CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313340
Which of the following metals require radiation of highest frequency to cause emission of electrons?
1 Na
2 Mg
3 K
4 Ca
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313341
Statement A : Second ionization enthalpy will be higher than the first ionization enthalpy. Statement B : Ionization enthalpy is a quantitative measure of the tendency of an element to lose electron.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
It is difficult to remove an electron frrom a positively charged ion than a neutral atom due to which \({\rm{I}}{{\rm{E}}_{\rm{2}}}{\rm{ > I}}{{\rm{E}}_{\rm{1}}}{\rm{.}}\) So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313342
Which of the following has the lowest ionisation enthalpy?
1 \({\rm{4}}{{\rm{s}}^{\rm{1}}}\)
2 \({\rm{3}}{{\rm{d}}^{\rm{2}}}\)
3 \({\rm{3}}{{\rm{p}}^{\rm{6}}}\)
4 \({\rm{2}}{{\rm{p}}^{\rm{6}}}\)
Explanation:
\({\rm{4}}{{\rm{s}}^{\rm{1}}}\) is a s-block element.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313343
Which of the following has lowest \(1^{\text {st }}\) ionisation energy?
1 \(\mathrm{Li}\)
2 \(\mathrm{C}\)
3 \(\mathrm{O}\)
4 \(\mathrm{F}\)
Explanation:
Lithium being alkali metal, it has lowest \(1^{\text {st }}\) I.E. among given Order of \(1^{\text {st }}\) IP \(\mathrm{F}>\mathrm{O}>\mathrm{C}>\mathrm{Li}\)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313344
The correct order in which the first ionization potentital increases is
1 K, Be, Na
2 Be, Na, K
3 Na, K, Be
4 K, Na, Be
Explanation:
The electronic configuration of the elements are \(_{\rm{4}}{\rm{Be - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{;}}\,{\,_{{\rm{11}}}}{\rm{Na - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{1}}}\) \(_{{\rm{19}}}{\rm{K - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{4}}{{\rm{s}}^{\rm{1}}}\) The first ionization energy of Be is maximum because electron is to be drawn from stable (fully filled) orbital. The \({{\rm{1}}^{{\rm{st}}}}\) ionization energy of Na is greater than K because size of the K is bigger than Na which facilitates easy removal of electron from its outermost shell. So, the sequence is K < Na < Be.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313340
Which of the following metals require radiation of highest frequency to cause emission of electrons?
1 Na
2 Mg
3 K
4 Ca
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313341
Statement A : Second ionization enthalpy will be higher than the first ionization enthalpy. Statement B : Ionization enthalpy is a quantitative measure of the tendency of an element to lose electron.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
It is difficult to remove an electron frrom a positively charged ion than a neutral atom due to which \({\rm{I}}{{\rm{E}}_{\rm{2}}}{\rm{ > I}}{{\rm{E}}_{\rm{1}}}{\rm{.}}\) So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313342
Which of the following has the lowest ionisation enthalpy?
1 \({\rm{4}}{{\rm{s}}^{\rm{1}}}\)
2 \({\rm{3}}{{\rm{d}}^{\rm{2}}}\)
3 \({\rm{3}}{{\rm{p}}^{\rm{6}}}\)
4 \({\rm{2}}{{\rm{p}}^{\rm{6}}}\)
Explanation:
\({\rm{4}}{{\rm{s}}^{\rm{1}}}\) is a s-block element.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313343
Which of the following has lowest \(1^{\text {st }}\) ionisation energy?
