration describes the arrangement of electrons in atoms, with valence electrons being crucial for bonding.
    • Principal energy levels increase in energy and distance from the nucleus, noted as n (n=1, 2, 3,...).
    • Each principal level has corresponding sublevels (s, p, d, f) that determine specific regions where electrons are likely to be found.

    Schrödinger’s Quantum Mechanics

    • Schrödinger developed equations to describe electrons' probable positions, integrating particle and wave characteristics.
    • Each principal level contains sublevels, with the capacity of each level calculated as 2(n)^2, defining maximum electron holdings (e.g., n=2 holds 8 electrons).

    Energy Levels

    • As n increases, energy levels rise, with each having the same number of sublevels as its value (e.g., n=3 has three sublevels).

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    Description

    Test your knowledge on the fundamentals of chemistry tailored for health sciences. This quiz covers key concepts from atomic structure to the properties of various compounds and states of matter. Perfect for students looking to solidify their understanding of chemistry in a health-related context.

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