Ionization energy, electronegativity and reactivity trends

Answer Key - Grade 10 Science Worksheet

Circle the best answer, or write your answer on the line.

1. 1.

   Magnesium's first ionization energy is 7.646 eV per atom. With 1 eV per atom = 96.485 kJ/mol, what is it in kJ/mol, to 0.01, Bo?

   737.72 kJ/mol
2. 2.

   Chlorine's first ionization energy is 12.968 eV per atom. With 1 eV per atom = 96.485 kJ/mol, what is it in kJ/mol, to 0.01, Esme?

   1251.22 kJ/mol

3. Read this first

   First ionization energies down group 1 (PubChem) (PubChem)

   metal	first ionization energy (eV)
   lithium	5.392
   sodium	5.139
   potassium	4.341
   rubidium	4.177
   cesium	3.894

4. 3.

   Using the table, which metal loses its outer electron most easily, Jun?

   • Sodium
   • Lithium
   • Cesium
5. 4.

   Using the table, why do the energies fall down group 1, Kira?

   • The outer electron is farther out
   • The nucleus has fewer protons in it
   • The metals get lighter
6. 5.

   Using the table, how do the energies match group 1's reactivity, Luz?

   • They aren't linked
   • Higher energy, more reactive
   • Lower energy, more reactive
8. 6.

   Using the table, which pulls shared electrons more strongly, carbon or nitrogen, Noah?

   • They pull equally
   • Carbon
   • Nitrogen
9. 7.

   Using the table, why does electronegativity rise across period 2, Pia?

   Use the picture in question 6.

   • More protons pull the same shell
   • The atoms get bigger across the row
   • Electrons are lost
10. 8.

    Why are metals with low ionization energy very reactive, Ren?

    • They give up electrons easily
    • They hold their electrons very tightly
    • They have no electrons
11. 9.

    Why is fluorine such a reactive nonmetal, Tala?

    • It pulls electrons very strongly
    • It has a full shell
    • It is a metal
12. 10.

    Which halogen is most reactive, Zee?

    • Fluorine
    • Bromine
    • Iodine