Which of the following statements is true regarding sodium and chlorine? a.) sodium has greater electronegativity and a larger first ionization energyb.) sodium has a larger first ionization energy and a larger atomic radiusc.) chlorine has a larger atomic radius and greater electronegativityd.) chlorine has greater electronegativity and a larger first ionization energy

D.) Chlorine has greater electronegativity and a larger first ionization energy

Explanation:

first we have to consider where sodium and chlorine are in the atomic table. Both are in the third row and both are nearly opposite ends of third row. sodium have high tendency to lose an electron while chlorine have higher tendency to gain an electron. so because of this fact chlorine is more electronegative than sodium.

As we move left to right in the periodic table, there is increase in the number of protons in atom and therefore there is increase in attraction between the nucleus and electrons and shrinking down the atom which is general trend when we move from left to right in the periodic table. so chlorine will be smaller than sodium because of the shrinking of the atom and smaller atoms have higher ionization energy because their electrons are close to the nucleus. They require more energy to remove. so this will make  chlorine have both a smaller atomic radius and larger ionization energy. so D is the right answer.

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the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.