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3 years ago

Which compound is composed of oppositely charged ions? A. OCl2 B. Na2O C. NH3 D. SCl2

Chemistry

2 answers:

Roman55 [17]3 years ago

6 0

Answer: The correct answer is Option B.

Explanation:

Compound having oppositely charged ions are considered as ionic compounds.

Ionic compounds are formed when complete transfer of electrons takes place between the atoms forming a bond. This bond is formed between a metal and a non-metal or a polyatomic cation and an non-metal or a metal and a polyatomic anion. For Example: $NaCl,NH_4Cl,BaSO_4$ etc..

Covalent compounds are formed when sharing of electrons takes place between the atoms forming a bond. This bond is formed between two non-metals. For Example: $H_2O,SO_2$ etc..

For the given options:

Option A: $OCl_2$

Oxygen and chlorine both are non-metals. Thus, it is forming a covalent compound.

Option B: $Na_2O$

Sodium is a metal and oxygen is a non-metal. Thus, it is forming an ionic compound and contain oppositely charged ions.

Option C: $NH_3$

Nitrogen and hydrogen both are non-metals. Thus, it is forming a covalent compound.

Option D: $SCl_2$

Sulfur and chlorine both are non-metals. Thus, it is forming a covalent compound.

Hence, the correct answer is Option B.

vazorg [7]3 years ago

5 0

It would be B, so yeah hope that helps ya ;)

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3 years ago

How many moles of gas sample are 5.0 L container at 373K and 203kPa

Rom4ik [11]

For the purpose we will here use the ideal gas law:

p×V=n×R×T

V= 5.0 L

T= 373K

p= 203kPa

R is universal gas constant, and its value is 8.314 J/mol×K

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6 0

3 years ago

A chemist prepares a solution of copper(II) fluoride by measuring out of copper(II) fluoride into a volumetric flask and filling

Simora [160]

The question is incomplete, here is the complete question.

A chemist prepares a solution of copper(II) fluoride by measuring out 0.0498 g of copper(II) fluoride into a 100.0mL volumetric flask and filling the flask to the mark with water.

Calculate the concentration in mol/L of the chemist's copper(II) fluoride solution. Round your answer to 3 significant digits.

Answer: The concentration of copper fluoride in the solution is $4.90\times 10^{-3}mol/L$

Explanation:

To calculate the molarity of solute, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

We are given:

Given mass of copper (II) fluoride = 0.0498 g

Molar mass of copper (II) fluoride = 101.54 g/mol

Volume of solution = 100.0 mL

Putting values in above equation, we get:

$\text{Molarity of copper (II) fluoride)=\frac{0.0498\times 1000}{101.54\times 100.0}\\\\\text{Molarity of copper (II) fluoride}=4.90\times 10^{-3}mol/L$