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Chapter 6 Test Periodic table

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Chapter 6 Test Periodic table Name________________________________ Part 1 Fill in the blank with the best answer: [1pt each]

1____________________ man called the “father of the periodic table” 2____________________ man who arranged elements by atomic number

3____________________ man who left gaps in his table for yet undiscovered elements 4____________________ name for element “Uup”

5____________________ Latin /Greek name for gold 6____________________ what does “periodic” mean? 7____________________ Latin / Greek name for tin

8____________________ give an example of an alkali metal 9____________________ give an example of a chalcogen 10___________________ give an example of a metalloid 11___________________ give an example of a halogen

12___________________ give an example of an alkali earth metal 13___________________ give an example of a transition element 14___________________ give an example of a lanthanoid element 15___________________ give an example of an actinoid element 16___________________ Who came up with the law of octaves?? 17___________________ where was helium first discovered?

18___________________ what was the old name for the noble gas family?

19___________________ why was the name changed? (from the old name to noble gas)

20___________________ according to Mendeleev, the properties of elements were periodic functions of what? 21___________________ according to the modern periodic law, the properties of elements are periodic

functions of what?

22___________________ what does the name “alkali” mean?

23___________________ which element is more stable, oxygen (8) or nitrogen (7) ? 24___________________ which element is more stable, manganese (25) or cobalt (27)? 25___________________ which element is more reactive potassium (19) or sodium (11)? 26___________________ what element has this outer configuration: 7s26d3 ?

27___________________ what element has this outer configuration: 5s25p4 ?

28___________________ from the chart hanging up in the room, how can you tell if an element is synthetic? 29___________________ who arranged elements by mass to find the properties repeated every 8th one? 30___________________ how many elements make up the 4th series on the periodic table?

Part 2: Give a) the noble gas notation electron configuration and b) the Lewis electron dot diagram for each: [2pts each]

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Part 2 Answer all

1. Define the Law of Octaves. 2. Define atomic radius.

What is the trend for radius going down the table? Why? What is the trend for radius going across the table? Why? 3. What are the Latin/Greek names for mercury, lead, and copper?

4. Define electronegativity. What is the trend going down the table and across. 5. State which element would be:

a) in group 8, period 5 e) a metal in the chalogen family b) in series 2, group VA f) a nonmetal in the 6th series

c) in the 4th period of the halogens g) a “d block” element with a ½ full d subshell d) ½ full of p electrons in the 3rd period h) an “f block” element with a ½ full f subshell

6. State the octet rule. What group of elements follows this rule? Which element in that group is an exception to the rule?

7. Why did John Newlands not include the noble gases in his octaves? 8. Write a name for a fictional elements # 157 and # 326.

9. True or false:

a) ________________ metals have 3 or less electrons in their outer shell b) ________________ nonmetals are usually shiny

c) ________________ elements in a series are usually similar in chemical properties d) ________________ there are many more metals than nonmetals

e) ________________ iron is a transition element f) ________________ transition elements are metals

g) ________________ francium is the most reactive alkali metal

h) ________________ tungsten is the element with the highest melting temperature i) ________________ an element with an outer configuration of 2s22p4 is a nonmetal j) ________________ an element with an outer configuration of 3s23p4 would be a halogen k) ________________ an element with an outer configuration of 4s24p4 would have 6 dots

l) ________________ an element with an outer configuration of 5s25p4 would have 2 pairs of dots m) ________________ elements in i) through l) above belong in the same family

n) ________________ elements in i) through l) above belong in the same series o) ________________ the 1st period has 2 elements in it.

p) ________________ actinoid elements add electrons to the 5f sublevel 10. Given these outer shell configurations:

A = 2s22p1 B = 5s1 C = 6s24f5 D = 3s23p5 E = 4s24p1 F = 7s2 G = 2s22p6 a) __________which 2 would be in the same family?

b) __________which 2 would be in the same series? c) __________which one(s) would be metallic? d) __________which one(s) would be nonmetallic?

e) __________which one would be the least reactive (and therefore the most stable)? f) __________which, if any, would have 7 dots in its Lewis electron dot diagram?

