How does electronegativity affect the polarity of the bond between twoatoms?
A. The more electronegative atom will form the positive pole of a
polar bond.
B. The more electronegative atom will form a nonpolar end of the
bond.
C. The more electronegative atom will make its end of the bond more
negative.
D. Electronegativity differences between the atoms will cancel out
bond polarity

Answers

Answer 1

Answer:

The electronegativity affects the polarity of the bond between two atoms, as the more electronegative atom will make its end of the bond more negative. The correct option is C.

What is electronegativity?

Electronegativity is a charge that shows the ability of an element to gain electron pairs with other elements during bonding. Electronegativity is altered by the distance between the electron and the nuclei and the atomic number of the element.

Polarity is the state of the atomic body in which it has placed charges in an opposite way to the other atoms so that they can join together.

Thus, the correct option is C. The more electronegative atom will make its end of the bond more negative.

To learn more about electronegativity, refer to the link:

brainly.com/question/17762711

#SPJ5

Answer 2

Answer:

Answer:

C. The more electronegative atom willl make its end of the

bond more negative

A P E X

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Which is the weakest type of intramolecular force/bond?a. Polar covalent b. Ionic c. Metallic d. Nonpolar covalent

Answers

Answer:

Non polar covlant

Explanation:

A mixture of neon and xenon gases, at a total pressure of 739 mm Hg, contains 0.919 grams of neon and 19.1 grams of xenon. What is the partial pressure of each gas in the mixture?_______g Xe

Answers

Answer:

Partial pressure of neon = 175 mmHg

Partial pressure of xenon = 564 mmHg

Explanation:

The partial pressure of a gas in a mixture can be calculated as the product of the mole fraction of the gas (Xi) and the total pressure (Pt), as follows:

Pi = Xi Pt

The total pressure is 739 mmHg ⇒ Pt = 739 mmHg

In order to calculate the mole fraction of each gas, we have to first calculate the number of moles of each gas (n) by dividing the mass of the gas into the molar mass (MM):

For neon gas (Ne):

MM(Ne) = 20.18 g/mol

n(Ne)= mass/MM = 0.919 g x 1 mol/20.18 g = 0.045 mol Ne

For xenon gas (Xe):

MM(Xe) = 131.3 g/mol

n(Xe)= mass/MM = 19.1 g x 1 mol/131.3 g = 0.145 mol Xe

Now, we calculate the mole fraction (X) by dividing the number of moles of the gas into the total number of moles (nt):

nt= moles Ne + moles Xe = 0.045 mol + 0.145 mol = 0.190 mol

X(Ne) = moles Ne/nt = 0.045 mol/0.190 mol = 0.237

X(Xe) = moles Xe/nt = 0.145/0.190 mol = 0.763

Finally, we calculate the partial pressures of Ne and Xe as follows:

P(Ne) = X(Ne) x Pt = 0.237 x 739 mmHg = 175 mmHg

P(Xe) = X(Xe) x Pt = 0.763 x 739 mmHg = 564 mmHg

5. What is the speed (Velocity) of a cyclist who covers 10 km (convert to metersfirst!) in 14 minutes and 30 seconds? Remember time must be in seconds first!

Answers

$\mathfrak{\huge{\pink{\underline{\underline{AnSwEr:-}}}}}$

Actually Welcome to the Concept of the Kinematics.

Here, we know that, Velocity = Distance / Time,

So here, Distance = 10km = 10×1000 = 10000 metres.

, Time = 14 min 30 sec = 870 seconds,

so now, we get velocity as,

=> V = 10000 ÷ 870 => 11.49 m/s .

Hence, Velocity is 11.49 m/s.

A cubic box with sides of 20.0 cm contains 2.00 × 1023 molecules of helium with a root-mean-square speed (thermal speed) of 200 m/s. The mass of a helium molecule is 3.40 × 10-27 kg. What is the average pressure exerted by the molecules on the walls of the container? (The Boltzmann constant is 1.38 × 10-23 J/K and the ideal gas constant is R = 8.314 J/mol•K .) (12 pts.)

Answers

Answer:

1.133 kPa is the average pressure exerted by the molecules on the walls of the container.

