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Ugo [173]
2 years ago
7

Why is a hydrogen bond a relatively weak bond?

Chemistry
1 answer:
DerKrebs [107]2 years ago
5 0

Hydrogen bonds are intermolecular (“between-molecule”) bonds, rather than intramolecular (“within-molecule”) bonds. They occur not only in water but in other polar molecules in which positive hydrogen atoms are attracted to negative atoms in nearby molecules. Hydrogen bonds are <em>relatively weaker</em> as chemical bonds. For example, they are much weaker than the bonds holding atoms together within molecules of covalent compounds.

Hydrogen bond is<em> weaker </em>than ionic and covalent bonds. Example: Water molecules are held to each other by intermolecular forces of attraction. Covalent bonds are the strongest bonds, meaning that atoms are actually held together by the physical sharing of electrons.

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What do the coefficients in the following balanced chemical equation mean?
mafiozo [28]
It's either B or D because there would be 2 coefficients of hydrogen and one of oxygen
6 0
3 years ago
Lead (II) nitrate reacts with ammonium carbonate to produce ammonium nitrate
vitfil [10]

Pb(NO₃)₂ + (NH₄)₂CO₃ → PbCO₃ + 2 NH₄NO₃

Explanation:

Reaction of lead (II) nitrate with ammonium carbonate will produce lead (II) carbonate and ammonium nitrate.

The balanced chemical equation is:

Pb(NO₃)₂ + (NH₄)₂CO₃ → PbCO₃ + 2 NH₄NO₃

To balance the chemical equation the number of atoms of each element   entering the reaction have to be equal to the number of atoms of each   element leaving the reaction, in order to conserve the mass.

Learn more about:

balancing chemical reactions

brainly.com/question/13911443

#learnwithBrainly

3 0
3 years ago
Determine the empirical formula of a compound containing 48.38 grams of carbon, 6.74 grams of hydrogen, and 53.5 grams of oxygen
Darya [45]

Answer: The empirical formula of the compound becomes CH_2O

<u>Explanation:</u>

The empirical formula is the chemical formula of the simplest ratio of the number of atoms of each element present in a compound.

We are given:

Mass of C = 48.38 g

Mass of H = 6.74 g

Mass of O = 53.5 g

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ......(1)

To formulate the empirical formula, we need to follow some steps:

  • <u>Step 1:</u> Converting the given masses into moles.

Molar mass of C = 12 g/mol

Molar mass of H = 1 g/mol

Molar mass of O = 16 g/mol

Putting values in equation 1, we get:

\text{Moles of C}=\frac{48.38g}{12g/mol}=3.023 mol

\text{Moles of H}=\frac{6.74g}{1g/mol}=6.74 mol

\text{Moles of O}=\frac{53.5g}{1g/mol}=3.34 mol

  • <u>Step 2:</u> Calculating the mole ratio of the given elements.

Calculating the mole fraction of each element by dividing the calculated moles by the least calculated number of moles that is 3.023 moles

\text{Mole fraction of C}=\frac{3.023}{3.023}=1

\text{Mole fraction of H}=\frac{6.74}{3.023}=2.23\approx 2

\text{Mole fraction of O}=\frac{3.34}{3.023}=1.105\approx 1

  • <u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of C : H : O = 1 : 2 : 1

Hence, the empirical formula of the compound becomes CH_2O

5 0
2 years ago
What's the answer to the question in the picture??
Burka [1]

Answer:

B

Explanation:

3 0
3 years ago
The empirical formula for trichloroisocyanuric acid, the active ingredient in many household bleaches is OCNCI. The molar mass o
TEA [102]

Answer:

These two are equivalent and valid:

       C_3Cl_3N_3O_3

       Cl_3(CN)_3O_3

Explanation:

The molecular superscripts for each atom in the <em>molecular formula</em> are determined by the number of times that the mass of the<em> empirical formula</em> is contained in the<em> molar mass</em>.

<u />

<u>1. Determine the mass of the empirical formula:</u>

OCNCl:

Atomic masses:

  • O: 15.999g/mol
  • C: 12.011g/mol
  • N: 14.007g/mol
  • Cl: 35.453g/mol

Total mass:

  • 15.999g/mol + 12.011g/mol + 14.007g/mol + 35.453g/mol = 77.470g/mol

<u />

<u>2. Divide the molar mass by the mass of the empirical formula:</u>

  • 232.41g/mol / 77.470g/mol = 3

<u>3. Multiply each superscript of the empirical formula by the previous quotient: 3</u>

       O_3C_3N__3Cl_3

Or:

       C_3Cl_3N_3O_3

You might also write CN as a group:

          Cl_3(CN)_3O_3

8 0
3 years ago
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