Atomic orbitals worksheet - Free Printable
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Step-by-step solution for: Atomic orbitals worksheet
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Show Answer Key & Explanations
Step-by-step solution for: Atomic orbitals worksheet
Here are the answers to the questions on your worksheet, broken down step-by-step.
1. How did Bohr expand on Rutherford’s model of the atom?
Rutherford discovered the nucleus but couldn't explain why electrons didn't spiral into it. Bohr expanded this by proposing that electrons travel in specific, fixed circular paths (orbits) around the nucleus, similar to planets orbiting the sun. He stated that electrons can only exist at certain energy levels and cannot exist in between them.
2. Compare the energy of an electron in the ground state and an electron in the excited state.
The ground state is the lowest possible energy level for an electron; it is the most stable position, closest to the nucleus. An excited state occurs when an electron absorbs energy and jumps to a higher energy level further away from the nucleus. Therefore, an electron in an excited state has more energy than one in the ground state.
3. When an electron falls from a higher energy level to a lower energy level, how is the energy released?
When an electron drops down to a lower level, it loses the extra energy it was holding. This energy is released in the form of light, specifically as a photon (a packet of electromagnetic radiation). The color of the light depends on exactly how much energy is released.
4. What is the difference between the previous models of the atom and the modern quantum mechanical model?
Previous models (like Bohr's) treated electrons like solid particles moving in definite, predictable paths or tracks. The modern quantum mechanical model treats electrons more like waves. It does not predict the exact path of an electron; instead, it calculates the probability of finding an electron in a certain region of space (called an orbital).
5. The further the electron is from the nucleus, the \_\_\_\_\_\_\_\_\_\_ energy the electron has.
Electrons are attracted to the positive nucleus. To move an electron further away against this attraction requires work/energy. Therefore, the further away it is, the more potential energy it holds.
*Answer:* higher (or more)
6. A(n) \_\_\_\_\_\_\_\_\_\_ is often thought of as a region of space in which there is a high probability of finding an electron.
In the modern model, we don't use "orbits" (lines); we use 3D shapes where the electron is likely to be found 90% of the time.
*Answer:* atomic orbital (or just orbital)
7. What is the term used to label the energy levels of electrons?
The main energy levels are labeled with whole numbers starting from 1 ($n=1, n=2, n=3$, etc.). These are called principal energy levels.
*Answer:* Principal Quantum Number (represented by the letter $n$)
8. How are s orbitals different from p orbitals?
This refers to their shape.
* s orbitals are shaped like a sphere.
* p orbitals are shaped like a dumbbell (or two lobes).
9. How many electrons can each of the following orbitals hold?
*Rule:* No matter what type of orbital it is ($s, p, d,$ or $f$), a single orbital can hold a maximum of 2 electrons (with opposite spins).
* a. 2s: 2
* b. 3p: 2
* c. 5f: 2
* d. 6d: 2
* e. 4p: 2
* f. 3d: 2
10. How many “p” orbitals can there be in any energy level?
The $p$ sublevel always consists of three distinct orbitals oriented along the x, y, and z axes ($p_x, p_y, p_z$).
*Answer:* 3
11. What is the *maximum* number of electrons in the 3rd principle energy level?
To find the max electrons in a main energy level ($n$), use the formula $2n^2$.
* Here, $n = 3$.
* Calculation: $2 \times (3)^2 = 2 \times 9 = 18$.
* *Check:* Level 3 has sublevels $3s$ (2 e-), $3p$ (6 e-), and $3d$ (10 e-). Total = $2 + 6 + 10 = 18$.
*Answer:* 18
12. How many orbitals are in each of the following sublevels?
* s sublevel: Always has 1 orbital.
* p sublevel: Always has 3 orbitals.
* d sublevel: Always has 5 orbitals.
* f sublevel: Always has 7 orbitals.
* a. 4p sublevel: 3
* b. 3d sublevel: 5
* c. 4f sublevel: 7
* d. 2s sublevel: 1
──────────────────────────────────────
Final Answer:
1. Bohr proposed that electrons move in fixed, circular orbits (energy levels) around the nucleus, rather than randomly.
2. An electron in an excited state has higher energy than an electron in the ground state.
3. The energy is released as light (a photon).
4. Previous models viewed electrons as particles in fixed paths; the quantum mechanical model views them as waves and predicts the probability of their location (orbitals).
5. higher (or more)
6. orbital (or atomic orbital)
7. Principal Quantum Number (or $n$)
8. s orbitals are spherical, while p orbitals are dumbbell-shaped.
