CHM 143 Lecture Notes - Lecture 22: Ionic Radius, Lewis Structure, Lattice Energy

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17 Nov 2016

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Ex nacl total= +147 kj ie na = +496 kj. Na (s) + cl 2 (g) nacl (s) release energy. The energy comes from the formation of salt = +/- attraction. To determine why then need to look at overall process of salt formation starting with elements in standard states. Must include: h vap = gets elements into gas state. 2. ie= if need to remove electrons (2nd ie if need to remove 2 electrons etc. )(determined for elements in gas state: ea if gaining electron (determined for elements in gas state, bond energy= if need to separate into single atom from, lattice energy= formation ionic compound from ions in gas state. Lower energy= lower stability a: h f o = for overall formation of salt from elements in standard states. Lattice energy = the energy released from the formation of a solid ionic compound from the individual ions in the gas state.

Related Questions

1)The NaCl2 ionic salt does not exist. Which of the followingstatements best explains why?

A. Because the formation of Na2+ is an unfavorable process due tothe great amount of energy required to remove the 2nd electron fromthe Na atom (the 2nd electron would have to be removed from thecore electrons of the Na atom).
B. Because the Cl- anion is too large for there to be two of themattached to one Na+ ion.
C. Because NaCl2 is actually a polyatomic ion with a -1 charge, andnot an ionic salt. In the presence of another Na+ ion, the Na2Cl2salt would form.
D. Because Cl2 has no charge and therefore would not be attractedelectrostatically to the positively charged Na2+ cation.

2)Select the false statement below.

A. The first ionization energy of an atom is smaller than thesecond ionization energy of the same atom.
B. Phosphorus has a greater first ionization energy than magnesium,and the reason for this is because P has a greater effectivenuclear charge (Zeff) than Mg.
C. The following process is an endothermic process and representsthe first ionization energy of an atom A:A(g) ? A1+(g) + e1-
D. Fluorine has a greater first ionization energy than iodine, andthe reason for this is because fluorine has a greater amount ofshielding of outer electrons by inner electrons than doesiodine.

3)The Group 5A elements N,P,As have lower (less negative) electronaffinities than most of the Group 4A or Group 6A elements becauseN,P,As have half-filled subshells.

True
False

4)A fluorine atom is smaller than a bromine atom, and a potassiumatom is larger than a lithium atom.

True
False

5)A certain main-group element exhibits the following successiveionization energies in kJ/mol:

IE1 = 100; IE2 = 1200; IE3 = 2300; IE4 = 3100; IE5 = 4200

Select the false statement about this element below.

A. This is likely a Group 1A element.
B. This element is typically found uncombined in nature (that is,it is not usually found in compounds, but rather as a freeelement).
C. If this element is given a symbol of "J", it would form an ioniccompound with sulfur as J2S.
D. If this element was in period 2 of the periodic table, it wouldbe lithium.

6)Select the false statement below.

A. Generally speaking, non-metallic elements have greater effectivenuclear charge (Zeff) than metallic elements in the sameperiod.
B. Generally speaking, as you go down a group in the periodictable, there is successively greater shielding of the outer-shellelectrons by the inner-shell electrons.
C. Generally speaking, the heavier alkali metals can be predictedto exhibit greater shielding of the outer-shell electrons by theinner-shell electrons than lighter alkali metals.
D. Generally speaking, as you go across a period in the periodictable, the effective nuclear charge (Zeff) decreases because eachsuccessive element contains more protons in the nucleus than theprevious element and the outer electrons are all in the same shellas you go across a period.

7)Place the following in order of increasing size:

O2-, F1-, Li1+

A. F1- < Li1+ < O2-
B. Li1+ < O2- < F1-
C. Li1+ < F1- < O2-
D. F1- < O2- < Li1+

8)Select the false statement below.

A. The following set of quantum numbers is allowed:
n = 4, l = 2, ml = -2, ms = +1/2
B. The n = 1 shell of any given atom can accomodate up to 2electrons.
C. The n = 4 shell of any given atom can accomodate up to 16electrons.
D. In any given atom, the l = 2 subshell can accomodate up to 5electrons that have negative spins (ms =

redgoldfish403

Practice problems for exam 2 ______________

Useful Information:

h=6.626Ã10-34JÂ·s.; c=3.0Ã108 m/sec; E=hï® ; E= hc , ï¬ = h/mv; 1J = 1 kg-m2/s2 ï¬

mass of electron = 9.11 Ã 10-28 g, ïE= q + w ; 1 cal = 4.184 Joules Please Show all Work

1. Which of the following substances have standard heats of formation that are equal to zero by definition (circle your answers): H2(g), H(g), O3(g), H2O(s), H2O(l), Hg(l), Hg(s), Hg(g).

2. Limestone stalactites are formed in the reaction: Ca2+(aq) + HCO3-(aq) ï CaCO3(s) + CO2(g) +

H2O(l)
If one mole of CaCO3 is produced at 298 K under one atmosphere of pressure, the reaction performs 590 calories of expansion work, pushing back the atmosphere as CO2 is formed. At the same time, 9310 calories of heat are absorbed from the environment. What is ïE in Kcal/mole for CaCO3.

3. What is the minimum wavelength of light in AÌ (1 AÌ = 10-8 cm) needed to provide enough energy per quantum to rupture the chemical bond in hydrogen iodide (HI). The bond dissociation energy of HI is 71.4 Kcal/mole.

