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The Periodic Law

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The Periodic LawHRW material copyrighted under notice appearing earlier in this work.

DIRECTIONS: Write on the line at the right of each statement the letter preceding the word or expression that best

completes the statement.

1. Mendeleev did not always list elements in his periodic table in order of increasing atomicmass, so that he could group together elements with similar (a) properties; (b) atomic numbers;(c) densities; (d) colors.

2. The principle that states that the physical and chemical properties of the elements are periodicfunctions of their atomic numbers is known as (a) the periodic table; (b) the periodic law;

(c) the law of properties; (d) Mendeleev's law.

3. The elements with atomic numbers from 58 to 71 in the Periodic Table are referred to as

(a) lanthanide elements; (b) noble gases; (c) actinide elements; (d) alkali metals.

4. The discovery of the noble gases changed Mendeleev's periodic table by adding a new(a) period; (b) series; (c) group; (d) sublevel block.

5. Barium, atomic number 56, is the fifth element in Group 2. What is the atomic number ofradium, the next element in Group 2? (a) 64 (b) 74 (c) 88 (d) 103

6. Since the first energy level contains only a Is sublevel, the number of elements in this periodis (a) 1; (b) 2; (c) 4; (d) 8.

7. In Period 3 there are 8 elements. What sublevel(s) is(are) being filled? (a) s (b) s and d(c) sand p (d) d and f

8. An element has an electron-configuration notation of [Ar] 3d I04s24p 5. The element is in the__ period. (a) second (b) third (c) fourth (d) fifth

9. Within the p-block element group, the elements at the top of the table, compared with thoseat the bottom, (a) have larger radii; (b) are more metallic; (c) have lower ionization energies;(d) are more nonmetallic.

10. Nitrogen's electron configuration is Is22s22p3. To what group does nitrogen belong? (a) 2 (b) 7(c) 15 (d) 17

11. The elements located on the periodic chart in Group 1 are also known as the (a) alkali metals;(b) rare earth series; (c) Period 1 elements; (d) actinide series.

12. The most characteristic property of the noble gases is that they are (a) metallic;(b) all radioactive; (c) metalloids; (d) largely unreactive.

13. Atomic size is determined by measuring the (a) radius of an individual atom; (b) distancebetween nuclei of adjacent atoms; (c) diameter of an individual atom; (d) volume of theelectron cloud of adjacent atoms.

14. In equation form, the acquisition of an electron, resulting in an exothermic change is(a) A + e - + energy -> A -; (b) A + e - -> A - - energy; (c) A + e - -> A - + energy;(d) A - + energy -> A + e - .

15. Within a group of elements, as the atomic number increases, the atomic radius (a) increases;(b) remains generally constant; (c) decreases regularly; (d) decreases, but not regularly.

16. For each successive electron removed from an atom, the ionization energy (a) increases;

(b) decreases; (c) remains the same; (d) shows no pattern.

17. In the formation of chemical compounds, valence electrons are those that may be (a) lost only;(b) gained only; (c) shared only; (d) lost, gained, or shared.

18. The number of valence electrons in Group 2 elements is (a) 2; (b) 8; (c) 18; (d) equal to the

period number.

19. The electron configuration of a potassium ion (atomic number 19) matches that of an atom of(a) He (Z =2); (b) Ne (Z = 10); (c) Ar (Z = 18); (d) Kr (Z = 36).

20. Iron (Fe) has the electron configuration [Ar] 3d64s2• What is the electron configuration ofFe2+? (a) [Ar] 3d5 (b) [Ar] 3d54s2 (c) [Ar] 3d6 (d) [Ar] 3d64s24p I

DIRECTIONS: Complete the following statements, forming accurate sentences.

21. Elements whose atoms contain partially filled d sublevels are called . 21

22. The elements of the sand p- blocks are referred to as . 22

23. An atom or group of atoms that has a positive or negative charge is called a(n) _

---- .23

24. The energy change that occurs when an electron is acquired by a neutral atom is called _

______________________________ .24

25. The power of an atom to attract electrons in a chemical compound is called . 25

DIRECTIONS: In the parentheses at the right of each expression in the first column, write the letter of theexpression in the second column that is most closely related.

26. contain a pair of electrons in the outermost s sublevel and no p electronsin the outermost level

27. very reactive elements that make up Group 17 and are found in salts

28. the least reactive of all elements

29. Group 1 elements never found free in nature

30. represent filling of 4f sublevel, sometimes called rare earths

a. alkali metals

b. halogens

c. alkaline-earthmetals

d. lanthanides

e. noble gases

DIRECTIONS: Write on the line to the right the period and block to which each of the following elements belongs.Base your answer on the electron configuration of each element.

31. Phosphorus: ls22s22p63~3p3 31

32. Calcium: 1~2~2p63~3p64~ 32

33. Zirconium: 1~2s22p63~3p63dl°4~4p64d25~ 33

34. Krypton: lS22s22p63s23p63dlo4~4p6 34

35. Neodymium: ls22~2p63s23p63dI04s24p64dl°4r5~5p66~ 35

DIRECTIONS: Write on the line to the right the group number to which each of the following elements belongs,and identify the element as an active metal, transition metal, nonmetal, or noble gas. Base your answer on theelectron configuration of each element.

36. Magnesium: ls22s22p63s2 36

37. Argon: 1~2~2p63~3p6 37

38. Vanadium: 1~2s22p63~3p63d34~ 38

39. Bromine: 1~2~2p63~3p63dlo4~4p5 39

40. Rubidium: 1~2s22p63s23p63dl04~4p65s1 40

22 Chapter 5 The Periodic LawHRW material copyrighted under notice appearing earlier in this work.