Question

question 3. complete the statements by identifying the noble gas configuration achieved by the following ions:

1. the electron configuration of li⁺ matches the noble gas
2. the electron configuration of rb⁺ matches the noble gas
3. the electron configuration of cl⁻ matches the noble gas
4. mg²⁺ achieves the noble gas configuration of
5. ra²⁺ achieves the noble gas configuration of
6. o²⁻ achieves the noble gas configuration of
7. p³⁻ achieves the noble gas configuration of

Explanation:

Step1: Analyze \( \text{Li}^+ \)

Lithium (Li) has an atomic number of 3, so \( \text{Li} \) has 3 electrons. When \( \text{Li} \) loses 1 electron to form \( \text{Li}^+ \), it has \( 3 - 1 = 2 \) electrons. The noble gas with 2 electrons is Helium (He).

Step2: Analyze \( \text{Rb}^+ \)

Rubidium (Rb) has an atomic number of 37, so \( \text{Rb} \) has 37 electrons. When \( \text{Rb} \) loses 1 electron to form \( \text{Rb}^+ \), it has \( 37 - 1 = 36 \) electrons. The noble gas with 36 electrons is Krypton (Kr).

Step3: Analyze \( \text{Cl}^- \)

Chlorine (Cl) has an atomic number of 17, so \( \text{Cl} \) has 17 electrons. When \( \text{Cl} \) gains 1 electron to form \( \text{Cl}^- \), it has \( 17 + 1 = 18 \) electrons. The noble gas with 18 electrons is Argon (Ar).

Step4: Analyze \( \text{Mg}^{2+} \)

Magnesium (Mg) has an atomic number of 12, so \( \text{Mg} \) has 12 electrons. When \( \text{Mg} \) loses 2 electrons to form \( \text{Mg}^{2+} \), it has \( 12 - 2 = 10 \) electrons. The noble gas with 10 electrons is Neon (Ne).

Step5: Analyze \( \text{Ra}^{2+} \)

Radium (Ra) has an atomic number of 88, so \( \text{Ra} \) has 88 electrons. When \( \text{Ra} \) loses 2 electrons to form \( \text{Ra}^{2+} \), it has \( 88 - 2 = 86 \) electrons. The noble gas with 86 electrons is Radon (Rn).

Step6: Analyze \( \text{O}^{2-} \)

Oxygen (O) has an atomic number of 8, so \( \text{O} \) has 8 electrons. When \( \text{O} \) gains 2 electrons to form \( \text{O}^{2-} \), it has \( 8 + 2 = 10 \) electrons. The noble gas with 10 electrons is Neon (Ne).

Step7: Analyze \( \text{P}^{3-} \)

Phosphorus (P) has an atomic number of 15, so \( \text{P} \) has 15 electrons. When \( \text{P} \) gains 3 electrons to form \( \text{P}^{3-} \), it has \( 15 + 3 = 18 \) electrons. The noble gas with 18 electrons is Argon (Ar).

Answer:

s (for each sub - question):

1. The electron configuration of \( \text{Li}^+ \) matches the noble gas \(\boldsymbol{\text{Helium (He)}}\).
2. The electron configuration of \( \text{Rb}^+ \) matches the noble gas \(\boldsymbol{\text{Krypton (Kr)}}\).
3. The electron configuration of \( \text{Cl}^- \) matches the noble gas \(\boldsymbol{\text{Argon (Ar)}}\).
4. \( \text{Mg}^{2+} \) achieves the noble gas configuration of \(\boldsymbol{\text{Neon (Ne)}}\).
5. \( \text{Ra}^{2+} \) achieves the noble gas configuration of \(\boldsymbol{\text{Radon (Rn)}}\).
6. \( \text{O}^{2-} \) achieves the noble gas configuration of \(\boldsymbol{\text{Neon (Ne)}}\).
7. \( \text{P}^{3-} \) achieves the noble gas configuration of \(\boldsymbol{\text{Argon (Ar)}}\).