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Without using Fig. $13.3,$ predict the order of increasing electronegativity in each of the following groups of elements. a. $\mathrm{C}, \mathrm{N}, \mathrm{O}$ b. $\mathrm{S}, \mathrm{Se}, \mathrm{Cl}$ c. $\mathrm{Si}, \mathrm{Ge}, \mathrm{Sn}$ d. $\mathrm{Tl}, \mathrm{S}, \mathrm{Ge}$ e. $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$ f. $\mathrm{B}, \mathrm{O}, \mathrm{Ga}$

Name: Problem 15, Chapter 13: Chemical Principle
Uploaded: 2020-08-09T14:59:54-08:00
Duration: 1 min 4 s
Channel: Lottie Adams
Description: Without using Fig. 13.3, predict the order of increasing electronegativity in each of the following groups of elements. a. C, N, O b. S, Se, Cl c. Si, Ge, Sn d. Tl, S, Ge e. Na, K, Rb f. B, O, Ga

   Without using Fig. $13.3,$ predict the order of increasing electronegativity in each of the following groups of elements.
a. $\mathrm{C}, \mathrm{N}, \mathrm{O}$
b. $\mathrm{S}, \mathrm{Se}, \mathrm{Cl}$
c. $\mathrm{Si}, \mathrm{Ge}, \mathrm{Sn}$
d. $\mathrm{Tl}, \mathrm{S}, \mathrm{Ge}$
e. $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$
f. $\mathrm{B}, \mathrm{O}, \mathrm{Ga}$

Chemical Principle

Steven S. Zumdahl,… 7th Edition

Chapter 13, Problem 15

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Solved by Expert Lottie Adams

08/09/2020

Step 1

Electronegativity increases as we move from left to right across a period and decreases as we move down a group. This is because as we move from left to right, the number of protons in the nucleus increases, attracting the electrons more strongly. As we move down Show more…

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Without using Fig. $13.3,$ predict the order of increasing electronegativity in each of the following groups of elements. a. $\mathrm{C}, \mathrm{N}, \mathrm{O}$ b. $\mathrm{S}, \mathrm{Se}, \mathrm{Cl}$ c. $\mathrm{Si}, \mathrm{Ge}, \mathrm{Sn}$ d. $\mathrm{Tl}, \mathrm{S}, \mathrm{Ge}$ e. $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$ f. $\mathrm{B}, \mathrm{O}, \mathrm{Ga}$

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Key Concepts

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold electrons in a chemical bond. It plays a crucial role in determining bond polarity and the reactivity of molecules, influencing many chemical properties and behavior in reactions.

Periodic Trends

Periodic trends are patterns in elemental properties observed across periods and down groups in the periodic table. For electronegativity, it generally increases from left to right across a period due to a higher effective nuclear charge and decreases from top to bottom within a group because of increasing atomic size and electron shielding.

Effective Nuclear Charge

Effective nuclear charge refers to the net positive charge experienced by valence electrons after accounting for shielding effects from inner electrons. An increased effective nuclear charge leads to a stronger attraction for bonding electrons, thus contributing to higher electronegativity as one moves across a period.

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