Textbook Question
Name an element in the third period (row) of the periodic table with the following: d. two 3s electrons and no 3p electrons
Ch.8 - Periodic Properties of the Elements
Chapter 8, Problem 52
Determine the number of valence electrons in each element. Which elements do you expect to lose electrons in chemical reactions? Which do you expect to gain electrons? a. Al b. Sn c. Br d. Se
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Identify the number of valence electrons for each element by looking at their group number in the periodic table. Elements in the same group have the same number of valence electrons. For example, Group 1 elements have 1 valence electron, Group 2 elements have 2, and so on. Transition metals and inner transition metals may have varying numbers of valence electrons.
For Aluminum (Al), which is in Group 13, it typically has 3 valence electrons. Tin (Sn) is in Group 14, generally having 4 valence electrons. Bromine (Br) is in Group 17, with 7 valence electrons. Selenium (Se) is in Group 16, having 6 valence electrons.
Determine the tendency of each element to lose or gain electrons based on their position in the periodic table. Elements in Groups 1-3 tend to lose electrons to achieve a noble gas configuration, while elements in Groups 15-17 tend to gain electrons.
Predict that Aluminum (Al) and Tin (Sn), being in Groups 13 and 14 respectively, are more likely to lose electrons during chemical reactions to achieve a stable electron configuration.
Predict that Bromine (Br) and Selenium (Se), being in Groups 17 and 16 respectively, are more likely to gain electrons during chemical reactions to fill their outer electron shells and reach stability.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial in determining how an element interacts chemically. The number of valence electrons influences an element's reactivity, as these electrons are involved in forming bonds with other atoms. For main group elements, the number of valence electrons corresponds to their group number in the periodic table.
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Transition Metals Valence Electrons
Electron Loss and Gain
Elements tend to lose or gain electrons to achieve a stable electron configuration, often resembling that of the nearest noble gas. Metals, such as aluminum (Al) and tin (Sn), typically lose electrons to form positive ions, while nonmetals, like bromine (Br) and selenium (Se), usually gain electrons to form negative ions. This behavior is driven by the desire to minimize energy and achieve stability.
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Periodic Trends
Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. For instance, electronegativity and ionization energy generally increase across a period and decrease down a group. Understanding these trends helps predict how elements will behave in chemical reactions, including their tendency to lose or gain electrons.
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Related Practice
Textbook Question
Determine the number of valence electrons in an atom of each element. a. Ba c. Ni d. S
Textbook Question
Determine the number of valence electrons in an atom of each element. b. Cs
Textbook Question
Which outer electron configuration would you expect to belong to a reactive metal? a. ns2 b. ns2np6 c. ns2np5 d. ns2np2
Textbook Question
Which outer electron configuration would you expect to belong to a reactive nonmetal? a. ns2 b. ns2np6 c. ns2np5 d. ns2np2
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Textbook Question
Which outer electron configurations would you expect to belong to a noble gas? a. ns2 b. ns2np6 c. ns2np5 d. ns2np2