Medical Chemistry L2: Periodic Table of Elements
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Questions and Answers

What is the primary basis for organizing elements in the Periodic Table?

  • Similar chemical properties (correct)
  • Geographical abundance
  • Increasing size of atoms
  • Atomic mass only
  • Which of the following statements about metals is NOT correct?

  • They are often malleable and shiny.
  • They form positive ions when reacting.
  • They are usually solid at room temperature.
  • They are poor conductors of electricity. (correct)
  • What is the relative atomic mass of oxygen?

  • 14.007 uma
  • 16.00 uma
  • 15.9994 uma (correct)
  • 12.011 uma
  • What mass unit is one twelfth the mass of a carbon-12 atom called?

    <p>Atomic mass unit (u or uma)</p> Signup and view all the answers

    Which property is associated with metalloids?

    <p>Intermediate electrical conductivity</p> Signup and view all the answers

    Which scientist is NOT credited with the independent cataloging of elements?

    <p>John Dalton</p> Signup and view all the answers

    What reaction characteristic describes how metals behave?

    <p>Forming positive ions</p> Signup and view all the answers

    What is the relationship between the mass of a proton and an electron?

    <p>Proton mass is 1836 times greater than electron mass</p> Signup and view all the answers

    What primarily affects the increase in electron affinity across a period?

    <p>Increase in effective nuclear charge</p> Signup and view all the answers

    Which of the following characteristics is NOT associated with non-metals?

    <p>Positive electron affinities</p> Signup and view all the answers

    What type of cation do alkali metals typically form?

    <p>Cations with a +1 charge</p> Signup and view all the answers

    The most electronegative element is:

    <p>Fluorine (F)</p> Signup and view all the answers

    Which group of metals is characterized by having two electrons in their outer shell?

    <p>Alkaline Earth Metals</p> Signup and view all the answers

    What is a common characteristic of transition metals?

    <p>They have multiple oxidation states</p> Signup and view all the answers

    Which statement about halogens is true?

    <p>They are highly reactive non-metals.</p> Signup and view all the answers

    What happens to the ionic radius when an atom forms a cation?

    <p>The ionic radius decreases.</p> Signup and view all the answers

    What is the effect of increasing nuclear charge on ionization energy across a period?

    <p>Ionization energy increases.</p> Signup and view all the answers

    Which statement about electron affinity is correct?

    <p>It is the energy change associated with acquiring an electron.</p> Signup and view all the answers

    How does the atomic radius compare to the cation radius?

    <p>The atomic radius is larger than the cation radius.</p> Signup and view all the answers

    What happens to the first ionization energy as you move down a group in the periodic table?

    <p>It decreases.</p> Signup and view all the answers

    What is the significance of measuring ionization energy experimentally?

    <p>It reveals the energies of electronic levels of an atom.</p> Signup and view all the answers

    Why do anions have a larger ionic radius compared to their atomic radius?

    <p>The addition of electrons increases the electron cloud and distance from the nucleus.</p> Signup and view all the answers

    What is the characteristic of the second ionization energy compared to the first ionization energy for an atom?

    <p>It is always higher than the first ionization energy.</p> Signup and view all the answers

    How many groups are present in the modern periodic table design?

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

    What is the filling order for the s and p orbitals in the modern periodic table?

    <p>s orbitals can hold 2 electrons, p orbitals can hold 6</p> Signup and view all the answers

    Which block in the periodic table contains elements with their outermost electrons in the s orbitals?

    <p>s-block</p> Signup and view all the answers

    What characterizes elements within the same group of the periodic table?

    <p>Similar outer electron configurations</p> Signup and view all the answers

    What is the total number of columns in the d-block of the periodic table?

    <p>10</p> Signup and view all the answers

    In the context of periodic table organization, what does moving from left to right across a period indicate?

    <p>Increasing atomic number</p> Signup and view all the answers

    How many columns are available for f orbitals in the periodic table?

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

    Which group in the periodic table is commonly referred to as group 0?

    <p>Noble gases</p> Signup and view all the answers

    What primarily characterizes the transition metals in the d-block?

    <p>They can form multiple oxidation states.</p> Signup and view all the answers

    How does the atomic radius change as you move down a group in the periodic table?

    <p>It increases.</p> Signup and view all the answers

    What effect does the increase in effective nuclear charge have as you move across a period?

    <p>It causes the atomic radius to decrease.</p> Signup and view all the answers

    How do electrons in the same shell affect each other's repulsive forces?

