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CHXI02:STRUCTURE OF ATOM

307449 What is the maximum number of electrons that can be associated with a following set of quantum numbers?
$(n = 3, l = 1 a n d m = - 1)$

1

2

2

4

3

6

4

10

Explanation:

$(n = 3, l = 1$ is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital $(m = - 1)$
$n = 5, l = 0, m = 0, s = + \frac{1}{2}$ or $- \frac{1}{2}$

CHXI02:STRUCTURE OF ATOM

307450 The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is

1

14

2

7

3

5

4

10

CHXI02:STRUCTURE OF ATOM

307468 Which one of the following set of quantum numbers is not possible for 4p electron?

1

n = 4, l = 1, m = - 1, m_{s} = + \frac{1}{2}

2

n = 4, l = 1, m = 0, m_{s} = + \frac{1}{2}

3

n = 4, l = 1, m = 2, m_{s} = + \frac{1}{2}

4

n = 4, l = 1, m = - 1, m_{s} = - \frac{1}{2}

CHXI02:STRUCTURE OF ATOM

307451 What is the correct orbital designation of an electron with the quantum number, $n = 4, l = 3, m = - 2, s = 1 / 2$ ?

1

3 s

2

4 f

3

5 p

4

6 s

Explanation:

$n = 4$ represents $4^{t h}$ orbit
$l = 3$ represents f subshell
$m = - 2$ represents orientation of f-orbital
$s = 1 / 2$ represents direction of spin of electron.
$∴$ The orbital is $4 f .$

CHXI02:STRUCTURE OF ATOM

307449 What is the maximum number of electrons that can be associated with a following set of quantum numbers?
$(n = 3, l = 1 a n d m = - 1)$

1

2

2

4

3

6

4

10

Explanation:

$(n = 3, l = 1$ is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital $(m = - 1)$
$n = 5, l = 0, m = 0, s = + \frac{1}{2}$ or $- \frac{1}{2}$

CHXI02:STRUCTURE OF ATOM

307450 The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is

1

14

2

7

3

5

4

10

CHXI02:STRUCTURE OF ATOM

307468 Which one of the following set of quantum numbers is not possible for 4p electron?

1

n = 4, l = 1, m = - 1, m_{s} = + \frac{1}{2}

2

n = 4, l = 1, m = 0, m_{s} = + \frac{1}{2}

3

n = 4, l = 1, m = 2, m_{s} = + \frac{1}{2}

4

n = 4, l = 1, m = - 1, m_{s} = - \frac{1}{2}

CHXI02:STRUCTURE OF ATOM

307451 What is the correct orbital designation of an electron with the quantum number, $n = 4, l = 3, m = - 2, s = 1 / 2$ ?

1

3 s

2

4 f

3

5 p

4

6 s

Explanation:

$n = 4$ represents $4^{t h}$ orbit
$l = 3$ represents f subshell
$m = - 2$ represents orientation of f-orbital
$s = 1 / 2$ represents direction of spin of electron.
$∴$ The orbital is $4 f .$

CHXI02:STRUCTURE OF ATOM

307449 What is the maximum number of electrons that can be associated with a following set of quantum numbers?
$(n = 3, l = 1 a n d m = - 1)$

1

2

2

4

3

6

4

10

Explanation:

$(n = 3, l = 1$ is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital $(m = - 1)$
$n = 5, l = 0, m = 0, s = + \frac{1}{2}$ or $- \frac{1}{2}$

CHXI02:STRUCTURE OF ATOM

307450 The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is

1

14

2

7

3

5

4

10

CHXI02:STRUCTURE OF ATOM

307468 Which one of the following set of quantum numbers is not possible for 4p electron?

1

n = 4, l = 1, m = - 1, m_{s} = + \frac{1}{2}

2

n = 4, l = 1, m = 0, m_{s} = + \frac{1}{2}

3

n = 4, l = 1, m = 2, m_{s} = + \frac{1}{2}

4

n = 4, l = 1, m = - 1, m_{s} = - \frac{1}{2}

CHXI02:STRUCTURE OF ATOM

307451 What is the correct orbital designation of an electron with the quantum number, $n = 4, l = 3, m = - 2, s = 1 / 2$ ?

1

3 s

2

4 f

3

5 p

4

6 s

Explanation:

$n = 4$ represents $4^{t h}$ orbit
$l = 3$ represents f subshell
$m = - 2$ represents orientation of f-orbital
$s = 1 / 2$ represents direction of spin of electron.
$∴$ The orbital is $4 f .$

CHXI02:STRUCTURE OF ATOM

307449 What is the maximum number of electrons that can be associated with a following set of quantum numbers?
$(n = 3, l = 1 a n d m = - 1)$

1

2

2

4

3

6

4

10

Explanation:

$(n = 3, l = 1$ is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital $(m = - 1)$
$n = 5, l = 0, m = 0, s = + \frac{1}{2}$ or $- \frac{1}{2}$

CHXI02:STRUCTURE OF ATOM

307450 The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is

1

14

2

7

3

5

4

10

CHXI02:STRUCTURE OF ATOM

307468 Which one of the following set of quantum numbers is not possible for 4p electron?

1

n = 4, l = 1, m = - 1, m_{s} = + \frac{1}{2}

2

n = 4, l = 1, m = 0, m_{s} = + \frac{1}{2}

3

n = 4, l = 1, m = 2, m_{s} = + \frac{1}{2}

4

n = 4, l = 1, m = - 1, m_{s} = - \frac{1}{2}

CHXI02:STRUCTURE OF ATOM

307451 What is the correct orbital designation of an electron with the quantum number, $n = 4, l = 3, m = - 2, s = 1 / 2$ ?

1

3 s

2

4 f

3

5 p

4

6 s

Explanation:

$n = 4$ represents $4^{t h}$ orbit
$l = 3$ represents f subshell
$m = - 2$ represents orientation of f-orbital
$s = 1 / 2$ represents direction of spin of electron.
$∴$ The orbital is $4 f .$

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