August 2010 Chemistry Regents #54-56

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Questions

Base your answers to questions 54 through 56 on the elements in Group 2 on the Periodic Table.

54 State the general trend in first ionization energy for the elements in Group 2 as these elements are considered in order from top to bottom in the group. [1]

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Use Table S and the Periodic table

As atomic number increases, first ionization energy decreases.

First ionization energy decreases.

55 State, in terms of the number of electron shells, why the radius of a strontium atom in the ground state is larger than the radius of a magnesium atom in the ground state. [1]

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Use the Periodic Table and analyze the electron configuration on the bottom (Sr = 2-8-18-8-2  and Mg =2-8-2)

A strontium atom in the ground state has two more electron shells than a magnesium atom in the ground state.

An Mg atom has fewer electron shells.

56 Explain, in terms of atomic structure, why the elements in Group 2 have similar chemical properties. [1]

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"in terms of atomic structure" so same group is now a wrong answer

In the ground state, an atom of each element has two valence electrons.

The number of electrons in the outermost shell of each atom is the same.

 

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Questions 1-10 Questions 11-20 Questions 21-30 Questions 31-40 Questions 41-50

Questions 51-53 Questions 54-56 Questions 57-58 Questions 59-60 Questions 61-63 Questions 64-66 Questions 67-69 Questions 70-72 Questions 73-74 Questions 75-78 Questions 79-81

 

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