1 \(\mathrm{Li}\)
2 \(\mathrm{C}\)
3 \(\mathrm{O}\)
4 \(\mathrm{F}\)
Explanation:
Lithium being alkali metal, it has lowest \(1^{\text {st }}\) I.E. among given Order of \(1^{\text {st }}\) IP \(\mathrm{F}>\mathrm{O}>\mathrm{C}>\mathrm{Li}\)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313344
The correct order in which the first ionization potentital increases is
1 K, Be, Na
2 Be, Na, K
3 Na, K, Be
4 K, Na, Be
Explanation:
The electronic configuration of the elements are \(_{\rm{4}}{\rm{Be - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{;}}\,{\,_{{\rm{11}}}}{\rm{Na - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{1}}}\) \(_{{\rm{19}}}{\rm{K - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{4}}{{\rm{s}}^{\rm{1}}}\) The first ionization energy of Be is maximum because electron is to be drawn from stable (fully filled) orbital. The \({{\rm{1}}^{{\rm{st}}}}\) ionization energy of Na is greater than K because size of the K is bigger than Na which facilitates easy removal of electron from its outermost shell. So, the sequence is K < Na < Be.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313340
Which of the following metals require radiation of highest frequency to cause emission of electrons?
1 Na
2 Mg
3 K
4 Ca
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313341
Statement A : Second ionization enthalpy will be higher than the first ionization enthalpy. Statement B : Ionization enthalpy is a quantitative measure of the tendency of an element to lose electron.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
It is difficult to remove an electron frrom a positively charged ion than a neutral atom due to which \({\rm{I}}{{\rm{E}}_{\rm{2}}}{\rm{ > I}}{{\rm{E}}_{\rm{1}}}{\rm{.}}\) So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313342
Which of the following has the lowest ionisation enthalpy?
1 \({\rm{4}}{{\rm{s}}^{\rm{1}}}\)
2 \({\rm{3}}{{\rm{d}}^{\rm{2}}}\)
3 \({\rm{3}}{{\rm{p}}^{\rm{6}}}\)
4 \({\rm{2}}{{\rm{p}}^{\rm{6}}}\)
Explanation:
\({\rm{4}}{{\rm{s}}^{\rm{1}}}\) is a s-block element.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313343
Which of the following has lowest \(1^{\text {st }}\) ionisation energy?
1 \(\mathrm{Li}\)
2 \(\mathrm{C}\)
3 \(\mathrm{O}\)
4 \(\mathrm{F}\)
Explanation:
Lithium being alkali metal, it has lowest \(1^{\text {st }}\) I.E. among given Order of \(1^{\text {st }}\) IP \(\mathrm{F}>\mathrm{O}>\mathrm{C}>\mathrm{Li}\)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313344
The correct order in which the first ionization potentital increases is
1 K, Be, Na
2 Be, Na, K
3 Na, K, Be
4 K, Na, Be
Explanation:
The electronic configuration of the elements are \(_{\rm{4}}{\rm{Be - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{;}}\,{\,_{{\rm{11}}}}{\rm{Na - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{1}}}\) \(_{{\rm{19}}}{\rm{K - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{4}}{{\rm{s}}^{\rm{1}}}\) The first ionization energy of Be is maximum because electron is to be drawn from stable (fully filled) orbital. The \({{\rm{1}}^{{\rm{st}}}}\) ionization energy of Na is greater than K because size of the K is bigger than Na which facilitates easy removal of electron from its outermost shell. So, the sequence is K < Na < Be.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313340
Which of the following metals require radiation of highest frequency to cause emission of electrons?
1 Na
2 Mg
3 K
4 Ca
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313341
Statement A : Second ionization enthalpy will be higher than the first ionization enthalpy. Statement B : Ionization enthalpy is a quantitative measure of the tendency of an element to lose electron.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
It is difficult to remove an electron frrom a positively charged ion than a neutral atom due to which \({\rm{I}}{{\rm{E}}_{\rm{2}}}{\rm{ > I}}{{\rm{E}}_{\rm{1}}}{\rm{.}}\) So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313342
Which of the following has the lowest ionisation enthalpy?
