Identify the species which obey the octet rule for every atom. (The central atoms are underlined).
a. ClO3- (Cl is underlined)
b. SO2 (S is underlined)
c. NO2+ (N is underlined)
d. NO2 (N is underlined)
e. ClO- (Cl is underlined)
SO2
To identify the species that obey the octet rule for every atom, we need to examine the Lewis structures of each molecule. The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a full valence shell of eight electrons.
a. ClO3- (Cl is underlined):
- The Lewis structure for ClO3- has a central atom (Cl) surrounded by three oxygen atoms (O).
- Each O atom has six valence electrons, while the Cl atom has seven.
- By sharing electrons with the three O atoms, the Cl atom can complete its octet, resulting in a stable structure.
- Therefore, ClO3- obeys the octet rule for every atom.
b. SO2 (S is underlined):
- The Lewis structure for SO2 has a central atom (S) surrounded by two oxygen atoms (O).
- Each O atom has six valence electrons, while the S atom has six.
- By sharing electrons with the two O atoms, the S atom can complete its octet, resulting in a stable structure.
- Therefore, SO2 obeys the octet rule for every atom.
c. NO2+ (N is underlined):
- The Lewis structure for NO2+ has a central nitrogen atom (N) with a positive charge surrounded by two oxygen atoms (O).
- Each O atom has six valence electrons, while the N atom has five.
- Although sharing electrons helps the N atom achieve an octet, it still has one fewer electron due to the positive charge.
- Therefore, NO2+ does not obey the octet rule for every atom.
d. NO2 (N is underlined):
- The Lewis structure for NO2 has a central nitrogen atom (N) surrounded by two oxygen atoms (O).
- Each O atom has six valence electrons, while the N atom has five.
- By sharing electrons with the two O atoms, the N atom can achieve an octet, resulting in a stable structure.
- Therefore, NO2 obeys the octet rule for every atom.
e. ClO- (Cl is underlined):
- The Lewis structure for ClO- has a central chlorine atom (Cl) with a negative charge surrounded by one oxygen atom (O).
- The O atom has six valence electrons, while the Cl atom has seven.
- By sharing electrons with the O atom, the Cl atom can achieve an octet, resulting in a stable structure.
- Therefore, ClO- obeys the octet rule for every atom.
So, the species that obey the octet rule for every atom are ClO3- (option a), SO2 (option b), NO2 (option d), and ClO- (option e).
To determine which species obey the octet rule for every atom, we need to examine the electron configurations of the central atoms in each species.
The octet rule states that, in most cases, atoms tend to gain, lose, or share electrons in order to have a full outer shell of eight electrons (except for hydrogen and helium, which only require two electrons).
Let's analyze each option:
a. ClO3-
In ClO3-, Cl is the central atom. Chlorine (Cl) has 7 valence electrons. Oxygen (O) has 6 valence electrons, and there are three oxygen atoms bonded to chlorine. Thus, the total number of valence electrons is 7 + 6(3) + 1 (extra negative charge) = 26.
By distributing these electrons, we can see that the central atom Cl has 7 + 6 = 13 electrons. It does not obey the octet rule. Therefore, this species does not obey the octet rule.
b. SO2
In SO2, S is the central atom. Sulfur (S) has 6 valence electrons. Oxygen (O) has 6 valence electrons, and there are two oxygen atoms bonded to sulfur. Thus, the total number of valence electrons is 6 + 6(2) = 18.
By distributing these electrons, we can see that the central atom S has 6 + 6 + 2 = 14 electrons. It does not obey the octet rule. Therefore, this species does not obey the octet rule.
c. NO2+
In NO2+, N is the central atom. Nitrogen (N) has 5 valence electrons. Oxygen (O) has 6 valence electrons, and there are two oxygen atoms bonded to nitrogen. Additionally, there is a positive charge on this ion, indicating the loss of one electron. Thus, the total number of valence electrons is 5 + 6(2) - 1 (positive charge) = 16.
By distributing these electrons, we can see that the central atom N has 5 + 6 = 11 electrons. It does not obey the octet rule. Therefore, this species does not obey the octet rule.
d. NO2
In NO2, N is the central atom. Nitrogen (N) has 5 valence electrons. Oxygen (O) has 6 valence electrons, and there are two oxygen atoms bonded to nitrogen. Thus, the total number of valence electrons is 5 + 6(2) = 17.
By distributing these electrons, we can see that the central atom N has 5 + 6 + 6 = 17 electrons. It obeys the octet rule, as it has eight valence electrons. Therefore, this species does obey the octet rule.
e. ClO-
In ClO-, Cl is the central atom. Chlorine (Cl) has 7 valence electrons. Oxygen (O) has 6 valence electrons, and there is one oxygen atom bonded to chlorine. Additionally, there is a negative charge on this ion, indicating the gain of one electron. Thus, the total number of valence electrons is 7 + 6 + 1 (negative charge) = 14.
By distributing these electrons, we can see that the central atom Cl has 7 + 6 = 13 electrons. It does not obey the octet rule. Therefore, this species does not obey the octet rule.
From our analysis, we can conclude that only option d. NO2 obeys the octet rule for every atom.
I don't think it will do you any good for me to give you the answers. If you have a specific problem about how to do them try posting that question. You really need to learn to do these yourself.
For starters, Cl has an octet in ClO3^-.
I believe S has an octet in SO2 but check me out on both of those.