Ionic Compound Names:

1. SnCl2 – Tin (II) Chloride
2. FeO – Iron (II) Oxide
3. Cu2S – Copper (I) Sulfide
4. CuS – Copper (II) Sulfide
5. CdBr2 – Cadmium Bromide
6. HgCl2 – Mercury (II) Chloride

Gas Temperature Calculation:

Given:

– Initial gas volume (V1) = 0.256 L
– Final gas volume (V2) = 0.198 L
– Final temperature (T2) = 32°C

Using the combined gas law formula:
[ \dfrac{P_1V_1}{T_1} = \dfrac{P_2V_2}{T_2} ]

Since pressure and amount of gas remain constant:
[ \dfrac{V_1}{T_1} = \dfrac{V_2}{T_2} ]

Substitute the values:
[ \dfrac{0.256}{T_1} = \dfrac{0.198}{32 + 273.15} ]

Solve for ( T_1 ):
[ T_1 = \dfrac{0.256 \times (32 + 273.15)}{0.198} – 273.15 ]

The initial temperature of the gas can be calculated using the above formula.

Number of Electrons Lost or Gained:

1. Sr (Strontium) – Group 2 metal, typically loses 2 electrons to form Sr^2+ ion.
2. P (Phosphorus) – Group 5 nonmetal, typically gains 3 electrons to form P^3- ion.
3. Group 17A (17):- Fluorine (F) gains 1 electron to form F^- ion.
– Chlorine (Cl) gains 1 electron to form Cl^- ion.
– Bromine (Br) gains 1 electron to form Br^- ion.

These elements follow the octet rule, where they tend to gain or lose electrons to achieve a stable electron configuration.