Multiple Choice
Which of the following trends can be identified on the periodic table?
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10. Periodic Properties of the Elements
Periodic Trend: Cumulative
Multiple Choice
Which of the following statements is true?
A
Valence electrons are more difficult to remove than inner core electrons.
B
Argon and bromide are isoelectronic species.
C
Francium possesses the greatest electronegativity.
D
The second ionization energy of an atom is always larger than its first ionization energy.
E
The aluminum atom will experience a larger jump in its third ionization energy than its fourth.
Verified step by step guidance1
Understand the concept of ionization energy: Ionization energy is the energy required to remove an electron from an atom in the gaseous state. The first ionization energy refers to the energy needed to remove the first electron, while the second ionization energy is for removing the second electron, and so on.
Consider the statement about valence and core electrons: Valence electrons are the outermost electrons and are generally easier to remove than core electrons, which are closer to the nucleus and more tightly bound.
Examine the isoelectronic species statement: Isoelectronic species have the same number of electrons. Argon (Ar) has 18 electrons, and bromide (Br⁻) also has 18 electrons after gaining one electron, making them isoelectronic.
Evaluate the statement about electronegativity: Electronegativity is the tendency of an atom to attract electrons in a chemical bond. Francium is at the bottom of the alkali metals and has the lowest electronegativity, not the greatest.
Analyze the ionization energy statements: The second ionization energy is always larger than the first because it is harder to remove an electron from a positively charged ion. For aluminum, the third ionization energy involves removing an electron from a stable noble gas configuration, resulting in a larger jump compared to the fourth ionization energy.
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