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Morgarella [4.7K]
3 years ago
6

Use lewis structures to explain why br3- and i3- are stable, while f3- is not

Chemistry
1 answer:
MAXImum [283]3 years ago
4 0

If you sketch a Lewis dot structure of I3-, you'll perceive that the center I atom formulates two bonds, and also has three non-bonding pairs of electrons. That's an over-all of five electron pairs - beyond an octet. Lots of compounds disrupt the octet rule that means, but the first long-row elements like F can't because the lower elements like iodine can use an obtainable d-orbital to house the additional pair of electrons (sp3d hybridization), but F just doesn't have a d-orbital that it can use.

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When 2.499 g of AX (s) dissolves in 135.3 g of water in a coffee-cup calorimeter the temperature rises from 23.6 °C to 35.2 °C.
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Answer:

The enthalpy change for the solution process \Delta H_{rxn} = - 158.34 kJ/mol

Explanation:

Given that:

The mass of salt AX = 2.499 g

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The specific heat of salt solution s is known to be = 4.18 J/g° C

The change in temperature i.e. ΔT = 35.2 °C -  23.6 °C = 11.6 °C

Thus, the amount of heat raised is equal to the heat absorbed by the calorimeter.

∴

q_{reaction} = q_{solution}

q_{reaction} = -ms_{solution} \Delta T

q_{reaction} = -137.799 \ g \times 4.18 \dfrac{J}{g^0C}\times 11.6^0C

q_{reaction} = - 6682 \ J

q_{reaction} = - 6.682 \ kJ

Recall that the mass of the salt = 2.499 g

The number of moles of the salt = 2.499 \ g \times \dfrac{1 \ mol  \ of  \ AX}{59.1097 \ g}

= 0.0422 mol of AX

Finally the enthalpy change, \Delta H_{rxn} =  \dfrac{- 6.682 \ kJ}{ 0.0422 \ mol}

= - 158.34 kJ/mol

The enthalpy change for the solution process \Delta H_{rxn} = - 158.34 kJ/mol

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