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3 years ago

Which pair of atoms has the most polar bond? (1) H−Br (2) H−Cl (3) I−Br (4) I−Cl

Chemistry

2 answers:

natka813 [3]3 years ago

7 0

Answer: option (2) H - Cl

Explanation:

1) The polar character of a covalent bond is defined by the difference in the electronegativities of the atoms. The higher the diffrerence the greater the polar character of the bond.

2) The electronegativities of the elements are found in tables.

These are the electronegativities of the four elements of the question:

H: 2.20 ← lowest

I: 2.66

Br: 2.96

Cl: 3.16 ← highest

3) Since Cl has the greatest electronegativity of the four elements, and H has the lowest one, it is the bond H - Cl which will have the greatest difference of electronegativities, and it is the most polar bond.

S_A_V [24]3 years ago

6 0

For the question given above, option 2 which is H-Cl pair of atoms has the most polar bond among the four of them.

The larger the value of the electronegativity, the greater the atom’s strength to attract a bonding pair of electrons. <span>Hydrogen has an electronegativity of 2.1, and chlorine has an electronegativity of 3.0. The electron pair that is bonding HCl together shifts toward the chlorine atom because it has a larger electronegativity value.</span>

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Helga [31]

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If an acceleration is 0, it means that it neither slowed down nor sped up.

Now let us analyze your problem by listing down the speed and the time:

At noon: 4 mi/hr
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3 years ago

The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of O2 from the air

IceJOKER [234]

Answer:

$1.75\cdot 10^{-4} M$

Explanation:

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$S = k_H p^o$

Where $k_H$ is Henry's law constant.

Our strategy will be to identify the Henry's law constant for oxygen given the initial conditions and then use it to find the solubility at different conditions.

Given initially:

$S_1 = 2.67\cdot 10^{-4} M$

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$p = 1.00 atm$

Given mole fraction:

$\chi_{O_2} = 0.209$

According to Dalton's law of partial pressures, the partial pressure of oxygen is equal to the product of its mole fraction and the total pressure:

$p^o = \chi_{O_2} p$

Then the equation becomes:

$S_1 = k_H \chi_{O_2} p$

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$k_H = \frac{S_1}{\chi_{O_2} p} = \frac{2.67\cdot 10^{-4} M}{0.209\cdot 1.00 atm} = 0.001278 M/atm$

Now we're given that at an altitude of 12,000 ft, the atmospheric pressure is now:

$p = 0.657 atm$

Apply Henry's law using the constant we found:

$S_2 = k_H \chi_{O_2} p = 0.001278 M/atm\cdot 0.209\cdot 0.657 atm = 1.75\cdot 10^{-4} M$

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3 years ago

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3 years ago

What is the ph of a solution that has a poh of 11.24

galina1969 [7]

Always remember that pH + pOH = 14
Here, you have a pOH of 11.24, so you replace it in the equation, and u get:
pH + 11.24 = 14

Then, You move 11.24 to the other part. and moving from a part to another change the sign of the equation. And you get:
pH = 14 - 11.24 = 2.76

So, the pH of a solution that has a pOH of 11.24 is pH = 2.76

Hope this Helps :)

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3 years ago