Write the correct formula for the compound formed by each of the following pairs of ions.1.) Ni^2+, SO4^2-
2.) Al^3+, O^2-
3.) Ca^2, ClO3-
4.) NH4+, P^3-
5.) Cu+, NO3-
Answers
Answer:
1.) NiSO₄; 2.) Al₂O₃; 3.) Ca(ClO₃)₂; 4.) (NH₄)₃P; 5.) CuNO₃
Step-by-step explanation:
We can use the criss-cross method to work out the formulas. The steps are
- Write the symbols of the anion and cation.
- Criss-cross the numbers of the charges to become the subscripts of the other ion (as in the image).
- Write the formula with the new subscripts.
- Divide the subscripts by their highest common factor.
- Omit all subscripts that are 1.
If we use this method, the formula for the compound formed from Na⁺, SO₃²⁻ becomes Na₂SO₃.
1.) Ni²⁺ + SO₄²⁻ ⟶ Ni₂(SO₄)₂ ⟶ NiSO₄
2.) Al³⁺ + O²⁻ ⟶ Al₂O₃
3.) Ca²⁺ + ClO₃⁻ ⟶ Ca(ClO₃)₂
4.) NH₄⁺ + P³⁻ ⟶ (NH₄)₃P
5.) Cu⁺ + NO₃⁻ ⟶ CuNO₃
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Answer: (1) H+ ions in aqueous solution
Answers
Answer:
(Ca2 +, Mg2 +, Na+, and K+) and four major anions ( , , SO 4 2 - , and Cl-) with ionic forms of N, P, Fe, and other trace elements at lower concentrations (Livingstone 1963, Meybeck 1979) (Table 4.7).
Answers
Answer:
B. Two chlorine atoms
Explanation:
This electronic configuration shows that the given atom is magnesium.
Electronic configuration of magnesium:
Mg¹² = 1s² 2s² 2p⁶ 3s²
There are two valance electrons of magnesium that's why it would react with two atoms of chlorine. Chlorine is present in seventeen group. It has seven valance electrons. It required just one electron to get complete octet. While magnesium needed to lose two electrons to get complete octet. That's why two chlorine atoms bonded with one magnesium atom. Thus both would get complete octet.
Mg + Cl₂ → MgCl₂
Answers
Answer: When the pressure exerted on a confined gas at constant temperature is doubled, the volume of the gas is halved.
Explanation:
To calculate the new volume, we use the equation given by Boyle's law. This law states that pressure is inversely proportional to the volume of the gas at constant temperature.
The equation given by this law is:
where,
= initial pressure of gas = p
= initial volume of gas = v
= final pressure of gas= 2p
= final volume of gas = ?
Putting values in above equation, we get:
Thus the final volume of the gas is half of the initial volume.