Introduction to s and p Block Elements Lecture 1 PDF

Introduction to s and p Block Elements This session explores the fascinating world of s and p block elements, their properties, trends, and applications. Dr. Nesma A. Fekry...

Introduction to s and p Block Elements This session explores the fascinating world of s and p block elements, their properties, trends, and applications. Dr. Nesma A. Fekry preencoded.png Groups and Periods 1 8 1 2 3 4 5 6 7 2 3 4 5 6 7 preencoded.png  Group Classification P d F Alkali Alkali Metals Earth Metals preencoded.png Valence Electron Configuration Block Valence Electron Configuration s Block ns1 or ns2 p Block ns2 np1-6 preencoded.png Electronegativity and Ionization Energy Electronegativity Electronegativity is the tendency of an atom to attract electrons. Electronegativity increases across a period and decreases down a group in the periodic table. Ionization Energy Ionization energy is the energy required to remove an electron from an atom. Ionization energy generally increases across a period and decreases down a group. preencoded.png Chemical Reactivity and Trends preencoded.png Chemical Reactivity and Trends Down a Group Reactivity increases down a group for both s and p block elements. This is because the valence electrons are further away from the nucleus and easier to remove. Across a Period For s block elements, reactivity decreases across a period. For p block elements, the reactivity is more complex and influenced by electronegativity and ionization energy. Oxidation States The oxidation state of an element is the charge it would have if it were a monatomic ion. The oxidation states of s and p block elements vary depending on their position in the periodic table. preencoded.png Characteristics of s Block Elements 1 Highly Reactive 2 Low Ionization Energy Most s block elements are They readily lose their valence highly reactive, particularly the electrons to form cations, alkali metals in Group 1. often forming ionic bonds with nonmetals. 3 Good Conductors 4 Form Strong Bases The alkali metals are excellent When s block elements react conductors of electricity and with water, they form strong heat due to their loosely bound bases, which are highly valence electrons. alkaline. preencoded.png  Metals (83) Non-Metals (16) Metals can be found on Metals can be found on the left and in the middle the Right of the periodic of the periodic table table Semi-Metals (8) Metalloids B, Si, Ge, As, Sb, Te, Po, At preencoded.png  Metals Semi-Metals Non-Metals Vary 1. All are1. greatly Intermediate solids in appearance atbetween except mercury 25oC and 1 atm Carbon ,metals 2. Lustrous appearanceand Phosphorous, nonSelenium, Sulfur, metals Sulfur and2. 3. Readily they iodine areheat are solids conduct semiconductors, and Discover with me Bromine is liquid electricity Hydrogen, intermediate oxygen, fluorine areelectrical and diatomic gases Nobel 4. Can be gasesthermal squeezed conductivities. ; He, Ne,Ar, orKr, Xe and Rn hammered into 3.variousBrittles shapes (malleable) 5. 1. Drawn 4. intoTheir Insulators oxides wires are amphoteric (low(ductile) thermal and 6. Oxides 5. ofHalides electrical metals and arehydrides conductivity basic eg;are O volatile Na2Neither 2. covalent malleable norcompounds ductile. 7. 3. Halides, Oxides (oxides low of mp) and hydrides nonmetals are ofacidic metals 6. SO2 eg: are1.8 ≤ Electronegativity ionic compounds < ( high 4. mp, Halides, 2.2bp and and oxides non hydrides volatile) of 8. 0.7 ≤ Electronegativity metals are volatile covalent < 1.8 9. Form positive (low compounds ions, mp, Na+bp e.g. low , ) preencoded.png Mg2+2.2 5. , and ≤ Electronegativity Al3+