Regents Review 1
Periodic Table
Notes
1. Which trends appear as the elements in Period 3 are considered from
left to right?
(1) Metallic character decreases,, and electronegativity decreases.
(2) Metallic character decreases, and electronegativity increases.
(3) Metallic character increases, and electronegativity decreases.
(4) Metallic character increases, and electronegativity increases.
2. Arsenic and silicon are similar in that they both
(1) have the same ionization energy
(2) have the same covalent radius
(3) are transition metals
(4) are metalloids
3. The ability of carbon to attract electrons is
(1) greater than that of nitrogen, but less than that of oxygen
(2) less than that of nitrogen, but greater than that of oxygen
(3) greater than that of nitrogen and oxygen
(4) less than that of nitrogen and oxygen
4. Which statement explains why the radius of a lithium atom is larger than
the radius of a lithium ion?
(1) Metals lose electrons when forming an ion.
(2) Metals gain electrons when forming an ion.
(3) Nonmetals lose electrons when forming an ion.
(4) Nonmetals gain electrons when forming an ion.
5. The atoms of the elements in Group 2 have the same
(1) mass number
(2) atomic number
(3 ) number of protons
(4) number of valence electrons
6. Which element has the highest electrical conductivity?
(l)Mg
(3) He
(2)H
(4)C1
7. Given the equation:
This equation represents the formation, of a
(1) fluoride ion, which is smaller in radius than a fluorine atom
(2) fluoride ion, which is larger in radius than a fluorine atom
(3) fluorine atom, which is smaller in radius than a fluoride ion
(4) fluorine atom, which is larger is radius than a fluoride ion
8. Which element is a noble gas?
(1) krypton
(3) antimony
(2) chlorine
(4) manganese
Regents Review
9. Most metals haye the properties of
(1) brittleness and high ionization energy
(2) brittleness and low ionization energy
(3) ductility and high ionization energy
(4) ductility and low ionization energy
10. The high electrical conductivity of metals is primarily due to
(1) high ionization energies
(2) filled energy levels
(3) mobile electrons
(4) high electronegativities
11. Element X is a solid that is brittle, lacks luster, and has six valence electrons.
In which group on the Periodic Table would element^be found?
(1)1
(3)15
(2)2
(4)16
12. On the present Periodic Table of the Elements, the elements are arranged
according to increasing
(1) number of oxidation states
(2) number of neutrons
(3) atomic mass
(4) atomic number
13. The amount of energy required to remove the outermost electron from a
gaseous atom in the ground state is known as
(1) first ionization energy
(2) activation energy
(3) conductivity
(4) electronegativity
14. As the atoms of the Group 17 elements in the ground state are considered
from top to bottom, each successive element has
(1) the same number of valence electrons and similar chemical properties
(2) the same number of valence electrons and identical chemical properties
(3) an increasing number of valence electrons and similar chemical properties
(4) an increasing number of valence electrons and identical chemical properties
15. As the elements in Group 17 on the Periodic Table are considered from
top to bottom, what happens to the atomic radius and the metallic character
of each successive element?
(1) The atomic radius and the metallic character both increase.
(2) The atomic radius increases and the metallic character decreases.
(3) The atomic radius decreases and the metallic character increases.
(4) The atomic radius and the metallic character both decrease.
16. What are two properties of most nonmetals?
(1) high ionization energy and poor electrical conductivity
(2) high ionization energy and good electrical conductivity
(3) low ionization energy and poor electrical conductivity
(4) low ionization energy and good electrical conductivity
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Regents Review
17. An unknown element X can form a compound with the formula XBrs.
In which group on the Periodic Table would element X be found?
(1) 1
(3) 13
(2)2
(4)14
18. Compared to the radius of a chlorine atom, the radius of a chloride ion is
(1) larger because chlorine loses an electron
(2) larger because chlorine gains an electron
(3) smaller because chlorine loses an electron
(4) smaller because chlorine gains an electron
19. Which of the following atoms has the greatest tendency to attract electrons?
(1) barium
(3) boron
(2) beryllium
(4) bromine
20. In which shell are the valence electrons of the elements in Period 2 found?
(1)1
(3)3
(2)2
(4)4
21. Which of the following ions has the smallest radius?
(1)F(3)K+
(2) Cr
(4) Ca2+
22. Which is a property of most nonmetallic solids?
(1) high thermal conductivity
(2) high electrical conductivity
(3) brittleness
(4) malleability
23. Which list of elements contains two metalloids?
(1) Si, Ge, Po, Pb
(3) Si, P, S, Cl
(2) As, Bi, Br, Kr
(4) Po, Sb, I, Xe
24. Which list of elements is arranged in order of increasing atomic radii?
(1) Li, Be, B, C
(3) Sc, Ti, V, Cr
(2)Sr,Ca,Mg,Be
(4) F, Cl, Br, I
25. Which principal energy level can hold a maximum of eight electrons?
(1) 1
(3) 3
(2)2
(4)4
.
26. Which element has properties most like those of magnesium?
(1) calcium
(3) potassium
(2) cesium
(4) sodium
27. Which compound forms a green aqueous solution?
(l)RbCl
(3)NiCl2
(2) CaCl2
(4) ZnCl2
28. Which species does not have a noble gas electron configuration?
(l)Na+
(3) Ar
(2)M g2+
(4)S
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Regents Review 4
29. As the elements of Group 16 are considered in order from top to bottom,
the covalent radius of each successive element increases. This increase
is primarily due to an increase in
(1) atomic number
(2) mass number
(3) the number of protons occupying the nucleus
(4) the number of occupied principal energy levels
30. In Period 3, from left to right in order, each successive element will
(1) decrease in electronegativity
(2) decrease in atomic mass
(3) increase in number of protons
(4) increase in metallic character
31. One electron is removed from both an Na atom and a K atom, producing two ions. Using
principles of atomic structure, explain why the Na ion is much smaller than the K ion. Discuss
both ions in your answer. [2]
32. As a neutral sulfur atom gains two electrons, what happens to the radius of the atom? [1]
33. After a neutral sulfur atom gains two electrons, what is the resulting charge of the ion? [1]
Base your answers to questions 34 and 35 on the information below.
Given: Samples of Na, Ar, As, Rb
34. Which two of the given elements have the most similar chemical properties? [1]
35. Explain your answer in terms of the Periodic Table of the Elements. [1]
Base your answers to questions 36 to 38 on the Reference Tables for Physical Setting/Chemistry.
36. Complete the data table provided in your answer booklet for the following Group 18 elements:
He, Ne, Ar, Kr, Xe [1]