Question

1. Using their valence electrons, build the Covalent Bonds below:
a. Nitrogen + Bromine
d. 2 Bromine
b. Sulfur + Hydrogen e. Chlorine + Iodine
c. Fluorine + Phosphorus
f. Oxygen + Carbon

Answer 1

To understand covalent bonding and how to build covalent bonds between different elements, we recognize that covalent bonds form when two atoms share pairs of valence electrons. Below, I will break down the bonds formed between each specified pair of elements:

### a. Nitrogen + Bromine
- **Nitrogen (N)** has 5 valence electrons.
- **Bromine (Br)** has 7 valence electrons.
- Nitrogen can form **one triple bond** with another nitrogen atom or **three single bonds** with other atoms. In this case, it can share one of its electrons with one of bromine’s electrons to form **one single bond (1 pair)**, and the remaining six valence electrons will remain around bromine.

**Bonding:**
- N (5) : ••N••
- Br (7) : ••Br••

### b. Sulfur + Hydrogen
- **Sulfur (S)** has 6 valence electrons.
- **Hydrogen (H)** has 1 valence electron.
- Each hydrogen atom can form **one single bond** with sulfur. Sulfur can bond with **two hydrogen atoms** to satisfy its octet rule by sharing one electron from each hydrogen.

**Bonding:**
- S (6) : ••S••
- H (1) : •H , H

### c. Fluorine + Phosphorus
- **Fluorine (F)** has 7 valence electrons.
- **Phosphorus (P)** has 5 valence electrons.
- Phosphorus can share **three electrons** with three fluorine atoms to form **three single bonds** while phosphorous retains its remaining two.

**Bonding:**
- P (5): ••P••
- F (7): ••F •••, 3 times

### d. 2 Bromine
- Since there are **two bromine (Br)** atoms, they can share electrons to form a **single bond** between themselves.

**Bonding:**
- Br (7): ••Br•• , creates a bond with another Br
- Br (7): ••Br••

### e. Chlorine + Iodine
- **Chlorine (Cl)** has 7 valence electrons.
- **Iodine (I)** has 7 valence electrons.
- Chlorine and iodine can share **one pair** of electrons to form a **single bond**.

**Bonding:**
- Cl (7): ••Cl••
- I (7): ••I••

### f. Oxygen + Carbon
- **Oxygen (O)** has 6 valence electrons.
- **Carbon (C)** has 4 valence electrons.
- Oxygen can share **two pairs** of electrons with carbon, forming a **double bond** (2 pairs).

**Bonding:**
- O (6): ••O••
- C (4): ••C••

To diagrammatically represent them:
- The shared pairs are represented as lines or dots between the atoms.

Overall, bond formation involves sharing of their unpaired electrons leading to stable electron configurations for both atoms involved.