Periodic Trends Practice Quiz
Name___________
____1. The energy required to remove an electron from an atom is called ionization energy
____2. From which of the following is it easiest to remove an electron? F Cl O I Ne N
Iodine because it is lower on the periodic table. Second easiest would be Nitrogen.
____3. The tendency for an atom to attract electrons to itself and form compounds is called electronegativity
____4. Draw an arrow that starts at the element with lowest
……………..electronegativity and ends with the highest. Fr lowest F highest
____5. Which of the following is most likely to gain electrons in a chemical
reaction? Mg Si O F P Why? Fluorine because it is the most electronegative.
____6. Which of the following elements is most metallic? Ca F Al Si Pb
Calcium because it is closest to the left. (Francium is the most metallic element. )
____7. Which of the following in each pair has a smaller radius? (Circle the smallest in each pair.)
O or O-2 (Oxygen with a minus 2 charge has gained two electrons, so it is larger than oxygen.)
Na or Na+ (Sodium with a + 1 charge has lost an electron, so it is smaller than sodium.)
Cl or Cl(Chlorine with a -1 charge has gained one electron, so it is larger than chlorine.)
Cl or I (iodine has 5 energy levels while chlorine only has 3, so chlorine is smaller)
Na or Cl (atomic radius goes down across rows because the nuclear charge is greater, so chlorine is smaller.)
____8. High ionization energy is characteristic of: metals non-metals metalloids Why? Non metals have high
electronegativity and more valence electrons.
____9. Which of the following has the most electrons? Ne
electrons except for Na which has 11.
O-2 F-
Na+
Na Al
+3
All of these have 10
____10. Which of the following is least likely to lose an electron? Kr Br Ca K Fr Why? Krypton is a Noble Gas
and they don’t lose electrons because they have a full outer level. (8 valence electrons—an octet)
____11. Rank the following elements from low to high electronegativity: N, Al, O, K. K Al N O
____12. Rank the following from least number of valence electrons to most. O, N, C, Li, Ne Li-1 C-4 N-5 Ne-8
____13. Which of the atoms has the highest Ionization energy? Na S Fr O F H Fluorine
____14. Which of the atoms is the largest? O, S , Se, Te , I
Telurium has more energy levels, so it is the
largest. Iodine is smaller because atomic radius goes down across a period.
____15. Which of the following is highest in electronegativity. Ne, Ni, Na, Nb, N Nitrogen is closest to the
right and top. Ne doesn’t have an EN value because it is a Noble gas and already has 8 valence electrons.
16. Why do the Noble gases lack electronegativity values? They already have an octet and don’t need any more
electrons.
17. Write the Noble gas configuration for Ba (56). [Xe]6s2
18. Which electron configuration rule states that electrons occupy lower energy levels first before filling higher
energy levels? Aufbau
19. Which electron configuration rule states that you put 1 electron in each orbital before adding the second?
Hunds Rule
20. Label the spdf blocks on a periodic table. Be able to identify which element ends at a specific spot based on
the last electron filled. [example 3p5, 4d5, 5s2]
3p5
5s2
4d5
21. Write the Noble gas configuration for the phosphide ion. Phosphorus has 15 electrons because its atomic
number is 15. The phosphide ion has a charge of -3 because phosphorus needs to gain 3 electrons to obtain
an octet. So, it will have 18 electrons and have the same configuration of Argon. [Ar]
22. Draw a Bohr model for the element with this configuration. [Kr] 5s2 4d2
1s2 2s2p6 3s2p6d10 4s2p6d2 5s2
2
8
18
10
2