When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to f

step 1 Here we are continuing to look at bonding, and so we're looking at a reaction that forms a singl

When atoms of the hypothetical element X are placed...

When atoms of the hypothetical element $\mathrm{X}$ are placed together, they rapidly undergo reaction to form the $\mathrm{X}_{2}$ molecule: $\mathrm{X}(g)+\mathrm{X}(g) \longrightarrow \mathrm{X}_{2}(g)$ A. Would you predict that this reaction is exothermic or endothermic? Explain. Is the bond enthalpy of $\mathrm{X}_{2}$ a positive or a negative B. Is the bond enthalpy of $\mathrm{X}_{2}$ a positive or a negative quantity? Why? C. Suppose $\Delta H$ for the reaction is $-500 \mathrm{~kJ} / \mathrm{mol}$. Estimate the bond enthalpy of the $\mathrm{X}_{2}$ molecule. D. Another hypothetical molecular compound, $\mathrm{Y}_{2}(g)$ has a bond enthalpy of $750 \mathrm{~kJ} / \mathrm{mol}$, and the molecular compound $\mathrm{XY}(g)$ has a bond enthalpy of $1500 \mathrm{~kJ} / \mathrm{mol}$. Using bond enthalpy information, calculate $\Delta H$ for the following reaction. $$\mathrm{X}_{2}(g)+\mathrm{Y}_{2}(g) \longrightarrow 2 \mathrm{XY}(g)$$ E, Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound $\mathrm{AX}$ is likely to form. In this compound, A forms the $\mathrm{A}^{+}$ cation, and $\mathrm{X}$ forms the $\mathrm{X}^{-}$ anion. Be sure to justify your answer. Reaction: $\mathrm{A}(g)+\frac{1}{2} \mathrm{X}_{2}(g) \longrightarrow \mathrm{AX}(s)$ The first ionization energy of $\mathrm{A}(g)$ is $400 \mathrm{~kJ} / \mathrm{mol}$. The electron affinity of $\mathrm{X}(g)$ is $525 \mathrm{~kJ} / \mathrm{mol}$. The lattice energy of $\mathrm{AX}(s)$ is $100 \mathrm{~kJ} / \mathrm{mol}$. F. If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of $\mathrm{AX}(s)$ lattice energy might lead to compound formation?

When atoms of the hypothetical element $\mathrm{X}$ are placed together, they rapidly undergo reaction to form the $\mathrm{X}_{2}$ molecule:
$\mathrm{X}(g)+\mathrm{X}(g) \longrightarrow \mathrm{X}_{2}(g)$
A. Would you predict that this reaction is exothermic or endothermic? Explain.
Is the bond enthalpy of $\mathrm{X}_{2}$ a positive or a negative
B. Is the bond enthalpy of $\mathrm{X}_{2}$ a positive or a negative quantity? Why?
C. Suppose $\Delta H$ for the reaction is $-500 \mathrm{~kJ} / \mathrm{mol}$. Estimate the bond enthalpy of the $\mathrm{X}_{2}$ molecule.
D. Another hypothetical molecular compound, $\mathrm{Y}_{2}(g)$ has a bond enthalpy of $750 \mathrm{~kJ} / \mathrm{mol}$, and the molecular compound $\mathrm{XY}(g)$ has a bond enthalpy of $1500 \mathrm{~kJ} / \mathrm{mol}$. Using bond enthalpy information, calculate $\Delta H$ for the following reaction.
$$\mathrm{X}_{2}(g)+\mathrm{Y}_{2}(g) \longrightarrow 2 \mathrm{XY}(g)$$
E, Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound $\mathrm{AX}$ is likely to form. In this compound, A forms the $\mathrm{A}^{+}$ cation, and $\mathrm{X}$ forms the $\mathrm{X}^{-}$ anion. Be sure to justify your answer. Reaction: $\mathrm{A}(g)+\frac{1}{2} \mathrm{X}_{2}(g) \longrightarrow \mathrm{AX}(s)$
The first ionization energy of $\mathrm{A}(g)$ is $400 \mathrm{~kJ} / \mathrm{mol}$. The electron affinity of $\mathrm{X}(g)$ is $525 \mathrm{~kJ} / \mathrm{mol}$. The lattice energy of $\mathrm{AX}(s)$ is $100 \mathrm{~kJ} / \mathrm{mol}$.
F. If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of $\mathrm{AX}(s)$ lattice energy might lead to compound formation?

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