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chemistry principles and practice
Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions
In each of the following pairs of bonds, which bond is more polar? Show the direction of the dipole moment for the more polar bond.(a) H–C or H–N(b) O–C or Cl–N(c) S–O or S–FStrategyUse the table of electronegativities in Figure 9.9 to determine the electronegativity difference. The
Write the Lewis structure of acetone, CH3C(O)CH3. The skeleton structure is Η Ο Η Ο ||| H=C=C=C-H H Η
Which bond is more polar: P–S or Sb–S?
Given that the lattice energy of an ionic solid increases with the charges of the anion and cation, discuss why the formula of NaF is not NaF2.
Write the Lewis structure of CH3CN.
Write the Lewis structure of CH2CCH2.
Explain why(a) The lattice energy of LiCl is greater than that of LiBr.(b) The lattice energy of Na2O is greater than that of NaF.
Write the Lewis structure of ethylene, CH2CH2.StrategyWrite the skeleton structure, sum the valence electrons, take into account the number of bonds in the skeleton structure, and determine whether the structure can be finished by lone pairs. If there are fewer electrons than needed, add one bond
Explain why(a) The lattice energy of NaI is greater than that of KI.(b) The lattice energy of MgCl2 is greater than that of NaCl.
Write the Lewis structure of BF4-.StrategyWrite the skeleton structure, sum the valence electrons, take into account the number of bonds in the skeleton structure, and determine whether the structure can be finished by lone pairs. For this polyatomic ion, one electron is added to the valence
What main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.
Write the Lewis structure of dimethyl ether, CH3OCH3.
Explain why the lattice energy of Na2O is considerably greater than that of NaF.StrategyLattice energies are evaluated by using the relationshipIn general, the changes that can take place with the Q terms are more important than small changes in r. E = kQ1 Q₂ r
Explain why the lattice energy of Na2O is considerably greater than that of NaF.StrategyLattice energies are evaluated by using the relationshipIn general, the changes that can take place with the Q terms are more important than small changes in r. E = kQ1 Q₂ r
Explain why the lattice energy of Na2O is considerably greater than that of NaF.StrategyLattice energies are evaluated by using the relationshipIn general, the changes that can take place with the Q terms are more important than small changes in r. E = kQ1 Q₂ r
Use Lewis electron-dot symbols to show the electron transfer during the formation of each compound from the appropriate atoms.(a) Beryllium oxide(b) Yttrium chloride
Explain why the lattice energy of KCl is greater than that of KI.
Use Lewis electron-dot symbols to show the formation of(a) Magnesium oxide(b) Calcium fluoride from the atoms.StrategyMove the valence electrons from the metal to the nonmetal, placing eight around each nonmetal, and indicate the charges as superscripts.
Use Lewis electron-dot symbols to show the electron transfer during the formation of each compound from the appropriate atoms.(a) Barium bromide(b) Potassium sulfide
Use Lewis electron-dot symbols to show the formation of lithium sulfide from the atoms.
Write the Lewis electron-dot symbol for(a) Fluorine atom(b) Be2+ ion(c) Br- ionStrategyDetermine the number of valence electrons and arrange them sequentially around the four sides of the element symbol. For ions, add or subtract valence electrons consistent with the charge and add the
What is a Lewis electron-dot symbol?
What are the Lewis electron-dot symbols for a tin atom and the Sn2+ ion?
(a) A 10.76-g sample of impure CsF was dissolved in 100 mL water. Th e sample was mixed with excess aqueous calcium nitrate solution to precipitate insoluble calcium fluoride. Th e precipitate was filtered, dried, and weighed. A total of 2.35 g calcium fluoride was collected. What was the
What is the mass percent of a transition metal, M, in a compound of the formula MCl3 if the electron configuration of the metal cation in this compound is 1s22s22p63s23p63d5?
Write an equation for the reaction with water of a metal that, in its ground state, has one electron in a 3s orbital. What mass of water is needed to react with 2.34 g of this metal?
Identify which member of Group 5A has the following characteristics:(a) Largest size(b) Smallest ionization energy
What is the trend in reactivity as you go down from F to I in the periodic table? Give a reason for this trend.
Which element in the second period has the largest atomic radius? Why?
Identify the block of the periodic table where each of the following elements is.(a) Tl(b) Be(c) Xe(d) U
Write the electron configurations of the following elements after finding their locations in the periodic table.(a) B(b) Bi(c) Ba(d) Cd
Describe the physical properties of the elements in Group 7A.
