QBManager

Classification of Elements and Periodicity in Properties

89530 Bond between $A$ and $B$ can $b$ represented by :
$A - B, A^{+} B^{-}, A^{-} B^{+}$
(I) (II) (III)
If $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from:

1 I

2 II

3 III

4 All the structures have equal contribution

Explanation:

A polar covalent bond is formed between the two element of different electronegativities. The polarity of a bond depends on the electronegativity difference.
Hence, the $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from the II.

Manipal-2019

Classification of Elements and Periodicity in Properties

89540 The electro-negativity difference between $N$ and $F$ is greater than that between $N$ and $H$ yet the dipole moment of ${NH}_{3} (1.5 D)$ is larger than that of ${NF}_{3} (0.2 D)$ . This is because

1 in

{NH}_{3}

the atomic dipole and bond dipole are in the opposite directions whereas in

{NF}_{3}

these are in the same direction

2 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in the same direction

3 in

{NH}_{3}

the atomic dipole and bond dipole are in the same direction whereas in

{NF}_{3}

these are in opposite directions

4 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in opposite directions.

Explanation:

Electronegativity of $N$ is greater than that of $H$ but in ${NF}_{3}$ electronegativity of $F$ is greater than that of $N$ . So, in ${NH}_{3}$ the atomic dipole and bond-dipole are in the same direction whereas in ${NF}_{3}$ these are in opposite direction.

NEET-2006

Classification of Elements and Periodicity in Properties

89543 Which carbon is more electronegative?

1

{sp}^{3}

-hybridized carbon

2 sp-hybridized carbon

3

{sp}^{2}

-hybridized carbon

4 Always same irrespective of its hybrid state

5 None of the above

Explanation:

Electronegativity is defined as the relative tendency of an atom or species to attract towards it and we know that attract the electron, positive charge is required that comes from the nucleus.
In sp hybridized carbon two orbitals are involved in hybridization among only one is $s$ . The percentage of $s -$ character it will be equal to $50 %$ . For ${sp}^{2}$ hybridised the percentage of s-character will be $33.3 %$ and for ${sp}^{3}$ hybridised the percentage of s-character will be $25 %$ . Hence, the sp-hybridsed carbon is more electronegative.

Kerala-CEE-2004

Classification of Elements and Periodicity in Properties

89545 Which one of the following is most basic?

1

{Cl}^{-}

2

F^{-}

3

I^{-}

4

{Br}^{-}

AMU 2002

Classification of Elements and Periodicity in Properties

89546 In $X - H$ .......... $Y, X$ and $Y$ both are electronegative elements. Then

1 electron density on

X

will increase and on

H

will decrease

2 in both electron density will increase

3 in both electron density will decrease

4 on

X

electron density will decrease and on

H

increases

Explanation:

For $X - H$ ----- $Y$ , ' $H$ ' is directly bonded to ' $X$ ' and there is a hydrogen, bond between ' $H$ ' and ' $Y$ ' As ' $X$ ' and ' $Y$ ' are electronegative active element that pull electron density towards themselves.
Therefore, the electron density on $X$ increases on ' $H$ ' electron density decreases.

NEET-2001

Classification of Elements and Periodicity in Properties

89530 Bond between $A$ and $B$ can $b$ represented by :
$A - B, A^{+} B^{-}, A^{-} B^{+}$
(I) (II) (III)
If $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from:

1 I

2 II

3 III

4 All the structures have equal contribution

Explanation:

A polar covalent bond is formed between the two element of different electronegativities. The polarity of a bond depends on the electronegativity difference.
Hence, the $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from the II.

Manipal-2019

Classification of Elements and Periodicity in Properties

89540 The electro-negativity difference between $N$ and $F$ is greater than that between $N$ and $H$ yet the dipole moment of ${NH}_{3} (1.5 D)$ is larger than that of ${NF}_{3} (0.2 D)$ . This is because

1 in

{NH}_{3}

the atomic dipole and bond dipole are in the opposite directions whereas in

{NF}_{3}

these are in the same direction

2 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in the same direction

3 in

{NH}_{3}

the atomic dipole and bond dipole are in the same direction whereas in

{NF}_{3}

these are in opposite directions

4 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in opposite directions.

