CHEMISTRY-TEXT
8th Edition
ISBN: 9780134856230
Author: Robinson
Publisher: PEARSON
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Textbook Question
Chapter 6, Problem 6.72SP
No element has a negative second
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A) Which of the halogen elements has the highest density in its standard state?
B) Which of the elements of the third period should have the highest 2nd ionization energy?
C) For which of Al, Si or P is the absolute value of the Electron Affinity greatest?
D) Which of the ions Mg2+, Sr2+, Ca2+, Be2+, Ba2+, or Ra2+ is the smallest?
E) For the elements: X = Br, I, Cl, or H, which has the the smallest average X-C bond energy?
Despite the expected decrease in atomic size, there is an unexpected drop in IE1 values between Groups 2A(2) and 3A(13) in Periods 2 through 4. Explain this pattern in terms of electron configurations and orbital energies.
An atom with a stronger electron affinity is often more reactive. Given a pressurized chamber containing H2, which species would you expect to react more with hydrogen, Cl or Br? Explain.
Chapter 6 Solutions
CHEMISTRY-TEXT
Ch. 6 - Prob. 6.1PCh. 6 - APPLY 6.2 Which of the following sets of ions are...Ch. 6 - Which atom or ion has the largest radius:...Ch. 6 - Conceptual APPLY 6.4 Which of the following...Ch. 6 - Use the periodic table to order the elements from...Ch. 6 - Given the orbital filling diagrams for the valence...Ch. 6 - Which has the largest third ionization energy: Be,...Ch. 6 - Conceptual APPLY 6.8 The figure on the right...Ch. 6 - Order the following elements from least to most...Ch. 6 - Conceptual APPLY 6.10 Which of the indicated three...
Ch. 6 - What electron configuration does the strontium...Ch. 6 - Prob. 6.12ACh. 6 - Prob. 6.13PCh. 6 - APPLY 6.14 Calculate the energy of electrostatic...Ch. 6 - Which substance has the largest lattice energy:...Ch. 6 - One of the following pictures represents NaCl and...Ch. 6 - Prob. 6.17PCh. 6 - What structural features do ionic liquids havethat...Ch. 6 - PROBLEM 6.18 Compare the following two ionic...Ch. 6 - PROBLEM 6.19 An ionic liquid consisting of a bulky...Ch. 6 - Where on the periodic table would you find the...Ch. 6 - Which of the following spheres is likely to...Ch. 6 - Circle the approximate part or parts of the...Ch. 6 - Prob. 6.24CPCh. 6 - This figure represents the successive ionization...Ch. 6 - In the following drawings, red spheres represent...Ch. 6 - Which of the following drawings is more likely to...Ch. 6 - Prob. 6.28CPCh. 6 - Which of the following alkali metal halides has...Ch. 6 - Which of the following alkali metal halides has...Ch. 6 - Three binary compounds are represented on the...Ch. 6 - Prob. 6.32CPCh. 6 - Prob. 6.33CPCh. 6 - What is the difference between a covalent bond and...Ch. 6 - Prob. 6.35SPCh. 6 - What is the difference between a molecule and an...Ch. 6 - Prob. 6.37SPCh. 6 - How many protons and electrons are in each of the...Ch. 6 - What is the identity of the element X in the...Ch. 6 - Prob. 6.40SPCh. 6 - Prob. 6.41SPCh. 6 - Prob. 6.42SPCh. 6 - Prob. 6.43SPCh. 6 - What doubly positive ion has the following...Ch. 6 - Prob. 6.45SPCh. 6 - Prob. 6.46SPCh. 6 - Which element in the transition-metal series Sc...Ch. 6 - Prob. 6.48SPCh. 6 - Prob. 6.49SPCh. 6 - Order the following ions from smallest to largest:...Ch. 6 - Order the following ions from smallest to largest:...Ch. 6 - Which ion has a larger atomic radius, Cu+ or Cu2+...Ch. 6 - Which ion hasa larger atomic radius, Fe2+ or Fe3+...Ch. 6 - The following ions all have the same number of...Ch. 6 - Which of the ions Se2,F,O2 and Rb+ has the largest...Ch. 6 - Which group of elements in the periodic table has...Ch. 6 - Prob. 6.57SPCh. 6 - Which element in each of the following sets has...Ch. 6 - Order the elements in each set from the smallest...Ch. 6 - (a) Which has the smaller second ionization...Ch. 6 - (a) Which has the smaller fourth ionization...Ch. 6 - Three atoms have the following electron...Ch. 6 - Three atoms have the following electron...Ch. 6 - The first four ionization energies in kJ/mol of a...Ch. 6 - The first four ionization energies in kJ/mol of a...Ch. 6 - Prob. 6.66SPCh. 6 - Prob. 6.67SPCh. 6 - Prob. 6.68SPCh. 6 - Prob. 6.69SPCh. 6 - Why is energy usually released when an electron is...Ch. 6 - Why does ionization energy increase regularly...Ch. 