Question
Predict the ground state configuration for each and explain your answer (a) Ra²+ (b) y³+ (c)T⁴+ (d)N³- (e)fe³+ (f) P³- (g) O²-
(2) which atom in each of the following pair would you expect to be larger(a) MG or B (b) Si or Sn (c) Os or Lu
(2) which atom in each of the following pair would you expect to be larger(a) MG or B (b) Si or Sn (c) Os or Lu
Answers
GPT-4o mini
### Ground State Configuration Predictions
To determine the ground state electron configuration of each ion, we start with the atomic number of the neutral element, adjust for the number of electrons lost or gained due to ionization, and follow the order of filling based on the Aufbau principle.
(a) **Ra²+ (Radium ion)**:
- Atomic number of Radium (Ra) = 88
- For Ra²+, we remove 2 electrons from its neutral state.
- Neutral configuration: \[ \text{[Rn]} \, 7s^2 \]
- After removing 2 electrons: \[ \text{[Rn]} \]
(b) **Y³+ (Yttrium ion)**:
- Atomic number of Yttrium (Y) = 39
- For Y³+, we remove 3 electrons.
- Neutral configuration: \[ \text{[Kr]} \, 5s^2 \, 4d^1 \]
- After removing 3 electrons (removing 2 from 5s and 1 from 4d): \[ \text{[Kr]} \]
(c) **T⁴+ (Titanium ion)**:
- Atomic number of Titanium (Ti) = 22
- For Ti⁴+, we remove 4 electrons.
- Neutral configuration: \[ \text{[Ar]} \, 4s^2 \, 3d^2 \]
- After removing 4 electrons (2 from 4s and 2 from 3d): \[ \text{[Ar]} \]
(d) **N³- (Nitride ion)**:
- Atomic number of Nitrogen (N) = 7
- For N³-, we gain 3 electrons.
- Neutral configuration: \[ 1s^2 \, 2s^2 \, 2p^3 \]
- After gaining 3 electrons: \[ 1s^2 \, 2s^2 \, 2p^6 \] (which is the configuration of Neon, Ne)
(e) **Fe³+ (Iron ion)**:
- Atomic number of Iron (Fe) = 26
- For Fe³+, we remove 3 electrons.
- Neutral configuration: \[ \text{[Ar]} \, 4s^2 \, 3d^6 \]
- After removing 3 electrons (2 from 4s and 1 from 3d): \[ \text{[Ar]} \, 3d^5 \]
(f) **P³- (Phosphide ion)**:
- Atomic number of Phosphorus (P) = 15
- For P³-, we gain 3 electrons.
- Neutral configuration: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^3 \]
- After gaining 3 electrons: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \] (which is the configuration of Argon, Ar)
(g) **O²- (Oxide ion)**:
- Atomic number of Oxygen (O) = 8
- For O²-, we gain 2 electrons.
- Neutral configuration: \[ 1s^2 \, 2s^2 \, 2p^4 \]
- After gaining 2 electrons: \[ 1s^2 \, 2s^2 \, 2p^6 \] (which is the configuration of Neon, Ne)
### Summary of Ground State Configurations
- (a) Ra²+: \[ \text{[Rn]} \]
- (b) Y³+: \[ \text{[Kr]} \]
- (c) T⁴+: \[ \text{[Ar]} \]
- (d) N³-: \[ \text{Ne} \]
- (e) Fe³+: \[ \text{[Ar]} \, 3d^5 \]
- (f) P³-: \[ \text{Ar} \]
- (g) O²-: \[ \text{Ne} \]
### Which Atom is Larger?
(a) **Mg or B**: Mg (Magnesium) is larger. Both are in the same period (period 2 for B and period 3 for Mg), and since Mg has one more shell, it is larger.
(b) **Si or Sn**: Sn (Tin) is larger. Sn is further down the periodic table (group 14) compared to Si (also group 14 but in period 3). As we go down a group, atomic size increases due to additional electron shells.
(c) **Os or Lu**: Lu (Lutetium) is slightly larger than Os (Osmium). Although they are close in terms of atomic numbers (Os = 76 and Lu = 71), Lu has more electron shells contributing to a larger atomic radius. However, the differences are relatively minor compared to typical trends in a group.