9. a. 2, b. 2, c. 2, d. 2, e. 2, f. 2
10. 3
11. 18
12. a. 3, b. 5, c. 7, d. 1
Step-by-Step Solutions
1. How did Bohr expand on Rutherford’s model of the atom?
Rutherford discovered the nucleus but couldn't explain why electrons didn't spiral into it. Bohr expanded this by proposing that electrons travel in specific, fixed circular paths (orbits) around the nucleus, similar to planets orbiting the sun. He stated that electrons can only exist at certain energy levels and cannot exist in between them.
2. Compare the energy of an electron in the ground state and an electron in the excited state.
The ground state is the lowest possible energy level for an electron; it is the most stable position, closest to the nucleus. An excited state occurs when an electron absorbs energy and jumps to a higher energy level further away from the nucleus. Therefore, an electron in an excited state has more energy than one in the ground state.
3. When an electron falls from a higher energy level to a lower energy level, how is the energy released?
When an electron drops down to a lower level, it loses the extra energy it was holding. This energy is released in the form of light, specifically as a photon (a packet of electromagnetic radiation). The color of the light depends on exactly how much energy is released.
4. What is the difference between the previous models of the atom and the modern quantum mechanical model?
Previous models (like Bohr's) treated electrons like solid particles moving in definite, predictable paths or tracks. The modern quantum mechanical model treats electrons more like waves. It does not predict the exact path of an electron; instead, it calculates the probability of finding an electron in a certain region of space (called an orbital).
5. The further the electron is from the nucleus, the \_\_\_\_\_\_\_\_\_\_ energy the electron has.
Electrons are attracted to the positive nucleus. To move an electron further away against this attraction requires work/energy. Therefore, the further away it is, the more potential energy it holds.
*Answer:* higher (or more)
6. A(n) \_\_\_\_\_\_\_\_\_\_ is often thought of as a region of space in which there is a high probability of finding an electron.
In the modern model, we don't use "orbits" (lines); we use 3D shapes where the electron is likely to be found 90% of the time.
*Answer:* atomic orbital (or just orbital)
7. What is the term used to label the energy levels of electrons?
The main energy levels are labeled with whole numbers starting from 1 ($n=1, n=2, n=3$, etc.). These are called principal energy levels.
*Answer:* Principal Quantum Number (represented by the letter $n$)
8. How are s orbitals different from p orbitals?
This refers to their shape.
* s orbitals are shaped like a sphere.
* p orbitals are shaped like a dumbbell (or two lobes).
9. How many electrons can each of the following orbitals hold?
*Rule:* No matter what type of orbital it is ($s, p, d,$ or $f$), a single orbital can hold a maximum of 2 electrons (with opposite spins).
* a. 2s: 2
* b. 3p: 2
* c. 5f: 2
* d. 6d: 2
* e. 4p: 2
* f. 3d: 2
10. How many “p” orbitals can there be in any energy level?
The $p$ sublevel always consists of three distinct orbitals oriented along the x, y, and z axes ($p_x, p_y, p_z$).
*Answer:* 3
11. What is the *maximum* number of electrons in the 3rd principle energy level?
To find the max electrons in a main energy level ($n$), use the formula $2n^2$.
* Here, $n = 3$.
* Calculation: $2 \times (3)^2 = 2 \times 9 = 18$.
* *Check:* Level 3 has sublevels $3s$ (2 e-), $3p$ (6 e-), and $3d$ (10 e-). Total = $2 + 6 + 10 = 18$.
*Answer:* 18
12. How many orbitals are in each of the following sublevels?
* s sublevel: Always has 1 orbital.
* p sublevel: Always has 3 orbitals.
* d sublevel: Always has 5 orbitals.
* f sublevel: Always has 7 orbitals.
* a. 4p sublevel: 3
* b. 3d sublevel: 5
* c. 4f sublevel: 7
* d. 2s sublevel: 1
──────────────────────────────────────
Final Answer:
1. Bohr proposed that electrons move in fixed, circular orbits (energy levels) around the nucleus, rather than randomly.
2. An electron in an excited state has higher energy than an electron in the ground state.
3. The energy is released as light (a photon).
4. Previous models viewed electrons as particles in fixed paths; the quantum mechanical model views them as waves and predicts the probability of their location (orbitals).
5. higher (or more)
6. orbital (or atomic orbital)
7. Principal Quantum Number (or $n$)
8. s orbitals are spherical, while p orbitals are dumbbell-shaped.
9. a. 2, b. 2, c. 2, d. 2, e. 2, f. 2
10. 3
11. 18
12. a. 3, b. 5, c. 7, d. 1
Parent Tip: Review the logic above to help your child master the concept of atomic orbitals worksheet.