Describe the physical properties of the elements in Group 2A.
Describe the physical properties of the elements in Group 1A.
Predict which species has the greater first ionization energy: Al or Si.
List the elements O, S, and Al in order of increasing size.
Find the following elements in the periodic table, identify which block they are in, and give their electron configurations by using the structure of the periodic table rather than consulting Table 7.3.(a) Br(b) TiTable 7.3 TABLE 7.3 Ground-State Electron Configurations of the
Use the aufbau procedure to obtain the electron configuration and orbital diagram for atoms of the following elements.(a) Be(b) B(c) Ne(d) Rb
In the photoelectric effect, the energy of the absorbed photon is equal to the sum of the energy for the threshold frequency of the metal and the kinetic energy of the ejected electron. When light with a wavelength of 400 nm strikes potassium metal, the ejected electrons have a kinetic energy of
Write the electron configuration and orbital diagram for an atom of a gaseous diatomic element that has a density of 1.14 g/L at 27 °C and 1.00 atm pressure.
What masses of iron and Cl2 are needed to prepare 7.88 g of the metal halide product if, under the conditions of the reaction, the electron confi guration of the iron cation in the product is 1s22s22p63s23p63d 6?
Given the following two equations, where the metals (M and M') are from the second period, what are the metals, and which metal cation in the product has a larger radius? 2M + F₂ → 2MF M' + F₂ → M'F₂
Write the electron confi guration of the alkali metal (M) that reacts with oxygen to yield an oxide, M2O, if 1.22 g of the metal reacts with 1.41 g of oxygen to form 2.63 g of the oxide.
Chlorine gas can be prepared by passing electricity through a solution of NaCl. What volume of chlorine at standard temperature and pressure can be prepared from 2.44 g NaCl?
Write the electron configuration and orbital diagram for the noble gas that has a density of 1.62 g/L at 27 °C and 1.00 atm pressure.
Arrange the elements lithium, carbon, and oxygen in order of(a) Increasing size.(b) Increasing first ionization energy.(c) Increasing second ionization energy.(d) Number of unpaired electrons.
Rank the following ions in order of increasing sizes and increasing ionization energies: S2-, K+, Ca2+.
Which of the cations Ga4+ and Mn4+ is not a stable species? Why?
The mineral magnetite has the overall formula Fe3O4 (as Fe2O3 · FeO) and contains both Fe2+ and Fe3+. Write the electron configurations of both cations of iron.
Of the following electron configurations:(1) 1s22s22p1(2) 1s22s22p4(3) 1s22s22p5 which represents the element with the(a) Largest size?(b) Smallest ionization energy?(c) Greatest electron affinity?
Determine the number of unpaired electrons for a Cr4+ cation.
List the element for which the 2+ cation has the electron configuration [Ar]3d4.
Palladium, with an electron configuration of [Kr]4d10, is an exception to the aufbau principle. Write the electron configuration of the 2+ cation of palladium. Does the fact that palladium is an exception influence the electron configuration of Pd2+? tabe 3209.5% 90 99.95
Write the electron configuration of the copper atom and the 2+ cation of copper. Remember that the electron configuration of copper atom is unusual. Does the fact that copper is an exception to the aufbau principle influence the electron configuration of Cu2+?
Three elements have the electron configurations 1s22s22p63s2, [Ar]4s2, and 1s22s22p63s23p5. The atomic radii of these elements (not necessarily in the same order) are 99, 160, and 231 pm. Identify the elements from the electron confi gurations, and match the sizes with these elements.
Write the electron configuration for the 2+ cation of calcium.
One sphere below represents a boron atom, while the other sphere represents an oxygen atom. Select the one that represents the boron atom. Explain your choice. (D) (b)
Write the electron configuration for the 3+ cation of titanium.
What are the changes in(a) Size,(b) Ionization energy, and(c) Electron affinity from potassium to calcium?
The presence of radioactive strontium in nuclear fallout (which is residue from atmospheric testing of nuclear bomb testing) is a major health concern because of strontium’s periodic table relationship with calcium, a necessary nutrient. What is the reason for this concern?
One way to generate hydrogen gas in the laboratory is to combine a reactive metal with water. The ensuing chemical reaction produces hydrogen gas as one product. Which element would generate hydrogen gas more vigorously when combined with water: potassium or calcium? Explain your answer. Write the
What is the trend in reactivity as you go down from Li to Cs in the periodic table? Give a reason for this trend.
