Quiz: Principles of electronic distribution

Electron Configuration Challenges Quiz

Introduction:

Test your knowledge on quantum numbers and their applications.Identify key concepts related to orbital shapes and electron arrangements.

Test your grasp of fundamental chemistry concepts with this diverse quiz. From electron configurations to orbital shapes, challenge yourself with questions covering a range of topics. Perfect for reinforcing your knowledge and identifying areas for improvement

Quiz 1

Here’s a multiple-choice quiz based on the lesson about quantum numbers and electron configurations:

1)What does the Pauli Exclusion Principle state?

1. Electrons in the same orbital have opposite spins.
2. Electrons in the same atom can have the same set of quantum numbers.
3. No two electrons in an atom can have the same set of four quantum numbers.
4. Electrons fill orbitals from lowest energy to highest energy.

2)Which of the following quantum numbers specifies the orientation or spatial orientation of an orbital?

1. Principal Quantum Number (n)
2. Azimuthal Quantum Number (l)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

3)According to Hund’s Rule, how do electrons fill degenerate orbitals?

1. Electrons fill degenerate orbitals with parallel spins before pairing up.
2. Electrons fill degenerate orbitals with opposite spins before pairing up.
3. Electrons always pair up in degenerate orbitals first.
4. Electrons fill orbitals based on their energy level.

4)The electron configuration for carbon (C) using the building-up principle is:

1. 1s² 2s² 2p³
2. 1s² 2s² 2p⁴
3. 1s² 2s¹ 2p²
4. 1s² 2s² 2p²

5)If the sum of (n + l) is the same for two sublevels, how do they compare in energy?

1. The sublevel with the larger value of (n + l) is lower in energy.
2. The sublevel with the smaller value of (n + l) is lower in energy.
3. They have the same energy.
4. The value of (n + l) doesn’t affect energy.

6)What is the maximum number of electrons that an “s” orbital can hold?

1. 1
2. 2
3. 6
4. 8

7)Which of the following represents the quantum numbers for the valence electrons in an aluminum (Al) atom?

1. (n = 3, l = 1, ml = 0, ms = +1/2)
2. (n = 3, l = 0, ml = 0, ms = +1/2)
3. (n = 2, l = 2, ml = 0, ms = -1/2)
4. (n = 4, l = 2, ml = 2, ms = +1/2)

8)What is the electron configuration for neon (Ne) following the building-up principle?

1. 1s² 2s² 2p⁶
2. 1s² 2s² 2p⁴
3. 1s² 2s² 2p⁶ 3s²
4. 1s² 2s² 2p⁶ 3s² 3p⁶

Answers:

1)c. No two electrons in an atom can have the same set of four quantum numbers.

2)c. Magnetic Quantum Number (ml)

3)a. Electrons fill degenerate orbitals with parallel spins before pairing up.

4)b. 1s² 2s² 2p⁴

5)b. The sublevel with the smaller value of (n + l) is lower in energy.

6)b. 2

7)b. (n = 3, l = 0, ml = 0, ms = +1/2)

8)d. 1s² 2s² 2p⁶ 3s² 3p⁶

Quiz 3

1)What is the maximum number of electrons that can occupy the 3p sublevel?

1. 2
2. 6
3. 8
4. 10

2)Which quantum number determines the shape of an orbital?

1. Principal Quantum Number (n)
2. Azimuthal Quantum Number (l)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

3)What is the electron configuration for sulfur (S) using the building-up principle?

1. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁴
2. 1s² 2s² 2p⁶ 3s² 3p³
3. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹
4. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

4)Which quantum number is responsible for dividing electron sublevels into orbitals?

1. Principal Quantum Number (n)
2. Azimuthal Quantum Number (l)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

5)The quantum numbers for the valence electrons of a nitrogen (N) atom are:

1. (n = 2, l = 0, ml = 0, ms = +1/2) and (n = 2, l = 0, ml = 0, ms = -1/2)
2. (n = 2, l = 1, ml = -1, ms = +1/2) and (n = 2, l = 1, ml = -1, ms = -1/2)
3. (n = 1, l = 0, ml = 0, ms = +1/2) and (n = 2, l = 0, ml = 0, ms = -1/2)
4. (n = 2, l = 1, ml = 0, ms = +1/2) and (n = 2, l = 1, ml = 0, ms = -1/2)

6)Which of the following elements has an electron configuration that ends with “4p³”?

