Is NO a polar molecule?

Answers

Answer 1

Answer: Electronegativity values are useful in determining if a bond is to be classified as nonpolar covalent, polar covalent or ionic. The electronegativities of oxygen and nitrogen are respectively, 3.44 and 3.04 on Pauling scale, the electronegativity difference being, 0.4. The bond is considered to be non-polar covalent.
IF IT HELP U PLZ PICK AS BEST TNX:)

Related Questions

Which of the following is a biogeochemical cycle?a. Atmospheric cycle b. Iconic cycle c. Neonic cycle d. Water cycle
What is the maximum amount of p4 that can be produced from 1.0 kg of phosphorite?
Enter the symbol of a sodium ion, Na+, followed by the formula of a sulfate ion, SO42−. Separate the ions with a comma only—spaces are not allowed. Express your answers as ions separated by a comma.
How many hydrogen atoms are represented in the formula (CH3)2CH2?
What was John Dalton's contribution to the development of the atomic theory?A Dalton recognized that tiny atoms combined to form complex structures.B Dalton recognized the presence of electrons around a nucleus.C Dalton recognized the presence of protons in the nucleus.

2 How many
molecules of water are
there in 1g of water CH₂)

Answers

Answer:

3.3345 x 10^22

The molar mass of the water molecule is 18 g/mol. It implies that 1 mol of water molecules weigh 18 g.

Now you can calculate easily the number of water molecules present in 1 g of water. Calculation follows

18 g of water contains 1 mol of water molecules.

or 18 g of water contains 6.022 x 10^23 water molecules.

or 1 g of water contains (6.022 x 10^23)/ 18 water molecules and the number comes out to be 3.3455 x 10^22.

So the number of water molecules present in 1 g of water is 3.3455 x 10^22.

I

Hope this helps you

Ernest Rutherford's gold-foil experiment showed which of the following?

Answers

Ernest Rutherford's gold-foil experiment showed the density of atoms.
The experiment proved that most of an atom is empty space with a very small positively charged nucleus in the middle.
So, from the given statements he following is true:
Ernest Rutherford's gold-foil experiment showed the existence of a dense, positively charged center in an atom.

Does anyone know how to do this? the solubility of barium carbonate, BaCO3, is 0.0100 g/L. Its molar mass is 197.3 g/mol. What is the Ksp of barium carbonate?

Answers

The value of ${{\text{K}}_{{\text{sp}}}}$ for barium carbonate is $\boxed{{\text{2}}{{.6 * 1}}{{\text{0}}^{{\text{ - 9}}}}}$ .

Further explanation:

Solubility product constant:

The equilibrium constant between the compound and its ion, when dissolved in solution, is known as solubility product constant. It is denoted by ${{\text{K}}_{{\text{sp}}}}$ . The solubility product constant is used to calculate the product of the concentration of ions at equilibrium.

Higher the solubility product constant more will be the solubility of the compound.

The general reaction is as follows:

${\text{AB}}\left({aq}\right)\to{{\text{A}}^+}\left({aq}\right)+{{\text{B}}^-}\left({aq}\right)$

The expression to calculate the solubility product for the general reaction is as follows:

$\boxed{{{\text{K}}_{{\text{sp}}}}=\left[{{{\text{A}}^+}}\right]\left[{{{\text{B}}^-}}\right]}$

Here,

${{\text{K}}_{{\text{sp}}}}$ is the solubility product constant.

$\left[ {{{\text{A}}^ + }} \right]$ is the concentration of ${{\text{A}}^ + }$ ions.

$\left[ {{{\text{B}}^ - }} \right]$ is the concentration of ${{\text{B}}^ - }$ ions.

The dissociation of ${\text{BaC}}{{\text{O}}_{\text{3}}}$ occurs as follows:

${\text{BaC}}{{\text{O}}_3}\to{\text{B}}{{\text{a}}^(2+)}+{\text{CO}}_3^(2-)$

The given solubility of ${\text{BaC}}{{\text{O}}_{\text{3}}}$ is 0.0100 g/L. Firstly, it is to be converted in mol/L. So the solubility of ${\text{BaC}}{{\text{O}}_{\text{3}}}$ is calculated as follows:

${\text{Solubility of BaC}}{{\text{O}}_{\text{3}}}\left({{\text{mol/L}}}\right)= \frac{{{\text{Solubility of BaC}}{{\text{O}}_{\text{3}}}\left({{\text{g/L}}}\right)}}{{{\text{Molar mass of BaC}}{{\text{O}}_{\text{3}}}\left({{\text{g/mol}}}\right)}}$ …… (1)

The solubility of ${\text{BaC}}{{\text{O}}_{\text{3}}}$ is 0.0100 g/L.

The molar mass of ${\text{BaC}}{{\text{O}}_{\text{3}}}$ is 197.3 g/mol.

