Practice Exam 5 Spring 2024

The following ionic solids have measured distances between their cations and anions. (1 Angstrom, a common unit of measure at the atomic level, is 10-10 m.) LiF: 2.01 Angstroms NaCl: 2.83 Angstroms KBr: 3.30 Angstroms Rbl: 3.67 Angstroms Which compound would you predict has the highest lattice energy? O NaCl O LiF Rbl O KBr Save Answer

N Calculate the lattice enthalpy for RbCl. You will need the following information: Species A,H, kJ/mol Rb(e) RbCl() CI(g) Enthalpy of ionization for Rb(g) is 403.0 kl/mol; electron attachment enthalpy for Cl(g) is-349.0 kJ/mol Lattice enthalpy kJ/mol Submit Answer *** 1 43 E D 80.9 -435.4 121.3 Try Another Version 80 54 R F di a 25 2 item attempts remaining T G ‹6 P FA Y & 29 7 H 8 #7 U 8 Dil FA - 6 8 K

Fur 三 O Advanced Material Predicting the relative lattice energy of binary ionic compounds In each row, pick the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? CsCl CsI LiF tab Na, O Explanatn X Esc ~ RbF O MgO Check Type here to search x ! 1 F1 Q J F2 @ 2 W 10 F3 #m 3 Ox E F4 $ 4 F5 % R 5 0: DELL F6 A 10 T 20. 6 F

An ionic substance of formula MX has a lattice energy of6 * 103 kJ>mol. Is the charge on the ion M likely to be1+, 2+, or 3+? Explain.

Use the following table to rank the compounds in order of decreasing (strongest to weakest) lattice energy. Cation Anion Bond length (pm) M2+ A2– 204 M2+ B2– 192 M+ C– 215   Group of answer choices MA  >  MB  >  MC  MC  >  MB  >  MA MB  >  MA  >  MC MB  >  MC  >  MA

lattice 2.0

The lattice energy of NaBr is –752 kJ/mol. This energy corresponds to which reaction below?     Na(s) + 1/2 Br2(g) → NaBr(s) Na(g) + Br(g) → NaBr(s) Na(g) + Br(g) → NaBr(s) Na+(g) + Br–(g) → NaBr(s) Na+(aq) + Br–(aq) → NaBr(s)

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Elements with only longer bonds (Enter your answer in accordance with the question statement): Now from the answer to the first part, pick the elements with stronger bonds only (do not include if not listed)

Which one of the following trends appears when considering lattice energies? Anion A) The higher the charge on the ions, the higher the lattice energy. Cation F- CI- Br- |- O2- B) The more ions present in an ionic compound, the smaller the lattice energy. Lit 1036 853 807 757 2925 Na+ 923 787 747 704 2695 C) The larger the distance between ions in the ionic compound, the higher the lattice energy. K+ 821 715 682 649 2360 Mg2+ 2957 2524 2440 2327 3791 D) In general, alkali metals have larger lattice energies than alkaline earth metals with the same anions. Ca2+ 2630 2258 2176 2074 3401 Al3+ 5215 5492 5361 5217 15,916

Predicting the relative lattice energy of binary ionic compounds In each row, pick the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? MgS Be S O ΚΙ O SrO O Explanation Cal₂ O SrF₂ Esc Check Type here to search 2 ! 1 F1 F2 @ NO 2 81 Z F3 # 3 Ox F4 $ 4 F5 % 01 4s DELL F6 A T

In each row, pick the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? SrF 2 CaF2 O Be Br2 O K₂S X LiBr K₂0

In each row, pick the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? k₂s K₂0 O LiBr C₁₂ X Be Br₂ aCl₂ S

need help with the lattice energy

Predicting the relative lattice energy of binary ionic compounds In each row, pick the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? ΚΙ Cal₂ RbF CsBr X Rb₂ O CsCl 3/5

Which statement below is not correct? O The lattice energy depends on the sizes and charges of the ions present. Olonic bonding is favored over other types when atoms with small ionization energies combine with atoms that have large exothermic electron affinities. O The attraction of positive and negative ions leads to an ionic bond between two ions. The lattice energy of NaCl is the energy released when 1 mole of this ionic compound forms from Na(s) and Cl2(g).

The lattice energies of rubidium fluoride (RbF) and caesium chloride (CsCl) are -760kJmol^-1 and -650kJmol^-1 respectively. What is the lattice energy of caesium fluoride (CsF) likely to be? (Atomic number Rb 37; Cs 55)

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Chemistry just a brief answer, thanks.