Quantum Chemistry and Electron Configurations

What is a quantum?

• A "particle" of energy

• A light wave

• A proton

• A neutron

Tags

NGSS.HS-PS4-3

Light and electrons have properties of....(select all that apply)

• Waves

• Particles

• neutrons

• protons

Tags

NGSS.HS-PS4-3

The line spectrum of hydrogen is caused by when electrons release energy by

• Moving to a lower energy level

• Moving to a higher energy level

• Moving to an excited state

• Absorbing energy

Tags

NGSS.HS-PS4-3

What happens when an electron moves from n=1 to n=2?

• Absorbs energy

• Releases energy

• nothing

• releases a photon

Tags

NGSS.HS-PS1-2

What things does the Heisenberg Uncertainty Principle say that you CAN NOT know at the same time? (select all that apply)

• position

• momentum

• mass

• energy

Which of these only applies to the Bohr Model? (select all that apply)

• Described as an electron cloud

• Electrons are in orbitals

• Electrons behave like a particle

• Tried to determine the exact location of an electron

• Model was based on math equations

The major difference between a 1s orbital and a 2 s orbital is that

• the 2 s orbital is at a higher energy level.
• the 2s orbital has a slightly different shape.
• the 1 s orbital can have only one electron.
• the 2s orbital can hold more electrons.

The p orbitals are shaped like

• circles.
• dumbbells.
• spheres.
• electrons.

A spherical electron cloud surrounding an atomic nucleus would best represent

• a p_x orbital.
• a combination of an s and a p_x orbital.
• an s orbital.
• a combination of p_x and p_y orbitals.

The Pauli exclusion principle states that no two electrons in the same orbital can 

• have the same set of quantum numbers.
• be at the same main energy level.
• have the same spin.
• occupy the same orbital.