Explanation:

Electronegativity of $N$ is greater than that of $H$ but in ${NF}_{3}$ electronegativity of $F$ is greater than that of $N$ . So, in ${NH}_{3}$ the atomic dipole and bond-dipole are in the same direction whereas in ${NF}_{3}$ these are in opposite direction.

NEET-2006

Classification of Elements and Periodicity in Properties

89543 Which carbon is more electronegative?

1

{sp}^{3}

-hybridized carbon

2 sp-hybridized carbon

3

{sp}^{2}

-hybridized carbon

4 Always same irrespective of its hybrid state

5 None of the above

Explanation:

Electronegativity is defined as the relative tendency of an atom or species to attract towards it and we know that attract the electron, positive charge is required that comes from the nucleus.
In sp hybridized carbon two orbitals are involved in hybridization among only one is $s$ . The percentage of $s -$ character it will be equal to $50 %$ . For ${sp}^{2}$ hybridised the percentage of s-character will be $33.3 %$ and for ${sp}^{3}$ hybridised the percentage of s-character will be $25 %$ . Hence, the sp-hybridsed carbon is more electronegative.

Kerala-CEE-2004

Classification of Elements and Periodicity in Properties

89545 Which one of the following is most basic?

1

{Cl}^{-}

2

F^{-}

3

I^{-}

4

{Br}^{-}

AMU 2002

Classification of Elements and Periodicity in Properties

89546 In $X - H$ .......... $Y, X$ and $Y$ both are electronegative elements. Then

1 electron density on

X

will increase and on

H

will decrease

2 in both electron density will increase

3 in both electron density will decrease

4 on

X

electron density will decrease and on

H

increases

Explanation:

For $X - H$ ----- $Y$ , ' $H$ ' is directly bonded to ' $X$ ' and there is a hydrogen, bond between ' $H$ ' and ' $Y$ ' As ' $X$ ' and ' $Y$ ' are electronegative active element that pull electron density towards themselves.
Therefore, the electron density on $X$ increases on ' $H$ ' electron density decreases.

NEET-2001

Classification of Elements and Periodicity in Properties

89530 Bond between $A$ and $B$ can $b$ represented by :
$A - B, A^{+} B^{-}, A^{-} B^{+}$
(I) (II) (III)
If $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from:

1 I

2 II

3 III

4 All the structures have equal contribution

Explanation:

A polar covalent bond is formed between the two element of different electronegativities. The polarity of a bond depends on the electronegativity difference.
Hence, the $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from the II.

Manipal-2019

Classification of Elements and Periodicity in Properties

89540 The electro-negativity difference between $N$ and $F$ is greater than that between $N$ and $H$ yet the dipole moment of ${NH}_{3} (1.5 D)$ is larger than that of ${NF}_{3} (0.2 D)$ . This is because

1 in

{NH}_{3}

the atomic dipole and bond dipole are in the opposite directions whereas in

{NF}_{3}

these are in the same direction

2 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in the same direction

3 in

{NH}_{3}

the atomic dipole and bond dipole are in the same direction whereas in

{NF}_{3}

these are in opposite directions

4 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in opposite directions.

Explanation:

Electronegativity of $N$ is greater than that of $H$ but in ${NF}_{3}$ electronegativity of $F$ is greater than that of $N$ . So, in ${NH}_{3}$ the atomic dipole and bond-dipole are in the same direction whereas in ${NF}_{3}$ these are in opposite direction.

