Atomic Structure and Isotopes Quiz
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Questions and Answers

What is the primary function of the mass spectrometer?

  • To calculate the density of an element
  • To analyze the chemical reactivity of compounds
  • To determine the isotopes present in a sample (correct)
  • To measure the temperature of a sample
  • In isotopes, what remains constant among them?

  • Number of electrons
  • Mass number
  • Number of neutrons
  • Number of protons (correct)
  • Which technique is NOT used for ionization in a mass spectrometer?

  • Chemical vapor deposition (correct)
  • Electron impact
  • Ion drift
  • Electro spray ionization
  • What is the correct relationship for calculating the number of neutrons in an atom?

    <p>Number of neutrons = Mass number - Atomic number</p> Signup and view all the answers

    What happens during the electron impact ionization process?

    <p>Electrons from an electron gun knock out outer electrons</p> Signup and view all the answers

    What primarily causes the increase in first ionisation energy across a period?

    <p>The effective attraction of the nucleus increases due to more protons.</p> Signup and view all the answers

    Why does sodium (Na) have a lower first ionisation energy than neon (Ne)?

    <p>Na's outer electron is in a higher energy level shell.</p> Signup and view all the answers

    Which characteristic is true for heavier ions in a mass spectrometer?

    <p>They have a longer drift time than lighter ions</p> Signup and view all the answers

    What accounts for the small drop in first ionisation energy from magnesium (Mg) to aluminium (Al)?

    <p>3p electrons are higher in energy and more shielded.</p> Signup and view all the answers

    What is a defining feature of electro spray ionization?

    <p>It is ideal for larger organic molecules and avoids fragmentation</p> Signup and view all the answers

    What is the reason for the drop from phosphorus (P) to sulfur (S) in first ionisation energy?

    <p>The fourth 3p electron experiences repulsion from other electrons.</p> Signup and view all the answers

    In an atom of Lithium (Li), what is the mass number?

    <p>7</p> Signup and view all the answers

    Which of the following accurately describes the trend in second ionisation energy across periods?

    <p>It displays a similar pattern but shifted one to the left.</p> Signup and view all the answers

    What is unique about lithium's second ionisation energy compared to helium's?

    <p>Lithium's second electron is removed from the 1s shell with no shielding.</p> Signup and view all the answers

    Which factor does NOT contribute to the trend of ionisation energy across a period?

    <p>Increased electron shielding.</p> Signup and view all the answers

    What is meant by periodicity in the context of ionisation energy?

    <p>The repeating pattern of ionisation energy across periods.</p> Signup and view all the answers

    What effect does increasing the mass of a particle have on its velocity, given constant kinetic energy?

    <p>Velocity decreases</p> Signup and view all the answers

    How is the time of flight for an ion in a mass spectrometer determined?

    <p>By its velocity and the length of the flight tube</p> Signup and view all the answers

    What is the relationship between the size of the current generated by ions at the detector and their abundance?

    <p>Directly proportional</p> Signup and view all the answers

    When calculating relative atomic mass, what factors must be included in the equation?

    <p>Isotopic mass and abundance</p> Signup and view all the answers

    What happens during electron impact ionization in a mass spectrometer?

    <p>It breaks the molecules into fragments</p> Signup and view all the answers

    When using electro spray ionization in a mass spectrometer, what is observed?

    <p>Only the molecular ion peak is detected</p> Signup and view all the answers

    What is the m/z value for a 2+ ion of 24Mg?

    <p>12</p> Signup and view all the answers

    How do mass spectrometers assist in identifying elements on other planets?

    <p>By determining the isotopic composition</p> Signup and view all the answers

    What is the significance of the molecular ion peak in mass spectrometry?

    <p>It corresponds to the relative atomic mass of the molecule</p> Signup and view all the answers

    In the calculation of relative atomic mass, what needs to be done when using relative abundance instead of percentage abundance?

    <p>Use the same equation with different values</p> Signup and view all the answers

    During the mass spectrum analysis of Cl2, which isotopes are involved?

    <p>Cl35 and Cl37</p> Signup and view all the answers

    What assumption can be made about ions with smaller m/z values in a flight tube?

    <p>They achieve the same energy but have higher velocities</p> Signup and view all the answers

    What is a key feature of the Bohr model of the atom?

    <p>Electrons are arranged in shells</p> Signup and view all the answers

    Which combination of isotopes would yield an average atomic mass of approximately 63.5 for copper?

    <p>75% of 63Cu and 25% of 65Cu</p> Signup and view all the answers

    Which of the following correctly describes the filling order of sublevels in an atom?

    <p>1s → 2s → 2p → 3s → 3p → 4s → 3d</p> Signup and view all the answers

    What is the electronic configuration of a calcium atom?

    <p>1s2 2s2 2p6 3s2 3p6 4s2</p> Signup and view all the answers

    Which subshell is filled first for d-block elements when they form ions?

    <p>4s before 3d</p> Signup and view all the answers

    What is the correct definition of first ionisation energy?

    <p>Energy change when one mole of gaseous atoms forms gaseous ions</p> Signup and view all the answers

    Which factor does NOT affect the first ionisation energy?

    <p>Mass of the atom</p> Signup and view all the answers

    Which statement is true regarding successive ionisation energies?

    <p>Successive ionisation energies generally increase</p> Signup and view all the answers

    What electronic structure corresponds to the ion Mg2+?

