Chapter 4: Periodicity
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How are elements arranged in the Periodic Table?
By increasing atomic number.
What do the vertical columns in the Periodic Table represent?
Groups.
What do the rows in the Periodic Table represent?
Periods.
What trend is observed in atomic radii across a period?
Atomic radii decrease.
Why do atomic radii decrease across a period?
Increased nuclear charge pulls electrons closer.
What trend is observed in atomic radii down a group?
Atomic radii increase.
Why do atomic radii increase down a group?
More electron shells increase shielding.
How does the size of positive ions compare to their parent atoms?
Positive ions are smaller.
How does the size of negative ions compare to their parent atoms?
Negative ions are larger.
What is the trend in ionic radii for positive ions from Groups 1 to 14?
Ionic radii decrease.
What is the trend in ionic radii for negative ions from Groups 14 to 17?
Ionic radii decrease.
Why do ionic radii decrease across a period?
Increased nuclear charge.
What is the trend in ionic radii down a group?
Ionic radii increase.
What is the general trend of ionization energy across a period?
Ionization energy increases.
Why does ionization energy increase across a period?
Greater nuclear attraction makes electrons harder to remove.
What is the general trend of ionization energy down a group?
Ionization energy decreases.
Why does ionization energy decrease down a group?
Increased distance reduces nuclear attraction.
What is electronegativity?
An atom’s ability to attract electrons in a covalent bond.
What is the trend in electronegativity across a period?
Electronegativity increases.
What is the trend in electronegativity down a group?
Electronegativity decreases.
Which element has the highest electronegativity?
Fluorine (4.0).
Which element has the lowest electronegativity?
Caesium (0.7).
What happens to melting points down Group 1?
Melting points decrease.
Why do melting points decrease down Group 1?
Decreased attraction between delocalized electrons and ions.