### Summary of Size Comparisons
- (a) Mg is larger than B.
- (b) Sn is larger than Si.
- (c) Lu is slightly larger than Os.
To determine the ground state electron configuration of each ion, we start with the atomic number of the neutral element, adjust for the number of electrons lost or gained due to ionization, and follow the order of filling based on the Aufbau principle.
(a) **Ra²+ (Radium ion)**:
- Atomic number of Radium (Ra) = 88
- For Ra²+, we remove 2 electrons from its neutral state.
- Neutral configuration: \[ \text{[Rn]} \, 7s^2 \]
- After removing 2 electrons: \[ \text{[Rn]} \]
(b) **Y³+ (Yttrium ion)**:
- Atomic number of Yttrium (Y) = 39
- For Y³+, we remove 3 electrons.
- Neutral configuration: \[ \text{[Kr]} \, 5s^2 \, 4d^1 \]
- After removing 3 electrons (removing 2 from 5s and 1 from 4d): \[ \text{[Kr]} \]
(c) **T⁴+ (Titanium ion)**:
- Atomic number of Titanium (Ti) = 22
- For Ti⁴+, we remove 4 electrons.
- Neutral configuration: \[ \text{[Ar]} \, 4s^2 \, 3d^2 \]
- After removing 4 electrons (2 from 4s and 2 from 3d): \[ \text{[Ar]} \]
(d) **N³- (Nitride ion)**:
- Atomic number of Nitrogen (N) = 7
- For N³-, we gain 3 electrons.
- Neutral configuration: \[ 1s^2 \, 2s^2 \, 2p^3 \]
- After gaining 3 electrons: \[ 1s^2 \, 2s^2 \, 2p^6 \] (which is the configuration of Neon, Ne)
(e) **Fe³+ (Iron ion)**:
- Atomic number of Iron (Fe) = 26
- For Fe³+, we remove 3 electrons.
- Neutral configuration: \[ \text{[Ar]} \, 4s^2 \, 3d^6 \]
- After removing 3 electrons (2 from 4s and 1 from 3d): \[ \text{[Ar]} \, 3d^5 \]
(f) **P³- (Phosphide ion)**:
- Atomic number of Phosphorus (P) = 15
- For P³-, we gain 3 electrons.
- Neutral configuration: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^3 \]
- After gaining 3 electrons: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \] (which is the configuration of Argon, Ar)
(g) **O²- (Oxide ion)**:
- Atomic number of Oxygen (O) = 8
- For O²-, we gain 2 electrons.
- Neutral configuration: \[ 1s^2 \, 2s^2 \, 2p^4 \]
- After gaining 2 electrons: \[ 1s^2 \, 2s^2 \, 2p^6 \] (which is the configuration of Neon, Ne)
### Summary of Ground State Configurations
- (a) Ra²+: \[ \text{[Rn]} \]
- (b) Y³+: \[ \text{[Kr]} \]
- (c) T⁴+: \[ \text{[Ar]} \]
- (d) N³-: \[ \text{Ne} \]
- (e) Fe³+: \[ \text{[Ar]} \, 3d^5 \]
- (f) P³-: \[ \text{Ar} \]
- (g) O²-: \[ \text{Ne} \]
### Which Atom is Larger?
(a) **Mg or B**: Mg (Magnesium) is larger. Both are in the same period (period 2 for B and period 3 for Mg), and since Mg has one more shell, it is larger.
(b) **Si or Sn**: Sn (Tin) is larger. Sn is further down the periodic table (group 14) compared to Si (also group 14 but in period 3). As we go down a group, atomic size increases due to additional electron shells.
(c) **Os or Lu**: Lu (Lutetium) is slightly larger than Os (Osmium). Although they are close in terms of atomic numbers (Os = 76 and Lu = 71), Lu has more electron shells contributing to a larger atomic radius. However, the differences are relatively minor compared to typical trends in a group.
### Summary of Size Comparisons
- (a) Mg is larger than B.
- (b) Sn is larger than Si.
- (c) Lu is slightly larger than Os.