Chapter 6 Test Study Guide
Why is the first ionization energy of a nonmetal much higher than that of an alkali metal?
Across a period, the first ionization energy increases, making the first ionization of a nonmetal much higher than that of an alkali metal.
How did Mendeleev's work contribute to the discovery of electrons?
Mendeleev's work contributed to the discovery of electrons by developing his table before scientists knew about the structure of atoms.
Which of the following are symbols for representative elements: Na, Mg, Fe, Ni, Cl?
Na, Mg, Cl
Why are noble gases not included in the Electronegativity Values for Selected Elements figure?
The noble gases are omitted because they do not form many compounds.
Why does it take more energy to remove a 4s electron from zinc than from calcium?
Zinc has a greater nuclear charge (more protons) than calcium.
Write the symbol of the element or elements that fit each description. a. a nonmetal in group 4A b. the inner transition metal with the lowest atomic number c. all of the nonmetals for which the atomic number is a multiple of five d. a metal in group 5A
a. C b. La c. P, Br d. As, Sb, Bi, Uup
List the symbols for all the elements with electron configurations that end as follows. Each "n" represents an energy level. a. ns1 b. ns2np4 c. ns2nd10
a. H, Li, Na, K, Rb, Cs, Fr b. O, S, Se, Te, Po c. Zn, Cd, Hg, Uub
In each pair, which ion is larger? a. Ca2+, Mg2+ b. Cl-, P3- c. Cu+, Cu2+
a. Mg2+ b. P3- c. Cu2+
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
Identify each property below as more characteristic of a metal or 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
What effect did the discovery of gallium have on the acceptance of Mendleev'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 increase in energy between the first and second ionization energies is large.
Which element in each pair has a higher electronegativity value? a. Cl, F b. C, N c. Mg, Ne d. As, Ca
a. F b. N c. Ne d. As
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. First ionization energy b. electronegativity
Which particle has the larger radius in each atom/ion pair? a. Na, Na+ b. S, S2- c. I, I- d. Al, Al3+
a. Na+ b. S c. I- d. Al3+
What pattern is revealed when the elements are arranged in a periodic table in order of increasing atomic number?
periodic repetition of the elements' physical and chemical properties
Do you think there are more elements left to discover? If so, what is the lowest atomic number a new element could have? Explain.
I do not think that there are more elements to be discovered.
Explain why there should be a connection between an element's electron configuration and its location on the periodic table.
There should be a connection between an element's electron configuration and its location on the periodic table because electrons play a key role in determining the properties of elements.
Which equation represents the first ionization of an alkali metal atom? a. Cl----Cl(+)+e- b. Ca----Ca(+)+e- c. K----K(+)+e- d. H----H(+)+e-
K----Ca(+)+e-
In general, how are metalloids different from metals and nonmetals?
Metalloids behave differently, but similarly to metals and nonmetals
Why is there a large increase between the first and second ionization energies of the alkali metals?
There is a large increase between the first and second ionization energies of the alkali metals because it is relatively easy to remove one electron from a Group 1A metal atom, but it is difficult to remove a second electron.
Locate each of the following elements in the periodic table and decide whether its atoms are likely to form anions or cations. a. sodium b. fluorine c. calcium d. potassium e. iodine f. beryllium g. oxygen h. lithium
a. Na, cation b. F, anion c. Ca, cation d. K, cation e. I, anion f. Be, cation g. O, anion h. Li, cation
Give a reason for each of the following comparisons: a. Calcium has a smaller second ionization energy than does potassium. b. Lithium has a larger first ionization energy than does cesium. c. Magnesium has a larger third ionization energy than does aluminum
a. The electrons in calcium are removed from the same energy level. In potassium, the second electron is removed from a lower energy level. b. Because cesium has a larger atomic radius than lithium, the nuclear charge in a cesium atom has a smaller effect on the electrons in the highest occupied energy level. c. The third electron removed from a magnesium atom is in a lower energy level.
Which of these metals isn't a transition metal? a. aluminum b. silver c. iron d. zirconium
a. aluminum
Which element in each pair has a greater first ionization energy? a. lithium, boron b. magnesium, strontium c. cesium, aluminum
a. boron b. strontium c. cesium
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 noble gas does not have eight electrons in its highest occupied energy level?
helium
What trend is demonstrated by the following series of equations? Li+520 kJ/mol----Li(+)+e- O+1314 kJ/mol----O(+)+e- F+1681 kJ/mol----F(+)+e- Ne+2080 kJ/mol----Ne(+)+e-
ionization energy
Based on their locations in the periodic table, would you expect carbon and silicon to have similar properties? Explain your answer.
I would not expect carbon and silicon to have similar properties, for silicon has a higher atomic mass than carbon, and silicon is a metalloid, while carbon is a nonmetal.
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.
Where are the alkali metals, the alkaline earth metals, the halogens, and the noble gases located in the periodic table?
Alkali: Group 1A Alkaline earth: Group 2A Halogen: Group 7A Noble Gas: Group 8A
Explain why fluorine has a smaller atomic radius than both oxygen and chlorine
Fluorine has a smaller atomic radius than both oxygen and chlorine because the distance of Fluorine's nuclei is closer together than the other two elements.
Why did Mendleev leave spaces in his periodic table?
He predicted that elements would be discovered to fill those spaces, and he predicted what their properties would be based on their locations in the table.
Would you expect metals or nonmetals in the same period to have higher ionization energies? Give a reason for your answer.
I would expect nonmetals in the same period to have higher ionization energies because the atomic mass increases as the period goes from right to left.
There is a large jump between the second and third ionization energies of magnesium. There is a large jump between the third and fourth ionization energies of aluminum. Explain these observations.
It is relatively easy to remove two electrons from magnesium; it is much more difficult to remove a third electron. It is relatively easy to remove three electrons from aluminum; it is much more difficult to remove a fourth electron.
When the elements in each pair are chemically combined, which element in each pair has a greater attraction for electrons? a. Ca or O b. O or F c. H or O d. K or S
a. O b. F c. O d. S
Write the electron configurations of the following ions: a. the liquid in Group 7A with a 1- charge b. the metalloid in Period 3 with a 4+ charge c. the gas in Group 6A with a 2- charge d. the alkali earth metal in period 3 with a 2+ charge
a.1s22s22p63s23p63d104s24p6 b.1s22s22p6 c.1s22s22p6 d.1s22s22p6
In which pair of elements are the chemical properties of the elements most similar? Explain your reasoning. a. sodium and chlorine b. nitrogen and phosphorus c. boron and oxygen
b; nitrogen and phosphorus are in the same group (Group 5A)
