Question

prepwork part 1: for each of the atoms/ions below, write the full electron configuration. 1. *neutral atom of cobalt 2. chlorine ion with a charge of - 1 for each of the atoms/ions below, write the abbreviated notation. 1. *neutral atom of iodine 2. neutral atom of vanadium for each of the atoms/ions below, write the orbital notation. 1. oxygen ion with a charge of - 2 2. neutral atom of sodium 1. write the electron configuration of an ion that is isoelectronic to na. include the ion’s name and charge. (there is more than one possible answer!) 2. two students are studying an ion that has similar properties to al. they determine that it is isoelectronic to al. they also know based on evidence that this ion is positively charged. student a says that the ion must be: p³⁺ student b says that the ion must be: si⁺¹ with which student do you agree, and why? 3. bismuth is the main ingredient in pepto - bismol, the popular drug used to cure digestive ailments. in victorian times, before bismuth was well known as a digestive aid, people used a different metal

Explanation:

Step1: Recall electron - configuration rules

Electrons fill orbitals in the order of increasing energy: 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p. The s - orbital can hold 2 electrons, the p - orbital can hold 6 electrons, the d - orbital can hold 10 electrons, and the f - orbital can hold 14 electrons.

Step2: Find electron configurations for given atoms/ions

Neutral atom of cobalt (Co)

Cobalt has an atomic number of 27. Its full electron configuration is 1s²2s²2p⁶3s²3p⁶4s²3d⁷.

Chlorine ion with a charge of - 1 (Cl⁻)

Chlorine has an atomic number of 17. Cl⁻ has 18 electrons. Its full electron configuration is 1s²2s²2p⁶3s²3p⁶.

Neutral atom of iodine (I)

Iodine has an atomic number of 53. Its abbreviated notation uses the noble - gas core of krypton (Kr). Kr has 36 electrons. So the abbreviated notation is [Kr]5s²4d¹⁰5p⁵.

Neutral atom of vanadium (V)

Vanadium has an atomic number of 23. Its abbreviated notation using the argon (Ar) core (Ar has 18 electrons) is [Ar]4s²3d³.

Oxygen ion with a charge of - 2 (O²⁻)

Oxygen has an atomic number of 8. O²⁻ has 10 electrons. Its orbital notation:
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓

Neutral atom of sodium (Na)

Sodium has an atomic number of 11. Its orbital notation:
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑

Ion isoelectronic to Na

Neon (Ne) has 10 electrons and if we consider a positive ion, Mg⁺ has 11 electrons. The electron configuration of Mg⁺ is 1s²2s²2p⁶3s¹. Another example is Na itself (but we can also consider other ions). If we take a negative ion, F⁻ has 10 electrons and is isoelectronic to Ne.

Comparing student answers for ion similar to Al

Aluminum has an atomic number of 13. Its electron configuration is 1s²2s²2p⁶3s²3p¹.
Si⁺ has 13 electrons (silicon has 14 electrons originally, Si⁺ has lost 1 electron), and its electron configuration is 1s²2s²2p⁶3s²3p¹ which is isoelectronic to Al. P³⁺ has 13 electrons (phosphorus has 15 electrons originally, P³⁺ has lost 3 electrons), and its electron configuration is also 1s²2s²2p⁶3s²3p¹. Both students are correct as both Si⁺ and P³⁺ are isoelectronic to Al and have similar properties in terms of electron - shell structure.

Answer:

1. Neutral atom of cobalt: 1s²2s²2p⁶3s²3p⁶4s²3d⁷
2. Chlorine ion with a charge of - 1: 1s²2s²2p⁶3s²3p⁶
3. Neutral atom of iodine: [Kr]5s²4d¹⁰5p⁵
4. Neutral atom of vanadium: [Ar]4s²3d³
5. Oxygen ion with a charge of - 2: Orbital notation: 1s: ↑↓; 2s: ↑↓; 2p: ↑↓ ↑↓ ↑↓
6. Neutral atom of sodium: Orbital notation: 1s: ↑↓; 2s: ↑↓; 2p: ↑↓ ↑↓ ↑↓; 3s: ↑
7. Ion isoelectronic to Na: Mg⁺ (1s²2s²2p⁶3s¹)
8. For the ion similar to Al: Both Student A (Si⁺) and Student B (P³⁺) are correct as both are isoelectronic to Al.