1 \({\rm{4}}{{\rm{s}}^{\rm{1}}}\)
2 \({\rm{3}}{{\rm{d}}^{\rm{2}}}\)
3 \({\rm{3}}{{\rm{p}}^{\rm{6}}}\)
4 \({\rm{2}}{{\rm{p}}^{\rm{6}}}\)
Explanation:
\({\rm{4}}{{\rm{s}}^{\rm{1}}}\) is a s-block element.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313343
Which of the following has lowest \(1^{\text {st }}\) ionisation energy?
1 \(\mathrm{Li}\)
2 \(\mathrm{C}\)
3 \(\mathrm{O}\)
4 \(\mathrm{F}\)
Explanation:
Lithium being alkali metal, it has lowest \(1^{\text {st }}\) I.E. among given Order of \(1^{\text {st }}\) IP \(\mathrm{F}>\mathrm{O}>\mathrm{C}>\mathrm{Li}\)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313344
The correct order in which the first ionization potentital increases is
1 K, Be, Na
2 Be, Na, K
3 Na, K, Be
4 K, Na, Be
Explanation:
The electronic configuration of the elements are \(_{\rm{4}}{\rm{Be - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{;}}\,{\,_{{\rm{11}}}}{\rm{Na - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{1}}}\) \(_{{\rm{19}}}{\rm{K - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{4}}{{\rm{s}}^{\rm{1}}}\) The first ionization energy of Be is maximum because electron is to be drawn from stable (fully filled) orbital. The \({{\rm{1}}^{{\rm{st}}}}\) ionization energy of Na is greater than K because size of the K is bigger than Na which facilitates easy removal of electron from its outermost shell. So, the sequence is K < Na < Be.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313340
Which of the following metals require radiation of highest frequency to cause emission of electrons?
1 Na
2 Mg
3 K
4 Ca
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313341
Statement A : Second ionization enthalpy will be higher than the first ionization enthalpy. Statement B : Ionization enthalpy is a quantitative measure of the tendency of an element to lose electron.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
It is difficult to remove an electron frrom a positively charged ion than a neutral atom due to which \({\rm{I}}{{\rm{E}}_{\rm{2}}}{\rm{ > I}}{{\rm{E}}_{\rm{1}}}{\rm{.}}\) So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313342
Which of the following has the lowest ionisation enthalpy?
1 \({\rm{4}}{{\rm{s}}^{\rm{1}}}\)
2 \({\rm{3}}{{\rm{d}}^{\rm{2}}}\)
3 \({\rm{3}}{{\rm{p}}^{\rm{6}}}\)
4 \({\rm{2}}{{\rm{p}}^{\rm{6}}}\)
Explanation:
\({\rm{4}}{{\rm{s}}^{\rm{1}}}\) is a s-block element.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313343
Which of the following has lowest \(1^{\text {st }}\) ionisation energy?
1 \(\mathrm{Li}\)
2 \(\mathrm{C}\)
3 \(\mathrm{O}\)
4 \(\mathrm{F}\)
Explanation:
Lithium being alkali metal, it has lowest \(1^{\text {st }}\) I.E. among given Order of \(1^{\text {st }}\) IP \(\mathrm{F}>\mathrm{O}>\mathrm{C}>\mathrm{Li}\)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313344
The correct order in which the first ionization potentital increases is
1 K, Be, Na
2 Be, Na, K
3 Na, K, Be
4 K, Na, Be
Explanation:
The electronic configuration of the elements are \(_{\rm{4}}{\rm{Be - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{;}}\,{\,_{{\rm{11}}}}{\rm{Na - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{1}}}\) \(_{{\rm{19}}}{\rm{K - 1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{4}}{{\rm{s}}^{\rm{1}}}\) The first ionization energy of Be is maximum because electron is to be drawn from stable (fully filled) orbital. The \({{\rm{1}}^{{\rm{st}}}}\) ionization energy of Na is greater than K because size of the K is bigger than Na which facilitates easy removal of electron from its outermost shell. So, the sequence is K < Na < Be.
