Group 13 Elements Quiz
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Questions and Answers

Which element has the highest electronegativity among group 13 elements?

  • Indium
  • Gallium
  • Thallium
  • Boron (correct)

    • What trend does electronegativity follow in group 13 elements?

  • Remains constant down the group
  • Increases consistently down the group
  • Increases from Al to Ti
  • Decreases from B to Al and then increases slightly (correct)

    • Which of the following statements is correct regarding electronegativity in group 13?

  • Gallium has similar electronegativity to Boron.
  • Thallium has higher electronegativity than Indium.
  • Boron forms pr-pr multiple bonds. (correct)
  • Aluminum is the most electronegative element.

    • Which element exists in a liquid state during summer?

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

    What is the incorrect characteristic of Boron?

    <p>It is metallic in nature.</p> Signup and view all the answers

    Which element has the lowest electronegativity among group 13 elements?

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

    What is the main reason for Boron's high melting point?

    <p>It is a covalent solid.</p> Signup and view all the answers

    Which order correctly represents the size trend among group 13 elements?

    <p>B &lt; Al &lt; Ga &lt; In &lt; Ti</p> Signup and view all the answers

    What is the outer electronic configuration of group-13 elements?

    <p>ns² np</p> Signup and view all the answers

    What factor significantly influences the stability of aluminum compounds?

    <p>The oxidation states of aluminum</p> Signup and view all the answers

    What is the atomic number of thallium?

    <p>81</p> Signup and view all the answers

    What is the outermost electronic configuration of a group-13 element E if it is denoted as 4s² 4p?

    <p>(Ar) 3d¹⁰ 4s² 4p²</p> Signup and view all the answers

    Which statement correctly describes the behavior of aluminum in terms of oxidation?

    <p>Aluminum typically exhibits a +3 oxidation state.</p> Signup and view all the answers

    Which elements belong to the p-block of the periodic table?

    <p>Elements from groups 13 to 18</p> Signup and view all the answers

    What does not prevent oxidation in aluminum compounds?

    <p>Presence of ionic bonds</p> Signup and view all the answers

    How does the density of group-13 elements change down the group?

    <p>Increases down the group</p> Signup and view all the answers

    What can be inferred about aluminum's ionic and covalent character?

    <p>Aluminum shows mixed bonding characteristics depending on its oxidation state.</p> Signup and view all the answers

    Which statement is correct regarding the reaction of aluminum and oxidation?

    <p>Aluminum may oxidize and reduce depending on the reaction conditions.</p> Signup and view all the answers

    Which of the following electronic configurations corresponds to a p-block element?

    <p>[Kr] 4d¹⁰ 5s² 5p²</p> Signup and view all the answers

    Which statement about the elements from group 13 is correct?

    <p>They exhibit similar chemical reactivity.</p> Signup and view all the answers

    Why is aluminum considered to have a +3 oxidation state?

    <p>It readily loses three electrons.</p> Signup and view all the answers

    In which period of the periodic table does thallium belong?

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

    Which characteristic enhances the stability of aluminum compounds?

    <p>Inert pair effect</p> Signup and view all the answers

    Which element's behavior is important when analyzing aluminum's compound formation?

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

    What role does nuclear bonding play in chemical properties?

    <p>It enhances the stability of ionic compounds.</p> Signup and view all the answers

    Which statement is true regarding the bonding in inert gases?

    <p>They exhibit little tendency to form stable bonds.</p> Signup and view all the answers

    How does the position in the periodic table affect ion charge?

    <p>Elements lower in the table consistently form positive ions.</p> Signup and view all the answers

    What is indicated by increase in ion reactivity as charge increases?

    <p>Increased charge results in stronger electrostatic forces.</p> Signup and view all the answers

    What general trend is observed as you move down a group in the periodic table?

    <p>Bonding enthalpies generally become lower.</p> Signup and view all the answers

    Which of the following correctly explains the bond formation in smaller ions?

    <p>Small ions create strong bonds owing to closer distance of nuclei.</p> Signup and view all the answers

    In the context of chemical properties, what effect does an increase in enthalpy have?

    <p>Higher enthalpy values correlate to decreased reaction rates.</p> Signup and view all the answers

    What effect does charge have as it relates to bond energy in ions?

