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3 years ago

How many electrons does a single hydrogen gain or lose in the following reaction? H 2 + O 2 → H 2 O

Chemistry

2 answers:

True [87]3 years ago

4 0

Answer:

Lose 1

Explanation:

Answer via Educere/ Founder's Education

wariber [46]3 years ago

3 0

Answer:

option B. Lose 1.

Explanation:

To determine the number of electrons that a single hydrogen gains or loses you need to realize that the chemical reaction is an oxidation-reduction (redox) reaction and state the changes in the oxidation states.

The substance that gains electrons is being reduced, reducing its oxidation number, and the substance that lose electrons is being oxidized, increasing its oxidation state.

1) State the oxidation state of hydrogen atoms in the rectant side:

H₂: the oxidation state of any element in its atomic or molecular form is zero. That is indicated as a superscript to the right of the chemical symbol: H₂⁰

2) State the oxidation state of the hydrogen atoms in the product side:

H₂O: the rule says that the oxidation state of oxygen, when combined with other elements, except in the case of peroxides, is -2.

Hence, in order to the molecule H₂O be neutral, the total charge contributed by the two atoms of hydrogen must be + 2: +2 - 2 = 0.

Since there are two hydrogen atoms, each contributes +2 / 2 = +1 charge.

3) Conclusion:

Every atom of hydrogen changes from a 0 oxidation number to a +1 oxidation number, which, in turn, means that every hydrogen atom loses one electron.

Thus, the answer is, the option B. Lose 1.

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3 years ago

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A sample of calcium phosphate was found to have a mass of 125.3 g. How many molecules were contained in the sample?

Viktor [21]

The answer for the following problem is mentioned below.

Therefore number of molecules(N) present in the calcium phosphate sample are 19.3 × 10^23 molecules.

Explanation:

Given:

mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = 125.3 grams

We know;

molar mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = (40×3) + 3 (31 +(4×16))

molar mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = 120 + 3(95)

molar mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = 120 +285 = 405 grams

We also know;

No of molecules at STP conditions( $N_{A}$ ) = 6.023 × 10^23 molecules

To solve:

no of molecules present in the sample(N)

We know;

$\frac{m}{M} =\frac{N} }{}$ N÷ $N_{A}$

$\frac{405}{125.3}$ = $\frac{N}{6.023*10^23}$

N =(405×6.023 × 10^23) ÷ 125.3

N = 19.3 × 10^23 molecules

Therefore number of molecules(N) present in the calcium phosphate sample are 19.3 × 10^23 molecules

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3 years ago

What is the nature of the Ca-Cl bond in a molecule of calcium chloride (CaCl2) if the electronegativity value of calcium is 1.0

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3 years ago

A glass blower can bend and shape a piece of glass that has been heated. Is glass a crystalline or an amorphous solid?

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3 years ago

In an experiment, students were given an unknown mineral. The unknown mineral was placed in 150 ml of water. Once in the water,

Dahasolnce [82]

Answer:

Explanation:

The density of a substance can be found by using the formula

$density = \frac{mass}{volume} \\$

But from the question

volume = final volume of water - initial volume of water

volume = 165 - 150 = 15 mL

We have

$density = \frac{225}{15} = 15 \\$

We have the final answer as

Hope this helps you

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2 years ago