QuestionDraw $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{CH}_{4}$ , showing valence electrons, bond types, and partial charges. Describe their reaction.

Studdy Solution

STEP 1

Assumptions1. We are dealing with two compounds $\mathrm{H}_{} \mathrm{}$ (water) and $\mathrm{CH}_{4}$ (methane). . We need to draw these compounds showing their valence electrons and respective orbitals.
3. We need to label the type of covalent bonds (polar or nonpolar) and assign partial charges.
4. We also need to describe how methane would react with water if added to a beaker of it.

STEP 2

Let's start with water ( $\mathrm{H}_{2} \mathrm{}$ ). The oxygen atom has6 valence electrons and each hydrogen atom has1 valence electron. Oxygen shares one electron with each hydrogen atom to form two single covalent bonds. The remaining4 electrons on oxygen are non-bonding electrons, also known as lone pairs.

STEP 3

Draw the Lewis structure of water. The oxygen atom is in the center with two hydrogen atoms attached to it. The two lone pairs of electrons on oxygen are also shown.
$\begin{array}{c} \mathrm{H}-\mathrm{}-\mathrm{H} \\ \,|\, \\ \mathrm{} \end{array}$

STEP 4

Label the covalent bonds in water as polar. This is because oxygen is more electronegative than hydrogen, meaning it pulls the shared electrons closer to itself. This creates a partial negative charge ( $-\delta$ ) on the oxygen atom and a partial positive charge ( $+\delta$ ) on each hydrogen atom.

STEP 5

Now let's move on to methane ( $\mathrm{CH}_{4}$ ). Carbon has4 valence electrons and each hydrogen atom has1 valence electron. Carbon shares one electron with each hydrogen atom to form four single covalent bonds.

STEP 6

Draw the Lewis structure of methane. The carbon atom is in the center with four hydrogen atoms attached to it.
$\mathrm{H} \\ |\ \\ \mathrm{H}-\mathrm{C}-\mathrm{H} \\ |\ \\ \mathrm{H}$

STEP 7

Label the covalent bonds in methane as nonpolar. This is because carbon and hydrogen have similar electronegativities, meaning the shared electrons are roughly equally distributed. Therefore, there are no partial charges in methane.

STEP 8

Finally, let's describe how methane would react with water if added to a beaker of it. Methane is a nonpolar molecule, while water is a polar molecule. Due to this difference in polarity, methane does not dissolve or react with water. Instead, it would form bubbles and rise to the surface because it is less dense than water.

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QuestionDraw $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{CH}_{4}$ , showing valence electrons, bond types, and partial charges. Describe their reaction.

Studdy Solution

STEP 1

STEP 2

STEP 3

Draw the Lewis structure of water. The oxygen atom is in the center with two hydrogen atoms attached to it. The two lone pairs of electrons on oxygen are also shown.
$\begin{array}{c} \mathrm{H}-\mathrm{}-\mathrm{H} \\ \,|\, \\ \mathrm{} \end{array}$

STEP 4

Label the covalent bonds in water as polar. This is because oxygen is more electronegative than hydrogen, meaning it pulls the shared electrons closer to itself. This creates a partial negative charge ( $-\delta$ ) on the oxygen atom and a partial positive charge ( $+\delta$ ) on each hydrogen atom.

STEP 5

Now let's move on to methane ( $\mathrm{CH}_{4}$ ). Carbon has4 valence electrons and each hydrogen atom has1 valence electron. Carbon shares one electron with each hydrogen atom to form four single covalent bonds.

STEP 6

Draw the Lewis structure of methane. The carbon atom is in the center with four hydrogen atoms attached to it.
$\mathrm{H} \\ |\ \\ \mathrm{H}-\mathrm{C}-\mathrm{H} \\ |\ \\ \mathrm{H}$

STEP 7

Label the covalent bonds in methane as nonpolar. This is because carbon and hydrogen have similar electronegativities, meaning the shared electrons are roughly equally distributed. Therefore, there are no partial charges in methane.

STEP 8

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QuestionDraw H2O\mathrm{H}_{2} \mathrm{O}H2​O and CH4\mathrm{CH}_{4}CH4​, showing valence electrons, bond types, and partial charges. Describe their reaction.

Studdy Solution

STEP 1

STEP 2

STEP 3

Draw the Lewis structure of water. The oxygen atom is in the center with two hydrogen atoms attached to it. The two lone pairs of electrons on oxygen are also shown.H−−H ∣ \begin{array}{c} \mathrm{H}-\mathrm{}-\mathrm{H} \\ \,|\, \\ \mathrm{} \end{array} H−−H∣​

STEP 4

STEP 5

Now let's move on to methane (CH4\mathrm{CH}_{4}CH4​). Carbon has4 valence electrons and each hydrogen atom has1 valence electron. Carbon shares one electron with each hydrogen atom to form four single covalent bonds.

STEP 6

Draw the Lewis structure of methane. The carbon atom is in the center with four hydrogen atoms attached to it.H∣ H−C−H∣ H\mathrm{H} \\ |\ \\ \mathrm{H}-\mathrm{C}-\mathrm{H} \\ |\ \\ \mathrm{H} H∣ H−C−H∣ H

STEP 7

Label the covalent bonds in methane as nonpolar. This is because carbon and hydrogen have similar electronegativities, meaning the shared electrons are roughly equally distributed. Therefore, there are no partial charges in methane.

STEP 8

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QuestionDraw $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{CH}_{4}$ , showing valence electrons, bond types, and partial charges. Describe their reaction.

Draw the Lewis structure of water. The oxygen atom is in the center with two hydrogen atoms attached to it. The two lone pairs of electrons on oxygen are also shown.
$\begin{array}{c} \mathrm{H}-\mathrm{}-\mathrm{H} \\ \,|\, \\ \mathrm{} \end{array}$

Now let's move on to methane ( $\mathrm{CH}_{4}$ ). Carbon has4 valence electrons and each hydrogen atom has1 valence electron. Carbon shares one electron with each hydrogen atom to form four single covalent bonds.

Draw the Lewis structure of methane. The carbon atom is in the center with four hydrogen atoms attached to it.
$\mathrm{H} \\ |\ \\ \mathrm{H}-\mathrm{C}-\mathrm{H} \\ |\ \\ \mathrm{H}$