NEET-2006

Classification of Elements and Periodicity in Properties

89543 Which carbon is more electronegative?

1

{sp}^{3}

-hybridized carbon

2 sp-hybridized carbon

3

{sp}^{2}

-hybridized carbon

4 Always same irrespective of its hybrid state

5 None of the above

Explanation:

Electronegativity is defined as the relative tendency of an atom or species to attract towards it and we know that attract the electron, positive charge is required that comes from the nucleus.
In sp hybridized carbon two orbitals are involved in hybridization among only one is $s$ . The percentage of $s -$ character it will be equal to $50 %$ . For ${sp}^{2}$ hybridised the percentage of s-character will be $33.3 %$ and for ${sp}^{3}$ hybridised the percentage of s-character will be $25 %$ . Hence, the sp-hybridsed carbon is more electronegative.

Kerala-CEE-2004

Classification of Elements and Periodicity in Properties

89545 Which one of the following is most basic?

1

{Cl}^{-}

2

F^{-}

3

I^{-}

4

{Br}^{-}

AMU 2002

Classification of Elements and Periodicity in Properties

89546 In $X - H$ .......... $Y, X$ and $Y$ both are electronegative elements. Then

1 electron density on

X

will increase and on

H

will decrease

2 in both electron density will increase

3 in both electron density will decrease

4 on

X

electron density will decrease and on

H

increases

Explanation:

For $X - H$ ----- $Y$ , ' $H$ ' is directly bonded to ' $X$ ' and there is a hydrogen, bond between ' $H$ ' and ' $Y$ ' As ' $X$ ' and ' $Y$ ' are electronegative active element that pull electron density towards themselves.
Therefore, the electron density on $X$ increases on ' $H$ ' electron density decreases.

NEET-2001

Classification of Elements and Periodicity in Properties

89530 Bond between $A$ and $B$ can $b$ represented by :
$A - B, A^{+} B^{-}, A^{-} B^{+}$
(I) (II) (III)
If $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from:

1 I

2 II

3 III

4 All the structures have equal contribution

Explanation:

A polar covalent bond is formed between the two element of different electronegativities. The polarity of a bond depends on the electronegativity difference.
Hence, the $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from the II.

Manipal-2019

Classification of Elements and Periodicity in Properties

89540 The electro-negativity difference between $N$ and $F$ is greater than that between $N$ and $H$ yet the dipole moment of ${NH}_{3} (1.5 D)$ is larger than that of ${NF}_{3} (0.2 D)$ . This is because

1 in

{NH}_{3}

the atomic dipole and bond dipole are in the opposite directions whereas in

{NF}_{3}

these are in the same direction

2 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in the same direction

3 in

{NH}_{3}

the atomic dipole and bond dipole are in the same direction whereas in

{NF}_{3}

these are in opposite directions

4 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in opposite directions.

Explanation:

Electronegativity of $N$ is greater than that of $H$ but in ${NF}_{3}$ electronegativity of $F$ is greater than that of $N$ . So, in ${NH}_{3}$ the atomic dipole and bond-dipole are in the same direction whereas in ${NF}_{3}$ these are in opposite direction.

NEET-2006

Classification of Elements and Periodicity in Properties

89543 Which carbon is more electronegative?

1

{sp}^{3}

-hybridized carbon

2 sp-hybridized carbon

3

{sp}^{2}

-hybridized carbon

4 Always same irrespective of its hybrid state

5 None of the above

Explanation:

Electronegativity is defined as the relative tendency of an atom or species to attract towards it and we know that attract the electron, positive charge is required that comes from the nucleus.
In sp hybridized carbon two orbitals are involved in hybridization among only one is $s$ . The percentage of $s -$ character it will be equal to $50 %$ . For ${sp}^{2}$ hybridised the percentage of s-character will be $33.3 %$ and for ${sp}^{3}$ hybridised the percentage of s-character will be $25 %$ . Hence, the sp-hybridsed carbon is more electronegative.

