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Dungeon
Ikut Turutan
Universiti
Kimia
Quantum Numbers and Atomic Orbitals
Shaikh Ameerul
35
Masalah tambahan (15/ 20)
Allow incorrect answer
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# 1

pilihan

What is an orbital?

  • A 3D region around an atom's nucleus where there is a high probability of finding an electron.

  • A pathway that electrons follow in a fixed circle around the nucleus.
  • A positively charged particle found inside the nucleus of an atom.
  • A type of chemical bond formed by the sharing of electron pairs between atoms.

# 2

pilihan

What does the principal quantum number (n) indicates?

  • It indicates the spin direction of an electron.

  • It indicates the energy level of an orbital and relates the average distance of the electron from the nucleus

  • It determines the orientation of an orbital in space.

  • It describes the shape of the orbital.

# 3

pilihan

What does the angular momentum quantum number (l) indicates?

  • It describes the total number of electrons in an atom.

  • It determines the energy level of an orbital.

  • It indicates the orientation of orbital in space.

  • It indicates the type of orbitals and their shape in shell.

# 4

pilihan

What does the magnetic quantum number (m) indicates?

  • The size of the atomic orbital.

  • The energy level of the orbital

  • The orientation of an atomic orbital in space relative to the other orbitals.
  • The shape of the atomic orbital.

# 5

pilihan

What does the electron spin quantum number indicates?

  • How fast the electron spins.

  • How many times the electron can spin

  • The spin of electron on its own axis (clockwise or counterclockwise)

  • The spin energy of an electron.

# 6

pilihan

If n = 1, what possible values can 'l' have?

  • l = 2

  • l = 0

  • l = 1

  • l = -1

# 7

pilihan

Name the subshell with n = 1 and l = 0

  • 1p

  • s

  • 1d

  • 1s

# 8

pilihan

Name the subshell with n = 3, l = 2

  • 3f

  • 3d

  • 3p

  • 3s

# 9

pilihan

(Multiple Answer Question): Which of the following are the orbitals associated with n = 3, l = 2? (Select all that applies)

  • ​3dxy​​3d_{xy}​

  • ​3dz2​​3d_{z^2}​

  • ​3px​​3p_{x}​

  • ​3dx2−y2​​3d_{x^2-y^2}​

  • ​3pz​​3p_{z}​

# 10

pilihan

Which of the following 4 set of quantum numbers (n, l, m, s) CANNOT exist? (Select all that applies)

  • (2, 0, 0, +1/2)

  • (3, 1, -3, -1/2)

  • (0, 1, 0, -1/2)

  • (2, 2, +1, +1/2)

  • (2, 1, 0, +1)

# 11

pilihan

Which of the following orbitals CAN exist? (Select all that applies)

  • 1s

  • 2p

  • 3f

  • 4s

  • 2d

# 12

pilihan

What is the 4 set of quantum numbers (n, l, m, s) of an electron inside this orbital?

  • (3, 1, -1, +1/2)

  • (2, 2, +1, +1/2)

  • (2, 1, 0, -1/2)

  • (3, 2, +2, +1/2)

<p>What is the 4 set of quantum numbers (n, l, m, s) of an electron inside this orbital?</p>

# 13

pilihan

What orbital is this?

  • ​3px​​3p_{x}​

  • ​3dz2​​3d_{z^2}​

  • ​3dxy​​3d_{xy}​

  • ​3dx2−y2​​3d_{x^2-y^2}​

<p>What orbital is this?</p>

# 14

pilihan

Given n = 5, l = 2, how many orbitals are there, and how many electrons can be placed inside?

  • 1 orbital, 2 electrons

  • 2 orbitals, 4 electrons

  • 3 orbitals, 6 electrons

  • 5 orbitals, 10 electrons

# 15

pilihan

Given n = 6, l = 1, how many orbitals are there, and how many electrons can be placed inside?

  • 1 orbital, 2 electrons

  • 3 orbitals, 6 electrons

  • 5 orbitals, 10 electrons

  • 6 orbitals, 12 electrons

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