Chemistry 1
Test on Periodic table: Form B
1. A particular element is a poor conductor of electricity. Which class of elements could this
element belong to?
A transition metals
B alkali metals
C alkali earth metals
D halogens
2. Lithium, sodium, and potassium are all:
a. alkaline earth metals
b. alkali metals
c. semimetals
d. transition metals
3. An example of an alkaline earth metal is:
a. hydrogen
b. silicon
c. cobalt
d. magnesium
e. tin
4.
In which one of these parts of the periodic table are transition metals located?
a.
in groups 1 &2 at the left side of the table
b.
in group 18 at the right side of the table
c.
d.
in groups 3-12 across the middle of the table
in the lanthanide and actinide series
5. Which chemical group is called the halogens?
a. group 1
b. group 2
c. groups 3-12
d. group 17
e. group 18
6. In general, as you move across a period (from left to right), ionization energies
a. decrease
b. increase
c. stay the same
7. Which would have the higher ionization energy, boron or oxygen?
a. boron
b. oxygen
c. they would be the same
d. neither ionizes
8. The reason that the ionization energies of elements decrease as you move down a column on
the periodic table is that as you go down the column:
a.
the number of protons increases
b.
the electrons are farther away from the nucleus
c.
there are more neutrons
d.
each element is more stable
9. Which would be the most electronegative?
a. bromine
b. copper
c. calcium
d. potassium
10. As you move across a period, from left to right, the size of the atoms of each element
a. decreases
b. increases
c. stays the same
11. An atom of boron would be:
12.
a.
larger than an atom of beryllium
b.
smaller than an atom of lithium
c.
d.
smaller than an atom of nitrogen
smaller than an atom of neon
Which would be larger than a sodium ion?
a.
b.
a helium atom
a sodium atom
13. Which of the following atoms is the largest?
a. Al
b. Mg
c. Ca
d. Sr
e. Rb
c.
d.
a lithium ion
none of the above
14. For each of the following pairs, which element will have the greater metallic character: Li, Be
and Li, Na?
a. Li, Li
b. Li, Na
c. Be, Li
d. Be, Na
15. Group 8 noble gases are inert because
a. they readily form positive ions.
b. they can have either a positive or a negative charge.
c. their outermost energy level is missing one electron.
d. their outermost energy level is full.
16. Carbon and other non-metals are found in which area of the periodic table?
a. On the left-most side.
b. On the right side.
c. In the middle column of the periodic table.
d. In the bottom rows.
17. Which of the following sets of elements is in the correct order of increasing atomic radius
(smallest to largest)?
a. P, Si, Al
b. Cl, Br, I
c. S, As, Sn
d. Se, As, Sb
e. Cl, S, O
18. Silicon is lustrous and is a conductor of heat and electricity, but is not malleable or ductile.
For this reason, silicon is known to be a…
A metal
B non-metal
C metalloid
D
all of the above
19 . Which of the following is true regarding Chlorine and Tellurium?
a) Chlorine has a higher electronegativity and a larger atomic radius
b) Chlorine has a higher electronegativity and a smaller atomic radius
c) Chlorine has a lower electronegativity and a larger atomic radius
d) Chlorine has a lower electronegativity and a smaller atomic radius
20. Given the representation of a chlorine atom, which circle might represent an atom of
bromine?
a
Circle D
b Circle C
c
Circle B
d None of these
21. What is another name for the representative elements?
a. Group A elements
c. Group C elements
b. Group B elements
d. transition elements
22. What is another name for the transition metals?
a. noble gases
c. Group B elements
b. Group A elements
d. Group C elements
23. Which of the following elements is in the same period as phosphorus?
a. carbon
b. magnesium
c. nitrogen
d. oxygen
24. 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
25. 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
26.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
27. Which of the following factors contributes to the increase in atomic size within a group in the
periodic table as the atomic number increases?
a. more shielding of the electrons by the highest occupied energy level
b. an increase in size of the nucleus
c. an increase in number of protons
d. fewer electrons in the highest occupied energy level
28. 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.
