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THE PERIODIC TABLE
Honors Practice Test
A. Matching
Match each description in Column B with the correct term in Column A .Write the letter of the correct
description on the line.
Column A
Column B
1. metal
a. positively charged ion
2. halogen
b. an element whose highest occupied s or p sublevels are
partially filled
3. inner transition metal
c. the energy needed to remove an electron from an atom
in the gaseous state
4. representative element
5. ionization energy
6. alkaline earth metal
7. cation
8. electronegativity
9. transition metal
10. noble gas
d. good conductor of heat and electric current
e. an element whose highest occupied s sublevel and a
nearby d sublevel contain electrons
f. any nonmetal in Group 7A
g. the tendency of an atom to attract electrons when the
atom is in a compound
h. an element in which the highest occupied s and p
sublevels are filled
i. an element in Group 2A
j. an element whose highest occupied s sublevel and a
nearby f sublevel contain electrons
B. Multiple Choice
Choose the best answer and write its letter on the line.
_______ 11. In the modern periodic table, there is a periodic pattern in the physical and chemical
properties of elements when they are arranged in order of
a. increasing atomic mass.
b. increasing electronegativity.
c. increasing atomic radius.
d. increasing atomic number.
12. Which sublevel corresponds to the transition metals in the periodic table?
a. s
b. p
c. d
d. f
13. The category of elements that is characterized by the filling of f orbitals is the
a. inner transition metals.
c. alkali earth metals.
b. alkali metals.
d. transition metals.
14. The representative elements are
a. inner transition metals.
b. transition metals.
c. Group B elements.
d. Group A elements.
15. Which of the following elements is a metalloid?
a. As
b. Se
c. Br
d. Kr
16. The element iodine, I, is a
a. period 5 alkali metal.
b. period 4 halogen.
c. period 5 halogen.
d. period 5 transition metal.
17. The alkali metals do not include
a. Li
b. Ca.
c. Na.
d. Rb.
18. The subatomic particle that plays the greatest role in determining the physical and chemical
properties of an element is the
a. proton.
c. electron.
b. neutron.
d. photon.
19. Atomic size generally
a. increases from left to right across a period.
b. decreases from top to bottom within a group.
c. remains constant within a period.
d. decreases from left to right across a period.
20. Where are the smallest atoms located on the periodic table?
a. upper left
b. lower left
c. upper right
d. lower right
21.Which of the following atoms would you expect to have the largest atomic radius?
a. I
b. K
c. Ca
d. Rb
22. The largest atom from among the following is
a. Li.
b. Na.
c. Rb.
d. Fr.
23. The smallest atom from among the following is
a. Na.
b. Mg.
c. Si
d. Cl
24. Which of the following are always larger than the neutral atoms from which they are formed?
a. positive ions
c. cations
b. negative ions
d. none of the above
25. The smallest particle from among the following is
a. Li.
b. Li.
c. F.
d. F.
26. From left to right across the second period of the periodic table,
a. ionization energy increases.
c. electronegativity decreases.
b. atomic radii increase.
d. atomic mass decreases.
27. Of the following atoms, which one has the smallest ionization energy?
a. boron
c. nitrogen
b. aluminum
d. silicon
28. Among the following, which element has the lowest ionization energy?
a. Na
b. Cl
c. Cs
d. I
29. Electronegativity
a. generally decreases from left to right across a period.
b. is the energy change that accompanies the loss of an electron from a gaseous atom.
c. generally decreases from top to bottom within a group.
d. is generally higher for metals than for nonmetals.
30. The least electronegative element from among the following is
a. Na.
b. Cl.
c. Cs.
d. S.
31. Which of the following factors contributes to the relatively greater electronegativity of
elements on the right side of the periodic table?
a. more shells
b. less shielding
c. increased nuclear charge
d. smaller number of valence electrons
C. Questions
Answer the following in the space provided.
32. Arrange the following elements in order of decreasing ionization energy:
a. Cl, Si, P, Ar
b. Ca, Ba, Be, Sr
33. Tell whether each of the following elements is a transition metal, a noble gas, an alkali
metal, an alkaline earth metal, or a halogen.
a. calcium
b. cesium
c. fluorine
d. chromium
e. neon
f. silver
34. In each group circle the atom with…
highest
electronegativity
lowest
ionization
energy
Greatest Atomic
Radius
Na
Mg
Na
Mg
Na
Mg
Cs
Ba
Cs
Ba
Cs
Ba
35. Arrange the following elements as described below.
Li, C, K, F, Cs
a. In order of decreasing atomic size
___________________________________
b. In order of increasing ionization energy___________________________________
c. In order of decreasing electronegativity___________________________________
36. Among the following pairs of atoms, identify the larger of the two, the one with the greater first ionization
energy, and the one with the lower electronegativity.
Atom
Li, K
C, F
Mg, Ca
O, S
Larger
Radius
Greater Ionization Energy
Lower Electronegativity