Write the equation for the reaction, if any, of calcium with the following substances.(a) Oxygen(b) Water
Write the equation for the reaction, if any, of barium with the following substances.(a) Oxygen(b) Water
Write the equation for the reaction, if any, of lithium with the following substances.(a) Oxygen(b) Nitrogen(c) Chlorine(d) Water
Write the equation for the reaction, if any, of sodium with the following substances.(a) Oxygen(b) Nitrogen(c) Chlorine(d) Water
Indicate which species in each pair has the more favorable (more negative) electron affinity. Explain your answer.(a) Br or Te(b) O or B(c) In or Se
Indicate which species in each pair has the more favorable (more negative) electron affinity. Explain your answer.(a) O or F(b) P or Cl(c) Se or Br
Indicate which species in each pair has the more favorable (more negative) electron affinity. Explain your answer.(a) Se or Br(b) S or P(c) Br or As
Indicate which species in each pair has the more negative electron affinity. Explain your answer.(a) S or Cl(b) N or O(c) S or F
On which ionization (first, second, third, fourth, etc.) will the ionization energy of an Al atom increase dramatically? Explain why.
What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.
Suggest a reason for the lack of metal cations with a 4+ charge.
Li2+ is not a common charge for a lithium ion. Use the ionization energies of lithium to explain why.
Which second ionization energy is greater, that of oxygen or that of fluorine? Explain your answer.
Predict which of these elements would have the greatest difference between the first and second ionization energies: Si, Na, P, Mg. Briefly explain your answer.
Which third ionization energy is greater, that of aluminum or that of magnesium? Explain your answer.
Which second ionization energy is greater, that of aluminum or that of magnesium? Explain your answer.
Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.(a) K, Se, S(b) Cr, As, O(c) O, O-, F
Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.(a) N, N3-, Ne(b) P, Si, Cl(c) Ga, O, Se
Using only a periodic table as a guide, arrange each of the following series of species in order of increasing fi rst ionization energy.(a) S, Se2-, O(b) Fe, Br, F(c) Cl, Cl-, F
Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.(a) O, O2-, F(b) C, Si, N(c) Te, Ru, Sr
Indicate which species in each pair has the higher ionization energy. Explain your answer.(a) K or I(b) Al or Al+(c) Cl- or Ar
Indicate which species in each pair has the higher ionization energy. Explain your answer.(a) Ge or Cl(b) B or F(c) Al3+ or Na+
Indicate which species in each pair has the higher ionization energy. Explain your answer.(a) N or F(b) Mg2+ or Na+(c) K or Si
Indicate which species in each pair has the higher first ionization energy. Explain your answer.(a) Si or Cl(b) Na or Rb(c) O2-or F-
Of the atoms with the electron configurations 1s22s22p4 and 1s22s22p2, which is smaller?
Of the atoms with the electron configurations 1s22s22p63s23p5 and 1s22s22p63s23p3, which is larger?
Which is larger, Na+ or F-? For each of these ions, draw a representation of the shape of the highest energy occupied orbital.
Using only a periodic table as a guide, arrange each of the following series of species in order of increasing size.(a) F, F-, O2-(b) Al3+, Mg, Na(c) N, P, Si
Using only a periodic table as a guide, arrange each of the following series of species in order of increasing size.(a) Li, Be2+, Be(b) S, S2-, Cl(c) O, S, Si
Using the abbreviated notation, write the ground-state electron configuration of the following ions.(a) Y3+(b) Br-(c) Rh2+
Using only a periodic table as a guide, arrange each of the following series of atoms in order of increasing size.(a) B, O, Li(b) C, N, Si(c) S, As, Sn
Which species in each of the following pairs is larger? Explain your answer.(a) Li or Na(b) O or P(c) Rb or Rb+
Which species in each of the following pairs is larger? Explain your answer.(a) Na or Mg(b) B or O(c) Be2+ or Be3+
Select the atom or ion in each pair that has the smaller radius.(a) Cs or Rb(b) O2- or O(c) Br or As
Which species in each of the following pairs is larger? Explain your answer.(a) Na or Na+(b) O2- or F-(c) Ni2+ or Ni3+
Which of the following species are not isoelectronic with the rest: F-, Ne, Na+, Ca2+?
Which of the following species are not isoelectronic with the rest: Ar, K+, Ca2+, Y3+?
What neutral atoms are isoelectronic with the following ions?(a) Pb4+(b) Br-(c) S2-(d) Ni3+
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