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CHEM 14A Chapter Notes - Chapter 2A.2-3: Lattice Energy, Joule, Sodium Chloride

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18 Nov 2020

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Chemistry and Biochemistry

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Dr.Laurence Lavelle

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Document Summary

Many of the basic ideas about the chemical bond were proposed by g. n. He represented each valence electron as a dot and arranged the dots around the symbol of the element. The lewis symbol is a visual is a visual summary of the valence-shell electron configuration of an atom or ion. To work out the formula of an ionic compound using lewis symbol. Represent the cation by removing the appropriate number of dots from the symbol for the atom of the metallic element. Represent the anion by transferring those dots to the lewis symbol for the atom of the nonmetallic elements to complete it valence shell. If necessary, adjust the numbers of atoms of each kind so that all the dots removed front he atom of the metallic element are accommodated by the atom of the nonmetallic element. Write the charge of each ion as a superscript.

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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 =

1.
Which of the following is true of a cation?
A) it has equal numbers of protons and electrons
B) it has fewer protons than electrons
C) it has more protons than electrons
D) the relationship between protons and electrons depends on thespecific cation
2.
Which is most likely true for an atom with six valenceelectrons?
A) it will gain one electron
B) it will gain two electrons
C) it will lose one electron
D) it will lose two electrons
3.
Which is most likely true for an atom with one valenceelectron?
A) it will gain one electron
B) it will gain two electrons
C) it will lose one electron
D) it will lose two electrons
4.
Which of the following atoms is least likely to form an ion?
A) fluorine
B) magnesium
C) silicon
D) sodium
5.
For which of the following atoms do we not try to apply the octetrule?
A) oxygen
B) nickel
C) sodium
D) xenon
6.
Which of the following is likely to form an ion with the largestpositive charge?
A) potassium
B) calcium
C) aluminum
D) silicon
7.
Which of the following is likely to form an ion with the mostnegative charge?
A) aluminum
B) sulfur
C) chlorine
D) argon
8.
Which of the following ions has the same electronic configurationas neon?
A) Mg2+
B) F -
C) both (a) and (b)
D) neither (a) nor (b)
9.
What is the name of the species formed when a sodium atom loses anelectron?
A) sodate
B) sodide
C) sodium
D) sodium ion
10.
What is the name of the species formed when a bromine atom gains anelectron?
A) bromate
B) bromide
C) bromine
D) bromine ion
11.
Which of the following endings is generally associated with amonatomic anion?
A) ...ade
B) ...ate
C) ...ic
D) ...ide
12.
If the name of an ion ends in "ate" what type of ion is it mostlikely to be?
A) a monatomic anion
B) a monatomic cation
C) a polyatomic anion
D) a polyatomic cation
13.
The preferred name for HSO4- is hydrogen sulfate. What is thecommon name for this ion?
A) bisulfate
B) disulfate
C) bisulfide
D) disulfide
14.
Which pair of species is most likely to form an ionic bond?
A) two electrically neutral species
B) two electrically charged species, one positive and onenegative
C) two negatively charged species
D) two positively charged species
15.
Which of the following situations is most likely to result information of a covalent bond?
A) when an electrically positive species interacts with anelectrically negative species
B) when two nonmetallic elements interact to form a compound
C) when two electrically negative species interact
D) when two electrically positive species interact
16.
Which of the following statements is generally true aboutelectronegativity?
A) electronegativity decreases as we move left to right anddecreases as we move top to bottom
B) electronegativity decreases as we move left to right andincreases as we move top to bottom
C) electronegativity increases as we move left to right anddecreases as we move top to bottom
D) electronegativity increases as we move left to right andincreases as we move top to bottom
17.
For which of the following pairs are the atoms most likely to forman ionic bond with each other?
A) carbon and oxygen
B) calcium and chlorine
C) chlorine and oxygen
D) sodium and magnesium
18.
What is the formula of the compound formed by magnesium andiodine?
A) MgI
B) MgI2
C) MgI3
D) Mg2I
19.
What is the formula of the compound formed between the ammonium ionand the carbonate ion?
A) NH4CO3
B) NH4(CO3)2
C) (NH4)2CO3
D) (NH4)3CO3
20.
What is the formula of the compound formed between the magnesiumion and the acetate ion?
A) MgC2H3O2
B) Mg2C2H3O2
C) Mg(C2H3O2)2
D) Mg(C2H3O2)3
21.
What is the correct name for KI?
A) monopotassium monoiodide
B) potassium iodine
C) potassium iodide
D) potassium ion iodine ion
22.
A compound used to treat manic depressives has the formula Li2CO3.Which of the following is the correct name for this compound?
A) dilithium carbonate
B) lithium carbon trioxide
C) lithium carbonate
D) lithium carboxide
23.
Which of the following bonds is the most polar?
A) H__F
B) H__Cl
C) H__Br
D) H__I
24.
How many electrons are associated with a double bond?
A) 1
B) 2
C) 4
D) 6
25.
How many bonds does a carbon atom typically form?
A) 2
B) 4
C) 6
D) 8
26.
Laughing gas, sometimes called nitrous oxide, has the formula N2O.What is the proper chemical name for nitrous oxide?
A) nitrogen oxide
B) nitrogen dioxide
C) dinitrogen oxide
D) dinitrogen oxygen
27.
Which of the following is the correct formula for dinitrogenpentoxide?
A) O2N5
B) O5N2
C) N2O5
D) N5O2
28.
What is the proper chemical name for water?
A) dihydrogen oxide
B) dihydrogen oxygen
C) hydrogen oxide
D) hydrogen oxygen
29.
To use the VSEPR model to determine the geometry of a molecule weneed to know which of the following?
A) the number of atoms in the molecule
B) the number of atoms bonded to the central atom
C) the number of lone pairs around the central atom
D) both (b) and (c)
30.
What bond angle is most closely associated with a tetrahedraldistribution of electron density?
A) 90o
B) 109.5o
C) 120o
D) 180o
31.
What bond angle is most closely associated with a trigonal planardistribution of electron density?
A) 90o
B) 109.5o
C) 120o
D) 180o
32.
What bond angle is most closely associated with a lineardistribution of electron density?
A) 90o
B) 109.5o
C) 120o
D) 180o
33.
Which of the following molecules is best described as having anearly tetrahedral distribution of electron density?
A) BeCl2
B) OF2
C) SnCl2
D) none of these
34.
In which of the following molecules does the carbon atom have alinear distribution of electron density?
A) C2H2
B) C2H4
C) C2H6
D) none of these
35.
Which of the following is true for the molecule O=C=S?
A) it is nonpolar because it contains only double bonds
B) it is polar because the polarities of the O=C and C=S do notcancel
C) it is polar because it has a bent shape
D) it is nonpolar because it is linear