Input interpretation
1c of 1, 3-butadiene
Unit conversions
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Lewis structure
Draw the Lewis structure of 1, 3-butadiene. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4) and hydrogen (n_H, val = 1) atoms: 4 n_C, val + 6 n_H, val = 22 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8) and hydrogen (n_H, full = 2): 4 n_C, full + 6 n_H, full = 44 Subtracting these two numbers shows that 44 - 22 = 22 bonding electrons are needed. Each bond has two electrons, so in addition to the 9 bonds already present in the diagram add 2 bonds. To minimize formal charge carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |
Chemical names and formulas
formula | CH_2=CHCH=CH_2 Hill formula | C_4H_6 name | 1, 3-butadiene IUPAC name | buta-1, 3-diene
Substance properties
molar mass | 54.09 g/mol phase | gas (at STP) melting point | -109 °C boiling point | -4.5 °C density | 0.62 g/cm^3 (at 20 °C) solubility in water | insoluble surface tension | 0.0134 N/m dynamic viscosity | 7.54×10^-6 Pa s (at 20 °C)
Units
