Atomic Structure, Compounds, and Chemical Formulas

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Atomic Structure and Chemistry Fundamentals

Organic chemistry is the science of matter. All matter occupies space. Plasma is when atoms are in a high-temperature environment.

  • Elements: A single type of atom that cannot be transformed into simpler substances.
  • Compounds: Substances formed by different types of atoms combined in a constant ratio.
  • Homogeneous: Has a single phase, and components are indistinguishable (H2O + C6H12O6). Can be separated by evaporation or distillation.
  • Heterogeneous: Components can be distinguished from each other.
  • Phase: A portion of matter with definite limits. Can be separated by filtering or decanting.

d = mass / volume

Prefixes: milli (m) - 10-3 / micro (μ) - 10-6 / nano (n) - 10-9

1 kg = 1000 g and 1 dozen = 12 units

Temperature Conversions:

  • C° = 5 / 9 (F° - 32)
  • K° = C° + 273.15
  • F° = 9 / 5 (C° + 32)

Atomic Structure

The atomic theory of Dalton (1808) states that matter is made up of tiny particles called atoms.

  • Nucleus: Made up of protons and neutrons.
  • Electrons: Move away from the nucleus.

Particle Properties:

  • Proton (P+): Charge +1, Location: Nucleus, Mass: 1.67 x 10-24 g
  • Neutron (N0): Charge 0, Location: Nucleus, Mass: 1.67 x 10-24 g
  • Electron (e-): Charge -1, Location: Exterior, Mass: 9.11 x 10-28 g

Example: O8p+ = 8 x 1.97 x 10-19 = 1.576 x 10-18

Atoms differ in the number of neutrons and protons in their nucleus.

AZC, e.g., 126C

4019K+: P+ = 19, N0 = 21, e- = 18

Isotopes are atoms of the same element with a different number of neutrons in the nucleus.

Electron Configuration: 1s22s22p63s23p64s23d2

Quantum Numbers:

  • m = -1 for 3d2
  • s = 0 / p = 1 / d = 2 / f = 3
  • l = 2, then the sequence is -2, -1, 0, +1, +2
  • If s = +1/2, the rest are -1/2
  • n = 3
  • s = +1/2

Calculations with Moles and Atoms

Calcium has a mass of 40.8 g/mol. How many atoms are in 10g of Ca?

40.8 g contains 6.02 x 1023 atoms
10 g contains X atoms
X = 1.475 x 1023 atoms

Epinephrine: 59.0% C, 7.1% H, 26.2% O, 7.7% N

C = 59/12 = 4.91
H = 7.1/1.01 = 7.02
O = 26.2/16 = 1.63
N = 7.7/14 = 0.55
Divide by the smallest value (0.55):
C9H13O3N

How many molecules of quinine (C20H24O2N2) are in 1.08 g of quinine? How many moles?

C = 12 x 20 = 240
H = 1.01 x 24 = 24.24
O = 16 x 2 = 32
N = 14 x 2 = 28
Total molar mass = 324.24 g/mol

324.24 g contains 6.02 x 1023 molecules
1.08 g contains X molecules
X = 2.005 moles
XX = 2.01 x 1021 molecules

315 g of acetic acid (CH3COOH):

a) Moles of CH3COOH
C = 12 x 2 = 24
H = 1 x 4 = 4
O = 16 x 2 = 32
Molar mass = 60.04 g/mol
Moles = mass / molar mass = 315 g / 60.04 g/mol = 5.246 moles

b) Moles of each element
1 mol CH3COOH contains 2 mol C
5.246 mol CH3COOH contains X mol C
X = 10.492 mol C

c) Number of atoms of each element
315 g x (1 mol CH3COOH / 60.04 g/mol) x (2 mol C / 1 mol CH3COOH) x (6.02 x 1023 atoms / 1 mol C)
X = 6.32 x 1024 C atoms

SO3:
S = (32 x 1 / 80) x 100 = 40%
O = (16 x 3 / 80) x 100 = 60%

Ionic Compounds and Nomenclature

Ionic compound, ANION

  • K+ = Potassium ion
  • N3- = Nitride
  • O2- = Oxide
  • Br- = Bromide
  • CN- = Cyanide
  • Fe2+ = Ferrous ion
  • Fe3+ = Ferric ion
  • FeCl2 = Ferrous chloride
  • Mn2+: Manganese oxide MnO (II)
  • N2O4 = Nitrogen tetroxide
  • CH4 = Methane
  • HCl = Hydrochloric acid
  • H2SO4 = Sulfuric acid

Acid Nomenclature:

  • -1, Hypo-ous
  • -2, -ous
  • -3, -ic
  • -4, Per-ic

Anion Nomenclature:

  • -1, Hypo-ite
  • -2, -ite
  • -3, -ate
  • -4, Per-ate

Examples:

  • NaOH = Sodium hydroxide
  • KOH = Potassium hydroxide
  • Ba(OH)2 = Barium hydroxide
  • ClO- = Hypochlorite
  • ClO2- = Chlorite
  • ClO3- = Chlorate
  • ClO4- = Perchlorate
  • Mn(OH)2 = Manganese hydroxide
  • CO2 = Carbon dioxide
  • Al2O3 = Aluminum oxide
  • Cu2O = Cuprous oxide
  • HBrO = Hypobromous acid
  • Fe2O3 = Ferric oxide
  • KClO2 = Potassium chlorite
  • NH4OH = Ammonium hydroxide
  • MnO2 = Manganese dioxide
  • FeSO4 = Iron sulfate
  • H2Se = Selenhydric acid
  • CaCO3 = Calcium carbonate
  • NH3 = Ammonia
  • KClO3 = Potassium chlorate
  • HCl = Hydrochloric acid
  • KMnO4 = Potassium permanganate
  • RbH = Rubidium hydride
  • CsBr = Cesium bromide
  • HF = Hydrofluoric acid
  • CuSO4 x 5H2O = Copper sulfate pentahydrate
  • Ni(OH)3 = Nickel hydroxide
  • KHCO3 = Potassium bicarbonate (Potassium hydrogen carbonate)
  • NaHSO4 = Sodium bisulfate (Sodium hydrogen sulfate)
  • HClO2 = Chlorous acid
  • Mg(ClO2)2 = Magnesium chlorite
  • Au2Se3 = Auric selenide
  • ZnCl2 = Zinc chloride
  • Barium hydroxide = Ba(OH)2
  • Perbromic acid = HBrO4
  • Silver nitrate = AgNO3
  • Hydrogen sulfide = H2S
  • Sodium silicate = Na2SiO3
  • Aluminum sulfate = Al2(SO4)3
  • Calcium carbonate = CaCO3
  • Nitrogen dioxide = NO2
  • Hydrogen peroxide = H2O2
  • Mercuric oxide = HgO
  • Magnesium phosphate = Mg3(PO4)2
  • Aluminum fluoride = AlF3

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