Atomic Structure and Ionization Energy
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Atomic Structure and Ionization Energy

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Questions and Answers

Which ionization numbers correspond to the removal of an electron from an s-orbital?

  • 1st and 2nd (correct)
  • 1st and 3rd
  • 2nd and 3rd
  • 3rd and 4th

    • What best defines first ionization energy?

  • The energy released when an electron is added to a neutral atom in its gaseous state
  • The energy needed to convert an atom into a cation
  • The energy needed to remove multiple electrons from a neutral atom
  • The energy required to remove one electron from a neutral atom in its gaseous state (correct)

    • Why does the first ionization energy of Group 1 elements decrease down the group?

  • Increased distance of the outermost electron from the nucleus due to additional electron shells (correct)
  • Reduced shielding effect leads to greater force on outer electrons
  • Increased nuclear charge compensates for increased distance of electrons
  • First ionization energy is constant across Group 1 elements

    • What trend in ionization energies would you expect as you move down the periodic table in Group 1?

    <p>Ionization energy decreases steadily</p> Signup and view all the answers

    Which statement correctly describes a characteristic of the ionization energies listed for sodium?

    <p>There are significant jumps between certain ionization energies</p> Signup and view all the answers

    What is the main principle governing the filling of sub-shells in atomic structure?

    <p>Sub-shells fill in order of increasing energy.</p> Signup and view all the answers

    Which of the following sub-shells would be filled after 3p?

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

    What is an orbital?

    <p>A region in an atom where there is a high probability of finding an electron.</p> Signup and view all the answers

    What shape is associated with an s-orbital?

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

    What is the maximum number of electrons that can occupy a p-orbital?

    <p>6</p> Signup and view all the answers

    Which of the following statements about orbitals is false?

    <p>Orbitals have defined shapes that do not vary.</p> Signup and view all the answers

    In the order of filling sub-shells, which of the following represents the correct sequence after 4s?

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

    Which of these statements best describes the arrangement of electrons in an atom?

    <p>Electrons occupy energy levels and sub-shells organized by increasing energy.</p> Signup and view all the answers

    What is defined as the energy required to remove the outermost electron from an atom in its gaseous state?

    <p>First ionization energy</p> Signup and view all the answers

    Based on general trends in the periodic table, which element would likely have the highest first ionization energy?

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

    In the transition from sodium to magnesium, how does the first ionization energy typically change?

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

    Why does potassium likely possess a lower first ionization energy compared to argon?

    <p>Argon has a stable electron configuration</p> Signup and view all the answers

    If the first ionization energy of magnesium is higher than that of sodium, which statement is true regarding their atomic structure?

    <p>Sodium has a larger atomic radius than magnesium.</p> Signup and view all the answers

    What is a common trend in first ionization energies as you move down a group in the periodic table?

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

    Which factor contributes to the variation of first ionization energy amongst the elements from neon to argon?

    <p>The effective nuclear charge acting on the outer electrons</p> Signup and view all the answers

    If the first ionization energy of an element is significantly less than those of its neighboring elements, what might be inferred about that element?

    <p>It may be more reactive than its neighbors</p> Signup and view all the answers

    What is the primary factor that leads to silicon having a higher melting temperature than sulfur?

    <p>Silicon has a stronger covalent bonding compared to sulfur's weaker bonding.</p> Signup and view all the answers

    What type of bonding is primarily present in sodium?

    <p>Metallic bonding</p> Signup and view all the answers

    How does the melting temperature trend from sodium to aluminum in Period 3 of the Periodic Table?

    <p>It increases due to stronger metallic bonding.</p> Signup and view all the answers

    What is the expected ionization energy for potassium?

    <p>Approximately 400 kJ mol</p> Signup and view all the answers

    Which of the following correctly describes the bonding in magnesium oxide (MgO)?

    <p>Ionic bonding</p> Signup and view all the answers

    Why is magnesium oxide (MgO) almost insoluble in water?

    <p>The lattice structure is too strong to break in water.</p> Signup and view all the answers

    Which element in Period 3 has the highest melting temperature based on the provided graph?

