Periodic Trends: Atomic, Ionic Radii & Electronegativity

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Questions and Answers

Considering the trends in atomic radii across the periodic table, which of the following comparisons between atoms is most accurate?

Sodium (Na) has a smaller atomic radius than Magnesium (Mg).
Chlorine (Cl) has a larger atomic radius than Sulfur (S).
Potassium (K) has a smaller atomic radius than Sodium (Na).
Aluminum (Al) has a larger atomic radius than Silicon (Si). (correct)

Which of the following scenarios best illustrates the application of ionization energy principles?

Determining the rate of a nuclear decay process.
Calculating the lattice energy of an ionic crystal.
Explaining why noble gases are chemically inert. (correct)
Predicting the colour intensity of a metal compound in solution.

How does ionic radius change when a neutral atom forms an ion, and what is the underlying reason for this change?

Cations are larger because electron-electron repulsion increases, and anions are smaller because of increased effective nuclear charge.
Cations and anions are both smaller due to the increased nuclear attraction.
Cations and anions both increase in size due to polarization effects.
Cations are smaller because of increased effective nuclear charge, and anions are larger because electron-electron repulsion increases. (correct)

If element X has a higher electronegativity than element Y, what can be inferred about their behavior in forming a chemical bond?

<p>Element X will likely attract electrons more strongly, forming a polar covalent bond with a partial negative charge on X. (B)</p> Signup and view all the answers

Consider two elements, A and B. Element A has a significantly lower ionization energy and lower electronegativity compared to element B. In what type of compound are they most likely to combine and what properties would you expect the resulting compound to exhibit?

<p>An ionic compound that is brittle and has high melting point because element A will readily donate its valence electrons to element B. (C)</p> Signup and view all the answers

Flashcards

Atomic Radius

Half the distance between the nuclei of two identical atoms bonded together.

Ionization Energy

The energy required to remove an electron from a gaseous atom or ion.

Ionic Radius

The distance from the nucleus to the outer electron shell in an ion.

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons.

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Atomic Radius Trend

Generally, atomic radius decreases across a period (left to right) and increases down a group (top to bottom).

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Study Notes

Additional questions regarding periodic trends are provided for atomic radii, ionization energy, ionic radii, and electronegativity.

Atomic Radii

Explain the trends seen in atomic radii on the periodic table.
Determine if there is a general trend in atomic radii going diagonally down (or up) the periodic table.
Assess whether the representation of atomic radii as diameters, despite the given values being radii, invalidates observations.

Ionization Energy

Explain the trends observed in ionization energy on the periodic table.
Determine whether there is a general trend in ionization energy going diagonally down (or up) the periodic table.
Account for any anomalies observed in ionization energy trends.

Ionic Radii

Explain the trends seen in ionic radii on the periodic table.
Give reasons as to why values for noble gases aren't listed in relation to ionic radii.

Electronegativity

Explain the trends seen in electronegativity on the periodic table.
Give reasons as to why noble gases would not have electronegativity values listed.

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Description

Explore periodic trends with additional questions on atomic radii, ionization energy, ionic radii, and electronegativity. Understand the trends and variations across the periodic table. Investigate diagonal trends and anomalies in ionization energy.