(a)
Interpretation: the given compounds are needed to be placed to the given conditions by using Arkel diagram.
Concept introduction:
In Arkel diagram,
- Down-left portion shows metallic compounds.
- Down-right portion shows covalent compounds.
- Down-mid (in between metallic and covalent) shows semiconducting compounds.
- Top shows ionic compounds.
(b)
Interpretation: the given compounds are needed to be placed to the given conditions by using Arkel diagram.
Concept introduction:
In Arkel diagram,
- Down-left portion shows metallic compounds.
- Down-right portion shows covalent compounds.
- Down-mid (in between metallic and covalent) shows semiconducting compounds.
- Top shows ionic compounds.
(c)
Interpretation: the given compounds are needed to be placed to the given conditions by using Arkel diagram.
Concept introduction:
In Arkel diagram,
- Down-left portion shows metallic compounds.
- Down-right portion shows covalent compounds.
- Down-mid (in between metallic and covalent) shows semiconducting compounds.
- Top shows ionic compounds.
(d)
Interpretation: the given compounds are needed to be placed to the given conditions by using Arkel diagram.
Concept introduction:
In Arkel diagram,
- Down-left portion shows metallic compounds.
- Down-right portion shows covalent compounds.
- Down-mid (in between metallic and covalent) shows semiconducting compounds.
- Top shows ionic compounds.
(e)
Interpretation: the given compounds are needed to be placed to the given conditions by using Arkel diagram.
Concept introduction:
In Arkel diagram,
- Down-left portion shows metallic compounds.
- Down-right portion shows covalent compounds.
- Down-mid (in between metallic and covalent) shows semiconducting compounds.
- Top shows ionic compounds.
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Chemistry & Chemical Reactivity
- 1) Using principles of chemical bonding and/or intermolecular forces, explain each of the following. (a) Xenon has a higher boiling point than neon has. (b) Solid copper is an excellent conductor of electricity, but solid copper chloride is not. (c) SiO2 melts at a very high temperature, while CO2 is a gas at room temperature, even though Si and C are in the same chemical family. (d) Molecules of NF3 are polar, but those of BF3 are not. 2) Using principles of chemical bonding and/or intermolecular forces, explain each of the following: (a) MgCl2 and SiCl4 (b) MgCl2 and MgF2 (c) F2 and Br2 (d) F2 and N2 Note: Please Briefly Explainarrow_forwardWhich member of each pair is less metallic?(a) I or O(b) Be or Ba(c) Se or Gearrow_forwardConsider the element silicon, Si. (a) Write its electron configuration.(b) How many valence electrons does a siliconatom have? (c) Which subshells hold the valenceelectrons?arrow_forward
- (b) Shown below are two schematic band diagrams for silicon. Answer the following questions: (i) For phosphorous-doped silicon, draw a dashed line denoting the location of the additional state(s) created by the phosphorus at room temperature. Explain your answer. (ii) For phosphorous-doped silicon, draw a dashed line denoting the location of electrons donated by the phosphorus at room temperature. Explain your answer. Conduction Conduction band band Band Band дар gap Valence Valence band band (i) (ii)arrow_forwardWhich compound in each of the following pairs has the larger lattice energy? Note: Ba2+ and K+ have similar radii; S2– and Cl– have similar radii. Explain your choices.(a) K2O or Na2O(b) K2S or BaS(c) KCl or BaS(d) BaS or BaCl2arrow_forwardThe energy for the following reaction was measured to be -653.0 kJ/mol. K(g) + Cl(g) →→KCI(s). Using this fact and the data in the table below, calculate the enthalpy (in kJ/mol) required to separate the ions from the lattice for this reaction: KCI(s) → K+(g) + Cl-(g). Substance K (g) CI (g) Ionization Energies (kJ/mol) 418.8 1251.1 Electron Affinities (kJ/mol) -48.384 -349arrow_forward
- NaCl and KF have the same crystal structure. The only differencebetween the two is the distance that separates cationsand anions. (a) The lattice energies of NaCl and KF are givenin Table 8.1. Based on the lattice energies, would you expectthe Na¬Cl or the K¬F distance to be longer? (b) Use theionic radii given in Figure 7.8 to estimate the Na¬Cl andK¬F distances.arrow_forwardFor many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains 77.55% Xe and 22.45% F by mass.(a) What is the formula of the compound?(b) Write a Lewis structure for the compound.(c) Predict the shape of the molecules of the compound.(d) What hybridization is consistent with the shape you predicted?arrow_forwardThe attractive force between a pair of Sr2+ and O2- ions is 1.52 x 108 N and the ionic radius of O2- ions is 0.134 nm. Calculate the ionic radius of the Sr2+ ion. (Given: Electron charge, e = 1.6 x 101ºC, the permittivity of free space, Eo = 8.85 x 101ºC²N'm²)arrow_forward
- Which of the following compounds requires the most energy to convert one mole of the solid into separate ions?(a) K2S(b) K2O(c) CaS(d) Cs2S(e) CaOarrow_forwardMixing SbCl3 and GaCl3 in a 1:1 molar ratio using liquid sulfur dioxide as a solvent gives a solidionic compound with the empirical formula GaSbCl6. A controversy arose over whether this compoundis [SbCl2]+[GaCl4]− or [GaCl2]+[SbCl4]−.(a) Predict the molecular structure of the two anions from the two choices using VSEPR theory.(b) It is learned that the cation in the compound has a bent structure. Based on this fact, whichformulation is the correct one?arrow_forwardConsider the lattice energies of the following Group 2Acompounds: BeH2, 3205 kJ/mol; MgH2, 2791 kJ/mol;CaH2, 2410 kJ/mol; SrH2, 2250 kJ/mol; BaH2, 2121 kJ/mol.(a) What is the oxidation number of H in these compounds?(b) Assuming that all of these compounds have the samethree-dimensional arrangement of ions in the solid, whichof these compounds has the shortest cation–anion distance?(c) Consider BeH2. Does it require 3205 kJ of energyto break one mole of the solid into its ions, or does breakingup one mole of solid into its ions release 3205 kJ of energy?(d) The lattice energy of ZnH2 is 2870 kJ/mol. Consideringthe trend in lattice enthalpies in the Group 2A compounds,predict which Group 2A element is most similar in ionic radiusto the Zn2+ ion.arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning