Chemistry ch.13 review

............................. is the way in which electrons are arranged in various orbitals around the nuclei of atoms.

• Electron configuration

• Proton configuration

• Neutron configuration

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NGSS.HS-PS1-1

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“electrons occupy the orbitals of the lowest energy first”.

• Aufbau principle

• Pauli Exclusion Principle

• Hund’s rule

“An atomic orbital may describe at most two electrons”.

• Aufbau principle

• Pauli Exclusion Principle

• Hund’s rule

Write the electronic configuration of hydrogen atom.

• 1s²

• 1s¹

• 2s¹

Write the electronic configuration of carbon atom.

• 1s² 2s² 2p⁶

• 1s² 2s² 2p²

• 1s¹ 2s¹ 2p⁴

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NGSS.HS-PS1-1

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Write the electronic configuration of calcium atom.

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁹

• 1s²2s²2p⁶3s²3p⁶4s²

• 1s²2s²2p⁶3s²3p⁶

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NGSS.HS-PS1-1

Write the electronic configuration of neon atom.

• 1s² 2s² 2p⁶

• 1s² 2s¹ 2p⁵ 3s²

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁴

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NGSS.HS-PS1-1

Write the electronic configuration of lithium atom.

• 1s² 2s¹

• 1s² 2s² 2p³

• 1s¹ 2s²

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NGSS.HS-PS1-1

How many electrons can the d sublevel hold?

• 8
• 10
• 2
• 4

Which rule says orbitals are filled from lowest energy to highest?

• Aufbau's principle

• Hund's principle

• Pauli exclusion principle

• Law of conservation of mass