Input interpretation
![acetate anion](../image_source/885f9edcdd54fbaa168c5680b5aa0589.png)
acetate anion
Lewis structure
![Draw the Lewis structure of acetate 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), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms, including the net charge: 2 n_C, val + 3 n_H, val + 2 n_O, val - n_charge = 24 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): 2 n_C, full + 3 n_H, full + 2 n_O, full = 38 Subtracting these two numbers shows that 38 - 24 = 14 bonding electrons are needed. Each bond has two electrons, so in addition to the 6 bonds already present in the diagram add 1 bond. To minimize formal charge oxygen wants 2 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, oxygen: Fill in the 1 bond by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms. Double bonding carbon to the other highlighted oxygen atom would result in an equivalent molecule: Answer: | |](../image_source/4f0c92e6d6b0d1c366267f85b7fa5507.png)
Draw the Lewis structure of acetate 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), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms, including the net charge: 2 n_C, val + 3 n_H, val + 2 n_O, val - n_charge = 24 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): 2 n_C, full + 3 n_H, full + 2 n_O, full = 38 Subtracting these two numbers shows that 38 - 24 = 14 bonding electrons are needed. Each bond has two electrons, so in addition to the 6 bonds already present in the diagram add 1 bond. To minimize formal charge oxygen wants 2 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, oxygen: Fill in the 1 bond by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms. Double bonding carbon to the other highlighted oxygen atom would result in an equivalent molecule: Answer: | |
General properties
![formula | (CH_3CO_2)^- net ionic charge | -1 alternate names | ethanoate | acetate | acetate(1-)](../image_source/dc5f75872af287ee99e6401ed204bea2.png)
formula | (CH_3CO_2)^- net ionic charge | -1 alternate names | ethanoate | acetate | acetate(1-)
Ionic radius
![thermochemical radius | 162 pm](../image_source/2ecb5dde2ad98e1854c42e2b369e4e03.png)
thermochemical radius | 162 pm
Units
Other properties
![ion class | anions | carboxylate ions | ionic conjugate bases | oxoanions | polyatomic ions common sources of ion | tin(IV) acetate (4 eq) | stannous acetate (2 eq) | tetramethylammonium acetate (1 eq) | tetrabutylammonium acetate (1 eq) | strontium acetate (2 eq) | sodium diacetate (1 eq)](../image_source/72e6572e0953aa6e4712ed954fac0f5b.png)
ion class | anions | carboxylate ions | ionic conjugate bases | oxoanions | polyatomic ions common sources of ion | tin(IV) acetate (4 eq) | stannous acetate (2 eq) | tetramethylammonium acetate (1 eq) | tetrabutylammonium acetate (1 eq) | strontium acetate (2 eq) | sodium diacetate (1 eq)