How many valence electrons are represented here?

• 7

• 5

• 2

• 8

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

What is this element?

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶

• Argon

• Krypton

• Selenium

• Bromide

Tags

NGSS.HS-PS1-1

There are 4 different types of subshells(orbitals) s,p,d,f

• true

• false

Which electron configuration belongs to Copper (Cu)?

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁹

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

Tags

NGSS.HS-PS1-1

How many electron can be found in a p orbital?

• 2

• 3

• 4

• 6

What is the electronic configuration of iron?

• 1s²2s²2p⁶3s²3p⁶4s²3d⁶

• 1s²2s²2p⁶3s²3p⁶3d⁸

• 1s²2p⁶3s²3p⁶4s²3d⁶

• 1s²2s²2p⁶3s²3p⁶4s¹3d⁶

Tags

NGSS.HS-PS1-1

What atom matches this electron configuration?
1s² 2s² 2p⁶ 3s²

• Neon

• Magnesium

• Aluminum

• Potassium

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which area on the periodic table represents the electrons in the "d" sublevel?

• representative elements

• columns 3-8

• rare earth elements

• transition elements

According to Pauli Exclusion Principle, how many electrons may occupy a single orbital?

• 1

• 2

• 4

• 8

What rule states that single electrons must occupy each equal-energy orbital before additional electrons can occupy the same orbitals.

• Hund's rule

• Pauli Exclusion Principle

• Aufbau Principle

• None of the choices.