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What charge is likely for an ion formed from this element?

What charge is likely for an ion formed from this element?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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What charge is likely for an ion formed from this element?
Below is a multiple-choice question section. Each option is preceded by a radio button, indicating that only one selection can be made at a time. The options provided include both positive and negative numbers, likely indicating a question related to numerical values or calculations. Options: - ○ -1 - ○ -3 - ○ +3 - ○ +5 The user needs to select one of the options by clicking on the corresponding radio button.
Transcribed Image Text:Below is a multiple-choice question section. Each option is preceded by a radio button, indicating that only one selection can be made at a time. The options provided include both positive and negative numbers, likely indicating a question related to numerical values or calculations. Options: - ○ -1 - ○ -3 - ○ +3 - ○ +5 The user needs to select one of the options by clicking on the corresponding radio button.
### Understanding Electron Configuration In this section, we will explore the electron configuration of main group elements, focusing specifically on those with an outer electron configuration of \( ns^2np^5 \). #### Main Group Elements and Electron Configuration Main group elements are those found in the s- and p-blocks of the periodic table. These elements include the alkali metals, alkaline earth metals, and the nonmetals, as well as the noble gases. The outer electron configuration of an element describes the distribution of electrons in the outermost shell of an atom. ##### Example: \( ns^2np^5 \) When an element has an outer electron configuration of \( ns^2np^5 \), it means: - There are two electrons in the s-orbital of the outermost shell. - There are five electrons in the p-orbital of the same shell. This type of configuration is indicative of elements in Group 17 of the periodic table, also known as the halogens. ###### Halogens The halogens include: - Fluorine (F) - Chlorine (Cl) - Bromine (Br) - Iodine (I) - Astatine (At) - Tennessine (Ts) Each of these elements has seven electrons in their outermost shell, with a full s-orbital (2 electrons) and five electrons in the p-orbital, which gives them their characteristic reactivity and allows them to form salts when they react with metals. Understanding the electron configuration helps in predicting the chemical behavior of elements, their reactivity, and the types of bonds they are likely to form.
Transcribed Image Text:### Understanding Electron Configuration In this section, we will explore the electron configuration of main group elements, focusing specifically on those with an outer electron configuration of \( ns^2np^5 \). #### Main Group Elements and Electron Configuration Main group elements are those found in the s- and p-blocks of the periodic table. These elements include the alkali metals, alkaline earth metals, and the nonmetals, as well as the noble gases. The outer electron configuration of an element describes the distribution of electrons in the outermost shell of an atom. ##### Example: \( ns^2np^5 \) When an element has an outer electron configuration of \( ns^2np^5 \), it means: - There are two electrons in the s-orbital of the outermost shell. - There are five electrons in the p-orbital of the same shell. This type of configuration is indicative of elements in Group 17 of the periodic table, also known as the halogens. ###### Halogens The halogens include: - Fluorine (F) - Chlorine (Cl) - Bromine (Br) - Iodine (I) - Astatine (At) - Tennessine (Ts) Each of these elements has seven electrons in their outermost shell, with a full s-orbital (2 electrons) and five electrons in the p-orbital, which gives them their characteristic reactivity and allows them to form salts when they react with metals. Understanding the electron configuration helps in predicting the chemical behavior of elements, their reactivity, and the types of bonds they are likely to form.
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