Question

1. a) write the full and condensed electron configuration for one of the following: sc, ga or ge. b) what charge would you expect on your chosen elements ion? explain/show why in terms of electrons lost or gained. part a: knowledge and understanding multiple choice (10 marks) - done on minds online true and false (10 marks) - done on minds online matching (3 marks) - done on minds online multi - select (2 marks) - done on minds online part b: thinking and inquiry please use a different colour for your solutions (if typing) overall expectations: c2 and c3 not yet level 1 55% 12 - 14 level 2 65% 15 - 17 level 3 75% 18 - 19 level 4 85% 20 - 22 level 4+ 95% 23 level 4++ 100% 24 - 25 structure and properties of matter - summative #1 sch 4u - el

Explanation:

Step1: Recall electron - configuration rules

Electrons are filled in orbitals according to the Aufbau principle, Pauli - exclusion principle, and Hund's rule. For ions, electrons are either lost (for cations) or gained (for anions).

Step2: Analyze Scandium (Sc)

Sc has an atomic number of 21. Its ground - state electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{1}$. When Sc forms a cation, it loses electrons starting from the outermost shell. Sc typically forms $Sc^{3 + }$. The electron configuration of $Sc^{3+}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$, which is a noble - gas configuration (argon - like). It loses 2 electrons from the 4s orbital and 1 electron from the 3d orbital. The charge is + 3 because it loses 3 electrons.

Step3: Analyze Gallium (Ga)

Ga has an atomic number of 31. Its ground - state electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{1}$. Ga typically forms $Ga^{3+}$. It loses 2 electrons from the 4s orbital and 1 electron from the 4p orbital. The electron configuration of $Ga^{3+}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}$, and the charge is + 3.

Step4: Analyze Germanium (Ge)

Ge has an atomic number of 32. Its ground - state electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{2}$. Ge can form $Ge^{4+}$. It loses 2 electrons from the 4s orbital and 2 electrons from the 4p orbital. The electron configuration of $Ge^{4+}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}$, and the charge is + 4.

Let's assume we choose Sc as an example for part (a):
The full electron configuration of $Sc^{3+}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$. The condensed electron configuration is $[Ar]$. It loses 3 electrons, so the charge is + 3. The reason is that Sc, with its outer - shell configuration of $4s^{2}3d^{1}$, loses electrons from the 4s and 3d orbitals to achieve a stable noble - gas configuration.

For part (b), if Sc forms $Sc^{3+}$, it loses 3 electrons.

Answer:

For part (a) (using Sc as an example): Full electron configuration: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$, Condensed electron configuration: $[Ar]$.
For part (b) (using Sc as an example): Charge is + 3, 3 electrons are lost.