Periodic Table Test Review Packet

Periodic Table Test Review Packet D 1. Elements in the same chemical family have the same a. atomic numbers b. atomic masses c. electron configurations d. numbers of valence electrons

A 2. Which of the following metals is the most reactive? a. Cesium b. Barium c. Magnesium d. Calcium

B 3. Ionization energy is the energy required to do which of the following? a. add an electron to an atom b. remove an electron from an atom c. remove a proton from an atom d. remove a neutron from an atom

C 4. Neon, a noble gas, has a stable electron arrangement. Which of the following has the same electron arrangement as neon?

a. Cl- b. Mg+ c. O2– d. N2– e. Ga3+

B 5. The trend in atomic radii as you move from left to right across a period can be explained by a. decreasing nuclear charge and increasing energy levels b. increasing nuclear charge with no change in electron shells c. increasing number of electrons d. the p orbitals having different shape than s orbitals

D 6. The trend in atomic radii down a family or group can be explained by a. increasing number of protons b. decrease in energy level of electrons c. the p orbitals having different shape than s orbitals d. increasing number of electrons at higher energy levels

D 7.The next noble gas (as yet undiscovered) on the periodic table should have atomic number 118. On the basis of your knowledge of the noble gases, which of the following characteristics would not be expected for this element? a. Element 118 will be a gas at room temperature. b. Element 118 will probably have 8 valence electrons. c. Element 118 will have the lowest ionization energy in its family. d. Element 118 will have smallest atomic radius in the group.

C 8. Compared to neutral atoms of an element, cations (positive ions) are a. larger because they have gained protons b. larger because they have gained electrons c. smaller because they have lost electrons d. either larger or smaller depending on the family or group I VIII

II III IV V VI VII

A B A B D E C

In the diagram above, which arrow correctly indicates each of the following trends?

C 9. increasing atomic radius in a period

A 10. increasing reactivity for the alkali metals

B 11. increasing ionization energy within a group

A 12. increasing atomic size within a group

Which letter on the diagram above indicates each of the following?

E 13. noble gases

C 14. transition metals

D 15. halogens

A 16. alkali metals

Which of the following would you predict to be smaller(est)?

A 17. a. Pb4+ b. Pb2+ c. Pb

B 18. a. Cl– b. Cl

A 19. a. Kr b. K c. Br d. Ca 20. Many people are trying to eliminate NaCl from their diet. What element is the most likely substitute for sodium in table salt?

Potassium (K) 2- 21. Predict the charge on the most common ion for sulfur.

Larger Would this ion be larger or smaller than the neutral atom?

22. An old prospector was panning for gold in the Superstitions. One day, instead of gold, he discovered little pieces of metal in the bottom of his pan. When he took some of these "nuggets" to the assay office, he was congratulated for discovering a deposit of sodium metal. What's unlikely about this story?

Pure sodium is too unstable to exist in nature and pure sodium reacts violently with water.

Consider the graph at right.

23. What group of elements do the highest peaks represent?

Noble Gases Group 18

24. Why is the ionization energy for elements 3, 11, and 19 so low? These elements only have one valence electron and group one metals spontaneously lose an electron.

25. a. Does carbon or fluorine have a larger atomic radius? Why?

Carbon has a larger radius because it has the same electron shielding as fluorine but fewer protons. Carbon’s smaller nucleus is not as good at attracting electrons. b. Does sodium or cesium have a larger ionization energy? Why?

Sodium because it has less shielding and can hold onto its outer electron with a stronger pull. c. Does phosphorus or chlorine have larger electronegativity? Why?

Chlorine because it has the same amount of shielding as phosphorus but more protons, which means chlorine has a greater ability to attract electrons.