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3 years ago

How do the isotopes hydrogen-1 and hydrogen-2 differ?

Chemistry

2 answers:

g100num [7]3 years ago

4 0

Hydrogen-2 has one neutron; hydrogen-1 has none

galina1969 [7]3 years ago

3 0

Answer: They differ by the number of neutrons

Explanation:

Isotopes are defined as the chemical species which have same number of protons but differ in the number of neutrons.

The general isotopic representation is $_{Z}^A\textrm{X}$

where,

Z = Atomic number of the atom

A = Mass number of the atom

X = Symbol of the atom

Atomic number is defined as the number of protons or electrons that are present in a neutral atom.

Atomic number = number of protons = number of electrons

Mass number is defined as the sum of number of protons and number of neutrons present in an atom.

Mass number = Number of neutrons + Number of protons.

We are given two isotopes:

$_1^1\textrm{H}\text{ and }_1^2\textrm{H}$

For $_1^1\textrm{H}$ isotope:

Number of protons = 1

Mass number = 1

Number of neutrons = 1 - 1 = 0

For $_1^2\textrm{H}$ isotope:

Number of protons = 1

Mass number = 2

Number of neutrons = 2 - 1 = 1

Hence, they differ by the number of neutrons

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There are two binary compounds of mercury and oxygen. heating either of them results in the decomposition of the compound, with

grandymaker [24]

$\text{Hg} \text{O}$ and $\text{Hg}_{2} \text{O}$ .

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$n(\text{O atoms}) = 0.048 \; g / 16 \; g \cdot mol^{-1}= 0.003 \; mol$
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Oxygen and mercury atoms seemingly exist in the first compound at a $1:1$ ratio; thus the empirical formula for this compound would be $\text{Hg} \text{O}$ where the subscript "1" is omitted.

Similarly, for the second compound

$m(\text{O}) = m(\text{loss}) = 0.016 \; g$
$m(\text{Hg}) = m(\text{residure}) = 0.4172 - 0.016 = 0.4012 \; g$

$n = m/M$ ; $0.4172 \; g$ of the first compound would contain

$n(\text{O atoms}) = 0.016 \; g / 16 \; g \cdot mol^{-1}= 0.001 \; mol$
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$n(\text{Hg}) : n(\text{O}) \approx 2:1$ and therefore the empirical formula

$\text{Hg}_{2} \text{O}$ .

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Answer:

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