1. Oxygen (O)
2. Fluorine (F)
3. Sulfur (S)
4. Phosphorus (P)

Answers:

1) b. 6

2)b. Azimuthal Quantum Number (l)

3)a. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁴

4)c. Magnetic Quantum Number (ml)

5)b. (n = 2, l = 1, ml = -1, ms = +1/2) and (n = 2, l = 1, ml = -1, ms = -1/2)

6)c. Sulfur (S)

Quiz 4

1)What is the electron configuration for a neutral helium (He) atom?

1. 1s²
2. 1s² 2s²
3. 1s² 2s² 2p⁶
4. 1s² 2s² 2p⁶ 3s²

 

2)In which sublevel would you find an electron with the quantum numbers (n = 3, l = 2, ml = -1, ms = +1/2)?

 

1. 3s
2. 3p
3. 3d
4. 3f

3)How many unpaired electrons are there in an atom with the electron configuration 1s² 2s² 2p⁶ 3s² 3p³?

1. 0
2. 1
3. 2
4. 3

4)Which of the following elements has the highest principal quantum number (n) for its valence electrons?

1. Sodium (Na)
2. Potassium (K)
3. Calcium (Ca)
4. Magnesium (Mg)

5)What is the electron configuration of a chlorine (Cl) ion with a charge of -1?

1. 1s² 2s² 2p⁶ 3s² 3p⁵
2. 1s² 2s² 2p⁶ 3s² 3p⁶
3. 1s² 2s² 2p⁶ 3s² 3p³
4. 1s² 2s² 2p⁶ 3s² 3p⁴

6)Which of the following quantum numbers describes the shape of an orbital?

1. Principal Quantum Number (n)
2. Azimuthal Quantum Number (l)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

Answers:

1). a. 1s²

2)c. 3d

3)d. 3

4)b. Potassium (K)

5)a. 1s² 2s² 2p⁶ 3s² 3p⁵

6)b. Azimuthal Quantum Number (l)

Quiz

1)How many unpaired electrons are there in an atom with the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁵?

1. 0
2. 1
3. 2
4. 3

2)In the electron configuration 1s² 2s² 2p⁶ 3s² 3p³, which sublevel contains the valence electrons?

1. 2s
2. 2p
3. 3s
4. 3p

3)What is the electron configuration of a neutral nitrogen (N) atom?

1. 1s² 2s² 2p³
2. 1s² 2s² 2p⁴
3. 1s² 2s² 2p⁶
4. 1s² 2s² 2p⁶ 3s²

4)Which of the following quantum numbers describes the orientation or spatial orientation of an orbital?

1. Principal Quantum Number (n)
2. Azimuthal Quantum Number (l)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

5)How many electrons can the 2p sublevel hold?

1. 2
2. 4
3. 6
4. 8

6)Which of the following elements has an electron configuration ending in “3p³”?

1. Carbon (C)
2. Nitrogen (N)
3. Oxygen (O)
4. Fluorine (F)

Answers:

1). d. 3

2)d. 3p

3)a. 1s² 2s² 2p³

4)c. Magnetic Quantum Number (ml)

5)b. 4

6)b. Nitrogen (N)

Quiz

1)Which of the following elements has an electron configuration ending in “4p⁶”?

1. Chlorine (Cl)
2. Sulfur (S)
3. Argon (Ar)
4. Phosphorus (P)

2)What is the electron configuration of a neutral magnesium (Mg) atom?

1. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
2. 1s² 2s² 2p⁶ 3s² 3p³
3. 1s² 2s² 2p⁶ 3s² 3p⁶
4. 1s² 2s² 2p⁶ 3s² 3p⁴

3)In which sublevel would you find an electron with the quantum numbers (n = 4, l = 1, ml = 0, ms = -1/2)?

1. 4s
2. 4p
3. 4d
4. 4f

4)How many electrons can the “d” sublevel hold?

1. 2
2. 6
3. 10
4. 14

5)The electron configuration for oxygen (O) using the building-up principle is:

1. 1s² 2s² 2p⁶
2. 1s² 2s² 2p⁴
3. 1s² 2s² 2p⁶ 3s²
4. 1s² 2s² 2p⁶ 3s² 3p⁴

Answers:

1). b. Sulfur (S)

2)a. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

3)b. 4p

4)c. 10

5)a. 1s² 2s² 2p⁶

Quiz

1)What is the maximum number of electrons that can occupy the 2s sublevel?

1. 2
2. 4
3. 6
4. 8

2)What is the electron configuration for a neutral lithium (Li) atom?

