For each pair of molecules or ions, select the stronger base and write its lewis structure
a) CH3S- or CH3O-
b) CH3NH- or CH3O-
c) CH3COO- or OH-
d) CH3CH2O- or H-
e) NH3 or OH-
I would really appreciate the help!
To determine the stronger base for each pair of molecules or ions, we need to compare their abilities to accept a proton (H+). Stronger bases are better at accepting protons.
To write the Lewis structure of each molecule or ion, we need to count the total number of valence electrons and distribute them to form bonds and satisfy the octet rule.
a) CH3S- or CH3O-
To determine the stronger base, we compare the electronegativity of sulfur (S) and oxygen (O). Oxygen is more electronegative than sulfur, which means the negative charge is better stabilized in the CH3O- ion. Therefore, CH3O- is the stronger base.
To write the Lewis structure of CH3O-, follow these steps:
1. Find the total number of valence electrons:
- Carbon (C) has 4 valence electrons.
- Hydrogen (H) has 1 valence electron.
- Oxygen (O) has 6 valence electrons.
Total = 4 + (3 × 1) + 6 = 13 valence electrons
2. Write the skeletal structure: C - O
3. Distribute the remaining valence electrons:
Place one pair of electrons as a lone pair on the oxygen atom.
H H
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H - C - O : -
b) CH3NH- or CH3O-
To determine the stronger base, we compare the electronegativity of nitrogen (N) and oxygen (O). Oxygen is more electronegative than nitrogen, which means the negative charge is better stabilized in the CH3O- ion. Therefore, CH3O- is the stronger base.
To write the Lewis structure of CH3O-, follow the steps mentioned above.
c) CH3COO- or OH-
To determine the stronger base, we compare the electronegativity of the oxygen atoms (in both CH3COO- and OH-). In this case, OH- is the stronger base since both ions have the negative charge on oxygen, but OH- has a higher electron density than CH3COO-.
To write the Lewis structure of OH-, follow the steps mentioned above.
d) CH3CH2O- or H-
To determine the stronger base, we compare the electronegativity of oxygen (O) and hydrogen (H). Oxygen is more electronegative than hydrogen, and with the same negative charge, CH3CH2O- is the stronger base.
To write the Lewis structure of CH3CH2O-, follow the steps mentioned above.
e) NH3 or OH-
To determine the stronger base, we compare the electronegativity of nitrogen (N) and oxygen (O). In this case, OH- is the stronger base since oxygen is more electronegative than nitrogen.
To write the Lewis structure of OH-, follow the steps mentioned above.
Remember, determining the stronger base involves comparing electronegativities and electron densities to assess the stability of the negative charge. The Lewis structures are provided as per the steps mentioned.