Atomic Structure, Compounds, and Chemical Formulas
Classified in Chemistry
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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