Chemistry Exam > Chemistry Questions > O2-, F–, Na+ and Mg2+ are called as ___...
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O2-, F–, Na+ and Mg2+ are called as _______
- a)Isoelectronic species
- b)Isoneutral species
- c)Isotopes
- d)Isobars
Correct answer is option 'A'. Can you explain this answer?
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O2-, F–, Na+ and Mg2+ are called as _______a)Isoelectronic speci...
Understanding Isoelectronic Species
Isoelectronic species are atoms, ions, or molecules that have the same number of electrons. The species mentioned—O2-, F-, Na+, and Mg2+—all fit this description.
Electron Configuration of Each Species
- O2- (Oxide Ion):
- Has 8 protons and gains 2 electrons, resulting in 10 electrons.
- F- (Fluoride Ion):
- Contains 9 protons and gains 1 electron, totaling 10 electrons.
- Na+ (Sodium Ion):
- With 11 protons, it loses 1 electron, bringing its total to 10 electrons.
- Mg2+ (Magnesium Ion):
- Has 12 protons and loses 2 electrons, resulting in 10 electrons.
Common Electron Count
All four species have 10 electrons, which corresponds to the electron configuration of Neon (Ne), a noble gas. This similarity in electron configuration leads to similar chemical properties, even though they differ in their nuclear charge and physical properties.
Importance of Isoelectronic Species
- Chemical Stability:
- Isoelectronic species often exhibit similar stability and reactivity due to their identical electron arrangements.
- Comparative Studies:
- They serve as useful models in understanding ionic bonding and molecular structures.
In summary, O2-, F-, Na+, and Mg2+ are classified as isoelectronic species because they all possess the same total number of electrons, making option 'A' the correct choice.
Isoelectronic species are atoms, ions, or molecules that have the same number of electrons. The species mentioned—O2-, F-, Na+, and Mg2+—all fit this description.
Electron Configuration of Each Species
- O2- (Oxide Ion):
- Has 8 protons and gains 2 electrons, resulting in 10 electrons.
- F- (Fluoride Ion):
- Contains 9 protons and gains 1 electron, totaling 10 electrons.
- Na+ (Sodium Ion):
- With 11 protons, it loses 1 electron, bringing its total to 10 electrons.
- Mg2+ (Magnesium Ion):
- Has 12 protons and loses 2 electrons, resulting in 10 electrons.
Common Electron Count
All four species have 10 electrons, which corresponds to the electron configuration of Neon (Ne), a noble gas. This similarity in electron configuration leads to similar chemical properties, even though they differ in their nuclear charge and physical properties.
Importance of Isoelectronic Species
- Chemical Stability:
- Isoelectronic species often exhibit similar stability and reactivity due to their identical electron arrangements.
- Comparative Studies:
- They serve as useful models in understanding ionic bonding and molecular structures.
In summary, O2-, F-, Na+, and Mg2+ are classified as isoelectronic species because they all possess the same total number of electrons, making option 'A' the correct choice.
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O2-, F–, Na+ and Mg2+ are called as _______a)Isoelectronic speci...
O2-, F–, Na+ and Mg2+ are known as isoelectronic species as they all have the same no. of electrons(10). Isotopes contain the same no. of protons but a different number of neutrons. Isobars have the same mass number but a different atomic number.
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O2-, F–, Na+ and Mg2+ are called as _______a)Isoelectronic speciesb)Isoneutral speciesc)Isotopesd)IsobarsCorrect answer is option 'A'. Can you explain this answer?
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