Download Practice Periodic Table Review Name

Practice Periodic Table Review
Name_________________
1. An electron will emit energy in quanta when its
energy state changes from 4p to
A) 5s
B) 5p
C) 3s
D) 6p
2. Which electron configuration represents an atom
in the excited state?
A) 1s 22s 22p 63s 2
C) 1s 22s 22p 6
B) 1s 22s 22p 63s 1
D) 1s 22s 22p 53s 2
3. In the electron-dot symbol, the dots represent
electrons located in
A)
B)
C)
D)
4. What is the highest principal quantum number
assigned to an electron in an atom of zinc in the
ground state?
B) 2
C) 5
D) 4
5. Which orbital notation represents a noble gas in
the ground state?
A)
B)
B) metalloids
D) noble gases
9. Which element has chemical properties that are
most similar to the chemical properties of sodium?
A) beryllium
C) lithium
B) calcium
D) magnesium
10. Which statement explains why sulfur is classified
as a Group 16 element?
A sulfur atom has 6 valence electrons.
A sulfur atom has 16 neutrons.
Sulfur is a yellow solid at STP.
Sulfur reacts with most metals.
11. As the elements in Group 15 are considered in
order of increasing atomic number, which
sequence in properties occurs?
A)
B)
C)
D)
nonmetal ® metalloid ® metal
metalloid ® metal ® nonmetal
metal ® metalloid ® nonmetal
metal ® nonmetal ® metalloid
12. At STP, which element is a good conductor of
electricity?
A) chlorine
C) silver
C)
B) iodine
D) sulfur
13. Which element is a liquid at 305 K and 1.0
atmosphere?
D)
6. Which orbital notation represents a boron atom in
the ground state?
A) magnesium
C) gallium
B) fluorine
D) iodine
14. At STP, which element is solid, brittle, and a
poor conductor of electricity?
A)
B)
A) Al
B) K
C) Ne
D) S
15. What are two properties of most nonmetals?
C)
D)
7. The elements on the Periodic Table are arranged in
order of increasing
A) atomic mass
C) molar mass
A) metals
C) nonmetals
A)
B)
C)
D)
s sublevels, only
p sublevels, only
s and p sublevels, only
s, p, and d sublevels
A) 1
8. The elements in Group 2 are classified as
B) atomic number
D) oxidation number
A) high ionization energy and poor electrical
conductivity
B) high ionization energy and good electrical
conductivity
C) low ionization energy and poor electrical
conductivity
D) low ionization energy and good electrical
conductivity
16. An atom of argon in the ground state tends not to
bond with an atom of a different element because
the argon atom has
A)
B)
C)
D)
more protons than neutrons
more neutrons than protons
a total of two valence electrons
a total of eight valence electrons
17. Arsenic and silicon are similar in that they both
A)
B)
C)
D)
have the same ionization energy
have the same covalent radius
are transition metals
are metalloids
18. At STP, which list of elements contains a solid, a
liquid, and a gas?
A) Hf, Hg, He
C) Ba, Br2, B
B) Cr, Cl 2, C
D) Se, Sn, Sr
19. The carbon atoms in graphite and the carbon
atoms in diamond have different
A)
B)
C)
D)
atomic numbers
atomic masses
electronegativities
structural arrangements
20. The valence electron of which atom in the ground
state has the greatest amount of energy?
A) cesium
C) rubidium
B) lithium
D) sodium
21. Which set of properties is most characteristic of
transition elements?
A) colorless ions in solution, multiple positive
oxidation states
B) colorless ions in solution, multiple negative
oxidation states
C) colored ions in solution, multiple positive
oxidation states
D) colored ions in solution, multiple negative
oxidation states
22. What is the net charge of an ion that has 8
protons, 9 neutrons, and 10 electrons?
A) 1+
B) 2+
C) 1-
D) 2-
23. Compared to the radius of a chlorine atom, the
radius of a chloride ion is
A)
B)
C)
D)
larger because chlorine loses an electron
larger because chlorine gains an electron
smaller because chlorine loses an electron
smaller because chlorine gains an electron
24. As the elements is Period 3 are considered in
order of increasing atomic number, there is a
general decrease in
A)
B)
C)
D)
atomic mass
atomic radius
electronegativity
first ionization energy
25. Which of the following ions has the smallest
radius?
A) F–
B) Cl –
C) K+
D) Ca2+
26. Which element requires the least amount of
energy to remove the most loosely held electron
from a gaseous atom in the ground state?
A) bromine
C) sodium
B) calcium
D) silver
27. Which term represents the attraction one atom
has for the electrons in a bond with another
atom?
A)
B)
C)
D)
electronegativity
electrical conductivity
first ionization energy
mechanical energy
28. Based on Reference Table S, atoms of which of
these elements have the strongest attraction for
the electrons in a chemical bond?
A) Al
B) Si
C) P
D) S
29. The graph below represents the relationship
between atomic radii, in picometers, and
increasing atomic number for elements in Group
15.
Which element is most metallic
A) A
B) B
C) D
D) E
30. Base your answer to the following question on
the information below and on your knowledge of chemistry.
There are six elements in Group 14 on the Periodic Table. One of these elements has the
symbol Uuq, which is a temporary, systematic symbol. This element is now known as flerovium.
Explain, in terms of electron shells, why each successive element in Group 14 has a larger atomic radius, as
the elements are considered in order of increasing atomic number.
Base your answers to questions 31 and 32 on the
information below.
31. Calculate the volume of a tin block that has a
mass of 95.04 grams at STP. Your response must
include both a numerical setup and the calculated
result
32. Identify one element from this table for each
type of element: metal, metalloid, and nonmetal.
Base your answers to questions 33 through 35 on
the information below.
The ionic radii of some Group 2 elements are given in the table below.
33. Explain, in terms of electrons, why the ionic radius of a Group 2 element is smaller than its atomic
radius.
34. State the trend in ionic radius as the elements in Group 2 are considered in order of increasing
atomic number.
35. Estimate the ionic radius of strontium.
Answer Key
Periodic Table
1.
C
31.
7.31 g/cm3 =
2.
D
32.
3.
C
4.
D
5.
A
6.
B
7.
B
–Metal: Tin or Sn or
Lead or Pb
–Metalloid: Silicon or
Si or Germanium or
Ge
–Nonmetal: Carbon or
C
8.
A
33.
9.
C
10.
A
11.
A
12.
C
13.
C
14.
D
– The valence
electron shell of a
Group 2 atom is lost
when it becomes an
ion. – A Group 2 ion
has two fewer
electrons than the
atom from which it
was formed.
15.
A
34.
16.
D
17.
D
18.
A
– As the atomic
number of elements in
Group 2 increases, the
ionic radius increases.
– The ionic radius
increases.
19.
D
35.
– 117 pm
20.
A
21.
C
22.
D
23.
B
24.
B
25.
A
26.
C
27.
A
28.
D
29.
D
30.
–The atomic radius of
these elements
increases down the
group because each
successive element
has one more electron
shell. –The number of
shells per atom
increases.
2 pm