Unit 2: Periodic Trends

What is the definition of an ion?

• A charged particle formed when protons are gained or lost

• A neutral atom with extra neutrons

• An atom with a net electric charge due to loss or gain of electrons

• An atom with more than 8 valence electrons

Which of the following ions is isoelectronic with Argon (Ar)?

• Mg²⁺

• Be²⁺

• O²⁻

• Cl⁻

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NGSS.HS-PS1-1

Which element has the greatest ionization energy?

• Sodium (Na)

• Phosphorus (P)

• Oxygen (O)

• Fluorine (F)

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What causes ionization energy to increase across a period?

• Decreasing atomic radius

• Increasing shielding effect

• Increasing effective nuclear charge

• Decreasing proton number

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What happens to the ionization energy as you move down a group?

• It increases due to stronger nuclear charge

• It decreases due to increased shielding effect

• It stays the same due to electron balance

Which subshell do the electrons get removed from when Zinc (Zn) becomes a cation?

• 3s

• 3p

• 4s

• 3d

What charge will an atom in Group 16 typically form when ionizing?

• 2+

• 2−

• 6−

• 0

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Which of the following elements has the same number of valence electrons as sulfur (S)?

• Neon (Ne)

• Phosphorus (P)

• Iodine (I)

• Selenium (Se)

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What is the trend in atomic radius across a period from left to right?

• It increases

• It decreases

• It stays the same

• It increases then decreases

What causes shielding to remain constant across a period?

• Atomic radius increases

• Proton number stays the same

• Electrons are added to different energy levels

• Core electrons remain the same