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Chapter 6—The Periodic Table MATCHING

Match each item with the correct statement below.

a. electronegativity f. periodic law

b. ionization energy g. cation

c. atomic radius h. period

d. metal i. group

e. transition metal j. electrons

1. horizontal row in the periodic table 2. vertical column in the periodic table

3. A repetition of properties occurs when elements are arranged in order of increasing atomic number. 4. type of element that is a good conductor of heat and electric current

5. type of element characterized by the presence of electrons in the d orbital

6. one-half the distance between the nuclei of two atoms when the atoms are joined 7. type of ion formed by Group 2A elements

8. subatomic particles that are transferred to form positive and negative ions 9. ability of an atom to attract electrons when the atom is in a compound 10. energy required to remove an electron from an atom

MULTIPLE CHOICE

1. What is another name for the representative elements?

a. Group A elements c. Group C elements

b. Group B elements d. transition elements

2. What is another name for the transition metals?

a. noble gases c. Group B elements

b. Group A elements d. Group C elements

3. Which of the following elements is in the same period as phosphorus?

a. carbon c. nitrogen

b. magnesium d. oxygen

4. Each period in the periodic table corresponds to ____. a. a principal energy level c. an orbital b. an energy sublevel d. a suborbital

5. The modern periodic table is arranged in order of increasing atomic ____.

a. mass c. number

b. charge d. radius

6. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?

a. Henry Moseley c. John Dalton

b. Antoine Lavoisier d. Dmitri Mendeleev

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a. metalloids c. metals

b. liquids d. nonmetals

8. Of the elements Pt, V, Li, and Kr, which is a nonmetal?

a. Pt c. Li

b. V d. Kr

9. To what category of elements does an element belong if it is a poor conductor of electricity?

a. transition elements c. nonmetals

b. metalloids d. Metals

10. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a. In, 49 protons, 49 electrons c. Cs, 55 protons, 132.9 electrons b. Zn, 30 protons, 60 electrons d. F, 19 protons, 19 electrons

11. The atomic number of an element is the total number of which particles in the nucleus?

a. neutrons c. electrons

b. protons d. protons and electrons

12. What element has the electron configuration 1s 2s 2p 3s 3p ?

a. nitrogen c. silicon

b. selenium d. silver

13. Which of the following is true about the electron configurations of the noble gases? a. The highest occupied s and p sublevels are completely filled.

b. The highest occupied s and p sublevels are partially filled. c. The electrons with the highest energy are in a d sublevel. d. The electrons with the highest energy are in an f sublevel.

14. Elements that are characterized by the filling of p orbitals are classified as ____. a. groups 3A through 8A c. inner transition metals

b. transition metals d. groups 1A and 2A

15. Which of the following electron configurations is most likely to result in an element that is relatively inactive?

a. a half-filled energy sublevel b. a filled energy sublevel

c. one empty and one filled energy sublevel d. a filled highest occupied principal energy level

16. Which subatomic particle plays the greatest part in determining the properties of an element?

a. proton c. neutron

b. electron d. none of the above

17. Which of the following elements is a transition metal?

a. cesium c. tellurium

b. copper d. tin

18. Which of the following groupings contains only representative elements?

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b. Ni, Fe, Zn d. Hg, Cr, Ag

19. Which of the following is true about the electron configurations of the representative elements? a. The highest occupied s and p sublevels are completely filled.

b. The highest occupied s and p sublevels are partially filled. c. The electrons with the highest energy are in a d sublevel. d. The electrons with the highest energy are in an f sublevel. 20. What are the Group 1A and Group 7A elements examples of?

a. representative elements c. noble gases

b. transition elements d. nonmetallic elements 21. Of the elements Fe, Hg, U, and Te, which is a representative element?

a. Fe c. U

b. Hg d. Te

22. How does atomic radius change from top to bottom in a group in the periodic table? a. It tends to decrease. c. It first increases, then decreases. b. It tends to increase. d. It first decreases, then increases. 23. How does atomic radius change from left to right across a period in the periodic table?

a. It tends to decrease. c. It first increases, then decreases. b. It tends to increase. d. It first decreases, then increases. 24. Atomic size generally ____.

a. increases as you move from left to right across a period b. decreases as you move from top to bottom within a group c. remains constant within a period

d. decreases as you move from left to right across a period 25. What element in the second period has the largest atomic radius?

a. carbon c. potassium

b. lithium d. Neon

SHORT ANSWER

1. Which group of elements in the periodic table is known as the alkali metals?

2. An element has an atomic number of 80. How many protons and electrons are in an atom of the element? 3. What is the noble gas notation for the electron configuration of sulfur?

4. The s and p sublevels of an atom of an element in period 3 are filled with electrons. Which orbitals are filled in this atom?

5. How many electrons are present in the d sublevel of a neutral atom of nickel? 6. How many electrons are in a rubidium ion (Rb )?

References

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