Periodic Table and Basic Chemistry Concepts

Periodic Table of the Elements

  • Hydrogen (H) 1.00794
  • Helium (He) 4.003
  • Lithium (Li) 6.941
  • Beryllium (Be) 9.012182
  • Boron (B) 10.811
  • Carbon (C) 12.0107
  • Nitrogen (N) 14.00674
  • Oxygen (O) 15.9994
  • Fluorine (F) 18.9984032
  • Neon (Ne) 20.1797
  • Sodium (Na) 22.989770
  • Magnesium (Mg) 24.3050
  • Aluminum (Al) 26.981538
  • Silicon (Si) 28.0855
  • Phosphorus (P) 30.973761
  • Sulfur (S) 32.066
  • Chlorine (Cl) 35.4527
  • Argon (Ar) 39.948
  • Potassium (K) 39.0983
  • Calcium (Ca) 40.078
  • Scandium (Sc) 44.955910
  • Titanium (Ti) 47.867
  • Vanadium (V) 50.9415
  • Chromium (Cr) 51.9961
  • Iron (Fe) 55.845
  • Cobalt (Co) 58.933200
  • Nickel (Ni) 58.6934
  • Copper (Cu) 63.546
  • Zinc (Zn) 65.39
  • Gallium (Ga) 69.723
  • Germanium (Ge) 72.61
  • Arsenic (As) 74.92160
  • Selenium (Se) 78.971
  • Bromine (Br) 79.904
  • Krypton (Kr) 83.80
  • Rubidium (Rb) 85.4678
  • Strontium (Sr) 87.62
  • Yttrium (Y) 88.90585
  • Zirconium (Zr) 91.224
  • Niobium (Nb) 92.90638
  • Molybdenum (Mo) 95.94
  • Technetium (Tc) 98 (not commonly seen in standard periodic tables)
  • Ruthenium (Ru) 101.07
  • Rhodium (Rh) 102.90550
  • Palladium (Pd) 106.42
  • Silver (Ag) 107.8682
  • Cadmium (Cd) 112.411
  • Indium (In) 114.818
  • Tin (Sn) 118.710
  • Antimony (Sb) 121.760
  • Tellurium (Te) 127.60
  • Iodine (I) 126.90447
  • Xenon (Xe) 131.29
  • Cesium (Cs) 132.90545
  • Barium (Ba) 137.327
  • Lanthanum (La) 138.9055
  • Hafnium (Hf) 178.49
  • Tantalum (Ta) 180.9479
  • Tungsten (W) 183.84
  • Osmium (Os) 190.23
  • Iridium (Ir) 192.217
  • Platinum (Pt) 195.078
  • Gold (Au) 196.96655
  • Mercury (Hg) 200.59
  • Thallium (Tl) 204.3833
  • Lead (Pb) 207.2
  • Bismuth (Bi) 208.98038
  • Polonium (Po) (209)
  • Astatine (At) (210)
  • Radon (Rn) (222)
  • Francium (Fr) (223)
  • Radium (Ra) (226)
  • Actinium (Ac) (227)
  • Rutherfordium (Rf) (261)
  • Dubnium (Db) (262)
  • Seaborgium (Sg) (263)
  • Bohrium (Bh) (264)
  • Hassium (Hs) (265)
  • Meitnerium (Mt) (266)
  • Darmstadtium (Ds) (270)

Chemical Equations and Concepts

  • Molarity (M)

    • Definition: Molarity is defined as the number of moles of solute per liter of solution, given by the formula:
      M=nVM = \frac{n}{V}
      where:
    • n = number of moles of solute
    • V = volume of solution in liters

  • Ideal Gas Law (R)

    • The ideal gas constant can take two forms:
      R=8.314JmolimesKR = 8.314 \frac{J}{mol imes K}
      R=0.08206LimesatmmolimesKR = 0.08206 \frac{L imes atm}{mol imes K}
    • Note: Standard temperature is defined as 0°C, which is equivalent to 273.15 K.

  • Molality (m)

    • Definition: Molality is defined as the number of moles of solute per kilogram of solvent, given by the formula:
      m=nmsolventm = \frac{n}{m_{solvent}}

  • Equilibrium Constants

    • For a reaction:
      HA + H_2O
      ightleftharpoons H_3O^+ + A^-
      The equilibrium constant (K) is defined as:
      K=[H3O+][A−][HA]K = \frac{[H_3O^+][A^-]}{[HA]}
    • Another general expression for a reaction:
      B + H_2O
      ightleftharpoons HB^+ + OH^-
      The equilibrium constant (K') is given by:
      K′=[HB+][OH−][B]K' = \frac{[HB^+][OH^-]}{[B]}
    • Relationship between equilibrium constants:
      Kp=Kc(RT)rianglenK_p = K_c(RT)^{ riangle n}
    • The values for concentrations, pressure, and pH are critical in using these formulas.

  • Acid-Base Concepts

    • pH is defined by the formula:
      pH=−extlog[H3O+]pH = - ext{log}[H_3O^+]
    • pOH is defined similarly:
      pOH=−extlog[OH−]pOH = - ext{log}[OH^-]
    • The relationship between concentrations and pH is given by:
      [H3O+]=10−pH[H_3O^+] = 10^{-pH},
      [OH−]=10−pOH[OH^-] = 10^{-pOH}

  • Water Dissociation Constant (K_w)

    • The product of the concentrations of hydronium and hydroxide ions at 25°C is:
      Kw=1.0imes10−14K_w = 1.0 imes 10^{-14}

  • Henderson-Hasselbalch Equation

    • Used in buffer solution calculations:
      pH=pKa+extlog[base][acid]pH = pK_a + ext{log} \frac{[base]}{[acid]}
    • Notable definitions linked to these concepts include:
    • pK_a = -log K_a
    • pK_b = -log K_b

  • Acid-Base Neutralization Reactions

    • Example reactions include:
    • HA + OH^-
      ightarrow A^- + H_2O (weak acid with strong base)
    • B + H^+
      ightarrow BH^+ (weak base with strong acid)

  • pK Relationships

    • The relationship between pK_a and pK_b is given by:
      pKa+pKb=14.00=pKwpK_a + pK_b = 14.00 = pK_w