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thiocyanate anion

Input interpretation

thiocyanate anion
thiocyanate anion

Lewis structure

Draw the Lewis structure of thiocyanate anion. 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), nitrogen (n_N, val = 5), and sulfur (n_S, val = 6) atoms, including the net charge: n_C, val + n_N, val + n_S, val - n_charge = 16 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), nitrogen (n_N, full = 8), and sulfur (n_S, full = 8): n_C, full + n_N, full + n_S, full = 24 Subtracting these two numbers shows that 24 - 16 = 8 bonding electrons are needed. Each bond has two electrons, so in addition to the 2 bonds already present in the diagram add 2 bonds. To minimize formal charge sulfur wants 2 bonds, nitrogen wants 3 bonds, and carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom. The net charge has been given to the most electronegative atom, sulfur:  Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms: Answer: |   |
Draw the Lewis structure of thiocyanate anion. 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), nitrogen (n_N, val = 5), and sulfur (n_S, val = 6) atoms, including the net charge: n_C, val + n_N, val + n_S, val - n_charge = 16 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), nitrogen (n_N, full = 8), and sulfur (n_S, full = 8): n_C, full + n_N, full + n_S, full = 24 Subtracting these two numbers shows that 24 - 16 = 8 bonding electrons are needed. Each bond has two electrons, so in addition to the 2 bonds already present in the diagram add 2 bonds. To minimize formal charge sulfur wants 2 bonds, nitrogen wants 3 bonds, and carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom. The net charge has been given to the most electronegative atom, sulfur: Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms: Answer: | |

General properties

formula | (SCN)^- net ionic charge | -1 alternate names | thiocyanate | thiocyanate(1-)
formula | (SCN)^- net ionic charge | -1 alternate names | thiocyanate | thiocyanate(1-)

Other properties

ion class | anions | polyatomic ions common sources of ion | tetrabutylammonium thiocyanate (1 eq) | sodium thiocyanate (1 eq) | lithium thiocyanate hydrate (1 eq) | cobalt dithiocyanate (2 eq) | calcium thiocyanate tetrahydrate (2 eq) | barium thiocyanate hydrate (2 eq)
ion class | anions | polyatomic ions common sources of ion | tetrabutylammonium thiocyanate (1 eq) | sodium thiocyanate (1 eq) | lithium thiocyanate hydrate (1 eq) | cobalt dithiocyanate (2 eq) | calcium thiocyanate tetrahydrate (2 eq) | barium thiocyanate hydrate (2 eq)

Thermodynamic properties

molar heat capacity c_p | aqueous | -40.2 J/(mol K) (joules per mole kelvin difference) molar free energy of formation Δ_fG° | aqueous | 92.7 kJ/mol (kilojoules per mole) molar heat of formation Δ_fH° | aqueous | 76.4 kJ/mol (kilojoules per mole) molar entropy S° | aqueous | 144.3 J/(mol K) (joules per mole kelvin)
molar heat capacity c_p | aqueous | -40.2 J/(mol K) (joules per mole kelvin difference) molar free energy of formation Δ_fG° | aqueous | 92.7 kJ/mol (kilojoules per mole) molar heat of formation Δ_fH° | aqueous | 76.4 kJ/mol (kilojoules per mole) molar entropy S° | aqueous | 144.3 J/(mol K) (joules per mole kelvin)