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Answer :
To find the equation that represents the ionization of a neutral strontium atom to form its most stable ion, we need to consider the common ionization behavior of strontium (Sr), which is a Group 2 alkaline earth metal.
1. Understanding Ionization:
- Ionization is the process by which an atom loses or gains electrons to form ions.
- Alkaline earth metals, such as strontium, commonly lose electrons to form positive ions (cations).
2. Strontium's Valence Electrons:
- Strontium (Sr) has an atomic number of 38, and its electron configuration is [tex]\([Kr] 5s^2\)[/tex].
- This means it has 2 electrons in its outermost shell.
3. Most Stable Ion:
- For strontium, losing these 2 valence electrons will lead to a stable, positively charged ion.
- The ion formed will be [tex]\(Sr^{2+}\)[/tex].
Given these points, let's evaluate the options:
A: [tex]\( Sr + e^{-} \rightarrow Sr \)[/tex]
- This equation represents the addition of an electron to a neutral strontium atom, which is not relevant to ionization into a stable ion.
B: [tex]\( Sr + 2 e^{-} \rightarrow Sr^{2-} \)[/tex]
- This equation also represents the addition of electrons, resulting in a negatively charged ion, which is not typical for strontium.
C: [tex]\( Sr (s) + 2 H_2 O(l) \rightleftharpoons Sr(OH)_2(aq) + H_2(g) \)[/tex]
- This is a chemical reaction involving strontium and water, not an ionization equation.
D: [tex]\( Sr \rightarrow Sr^{+} + e^{-} \)[/tex]
- This represents the loss of only one electron, forming a singly charged positive ion, [tex]\(Sr^+\)[/tex]. However, this is not the most stable form.
E: [tex]\( Sr \rightarrow Sr^{2+} + 2 e^{-} \)[/tex]
- This represents the loss of two electrons from a neutral strontium atom, forming a stable [tex]\(Sr^{2+}\)[/tex] ion.
Correct Answer:
The correct equation representing the ionization of a neutral strontium atom to its most stable ion is:
[tex]\( E: Sr \rightarrow Sr^{2+} + 2 e^{-} \)[/tex]
1. Understanding Ionization:
- Ionization is the process by which an atom loses or gains electrons to form ions.
- Alkaline earth metals, such as strontium, commonly lose electrons to form positive ions (cations).
2. Strontium's Valence Electrons:
- Strontium (Sr) has an atomic number of 38, and its electron configuration is [tex]\([Kr] 5s^2\)[/tex].
- This means it has 2 electrons in its outermost shell.
3. Most Stable Ion:
- For strontium, losing these 2 valence electrons will lead to a stable, positively charged ion.
- The ion formed will be [tex]\(Sr^{2+}\)[/tex].
Given these points, let's evaluate the options:
A: [tex]\( Sr + e^{-} \rightarrow Sr \)[/tex]
- This equation represents the addition of an electron to a neutral strontium atom, which is not relevant to ionization into a stable ion.
B: [tex]\( Sr + 2 e^{-} \rightarrow Sr^{2-} \)[/tex]
- This equation also represents the addition of electrons, resulting in a negatively charged ion, which is not typical for strontium.
C: [tex]\( Sr (s) + 2 H_2 O(l) \rightleftharpoons Sr(OH)_2(aq) + H_2(g) \)[/tex]
- This is a chemical reaction involving strontium and water, not an ionization equation.
D: [tex]\( Sr \rightarrow Sr^{+} + e^{-} \)[/tex]
- This represents the loss of only one electron, forming a singly charged positive ion, [tex]\(Sr^+\)[/tex]. However, this is not the most stable form.
E: [tex]\( Sr \rightarrow Sr^{2+} + 2 e^{-} \)[/tex]
- This represents the loss of two electrons from a neutral strontium atom, forming a stable [tex]\(Sr^{2+}\)[/tex] ion.
Correct Answer:
The correct equation representing the ionization of a neutral strontium atom to its most stable ion is:
[tex]\( E: Sr \rightarrow Sr^{2+} + 2 e^{-} \)[/tex]
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