Class 11 Chemistry Chapter 3 Exercise Solutions | NCERT SOLUTIONS| #ncertsolutions
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Hi guys, This Dr. Nileshkumar
Hi guys, This Dr. Nileshkumar Vala from My Smart Class, and in this video I am going to teach you all about Exercise Solution of Classification of Elements and Periodicity In Properties,
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3.1 What is the basic theme of organisation in the periodic table?
3.2 Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that?
3.3 What is the basic difference in approach between the Mendeleev’s Periodic Law and the Modern Periodic Law?
3.4 On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.
3.5 In terms of period and group where would you locate the element with Z =114?
3.6 Write the atomic number of the element present in the third period and seventeenth group of the periodic table.
3.7 Which element do you think would have been named by
(i) Lawrence Berkeley Laboratory
3.8 Why do elements in the same group have similar physical and chemical properties?
3.9 What does atomic radius and ionic radius really mean to you?
3.10 How do atomic radius vary in a period and in a group? How do you explain the variation?
3.11 What do you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions.
3.12 Consider the following species :
3.13 Explain why cation are smaller and anions larger in radii than their parent atoms?
3.14 What is the significance of the terms — ‘isolated gaseous atom’ and ‘ground state’ while defining the ionization enthalpy and electron gain enthalpy?
3.15 Energy of an electron in the ground state of the hydrogen atom is
–2.18×10–18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.
3.16 Among the second period elements the actual ionization enthalpies Explain why (i) Be has higher ∆i H than B
(ii) O has lower ∆i H than N and F?
3.17 How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
3.18 What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?
3.19 The first ionization enthalpy values (in kJ mol–1) of group 13
3.20 Which of the following pairs of elements would have a more negative electron gain enthalpy?
3.21 Would you expect the second electron gain enthalpy of O as positive, more negative or less negative than the first? Justify your answer.
3.22 What is the basic difference between the terms electron gain enthalpy and electronegativity?
3.23 How would you react to the statement that the electronegativity of N on Pauling scale is 3.0 in all the nitrogen compounds?
3.24 Describe the theory associated with the radius of an atom as it
3.25 Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.
3.26 What are the major differences between metals and non-metals?
3.27 Use the periodic table to answer the following questions.
(a) Identify an element with five electrons in the outer subshell.
3.28 The increasing order of reactivity among group 1 elements is
3.29 Write the general outer electronic configuration of s-, p-, d- and f- block elements.
3.30 Assign the position of the element having outer electronic configuration
3.31 The first (∆ iH1) and the second (∆iH2) ionization enthalpies (in kJ mol–1) and the (∆egH)
3.32 Predict the formulas of the stable binary compounds that would be
formed by the combination of the following pairs of elements.
(a) Lithium and oxygen (b) Magnesium and nitrogen
3.33 In the modern periodic table, the period indicates the value of :
(a) atomic number
3.34 Which of the following statements related to the modern periodic table is incorrect?
3.35 Anything that influences the valence electrons will affect the chemistry of the element.
(a) Valence principal quantum number (n)
(b) Nuclear charge (Z )
3.36 The size of isoelectronic species — F–, Ne and Na+ is affected by
(a) nuclear charge (Z )
3.37 Which one of the following statements is incorrect in relation to ionization enthalpy?
3.38 Considering the elements B, Al, Mg, and K, the correct order of their metallic character is :
3.39 Considering the elements B, C, N, F, and Si, the correct order of their non-metallic character is :
3.40 Considering the elements F, Cl, O and N, the correct order of their chemical reactivity in terms of oxidizing property is :
Used mic: https://amzn.to/2SGomkD
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3.1 What is the basic theme of organisation in the periodic table?
3.2 Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that?
3.3 What is the basic difference in approach between the Mendeleev’s Periodic Law and the Modern Periodic Law?
3.4 On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.
3.5 In terms of period and group where would you locate the element with Z =114?
3.6 Write the atomic number of the element present in the third period and seventeenth group of the periodic table.
3.7 Which element do you think would have been named by
(i) Lawrence Berkeley Laboratory
3.8 Why do elements in the same group have similar physical and chemical properties?
3.9 What does atomic radius and ionic radius really mean to you?
3.10 How do atomic radius vary in a period and in a group? How do you explain the variation?
3.11 What do you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions.
3.12 Consider the following species :
3.13 Explain why cation are smaller and anions larger in radii than their parent atoms?
3.14 What is the significance of the terms — ‘isolated gaseous atom’ and ‘ground state’ while defining the ionization enthalpy and electron gain enthalpy?
3.15 Energy of an electron in the ground state of the hydrogen atom is
–2.18×10–18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.
3.16 Among the second period elements the actual ionization enthalpies Explain why (i) Be has higher ∆i H than B
(ii) O has lower ∆i H than N and F?
3.17 How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
3.18 What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?
3.19 The first ionization enthalpy values (in kJ mol–1) of group 13
3.20 Which of the following pairs of elements would have a more negative electron gain enthalpy?
3.21 Would you expect the second electron gain enthalpy of O as positive, more negative or less negative than the first? Justify your answer.
3.22 What is the basic difference between the terms electron gain enthalpy and electronegativity?
3.23 How would you react to the statement that the electronegativity of N on Pauling scale is 3.0 in all the nitrogen compounds?
3.24 Describe the theory associated with the radius of an atom as it
3.25 Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.
3.26 What are the major differences between metals and non-metals?
3.27 Use the periodic table to answer the following questions.
(a) Identify an element with five electrons in the outer subshell.
3.28 The increasing order of reactivity among group 1 elements is
3.29 Write the general outer electronic configuration of s-, p-, d- and f- block elements.
3.30 Assign the position of the element having outer electronic configuration
3.31 The first (∆ iH1) and the second (∆iH2) ionization enthalpies (in kJ mol–1) and the (∆egH)
3.32 Predict the formulas of the stable binary compounds that would be
formed by the combination of the following pairs of elements.
(a) Lithium and oxygen (b) Magnesium and nitrogen
3.33 In the modern periodic table, the period indicates the value of :
(a) atomic number
3.34 Which of the following statements related to the modern periodic table is incorrect?
3.35 Anything that influences the valence electrons will affect the chemistry of the element.
(a) Valence principal quantum number (n)
(b) Nuclear charge (Z )
3.36 The size of isoelectronic species — F–, Ne and Na+ is affected by
(a) nuclear charge (Z )
3.37 Which one of the following statements is incorrect in relation to ionization enthalpy?
3.38 Considering the elements B, Al, Mg, and K, the correct order of their metallic character is :
3.39 Considering the elements B, C, N, F, and Si, the correct order of their non-metallic character is :
3.40 Considering the elements F, Cl, O and N, the correct order of their chemical reactivity in terms of oxidizing property is :
Used mic: https://amzn.to/2SGomkD
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