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Chapter 8: Problem 39

Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Na, \(\mathrm{Mg}, \mathrm{K}, \mathrm{Ca} ;(\mathbf{b}) \mathrm{P}, \mathrm{S},\) As, \(\mathrm{Se} ;(\mathbf{c}) \mathrm{Be}, \mathrm{B}, \mathrm{C}, \mathrm{Si} ;(\mathbf{d}) \mathrm{Zn}, \mathrm{Ge}, \mathrm{Ga}, \mathrm{Gs}\)

Short Answer

Expert verified
The most electronegative elements in each set are: (a) $\mathrm{Mg}$; (b) $\mathrm{S}$; (c) $\mathrm{C}$; (d) $\mathrm{Ga}$.

Step by step solution

01

Set (a): Na, Mg, K, Ca

To determine the most electronegative atom among Na, Mg, K, and Ca, we need to locate these elements in the periodic table. They are all in the same period (Period 3) and belong to Groups 1 and 2. As electronegativity increases from left to right across a period, Mg (Group 2) is more electronegative than Na (Group 1). Similarly, Ca (Group 2) is more electronegative than K (Group 1). Between Mg and Ca, since electronegativity decreases down a group, Mg is more electronegative than Ca. Therefore, Mg is the most electronegative element in the given set.
02

Set (b): P, S, As, Se

To determine the most electronegative atom among P, S, As, and Se, we need to locate these elements in the periodic table. They belong to Groups 15 and 16. From left to right in the periodic table, electronegativity increases, so S (Group 16) is more electronegative than P (Group 15) and Se (Group 16) is more electronegative than As (Group 15). Between S and Se, since electronegativity decreases down a group, S is more electronegative than Se. Therefore, S is the most electronegative element in the given set.
03

Set (c): Be, B, C, Si

To determine the most electronegative atom among Be, B, C, and Si, we need to locate these elements in the periodic table. They are all in the same period (Period 2) and belong to Groups 13 and 14. As electronegativity increases from left to right across a period, C (Group 14) is more electronegative than B (Group 13) and Si (Group 14). Between C and Si, since electronegativity decreases down a group, C is more electronegative than Si. Therefore, C is the most electronegative element in the given set.
04

Set (d): Zn, Ge, Ga, Gs

To determine the most electronegative atom among Zn, Ge, Ga, and Gs, we need to locate these elements in the periodic table. They belong to Groups 12, 13, and 14. From left to right in the periodic table, electronegativity increases, so Gs (Group 14) is more electronegative than Ge (Group 13) and Ga (Group 13) is more electronegative than Zn (Group 12). Between Gs and Ga, since electronegativity increases from bottom to top in a group, Ga is more electronegative than Gs. Therefore, Ga is the most electronegative element in the given set.

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Most popular questions from this chapter

We can define average bond enthalpies and bond lengths for ionic bonds, just like we have for covalent bonds. Which ionic bond is predicted to have the smaller bond enthalpy, Li-F or \(\mathrm{Cs}-\mathrm{F}\) ?

List the individual steps used in constructing a Born-Haber cycle for the formation of \(\mathrm{Bal}_{2}\) from the elements. Which of the steps would you expect to be exothermic?

(a) Describe the molecule xenon trioxide, \(\mathrm{XeO}_{3},\) using four possible Lewis structures, one each with zero, one, two, or three \(\mathrm{Xe}-\mathrm{O}\) double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in part (a) yields the most favorable formal charges for the molecule?

Which of the following statements about electronegativity is false? (a) Electronegativity is the ability of an atom in a molecule to attract electron density toward itself. (b) Electronegativity is the same thing as electron affinity. (c) The numerical values for electronegativity have no units. (d) Fluorine is the most electronegative element. (e) Cesium is the least electronegative element.

(a) Which of these compounds is an exception to the octet rule: carbon dioxide, water, ammonia, phosphorus trifluoride, or arsenic pentafluoride? (b) Which of these compounds or ions is an exception to the octet rule: borohydride \(\left(\mathrm{BH}_{4}^{-}\right),\) borazine \(\left(\mathrm{B}_{3} \mathrm{N}_{3} \mathrm{H}_{6},\) which is analogous \right. to benzene with alternating \(\mathrm{B}\) and \(\mathrm{N}\) in the ring \(),\) or boron trichloride?
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