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Chapter 5: Problem 22

Without knowing electronegativity values, a student claims \(\mathrm{BaCl}_{2}\) is more ionic than \(\mathrm{BeCl}_{2}\). All she has access to is a periodic table. How does she know she is right?

Short Answer

Expert verified
The student can determine that BaCl\(_2\) is more ionic than BeCl\(_2\) by understanding the periodic trends in electronegativity. Since electronegativity generally decreases down a group, Beryllium (Be) has a higher electronegativity than Barium (Ba). Both compounds contain Chlorine (Cl). The electronegativity difference between Be-Cl is smaller compared to Ba-Cl, indicating that BaCl\(_2\) has a greater ionic character. This conclusion can be made without knowing the exact electronegativity values and by just using the periodic table.

Step by step solution

01

Identify the location of Ba and Be in the periodic table

When looking at the periodic table, we can find the locations of the elements involved in the two compounds. Barium (Ba) is in Group 2 and Period 6, while Beryllium (Be) is also in Group 2 but in Period 2.
02

Understand the electronegativity trend across the periodic table

Generally, electronegativity increases across a period (from left to right) and decreases down a group (from top to bottom) on the periodic table. Therefore, elements in the top-right corner have the highest electronegativity values, and elements in the bottom-left corner have the lowest electronegativity values.
03

Compare the relative electronegativity values of Ba and Be

Considering the periodic trend in electronegativity, we can conclude that Beryllium (Be), which is higher up in Group 2, will have a higher electronegativity than Barium (Ba), which is further down in Group 2.
04

Identify the location of Cl in the periodic table

Chlorine (Cl) can be found in Group 17 and Period 3 in the periodic table. Since both compounds contain Chlorine, the electronegativity of Chlorine will affect the ionic character of both compounds in the same way.
05

Compare the electronegativity difference between Ba-Cl and Be-Cl

As previously determined, Be has a higher electronegativity than Ba. Therefore, the electronegativity difference between Be and Cl will be smaller compared to the difference between Ba and Cl. Smaller electronegativity differences generally correspond to greater covalent character, while larger differences imply greater ionic character.
06

Conclude the relative ionic character of BaCl2 and BeCl2

The student can conclude that BaCl2 is more ionic than BeCl2 because the electronegativity difference between Ba and Cl is larger than the difference between Be and Cl. This conclusion can be reached without knowing the exact electronegativity values, but by understanding the periodic trends in electronegativity.

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