AP®︎ Chemistry: Topic 1.7 Flashcards

Master key terms and definitions for Topic 1.7 of AP Chemistry – Periodic Trends to help you prep for quizzes and the AP exam.

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Term

Periodicity

Definition

Recurring patterns in element properties caused by repeating valence electron configurations.

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Periodicity
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Recurring patterns in element properties caused by repeating valence electron configurations.

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Periods and Groups
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Periods are rows with the same occupied shells; groups are columns with similar valence electrons.

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Valence Electrons and Group Properties
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Elements in the same group have similar outer electrons and therefore similar chemical behavior.

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Shell Model
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Electrons occupy energy levels around the nucleus, with outer levels farther away and more shielded.

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Shielding
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Inner electrons reduce the nucleus's attraction for outer electrons through electron-electron repulsion.

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Effective Nuclear Charge
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Net positive attraction felt by an electron after accounting for shielding by other electrons.

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Coulomb's Law in Periodic Trends
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Electrostatic attraction increases with greater charge and decreases as distance between charges increases.

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Atomic Radius Trend
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Decreases across a period and increases down a group because of charge and shell effects.

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Ionic Radius
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Cations are smaller than their atoms; anions are larger than their atoms.

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Successive Ionization Energies
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Each removal requires more energy, with a large jump after all valence electrons are removed.

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Using Ionization Energies to Find Valence Electrons
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Identify the large jump in values; electrons removed before it are the valence electrons.

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Periodic Trend Predictions
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Use an element's position, shells, shielding, and effective nuclear charge to estimate atomic properties.

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Ionization Energy
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Energy required to remove an electron, generally increasing across periods and decreasing down groups.

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Electronegativity
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Ability to attract shared electrons in a bond, generally increasing across periods and decreasing down groups.

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Electron Affinity
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Energy change when a gaseous atom gains an electron, generally more negative across periods and down groups less negative.

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