a. Beryllium (Be) has a larger ionization energy.
b. Copper (Cu) has a larger ionization energy.
c. Vanadium (Va) has a larger ionization energy.
d. Tungsten (W) has a larger ionization energy.
Ionization energy can be defined as the minimum energy required to remove (detach) an electron from a neutral atom in its gaseous state.
In Chemistry, ionization energy generally tend to increase from left to right across a period on the periodic table and from bottom to top in each group of a periodic table.
Given the following pair of elements:
a. Beryllium (Be) or Barium (Ba).
The ionization energy of beryllium (Be) is 900 kJ/mol.
The ionization energy of barium (Ba) is 503 kJ/mol.
Thus, beryllium (Be) has a larger ionization energy.
b. Copper (Cu) or Radium (Ra)
- The ionization energy of copper (Cu) is 745 kJ/mol.
- The ionization energy of radium (Ra) is 509 kJ/mol.
Thus, copper (Cu) has a larger ionization energy.
c. Potassium (K) or Vanadium (Va)
- The ionization energy of potassium (K) is 419 kJ/mol.
- The ionization energy of vanadium (Va) is 651 kJ/mol.
Thus, vanadium (Va) has a larger ionization energy.
d. Tungsten (W) or Chromium (Cr)
- The ionization energy of tungsten (W) is 770 kJ/mol.
- The ionization energy of chromium (Cr) is 653 kJ/mol.
Thus, tungsten (W) has a larger ionization energy.
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