Chapter 5 test review
61.. Draw the electron dot formula for: H, B, N, F, Ca, Si, O, Ar
...
83. Predict the atomic radius, density, and melting point for radioactive francium:
0.284 nm; 2.21 g/mL; 17.9 C
51. Which energy sublevel is being filled by the lanthanide series?
4f sublevel
the elements with atomic numbers 90-103
A) actinide series
87. Explain why the ionization energy for hydrogen is much higher than that of other group 1 elements?
Although H and the group 1 metals each have one valence electron, in H the electron is closer to its nucleus. Because the negatively charged electron is closer to the positively charged nucleus, it requires more energy to remove the electron from hydrogen than a group 1 metal.
7. Which two elements in the fourth period violate the original periodic law as stated by Mendeleev?
Co and Ni
the inner electrons in an atom which are not available for bonding
D) core electrons
a method of writing an electron configuration in which core electrons are represented by a noble gas symbol in brackets followed by the valence electrons, for example, [Ne] 3s^2
E) core notation
a shorthand description of the arrangement of electrons by sublevels according to increasing energy levels
F) electron configuration
the chemical symbol of an element surrounded by a dot representing each valence electron
G) electron dot formula
5. Before Mosely'e discovery in 1913, the periodic law stated that physical and chemical properties tend to repeat periodically when elements are arranged according to what trend?
Increasing atomic mass
the elements in the lanthanide and actinide series
J) inner transition elements
an atom that bears a charge as a result of gaining or losing valence electrons
K) ion
refers to the positive charge on a metal atom that has lost electrons or to the negative charge on a nonmetal atom that has gained electrons
L) ionic charge
the amount of energy necessary to remove an electron from an atom
M) ionization energy
refers to ions having the same electron configuration; for example Mg ^2+ and O^2- each have 10 electrons
N) isoelectronic
the elements with atomic numbers 58-71
O) lanthanide series
19. Which radioactive elements are semimetals because their appearance resembles that of metals?
Po and At
The properties of elements recur in a repeating pattern when arranged by increasing atomic number.
R) Periodic Law
the elements with atomic numbers 21,39,57, and 58-71
S) rare earth elements
the group A (1,2 and 13-18) elements in the periodic table
T) representative elements
The group B (3-12) elements in the periodic table
U) transition elements
the elements beyond the atomic number 92
V) transuranium elements
the electrons that occupy the outermost s and p sublevels of an atom
W) valence electrons
23. According to IUPAC, what is the designation for each of the following groups indicated by the American convention? A) Group IA B) Group IIIA C) Group VA D) Group VIIA E) Group IB F) Group IIIB G) Group VB H) Group VIIB
a) 1 b) 13 c) 15 d) 17 e) 11 f) 3 g) 5 h) 7
57. State the number of Valence Electrons in each of the following groups. A) 1 B) 13 C) 15 D) 17 59. H, B, N, F, Ca, Si, O, Ar
a) 1 b) 3 c) 5 d) 7 1,3,5,7,2,4,6,8
71. State the predicted ionic charge of metal ions in each of the following groups of elements. A) 1 B) 2 C) 13 D) 14
a) 1+ b) 2+ c) 3+ d) 4+
73. Write the ionic charge for each of the following ions. a) Cs ion b) Ga ion C) O ion D) I ion
a) 1+ b) 3+ c) 2- d) 1-
53. Refer to the PT and state the highest energy sublevel for each of the following elements: A) H B) Na C) Sm D) Br E) Sr F) C G) Sn H) Cs
a) 1s b) 3s c) 4f d) 4p e) 5s f) 2p g) 5p h) 6s
6. Which energy sublevel is being filled by the elements Sc to Zn? 3d, 4s, 4p, 4d, 4f
a) 3d
