CHEMISTRY (LOOSELEAF) >CUSTOM<
13th Edition
ISBN: 9781264348992
Author: Chang
Publisher: MCGRAW-HILL HIGHER EDUCATION
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Textbook Question
Chapter 8, Problem 8.137QP
On the same graph, plot the effective nuclear charge (see Section 8.3) and atomic radius (see Figure 8.5) versus
The increase in effective nuclear charge from left to right across a period and from top to bottom in a group for representative elements.
Figure 8.5 Atomic radii (in picometers) of representative elements according to their
positions in the periodic table. Note that there is no general agreement on the size of atomic radii. We focus only on the trends in atomic radii, not on their precise values.
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Students have asked these similar questions
5. Explain, using Coulomb's law, the general trend in second and
successive ionization energies across a period for main group
Element
Na
496
4560
Mg
738
1450
7730
Core electrons
elements.
Al
578
1820
2750
11,600
SI
786
1580
3230
4360
16,100
1012
1900
2910
4960
6270
22,200
1000
2250
3360
4560
7010
8500
27,100
CI
1251
2300
3820
5160
6540
9460
11,000
Ar
1521
2670
3930
5770
7240
8780
12,000
11. How do the core charges for H, Li, and Na compare to each other? Based on this answer
and their respective ionization energies, which species has the valence shell with the
largest radius? Which has the valence shell with the smallest radius?
12. Can you deduce a trend in ionization energy as you move from left to right across a
period (row)? Can you deduce a trend in core charge as you move from left to right
across a period (row)? Explain.
Describe the periodic trends in ionization energies.
Typically, the ionization energy increases from left to right on the periodic table.
However, there are minor irregularities. For example, the ionization of oxygen
(Group 6A) is lower than nitrogen (Group 5A).
Considering the electron configuration of these two atoms, choose the best
explanation for this observation.
A) After the loss of an electron, oxygen
would have a stable noble gas
configuration.
lonization Energy (kJ/Mol)
3000
B) Oxygen has a smaller core charge, so the
atom is more likely to give up an electron.
2500
2000
1500
C) The valence electron is in a 2p orbital
1000
500
rather than a 2s orbital. This is further from the
nucleus and so it is not held as tightly.
H He Li Be BCNO F Ne Na Mg Al Si P Si CI Ar K
lonization Energy (kJ/Mol)
D) There is more pairing energy in oxygen's
electron configuration than in nitrogen's
electron configuration.
Chapter 8 Solutions
CHEMISTRY (LOOSELEAF) >CUSTOM<
Ch. 8.2 - An atom of a certain element has 20 electrons. (a)...Ch. 8.2 - Identify the elements that fit the following...Ch. 8.2 - What is the ground-state electron configuration...Ch. 8.3 - Prob. 2PECh. 8.3 - Prob. 3PECh. 8.3 - Prob. 1RCFCh. 8.3 - Arrange the following species in order of...Ch. 8.3 - Identify the spheres shown here with each of the...Ch. 8.4 - (a) Which of the following atoms should have a...Ch. 8.4 - Arrange the following atoms in order of increasing...
Ch. 8.4 - Label the plots shown here for the first, second,...Ch. 8.5 - Is it likely that Ar will form the anion Ar?Ch. 8.5 - Arrange the following atoms in order of increasing...Ch. 8.5 - Why is it possible to measure the successive...Ch. 8.6 - Classify the following oxides as acidic, basic, or...Ch. 8.6 - Prob. 1RCFCh. 8 - Briefly describe the significance of Mendeleevs...Ch. 8 - What is Moseleys contribution to the modern...Ch. 8 - Describe the general layout of a modern periodic...Ch. 8 - What is the most important relationship among...Ch. 8 - Prob. 8.5QPCh. 8 - Prob. 8.6QPCh. 8 - Prob. 8.7QPCh. 8 - What is a representative element? Give names and...Ch. 8 - Prob. 8.9QPCh. 8 - Prob. 8.10QPCh. 8 - You are given a dark shiny solid and asked to...Ch. 8 - What are valence electrons? For representative...Ch. 8 - Write the outer electron configurations for the...Ch. 8 - Use the first-row transition metals (Sc to Cu) as...Ch. 8 - The electron configurations of ions derived from...Ch. 8 - What do we mean when we say that two ions or an...Ch. 8 - What is wrong with the statement The atoms of...Ch. 8 - Give three examples of first-row transition metal...Ch. 8 - In the periodic table, the element hydrogen is...Ch. 8 - A neutral atom of a certain element has 17...Ch. 8 - Group the following electron configurations in...Ch. 8 - Group the following electron configurations in...Ch. 8 - Without referring to a periodic table, write the...Ch. 8 - Specify the group of the periodic table in which...Ch. 8 - Prob. 8.25QPCh. 8 - A metal ion with a net +3 charge has five...Ch. 8 - Prob. 8.27QPCh. 8 - Write the ground-state electron configurations of...Ch. 8 - Write the ground-state electron configurations of...Ch. 8 - Name the ions with +3 charges that have the...Ch. 8 - Which of the following species are isoelectronic...Ch. 8 - Group the species that are isoelectronic: Be2+, F,...Ch. 