This chemistry worksheet helps students practice identifying atomic properties and drawing Lewis dot structures for ionic bonds.

Let’s solve this step by step.

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Part 1: Fill in the chart

We need to find for each element:
- # of Protons = atomic number (from periodic table)
- # of Electrons = same as protons if it’s a neutral atom (which we assume here unless told otherwise)
- # of Valence Electrons = electrons in the outermost shell (based on group number for main group elements)

Let’s go one by one:

#### Sodium (Na)
- Atomic number = 11 → Protons = 11
- Neutral atom → Electrons = 11
- Group 1 → Valence electrons = 1

#### Chlorine (Cl)
- Atomic number = 17 → Protons = 17
- Neutral atom → Electrons = 17
- Group 17 → Valence electrons = 7

#### Beryllium (Be)
- Atomic number = 4 → Protons = 4
- Neutral atom → Electrons = 4
- Group 2 → Valence electrons = 2

#### Fluorine (F)
- Atomic number = 9 → Protons = 9
- Neutral atom → Electrons = 9
- Group 17 → Valence electrons = 7

#### Lithium (Li)
- Atomic number = 3 → Protons = 3
- Neutral atom → Electrons = 3
- Group 1 → Valence electrons = 1

#### Oxygen (O)
- Atomic number = 8 → Protons = 8
- Neutral atom → Electrons = 8
- Group 16 → Valence electrons = 6

#### Phosphorus (P)
- Atomic number = 15 → Protons = 15
- Neutral atom → Electrons = 15
- Group 15 → Valence electrons = 5

✔ Chart filled correctly.

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Part 2: Ionic Bonds

For each pair, we do:
1. Write symbols
2. Draw Lewis dot structures (valence electrons only)
3. Show electron transfer with arrows
4. Write ion charges
5. Write chemical formula (make sure total charge = 0)

Let’s do each one:

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#### a) Sodium + Chlorine

- Symbols: Na and Cl
- Lewis dots:
- Na: [Na] with 1 dot
- Cl: [Cl] with 7 dots (or 3 pairs + 1 single)
- Transfer: Na gives 1 electron to Cl → arrow from Na to Cl
- Ions: Na⁺ and Cl
- Formula: NaCl (charges cancel: +1 and -1)

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#### b) Magnesium + Iodine

- Symbols: Mg and I
- Lewis dots:
- Mg: [Mg] with 2 dots
- I: [I] with 7 dots
- Transfer: Mg gives 1 electron to each of two I atoms → so we need TWO iodine atoms!
- Arrow from Mg to first I, another arrow from Mg to second I
- Ions: Mg²⁺ and I⁻ (each iodine gains 1 electron)
- Formula: MgI₂ (because +2 needs two -1 ions)

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#### c) Sodium + Oxygen

- Symbols: Na and O
- Lewis dots:
- Na: 1 dot
- O: 6 dots (2 lone pairs + 2 singles)
- Transfer: Each Na gives 1 electron. Oxygen needs 2 electrons → so we need TWO sodium atoms.
- Two arrows: one from each Na to O
- Ions: Na⁺ and O²⁻
- Formula: Na₂O (two +1 ions balance one -2 ion)

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#### d) Calcium + Chlorine

- Symbols: Ca and Cl
- Lewis dots:
- Ca: 2 dots
- Cl: 7 dots
- Transfer: Ca gives 1 electron to each of two Cl atoms → two arrows
- Ions: Ca²⁺ and Cl⁻
- Formula: CaCl₂ (+2 balanced by two -1)

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#### e) Aluminum + Chlorine

- Symbols: Al and Cl
- Lewis dots:
- Al: 3 dots (Group 13)
- Cl: 7 dots
- Transfer: Al gives 1 electron to each of three Cl atoms → three arrows
- Ions: Al³⁺ and Cl⁻
- Formula: AlCl₃ (+3 balanced by three -1)

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✔ All parts solved carefully.

Final Answer:

Part 1 Chart:

| Element | # of Protons | # of Electrons | # of Valence Electrons |
|-------------|--------------|----------------|-------------------------|
| Sodium | 11 | 11 | 1 |
| Chlorine | 17 | 17 | 7 |
| Beryllium | 4 | 4 | 2 |
| Fluorine | 9 | 9 | 7 |
| Lithium | 3 | 3 | 1 |
| Oxygen | 8 | 8 | 6 |
| Phosphorus | 15 | 15 | 5 |

Part 2 Ionic Bonds:

a)
Symbols: Na, Cl
Lewis: Na• , •Cl: (with 6 more dots around Cl — total 7)
Arrow: Na → Cl
Ions: Na⁺, Cl
Formula: NaCl

b)
Symbols: Mg, I
Lewis: •Mg• , •I: (7 dots)
Arrows: Mg → I and Mg → I (needs 2 I atoms)
Ions: Mg²⁺, I⁻
Formula: MgI₂

c)
Symbols: Na, O
Lewis: Na• , :Ö: (6 dots)
Arrows: Na → O and Na → O (needs 2 Na atoms)
Ions: Na⁺, O²⁻
Formula: Na₂O

d)
Symbols: Ca, Cl
Lewis: •Ca• , •Cl: (7 dots)
Arrows: Ca → Cl and Ca → Cl (needs 2 Cl atoms)
Ions: Ca²⁺, Cl
Formula: CaCl₂

e)
Symbols: Al, Cl
Lewis: •Al• (3 dots), •Cl: (7 dots)
Arrows: Al → Cl, Al → Cl, Al → Cl (needs 3 Cl atoms)
Ions: Al³⁺, Cl⁻
Formula: AlCl₃