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

    What type of structure is found in sulfur?

    <p>Simple molecular</p> Signup and view all the answers

    What is formed when magnesium oxide reacts with dilute sulfuric acid?

    <p>Magnesium sulfate</p> Signup and view all the answers

    Which compound is soluble in water according to the provided data?

    <p>Magnesium sulfate</p> Signup and view all the answers

    What should be done immediately if dilute sulfuric acid spills on a laboratory bench?

    <p>Inform the teacher</p> Signup and view all the answers

    What gas is released in the reaction of magnesium carbonate with dilute sulfuric acid?

    <p>Carbon dioxide</p> Signup and view all the answers

    Why does the reaction between strontium carbonate and dilute sulfuric acid stop after a few seconds?

    <p>Strontium sulfate becomes insoluble</p> Signup and view all the answers

    Which of the following represents the ionic equation for the reaction between sodium sulfate and strontium chloride?

    <p>Sr^2+(aq) + SO4^2-(aq) → SrSO4(s)</p> Signup and view all the answers

    What is generated in the reaction of magnesium carbonate with dilute sulfuric acid besides magnesium sulfate?

    <p>Carbon dioxide</p> Signup and view all the answers

    What type of reaction occurs when strontium sulfate is formed from sodium sulfate and strontium chloride?

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

    Study Notes

    Atomic Structure

    • Electrons fill sub-shells in order of increasing energy levels.
    • The order of the sub-shells are: 1s, 2s, 2p, 3s, 3p, 4s
    • An orbital is a region of space around an atom's nucleus where there is a high probability of finding an electron.
    • s-orbitals are spherical in shape.
    • p-orbitals are dumbbell shaped.

    First Ionization Energy

    • The first ionization energy is the minimum energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous positive ions.
    • The first ionization energy decreases down Group 1 because the outer electron is further from the nucleus in larger atoms.
    • This results in weaker attraction between the electron and the nucleus.
    • Removal of an electron from an 's' orbital would correspond to the 1st, 2nd, 4th, 5th, 7th, 8th, 10th, 11th ionization energies for Sodium.

    Periodicity

    • Ionization energy increases across period 3 from Neon to Argon.
    • However, potassium has a significantly lower first ionization energy than Argon as its outer electron is in the 4s shell, further away from the nucleus and less attracted to the nucleus.

    Period 3 Elements

    • Na (Sodium) has a metallic structure with metallic bonding, resulting in a low melting point.
    • Si (Silicon) has a giant covalent structure with strong covalent bonds between atoms, resulting in a high melting point.
    • S (Sulphur) has a simple molecular structure with weak Van Der Waals forces between molecules, resulting in a low melting point.
    • Silicon has a higher melting point than sulfur due to stronger covalent bonds in its giant covalent structure, requiring more energy to break.
    • The melting point increases from sodium to aluminium due to the increase in the number of delocalised electrons.

    Magnesium Oxide Reactions

    • Magnesium oxide, MgO, is a basic oxide.
    • MgO reacts with dilute sulfuric acid to form magnesium sulfate, MgSO4, which is soluble in water.
    • This reaction can be used to prepare a pure sample of magnesium sulfate, by adding MgO to excess dilute sulfuric acid.
    • The reaction mixture should be filtered and then evaporated to dryness to obtain solid MgSO4.
    • Dilute sulfuric acid is corrosive, if spilled, immediately wash the area with water, and alert a teacher.

    Strontium Compounds

    • Strontium sulfate, SrSO4, is insoluble.
    • The reaction between strontium carbonate, SrCO3, and dilute sulfuric acid stops after the formation of SrSO4 as it creates an insoluble layer over the SrCO3.
    • The ionic equation for the reaction is: Sr2+(aq) + SO42-(aq) → SrSO4(s)

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    Description

    This quiz covers essential concepts of atomic structure, including the arrangement of electrons in sub-shells and the nature of orbitals. Additionally, it delves into the first ionization energy and periodic trends across groups and periods in the periodic table. Test your understanding of these fundamental topics in chemistry.

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