Question

1. draw diagrams to show how each of the covalent compounds below is formed by covalent bonding. hcl fcl of₂ nh₃

Explanation:

For HCl:

Step 1: Determine Valence Electrons

Hydrogen (H) has 1 valence electron, and Chlorine (Cl) has 7 valence electrons.

Step 2: Show Electron Sharing

H needs 1 more electron to fill its outer shell (duet rule), and Cl needs 1 more electron to fill its outer shell (octet rule). They share a pair of electrons. The Lewis structure is: $ \text{H} - \text{Cl} $, with Cl having 3 lone pairs (6 electrons) and H having 2 electrons (shared pair + its own).

For FCl:

Step 1: Determine Valence Electrons

Fluorine (F) has 7 valence electrons, Chlorine (Cl) has 7 valence electrons.

Step 2: Show Electron Sharing

Both F and Cl need 1 electron to complete their octets. They share a pair of electrons. The Lewis structure is: $ \text{F} - \text{Cl} $, with F and Cl each having 3 lone pairs (6 electrons each).

For $ \text{OF}_2 $:

Step 1: Determine Valence Electrons

Oxygen (O) has 6 valence electrons, each Fluorine (F) has 7 valence electrons.

Step 2: Show Electron Sharing

O needs 2 electrons to complete its octet, each F needs 1 electron. O shares one electron pair with each F. The Lewis structure: O is the central atom, bonded to two F atoms ($ \text{F} - \text{O} - \text{F} $). O has 2 lone pairs (4 electrons), and each F has 3 lone pairs (6 electrons).

For $ \text{NH}_3 $:

Step 1: Determine Valence Electrons

Nitrogen (N) has 5 valence electrons, each Hydrogen (H) has 1 valence electron.

Step 2: Show Electron Sharing

N needs 3 electrons to complete its octet, each H needs 1 electron. N shares one electron pair with each of the 3 H atoms. The Lewis structure: $ \text{H} - \text{N} - \text{H} $ (with a third H bonded to N), and N has 1 lone pair (2 electrons).

To draw the diagrams (Lewis structures):

• For HCl: Draw H connected by a single line to Cl. Cl has 3 pairs of dots (lone pairs) around it.
• For FCl: Draw F connected by a single line to Cl. Both F and Cl have 3 pairs of dots around them.
• For $ \text{OF}_2 $: Draw O in the center, connected by single lines to two F atoms. O has two pairs of dots, each F has three pairs of dots.
• For $ \text{NH}_3 $: Draw N in the center, connected by single lines to three H atoms. N has one pair of dots.

(Note: In Lewis structures, the lines represent shared electron pairs, and the dots represent lone electron pairs.)

Answer:

For HCl:

Step 1: Determine Valence Electrons

Hydrogen (H) has 1 valence electron, and Chlorine (Cl) has 7 valence electrons.

Step 2: Show Electron Sharing

H needs 1 more electron to fill its outer shell (duet rule), and Cl needs 1 more electron to fill its outer shell (octet rule). They share a pair of electrons. The Lewis structure is: $ \text{H} - \text{Cl} $, with Cl having 3 lone pairs (6 electrons) and H having 2 electrons (shared pair + its own).

For FCl:

Step 1: Determine Valence Electrons

Fluorine (F) has 7 valence electrons, Chlorine (Cl) has 7 valence electrons.

Step 2: Show Electron Sharing

Both F and Cl need 1 electron to complete their octets. They share a pair of electrons. The Lewis structure is: $ \text{F} - \text{Cl} $, with F and Cl each having 3 lone pairs (6 electrons each).

For $ \text{OF}_2 $:

Step 1: Determine Valence Electrons

Oxygen (O) has 6 valence electrons, each Fluorine (F) has 7 valence electrons.

Step 2: Show Electron Sharing

O needs 2 electrons to complete its octet, each F needs 1 electron. O shares one electron pair with each F. The Lewis structure: O is the central atom, bonded to two F atoms ($ \text{F} - \text{O} - \text{F} $). O has 2 lone pairs (4 electrons), and each F has 3 lone pairs (6 electrons).

For $ \text{NH}_3 $:

Step 1: Determine Valence Electrons

Nitrogen (N) has 5 valence electrons, each Hydrogen (H) has 1 valence electron.

Step 2: Show Electron Sharing

N needs 3 electrons to complete its octet, each H needs 1 electron. N shares one electron pair with each of the 3 H atoms. The Lewis structure: $ \text{H} - \text{N} - \text{H} $ (with a third H bonded to N), and N has 1 lone pair (2 electrons).

To draw the diagrams (Lewis structures):

• For HCl: Draw H connected by a single line to Cl. Cl has 3 pairs of dots (lone pairs) around it.
• For FCl: Draw F connected by a single line to Cl. Both F and Cl have 3 pairs of dots around them.
• For $ \text{OF}_2 $: Draw O in the center, connected by single lines to two F atoms. O has two pairs of dots, each F has three pairs of dots.
• For $ \text{NH}_3 $: Draw N in the center, connected by single lines to three H atoms. N has one pair of dots.

(Note: In Lewis structures, the lines represent shared electron pairs, and the dots represent lone electron pairs.)