Substitute these values in equation (1).

$\begin{aligned}{\text{Solubility of BaC}}{{\text{O}}_{\text{3}}}&=\left( {\frac{{{\text{0}}{\text{.0100 g}}}}{{{\text{1 L}}}}}\right)\left({\frac{{{\text{1 mol}}}}{{{\text{197}}{\text{.3 g}}}}} \right)\n&=0.00005068\;{\text{mol/L}}\n\end{aligned}$

It is evident from the chemical equation, one mole of ${\text{BaC}}{{\text{O}}_{\text{3}}}$ dissociates to form one mole of ${\text{B}}{{\text{a}}^(2+)}$ and one mole of ${\text{CO}}_3^(2-)$ . So the solubility of both ${\text{B}}{{\text{a}}^(2+)}$ and ${\text{CO}}_3^(2-)$ is 0.00005068 mol/L.

The formula to calculate the solubility product of is as follows:

${{\text{K}}_{{\text{sp}}}}=\left[{{\text{B}}{{\text{a}}^{{\text{2+}}}}}\right]\left[{{\text{CO}}{{_3^2}^-}}\right]$ …… (2)

Substitute 0.00005068 mol/L for $\left[{{\text{B}}{{\text{a}}^{{\text{2+}}}}}\right]$ and 0.00005068 mol/L for $\left[{{\text{CO}}_3^(2-)}\right]$ in equation (2).

$\begin{aligned}{{\text{K}}_{{\text{sp}}}}&=\left({{\text{0}}{\text{.00005068}}} \right)\left({{\text{0}}{\text{.00005068}}}\right)\n&=2.6*{10^(-9)}\n\end{aligned}$

Therefore, the value of ${{\mathbf{K}}_{{\mathbf{sp}}$ for ${\mathbf{BaC}}{{\mathbf{O}}_{\mathbf{3}$ is ${\mathbf{2}}{\mathbf{.6 * 1}}{{\mathbf{0}}^(-9)}$ .

Learn more:

1. Sort the solubility of gas will increase or decrease: brainly.com/question/2802008.

2. What is the pressure of the gas?: brainly.com/question/6340739.

Answer details:

Grade: School School

Subject: Chemistry

Chapter: Chemical equilibrium

Keywords: solubility, Ba2+, CO32-, BaCO3, Ksp, solubility product, molar mass, 197.3 g/mol, mol/L, g/L, 0.0100 g/L.

It's simple, just follow my steps.

1º - in 1 L we have $0.0100~g$ of $BaCO_3$

2º - let's find the number of moles.

$\eta=(m)/(MM)$

$\eta=(0.0100)/(197.3)$

$\boxed{\boxed{\eta=5.07*10^(-5)~mol}}$

3º - The concentration will be

$C=5.07*10^(-5)~mol/L$

But we have this reaction

$BaCO_3\rightleftharpoons Ba^(2+)+CO_3^(2-)$

This concentration will be the concentration of $Ba^(2+)~~and~~CO_3^(2-)$

$K_(sp)=([Ba^(2+)][CO_3^(2-)])/([BaCO_3])$

considering $[BaCO_3]=1~mol/L$

$K_(sp)=[Ba^(2+)][CO_3^(2-)]$

and

$[Ba^(2+)]=[CO_3^(2-)]=5.07*10^(-5)~mol/L$

We can replace it

$K_(sp)=(5.07*10^(-5))*(5.07*10^(-5))$

$K_(sp)\approx25.70*10^(-10)$

Therefore the $K_(sp)$ is:

$\boxed{\boxed{\boxed{K_(sp)\approx2.57*10^(-11)}}}$

Increasing the ? of a solvent increases the solubility of the solute

Answers

There are a lot of ways to increase the solubility of the solute. Increasing the temperature, mixing time and surface area of a solvent increases the solubility of the solute

The answer is temperature

Ice is nlaced in hot water What happens to the temperature of the ice and the water?

Answers

When ice is placed in hot water the hot water loses its own heat while the cold water from the ice gets heat.

Answer:when you add ice to hot water, the ice melts while the hot water cools. The exchange of heat energy from the hot water causes the ice to melt.

Explanation:

Hope this helped :)

What is the main intermolecular force in H2CO?(dipole dipole, hydrogen bond, London dispersion,polar/nonpolar)

Answers

Dipole-dipole interactions, and London dispersion interactions

Other Questions

Consider the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C. Calculate the change in internal energy, ΔE, for this reaction per mole of sucrose.

Which of the following is a synthesis reaction?C2H4 + 3O2 yields 2CO2 + 2 H2O 2HCl yields H2 + Cl2 2K + 2HCl yields 2KCl + H2 SO3 + H2O yields H2SO4

Describe the characteristics of compounds and explain how compounds are named

In the phase diagram below, point B describes the critical point.TRUEFALSE