2.2 QUANTUM MECHANICAL MODEL

How many orbitals make up the d subshell?

• 1

• 5

• 3

• 7

What orbital is shown in the picture?

• s orbital

• p orbital

• d orbital

• f orbital

Tags

NGSS.HS-PS1-1

Which quantum number represents the shape of the orbital?

• principal quantum number

• azimuthal (angular momentum) quantum number

• magnetic quantum number

• spin quantum number

What is the purpose of the quantum numbers?

• To calculate wavelength associated with the moving electron.

• To calculate velocity associated with the moving electron.

• To predict the probable location of an electron in the Bohr model.

• To predict the probable location of an electron in the quantum mechanical model.

What is the difference in a 1s orbital and a 2s orbital?

• The shape of the orbital

• The size of the orbital

• The number of electrons it can hold

• None of the above

Which quantum number represents the orientation of the orbital?

• principal quantum number

• azimuthal (angular momentum) quantum number

• magnetic quantum number

• spin quantum number

Which of the following values does NOT represent a valid electron?

• n=(2), l=(1), ml=(1), ms=(+1/2)

• n=(4), l=(2), ml=(-1), ms=(-1/2)

• n=(2), l=(0), ml=(0), m=(-1/2)

• n=(4), l=(2), ml=(-3), ms=(+1/2)

What states that every orbital of a subshell must be singly occupied before any orbital can have a pair?

• Pauli exclusion principle

• Hund's rule

• Aufbau principle

• None of the above

This states that no two electrons will have the same 4 quantum numbers in an atom or molecule. The two electrons of the same orbital must have opposite spin states.

• Pauli exclusion principle

• Hund's rule

• Aufbau principle

• None of the above

What states that electrons fill the lowest energy orbitals/levels first before occupying higher energy levels?

• Pauli exclusion principle

• Hund's rule

• Aufbau Principle

• None of the above