To determine the number of oxides that are paramagnetic in nature among the given options, we need to analyze the electronic configuration of each oxide. Paramagnetic substances have unpaired electrons, which means they have at least one electron in an orbital that is not paired with another electron.

Let's examine each oxide:

1. Na2O: Sodium oxide (Na2O) consists of sodium (Na) and oxygen (O) atoms. Sodium is a metal and typically forms cations with a +1 charge. Oxygen is a non-metal and typically forms anions with a -2 charge. In Na2O, the oxidation state of sodium is +1, and the oxidation state of oxygen is -2. The electronic configuration of oxygen in this oxide is 1s2 2s2 2p4, which means it has two unpaired electrons. Therefore, Na2O is paramagnetic.

2. KO2: Potassium superoxide (KO2) contains potassium (K) and oxygen (O) atoms. Potassium is a metal and typically forms cations with a +1 charge. Oxygen is a non-metal and typically forms anions with a -2 charge. In KO2, the oxidation state of potassium is +1, and the oxidation state of oxygen is -1/2. The electronic configuration of oxygen in this oxide is 1s2 2s2 2p4, which means it has two unpaired electrons. Therefore, KO2 is paramagnetic.

3. NO2: Nitrogen dioxide (NO2) consists of nitrogen (N) and oxygen (O) atoms. Nitrogen is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In NO2, the oxidation state of nitrogen is +4, and the oxidation state of oxygen is -2. The electronic configuration of nitrogen in this oxide is 1s2 2s2 2p3, which means it has one unpaired electron. Therefore, NO2 is paramagnetic.

4. N2O: Nitrous oxide (N2O) contains two nitrogen (N) atoms and one oxygen (O) atom. Nitrogen is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In N2O, the oxidation state of nitrogen is +1, and the oxidation state of oxygen is -2. The electronic configuration of nitrogen in this oxide is 1s2 2s2 2p3, which means it has one unpaired electron. Therefore, N2O is paramagnetic.

5. ClO2: Chlorine dioxide (ClO2) consists of chlorine (Cl) and oxygen (O) atoms. Chlorine is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In ClO2, the oxidation state of chlorine is +4, and the oxidation state of oxygen is -2. The electronic configuration of chlorine in this oxide is 1s2 2s2 2p6 3s2 3p5, which means it has one unpaired electron. Therefore, ClO2 is paramagnetic.

6. NO: Nitric oxide (NO) contains nitrogen (N) and oxygen (O) atoms. Nitrogen is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In NO, the oxidation state of nitrogen is +2, and the oxidation state of oxygen is -2. The electronic configuration of nitrogen in this oxide is 1s2 2s2 2p3, which means it has one unpaired electron. Therefore, NO is paramagnetic.

7. SO2: Sulfur dioxide (SO2) consists of sulfur (S) and oxygen (O) atoms. Sulfur is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In SO2, the oxidation state of sulfur is +4, and the oxidation state of oxygen is -2. The electronic configuration of sulfur in this oxide is 1s2 2s2 2p6 3s2 3p4, which means it has two unpaired electrons. Therefore, SO2 is paramagnetic.

8. Cl2O: Dichlorine monoxide (Cl2O) contains two chlorine (Cl) atoms and one oxygen (O) atom. Chlorine is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In Cl2O, the oxidation state of chlorine is +1, and the oxidation state of oxygen is -2. The electronic configuration of chlorine in this oxide is 1s2 2s2 2p6 3s2 3p5, which means it has one unpaired electron. Therefore, Cl2O is paramagnetic.

In summary, the oxides Na2O, KO2, NO2, N2O, ClO2, NO, SO2, and Cl2O are all paramagnetic in nature.

Question

To determine the number of oxides that are paramagnetic in nature among the given options, we need to analyze the electronic configuration of each oxide. Paramagnetic substances have unpaired electrons, which means they have at least one electron in an orbital that is not paired with another electron.

Let's examine each oxide:

1. Na2O: Sodium oxide (Na2O) consists of sodium (Na) and oxygen (O) atoms. Sodium is a metal and typically forms cations with a +1 charge. Oxygen is a non-metal and typically forms anions with a -2 charge. In Na2O, the oxidation state of sodium is +1, and the oxidation state of oxygen is -2. The electronic configuration of oxygen in this oxide is 1s2 2s2 2p4, which means it has two unpaired electrons. Therefore, Na2O is paramagnetic.

2. KO2: Potassium superoxide (KO2) contains potassium (K) and oxygen (O) atoms. Potassium is a metal and typically forms cations with a +1 charge. Oxygen is a non-metal and typically forms anions with a -2 charge. In KO2, the oxidation state of potassium is +1, and the oxidation state of oxygen is -1/2. The electronic configuration of oxygen in this oxide is 1s2 2s2 2p4, which means it has two unpaired electrons. Therefore, KO2 is paramagnetic.

3. NO2: Nitrogen dioxide (NO2) consists of nitrogen (N) and oxygen (O) atoms. Nitrogen is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In NO2, the oxidation state of nitrogen is +4, and the oxidation state of oxygen is -2. The electronic configuration of nitrogen in this oxide is 1s2 2s2 2p3, which means it has one unpaired electron. Therefore, NO2 is paramagnetic.

4. N2O: Nitrous oxide (N2O) contains two nitrogen (N) atoms and one oxygen (O) atom. Nitrogen is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In N2O, the oxidation state of nitrogen is +1, and the oxidation state of oxygen is -2. The electronic configuration of nitrogen in this oxide is 1s2 2s2 2p3, which means it has one unpaired electron. Therefore, N2O is paramagnetic.

5. ClO2: Chlorine dioxide (ClO2) consists of chlorine (Cl) and oxygen (O) atoms. Chlorine is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In ClO2, the oxidation state of chlorine is +4, and the oxidation state of oxygen is -2. The electronic configuration of chlorine in this oxide is 1s2 2s2 2p6 3s2 3p5, which means it has one unpaired electron. Therefore, ClO2 is paramagnetic.

6. NO: Nitric oxide (NO) contains nitrogen (N) and oxygen (O) atoms. Nitrogen is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In NO, the oxidation state of nitrogen is +2, and the oxidation state of oxygen is -2. The electronic configuration of nitrogen in this oxide is 1s2 2s2 2p3, which means it has one unpaired electron. Therefore, NO is paramagnetic.

7. SO2: Sulfur dioxide (SO2) consists of sulfur (S) and oxygen (O) atoms. Sulfur is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In SO2, the oxidation state of sulfur is +4, and the oxidation state of oxygen is -2. The electronic configuration of sulfur in this oxide is 1s2 2s2 2p6 3s2 3p4, which means it has two unpaired electrons. Therefore, SO2 is paramagnetic.

8. Cl2O: Dichlorine monoxide (Cl2O) contains two chlorine (Cl) atoms and one oxygen (O) atom. Chlorine is a non-metal and typically forms compounds with various oxidation states. Oxygen is a non-metal and typically forms anions with a -2 charge. In Cl2O, the oxidation state of chlorine is +1, and the oxidation state of oxygen is -2. The electronic configuration of chlorine in this oxide is 1s2 2s2 2p6 3s2 3p5, which means it has one unpaired electron. Therefore, Cl2O is paramagnetic.

In summary, the oxides Na2O, KO2, NO2, N2O, ClO2, NO, SO2, and Cl2O are all paramagnetic in nature.

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