CHE 106 Lecture Notes - Lecture 19: Bond-Dissociation Energy, Bond Energy, Formal Charge

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CHE 106 Full Course Notes

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The following rules let you write electron dot formulas even when the central atom doesn"t follow the octet rule. For a polyatomic cation, subtract the number of positive charges from this total. Step 2 : arrange elements with the element that is least electronegative in the center. Place electrons between the central element and the surrounding elements. On the periodic table, electronegativity increases from left to right across a row. The structure of ozone, o3, can be represented by two different lewis structures. According to theory, one pair of bonding electrons is spread over the region of all. Delocalized bonding : electron pairs are shared over multiple elements. ** need. Resonance description : you describe the electron structure of molecules with delocalized bonding by drawing all of these possible electron dot formulas. Sometimes, more than one feasible lewis structure can be drawn for a molecule. Formal charge : determined by subtracting the domain electrons from the group electrons.

Related Questions

STRC 454 riring Lewis Symibols and Lewis Senacesres Write the Lewis structure for the ionic com . Construct the Lewis structure modet for the cova pound potassium chloride in the box lent compound sulfur aifluoride (SF,) using the follow ing steps 1) The number of valence electrons in the sulfur The total number of valence electrons . Hence, the total Lewis structure of potassium chloride in the two fluonine atoms is number of valence clectrons in SF, is (5) tow does the written Lewis structure for po. ã tassum chlor de difor from that of hydrogen chionde? (2) Arrange the atormic cores for the two fluonine atoms with the suifur atom as the central atom in the space below. 13) Rewnibe the atomic cores in the space below Place an electron pair between each fluorine and sultfur 4, Construct the Lewis sructure model for the cova- ent compound hydrogen sulide (4,S) using the tol distributing the remaining valence electrons so that all owing steps (4) Write the Lewis structure for SF2 in the box, three atoms are in accordance with the octet rulo. (1) two hydrogen atoms is The total number of valonce electrons in the ; the sulfur aom has Hence, the total number of valence electrons in the compound is Leis sructure of SF2 (2) Write the atomic cores for the hydrogen atoms and the sultur below. 6. Construct the Lewis structure model for the cova atom in the space Because sulfur is the central atom in this moleculeÂ·ar. range the cores so that the hydrogen atoms are on e- lent compound methylene chioride (CHC17). (1) The number of valence electrons in the car- The total number of valence elec- trons in the two hydrogen atoms is The total 3) Rewnte the atomic cores in the space below number of valence electrons in the two chiorine atoms Henoe, the total number of valence elec- ther side of the suifur atom bon atomis Place an electron pair betwoon each hydragen atom is and the sultr atom _ trons in CH,C, is (2) Postion the atomic core for carbon as the (4) Write the Lewis structure for hydrogen sultide central atom in the space below, and place the ather in the box, distmbuting the remainingvaience electrons cores around it so that the hydrogen atoms are in accordance wth the duet rule and the sultur atom is in accordance with the actet rule (3) Rewrite your arrangement ot atomic cores in the space below, joiring the cores with electron pairs to form the necessary bonds Lewis structure of HS

4. (20 pts, 2 pts each) Multiple choice questions from chapter 7.Place the letter representing the
correct response in the blank provided.
_____ Which of the following do not exist under normal conditionsas a diatomic gas?
(A) hydrogen, (B) oxygen, (C) fluorine, (D) chlorine, (E)bromine
_____ In nature, the noble gases exist as
(A) monatomic gaseous atoms, (B) the gaseous fluorides, (C) solidsin minerals,
(D) alkali metal salts, (E) the sulfides
_____ Of the elements below, _____ has the highest electronaffinity.
(A) oxygen, (B) sodium, (C) fluorine, (D) hydrogen, (E)chlorine
_____ Of the following elements, which has the largest firstionization energy?
(A) Se, (B) As, (C) S, (D) Sb, (E) Ge
_____ Of the hydrogen halides, only _____ is a weak acid.
(A) HCl (aq), (B) HBr (aq), (C) HF (aq), (D) HI (aq), (E) all ofthem
_____ The carbonate of which alkali metal is used in treatment ofmanic-depressive illness?
(A) Li, (B) Na, (C) K, (D) Rb, (E) Cs
_____ The reaction of a metal with a nonmetal produces a(n)
(A) base, (B) salt, (C) acid, (D) oxide, (E) hydroxide
_____ Which element is solid at room temperature?
(A) Cl2, (B) F2, (C) Br2, (D) I2, (E) H2
_____ Which of the following correctly lists the five atoms inorder of increasing size (smallest to
largest)?_(A) F < K < Ge < Br < Rb, (B) F < Ge <Br < K < Rb,
(C) F < K < Br < Ge < Rb, (D) F < Br < Ge < K< Rb, (E) F < Br < Ge < Rb < K
_____ Which one of the following is a metalloid?
(A) Ge, (B) S, (C) Br, (D) Pb, (E) C
5. (20 pts, 2 pts each) Multiple choice questions from chapter 8.Place the letter representing the
correct response in the blank provided.
_____ Which of the following ions does not have a noble-gasconfiguration?
(A) V5+ (B) Si4+ (C) Nb3+ (D) S2â (E) Os8+
_____ Which of the following is correctly arranged with respect tothe size of the atom/ion?
(A) S < S1â < S2â (B) Mg2+ < Na+ < Ne (C) Ni < Cu+< Zn2+
_____ What type of covalent bond between like atoms is thelongest?
(A) triple (B) double (C) single (D) They are all the samelength.
_____ Arrange the following in order of increasing bond polarity:C-O, P-O, Cu-O, Mn-O
(A) C-O < P-O < Cu-O < Mn-O (B) C-O < P-O < Mn-O< Cu-O
(C) Mn-O < Cu-O < P-O < C-O (D) P-O < C-O < Cu-O< Mn-O
_____ Write a single Lewis structure that obeys the octet rule, andcalculate the formal charges on
all the atoms in PO4
3â.
(A) P 2+, O 1â (B) P 1+, O 1â (C) P 4+, O 2â (D) P 2+, O 2â (E) P1+, O 2â
_____ The Lewis structure of InBr3 contains how many valenceelectrons?
(A) 24 (B) 7 (C) 6 (D) 3 (E) 34
_____ Using Lewis structures that satisfy the octet rule, determinethe number of bonds formed by
the central element in each of the following: SiO4
4â, PO4
3â, SO4
2â, ClO4
1â.
(A) 4, 5, 6, 7 (B) 2, 3.5, 5, 6.5 (C) 4, 5, 5, 6 (D) 4, 4, 4, 4 (E)5, 6, 7, 8
_____ The Lewis electron-dot structure of IF5 gives the centralI
(A) an octet (B) 5 nonbonding pairs and 1 bonding pair (C) 5bonding pairs only
(D) 1 nonbonding pairs and 5 bonding pairs (E) 1 nonbonding pairand 4 bonding pairs
_____ In the thiocyanate anion, (SCN)â, which of the following isnot an accepted multiplicity for
the sulfur-carbon bond and the carbon-nitrogen bond,respectively?
(A) single, single (B) double, double (C) single, triple (D)triple, single
_____ Which of these ions (oxidation states) does not have anoble-gas configuration?
(A) Cr3+ (B) Cr with an oxidation state of 6+ (as in CrO4
2â)
(C) S with an oxidation state of 6+ (as in SO4
2â) (D) S2â (E) Hf 4+

CHE 106 Lecture Notes - Lecture 19: Bond-Dissociation Energy, Bond Energy, Formal Charge

CHE 106 Full Course Notes

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