    <p>1s2 2s2 2p6</p> Signup and view all the answers

    Why does helium have a higher first ionisation energy than hydrogen?

    <p>It has its first electron in the first shell with no shielding</p> Signup and view all the answers

    Which of the following ions has a configuration of [Ar] 4s03d10?

    <p>Zn2+</p> Signup and view all the answers

    In which group of the periodic table is an element with a large jump between its 2nd and 3rd ionisation energies likely to be found?

    <p>Group 2</p> Signup and view all the answers

    Which element displays an electronic configuration of 1s22s22p63s23p6 4s13d5?

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

    What is the ionisation energy trend as you move down a group in the periodic table?

    <p>Decreases due to increased shielding</p> Signup and view all the answers

    When filling orbitals within the same sublevel, according to Hund's rule, how should electrons be placed?

    <p>Fill each orbital singly before pairing up electrons</p> Signup and view all the answers

    What shape do p sublevels have?

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

    What is the electronic configuration of an oxygen ion (O2-)?

    <p>1s2 2s2 2p6</p> Signup and view all the answers

    Study Notes

    Atomic Structure

    • Subatomic Particles: Atoms have three fundamental particles:
      • Protons: Located in the nucleus, with a relative mass of 1 and a relative charge of +1.
      • Neutrons: Located in the nucleus, with a relative mass of 1 and a relative charge of 0.
      • Electrons: Located in orbitals, with a relative mass of 1/1840 and a relative charge of -1.

    Atomic Representation

    • Lithium (Li) Example: The representation ⁷Li₃ shows:
      • Atomic number (Z): 3 (number of protons).
      • Mass number (A): 7 (total number of protons and neutrons).
      • Number of neutrons: Calculated as A - Z = 7 - 3 = 4

    Isotopes

    • Definition: Atoms of the same element with the same number of protons but different numbers of neutrons are called isotopes.
    • Chemical properties: Isotopes have similar chemical properties due to the same electronic structure.
    • Physical properties: Isotopes may have slightly differing physical properties due to their varying masses.

    Mass Spectrometry

    • Purpose: Used to identify and quantify isotopes in a sample.

    • Conditions: Must be under vacuum to avoid interference from air particles.

    • Steps:

      • Ionisation: Sample is converted into ions (e.g., electron impact, electrospray ionisation). Electron impact is best for smaller molecules, while electrospray is preferred for larger organic molecules.
      • Acceleration: Positive ions are accelerated to a constant kinetic energy by an electric field.
        • Lighter ions accelerate faster.
        • Heavier ions accelerate slower.
      • Flight Tube: Ions travel through a tube where their flight time differs based on mass-to-charge ratio (m/z). Lighter ions move faster.
      • Detection: Ions reach a detector generating a current proportional to abundance.
    • Time of Flight (TOF) Calculations: Time taken for an ion to travel through the flight tube depends on its velocity and the length of the tube. The velocity in turn depends on the ion's mass, ensuring that heavier ions take longer to travel.

      • The mass-to-charge ratio (m/z) is determined for each isotope.
      • Relative atomic mass(RAM) calculation is based on the percentage abundance of isotopes.

    Calculating Relative Atomic Mass (RAM)

    • Formula: RAM = ∑ (isotopic mass × % abundance) / 100
    • Variations: can be used if relative abundance is used instead of percentage abundance.
    • Examples of calculations provided.

    Mass Spectra for Diatomic Molecules

    • Diatomic molecules: Examples for Cl₂and Br₂show that peaks are created due to different isotope combinations.

    Electronic Structure

    • Models: Early Bohr models, modern models consider principal energy levels(numbered 1,2,3..),
      • sub-energy levels labeled s , p, d, and f
      • s holds up to 2 electrons
      • p holds up to 6 electrons
      • d holds up to 10 electrons
      • f holds up to 14 electron
    • Filling Order: Electrons fill orbitals in order of increasing energy. (Example 3d is higher in energy than 4s) Specific filling order: 1s → 2s →2p → 3s → 3p → 4s → 3d → 4p and so on.)
    • Orbital Shapes: s orbitals are spherical, p orbitals are dumbbell-shaped, etc.
    • Electronic Configuration: Writing electronic arrangements using numbers and letters.
      • Example for oxygen: 1s²2s²2p⁴

    Electronic Structure of Ions

    • Positive Ions: Electrons are lost from the outermost shell.
    • Negative Ions: Electrons are gained.

    Ionization Energies

    • Definition: First ionization energy is the energy required to remove one mole of electrons from one mole of gaseous atoms.

    • Factors: Affecting ionization energy include:

      • Nuclear attraction: Stronger with more protons.
      • Electron distance: Greater distance, weaker attraction.
      • Shielding: Inner electrons repel outer electrons, reducing attraction.
    • Successive Ionization Energies: Energies required to remove successive electrons increase due to increased nuclear attraction on remaining electrons.

    • Patterns: -Increases across a period due to increasing nuclear attraction. -Decreases down a group due to increasing distance from the nucleus and shielding. -Specific drops in the graph, due to additional influencing factors, are explained in detail.

    • Groups 1 and 2: These patterns in successive ionization energies give information about the element's electronic structure.

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    Test your knowledge on atomic structure, including subatomic particles, atomic representation, and isotopes. Understand the differences between protons, neutrons, and electrons, and explore how isotopes affect chemical and physical properties.

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