Question

magnesium atom magnesium ion
atomic number: mass number: protons: neutrons: electrons: cation/anion: ion symbol:
aluminum atom aluminum ion
atomic number: mass number: protons: neutrons: electrons: cation/anion: ion symbol:
phosphorus atom phosphorus ion
atomic number: mass number: protons: neutrons: electrons: cation/anion: ion symbol:
sulfur atom sulfur ion
atomic number: mass number: protons: neutrons: electrons: cation/anion: ion symbol:
chlorine atom chlorine ion
atomic number: mass number: protons: neutrons: electrons: cation/anion: ion symbol:

Answer:

To solve this, we analyze each element (Magnesium, Aluminum, Phosphorus, Sulfur, Chlorine) for atoms and ions:

1. Magnesium (Mg)

• Atomic number (protons): \( 12 \) (Mg is element 12).
• Mass number: Typically \( 24 \) (most common isotope: \( ^{24}\text{Mg} \)).
• Neutrons: \( \text{Mass number} - \text{Atomic number} = 24 - 12 = 12 \).
• Electrons (atom): Equal to protons (\( 12 \)) (neutral atom).
• Electrons (ion): Mg loses 2 electrons (forms \( \text{Mg}^{2+} \)), so \( 12 - 2 = 10 \).
• Cation/Anion: Cation (loses electrons, positive charge).
• Ion symbol: \( \text{Mg}^{2+} \).

2. Aluminum (Al)

• Atomic number: \( 13 \) (Al is element 13).
• Mass number: Typically \( 27 \) (most common isotope: \( ^{27}\text{Al} \)).
• Neutrons: \( 27 - 13 = 14 \).
• Electrons (atom): \( 13 \) (neutral).
• Electrons (ion): Al loses 3 electrons (forms \( \text{Al}^{3+} \)), so \( 13 - 3 = 10 \).
• Cation/Anion: Cation.
• Ion symbol: \( \text{Al}^{3+} \).

3. Phosphorus (P)

• Atomic number: \( 15 \) (P is element 15).
• Mass number: Typically \( 31 \) (most common isotope: \( ^{31}\text{P} \)).
• Neutrons: \( 31 - 15 = 16 \).
• Electrons (atom): \( 15 \) (neutral).
• Electrons (ion): P gains 3 electrons (forms \( \text{P}^{3-} \)), so \( 15 + 3 = 18 \).
• Cation/Anion: Anion (gains electrons, negative charge).
• Ion symbol: \( \text{P}^{3-} \).

4. Sulfur (S)

• Atomic number: \( 16 \) (S is element 16).
• Mass number: Typically \( 32 \) (most common isotope: \( ^{32}\text{S} \)).
• Neutrons: \( 32 - 16 = 16 \).
• Electrons (atom): \( 16 \) (neutral).
• Electrons (ion): S gains 2 electrons (forms \( \text{S}^{2-} \)), so \( 16 + 2 = 18 \).
• Cation/Anion: Anion.
• Ion symbol: \( \text{S}^{2-} \).

5. Chlorine (Cl)

• Atomic number: \( 17 \) (Cl is element 17).
• Mass number: Typically \( 35 \) (most common isotope: \( ^{35}\text{Cl} \); or \( 37 \), but \( 35 \) is more abundant).
• Neutrons: \( 35 - 17 = 18 \) (for \( ^{35}\text{Cl} \)).
• Electrons (atom): \( 17 \) (neutral).
• Electrons (ion): Cl gains 1 electron (forms \( \text{Cl}^- \)), so \( 17 + 1 = 18 \).
• Cation/Anion: Anion.
• Ion symbol: \( \text{Cl}^- \).

Filling the Table (Example for Magnesium; repeat for others):

	Magnesium Atom	Magnesium Ion
Mass number	\( 24 \)	\( 24 \)
Protons	\( 12 \)	\( 12 \)
Neutrons	\( 12 \)	\( 12 \)
Electrons	\( 12 \)	\( 10 \)
Cation/Anion	-	Cation
Ion symbol	-	\( \text{Mg}^{2+} \)

Repeat this structure for Aluminum, Phosphorus, Sulfur, and Chlorine using their respective values.

Key Rules:

• Atomic number = protons (never changes for an element).
• Mass number = protons + neutrons (stable isotope, e.g., \( ^{24}\text{Mg} \), \( ^{27}\text{Al} \), etc.).
• Electrons (atom) = protons (neutral).
• Electrons (ion): Cations lose electrons (\( \text{Mg}^{2+} \), \( \text{Al}^{3+} \)); Anions gain electrons (\( \text{P}^{3-} \), \( \text{S}^{2-} \), \( \text{Cl}^- \)).

For example, the full table (abbreviated) would look like:

Element	Atom/ Ion	Atomic #	Mass #	Protons	Neutrons	Electrons	Cation/Anion	Ion Symbol
Magnesium	Ion	\( 12 \)	\( 24 \)	\( 12 \)	\( 12 \)	\( 10 \)	Cation	\( \text{Mg}^{2+} \)
Aluminum	Atom	\( 13 \)	\( 27 \)	\( 13 \)	\( 14 \)	\( 13 \)	-	-
Aluminum	Ion	\( 13 \)	\( 27 \)	\( 13 \)	\( 14 \)	\( 10 \)	Cation	\( \text{Al}^{3+} \)
Phosphorus	Atom	\( 15 \)	\( 31 \)	\( 15 \)	\( 16 \)	\( 15 \)	-	-
Phosphorus	Ion	\( 15 \)	\( 31 \)	\( 15 \)	\( 16 \)	\( 18 \)	Anion	\( \text{P}^{3-} \)
Sulfur	Atom	\( 16 \)	\( 32 \)	\( 16 \)	\( 16 \)	\( 16 \)	-	-
Sulfur	Ion	\( 16 \)	\( 32 \)	\( 16 \)	\( 16 \)	\( 18 \)	Anion	\( \text{S}^{2-} \)
Chlorine	Atom	\( 17 \)	\( 35 \)	\( 17 \)	\( 18 \)	\( 17 \)	-	-
Chlorine	Ion	\( 17 \)	\( 35 \)	\( 17 \)	\( 18 \)	\( 18 \)	Anion	\( \text{Cl}^- \)

This follows the rules of atomic structure (protons = atomic number, neutrons = mass - atomic, electrons adjust for charge) and ion formation (metals lose electrons, nonmetals gain electrons).