Periodic Review Name__________________________________________
1. Which element is in Group 2 and Period 7 of the Periodic Table?
(1) magnesium (2) Manganese (3) Radium (4) radon
2. Which group contains an element that is liquid at STP?
(1) 1 (2) 2 (3) 16 (4) 17
3. Which element forms an ion that is larger than its atom?
(1) Cl (2) Ca (3) Li (4) Mg
4. Which group contains elements composed of diatomic molecules at STP?
(1) 11 (2) 2 (3) 7 (4) 17
5. Which of the following elements in Period 3 has the greatest metallic character?
(1) Ar (2) Si (3) Mg (4) S
6. Nonmetals in the solid state are poor conductors of heat and tend to
(1) be brittle
(2) be malleable
(1) sulfur
(3) have a shiny luster
(4) have good electrical conductivity
7. Which element in Group 16 has no stable isotopes?
(2) selenium (3) tellurium (4) polonium
8. Which statement describes a chemical property of the element iodine?
(1) Its crystals are a metallic gray. (3) It forms a violet-colored gas.
(2) It dissolves in alcohol. (4) It reacts with hydrogen to form a gas.
9. Which three elements have the most similar chemical properties?
(1) Ar, Kr, Br (2) K, Rb, Cs (3) B, C, N (4) O, N, Si
10. An atom in the ground state contains 8 valence electrons. This atom is classified as a
(1) metal (2) semimetal (3) noble gas (4) halogen
11. The metalloids that are included in Group 15 are antimony (Sb) and
(1) N (2) P (3) As (4) Bi
12. When metals form ions, they tend to do so by
(1) losing electrons to form positive ions (3) gaining electrons to form positive ions
(2) losing electrons to form negative ions (4) gaining electrons to form negative ions
13. Which element is so active chemically that it occurs naturally only in compounds?
(1) potassium (2) silver (3) copper (4) sulfur
14. The chemical properties of the elements are periodic functions of their atomic
(1) masses (2) weights (3) numbers (4) radii
15. Which category is composed of elements that have both positive and negative oxidation states?
(1) the alkali metals (2) the transition metals (3) the halogens (4) the alkaline earths
16. Which ion has the same electron configuration as an H- ion?
(1) Cl (2) F (3) K + (4) Li +

17. How do the chemical properties of the Na atom and the Na + ion compare?
1. They are the same because each has the same atomic number.
2. They are the same because each has the same electron configuration.
3. They are different because each has a different atomic number.
4. They are different because each has a different electron configuration.
18. Group 18 elements Kr and Xe have selected oxidation states of other than zero. These oxidation states are an indication that these elements have
(1) no chemical reactivity
(2) some chemical reactivity
(3) stable nuclei
(4) unstable nuclei
19. Which kind of particle, when passed through an electric field, would be attracted to the negative electrode?
(1) an alpha particle (2) a beta particle (3) a neutron (4) an electron
20. Which radioactive emanations have a charge of 2+?
(1) alpha particles (2) beta particles (3) gamma rays (4) neutrons
21. Alpha particles are emitted during the radioactive decay of
(1) carbon-14 (2) neon-19 (3). calcium-37 (4) radon-222
22. Which type of radioactive emission has a positive charge and weak penetrating power?
(1) alpha particle (2) beta particle (3) gamma ray (4) neutron
23. Which of these types of nuclear radiation has the greatest penetrating power?
(1) alpha (2) beta (3) neutron (4) gamma
24. Given the nuclear equation: 19 Ne

X + 19 F
Which particle is represented by X?
(1) alpha (2) beta (3) neutron (4) positron
25. Which list of radioisotopes contains an alpha emitter, a beta emitter, and a positron emitter?
(1) C-14, N-16, P-32
(2) Cs-137, Fr-220, Tc-99
(1) β- (2) β+
26. What is the decay mode of K-37?
(3) Kr-85, Ne-19, Rn-222
(4) Pu-239, Th-232, U-238
(3) γ (4) α
27. What are the main advantages and disadvantages of fission and fusion?
28. What is the total mass of 222 Rn remaining in an original 160-milligram sample of 222 Rn after 19.1 days?
29. The half-life of a radioactive isotope is 20.0 minutes. What is the total amount of a 1.00-gram sample of this isotope remaining after 1.00 hour?
30. If 3.0 grams of strontium-90 in a rock sample remained in 1989, approximately how many grams of strontium-90 were present in the original rock sample in 1933?
31. Element M is a metal and its chloride has the formula MCl
2
. To which group of the Periodic Table does element M most likely belong?
32. Bombarding a nucleus with high-energy particles that change it from one element into another is called
33. Explain the trend in atomic radius across a period and down a group.