A sodium atom forms a sodium cation (Na⁺) by losing its outermost electron. Sodium, located in Group 1 of the periodic table, has one electron in its outermost energy level (3s¹). To achieve a stable, noble gas electron configuration similar to neon, sodium readily donates this lone electron. Upon lRead more
A sodium atom forms a sodium cation (Na⁺) by losing its outermost electron. Sodium, located in Group 1 of the periodic table, has one electron in its outermost energy level (3s¹). To achieve a stable, noble gas electron configuration similar to neon, sodium readily donates this lone electron. Upon losing the electron, sodium becomes a positively charged ion (Na⁺), with a completed electron configuration resembling that of a noble gas. This cationic state reflects sodium’s tendency to achieve a more stable, lower-energy configuration by giving up its outer electron during chemical reactions, typically forming ionic compounds with nonmetals.
The electronic configuration of a chlorine (Cl) atom is 1s² 2s² 2p⁶ 3s² 3p⁵. This configuration illustrates the distribution of electrons in the various energy levels and orbitals of the chlorine atom. More specifically, it indicates that chlorine has two electrons in the first energy level (1s²), eRead more
The electronic configuration of a chlorine (Cl) atom is 1s² 2s² 2p⁶ 3s² 3p⁵. This configuration illustrates the distribution of electrons in the various energy levels and orbitals of the chlorine atom. More specifically, it indicates that chlorine has two electrons in the first energy level (1s²), eight electrons in the second energy level (2s² 2p⁶), and seven electrons in the third energy level (3s² 3p⁵). Chlorine belongs to Group 17 of the periodic table and is a halogen, characterized by having seven electrons in its outermost energy level, making it highly reactive in chemical reactions.
A chlorine atom forms a chloride anion (Cl⁻) by gaining one electron. Chlorine, belonging to Group 17 (halogens) on the periodic table, has seven electrons in its outermost energy level (3s² 3p⁵) and tends to achieve a stable, noble gas electron configuration similar to argon with eight electrons. IRead more
A chlorine atom forms a chloride anion (Cl⁻) by gaining one electron. Chlorine, belonging to Group 17 (halogens) on the periodic table, has seven electrons in its outermost energy level (3s² 3p⁵) and tends to achieve a stable, noble gas electron configuration similar to argon with eight electrons. In chemical reactions, chlorine readily accepts an electron to complete its outer electron shell, resulting in the chloride anion. The added electron gives chlorine a negative charge, and the resulting chloride ion has an electron configuration resembling that of a noble gas, making it more stable and less reactive than the chlorine atom.
The relationship between sodium and chlorine exemplifies a give-and-take dynamic in chemical bonding. Sodium, a metal, readily donates its lone outer electron to chlorine, a nonmetal. By losing an electron, sodium achieves a stable, noble gas configuration, forming a positively charged sodium cationRead more
The relationship between sodium and chlorine exemplifies a give-and-take dynamic in chemical bonding. Sodium, a metal, readily donates its lone outer electron to chlorine, a nonmetal. By losing an electron, sodium achieves a stable, noble gas configuration, forming a positively charged sodium cation (Na⁺). Simultaneously, chlorine accepts the donated electron to complete its outer electron shell, forming a negatively charged chloride anion (Cl⁻). The resulting ionic bond between Na⁺ and Cl⁻ leads to the formation of sodium chloride (NaCl), commonly known as table salt. This exchange of electrons demonstrates the complementary nature of these elements, stabilizing each other through charge interaction.
Sodium and chlorine achieve stable electronic configurations through ionic bonding. Sodium, with one electron in its outer shell, donates this electron to chlorine, which has seven electrons in its outer shell. Sodium becomes a positively charged cation (Na⁺) with a stable noble gas configuration (lRead more
Sodium and chlorine achieve stable electronic configurations through ionic bonding. Sodium, with one electron in its outer shell, donates this electron to chlorine, which has seven electrons in its outer shell. Sodium becomes a positively charged cation (Na⁺) with a stable noble gas configuration (like neon), while chlorine forms a negatively charged anion (Cl⁻) with a stable noble gas configuration (like argon). The electrostatic attraction between Na⁺ and Cl⁻ ions results in the formation of sodium chloride (NaCl), where each ion’s electron deficiency or excess is compensated, leading to a more stable overall electronic configuration for both elements.
How does a sodium atom form a sodium cation (Na+)?
