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aev [14]
3 years ago
5

Select the true statements regarding these resonance structures of formate.? Each carbon-oyxgen bond is somewhere between a sing

le and double bond. The actual structure of formate switches back and forth between the two resonance forms. Each oxygen atom has a double bond 50% of the time.

Chemistry
2 answers:
Law Incorporation [45]3 years ago
8 0

True statement regarding the resonance structures of formate is that the .

\boxed{{\text{carbon - oxygen bond lies in between the single and double bond}}}

Further explanation:

The bonding between the different atoms in covalent molecules is shown by some diagrams known as the Lewis structures. These also show the presence of lone pairs in the molecule. These are also known as Lewis dot diagrams, electron dot diagrams, Lewis dot structures or Lewis dot formula. In covalent compounds, the geometry, polarity, and reactivity are predicted by these structures.

When more than one Lewis structures are possible for a single molecule but no single structure is able to explain all the properties of the molecule then resonance is used. All the structures thus formed are called resonating structures and the phenomenon is known as resonance. The resonance structures have the same placement of atoms but different locations of bond pairs and lone pairs of electrons. Moreover, various resonating structures can be converted to each other by moving lone pairs to bonding positions, and vice-versa.

The general rules that we follow to draw the resonance structures are as follows:

a. The \pi electrons or a lone pair of electrons can change their positions while the position of atoms remains fixed.

b. The count of the valence electrons in all the resonating structures should be same.

c. The transfer of electrons is shown by the curved arrows.

d. The resonating structure must follow octet rule that is all atoms should have 8 electrons

The resonating structures and resonance hybrid of the formate is represented in the attached image.

A single canonical structure such as (I) cannot describe all the experimentally observed properties of the formate ion. The non-bonding electrons belonging to the p orbitals of the oxygen undergo delocalization so that nature of the carbon-oxygen bond is neither purely single nor double bond but has an intermediate bond length that is 0.133{\text{ nm}}. This bond length is greater than the double bond 0.123{\text{ nm}} but less than the carbon-oxygen single bond that is  0.143{\text{ nm}}.

Learn more:

1. When titrating a strong acid with a strong base what will be pH? brainly.com/question/3168961

2. How many covalent bond nitrogen forms: brainly.com/question/5974553

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Molecular structure and chemical bonding

Keywords: Lewis structure, valence electrons, formal charge, HCO2-, oxygen, p orbitals, double bonds, a single bond, bonding electrons and non-bonding electrons.

son4ous [18]3 years ago
7 0

Answer : Option 1) The true statement is each carbon-oxygen bond is somewhere between a single and double bond and the actual structure of format is an average of the two resonance forms.

Explanation : The actual structure of formate is found to be a resonance hybrid of the two resonating forms. The actual structure for formate do not switches back and forth between two resonance forms.

The O atom in the formate molecule with one bond and three lone pairs, in the resonance form left with reference to the attached image, gets changed into O atom with two bonds and two lone pairs.

Again, the O atom with two bonds and two lone pairs on the resonance form left, changed into O atom with one bond and three lone pairs. It concludes that each carbon-oxygen bond is neither a single bond nor a double bond; each carbon-oxygen bond is somewhere between a single and double bond.

Also, it is seen that each oxygen atom does not have neither a double bond nor a single bond 50% of the time.

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Magnesium Oxide decomposes to produce 3.54 grams of oxygen gas. How many grams of magnesium oxide decomposed?
sukhopar [10]
<h2>Let us solve for it </h2>

Explanation:

Magnesium oxide

  • It is MgO  
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  • when 40 g of MgO decomposes it forms = 16g of oxygen  
  • or we can say that :
  • 16g of oxygen is produced when 40 g of MgO is decomposed .
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4 0
3 years ago
Where did you put H an He? What are your reasoning for placement?
aksik [14]

Answer:

On the placement of hydrogen and helium in the periodic system

H1=1

He2=2

3 0
3 years ago
Which is the empirical formula for a compound that contains 64.75g nitrogen and 185.25 oxygen
Svetach [21]

Answer:

What is the formula for a compound that contains 64.75 g nitrogen and 185.25 g oxygen? D. N2O5

The name of a hydrate is calcium chloride dihydrate. What is its formula? B. CaCl2 x 2H20

Explanation:

BRAINLIEST PLZZZZ

5 0
3 years ago
Formula New Combination Predicted Formula
creativ13 [48]
Answer:

<span>Formula      New Combination                     Predicted Formula
</span>

NaCl            potassium + chlorine                KCl


AlCl₃             aluminum + fluorine                AlF₃

CO₂              tin + oxygen                              SnO₂

MgCl₂           calcium + bromine                   CaBr₂

HCl               cesium + iodine                       CsI


<span> CCl₄              silicon + bromine                     SiBr₄</span>

Explanation:

1) The question is incomplete. The first part is missing.

