Textbook Question
Each of the following elements is capable of forming an ion in chemical reactions. By referring to the periodic table, predict the charge of the most stable ion of each: c. K
2. Atoms & Elements
Periodic Table: Charges
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Do elements in Group 2 tend to lose electrons to form cations with a charge of +2? Because?
A
Yes, because they have three valence electrons that they lose to achieve a stable electron configuration.
B
Yes, because they have two valence electrons that they lose to achieve a stable electron configuration.
C
No, because they gain two electrons to achieve a stable electron configuration.
D
No, because they share electrons to form covalent bonds.
Verified step by step guidance1
Identify the elements in Group 2 of the periodic table. These are known as alkaline earth metals and include beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
Understand the electron configuration of Group 2 elements. These elements have two valence electrons in their outermost shell, typically in the s-orbital.
Recognize the tendency of Group 2 elements to achieve a stable electron configuration. They do this by losing their two valence electrons, resulting in a full outer shell similar to the nearest noble gas configuration.
Explain why losing two electrons leads to the formation of cations with a +2 charge. When an atom loses electrons, it becomes positively charged because the number of protons exceeds the number of electrons.
Clarify why other options are incorrect. Group 2 elements do not gain electrons to form anions, nor do they typically share electrons to form covalent bonds, as their metallic nature favors the formation of ionic compounds.
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Periodic Table: Charges practice set
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