1. Figure 11.1: Graphical data for the ionization energies of the elements show
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Question
1. Figure 11.1: Graphical data for the ionization energies of the elements show sawtooth trends across the periods of the elements.
a. Locate the noble gas group of elements, What appears to be the periodic trend in ionization energies down the noble gas group (i.e., with increasing atomic number)?
b. Scanning the graphical data for elements adjacent to and then further removed from the halogens, what general statement can summarize the trend in the ionization energies when moving down a group of elements?
c. Which element has the highest ionization energy?
d. What general statement can summarize the trend in the ionization energies when moving across a period of elements?
2. Figure 11.2: Graphical data for the atomic radii of the elements show generally decreasing trends across a period of elements. The noble gases are an anomaly.
a. Which group of elements has the largest atomic radii?
b. Moving down a group of elements (increasing atomic number), what is the general trend for atomic radii?
c. Which element has the largest atomic radius?
d. What general statement can summarize the correlation of ionization energies to atomic radii for the elements?
3. Figure 11.3: Graphical data for the electron affinities of the elements show a number of irregularities, but a general increasing trend in values exists across a period of elements.
a. Which group of elements has the highest electron affinities?
b. Is the trend in electron affinities repetitive for Periods 2 and 3? Cite examples.
c. Which element has the highest electron affinity?
d. Is there a correlation of electron affinities to atomic radii for the elements? If so, what is it? Cite examples.
4. Figure 11.4 shows repeated trends in density for the periods of elements.
a. What is the general trend in densities for Periods 2 and 3?
b. What is the trend in the densities moving down a group of elements?
c. Which section of the periodic table (see Introduction) has elements with greater densities?
d. Which element has the greatest density?
Ne 275 lonization Energy (Raimo Atomic Radius (pm) 300 E. o 10 20 30 40 50 Atomic Number Figure 11.1 lonization energies (W/mol) plotted against atomic number 25 0 10 20 30 40 50 Figure 11.2 Atomic radii (pm) plotted against atomic number Electron Affinity (kJ/mol) 888.8888888 LA Density (kg/cm3) -- N - - 3 20 30 40 50 Atomic Number Figure 11.3 Electron affinities (kJ/mol) plotted against atomic number, defined here as energy released 0 10 20 30 40 50 Atomic Number Figure 11.4 Density (kg/m°) plotted against atomic number 1. Figure 11.1: Graphical data for the ionization energies of the elements show sawtooth trends across the periods of the elements. a. Locate the noble gas group of elements, What appears to be the periodic trend in ionization energies down the noble gas group (i.e., with increasing atomic number)? Tonization cancroy decreases down dhe mble ne b. Scanning the graphical data for elements adjacent to and then further removed from the halogens, what general statement can summarize the trend in the ionization energies when moving down a group of elements? Hems c. Which element has the highest ionization energy ennill Hogy nece d. What general statement can summarize the trend in the ionization energies when moving across a period of elements? 2. Figure 11.2: Graphical data for the atomic radii of the elements show generally decreasing trends across a period of elements. The noble gases are an anomaly. a. Which group of elements has the largest atomic radii? Group 1 has ne largest alomicrodus b. Moving down a group of elements (increasing atomic number), what is the general trend for atomic radii? cun grup c. Which element has the largest atomic radius? caesium har lenghest ale venis vadil io inic Paa; incrences d. What general statement can summarize the correlation of ionization energies to atomic radii for the elements? Due to lanthen, de Contraclien, Francium. has lower bomis Yedil-than CCSutim 3. Figure 11.3: Graphical data for the electron affinities of the elements show a number of irregularities, but a general increasing trend in values exists across a period of elements. a. Which group of elements has the highest electron affinities? b. Is the trend in electron affinities repetitive for Periods 2 and 3? Cite examples. c. Which element has the highest electron affinity? d. Is there a correlation of electron affinities to atomic radii for the elements? If so, what is it? Cite examples. 4. Figure 11.4 shows repeated trends in density for the periods of elements. a. What is the general trend in densities for Periods 2 and 32 b. What is the trend in the densities moving down a group of elements? e. Which section of the periodic table (see Introduction) has elements with greater densities? d. Which element has the greatest density?Explanation / Answer
1 a. He > Ne > Ar > Kr > Xe
Explanation: As you move from top to bottom in a group, the ionization energies decrease due to the decrease in nuclear attraction for the valence electron as the new shell is added in each element.
b. As you move down the group, the ionization energies (obtained by removing them from the halogens) decrease as shown below.
I.E. of He = 24.6 eV, for which there is no adjacent halogen
I.E. of Ne = 21.56 eV and that of adjacent F = 17.42 eV, the difference = 21.56 - 17.42 = 4.14 eV
I.E. of Ar = 15.76 eV and that of adjacent Cl = 12.97 eV, the difference = 15.76 - 12.97 = 2.79 eV
and so on..................
d. When you move across a period of elements, the ionization energies increase.
Explanation: As you move from the left to right in a period, the ionization energies increase due to the increase in nuclear charge.
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