2. (a) draw a model bohr diagram for lithium in the space provided.
(b) what process or change would turn this lithium atom into an ion?
(c) would the ion that it forms be positively or negatively charged?
explain.
3. (a) draw a bohr model diagram for fluorine in the space provided.
(b) what process or change would turn this fluorine atom into an ion?
(c) would this ion be positively charged or negatively charged?
explain.
4. lithium and fluorine react to form lithium fluoride. draw a diagram on the back of this page
to show how these two atoms would react.

Question

Accepted Answer

### 2. (a) Bohr Diagram for Lithium
# Explanation:
## Step1: Determine Protons, Neutrons, Electrons
Lithium (Li) has an atomic number of 3, so it has 3 protons (and 4 neutrons, but neutrons are not shown in a simple Bohr diagram). The electron configuration for Li is 2 electrons in the first shell (n=1) and 1 electron in the second shell (n=2).

## Step2: Draw the Nucleus and Shells
- Draw a small circle (nucleus) with “+3” (protons) inside.
- Draw the first electron shell (a circle around the nucleus) with 2 electrons (dots or crosses).
- Draw the second electron shell (a larger circle) with 1 electron.

### 2. (b) Process to Form a Lithium Ion
# Brief Explanations:
An atom becomes an ion by gaining or losing electrons. Lithium is a metal with 1 valence electron (in the outermost shell). To achieve a stable electron configuration (like a noble gas, He with 2 electrons in the first shell), lithium loses its 1 valence electron.

# Answer:
Losing its valence electron (or “losing an electron”).

### 2. (c) Charge of Lithium Ion
# Brief Explanations:
A lithium atom has 3 protons (+3 charge) and 3 electrons (-3 charge), so it is neutral. When it loses 1 electron, it has 3 protons (+3) and 2 electrons (-2). The net charge is $ +3 - 2 = +1 $, so it is positively charged (a cation).

# Answer:
Positively charged. Explanation: Lithium loses 1 electron, so protons (positive) outnumber electrons (negative), resulting in a net positive charge.

### 3. (a) Bohr Diagram for Fluorine
# Explanation:
## Step1: Determine Protons, Electrons
Fluorine (F) has an atomic number of 9, so 9 protons. Electron configuration: 2 electrons in the first shell (n=1), 7 electrons in the second shell (n=2).

## Step2: Draw the Nucleus and Shells
- Nucleus: “+9” (protons).
- First shell: 2 electrons.
- Second shell: 7 electrons.

### 3. (b) Process to Form a Fluorine Ion
# Brief Explanations:
Fluorine is a nonmetal with 7 valence electrons. To achieve a stable octet (8 electrons in the outermost shell, like Ne), it gains 1 electron.

# Answer:
Gaining an electron.

### 3. (c) Charge of Fluorine Ion
# Brief Explanations:
A fluorine atom has 9 protons (+9) and 9 electrons (-9), neutral. When it gains 1 electron, it has 9 protons (+9) and 10 electrons (-10). Net charge: $ +9 - 10 = -1 $, so it is negatively charged (an anion).

# Answer:
Negatively charged. Explanation: Fluorine gains 1 electron, so electrons (negative) outnumber protons (positive), resulting in a net negative charge.

### 4. Reaction of Lithium and Fluorine (Lithium Fluoride Formation)
# Explanation:
## Step1: Identify Ion Charges
Lithium (Li) loses 1 electron → $ \text{Li}^+ $ (cation). Fluorine (F) gains 1 electron → $ \text{F}^- $ (anion).

## Step2: Ionic Bonding Diagram
- Draw $ \text{Li}^+ $ (smaller ion, lost its valence electron) and $ \text{F}^- $ (larger ion, gained an electron to fill its valence shell).
- Show the transfer of the electron from Li to F: Li’s valence electron moves to F’s valence shell.
- The ions are attracted by electrostatic forces (opposite charges) to form $ \text{LiF} $.

(Note: For the diagram, represent Li with 2 electrons in the first shell (after losing 1), and F with 8 electrons in the second shell (after gaining 1). Draw the ions close together with a label like “Ionic bond: $ \text{Li}^+ $ and $ \text{F}^- $ attract.”)

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QUESTION IMAGE

Question

Explanation:

2. (a) Bohr Diagram for Lithium

Step1: Determine Protons, Neutrons, Electrons

Step2: Draw the Nucleus and Shells

2. (b) Process to Form a Lithium Ion

Answer:

2. (c) Charge of Lithium Ion