23-33 CHEM

Vocabulary practice flashcards covering electron configuration representations, orbital splitting, periodic table classification of elements, metal properties, and cation naming rules from the lecture notes.

Can be represented as a Box Diagram or as a Shell number with orbitals containing the appropriate number of electron(s).

Representations of Electron Configurations

Orbitals that remain unsplit in expanded electron configurations.

s-orbitals (Expanded Configuration)

Orbitals that are split into $p_x$, $p_y$, and $p_z$ orbitals in expanded electron configurations.

p-orbitals (Expanded Configuration)

Orbitals that are split into FIVE orbitals in expanded electron configurations.

d-orbitals (Expanded Configuration)

Orbitals that are split into SEVEN orbitals in expanded electron configurations.

f-orbitals (Expanded Configuration)

Orbitals that are split into NINE orbitals in expanded electron configurations.

g-orbitals (Expanded Configuration)

Elements including Group 1A-3A (20), Transition elements (40), Lanthanides (14), and Actinides (14).

Metals (Classification)

Elements including Group 4A-8A (17), with exceptions; Group 8A elements (6) are also known as Inert gas elements.

Non-Metals (Classification)

Elements classified as metalloids include B, Si, Ge, As, Sb, and Te.

Metalloids

The 6 non-metal elements located in Group 8A of the Periodic Table.

Inert Gas Elements

Metals donate or lose electron(s) to become CATIONS, where the positive charge corresponds to the position in the Periodic Table, represented as $n+$.

Properties of Metals (Cation Formation)

The principle of having Eight Electrons at the Valence Shell (VS); exceptions include Hydrogen, Transition elements, and Inner-transition elements.

Octet Rule

Elements of Groups 1A, 2A, and 3A form only one type of cation; the name of the cation is the name of the metal followed by the word "ion".

Naming of Cations (Groups 1A, 2A, 3A)

$H^+$ (Hydrogen ion), $Li^+$ (Lithium ion), $Na^+$ (Sodium ion), and $K^+$ (Potassium ion).

Group 1A Cations

$Mg^{2+}$ (Magnesium ion), $Ca^{2+}$ (Calcium ion), $Sr^{2+}$ (Strontium ion), and $Ba^{2+}$ (Barium ion).

Group 2A Cations

$Al^{3+}$ (Aluminum ion).

Group 3A Cation

$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1$, positioned at Group 3B.

Condensed Electronic Configuration of Scandium ($_{21}\text{Sc}$)

$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5$.

Condensed Electronic Configuration of Manganese ($_{25}\text{Mn}$)

$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10}$.

Condensed Electronic Configuration of Zinc ($_{30}\text{Zn}$)