Explanation:

Side of the cubic box = s = 20.0 cm

Volume of the box ,V= $s^3$

$V=(20.0 cm)^3=8000 cm^3=8* 10^(-3) m^3$

Root mean square speed of the of helium molecule : 200m/s

The formula used for root mean square speed is:

$\mu=\sqrt{(3kN_AT)/(M)}$

where,

= root mean square speed

k = Boltzmann’s constant = $1.38* 10^(-23)J/K$

T = temperature = 370 K

M = mass helium = $3.40* 10^(-27)kg/mole$

$N_A$ = Avogadro’s number = $6.022* 10^(23)mol^(-1)$

$T=(\mu _(rms)^2* M)/(3kN_A)$

Moles of helium gas = n

Number of helium molecules = N = $2.00* 10^(23)$

N = $N_A* n$

Ideal gas equation:

PV = nRT

Substitution of values of T and n from above :

$PV=(N)/(N_A)* R* (\mu _(rms)^2* M)/(3kN_A)$

$PV=(N* R* \mu ^2* M)/(3k* (N_A)^2)$

$R=k* N_A$

$PV=(N* \mu ^2* M)/(3)$

$P=(2.00* 10^(23)* (200 m/s)^2* 3.40* 10^(-27) kg/mol)/(3* 8* 10^(-3) m^3)$

$P=1133.33 Pa =1.133 kPa$

(1 Pa = 0.001 kPa)

1.133 kPa is the average pressure exerted by the molecules on the walls of the container.

Final answer:

The question asks for the average pressure exerted by helium gas molecules on the walls of a cubic container. Using the equation PV = Nmv^2, we can calculate pressure by substituting the given values for volume, number of molecules, mass of one molecule, and root-mean-square speed.

Explanation:

The question is asking to calculate the average pressure exerted by helium gas molecules on the walls of a cubic container. The important formula relating pressure (P), volume (V), number of molecules (N), mass of a molecule (m), and the square of the rms speed (v2) of the molecules in a gas is:

PV = Nmv2,

First, we need to determine the volume of the container, which is the cube of one side, so V = (20 cm)3 = (0.2 m)3. Inserting the given values into the equation and solving for P gives us the desired answer. Recall that the rms speed is given, so no temperature calculations are needed.

Therefore, using all given data points:

Volume (V) = (0.2 m)3

Number of molecules (N) = 2.00 × 1023

Mass of one helium molecule (m) = 3.40 × 10-27 kg

Root-mean-square speed (vrms) = 200 m/s

By substituting these values, we can find the pressure exerted by the gas. This represents an application of kinetic theory of gases which assumes the behavior of an ideal gas.

The ΔG°f of atomic oxygen is 230.1 kJ/mol. Find ΔG° for the following dissociation reactionO2 (g) <--> 2O (g)then calculate its equilibrium constant at 298 K.

Answers

Answer:

Kc = 2.145 × 10⁻⁸¹

Explanation:

Let's consider the following reaction:

O₂(g) ⇄ 2O(g)

The standard Gibbs free energy for the reaction (ΔG°) can be calculated using the following expression:

ΔG° = Σnp. ΔG°f(p) - Σnp. ΔG°f(p)

where,

ni are the moles of products and reactants

ΔG°f(p) are the standard Gibbs free energy of formation of products and reactants

In this case,

ΔG° = 2 × ΔG°f(O) - 1 × ΔG°f(O₂)

ΔG° = 2 × 230.1 kJ/mol - 1 × 0 kJ/mol

ΔG° = 460.2 kJ/mol

With this information, we can calculate the equilibrium constant (Kc) using the following expression:

$Kc=e^(-\Delta G \°/R.T ) = e^{-460.2 kJ/mol/(8.314 * 10^(-3)kJ/mol.K) * 298K }=2.145 * 10^(-81)$

Can anyone tell me about sulfuric acid in shampoo/soap?

Answers

The term sulfate is used in chemistry to denote a salt of sulfuric acid. ... This is the sulfate type which can be found in many cleaning and hygiene products including shampoos. The main reasons why it is added to shampoos are because this sulfate produces foam and is a powerful detergent.

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