Periodic Table Structure
📌 The periodic table organizes elements based on trends in their properties, divided into periods (horizontal rows) and groups (vertical columns).
⏳ There are seven periods: Period 1 (very short, 2 elements), Periods 2 & 3 (short, 8 elements each), Periods 4 & 5 (long, 18 elements each), Period 6 (very long, 30 elements, includes lanthanides), and Period 7 (includes actinides).
🏛️ Groups are categorized into main groups (Group A), transition groups (Group B), and inner transition groups (lanthanides and actinides).

Periodic Trends: Acidic/Basic Properties (Pianosa vs. Loriba)
🔬 Pianosa Properties (Acidic character, oxidation tendency, electronegativity, electron affinity) generally increase across a period (left to right) and decrease down a group.
🔧 Loriba Properties (Basicity, atomic radius, reducing strength, metallic character) are the opposite: they decrease across a period and increase down a group.
⚡️ Specifically for Pianosa properties, energy ionization extends its increase up to Group 8A.

Detailed Property Trends: Atomic Radius
📏 Atomic radius is the distance from the nucleus to the outermost occupied electron shell.
⬆️ In a group, the radius increases from top to bottom because the number of electron shells increases.
⬇️ In a period, the radius decreases from left to right because, despite having the same number of shells, the increasing nuclear charge (more protons) exerts a stronger pull on the electrons, drawing them closer to the nucleus (e.g., Mg radius is smaller than Na radius).

Detailed Property Trends: Ionization Energy and Electron Affinity
🔥 Ionization Energy (IE) is the energy required to remove the least tightly bound electron.
📉 IE decreases down a group (further distance from nucleus means weaker binding) and increases across a period (stronger nuclear pull).
⚡️ Electron Affinity (EA) is the energy released when an atom gains an electron; a more negative EA value indicates a greater tendency to attract electrons and form a negative ion.
➡️ EA generally increases (becomes more negative) across a period and decreases (becomes less negative) down a group.

Detailed Property Trends: Electronegativity
🔗 Electronegativity is the tendency of an atom to attract shared electron pairs in a bond.
📈 Electronegativity increases significantly from left to right across a period because atoms are trying harder to complete their valence shell.

Key Points & Insights
➡️ Understand the definitions of Periods (7 rows) and Groups (vertical columns) as the fundamental structure of the periodic table.
➡️ Atomic radius trend is dictated by two factors: Number of shells (dominates trends down a group) and Nuclear charge (dominates trends across a period).
➡️ Ionization Energy and Electronegativity are inversely related to atomic radius; smaller atoms generally require more energy to lose electrons and attract bonding electrons more strongly.
➡️ Remember the mnemonic for Loriba properties (Basicity, Radius, Reducer, Metal) which increase down a group.

📸 Video summarized with SummaryTube.com on Nov 20, 2025, 13:02 UTC