The energy required to separate the ions in a CsF crystal lattice into individual Cs^+1 (g) and F^-1 (g) ions is known as the lattice energy of CsF(s). As shown in the table below, the lattice energy of CsF(s) is smaller than the lattice energy of a similar compound, KF(s). Which of the following best explains why the lattice energy of CsF is smaller than the lattice energy of KF? CsF = 759
KF = 829

A.) Cs^+ contains more core electrons than K4+, so the valence electrons in Cs^+ are more shielded from the nucleus than the valence electrons in K+.

B.) Cs^+ has a larger ionic radius than K^+, so the distance between cation and anion is greater in CsF than in KF.

C.) Cesium and fluorine have a greater electronegativity difference than potassium and fluorine, so the Cs-F bond is more polar than the K-F bond.

D.) Cesium has a smaller first ionization energy than potassium, so less energy is required to form the Cs^+ ion than to form the K^+ ion.

thats a little if u want the answer just look it up on google thats what i do haha : )

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answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.