a. shared chemical properties among small groups of elements
b. the tendency of elements to combine with
other elements in fixed, whole-number ratios
c. atomic weights for all then-known elements
d. atomic numbers and the existence of subatomic particles
2.When Dmitri Mendeleev published his periodic table of the elements in 1869, there were 59 known elements. Today there are 118 known elements. Mendeleev's periodic table, despite the increase in the number of discovered elements, maintains much of its original structure.what is one feature of Mendeleev's periotic table design that made it possible to accommodate new elements.
3.Groups of elements in the periodic table have similar chemical properties based upon the atoms':
a. atomic mass
b. number of energy levels
c. atomic number
d. number of valence electrons
4.Elements 37-54 are located in a family.
5.Metalloids are elements that:
a. have a high luster
b. are excellent conductors of electricity
c. have properties of both metals and nonmetals
d. are excellent insulators
6.Which of the following groups contains reactive elements that need to gain only one electron to have a full outer energy level?
a. alkali metals
b. alkaline earth metals
d. noble gases
7.What is the name of the group (family) that includes the elements radium, strontium, and magnesium?
c. alkaline earth metals
d. alkali metals
8.Which of the following is not true of the chalcogen group?
a. atoms of this group have six electrons in the outermost s and p sub-levels
b. includes sulfur
c. includes only nonmetals
d. includes metalloids
9.The alkali metal group includes: hydrogen, lithium, sodium, potassium, rubidium, cesium, and francium.
10.Classify the following elements as alkali, alkaline earth, or halogen.
11.The atomic mass of an element is the:
a. combination of neutrons and protons in an atom of that element
b. weighted average of the masses of known, naturally-occurring isotopes of an element
c. number of electrons in an atom of that element
d. number of protons in an atom of that element
12.For any element, its atomic number is generally larger than the atomic mass.
13.The symbol for the element titanium is Tm.
14.Hf is the symbol for the element Heffner.
15.Which of the following four elements has the smallest radius?
a. potassium (K)
b. francium (Fr)
c. magnesium (Mg)
d. nitrogen (N)
16.Which of the following elements has the highest ionization energy?
17.The energy required to remove an electron from a neutral atom is the:
a. atomic size
b. ionization energy
18.The electron configuration 1s22s22p3 describes the electrons of the phosphorus atom.
19.The abbreviated electron configuration for cesium is [Kr] 5s24d105p66s1.
20.Which of the following noble gas cores should be used for the shorthand electron configuration of tin?
21.Which of the following groups of elements contains the most valence electrons per atom?
c. Noble gases
d. Alkali metals
22.Which of the following elements possesses the most valence electrons?
23.Atoms of the noble gas elements possess complete valence energy levels.
24.The chalcogens possess five electrons in the valence energy level.
25.How many dots should be drawn around the symbol, C, to create the Lewis dot structure for a carbon atom?
26.To achieve an octet in the valence energy level, an oxygen atom will gain two electrons.
27.To achieve an octet in the valence energy level, a fluorine atom will gain two electrons.
28.To achieve an octet of valence electrons, a magnesium atom becomes Mg2+.
29.To achieve an octet of valence electrons, a cesium atom will become an ion with what charge?
30.To achieve an octet of valence electrons, an iodine atom will become an ion with what charge?
31.To achieve an octet, the oxygen atom forms an ion. The name of this ion is:
a. oxide ion
b. oxygen ion
c. oxic ion
d. oxous ion
32.The correct name for a Mn4+ cation is:
a. -manganese ion
b. -manganese (IV) ion
d. -manganese4 ion
33.The suffix for the name of a monatomic anion (negatively charged particle) is:
34.It is possible for the transition metal zinc to form more than one possible ion.
35.In the name "copper (II) ion," the "II" stands for the number of electrons gained when the copper atom becomes an ion.
36.Fe2+ is known as the iron (II) ion.
37.how you can use the electron configuration to determine whether the element Gallium would form a cation or anion. What is the most common Gallium ion?