    <p>Higher charge typically increases bond energy.</p> Signup and view all the answers

    Which of the following halides is referred to as a trihalide?

    <p>BI3</p> Signup and view all the answers

    Which property is observed in BCl3 that affects its reactions?

    <p>Presence of vacant d-orbitals</p> Signup and view all the answers

    Which statement about BF3 is accurate?

    <p>It behaves as a Lewis acid.</p> Signup and view all the answers

    What is a characteristic feature of covalent compounds formed by boron?

    <p>They often involve delocalized electrons.</p> Signup and view all the answers

    Which compound is least likely to exhibit acidic behavior?

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

    Which statement describes the oxidation state of boron in its trihalides?

    <p>Boron has a +3 oxidation state.</p> Signup and view all the answers

    What trend is observed regarding the stability of boron halides?

    <p>Stability decreases with the size of the halogen.</p> Signup and view all the answers

    Which of the following is true regarding the covalent character of boron halides?

    <p>Covalent character varies with different halides.</p> Signup and view all the answers

    What type of hybridization is suggested by the tetrahedral nature of certain halides?

    <p>sp3</p> Signup and view all the answers

    Which of the following statements is false about the bonding in boron halides?

    <p>They exhibit hyperconjugation.</p> Signup and view all the answers

    Study Notes

    Group 13 Elements

    • Group 13 elements are called p-block elements as they belong to groups 13-18.
    • Group 13 elements have an outer electronic configuration of ns²np¹
    • The atomic number of thallium is 81.
    • The outer electronic configuration of a group 13 element is 4s²4p¹
    • The element diagonally placed to an element with an electronic configuration of [Kr]4d¹⁰ 5s²5p¹ has an electronic configuration of [Xe]4f¹⁴ 5d¹⁰ 6s²6p¹
    • Density of the elements increases down the group from boron to thallium.
    • Size: Ga < TI
    • Ionization Energy: In > TI
    • Electronegativity decreases from B to Al and then increases marginally down the group.
    • The reason for the irregular trend in electronegativity is discrepancies in atomic size.
    • Boron has the highest electronegativity among group 13 elements.
    • Thallium has the lowest electronegativity among group 13 elements.
    • The order of electronegativity in group 13 elements is B > Al > Ga > In > TI.
    • Gallium is a metal that exists in a liquid state during summer.
    • Gallium is a soft, heavy metal with a melting point of 30°C and is used in making heat sensitive thermometers.
    • Boron is a hard, black-colored solid.
    • Boron has unusually high melting point.
    • The high melting point of boron is due to the strong covalent bonds in boron.
    • Boron exists in many allotropic forms.
    • Boron forms covalent compounds due to its small size.
    • The tendency to form covalent compounds decreases with decreasing size down the group.
    • Due to its small size, boron has high ionization enthalpy and it prevents it from forming ionic compounds.
    • Boron forms covalent compounds with halogens, oxygen and nitrogen.
    • Boron trihalides, BF₃, BCl₃, BBr₃ and BI₃ have the following order of acid strength: BF₃< BCl₃ < BBr₃ < BI₃
    • BF₃ has the ability to accept a pair of electrons due to incomplete octet, forming a coordinate covalent bond.
    • This ability of BF₃ to accept a pair of electrons is known as "back bonding" due to overlap of p-orbitals of F and empty p-orbitals of boron.
    • The tendency to form covalent compounds decreases as we move down the group due to large size and metallic character.
    • Tl forms stable +1 oxidation state because of the inert pair effect and stability of ns² configuration.
    • The inert pair effect is the tendency of the two electrons in the outermost s orbital to not participate in bonding.
    • The inert pair effect is most pronounced for heavier elements, such as thallium.
    • The stability of the ns² configuration is due to the higher nuclear charge and poor shielding of d-orbitals
    • This results in a lower oxidation state of Tl being more stable.
    • The halides of group 13 elements are covalent in nature.
    • The covalent nature of the compounds is due to the small size of boron and the ability of the elements to form pπ-pπ bonds.

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    Test your knowledge on the properties and configurations of Group 13 elements. This quiz covers key characteristics, trends, and specific details regarding their electronegativity, ionization energy, and more. Challenge yourself and see how well you know these important p-block elements!

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