Chapter 4

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 element with electron configuration 1s²2s²2p⁶3s²3p²

• Si

• Mg

• S

• C

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.

The electron configuration for the carbon atom (C)is 1s²2s²2p². The atomic number of carbon is 

• 3.
• 11.
• 12.
• 6.

Tags

NGSS.HS-PS1-1

The atomic sublevel with the next hightest energy after 4p is

• 5s
• 4f
• 5p
• 4d

Tags

NGSS.HS-PS1-1

The part of the atom where the electrons CANNOT be fond is the 

• orbitals.
• nucleus.
• electron cloud.
• area surrounding the nucleus

With the quantum model of the atom, scientists have come to believe that determining an electron's exact location around the nucleus.

• can be done before 2005.
• can be done only with specialized equipment.
• is impossible.
• can be done easily.

The statement that an electron occupies the lowest available energy orbital is 

• the Pauli exclusion principle.
• Hund's rule.
• the Aufbau principle.
• Bohr's law.