Chapter 4: Problem 8
Write the symbol for the ion of each of the following: a. fluorine b. calcium c. sodium d. iodine
Short Answer
Expert verified
Fluorine: \( F^{-} \), Calcium: \( Ca^{2+} \), Sodium: \( Na^{+} \), Iodine: \( I^{-} \).
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
periodic table
The periodic table is an organized chart that displays all known chemical elements. Each element is placed based on its atomic number, electron configurations, and recurring chemical properties. The table is divided into groups (vertical columns) and periods (horizontal rows).
Groups help us understand the number of valence electrons in an element. For example, elements in Group 1 have 1 valence electron, while those in Group 17 have 7 valence electrons. This organization allows us to predict how elements will react and form ions, as all elements in the same group share similar properties.
Understanding the periodic table is essential for predicting the behavior of elements, especially their ability to form ions.
Groups help us understand the number of valence electrons in an element. For example, elements in Group 1 have 1 valence electron, while those in Group 17 have 7 valence electrons. This organization allows us to predict how elements will react and form ions, as all elements in the same group share similar properties.
Understanding the periodic table is essential for predicting the behavior of elements, especially their ability to form ions.
valence electrons
Valence electrons are the electrons found in the outermost shell of an atom. These electrons play a crucial role in chemical bonding and ion formation.
For instance, fluorine has 7 valence electrons, and calcium has 2 valence electrons. The number of valence electrons determines how an element will interact with others to achieve a stable electron configuration.
In forming ions, elements will either lose or gain electrons in their outermost shell to achieve stability. This leads to the formation of cations (positively charged ions) or anions (negatively charged ions).
For instance, fluorine has 7 valence electrons, and calcium has 2 valence electrons. The number of valence electrons determines how an element will interact with others to achieve a stable electron configuration.
In forming ions, elements will either lose or gain electrons in their outermost shell to achieve stability. This leads to the formation of cations (positively charged ions) or anions (negatively charged ions).
octet rule
The octet rule is a principle in chemistry that states that atoms tend to form ions in a way that they end up with eight valence electrons. This rule is based on the observation that atoms with eight valence electrons (such as the noble gases) are particularly stable.
For example, fluorine has 7 valence electrons and needs 1 more to reach eight, so it gains an electron to form \( F^{-} \). Sodium, with 1 valence electron, will lose that electron to end up with zero valence electrons, falling back to a full outer shell below, forming \( Na^{+} \).
This rule helps explain the general patterns observed in the formation of ions during chemical reactions.
For example, fluorine has 7 valence electrons and needs 1 more to reach eight, so it gains an electron to form \( F^{-} \). Sodium, with 1 valence electron, will lose that electron to end up with zero valence electrons, falling back to a full outer shell below, forming \( Na^{+} \).
This rule helps explain the general patterns observed in the formation of ions during chemical reactions.
ionic charge
Ionic charge refers to the electric charge that an ion carries, which results from the loss or gain of electrons. An ion with more protons than electrons is positively charged (cation), while an ion with more electrons than protons is negatively charged (anion).
For instance, when calcium loses 2 electrons, it forms \( Ca^{2+} \), a cation with a +2 charge. Conversely, when iodine gains one electron, it forms \( I^{-} \), an anion with a -1 charge.
The magnitude of the ionic charge is determined by the difference between the number of protons and electrons. This concept is vital for understanding the chemical behavior and bonding patterns of elements.
For instance, when calcium loses 2 electrons, it forms \( Ca^{2+} \), a cation with a +2 charge. Conversely, when iodine gains one electron, it forms \( I^{-} \), an anion with a -1 charge.
The magnitude of the ionic charge is determined by the difference between the number of protons and electrons. This concept is vital for understanding the chemical behavior and bonding patterns of elements.
