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Chapter 10: Problem 77

Choose the element with the higher ionization energy from each pair. (a) As or Bi (b) As or Br (c) \(\mathrm{S}\) or \(\mathrm{I}\) (d) \(\mathrm{S}\) or \(\mathrm{Sb}\)

Short Answer

Expert verified
The elements with higher ionization energy are: (a) As, (b) Br, (c) S, (d) S.

Step by step solution

01

Understanding Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It generally increases across a period from left to right and decreases down a group on the periodic table.
02

Comparing As and Bi

Arsenic (As) and Bismuth (Bi) are in the same group with arsenic being above bismuth. As you move down a group, ionization energy decreases, so As will have a higher ionization energy than Bi.
03

Comparing As and Br

Arsenic (As) and Bromine (Br) are in the same period. Bromine is to the right of arsenic, meaning it has a higher ionization energy. So, Br has a higher ionization energy than As.
04

Comparing S and I

Sulfur (S) and Iodine (I) are in the same group with sulfur being above iodine. As you move down a group, ionization energy decreases, so S will have a higher ionization energy than I.
05

Comparing S and Sb

Sulfur (S) and Antimony (Sb) are in the same group with sulfur being above antimony. As you move down a group, ionization energy decreases, so S will have a higher ionization energy than Sb.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Periodic Table Trends
Understanding the periodic table trends is essential when examining ionization energies across different elements. As you glance at the periodic table, you might notice it's organized into rows and columns, known as periods and groups, respectively.

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Most popular questions from this chapter

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. (a) \(\mathrm{Te}\) (b) \(\mathrm{Br}\) (c) \(\mathrm{I}\) (d) \(\mathrm{Cs}\)

Explain the difference between valence electrons and core electrons.

What type of electromagnetic radiation is used in communications devices such as cellular telephones?

List the number of elements in periods 1 and 2 of the periodic table. Why does each period have a different number of elements?

When an electron makes a transition from the \(n=3\) to the \(n=2\) hydrogen atom Bohr orbit, the energy difference between these two orbits \(\left(3.0 \times 10^{-19} \mathrm{~J}\right)\) is emitted as a photon of light. The relationship between the energy of a photon and its wavelength is given by \(E=h c / \lambda\), where \(E\) is the energy of the photon in \(\mathrm{J}, h\) is Planck's constant \(\left(6.626 \times 10^{-34} \mathrm{~J} \cdot \mathrm{s}\right)\), and \(c\) is the speed of light \(\left(3.00 \times 10^{8} \mathrm{~m} / \mathrm{s}\right)\). Find the wavelength of light emitted by hydrogen atoms when an electron makes this transition.
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