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3 years ago

What does O - H.....O - H represent?

Chemistry

2 answers:

Anon25 [30]3 years ago

7 0

Answer:

a. Hydrogen bond.

Explanation:

There is an attraction between the Hydrogen in one molecule with the oxygen in another molecule. This occurs in water.

yawa3891 [41]3 years ago

6 0

Answer:

Explanation:

It's a covalent bond because O and H are both non metals.

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Which of the following statements is TRUE? Which of the following statements is TRUE? Electrons placed in antibonding orbitals s

marusya05 [52]

Answer:

When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in energy than the separate atomic orbitals.

Explanation:

Which of the following statements is TRUE?

Electrons placed in antibonding orbitals stabilize the ion/molecule. FALSE. Electrons in the antibonding orbitals destabilize the ion/molecule.

The total number of molecular orbitals formed doesn't always equal the number of atomic orbitals in the set. FALSE. The total number of molecular orbitals is always equal to the number of atomic orbitals in the set.

When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in energy than the separate atomic orbitals. TRUE. The orbital with lower energy will be the bonding orbital and the one with higher energy will be the antibonding orbital.

A bond order of 0 represents a stable chemical bond. FALSE. A chemical bond is stable if the bond order is higher than zero.

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3 years ago

Walking across a tightrope is mostly controlled by the _____.

garik1379 [7]

It is one two ahdih2eferu

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4 years ago

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How many moles of hydrogen are needed to produce 13.78 mol of ethane

Eddi Din [679]

82.68 moles of Hydrogen is needed to produce 13.79 moles of Ethane.

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3 years ago

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Explain why the following chemical equation represents a Lewis acid-base reaction. H+ + NH3 —>NH4+

lozanna [386]

Answer:

Due to an electron-pair acceptor and donor.

Explanations:

Lewis acid can be defined as an electron-pair acceptor. An example is Hydrogen ion(H+). This is because it is a proton and it distributes positive charge which means that it accepts electrons(negative charge).

Lewis base can be defined as an electron-pair donor. This is because it donates electrons to be accepted by the proton. An example is ammonia(NH3).

7 0

3 years ago

Identify the types of intermolecular forces present in each of the following substances, and select the substance in each pair t

Sergeu [11.5K]

Answer:

a. Van der Waals forces, C8H18 has higher boiling point.

b. Van der Waals forces in both compounds

Dipole -Dipole in CH3OCH3

c. Van der Waals and dipole-dipole in both, higher boiling point for HOOH.

Additionally H bonding in HOOH

d. Van der Waals for both compounds, additionally dipole- dipole and hydrogen bonding for NH2NH2.

Higher boling point NH2NH2

Explanation:

To answer this question we have to know the hybridization of the atoms of interest and/or the presence of resultant dipole moments which make the molecule polar, and the van der Waals interactions. Also we have to look for the presence of hydrogen bonding.

Remember van der Waals forces will be present in all of the molecules since they are of the instantaneous type produced by the momentaneous distortions of the electron clouds.

a. These two compounds are hydrocarbons, the electronegativity difference between carbon and hydrogen is very small, so the only factor we need to consider are the van der Waals interactions.

The van der Waals interactions increase with molecular weight since they are interactions which are momentaneous between the atoms in the molecule, and the heavier the molecule the more these distortions are possible.

Since C8H18 has a higher molecular than C6H14, it follows it has a greater boiling point.

b. CH3OCH3 differs only on the added O atom to C3H8. They have similar molecular weights, 46 vs 44 g/mol, but the presence of the tehedral sp³ hybridized oxygen atom with its high electronegativity produces dipole moments and imparts a polarity to the molecule which make us to predict CH3OCH3 will have a higher boiling point.

c. In HOOH we have dipole-dipole moments since the oxygen atom is sp³ hybridized and the O-O-H is tetrahedral, the molecule is polar. Additionally we have the presence of H bond in this compound which is not possible in HSSH.

While the molecule HSSH is also polar since it has two dipole moments in the sp³ hybridized ( tetrahedral ) S, it is not as big as the dipole moment in O-H.

Therefore Hydrogen peroxide, HOOH, has a higher boiling point than HSSH

d. The N-H bond has a dipole moment, and since the N is tetrahedral there is a resultant dipole moment. As in case d., we have hydrogen bonding between H and N.

NH2NH2 then will have a higher boiling point than CH3CH3 where only van der Waals interactions are possible.

You are welcome.

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4 years ago