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Kazeer [188]
1 year ago
12

Two bidentate ligands used extensively in analytical chemistry are bipyridyl (bipy) and ortho-phenanthroline (o-phen):Draw struc

tures and discuss the possibility of isomers for(c) [Co(bipy)₂F₂]⁺
Chemistry
1 answer:
user100 [1]1 year ago
7 0

Isomers are compounds that contain exactly the same number of atoms, i.e., they have exactly the same empirical formula, but differ from each other by the way in which the atoms are arranged.

<h3>How do you identify isomers?</h3>

You can tell them apart by their bonding patterns and how they take up three-dimensional space. Identify structural (constitutional) isomers by their bonding patterns. The atoms of the compounds are the same but they are connected in such a way as to make different functional groups.

<h3>How isomers are formed?</h3>

Two main forms of isomerism are structural or constitutional isomerism, in which bonds between the atoms differ; and stereoisomerism or spatial isomerism, in which the bonds are the same but the relative positions of the atoms differ.

Learn more about isomers here:

<h3>brainly.com/question/18474884</h3><h3 /><h3>#SPJ4</h3>
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a chemist dissolves 0.564 moles of manganese (IV) oxide (MnO2) in water, and adds enough water to make 0.510 L of solution. Calc
ladessa [460]

Answer:

The molarity of the solution is 1.1 \frac{moles}{liter}

Explanation:

Molarity is a measure of the concentration of that substance that is defined as the number of moles of solute divided by the volume of the solution.

The molarity of a solution is calculated by dividing the moles of the solute by the volume of the solution:

molarity=\frac{number of moles of solute}{volume}

Molarity is expressed in units \frac{moles}{liter}

In this case

  • number of moles of solute= 0.564 moles
  • volume= 0.510 L

Replacing:

molarity=\frac{0.564 moles}{0.510 L}

Solving:

molarity= 1.1 \frac{moles}{liter}

<u><em>The molarity of the solution is 1.1 </em></u>\frac{moles}{liter}<u><em></em></u>

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In your own words, please describe the difference between a complete ionic equation and a net ionic equation.
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