Ch.7 - Periodic Properties of the Elements

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.7 - Periodic Properties of the Elements

Problem 6

Chapter 7, Problem 6

The graph below shows the ionization energies for a particular element. In which group is the element most likely a member of? [Section 7.3]

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Identify the pattern of ionization energies: Look at the graph and observe how the ionization energies change as electrons are removed.

Understand the concept of ionization energy: Ionization energy is the energy required to remove an electron from an atom in the gaseous state.

Recognize the significance of large jumps in ionization energy: A large increase in ionization energy indicates that an electron is being removed from a more stable, inner shell.

Determine the group based on the ionization energy pattern: Elements in the same group have similar outer electron configurations, leading to similar ionization energy patterns.

Relate the observed pattern to known group characteristics: For example, if there is a large jump after the first ionization energy, the element is likely in Group 1 (alkali metals), as they have one valence electron.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. It is a key indicator of an element's reactivity and is influenced by factors such as atomic size and nuclear charge. Generally, ionization energy increases across a period and decreases down a group in the periodic table.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. These trends include variations in ionization energy, electronegativity, and atomic radius. Understanding these trends helps in predicting the behavior of elements and their placement in groups.

Group Classification

Elements in the periodic table are organized into groups based on similar chemical properties and electron configurations. Each group shares common characteristics, such as reactivity and the number of valence electrons. Identifying the group of an element based on its ionization energy can provide insights into its chemical behavior and potential applications.

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Textbook Question

The prefix eka- comes from the Sanskrit word for 'one.' Mendeleev used this prefix to indicate that the unknown element was one place away from the known element that followed the prefix. For example, eka-silicon, which we now call germanium, is one element below silicon. Mendeleev also predicted the existence of eka-manganese, which was not experimentally confirmed until 1937 because this element is radioactive and does not occur in nature. Based on the periodic table shown in Figure 7.1, what do we now call the element Mendeleev called eka-manganese?

Which of these spheres represents F, which represents Br, and which represents Br-?

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Textbook Question

In the following reaction

which sphere represents a metal and which represents a nonmetal?

Consider the Mg²⁺, Cl^-, K⁺, and Se^2- ions. The four spheres below represent these four ions, scaled according to ionic size. (b) In terms of size, between which of the spheres would you find the (i) Ca²⁺ and (ii) S^2- ions?

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Textbook Question

Group 1A and 2A elements are sometimes called, collectively, “the s-block.” Therefore, what is an analogous name for the entire collection of the group 3A, 4A, 5A, 6A, 7A, and 8A elements?