In which of the properties listed below, hydrogen does not show similarity with halogens?
(i) nature of the oxide
(ii) Electropositive character
(iii) Combination with alkali metals
(iv) Atomicity

Options

A. (i) and (ii)
B. (iii) and (iv)
C. (ii) only
D. (i) and (iii)

Explanation

To determine in which property hydrogen does not show similarity with halogens, we will analyze each of the given options:

1. **Nature of the Oxide**:
- Hydrogen can form both positive and negative oxides. It can act as an electropositive element (like in metal hydrides) and also as an electronegative element (like in water, H2O). Halogens, on the other hand, primarily form negative oxides (e.g., ClO2, BrO3) and exhibit a consistent electronegative character. Therefore, hydrogen's behavior in terms of oxide formation is not similar to that of halogens.

2. **Electropositive Character**:
- Hydrogen can exhibit electropositive character, especially when it forms compounds with metals (like metal hydrides). Halogens, however, do not exhibit electropositive character; they are strictly electronegative. Thus, hydrogen's ability to be electropositive is a property that distinguishes it from halogens.

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