1. 1s² 2s²
2. 1s² 2s² 2p⁶
3. 1s² 2s¹
4. 1s² 2s² 2p⁶ 3s²

3)In the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁵, how many unpaired electrons are there?

1. 0
2. 1
3. 2
4. 3

4)Which of the following quantum numbers describes the spin direction of an electron?

1. Principal Quantum Number (n)
2. Azimuthal Quantum Number (l)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

5)What is the electron configuration of a fluoride ion (F-)?

1. 1s² 2s² 2p⁶
2. 1s² 2s² 2p⁶ 3s²
3. 1s² 2s² 2p⁶ 3s² 3p⁶
4. 1s² 2s² 2p⁶ 3s² 3p⁵

Answers:

1). a. 2

2)c. 1s² 2s¹

3)d. 3

4)d. Spin Quantum Number (ms)

5)d. 1s² 2s² 2p⁶ 3s² 3p⁵

 

1)What is the electron configuration for a neutral nitrogen (N) atom using the building-up principle?

1. 1s² 2s² 2p⁴
2. 1s² 2s² 2p⁵
3. 1s² 2s² 2p⁶
4. 1s² 2s² 2p⁶ 3s²

2)How many electrons can the “f” sublevel hold?

1. 2
2. 6
3. 10
4. 14

3)In the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s², which sublevel contains the valence electrons?

1. 2s
2. 3p
3. 4s
4. 3s

4)Which of the following elements has the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²?

1. Calcium (Ca)
2. Sodium (Na)
3. Potassium (K)
4. Argon (Ar)

Answers:

1). a. 1s² 2s² 2p⁴

2)d. 14

3)c. 4s

4)a. Calcium (Ca)

1)What is the maximum number of electrons that can occupy the 3d sublevel?

1. 2
2. 6
3. 10
4. 14

2)In the electron configuration 1s² 2s² 2p⁶ 3s² 3p³, how many unpaired electrons are there?

1. 0
2. 1
3. 2
4. 3

3)Which of the following quantum numbers describes the orientation or spatial orientation of an orbital?

1. Principal Quantum Number (n)
2. Azimuthal Quantum Number (l)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

4)What is the electron configuration of a chloride ion (Cl-)?

1. 1s² 2s² 2p⁶
2. 1s² 2s² 2p⁶ 3s²
3. 1s² 2s² 2p⁶ 3s² 3p⁶
4. 1s² 2s² 2p⁶ 3s² 3p⁵

5)How many orbitals are there in the “p” sublevel?

1. 1
2. 2
3. 3
4. 4

Answers:

1). c. 10

2)b. 1

3)b. Azimuthal Quantum Number (l)

4)d. 1s² 2s² 2p⁶ 3s² 3p⁵

5)c. 3

*********

1)Which of the following elements has an electron configuration that ends with “3p⁵”?

1. Phosphorus (P)
2. Sulfur (S)
3. Chlorine (Cl)
4. Argon (Ar)

2)How many unpaired electrons are there in an atom with the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁴?

1. 0
2. 1
3. 2
4. 3

3)In the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁴, which sublevel contains the valence electrons?

1. 3s
2. 3p
3. 2p
4. 2s

4)What is the electron configuration of a neutral potassium (K) atom?

1. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
2. 1s² 2s² 2p⁶ 3s² 3p³
3. 1s² 2s² 2p⁶ 3s² 3p⁶
4. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹

5)How many electrons can the “s” sublevel hold?

1. 1
2. 2
3. 6
4. 10

Answers:

1). a. Phosphorus (P)

2)b. 1

3)b. 3p

4)a. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

5)b. 2

1)What is the electron configuration for a neutral neon (Ne) atom?

1. 1s² 2s² 2p⁶
2. 1s² 2s² 2p⁴
3. 1s² 2s² 2p⁶ 3s²
4. 1s² 2s² 2p⁶ 3s² 3p⁶

2)How many unpaired electrons are there in an atom with the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²?

1. 0
2. 1
3. 2
4. 3

3)In the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶, which sublevel contains the valence electrons?

1. 3s
2. 3p
3. 2p
4. 2s

4)What is the electron configuration of a neutral iodine (I) atom?

1. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶
2. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶
3. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁶ 5s²
4. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁵

5)How many electrons can the “p” sublevel hold?

1. 1
2. 2
3. 6
4. 10

Answers:

1). a. 1s² 2s² 2p⁶

2)a. 0

3)a. 3s

4)a. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶

5)c. 6