Language of Chemistry - Lecture Notes

Introduction

• Welcome and subscribe to the channel for updates on upcoming videos.
• This video focuses on the Language of Chemistry, a highly requested topic.
• Mention of Maths Mastery course for Class 8 students, covering all chapters of maths in detail.

Symbols in Chemistry

• Review of symbols from previous classes (Class 7, 8, and 9).
• Definition of Symbols: One or two-letter abbreviation of the name of an element. Examples:
  • Hydrogen (H) - 1st letter capital
  • Carbon (C) - 1st letter capital
  • Calcium (Ca) - first letter capital, second lower
  • Boron (B) - 1st letter capital
• Atomic Numbers: Remember atomic numbers from 1 to 20.
• Important symbols to remember:
  • H = Hydrogen
  • He = Helium
  • Li = Lithium
  • Be = Beryllium
  • C = Carbon
  • N = Nitrogen
  • O = Oxygen
  • F = Fluorine
  • Ne = Neon
  • Na = Sodium
  • Mg = Magnesium
  • Al = Aluminium
  • Si = Silicon
  • P = Phosphorus
  • S = Sulfur
  • Cl = Chlorine
  • Ar = Argon
  • K = Potassium
  • Ca = Calcium
  • Sc = Scandium
  • Ti = Titanium
  • V = Vanadium
  • Cr = Chromium
  • Mn = Manganese
  • Fe = Iron
  • Co = Cobalt
  • Ni = Nickel
  • Cu = Copper
  • Zn = Zinc
  • Ga = Gallium
  • Ge = Germanium
  • As = Arsenic
  • Se = Selenium
  • Br = Bromine
  • Kr = Krypton
  • Rb = Rubidium
  • Sr = Strontium
  • Y = Yttrium
  • Zr = Zirconium
  • Nb = Niobium
  • Mo = Molybdenum
  • Tc = Technetium
  • Ru = Ruthenium
  • Rh = Rhodium
  • Pd = Palladium
  • Ag = Silver
  • Cd = Cadmium
  • In = Indium
  • Sn = Tin
  • Sb = Antimony
  • Te = Tellurium
  • I = Iodine
  • Xe = Xenon
  • Cs = Cesium
  • Ba = Barium
  • La = Lanthanum
  • Ce = Cerium
  • Pr = Praseodymium
  • Nd = Neodymium
  • Pm = Promethium
  • Sm = Samarium
  • Eu = Europium
  • Gd = Gadolinium
  • Tb = Terbium
  • Dy = Dysprosium
  • Ho = Holmium
  • Er = Erbium
  • Tm = Thulium
  • Yb = Ytterbium
  • Lu = Lutetium
  • Hf = Hafnium
  • Ta = Tantalum
  • W = Tungsten
  • Re = Rhenium
  • Os = Osmium
  • Ir = Iridium
  • Pt = Platinum
  • Au = Gold
  • Hg = Mercury
  • Tl = Thallium
  • Pb = Lead
  • Bi = Bismuth
  • Po = Polonium
  • At = Astatine
  • Rn = Radon
  • Fr = Francium
  • Ra = Radium
  • Ac = Actinium
  • Th = Thorium
  • Pa = Protactinium
  • U = Uranium
  • Np = Neptunium
  • Pu = Plutonium
  • Am = Americium
  • Cm = Curium
  • Bk = Berkelium
  • Cf = Californium
  • Es = Einsteinium
  • Fm = Fermium
  • Md = Mendelevium
  • No = Nobelium
  • Lr = Lawrencium
  • Rf = Rutherfordium
  • Db = Dubnium
  • Sg = Seaborgium
  • Bh = Bohrium
  • Hs = Hassium
  • Mt = Meitnerium
  • Ds = Darmstadtium
  • Rg = Roentgenium
  • Cn = Copernicium
  • Nh = Nihonium
  • Fl = Flerovium
  • Mc = Moscovium
  • Lv = Livermorium
  • Ts = Tennessine
  • Og = Oganesson

Valency and Valence Electrons

• Valence Electrons: Electrons in the outermost shell (valence shell) of an atom.
  • Example: Oxygen (atomic number 8) has 6 valence electrons.
• Electronic Configuration:
  • Example for Oxygen: 2 electrons in K shell, 6 in L shell.
  • Valence Shell: Last shell where valence electrons are located.
• Valency: Capacity of an atom to donate or accept electrons to form a bond.
  • Example: Sodium loses 1 electron (valency 1), Magnesium loses 2 electrons (valency 2), Oxygen accepts 2 electrons (valency 2).

Cations and Anions

• Cations: Formed when an atom loses electrons, resulting in a positive charge.
  • Examples: Na+, Mg2+, Al3+.
• Anions: Formed when an atom gains electrons, resulting in a negative charge.
  • Examples: Cl-, O2-, N3-.

Variable Valency

• Some metals can exhibit more than one valency, known as Variable Valency.
  • Example: Copper can show +1 (Cu+) and +2 (Cu2+).
  • Iron shows +2 (Fe2+) and +3 (Fe3+).
• Naming Convention:
  • Metals with variable valency use Latin names for the suffix:
    • Cuprous (Cu+), Cupric (Cu2+), Ferrous (Fe2+), Ferric (Fe3+).

Ions

• Monoatomic Ions: Ions made of a single atom with a charge.
  • Examples: Na+, Cl-.
• Polyatomic Ions: Ions made of more than one atom with an overall charge.
  • Examples: NH4+ (ammonium), OH- (hydroxide), SO4^2- (sulfate).

Conclusion

• Summary of key concepts covered.
• Encouragement to practice and review the material.
• Announcement for the second part of the lecture, which will cover how to write chemical formulas of compounds.