29. To which group do sodium and cesium belong?
a. the noble gases
b. the alkali metals
c. the halogens
d. the actinides
30. The metalloids are located where on the periodic table
a. Along the zigzag stair step line in the periodic table
b. Group 1
c. Group 18
d. In the d block
31. Electronegativity is
a. The energy required to remove and electrons from an atom
b. The measure of the ability of an atom in a chemical compound to attract electrons
c. The energy change when an electron is acquired by a neutral atom
d. The distance between radii of adjacent atoms
32. Atomic Radius is
a. The energy required to remove and electrons from an atom
b. The measure of the ability of an atom in a chemical compound to attract electrons
c. The energy change when an electron is acquired by a neutral atom
d. The distance between radii of adjacent atoms
33. Ionization Energy is
a. The energy required to remove an electron from an atom
b. The measure of the ability of an atom in a chemical compound to attract electrons
c. The energy change when an electron is acquired by a neutral atom
d. The distance between radii of adjacent atoms
34. Which element has the highest electronegativity?
a. Fluorine
b. iodine
c. lithium
d. rubidium
35. Which element has the largest atomic radius?
a. Lithium
b. Cesium
c. Radon
d. Neon
36. Which element has the lowest 1st ionization energy?
a. Lithium
b. Cesium
c. Radon
d. Neon
37. Which of the following elements is in the same family as sulfur?
a. carbon
c. nitrogen
b. chlorine
d. Tellurium
38. What element has the electron configuration 1s22s22p63s2 3p5?
a. nitrogen
c. silicon
b. chlorine
d. Silver
39. Which of the following is true about the electron configurations of the lanthanides and
actinides?
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.
40. What is another name for Group IIA?
a .alkali metals
b. alkaline earth metals
c. noble gases
d. Halogens
41. 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.
42 . Which of the following statements is true about ions?
a. Cations form when an atom gains electrons.
b. Cations form when an atom loses protons.
c. Anions form when an atom gains electrons.
d. Anions form when an atom loses protons.
43. The metals in Groups 1, 2, and 3 ____.
a. gain electrons when they form ions
b. all form ions with a negative charge
c. all have ions with a 1 charge
d. lose electrons when they form + ions
44. The halogens tend to form anions because….
a. They have low first ionization energies
b. They have low electron affinities
c. They have high electron affinities
d. They don’t; they form cations
45. Which element is the most malleable?
a) gold
b) sulfur
c) hydrogen
d) radon
46. Which is the most reactive non-metal on the Periodic Table of the Elements?
a) Fr
b) F
c) I
d) Cl
47. The number of valence electrons in an atom with the electron configuration 1s2 2s2 2p6 3s2 3p4
is:
a) 6
b) 2
c) 16
d) 4
48. The element in Period 3 that has the highest ionization energy is:
a) a Noble gas
b) a halogen
c) an Alkali metal
d) an Alkaline Earth metal
49. Name the only element touching the stair-step line that is NOT a metalloid
a. Aluminum
c. Nitrogen
b. Boron
d. Astatine
50. Element B is an:
A. halogen
B. transition metal
C. alkaline earth metal
D. alkali metal
51. According to the modern periodic law, the chemical properties of the elements are periodic
functions of their:
A. isotopic weight
B. atomic number
C. atomic weight
D. atomic mass
52. 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.
53. The vertical columns in the periodic table are known as:
A periods, and they contain elements with the same number of
outer-shell electrons
B periods, and they contain elements with the same number of occupied
electron shells
C groups, and they contain elements with the same number of
outer-shell electrons
D groups, and they contain elements with the same number of occupied
electron shells
54. Moving down Group 1 in the Periodic Table,
A
B
C
D
the number of occupied electron shells increases
the number of occupied electron shells increases at first then decreases
the number of occupied electron shells decreases
the number of occupied electron shells decreases at first then increases
55. An atom of potassium has 19 electrons. Its electron shell configuration would best be written
as:
A
B
C
D
19
2, 17
2, 8, 9
2, 8, 8, 1
56. Which of the following is a property of an element?
A
B
C
D
number of shells
the color, “white”
number of electrons
density