Statement-1. HF is an electron-deficient hydride.
Statements-2. In HF,F has three lone pairs of electrons.

Explanation

To address the question, we need to analyze both statements regarding hydrogen fluoride (HF) and determine their validity.

### Step 1: Analyze Statement 1
**Statement 1:** HF is an electron-deficient hydride.

- **Explanation:** Hydrogen fluoride (HF) consists of one hydrogen atom and one fluorine atom. In HF, the hydrogen atom shares its single electron with fluorine, forming a covalent bond. However, fluorine is highly electronegative and pulls the shared electron closer to itself, creating a polar covalent bond. This results in the hydrogen atom having a partial positive charge (δ+) and the fluorine atom having a partial negative charge (δ-).
- **Conclusion:** Since hydrogen has only one electron and is bonded to a highly electronegative atom (fluorine), it can be considered electron-deficient. Therefore, **Statement 1 is correct**.

### Step 2: Analyze Statement 2
**Statement 2:** In HF, F has three lone pairs of electrons.

- **Explanation:** Fluorine (F) has a total of 7 valence electrons. In HF, fluorine uses one of its valence electrons to form a bond with hydrogen, leaving it with 6 electrons. These remaining 6 electrons can be arranged as three lone pairs.
- **Conclusion:** Thus, **Statement 2 is also correct**.

### Final Conclusion
- **Statement 1:** Correct (HF is indeed an electron-deficient hydride).
- **Statement 2:** Correct (Fluorine has three lone pairs of electrons in HF).