4. Sketch the shape and orientation of the following types of orbitals: s, px, dxy, dz2, dx2-y2

5. Give the values of (n) , (l) and (ml) for each orbital in the 4p subshell.

6. Write the complete electron configuration for the following: Ti 2+_____________________________________ Cr_______________________________________

N______________________________________

7. Calculate the standard enthalpy of formation ( ï Ho) for diamond from graphite [i.e. C (graphite) ï C (diamond)] given that:

C (graphite) + O2 ï CO2 (g) ( ï Ho = -393.5 KJ/mole) C (diamond)] + O2 ï CO2 (g) ( ï Ho = -395.4 KJ/mole)

If 1.0g of graphite is converted to diamond, what is the energy change? Is this an endothermic or exothermic reaction?

8. An 160 pound astronaut on his way to Mars is buzzing along at 10,000 miles per hour. (a) Express his weight in grams (one pound = 454 grams) so that you can calculate the astronautâs wavelength (1mile/hour = 44.7 cm/sec)

(b) Suppose the astronaut detects outside his spacecraft a proton (m=1.7 x 10-24 g) from a âsolar windâ moving at exactly the spacecraft velocity. What is the proton wavelength is in AÌ (1 AÌ = 10-8 cm.

9. What is the maximum number of electrons that can occupy each of the following subshells? a) 3d_________________ b) 1s____________________ c) 2p ____________________

10. Identify the element represented by the following electronic configuration.

a) [Ne] 3s2____________________

b) What is the electron configuration for the first excited state of this atom.______________

11. Determine the number of valence electrons for each element.
(a) Br___________ (b) Na _________ (c) Sn __________

12. 175 g of Fe at 15.0oC is mixed with 225 g of H2O at 95.0oC. What is the final temperature of the mixture? The specific heats of iron= 0.448 J/g oC and water = 4.184 J/g oC). (keep in mind the following: heat gained + heat lost = 0 and q=mass x heat capacity x ïT)

13. (5 pts) Calculate values of ÎHrxn for the following reactions: CS2(g) + 3O2(g) ï® CO2(g) + 2SO2(g)

The heat of formation for the following substances is given in kJ/mol:

CS2 CO2 SO2 117.4 -393.51 -296.83

14. (6 pts) Use the electron configuration of Li and Be and determine which element has the greatest second ionization energy. Defend your answer.

15. Mark beside each of the following processes either âexoâ or âendoâ according to whether you think the process will release heat or absorb heat.

a. Ca(g) ï Ca(g)+2 + 2e-
b. I(g)+1e-ï I(g)-1
c. Ca(g)+2 + S(g)-2 ï CaS(s) d. I2(g)ï 2I(g)

( ) ( ) ( ) ( )

16. (6 pts) In each of the following pairs, which of the two species is larger?
a) O-2 or Na+ b) Ti+4 or Ti+2 c) B or C d) N or N-3

17. Write down the Lewis dot structure for the following (a) N_______________ (b) Ne________________

18. THE BORN HABER CYCLE: I may have a problem on the Born Haber cycle. Please check my lecture notes to see how to set up the process and then calculate the lattice energy from the various thermodynamic quantities such as in the NaCl example below;

ï H ï¯ f NaCl = -411KJ

Na(s) ï® Na(g) ï H =108KJ
1â2 Cl2 ï® Cl(g) ï H = 122KJ Ionization Energy of Na ï H = 496 KJ Electron affinity of Cl ï H = -349KJ

How do you answer 1-4?

Physical Constants R-00821 L.atm rnol. K: 1 atm = 760 Torr; h-6626 x 10". Js; c-3.00 x 10e mis Multiple Choice Question-4 points each. Circle the correct choice. 1. How many orbitals are there in the n - 3 shell? )3 b)6 )9 d) 12 e) none of the preceding choices 2. Which of the following is not a valid set of four quantum numbers to describe an electron in an atom? 3. Which pair of elements would you expect to exhibit the most similar physical and chemical properties? a) As and Se b) Na and Cl c) As and Sb d) B and Be 4) The number of unpaired electrons in the ground state of an atom of Co is.. (A) one (B) three (C) five (D) seven (E) none of the preceding choices S. Which of the following processes is exothermic? a) lonization of a sodium atom b) Formation of gaseous chlorine atoms from Cl, (g) c) Breaking apart of NaC1 (s) into ions d)Addition of an electron to a chlorine atom 6. Which of the following bonds is the most polar? a) N-O b)O-F e) B-O d)S-o e) all are equally polar At what temperature (in C) will 25.0 g of carbon dioxide (at 1,00 atm) occupy 21.5 L? 188Â°C b) 461Â°C c) -263Â°C d)-270Â°C e)113Â°C How many times more rapidly will hydrogen (H2) gas effuse through a pinhole than will deuterium (D ) gas? Deuterium is an isotope of hydrogen with a molecular mass of 4.0 g/mole. (A) V2 (B) 2 (C)2v2 (D) 4 9. Which of the following arrangements from lowest to highest in first ionization energies is correct ? 10. In which of the following compounds obeys the octet rule? 1. The bright spectral lines observed in the emission spectrum of a flame or gas discharge tube are due to a) XeF b) BF, c) Cio d) so e) none of the preceding choicees a) the absorption of light at specific wavelengths b) the formation of an excited state of atoms c) the transition of an atom from an excited state to a lower energy state d) the change from anti-parallel to parallel electron spins in an atom 2. A one-liter container is filled with one mole of hydrogen at 25 Â°C. A second one-liter container is filled with one mole f oxygen at 25 Â°C. Comparing the pressure of the hydrogen to the oxygen, the ratio will be Fro n Bond Dissociation Enthalpies: AHD (CI-CI)-243 kJrnolAMD (F-F )ä¸159 klinol; lculate the enthalpy, AH, for the chemical reaction: Cl: (g)+F: (g) 2CIF(R) )-147 kJ (b)-108 kJ (c)+171 kJ (d) +912 k AHD (CI F)-255 kJ mol ;

CHM 143 Lecture Notes - Lecture 22: Ionic Radius, Lewis Structure, Lattice Energy

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