Chemistry Chapter 6 Homework Questions
Compare the size of ions to the size of the atoms from which they form
Cations are always smaller than atoms from which they form. Anions are always larger than the atoms fem which they form.
How did chemists begin the process of organizing elements?
Chemists began the process of organizing elements by using the properties of elements to sort them into groups.
What pattern is revealed when the elements are arrange in a periodic table in order of increasing atomic number?
A periodic repetition of the physical and chemical properties.
Identify each element as a metal, metalloid, or nonmetal. A. Gold B. Silicon C. Sulfur D. Barium
A. Metal B. Metalloid C. Non-Metal D. Metal
13) Classify each element as a representative element, transition metal, or noble gas. (go back to the textbook)
A. Noble Gas B. Transition Metal (d block) C. Representative Element (p block)
Which of these metals isn't a transition metal? a. aluminum b. silver c. iron d. zirconium
Aluminum
How do atomic size change within groups and across periods?
Atomic size increases from top to bottom within a group and decreases from left to right across a period.
Which of the following elements are transition metals: Cu, Sr, Cd, Au, Al, Ge, Co?
Au, Cu,Cd, Co
5) Which of these sets of elements have similar physical and chemical properties? A. oxygen, nitrogen, carbon, boron B. Strontium, magnesium, calcium, beryllium C. Nitrogen, neon, nickel, Niobium
B. Strontium, Magnesium, Calcium, Beryllium
How does electronegativity vary within groups and across periods?
Electronegativity values decrease fem top to bottom within a group. Representative elements (values) tends to increase from left to right across period.
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
First Ionization Energy, Electronegativity
What happens to first ionization energy within groups and across periods?
First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period.
How many electrons are in the highest occupied energy level of a Group 5A element?
Five electrons are in the highest occupied energy level of a Group 5A element.
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, Group 8A
Which noble gas does not have eight electrons in its highest occupied energy level?
Helium
How are elements arranged in the modern periodic table?
In the modern periodic table, elements are arranged in order of increasing atomic number.
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.
Why did Mendeleev leave spaces in his periodic table?
Many elements had not been discovered yet.
In general, how are metalloids different from metals and non-metals?
Metalloids have properties that are similar to those of metals and nonmetals. Also 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.
When do ions form?
Positive ions are formed when positive and negative ions form when electrons are transferred between atoms.
Which element in each pair has the larger first ionization energy? a. sodium, potassium b. magnesium, phosphorus
Sodium has the larger first ionization energy and in the second pair, Phosphorus has the largest first ionization energy.
Arrange these elements in order of decreasing atomic size: sulfur, chlorine, aluminum, and sodium. Does your arrangement demonstrate a periodic trend or a group trend?
Sodium, Aluminum, Sulfur, Chlorine. Yes, my arrangement does demonstrate a periodic trend or a group trend.
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.
Why do the elements potassium and sodium have similar chemical properties?
The elements potassium and sodium have similar chemical properties because they have the same number of valence electrons and form +1 ions.
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.
Into what four classes can elements be sorted based on their electron configurations?
The four classes that elements can be sorted in based on their electron configurations are noble gases, representative elements, transition metals, or inner transition metals based on their electrons configurations.
What information can be included in a periodic table?
The information that can be included in a periodic table is symbols and names of elements, along with the information about the structure of their atoms.
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.
What property did Mendeleev use to organize his periodic table?
The property Mendeleev used to organize his periodic table was that he arranged the elements in his periodic table in order of increasing atomic mass.
Name these three broad classes of elements.
The three broad classes of elements are Metals, Nonmetals, and Metalloids.
In general, how can the periodic trends displayed by elements be explained?
The trends that exist among these properties can be explained by variations in atomic structure.
Write the electron configuration of these elements. a. the noble gas in period 3 b. the metalloid in period 3 c. the alkali earth metal in period 3
Write the electron configurations of these elements. a. Ar: 1s2 2s2 2p6 3s2 3p6 b. Si: 1s2 2s2 2p6 3s2 3p2 c. Mg: 1s2 2s2 2p6 3s2
Name two elements that have properties similar to those of the element sodium.
Two elements that have properties similar to those of the element sodium are Potassium (K) and Lithium (Li) because they are in the same group.
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.
Use Figure 6.12 to write the electron configurations of these elements. a. Boron b. Arsenic c. Fluorine d. Zinc e. Aluminum
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
Which element in each pair has a greater first ionization energy? a. Lithium, Boron b. Magnesium, Strontium c. Celsium, Aluminum
a. Boron C. magnesium c. Aluminum
Which element in each pair has a harder electronegativity value? a. Cl, F b. C, N c. Mg, Ne 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+ b. S, S²⁻ c. I, I⁻ d. Al, Al³⁺
a. Na, b. S²⁻, 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 b. O or F c. H or O d. K or S
a. O b. F c. O d. S
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
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 a nonmetal. 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
transition metal (block)
d block
representative element
p block