Lesson 2 chapter 2

The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?

• The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
• The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
• The ionization energy increases gradually as you move right across a period because you are adding more protons.
• The ionization energy increases when the valence electrons are more attracted to the nucleus.

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The bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?

• They are in the same period with W being furthest left.
• They are in the same period with W being furthest right.
• They are in the same group with W being furthest to the bottom.
• They are in a diagonal line with W being at the bottom right.

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Which of the following is true for alkaline earth metals as their atomic number increases?

• The atomic radius decreases.
• Ionization energy decreases.
• The number of valence electrons increases.
• The Coulombic attraction increases.

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Which of the following is true about a sulfur atom and a chlorine atom?

• Sulfur is larger and has higher ionization energy.
• Sulfur is larger and has lower ionization energy.
• Sulfur is smaller and has higher ionization energy.
• Sulfur is smaller and has lower ionization energy.

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 After the atom is ionised, it then requires more energy to remove a second electron because the second electronis nearer the nucleus.

• False
• True
• Not sure

 After the atom is ionised, it then requires more energy to remove a second electron because the second electronis nearer the nucleus.

• False
• True
• Not sure

The atom will spontaneously lose an electron to become stable.

• True
• False
• Not sure

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The nucleus is not attracted to the electrons.

• True
• False
• Not sure

Only one electron can be removed from the atom, as it then has a stable electronic configuration.

• True
• False
• Not sure

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After the atom is ionised, it then requires more energy to remove a second electron because it experiences agreater core charge than the first.

• True
• False
• Not sure