QUESTION IMAGE
Question
how does ionization energy change across a period? 1. label your x-axis as atomic number and the y-axis as ionization energy 2. fill in the table below 3. use this link: http://bit.ly/462joem 3. plot on your graphs
element name
lithium
boron
oxygen
fluorine
atomic number
ionization energy
To solve this problem, we first need to find the atomic number and ionization energy for each element:
Step 1: Determine Atomic Numbers
- Lithium (Li): Atomic number = 3
- Boron (B): Atomic number = 5
- Oxygen (O): Atomic number = 8
- Fluorine (F): Atomic number = 9
Step 2: Find Ionization Energies (using the provided link or reference data)
- Lithium (Li): First ionization energy ≈ 520 kJ/mol
- Boron (B): First ionization energy ≈ 801 kJ/mol
- Oxygen (O): First ionization energy ≈ 1314 kJ/mol
- Fluorine (F): First ionization energy ≈ 1681 kJ/mol
Step 3: Fill the Table
| Element Name | Atomic Number | Ionization Energy (kJ/mol) |
|---|---|---|
| Boron | 5 | 801 |
| Oxygen | 8 | 1314 |
| Fluorine | 9 | 1681 |
Step 4: Plot the Graph
- X - axis: Atomic number (3, 5, 8, 9)
- Y - axis: Ionization energy (520, 801, 1314, 1681)
- Plot points: (3, 520), (5, 801), (8, 1314), (9, 1681)
- Connect the points to observe the trend (ionization energy generally increases across a period due to increasing effective nuclear charge, pulling electrons closer to the nucleus, making them harder to remove).
Final Table (Filled)
| Element Name | Atomic Number | Ionization Energy (kJ/mol) |
|---|---|---|
| Boron | 5 | 801 |
| Oxygen | 8 | 1314 |
| Fluorine | 9 | 1681 |
Trend Observation
Across a period (from left to right), ionization energy increases because:
- The number of protons (atomic number) increases, so the nucleus pulls electrons more strongly (higher effective nuclear charge).
- Electrons are added to the same energy level, so shielding from inner electrons remains constant. This makes it harder to remove the outermost electron, increasing ionization energy.
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To solve this problem, we first need to find the atomic number and ionization energy for each element:
Step 1: Determine Atomic Numbers
- Lithium (Li): Atomic number = 3
- Boron (B): Atomic number = 5
- Oxygen (O): Atomic number = 8
- Fluorine (F): Atomic number = 9
Step 2: Find Ionization Energies (using the provided link or reference data)
- Lithium (Li): First ionization energy ≈ 520 kJ/mol
- Boron (B): First ionization energy ≈ 801 kJ/mol
- Oxygen (O): First ionization energy ≈ 1314 kJ/mol
- Fluorine (F): First ionization energy ≈ 1681 kJ/mol
Step 3: Fill the Table
| Element Name | Atomic Number | Ionization Energy (kJ/mol) |
|---|---|---|
| Boron | 5 | 801 |
| Oxygen | 8 | 1314 |
| Fluorine | 9 | 1681 |
Step 4: Plot the Graph
- X - axis: Atomic number (3, 5, 8, 9)
- Y - axis: Ionization energy (520, 801, 1314, 1681)
- Plot points: (3, 520), (5, 801), (8, 1314), (9, 1681)
- Connect the points to observe the trend (ionization energy generally increases across a period due to increasing effective nuclear charge, pulling electrons closer to the nucleus, making them harder to remove).
Final Table (Filled)
| Element Name | Atomic Number | Ionization Energy (kJ/mol) |
|---|---|---|
| Boron | 5 | 801 |
| Oxygen | 8 | 1314 |
| Fluorine | 9 | 1681 |
Trend Observation
Across a period (from left to right), ionization energy increases because:
- The number of protons (atomic number) increases, so the nucleus pulls electrons more strongly (higher effective nuclear charge).
- Electrons are added to the same energy level, so shielding from inner electrons remains constant. This makes it harder to remove the outermost electron, increasing ionization energy.