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Name ___________________________________ Date_________________ Blk_________

Unit 4 Review - The Periodic Table

Directions: Fill in the blank or circle the correct answer.

1. Where are the most reactive metals located? ____lower left_____________

2. Where are the most reactive nonmetals located? ____upper right_(halogens)_____

3. As you go from left to right across a period, the atomic radius (decreases/increases).

4. As you travel down a group, the atomic radius (decreases/increases). Why? _number of energy__

levels increase

5. A negative ion is (larger/smaller) than its parent atom.

6. A positive ion is (larger/smaller) than its parent atom.

7. As you go from left to right across a period, the ionization energy generally (decreases/increases).

8. As you go down a group, the ionization energy generally (decreases/increases).

9. Elements in group 1 are called _____Alkali Metals_________________

10. Elements in group 2 are called ____Alkaline Earth Metals___________________

11. Elements in group 3-12 are called ___Transition metals/elements_____________

12. As you go from left to right across the periodic table, the elements go from (metals/nonmetals) to (metals/nonmetals).

13. Group 17 elements are called ____Halogens______________________

14. The most reactive element in group 17 is ____fluorine_____________

15. Group 18 elements are called ____Noble Gases___________________________

16. What sublevels are filling across the Transition Elements? __d and f_(inner transition) _

17. Elements within a group have a similar number of _____valence electrons_____

18. Elements across a period have the same number of ___valence shells/energy levels_____

19. As you go down a group, the elements generally become (more/less) metallic.

20. The majority of elements in the periodic table are (metals/nonmetals)

21. Elements in the periodic table are arranged according to their __atomic number____

22. An element with both metallic and nonmetallic properties is called a __metalloid/semimetal)__

Directions: Fill in the blank using the following word list.

actinoid series

alkali metals

alkaline earth metals

atomic mass

atomic number

family

group

halogen

lanthanoid series

metal

semimetal

noble gas

period

periodic law

periodic table

nonmetal

transition element

Dimitri Mendeleev developed a chartlike arrangement of the elements called the _____(1)______. He stated that if the elements were listed in order of increasing ______(2)______, their properties repeated in a regular manner. He called this the ______(3)______ of the elements. The arrangement used today differs from that of Mendeleev in that the elements are arranged in order of increasing _____(4)______. Each horizontal row of elements is called a(n)_____(5)______. Each vertical column is called a(n)______(6)______, or, because of the resemblance between elements in the same column, a(n) _____(7)______.

In rows 4 through 7, there is a wide central section containing elements, each of which is called a(n) _____(8)_____. Rows 6 and 7 also contain two other sets of elements that are listed below the main chart. These are called the ______(9)______ and the _____(10)_____, respectively. Each of these elements, as well as those in the first two columns at the left end of the chart, is classified as a(n)_____(11)_____. Each of the elements at the right side of the chart is classified as a(n) ______(12)______. Each of the elements between these two main types of elements, having some properties in common with each, is called a(n) ______(13)______.

Each of the elements in the column labeled 1 is called a(n) _____(14)______. Each of the elements in the column labeled 2 is called a(n) ______(15)_____. Each of the elements in column 17 is called a(n)______(16)______. Each of the elements in column 18 is called a(n)_____(17)______.

1. ___periodic table_______

2. ___atomic mass_______

3. ____periodic law_______

4. ____atomic number_____

5. ______period_________

6. _______group_________

7. ________family________

8. ____transition element___

9. ______lanthanoid______

10. _____actinoid_________

11. _______metal_________

12. ______nonmetal_______

13. _____semimetal_______

14. _____alkali metals_____

15. __alkaline earth_metals_

16. _______halogen_______

17. _____noble gas________

Characteristics of Elements

Use a periodic table of the elements to help you answer the following questions.

1 a. How many protons does an atom of bromine (Br) have? 1 a. ______35__________

b. In which group (#) is bromine found? b. ______17__________

c. What is the name of its chemical family? c. ____halogen________

d. How many valence electrons does it have? d. _______7__________

e. Is it a metal, a nonmetal, or a semimetal? e. _____nonmetal______

f. How does its atomic radius compare to chlorine’s (Cl)? f. ______larger________

g. How does its atomic radius compare to arsenic’s (As)? g. ______smaller______

h. What ion is it most likely to form in compounds? h. ______Br1-__________

2. a. How many protons does an atom of magnesium (Mg) have?2 a. ______12__________

b. In which group (#) is magnesium found? b. _______2__________

c. What is the name of its chemical family? c. __ alkaline earth metals

d. How many valence electrons does it have? d. ________2_________

e. Is it a metal, a nonmetal, or a semimetal? e. ______metal________

f. How does its atomic radius compare to calcium’s (Ca)? f. _____smaller_______

g. How does its atomic radius compare to aluminum’s (Al)? g. _____larger________

h. What ion is it most likely to form in compounds? h. ______Mg2+________

3. a. How many protons does an atom of potassium (K) have? 3 a. _______19_________

b. In which group (#) is potassium found? b. _______1__________

c. What is the name of its chemical family? c. ___alkali metals_____

d. How many valence electrons does it have? d. _______1__________

e. Is it a metal, a nonmetal, or a semimetal? e. ____metal__________

f. How does its atomic radius compare to sodium’s (Na)? f. ____larger__________

g. How does its atomic radius compare to selenium’s (Se)? g. _____larger_________

h. What ion is it most likely to form in compounds? h. _______K1+_________

Directions: Matching. On the line at the left, write the letter of the contribution that each chemist made to the periodic table. Each letter will be used only once.

__C__ 1. Dmitri Mendeleev a. arranged elements by atomic number

__A__ 2. H.G.J. Moseley b. grouped elements into sets of three

__B___ 3. J.W. Dobereiner c. predicted the existence and properties of three undiscovered elements.

__D___ 4. J.A.R. Newlands d. organized elements into repeating groups of eight, which he termed octaves.

Directions: Write the electron configuration for the following elements using Noble Gas notation.

a. S [Ne] 3s23p4 S2- [Ne] 3s23p6 or [Ar]

b. Ba [Xe]6s2 Ba2+ [Kr]5s24d105p6 or [Xe]

c. Al [Ne]3s23p1 Al3+ 1s22s22p6 or [Ne]

Identify the element, the group to which it belongs, its valence shell and the number of valence electrons.

1. [Ar] 4s2 Ca Alkali Metal vs = 4 ve = 2

2. [He] 2s2 2p3 N Nitrogen group vs = 2 ve = 5

3. [Ne] 3s2 3p5 Cl Halogen vs = 3 ve = 7

4. [Xe] 6s2 4f14 5d10 Hg transition metal vs = 6 ve = 2

5. [Ar] 4s2 3d10 4p4 Se Oxygen/Chalcogen group vs = 4 ve = 6

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