6 - No element has a negative second electron...Ch. 6 - Why does phosphorus have a less negative electron...Ch. 6 - Prob. 6.74SPCh. 6 - What noble-gas configurations and charge are the...Ch. 6 - Each of the following pairs of elements will react...Ch. 6 - Each of the following pairs of elements will react...Ch. 6 - Element X reacts with element Y to give a product...Ch. 6 - Element X reacts with element Y to give a product...Ch. 6 - Calculate the energy change in kilojoules per mole...Ch. 6 - Prob. 6.81SPCh. 6 - Find the lattice energy of LiBr(s) in Table 6.3,...Ch. 6 - Look up the lattice energies in Table 6.3, and...Ch. 6 - Born-4-Iaber cycles, such as those shown in...Ch. 6 - Calculate a lattice energy for CaH2(s) in...Ch. 6 - Calculate the overall energy change in kilojoules...Ch. 6 - The estimated lattice energy for CsF2(s) is +2347...Ch. 6 - Calculate the overall energy change in kilojoules...Ch. 6 - Use the data in Problem 6.88 to calculate an...Ch. 6 - Use the data and the result in Problem 6.84 to...Ch. 6 - Prob. 6.91SPCh. 6 - Calculate overall energy changes in kilojoules per...Ch. 6 - Prob. 6.93SPCh. 6 - We saw in Section 6.7 that the reaction of solid...Ch. 6 - Draw a Born—Haber cycle for the reaction of sodium...Ch. 6 - Use the following information plus the data given...Ch. 6 - Prob. 6.97SPCh. 6 - Prob. 6.98SPCh. 6 - Order the following compounds according to their...Ch. 6 - Prob. 6.100MPCh. 6 - Heating elemental cesium and platinum together for...Ch. 6 - Given the following information, construct a...Ch. 6 - Consider the electronic structure of the element...Ch. 6 - Prob. 6.104MPCh. 6 - The ionization energy of an atom can be measured...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forwardOrder the following elements from smallest to largest electron affinity. 1. O, Ne, Na1+, F 2. Ca, Li, Sb, I 3. Zn, Fr, Cl, Ararrow_forwardDoes the reaction of a main-group nonmetal oxide in water produce an acidic or a basic solution? Write a balanced equation for the reaction of a Group 6A(16) nonmetal oxide with water.arrow_forward
- The alkali metal with an electron configuration of [Xe] 6s¹ is:arrow_forwardWhich of the ions Mg2+, Sr2+, Ca2+, Be2+, Ba2+, or Ra2+ is the smallest? Which of the elements of the third period should have the highest 2nd ionization energy? S, P, Si, Al, Mg, Na Which of the halogen elements has the highest density in its standard state? Br, Cl, F, Atarrow_forwardWhich of the following elements have the least electron affinity? P, Ne, Se, Asarrow_forward
- In a plot of IE1 for the Period 3 elements , why do the values for elements in Groups 3A(13) and 6A(16) drop slightly below the generally increasing trend?arrow_forwardWhich element would have the most favorable favorable (most negative) electron affinity? Ga, Ca, Se, or Br Which equation below illustrates the first electron affinity for silicon? Si⁺ (g) → Si⁺²(g) + e⁻, Si⁺² (g) + 2e⁻ → Si (g), Si (g) + e⁻ → Si⁻ (g), Si (g) → Si⁺ (g) + e⁻, Si (g) → Si⁺² (g) + 2e⁻, or Si (g) + 2e⁻ → Si⁻² (g)arrow_forwardWhich of the following does have the highest ionization energy? ? Z of Mg =12, K =19, Na = 11, Cl = 17arrow_forward
- Which element would have the most favorable (most negative) electron affinity? B, C, N, or O Which equation below illustrates the first electron affinity for phosphorus? P (g) + 2e⁻ → P⁻² (g), P (g) → P⁺² (g) + 2e⁻, P (g) + e⁻ → P⁻ (g), P⁺ (g) → P⁺²(g) + e⁻, P (g) → P⁺ (g) + e⁻, or P⁺² (g) + 2e⁻ → P (g)arrow_forwardThe electron affinity of the lutetium atom (element 71) was measured using the technique of photoelectron spectroscopy with an infrared laser (the essay on p. 310 describes this instrumental method, using X rays). In this experiment, a beam of lutetium negative ions, Lu, was prepared and irradiated with a laser beam having a wavelength at 1064 nm. The energy supplied by a photon in this laser beam removes an electron from a negative ion, leaving the neutral atom. The energy needed to remove the electron from the negative ion to give the neutral atom (both in their ground states) is the electron affinity of lutetium. Any excess energy of the photon shows up as kinetic energy of the emitted electron. If the emitted electron in this experiment has a kinetic energy of 0.825 eV, what is the electron affinity of lutetium?arrow_forward
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