Question

covalent compounds
show the electron movement, and then draw the lewis structure of the following covalent
compounds.

1. h₂s

electron movement lewis structure

1. cl₂

electron movement lewis structure

1. co₂

electron movement lewis structure

1. ccl₄

electron movement lewis structure

Explanation:

2. $\boldsymbol{H_2S}$

Electron Movement:

Hydrogen ($H$) has 1 valence electron, and sulfur ($S$) has 6 valence electrons. Each $H$ atom shares 1 electron with $S$, and $S$ shares 1 electron with each $H$. So, two single covalent bonds form (electron pairs shared between $H - S$).

Lewis Structure:

• Sulfur is the central atom.
• It forms single bonds with two $H$ atoms.
• Sulfur has two lone pairs (since $6 - 2$ (electrons used in bonding) $= 4$, so two lone pairs of 2 electrons each).

The Lewis structure is: $H - \ddot{S} - H$ (with two more lone pair electrons on $S$, total four lone pair electrons, represented as two pairs of dots).

3. $\boldsymbol{O_2}$

Electron Movement:

Each oxygen ($O$) has 6 valence electrons. They share two pairs of electrons (a double covalent bond) to achieve an octet. So, electron movement involves sharing two electron pairs between the two $O$ atoms.

Lewis Structure:

• The two $O$ atoms are connected by a double bond ($O = O$).
• Each $O$ has two lone pairs (since $6 - 2$ (electrons in double bond) $= 4$, so two lone pairs per $O$).

The Lewis structure is: $\ddot{O} = \ddot{O}$ (with two lone pairs on each $O$).

4. $\boldsymbol{CO_2}$

Electron Movement:

Carbon ($C$) has 4 valence electrons, and each oxygen ($O$) has 6. Carbon shares two pairs of electrons with each $O$ (double bonds). So, $C$ forms two double bonds (sharing two electron pairs with each $O$).

Lewis Structure:

• Carbon is the central atom, double - bonded to two $O$ atoms.
• Each $O$ has two lone pairs (since $6 - 2$ (electrons in double bond) $= 4$, so two lone pairs per $O$).

The Lewis structure is: $O = C = O$ (with two lone pairs on each $O$).

5. $\boldsymbol{CCl_4}$

Electron Movement:

Carbon ($C$) has 4 valence electrons, and each chlorine ($Cl$) has 7. Carbon shares 1 electron with each $Cl$, and each $Cl$ shares 1 electron with $C$. So, four single covalent bonds form (electron pairs shared between $C - Cl$).

Lewis Structure:

• Carbon is the central atom, single - bonded to four $Cl$ atoms.
• Each $Cl$ has three lone pairs (since $7 - 1$ (electron used in bonding) $= 6$, so three lone pairs per $Cl$).

The Lewis structure is:

$$\begin{matrix}&\ddot{Cl}&\\\ddot{Cl}-&C&-\ddot{Cl}\\\ &\ddot{Cl}&\end{matrix}$$

(with three lone pairs on each $Cl$).

Answer:

2. $\boldsymbol{H_2S}$

Electron Movement:

Hydrogen ($H$) has 1 valence electron, and sulfur ($S$) has 6 valence electrons. Each $H$ atom shares 1 electron with $S$, and $S$ shares 1 electron with each $H$. So, two single covalent bonds form (electron pairs shared between $H - S$).

Lewis Structure:

• Sulfur is the central atom.
• It forms single bonds with two $H$ atoms.
• Sulfur has two lone pairs (since $6 - 2$ (electrons used in bonding) $= 4$, so two lone pairs of 2 electrons each).

The Lewis structure is: $H - \ddot{S} - H$ (with two more lone pair electrons on $S$, total four lone pair electrons, represented as two pairs of dots).

3. $\boldsymbol{O_2}$

Electron Movement:

Each oxygen ($O$) has 6 valence electrons. They share two pairs of electrons (a double covalent bond) to achieve an octet. So, electron movement involves sharing two electron pairs between the two $O$ atoms.

Lewis Structure:

• The two $O$ atoms are connected by a double bond ($O = O$).
• Each $O$ has two lone pairs (since $6 - 2$ (electrons in double bond) $= 4$, so two lone pairs per $O$).

The Lewis structure is: $\ddot{O} = \ddot{O}$ (with two lone pairs on each $O$).

4. $\boldsymbol{CO_2}$

Electron Movement:

Carbon ($C$) has 4 valence electrons, and each oxygen ($O$) has 6. Carbon shares two pairs of electrons with each $O$ (double bonds). So, $C$ forms two double bonds (sharing two electron pairs with each $O$).

Lewis Structure:

• Carbon is the central atom, double - bonded to two $O$ atoms.
• Each $O$ has two lone pairs (since $6 - 2$ (electrons in double bond) $= 4$, so two lone pairs per $O$).

The Lewis structure is: $O = C = O$ (with two lone pairs on each $O$).

5. $\boldsymbol{CCl_4}$

Electron Movement:

Carbon ($C$) has 4 valence electrons, and each chlorine ($Cl$) has 7. Carbon shares 1 electron with each $Cl$, and each $Cl$ shares 1 electron with $C$. So, four single covalent bonds form (electron pairs shared between $C - Cl$).

Lewis Structure:

• Carbon is the central atom, single - bonded to four $Cl$ atoms.
• Each $Cl$ has three lone pairs (since $7 - 1$ (electron used in bonding) $= 6$, so three lone pairs per $Cl$).

The Lewis structure is:

$$\begin{matrix}&\ddot{Cl}&\\\ddot{Cl}-&C&-\ddot{Cl}\\\ &\ddot{Cl}&\end{matrix}$$

(with three lone pairs on each $Cl$).