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Lelu [443]
3 years ago
9

How many nonbonding electron pairs are there in the lewis structure of the peroxide ion, o22−?

Chemistry
2 answers:
Tom [10]3 years ago
8 0
There is 6 non - bonding pairs.
Let me show you one easy method to do this.
o22-, oxygen valence electron = 6 here we have two so total 12, and -2 that means we add electrons so it’s all equal to 14 right.
whenever need to find lone pair, subtract the number you get with the lowest multiple of 8.
here we total 14 valence electron right so lowest multiple of 8 would be 8.
so 14 - 8 = 6 and that is our answer.
Let me know if you have Problem with chemistry.
frosja888 [35]3 years ago
8 0

Answer:

The correct answer is that there are 6 pairs of non-binding electrons.

Explanation:

Hello!

Let's solve this!

In the Lewis structure of hydrogen peroxide we have a simple covalent bond between each of the hydrogen with each of the oxygen. To this is added a simple covalent bond between the oxygen. So we will have:

O22-: this means that we have 6 electrons for each of the oxygen, they are two oxygen so there are 12 electrons and there is a -2 so in total there are 14 electrons.

This must be deducted from the used electrons that are 2 + 2 (with the hydrogen) +2 (of the two oxygen): in total there are six electrons.

14-6 = 8

In other words, there are 4 pairs of non-binding electrons in hydrogen peroxide.

As is the peroxide ion, we must add two freer pairs, which are those that bind with the hydrogen.

The correct answer is that there are 6 pairs of non-binding electrons.

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Calculate the volume of 1 M NaOH needed to prepare 10.0 ml of a 0.10 M solution.
Mumz [18]
Answer is: <span>volume of 1 M NaOH is 1 ml.
</span>c₁(NaOH) = 1 M.
V₂(NaOH) = 10 ml.
c₂(NaOH) = 0,1 M.
V₁(NaOH) = ?
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c₂ - final concentration of the solution, after dilution.
V₁ - <span>volume to be diluted.
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c</span>₁ · V₁ = c₂ · V₂.
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7 0
3 years ago
A student is given 2.19 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine wh
Alina [70]

Answer:

The unknown acid is citric acid.

There is 0.0342 moles of NaOH consumed.

Explanation:

Step 1: Data given

Mass of the unknown acid = 2.19 gram

Titrating with 0.560 M of NaOH

The equivalence point is reached when 61.0 mL are added

Molar mass of oxalic acid = 90.03 g/mol

Molar mass of citric acid = 192.12 g/mol

<u>Step 2:</u> The balanced equations for both acids

The reaction between oxalic acid and NaOH is:

H2C2O4 + 2NaOH → Na2C2O4 + 2H2O

The reaction between citric acid and NaOH is:

H3C6H5O7 +3NaOH → Na3C6H5O7 + 3 H2O

<u>Step 3:</u> Calculate the number of moles of the acid

Moles = mass / Molar mass

In case of oxalic acid: 2.19 grams / 90.03 g/mol = 0.0243 moles

In case of citric acid: 2.19 grams /192.12 g/mol = 0.0114 moles

Step 4: Calculate number of moles of NaOH

The mole of NaOH required for titration;

number of moles  = Molar mass * volume = (0.560 M * 0.061 L) = 0.03416 mol

<u>Step 5:</u> Calculate which acid

For each mole of oxalic 2 moles of NaOH is required, for 0.0243 mol citric acid 0.0243 *2= 0.0486 mol NaOH is required. This is more than the number of moles consumed.

For each mole of citric acid 3 moles of NaOH is required, for 0.0114 mol citric acid 0.0114 * 3= 0.0342 mol NaOH is required. This is the number of moles NaOH used for the titration.

The unknown acid is citric acid. There is 0.0342 moles of NaOH consumed.

8 0
3 years ago
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