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3 years ago

Which is a binary ionic compound? A.MgCl2 B.C6H12O6 C.CO2 D.PO43- E.CH4

Chemistry

2 answers:

SSSSS [86.1K]3 years ago

8 0

The answer is A MgCI2

natali 33 [55]3 years ago

8 0

Answer : The correct option is, (A) $MgCl_2$

Explanation :

Binary ionic compound : It is a type of compound that is made up of the ions of the two different elements in which one element is a metal and another element is a non-metal.

From the given options, option (A) $MgCl_2$ is a binary ionic compound because in this compound Mg is a metal which combine with the a non-metal element chlorine.

While the other options are the covalent compounds that is formed by the combination of non-metal and non-metal elements.

Hence, the $MgCl_2$ is a binary ionic compound.

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4 years ago

Which statement below is true?

kykrilka [37]

Answer:

a) At a given temperature, C₂H₆ has a higher vapor pressure than C₄H₁₀.

Explanation:

Which statement below is true?

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c) HCl has a higher boiling point than LiCl. FALSE. LiCl (ionic compound) has a higher boiling point than HCl (covalent compound).

d) H₂O has a greater polarizability than H₂Se. FALSE. Se has a larger atomic radius than O which is why H₂Se has a greater polarizability than H₂O.

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3 years ago

Determine the concentrations of MgCl2, Mg2+, and Cl− in a solution prepared by dissolving 2.52 × 10−4 g MgCl2 in 2.00 L of water

dybincka [34]

Answer:

Explanation:

Given parameters:

Mass of MgCl₂ = 2.52 x 10⁻⁴g

Volume of water = 2L

Unkown:

Concentration of MgCl₂ =?

Concentration of Mg²⁺ = ?

Concentration of Cl⁻ =?

Solution:

Concentration is defined as the number of moles of a solute contained in a solution.

Concentration = $\frac{number of moles }{volume}$

To find the number of moles"

number of moles = $\frac{mass}{molar mass}$

Molar mass of MgCl₂ = 24.3 + (2 x 35.5) = 95.3g/mol

number of moles = $\frac{0.000}{molar mass}$ = 0.000252moles

Concentration of MgCl₂ = $\frac{0.000252}{95.3}$ = 2.64 x 10⁻⁶moldm⁻³

from the formula of the compound;

1 mole of MgCl₂ contains 1 mole of Mg²⁺

Therefore, 2.64 x 10⁻⁶moldm⁻³ of MgCl₂ will contains 2.64 x 10⁻⁶moldm⁻³ of Mg

Also;

1 mole of MgCl₂ contains 2 mole of Cl⁻

2.64 x 10⁻⁶moldm⁻³ contains 2 x 2.64 x 10⁻⁶moldm⁻³; 5.29 x 10⁻⁶moldm⁻³

Expressing in ppm;

1ppm = 1mg/L

2.64 x 10⁻⁶moldm⁻³ to mg/L for Mg²⁺

2.64 x 10⁻⁶moldm⁻³ = 2.64 x 10⁻⁶moldm⁻³ x molar mass(g/mol)

= 2.64 x 10⁻⁶moldm⁻³ x 24.3 = 6.43 x 10⁻⁵g/L

g/L to mg/L; 6.43 x 10⁻⁵g/L x 1000 = 6.43 x 10⁻²mg/L = 6.43 x 10⁻²ppm

5.29 x 10⁻⁶moldm⁻³ to mg/L for Cl⁻;

5.29 x 10⁻⁶moldm⁻³ = 5.29 x 10⁻⁶moldm⁻³ x 35.5 = 1.88 x 10⁻⁴g/L

g/L to mg/L; 1.88 x 10⁻⁴g/L x 1000 = 1.88 x 10⁻¹mg/L = 1.88 x 10⁻¹ppm

7 0

3 years ago

An element gain two electrons and has 16 protons and 17 neutrons. What is the atomic mass of this element and what is the charge

Taya2010 [7]

Answer:

atomic mass= 33

Charge= -2

Explanation:

In an atom, are contained three SUBATOMIC particles viz: proton and neutron found in the nucleus, electrons surrounding the nucleus. Protons contain the positive charge of an atom while electrons contain the negative charge of an atom. The number of protons and electrons in an atom determines the charge of an ion (charged atom). Also, the atomic mass or mass number of that atom is got by adding the number of protons + number of neutrons.

In this case where the number of protons and number of neutrons are 16 and 17 respectively, the mass no. or atomic mass is 17 + 16 = 33.

Also, since two electrons are gained by this atom, it means the electron numbe, which is normally equal to the proton number in a neutral atom, will be increased by 2. Hence, the electron number will be 18 in this case.

The charge of the atom= no. of protons - no. of electrons = 16 - 18 = -2.

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4 years ago

What happens if more product is added to a system at equalibrium

telo118 [61]

Answer:

When additional product is added, the equilibrium shifts to reactants to reduce the stress. If reactant or product is removed, the equilibrium shifts to make more reactant or product, respectively, to make up for the loss.

5 0

3 years ago