A sodium atom forms a sodium cation (Na⁺) by losing its outermost electron. Sodium, located in Group 1 of the periodic table, has one electron in its outermost energy level (3s¹). To achieve a stable, noble gas electron configuration similar to neon, sodium readily donates this lone electron. Upon lRead more
A sodium atom forms a sodium cation (Na⁺) by losing its outermost electron. Sodium, located in Group 1 of the periodic table, has one electron in its outermost energy level (3s¹). To achieve a stable, noble gas electron configuration similar to neon, sodium readily donates this lone electron. Upon losing the electron, sodium becomes a positively charged ion (Na⁺), with a completed electron configuration resembling that of a noble gas. This cationic state reflects sodium’s tendency to achieve a more stable, lower-energy configuration by giving up its outer electron during chemical reactions, typically forming ionic compounds with nonmetals.
See lessWhat is the electronic configuration of a chlorine atom?
The electronic configuration of a chlorine (Cl) atom is 1s² 2s² 2p⁶ 3s² 3p⁵. This configuration illustrates the distribution of electrons in the various energy levels and orbitals of the chlorine atom. More specifically, it indicates that chlorine has two electrons in the first energy level (1s²), eRead more
The electronic configuration of a chlorine (Cl) atom is 1s² 2s² 2p⁶ 3s² 3p⁵. This configuration illustrates the distribution of electrons in the various energy levels and orbitals of the chlorine atom. More specifically, it indicates that chlorine has two electrons in the first energy level (1s²), eight electrons in the second energy level (2s² 2p⁶), and seven electrons in the third energy level (3s² 3p⁵). Chlorine belongs to Group 17 of the periodic table and is a halogen, characterized by having seven electrons in its outermost energy level, making it highly reactive in chemical reactions.
See lessHow does a chlorine atom form a chloride anion (Cl-)?
A chlorine atom forms a chloride anion (Cl⁻) by gaining one electron. Chlorine, belonging to Group 17 (halogens) on the periodic table, has seven electrons in its outermost energy level (3s² 3p⁵) and tends to achieve a stable, noble gas electron configuration similar to argon with eight electrons. IRead more
A chlorine atom forms a chloride anion (Cl⁻) by gaining one electron. Chlorine, belonging to Group 17 (halogens) on the periodic table, has seven electrons in its outermost energy level (3s² 3p⁵) and tends to achieve a stable, noble gas electron configuration similar to argon with eight electrons. In chemical reactions, chlorine readily accepts an electron to complete its outer electron shell, resulting in the chloride anion. The added electron gives chlorine a negative charge, and the resulting chloride ion has an electron configuration resembling that of a noble gas, making it more stable and less reactive than the chlorine atom.
See lessDescribe the give-and-take relation between sodium and chlorine.
The relationship between sodium and chlorine exemplifies a give-and-take dynamic in chemical bonding. Sodium, a metal, readily donates its lone outer electron to chlorine, a nonmetal. By losing an electron, sodium achieves a stable, noble gas configuration, forming a positively charged sodium cationRead more
The relationship between sodium and chlorine exemplifies a give-and-take dynamic in chemical bonding. Sodium, a metal, readily donates its lone outer electron to chlorine, a nonmetal. By losing an electron, sodium achieves a stable, noble gas configuration, forming a positively charged sodium cation (Na⁺). Simultaneously, chlorine accepts the donated electron to complete its outer electron shell, forming a negatively charged chloride anion (Cl⁻). The resulting ionic bond between Na⁺ and Cl⁻ leads to the formation of sodium chloride (NaCl), commonly known as table salt. This exchange of electrons demonstrates the complementary nature of these elements, stabilizing each other through charge interaction.
See lessHow do sodium and chlorine achieve stable electronic configurations through their interaction?
Sodium and chlorine achieve stable electronic configurations through ionic bonding. Sodium, with one electron in its outer shell, donates this electron to chlorine, which has seven electrons in its outer shell. Sodium becomes a positively charged cation (Na⁺) with a stable noble gas configuration (lRead more
Sodium and chlorine achieve stable electronic configurations through ionic bonding. Sodium, with one electron in its outer shell, donates this electron to chlorine, which has seven electrons in its outer shell. Sodium becomes a positively charged cation (Na⁺) with a stable noble gas configuration (like neon), while chlorine forms a negatively charged anion (Cl⁻) with a stable noble gas configuration (like argon). The electrostatic attraction between Na⁺ and Cl⁻ ions results in the formation of sodium chloride (NaCl), where each ion’s electron deficiency or excess is compensated, leading to a more stable overall electronic configuration for both elements.
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