33. According to general trends in the PT, predict which element in each of the following pairs has greater metallic character: A) B or Al B) Na or K C) Mg or Ba D) H or Fe
a) Al b) K c) Ba d) Fe
45. Depending upon reaction conditions, nitrogen and oxygen can produce either N2O3 and N2O5. Predict two formulas for each of the following compounds. A) arsenic oxide B) antimony oxide
a) As2O3 and As2O5 b) Sb2O3 and Sb2O5
43. The chemical formula for barium chloride is BaCl2. Predict the formulas for each of the following similar compounds. A)calcium fluoride B)calcium chloride C)calcium bromide D) calcium iodide
a) CaF2 b) CaCl2 c) CaBr2 d) CaI2
69. Which elements in each of the following pairs had the lower ionization energy? A) Rb or Cs B) He or Ar C) B or Al D) F or I
a) Cs b) Ar c) Al d) I
41. The formulas for the chlorides of potassium, calcium, boron, and germanium are, representatively KCl, CaCl2, BCl3, and GeCl4. using the PT, predict the chemical formulas for each of the following similar compounds. A)potassium fluoride B)calcium fluoride c)boron bromide D) germanium iodide
a) KF b) CaF2 c) BBr3 d) GeI4
67. Which elements in each of the following pairs has the higher ionization energy. A) Mg or Ca B) S or Se C) Sn or Pb D) N or P
a) Mg b) S c) Sn d) N
35. According to general trends in the PT, predict which element in each of the following pairs has the larger atomic radius. A) Li or Na B) N or P C) Mg or Ca D) Ar or Kr
a) Na b) P c) Ca d) Kr
79. Write the electron configuration for each of the following negative ions using core notations: A) F- B) S2- C) N3- D) I3-
a) [He] 2s2, 2p6, or [Ne] b) [Ne] 3s2, 3p6, or [Ar] c) [He] 2s2, 2p6, or [Ne] d) [Kr] 5s2, 4d10, 5p6 or [Xe]
85. Write the electron configuration for each of the following elements using core notation: A) Sr B) Ru C) Sb D) Cs
a) [Kr] 5s2 b) [Kr] 5s2 4d6 c) [Kr] 5s2 4d10 5p3 d) [Xe] 6s1
77. Write the electron configuration for each of the following positive ions using core notation: A) Mg 2+ B) K+ C) Fe+ D) Zr2+
a) [Ne] b) [Ar] c) [Ar] 3d6 d) [Kr] 4d2
75. Which of the following ions are isoelectronic with the noble gas argon: A) Al3+ B) Ca2+ C) S2- D) N3-
b) Ca2+ c) S2-
9. Which of the following elements has the highest ionization energy. a) H b) He c) Ne d) Cl e) F
b) He
4. Which of the following elements has the most metallic character? A) Li B) Na C) Be D) Mg E) Al
b) Na
5. Calculate the predicted atomic radius for selenium, Se, given the atomic radius of sulfur, S (0.104 nm) and tellurium, Te, (0.143 nm).
c) 0.124 nm
Which of the following groups has a predictable ionic charge of three negative? a) 13 b) 3 c) 15 d) 5 e) 18
c) group 15
49. What type of energy sublevel is being filled by the transition elements?
d sublevel
7. Predict the number of valence electrons for group 17.
d) 7
29. According to the general trend, metallic character for a period of elements (increases/decreases) proceeding from left to right in the PT.
decreases
31. According to the general trend, the atomic radius for a period of elements (increases/decreases) proceeding from left to right in the PT
decreases
1. Which scientist contributed to the development of the periodic table of elements.
e) J.W. Dobereiner, Dmitri Mendeleev, H.G. Moseley, Newland
8. What is the electron dot formula for an atom of neon.
e) Ne
65. Which group of elements has the lowest ionization energy?
group 1
63. Ionization energy for a group of elements (+-) proceeding up a group in the periodic table.
increases
15. What is the term for the two series of elements that include Ce-Lu and Th-Lr
inner transition elements
17. What is the term for the elements on the left side of the periodic table?
metals
47. What type of energy sublevel is being filled by the elements in groups IA/1 and IIA/2
s sublevel
13. What is the term for the elements in the series that follows element 57?
the lanthanides