Kerala-CEE-2004

Classification of Elements and Periodicity in Properties

89545 Which one of the following is most basic?

1

{Cl}^{-}

2

F^{-}

3

I^{-}

4

{Br}^{-}

AMU 2002

Classification of Elements and Periodicity in Properties

89546 In $X - H$ .......... $Y, X$ and $Y$ both are electronegative elements. Then

1 electron density on

X

will increase and on

H

will decrease

2 in both electron density will increase

3 in both electron density will decrease

4 on

X

electron density will decrease and on

H

increases

Explanation:

For $X - H$ ----- $Y$ , ' $H$ ' is directly bonded to ' $X$ ' and there is a hydrogen, bond between ' $H$ ' and ' $Y$ ' As ' $X$ ' and ' $Y$ ' are electronegative active element that pull electron density towards themselves.
Therefore, the electron density on $X$ increases on ' $H$ ' electron density decreases.

NEET-2001

Classification of Elements and Periodicity in Properties

89530 Bond between $A$ and $B$ can $b$ represented by :
$A - B, A^{+} B^{-}, A^{-} B^{+}$
(I) (II) (III)
If $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from:

1 I

2 II

3 III

4 All the structures have equal contribution

Explanation:

A polar covalent bond is formed between the two element of different electronegativities. The polarity of a bond depends on the electronegativity difference.
Hence, the $A$ is more electronegative than $B$ , then least contribution to the actual structure comes from the II.

Manipal-2019

Classification of Elements and Periodicity in Properties

89540 The electro-negativity difference between $N$ and $F$ is greater than that between $N$ and $H$ yet the dipole moment of ${NH}_{3} (1.5 D)$ is larger than that of ${NF}_{3} (0.2 D)$ . This is because

1 in

{NH}_{3}

the atomic dipole and bond dipole are in the opposite directions whereas in

{NF}_{3}

these are in the same direction

2 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in the same direction

3 in

{NH}_{3}

the atomic dipole and bond dipole are in the same direction whereas in

{NF}_{3}

these are in opposite directions

4 in

{NH}_{3}

as well as in

{NF}_{3}

the atomic dipole and bond dipole are in opposite directions.

Explanation:

Electronegativity of $N$ is greater than that of $H$ but in ${NF}_{3}$ electronegativity of $F$ is greater than that of $N$ . So, in ${NH}_{3}$ the atomic dipole and bond-dipole are in the same direction whereas in ${NF}_{3}$ these are in opposite direction.

NEET-2006

Classification of Elements and Periodicity in Properties

89543 Which carbon is more electronegative?

1

{sp}^{3}

-hybridized carbon

2 sp-hybridized carbon

3

{sp}^{2}

-hybridized carbon

4 Always same irrespective of its hybrid state

5 None of the above

Explanation:

Electronegativity is defined as the relative tendency of an atom or species to attract towards it and we know that attract the electron, positive charge is required that comes from the nucleus.
In sp hybridized carbon two orbitals are involved in hybridization among only one is $s$ . The percentage of $s -$ character it will be equal to $50 %$ . For ${sp}^{2}$ hybridised the percentage of s-character will be $33.3 %$ and for ${sp}^{3}$ hybridised the percentage of s-character will be $25 %$ . Hence, the sp-hybridsed carbon is more electronegative.

Kerala-CEE-2004

Classification of Elements and Periodicity in Properties

89545 Which one of the following is most basic?

1

{Cl}^{-}

2

F^{-}

3

I^{-}

4

{Br}^{-}

AMU 2002

Classification of Elements and Periodicity in Properties

89546 In $X - H$ .......... $Y, X$ and $Y$ both are electronegative elements. Then

1 electron density on

X

will increase and on

H

will decrease

2 in both electron density will increase

3 in both electron density will decrease

4 on

X

electron density will decrease and on

H

increases

Explanation:

For $X - H$ ----- $Y$ , ' $H$ ' is directly bonded to ' $X$ ' and there is a hydrogen, bond between ' $H$ ' and ' $Y$ ' As ' $X$ ' and ' $Y$ ' are electronegative active element that pull electron density towards themselves.
Therefore, the electron density on $X$ increases on ' $H$ ' electron density decreases.

NEET-2001