Periodic Table Quiz 1 - Max Study



Periodic Properties Practice Quiz

NAME__________________________________ Period ___________Date____________

Matching

Match each item with the correct statement below.

|a. |electron affinity |f. |periodic law |k. electrons |

|b. |ionization energy |g. |cation |l. atomic radius |

|c. |group |h. |period |m. shielding effect |

|d. |metal |i. |non-metal |n. electronegativity |

|e. |transition metal |j. |anion | |

____ 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. type of ion formed by Group 2 elements

____ 7. subatomic particles that are transferred to form positive and negative ions

____ 8. ability of an atom to attract electrons when the atom is in a compound

Multiple Choice

Identify the letter of the choice that best completes the statement or answers the question.

____ 9. Which of the following elements is in the same period as phosphorus?

|a. |carbon |c. |nitrogen |

|b. |magnesium |d. |oxygen |

____ 10. Each period in the periodic table corresponds to ____.

|a. |a principal energy level |c. |an orbital |

|b. |an energy sublevel |d. |a suborbital |

____ 11. 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. |John Newlands |d. |Dmitri Mendeleev |

____ 12. What causes the shielding effect to remain constant across a period?

|a. |Electrons are added to the same principal energy level. |

|b. |Electrons are added to different principal energy levels. |

|c. |The charge on the nucleus is constant. |

|d. |The atomic radius increases. |

____ 13. What element in the second period has the largest atomic radius?

|a. |carbon |c. |potassium |

|b. |lithium |d. |neon |

____ 14. Why is the second ionization energy greater than the first ionization energy?

|a. |It is more difficult to remove a second electron from an atom. |

|b. |The size of atoms increases down a group. |

|c. |The size of anions decreases across a period. |

|d. |The nuclear attraction from protons in the nucleus decreases. |

____ 15. What is the element with the highest electronegativity value?

|a. |cesium |c. |calcium |

|b. |helium |d. |fluorine |

____ 16. Which of the following elements has the smallest ionic radius?

|a. |Li |c. |O |

|b. |K |d. |S |

____ 17. What is the energy required to remove an electron from an atom in the gaseous state called?

|a. |nuclear energy |c. |shielding energy |

|b. |ionization energy |d. |electronegative energy |

____ 18. Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?

|a. |increase in atomic size |

|b. |increase in size of the nucleus |

|c. |increase in number of protons |

|d. |fewer electrons in the highest occupied energy level |

____ 19. Which statement is true about electronegativity?

|a. |Electronegativity is the ability of an anion to attract another anion. |

|b. |Electronegativity generally increases as you move from top to bottom within a group. |

|c. |Electronegativity generally is higher for metals than for nonmetals. |

|d. |Electronegativity generally increases from left to right across a period. |

____ 20. Which of the following statements correctly compares the relative size of an ion to its neutral atom?

|a. |The radius of an anion is greater than the radius of its neutral atom. |

|b. |The radius of an anion is identical to the radius of its neutral atom. |

|c. |The radius of a cation is greater than the radius of its neutral atom. |

|d. |The radius of a cation is identical to the radius of its neutral atom. |

Periodic Table Quiz 1

Answer Section

MATCHING

1. ANS: H DIF: L1 REF: p. 157 OBJ: 6.1.1

2. ANS: I DIF: L1 REF: p. 157 OBJ: 6.1.1

3. ANS: F DIF: L1 REF: p. 157 OBJ: 6.1.1

4. ANS: D DIF: L1 REF: p. 158 OBJ: 6.1.3

5. ANS: E DIF: L1 REF: p. 166 OBJ: 6.2.2

6. ANS: G DIF: L1 REF: p. 172 OBJ: 6.3.2

7. ANS: J DIF: L1 REF: p. 172 OBJ: 6.3.2

8. ANS: A DIF: L1 REF: p. 177 OBJ: 6.3.3

MULTIPLE CHOICE

9. ANS: B DIF: L1 REF: p. 162, p. 163

OBJ: 6.1.1

10. ANS: A DIF: L2 REF: p. 157 OBJ: 6.1.1

11. ANS: D DIF: L1 REF: p. 156 OBJ: 6.1.2

12. ANS: A DIF: L2 REF: p. 171 OBJ: 6.3.1

13. ANS: B DIF: L2 REF: p. 171 OBJ: 6.3.1

14. ANS: A DIF: L2 REF: p. 173 OBJ: 6.3.2

15. ANS: D DIF: L1 REF: p. 177 OBJ: 6.3.3

16. ANS: A DIF: L2 REF: p. 175 OBJ: 6.3.3

17. ANS: B DIF: L2 REF: p. 173 OBJ: 6.3.3

18. ANS: A DIF: L2 REF: p. 174 OBJ: 6.3.1, 6.3.3

19. ANS: D DIF: L2 REF: p. 177 OBJ: 6.3.3

20. ANS: A DIF: L2 REF: p. 172, p. 176

OBJ: 6.3.3

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