Determine whether each compound is soluble or insoluble. if the compound is soluble, list the ions present in solution. agno3 pb(c2h3o2)2 kno3 (nh4)2s

According to the solubility rules:

1. Silver nitrate: AgNO₃ is soluble.

Reason: Nitrates (NO₃⁻) are soluble.

AgNO₃ (aq) → Ag⁺(aq) + NO₃⁻(aq)

Ions present: silver ion (Ag⁺) and nitrate ion (NO₃⁻)

2. Lead(II) acetate: Pb(C₂H₃O₂)₂ is soluble.

Reason: Acetates (C₂H₃O₂⁻) are soluble

Pb(C₂H₃O₂)₂ → Pb²⁺(aq) + 2 CH₃COO⁻(aq)

Ions present: lead(II) ion (Pb²⁺) and two acetate ions (CH₃COO⁻)

3. Potassium nitrate: KNO₃ is soluble.

Reason: Nitrates (NO₃⁻) are soluble and group-1 ions such as K⁺ are soluble.

KNO₃ (aq) → K⁺(aq) + NO₃⁻(aq)

Ions present: potassium ion (K⁺) and nitrate ion (NO₃⁻)

4. Ammonium sulfide: (NH₄)₂S is soluble.

Reason: Ammonium (NH₄⁺) ions are soluble

(NH₄)₂S (aq) → 2 NH₄⁺(aq) + S²⁻(aq)

Ions present: two ammonium ions (NH₄⁺) and sulphide ion (S²⁻)

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."