Which of the following pair below represents isotopes of the same element?

_{18}^{39} A

and

_{19}^{39} R

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_{27}^{60} X

and

_{28}^{59} Y

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_{6}^{12} L

and

_{6}^{14} L

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_{17}^{37} X

and

_{17}^{37} X

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_{2}^{3} E

and

_{1}^{3} G

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Solution

The correct option is D $_{6}^{12} L$ and $_{6}^{14} L$
Isotopes are atoms of the same element that contain an identical number of protons, but a different number of neutrons. Thus, isotopes have same atomic number (Z), but different mass number (A). That means, the elements having different atomic numbers (protons) are not isotopes. $_{6}^{12} L$ and $_{6}^{14} L$ are isotopes of same element with $6$ and $8$ neutrons respectively.

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Q. If an element

X

exists in its two isotopic form

_{17}^{35} X (75 %)

and

_{17}^{37} X (25 %)

. The average atomic mass of element

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Question 16
Which of the following are the characteristics of isotopes of an element?

(i) Isotopes of an element have same atomic masses
(ii) Isotopes of an element have same atomic number
(iii) Isotopes of an element show same physical properties
(iv) Isotopes of an element show same chemical properties

(a) (i), (iii) and (iv)
(b) (ii), (iii) and (iv)
(c) (ii) and (iii)
(d) (ii) and (iv)

Q. An element is represented by

_{Z} X^{A}

, where Z is atomic number which is also equal to number of proton, A is mass number and X is symbol of the element.
Mass number (A) = Number of protons (Z) + Number of neutrons.
Isoelectronic: Species/ elements having same number of electron
Isodiaphers: Elements having same value of

| (A - 2 Z) |

Isotopes: Atoms having same number of proton

Which of the following pairs of compounds is both isoelectronic and isotopic?

The symbols given below represents the nuclei of radioactive elements. Which among the following are isotopes?

$_{91}^{230} W$ , $_{92}^{235} X$ , $_{93}^{238} Y$ , $_{92}^{238} Z$

Q. Which of the following pair represents elements of same group?

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