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postnew [5]
2 years ago
14

Which type of bond does the phrase “opposites attract” apply to best? Explain.​

Chemistry
2 answers:
forsale [732]2 years ago
5 0

Answer:

The phrase "opposites attract" is true for atoms. The positively charged ion (cation) and the negatively charged ion (anion) are attracted to each other. It is this attraction, created by the transfer of electrons, that forms the ionic bond. The transfer of one electron creates a single bond.

Explanation:The phrase "opposites attract" is true for atoms. The positively charged ion (cation) and the negatively charged ion (anion) are attracted to each other. It is this attraction, created by the transfer of electrons, that forms the ionic bond. The transfer of one electron creates a single bond.

RideAnS [48]2 years ago
4 0

Answer:

phrase opposites attract definitely describes ionic bond because this is the only type of bonds that requires positive charge in one atom and negative charge in other atom to form an ionic compound. HOPE THIS ANSWER YOUR QUESTION!!!

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<u>Explanation:</u>

Bromothymol blue, Bromocresol green and Thymol blue are the indicators which change their color according to the change in pH of the solution.

The pH range and color change of these indicators are:

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As, the highest pH of all the indicators is 9.6, so every indicator will appear blue above pH 9.6.

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The equilibrium constant of a reaction does not depend on the pressure. For this particular reaction, the equilibrium quotient is:

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Note that the two sides of this balanced equation contain an equal number of gaseous particles. Indeed, both [\mathrm{SO_2\, (g)}] and [\mathrm{O_2\, (g)}] will increase if the pressure is increased through compression. However, because \rm SO_2\, (g) and \rm O_2\, (g) have the same coefficients in the equation, their concentrations are raised to the same power in the equilibrium quotient Q.

As a result, the increase in pressure will have no impact on the value of Q\!. If the system was already at equilibrium, it will continue to be at an equilibrium even after the change to its pressure. Therefore, no overall effect on the equilibrium position should be visible.

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