`1 g` of oxygen combines with `0.1260 g` of hydrogen to form `H_(2)O`. `1 g` of nitrogen combines with `0.2160 g` of hydrogen to form `NH_(3)`. Predict the weight of oxygen required to combine with `1 g` of nitrogen to form an oxide.

Explanation

To solve the problem, we need to find the weight of oxygen required to combine with 1 gram of nitrogen to form an oxide. We will use the information given in the question regarding the combinations of oxygen and hydrogen, and nitrogen and hydrogen.

### Step-by-Step Solution:

1. **Understanding the Reaction of Oxygen and Hydrogen:**
- We know that 1 g of oxygen combines with 0.1260 g of hydrogen to form water (H₂O).
- The balanced reaction is:
\[ 2H_2 + O_2 \rightarrow 2H_2O \]

2. **Calculating the Amount of H₂O Formed:**
- From the given data, we can say that:
\[ 1 \text{ g of } O_2 \text{ combines with } 0.1260 \text{ g of } H_2 \]
- Therefore, the total mass of water formed can be calculated as:
\[ \text{Mass of } H_2O = \text{Mass of } O_2 + \text{Mass of } H_2 = 1 \text{ g} + 0.1260 \text{ g} = 1.1260 \text{ g} \]

3. **Finding the Ratio of Oxygen to Hydrogen:**
- We can find the ratio of oxygen to hydrogen in terms of grams:
\[ \text{For } 1 \text{ g of } O_2, \text{ it combines with } 0.1260 \text{ g of } H_2 \]
- Thus, we can express the ratio:
\[ \frac{1 \text{ g O}_2}{0.1260 \text{ g H}_2} \approx 7.936 \]

4. **Understanding the Reaction of Nitrogen and Hydrogen:**
- Similarly, we know that 1 g of nitrogen combines with 0.2160 g of hydrogen to form ammonia (NH₃).
- The balanced reaction is:
\[ N_2 + 3H_2 \rightarrow 2NH_3 \]

5. **Finding the Ratio of Hydrogen to Nitrogen:**
- From the data:
\[ 1 \text{ g of } N_2 \text{ combines with } 0.2160 \text{ g of } H_2 \]
- Therefore, we can express the ratio:
\[ \frac{1 \text{ g N}_2}{0.2160 \text{ g H}_2} \approx 4.629 \]

6. **Finding the Ratio of Oxygen to Nitrogen:**
- Now we can find the ratio of oxygen to nitrogen based on the fixed weight of hydrogen (1 g):
- Using the ratios calculated:
\[ \text{Ratio of } O_2 \text{ to } N_2 = \frac{7.936}{4.629} \approx 1.71 \]

7. **Calculating the Weight of Oxygen Required:**
- Since we need to find the weight of oxygen that combines with 1 g of nitrogen:
\[ \text{Weight of } O_2 = 1.71 \text{ g} \]

### Final Answer:
The weight of oxygen required to combine with 1 g of nitrogen to form an oxide is **1.71 g**.