Podcast
Questions and Answers
Which element has the highest electronegativity among group 13 elements?
Which element has the highest electronegativity among group 13 elements?
- Indium
- Gallium
- Thallium
- Boron (correct)
What trend does electronegativity follow in group 13 elements?
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?
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?
Which element exists in a liquid state during summer?
What is the incorrect characteristic of Boron?
What is the incorrect characteristic of Boron?
Which element has the lowest electronegativity among group 13 elements?
Which element has the lowest electronegativity among group 13 elements?
What is the main reason for Boron's high melting point?
What is the main reason for Boron's high melting point?
Which order correctly represents the size trend among group 13 elements?
Which order correctly represents the size trend among group 13 elements?
What is the outer electronic configuration of group-13 elements?
What is the outer electronic configuration of group-13 elements?
What factor significantly influences the stability of aluminum compounds?
What factor significantly influences the stability of aluminum compounds?
What is the atomic number of thallium?
What is the atomic number of thallium?
What is the outermost electronic configuration of a group-13 element E if it is denoted as 4s² 4p?
What is the outermost electronic configuration of a group-13 element E if it is denoted as 4s² 4p?
Which statement correctly describes the behavior of aluminum in terms of oxidation?
Which statement correctly describes the behavior of aluminum in terms of oxidation?
Which elements belong to the p-block of the periodic table?
Which elements belong to the p-block of the periodic table?
What does not prevent oxidation in aluminum compounds?
What does not prevent oxidation in aluminum compounds?
How does the density of group-13 elements change down the group?
How does the density of group-13 elements change down the group?
What can be inferred about aluminum's ionic and covalent character?
What can be inferred about aluminum's ionic and covalent character?
Which statement is correct regarding the reaction of aluminum and oxidation?
Which statement is correct regarding the reaction of aluminum and oxidation?
Which of the following electronic configurations corresponds to a p-block element?
Which of the following electronic configurations corresponds to a p-block element?
Which statement about the elements from group 13 is correct?
Which statement about the elements from group 13 is correct?
Why is aluminum considered to have a +3 oxidation state?
Why is aluminum considered to have a +3 oxidation state?
In which period of the periodic table does thallium belong?
In which period of the periodic table does thallium belong?
Which characteristic enhances the stability of aluminum compounds?
Which characteristic enhances the stability of aluminum compounds?
Which element's behavior is important when analyzing aluminum's compound formation?
Which element's behavior is important when analyzing aluminum's compound formation?
What role does nuclear bonding play in chemical properties?
What role does nuclear bonding play in chemical properties?
Which statement is true regarding the bonding in inert gases?
Which statement is true regarding the bonding in inert gases?
How does the position in the periodic table affect ion charge?
How does the position in the periodic table affect ion charge?
What is indicated by increase in ion reactivity as charge increases?
What is indicated by increase in ion reactivity as charge increases?
What general trend is observed as you move down a group in the periodic table?
What general trend is observed as you move down a group in the periodic table?
Which of the following correctly explains the bond formation in smaller ions?
Which of the following correctly explains the bond formation in smaller ions?
In the context of chemical properties, what effect does an increase in enthalpy have?
In the context of chemical properties, what effect does an increase in enthalpy have?
What effect does charge have as it relates to bond energy in ions?
What effect does charge have as it relates to bond energy in ions?
Which of the following halides is referred to as a trihalide?
Which of the following halides is referred to as a trihalide?
Which property is observed in BCl3 that affects its reactions?
Which property is observed in BCl3 that affects its reactions?
Which statement about BF3 is accurate?
Which statement about BF3 is accurate?
What is a characteristic feature of covalent compounds formed by boron?
What is a characteristic feature of covalent compounds formed by boron?
Which compound is least likely to exhibit acidic behavior?
Which compound is least likely to exhibit acidic behavior?
Which statement describes the oxidation state of boron in its trihalides?
Which statement describes the oxidation state of boron in its trihalides?
What trend is observed regarding the stability of boron halides?
What trend is observed regarding the stability of boron halides?
Which of the following is true regarding the covalent character of boron halides?
Which of the following is true regarding the covalent character of boron halides?
What type of hybridization is suggested by the tetrahedral nature of certain halides?
What type of hybridization is suggested by the tetrahedral nature of certain halides?
Which of the following statements is false about the bonding in boron halides?
Which of the following statements is false about the bonding in boron halides?
Flashcards are hidden until you start studying
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.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