8 - Prob. 8.33QPCh. 8 - How does atomic radius change (a) from left to...Ch. 8 - Prob. 8.35QPCh. 8 - Explain why, for isoelectronic ions, the anions...Ch. 8 - Prob. 8.37QPCh. 8 - Arrange the following atoms in order of decreasing...Ch. 8 - Prob. 8.39QPCh. 8 - Which is the smallest atom in Group 7A?Ch. 8 - Why is the radius of the lithium atom considerably...Ch. 8 - Use the second period of the periodic table as an...Ch. 8 - Indicate which one of the two species in each of...Ch. 8 - List the following ions in order of increasing...Ch. 8 - Prob. 8.45QPCh. 8 - Explain which of the following anions is larger,...Ch. 8 - Give the physical states (gas, liquid, or solid)...Ch. 8 - Prob. 8.48QPCh. 8 - Prob. 8.49QPCh. 8 - Sketch the outline of the periodic table and show...Ch. 8 - Arrange the following in order of increasing first...Ch. 8 - Prob. 8.52QPCh. 8 - Prob. 8.53QPCh. 8 - In general, ionization energy increases from left...Ch. 8 - Prob. 8.55QPCh. 8 - Two atoms have the electron configurations...Ch. 8 - Prob. 8.57QPCh. 8 - Plasma is a state of matter consisting of positive...Ch. 8 - Prob. 8.59QPCh. 8 - Prob. 8.60QPCh. 8 - Arrange the elements in each of the following...Ch. 8 - Specify which of the following elements you would...Ch. 8 - Considering their electron affinities, do you...Ch. 8 - Explain why alkali metals have a greater affinity...Ch. 8 - What is meant by the diagonal relationship? Name...Ch. 8 - Prob. 8.66QPCh. 8 - Use the alkali metals and alkaline earth metals as...Ch. 8 - Based on your knowledge of the chemistry of the...Ch. 8 - As a group, the noble gases are very stable...Ch. 8 - Prob. 8.70QPCh. 8 - Prob. 8.71QPCh. 8 - Write balanced equations for the reactions between...Ch. 8 - Write formulas for and name the binary hydrogen...Ch. 8 - Which oxide is more basic, MgO or BaO? Why?Ch. 8 - State whether each of the following properties of...Ch. 8 - With reference to the periodic table, name (a) a...Ch. 8 - Write equations representing the following...Ch. 8 - List all the common ions of representative...Ch. 8 - Write the empirical (or molecular) formulas of...Ch. 8 - Element M is a shiny and highly reactive metal...Ch. 8 - Match each of the elements on the right with its...Ch. 8 - Arrange the following species in isoelectronic...Ch. 8 - Prob. 8.83QPCh. 8 - Which of the following properties show a clear...Ch. 8 - Prob. 8.85QPCh. 8 - Prob. 8.86QPCh. 8 - Prob. 8.88QPCh. 8 - For each pair of elements listed, give three...Ch. 8 - Name the element that forms compounds, under...Ch. 8 - Explain why the first electron affinity of sulfur...Ch. 8 - The H ion and the He atom have two 1s electrons...Ch. 8 - Predict the products of the following oxides with...Ch. 8 - Prob. 8.94QPCh. 8 - Prob. 8.95QPCh. 8 - Prob. 8.96QPCh. 8 - Prob. 8.97QPCh. 8 - The formula for calculating the energies of an...Ch. 8 - Why do noble gases have negative electron affinity...Ch. 8 - The atomic radius of K is 227 pm and that of K+ is...Ch. 8 - The atomic radius of F is 72 pm and that of F is...Ch. 8 - Prob. 8.102QPCh. 8 - Referring to the Chemistry in Action essay...Ch. 8 - Prob. 8.104QPCh. 8 - Prob. 8.105QPCh. 8 - Prob. 8.106QPCh. 8 - Identify the ions whose orbital diagrams for the...Ch. 8 - Prob. 8.108QPCh. 8 - Prob. 8.109QPCh. 8 - Prob. 8.110QPCh. 8 - Explain, in terms of their electron...Ch. 8 - The standard enthalpy of atomization of an element...Ch. 8 - Write the formulas and names of the hydrides of...Ch. 8 - Prob. 8.114QPCh. 8 - Prob. 8.115QPCh. 8 - Prob. 8.116QPCh. 8 - Write a balanced equation for the preparation of...Ch. 8 - Write chemical formulas for oxides of nitrogen...Ch. 8 - Prob. 8.119QPCh. 8 - In general, atomic radius and ionization energy...Ch. 8 - Explain why the electron affinity of nitrogen is...Ch. 8 - Prob. 8.122QPCh. 8 - Write a balanced equation that predicts the...Ch. 8 - Prob. 8.124QPCh. 8 - Prob. 8.125QPCh. 8 - Prob. 8.126QPCh. 8 - Prob. 8.127QPCh. 8 - Predict the atomic number and ground-state...Ch. 8 - Prob. 8.129QPCh. 8 - Prob. 8.130QPCh. 8 - Prob. 8.131QPCh. 8 - Prob. 8.132QPCh. 8 - Prob. 8.133QPCh. 8 - Both Mg2+ and Ca2+ are important biological ions....Ch. 8 - Match each of the elements on the right with its...Ch. 8 - Prob. 8.136QPCh. 8 - On the same graph, plot the effective nuclear...Ch. 8 - One allotropic form of an element X is a colorless...Ch. 8 - Prob. 8.139QPCh. 8 - Prob. 8.140QPCh. 8 - Use your knowledge of thermochemistry to calculate...Ch. 8 - Referring to Table 8.2, explain why the first...Ch. 8 - Prob. 8.143QPCh. 8 - One way to estimate the effective charge (Zeff) of...Ch. 8 - To prevent the formation of oxides, peroxides, and...Ch. 8 - Prob. 8.146QPCh. 8 - Recent theoretical calculations suggest that...Ch. 8 - Prob. 8.148QPCh. 8 - Compare the work function for cesium (206 kJ/mol)...Ch. 8 - Prob. 8.150QPCh. 8 - Prob. 8.151QPCh. 8 - Prob. 8.152QPCh. 8 - Using the following boiling-point data, estimate...Ch. 8 - Prob. 8.154QPCh. 8 - Prob. 8.155QP
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