    <p>They do not effectively shield each other from the nucleus.</p> Signup and view all the answers

    What happens to the ionic radius when an atom gains electrons?

    <p>It increases compared to the atomic radius.</p> Signup and view all the answers

    What is the primary reason for the size increase of an atom as you move down a group?

    <p>The addition of inner shell electrons that provides more shielding.</p> Signup and view all the answers

    Which of the following statements is true regarding the f-block elements?

    <p>They consist of the actinide and lanthanide series.</p> Signup and view all the answers

    Why do elements of the d-block show little variation in atomic radii across the series?

    <p>The filling of d orbitals does not affect size significantly.</p> Signup and view all the answers

    Study Notes

    Medical Chemistry L2

    • The lecturer is Professor Dr. Giovanni N. Roviello
    • The course is for Geomedi University, Tbilisi, Georgia
    • Topic: Periodic Table of Elements

    Periodic Table of Elements

    • A catalog of all known elements
    • Organized by characteristics
    • Similar elements in the same column
    • Elements with increasing mass placed sequentially
    • Developed independently by Dmitri Mendeleev and Lothar Meyer

    Arrangement of elements in the periodic table

    • Periods: Horizontal rows, increasing atomic size
    • Groups: Vertical columns, similar chemical properties (state of matter, reactivity)

    Types of Elements

    • Metals: Solids at room temperature, good conductors of electricity, malleable, shiny, form positive ions
    • Non-metals: Gases or solids at room temperature, poor conductors of electricity, form negative ions
    • Metalloids: Have intermediate properties, semiconductors used in technology.

    Elementary Properties of atoms-Mass

    • The mass of particles are: -Proton: 1.672623 x 10⁻²⁷ kg -Neutron: 1.674929 x 10⁻²⁷ kg -Electron: 9.1093690 x 10⁻³¹ kg
    • Proton mass is 1836 times greater than electron mass

    Atomic Mass Unit (UMA)

    • Atomic masses in kilograms are very small
    • Relative atomic masses are compared to a reference value, the atomic mass unit (uma): -One twelfth of the mass of a carbon-12 atom (1.66 x 10⁻²⁷ kg)
    • Relates atomic mass to carbon-12

    Periodic Table History and Modern Periodic Table

    • Mendeleev (1869) based classification on chemical properties
    • Meyer (1869) based classification on physical properties
    • Modern table reflects atomic structure insights and quantum theory
    • Organizes elements according to electron orbital filling principles (Aufbau Principle)

    Blocks in the Periodic Table

    • Four blocks (s, p, d, f) correspond to orbital types
    • Number of columns in each block corresponds to the number of electrons that can be accommodated in the relevant orbital subshells.
      • s-block: 2 columns
      • p-block: 6 columns
      • d-block: 10 columns
      • f-block: 14 columns

    Groups and Periods in the Periodic Table

    • Groups: Columns; Elements share similar outer electron configuration and have similar properties
    • Periods: Rows; Atomic number increases from left to right indicating the addition of one proton and electron

    Periodic Properties- Atomic Radius

    • Half the distance between two identical bonded atoms
    • Increases down a group (due to new electron shells)
    • Decreases across a period (due to increased nuclear charge, less shielding)

    Periodic Properties- Ionic Radius

    • Radius of an ion
    • Increases down a group; Increases going left
    • Decreases going across a period
    • Cations (loss of electrons) are smaller; Anions (gain of electrons) are larger

    Periodic Properties- Ionization Energy

    • Energy required to remove an electron from a neutral atom
    • Higher across a period because of stronger attraction to nucleus
    • Lower down a group as the atom increases in size and electrons are further from the positively charged nucleus.

    Periodic Properties- Electron Affinity

    • Energy change associated with acquiring an electron
    • Increases across a period (due to increased nuclear charge)
    • Decreases down a group as the atom size increases, decreased attraction

    Electronegativity

    • Atom's ability to attract electrons in a bond
    • Based on values of first ionization energy and electron affinity
    • Highest electronegativity is for fluorine
    • Lowest is for cesium

    Classification of Elements

    • Metals (e.g., Iron, Copper, Gold)
    • Non-metals (e.g., Oxygen, Chlorine)
    • Metalloids (e.g., Silicon, Boron)

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    Medical Chemistry L2 PDF

    Description

    Explore the intricate organization of the Periodic Table of Elements in this Medical Chemistry L2 quiz. Understand the classification of elements by their properties, including metals, non-metals, and metalloids, as well as the concepts of periods and groups. This quiz will enhance your knowledge of the fundamental building blocks of matter.

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