Ch 6
Where are the alkali metals, the alkaline earth metals, the halogens, and the noble gases located in the periodic table?
Group 1A, Group 2A, Group 7A, and Group 8A, respectively
Why is there a large increase between the first and second ionization energies of the alkali metals?
It is relatively easy to remove the first electron from an alkali metal atom; it is much more difficult to remove the second.
In general, how are metalloids different from metals and nonmetals?
Metalloids have properties that are similar to those of metals and nonmetals. How a metalloid behaves depends on the conditions.
Which of the following are symbols for representative elements: Na, Mg, Fe, Ni, Cl?
Na, Mg, Cl
Why are noble gases not included in Table 6.2?
Noble gases, with rare exception, do not form compounds.
What effect did the discovery of gallium have on the acceptance of Mendeleev's table?
The close match between the predicted properties and the actual properties of gallium helped gain wider acceptance for Mendeleev's periodic table.
Explain the difference between the first and second ionization energy of an element.
The first ionization energy is the energy needed to remove a first electron from an atom. The second ionization energy is the energy needed to remove a second electron.
How does the ionic radius of a typical metal compare with its atomic radius?
The ionic radius of a metal cation is smaller than the atomic radius of the metal atom.
Based on their locations in the periodic table, would you expect carbon and silicon to have similar properties? Explain your answer.
Yes; both carbon and silicon are in Group 4A, and each has four electrons in the highest occupied energy level.
For which of these properties does lithium have a larger value than potassium? a. first ionization energy b. atomic radius c. electronegativity d. ionic radius
a and c
What pattern is revealed when the elements are arranged in a periodic table in order of increasing atomic number?
a periodic repetition of their physical and chemical properties
Use Figure 6.13 to write the electron configurations of these elements. a. boron c. fluorine e. aluminum b. arsenic d. zinc
a. 1s2 2s2 2p1 b. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3 c. 1s2 2s2 2p5 d. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 e. 1s2 2s2 2p6 3s2 3p1
Write the electron configurations of these elements. a. the noble gas in Period 3 b. the metalloid in Period 3 c. the alkali earth metal in Period 3
a. Ar: 1s2 2s2 2p6 3s2 3p6 b. Si: 1s2 2s2 2p6 3s2 3p2 c. Mg: 1s2 2s2 2p6 3s2
Which element in each pair has a higher electronegativity value? a. Cl, F c. Mg, Ne b. C, N d. As, Ca
a. F b. N c. Mg d. As
Which particle has the larger radius in each atom/ion pair? a. Na, Na^+ c. I, I^- b. S, S^2- d. Al, Al^3+
a. Na b. S^2 c. I^- d. Al
When the elements in each pair are chemically combined, which element in each pair has a greater attraction for electrons? a. Ca or O c. H or O b. O or F d. K or S
a. O b. F c. O d. S
Arrange the following groups of elements in order of increasing ionization energy: a. Be, Mg, Sr b. Bi, Cs, Ba c. Na, Al, S
a. Sr, Mg, Be b. Cs, Ba, Bi c. Na, Al, S
Which element in each pair has a greater first ionization energy? a. lithium, boron b. magnesium, strontium c. cesium, aluminum
a. boron b. magnesium c. aluminum
Identify each property below as more characteristic of a metal or a nonmetal. a. a gas at room temperature b. brittle c. malleable d. poor conductor of electric current e. shiny
a. nonmetal b. nonmetal c. metal d. nonmetal e. metal
Which element in each pair has atoms with a larger atomic radius? a. sodium, lithium b. strontium, magnesium c. carbon, germanium d. selenium, oxygen
a. sodium b. strontium c. germanium d. selenium
Which of these metals isn't a transition metal? a. aluminum c. iron b. silver d. zirconium
aluminum
Which noble gas does not have eight electrons in its highest occupied energy level?
helium
Why did Mendeleev leave spaces in his periodic table?
so that undiscovered elements with similar properties could be placed in the same group
