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If bromine atom is available in the form of, say, two isotopes

Science

Class 9

NCERT

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Chapter 3: Atoms and Molecules

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Chapter 4: Structure of the Atom

19 questions

Explain

N a^{+}

has completely filled

K

and

L

shells.

If bromine atom is available in the form of, say, two isotopes

_{35}^{79} B r

(49.7%) and

_{35}^{81} B r

(50.3%), calculate the average atomic mass of bromine atom.

The average atomic mass of a sample of an element

X

16.2 u

. What are the percentages of isotopes

_{8}^{16} X

and

_{8}^{18} X

in the sample?

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29 questions

Question

Medium

Solving time: 4 mins

If bromine atom is available in the form of, say, two isotopes $_{35}^{79} B r$ (49.7%) and $_{35}^{81} B r$ (50.3%), calculate the average atomic mass of bromine atom.

Views: 6,212 students

Updated on: Oct 5, 2023

Book:

Science (NCERT)

Text solutionVerified

The average atomic mass of bromine atom

= (79 \times \frac{49.7}{100}) + (81 \times \frac{50.3}{100}) = 39.263 + 40.743 = 80.006 u

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Michael Discussed

If bromine atom is available in the form of, say, two isotopes

_{35}^{79} B r

(49.7%) and

_{35}^{81} B r

(50.3%), calculate the average atomic mass of bromine atom.

14 mins ago

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14 mins ago

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Practice more questions from Science (NCERT)

Explain

N a^{+}

has completely filled

K

and

L

shells.

If bromine atom is available in the form of, say, two isotopes

_{35}^{79} B r

(49.7%) and

_{35}^{81} B r

(50.3%), calculate the average atomic mass of bromine atom.

The average atomic mass of a sample of an element

X

16.2 u

. What are the percentages of isotopes

_{8}^{16} X

and

_{8}^{18} X

in the sample?

View all

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Question Text	If bromine atom is available in the form of, say, two isotopes $_{35}^{79} B r$ (49.7%) and $_{35}^{81} B r$ (50.3%), calculate the average atomic mass of bromine atom.
Updated On	Oct 5, 2023
Topic	Structure of the Atom
Subject	Science
Class	Class 9
Answer Type	Text solution:1 Video solution: 22
Upvotes	2220
Avg. Video Duration	5 min

If bromine atom is available in the form of, say, two isotopes $_{35}^{79} B r$ (49.7%) and $_{35}^{81} B r$ (50.3%), calculate the average atomic mass of bromine atom.

Text solutionVerified

Video solutions (22)

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Particle	Protons	Neutrons	Electrons
A	17	18	17
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If bromine atom is available in the form of, say, two isotopes 3579​Br (49.7%) and 3581​Br (50.3%), calculate the average atomic mass of bromine atom.

Text solutionVerified

Video solutions (22)

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If bromine atom is available in the form of, say, two isotopes $_{35}^{79} B r$ (49.7%) and $_{35}^{81} B r$ (50.3%), calculate the average atomic mass of bromine atom.