Which atom on the periodic table would require the most energy to take its electron

1 answer:

5 0

An atom on the period table that requires a relatively substantial amount of energy to remove an electron from its outer shell, and thus a high ionization energy would be Fluorine. Due to its small atomic size, and less electron shells, it has a stronger attraction to electrons in its electron shells and thus it is harder to remove the electron from it.

I believe this would be the solution.

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9 Cardiac disease is a major problem in the United States."

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Answer:

D It affects the heart

Explanation:

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3 years ago

Hydrogen reacts with chlorine to form hydrogen chloride (HCl (g), mc012-1.jpgHf = –92.3 kJ/mol) according to the reaction below.

Kobotan [32]

Given:

H2(g) + Cl2 (g) → 2HCl (g)

To determine:

The enthalpy of the reaction and whether it is endo or exothermic

Explanation:

Enthalpy of a reaction is given by the difference between the enthalpy of formation of reactants and products

ΔH = ∑nHf (products) - ∑nHf (reactants)

= [2Hf(HCl)] - [Hf(H2) + Hf(Cl2)] = 2 (-92.3) kJ = - 184.6 kJ

Since the reaction enthalpy is negative, the reaction is exothermic

Ans: The enthalpy of reaction is -184. kJ and the reaction is exothermic

3 0

3 years ago

Read 2 more answers

Asap please

MissTica

Answer:

When $\Delta H^o < 0$ and $\Delta S^o > 0$

Explanation:

The spontaneity of a reaction can be determined by the sign of the Gibbs free energy change. For a spontaneous reaction, the change in Gibbs free energy should be negative, meaning:

$\Delta G^o = \Delta H^o - T\Delta S^o < 0$

Since the temperature value here corresponds to the absolute temperature, this implies that T > 0 for any T. Therefore, to have a negative difference for any temperature value, the first term, the change in enthalpy, should be negative and the change in entropy should be positive, so that we always subtract a positive number from a negative number. This corresponds to a negative value in $\Delta G^o$ .