This is the first part of the question.

<span>Applying the principle that the elements of a particular column in the Periodic Table share the same chemical properties, complete the following chart. The first one has been done for you.
</span>

2) This is the given chart:

<span>Formula      New Combination                     Predicted Formula
</span>

Cu₂O           silver + oxygen                          Ag₂O   ← this is the example.

NaCl            potassium + chlorine 

<span> AlCl₃             aluminum + fluorine </span>

CO₂              tin + oxygen 

<span> MgCl₂           calcium + bromine </span>

<span> HCl               cesium + iodine </span>

<span> CCl₄              silicon + bromine </span>


3) This is how you find the new formula to complete the chart.

i) NaCl            potassium + chlorine 

Since potassium is in the same group of sodium, you predict that in the new formula Na is replaced by K giving KCl.

ii) AlCl₃             aluminum + fluorine 

Since fluorine is in the same group that Al, then you predict that in the new formula Cl is replaced by F leading to AlF₃

iii) CO₂              tin + oxygen 

Since tin is in the same group that C, you predict that in the new formula C is replaced by Sn leading to SnO₂

iv) MgCl₂           calcium + bromine 

Since calcium is in the same group that Mg, and bromine is in the same group that Cl, you predict thea in the new formula calcium replaces Mg and bromine replaces Cl, leading to CaBr₂

v) HCl               cesium + iodine 

Since H is in the same column that cesium and Cl is in the same colum that iodine, you predict that in the new formula Cs replaces H and I replaces Cl leading to: CsI


<span> vi) CCl₄              silicon + bromine
</span>

Since silicon is in the same column that C and bromine is in the same column that Cl, you predict that in the new formula Si replaces C and Br replaces Cl, leading to SiBr₄
5 0
3 years ago
A buffer consists of 0.120 M HNO2 and 0.150 M NaNO2 at 25°C. pka of HNO2 is 3.40. a. What is the pH of the buffer? b. What is th
Mashcka [7]

Explanation:

It is known that K_{a} of HNO_{2} = 4.5 \times 10^{-4}.

(a)  Relation between K_{a} and pK_{a} is as follows.

                       pK_{a} = -log (K_{a})

Putting the values into the above formula as follows.

                      pK_{a} = -log (K_{a})

                                    = -log(4.5 \times 10^{-4})

                                     = 3.347

Also, relation between pH and  pK_{a} is as follows.

              pH = pK_{a} + log\frac{[conjugate base]}{[acid]}

                     = 3.347+ log \frac{0.15}{0.12}

                    = 3.44

Therefore, pH of the buffer is 3.44.

(b)   No. of moles of HCl added = Molarity \times volume

                                            = 11.6 M \times 0.001 L

                                             = 0.0116 mol

In the given reaction, NO^{-}_{2} will react with H^{+} to form HNO_{2}

Hence, before the reaction:

No. of moles of NO^{-}_{2} = 0.15 M \times 1.0 L

                                           = 0.15 mol

And, no. of moles of HNO_{2} = 0.12 M \times 1.0 L

                                               = 0.12 mol

On the other hand, after the reaction :  

No. of moles of NO^{-}_{2} = moles present initially - moles added

                                          = (0.15 - 0.0116) mol

                                          = 0.1384 mol

Moles of HNO_{2} = moles present initially + moles added

                               = (0.12 + 0.0116) mol

                                = 0.1316 mol

As, K_{a} = 4.5 \times 10^{-4}

           pK_{a} = -log (K_{a})

                         = -log(4.5 \times 10^{-4})

                         = 3.347

Since, volume is both in numerator and denominator, we can use mol instead of concentration.

As, pH = pK_{a} + log \frac{[conjugate base]}{[acid]}

            = 3.347+ log {0.1384/0.1316}

            = 3.369

            = 3.37 (approx)

Thus, we can conclude that pH after the addition of 1.00 mL of 11.6 M HCl to 1.00 L of the buffer solution is 3.37.

6 0
3 years ago
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