Question 1

Which element would be expected to have the most favorable electron affinity ?

Accepted Answer

Fluorine (F) is the most electronegative element in the periodic table, which means that it strongly attracts electrons. A high electron affinity means that an atom is likely to gain an electron, and fluorine has the highest electron affinity of any element, meaning it is the most likely to gain an electron and form a negative ion.

Question 2

Which of the following processes listed below represents the experiment for measuring an electron affinity ?
("E" represents a neutral E lement, "M" represents a M etal cation and "X" represents a nonmetal anion)

Accepted Answer

Electron affinity measures the energy change when an electron is added to a neutral atom in the gas phase to form a negative ion, which is accurately represented by option A.

Question 3

With respect to electron affinity , arrange the following elements in order from least favorable to most favorable in terms of acquiring an additional electron. Barium, Fluorine, Sulfur

Accepted Answer

Electron affinity generally increases across a period from left to right and decreases down a group. Barium, being an alkaline earth metal, has a low electron affinity as it is more favorable for it to lose electrons than to gain. Sulfur, being to the right of barium in the periodic table, has a higher electron affinity due to its desire to complete its valence shell. Fluorine has the highest electron affinity of all elements because it is very electronegative and eagerly gains electrons to complete its valence shell. Therefore, the correct order from least to most favorable in terms of acquiring an additional electron is Barium < Sulfur < Fluorine.

Question 4

Three statements are listed below. Pick the best answer.
I. The halogens form ionic compounds with the alkali metal family.
II. The halogens form compounds with other elements on the right side of the periodic table that are generally nonionic gases or low-boiling liquids.
III. Halide salts react with water to form the elemental halogen and metal.

Accepted Answer

I. True, because halogens (Group 17) and alkali metals (Group 1) typically form ionic compounds due to the transfer of electrons from the alkali metal to the halogen. II. True, because halogens can form covalent bonds with other nonmetals to the right of the periodic table, often resulting in molecules that are gases or liquids at room temperature. III. False, because halide salts generally do not react with water to form elemental halogen and metal; instead, they dissolve in water to form aqueous solutions of the ions.

Question 5

Based upon the electron affinity trend, which group of atoms is most likely to acquire an additional electron?

Accepted Answer

The electron affinity trend shows that atoms that are closer to having a full outer shell of electrons (i.e. atoms that are closer to a noble gas configuration) have a higher electron affinity. Halogens, which are in Group 17, are only one electron away from a full outer shell and therefore have a high affinity for an additional electron.

Question 6

Which element listed below has the most exothermic electron affinity?

Accepted Answer

Iodine (I) has the most exothermic electron affinity among the options listed. This is because, in general, halogens have high electron affinities due to their desire to gain an electron to complete their valence shell, making them more stable. Iodine, being a halogen, fits this description.

Question 7

Three reactions are shown below. Pick the best answer. I. 2 Li + 2 H₂O→2 LiOH + H₂ II. 6 Li + N₂→2 Li₃N III. Cl₂ + H₂→2 HCl

Accepted Answer

All three reactions are correct: I is the reaction of lithium with water, II is the reaction of lithium with nitrogen to form lithium nitride, and III is the reaction of chlorine with hydrogen to form hydrogen chloride.

Question 8

Given the three statements below, pick the best answer. I. Cl has a higher electron affinity than P. II. The ionization energy for Si is greater than that for P⁺. III. The electron affinity for O is greater than that for Se.

Accepted Answer

I. Cl has a higher electron affinity than P. - This statement is true as Chlorine has a higher electron affinity than Phosphorous. II. The ionization energy for Si is greater than that for P⁺. - This statement is false as P⁺ is not a valid ion and cannot be compared. III. The electron affinity for O is greater than that for Se. - This statement is true as Oxygen has a higher electron affinity than Selenium. Therefore, only statements I and III are true and statement II is false, leading to option A as the correct choice.

Question 9

Given the three reactions shown below, pick the best answer. I. K + O₂→KO₂ II. 2 K + 2 H₂O→2 KOH + H₂ III. 2 NaOH + H₂SO₄→Na₂SO₄ + 2 H₂O

Accepted Answer

All three reactions are correctly balanced and represent plausible chemical reactions: I shows the formation of a compound from potassium and an element with a subscript notation, II represents a reaction between potassium and a hydrogen-containing compound to produce potassium hydroxide and another compound, and III depicts a reaction between sodium hydroxide and a sulfur-containing compound to produce another compound and water.

Question 10

Which atom listed below has the highest electron affinity?

Accepted Answer

Sulfur (S) has the highest electron affinity among the options given. Electron affinity generally increases across a period in the periodic table because the atoms become more eager to gain an electron to achieve a stable electronic configuration. Sulfur, being closer to the noble gases than the others listed, has a higher electron affinity.

Quiz 8: The Periodic Table: Structure and Trends

Which element would be expected to have the most favorable electron affinity ?

Which of the following processes listed below represents the experiment for measuring an electron affinity ? ("E" represents a neutral E lement, "M" represents a M etal cation and "X" represents a nonmetal anion)