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Name________________________________________& Discussion&Section_____________& Chapter&1&–&Covalent&Bonding&and&Shapes&of&Molecules& 1.24&Judging'from'their'relative'positions'in'the'Periodic'Table,'which'atom'in'each'set'is'more' electronegative?' ' ' (a)'Carbon'or'nitrogen' (b)'Chlorine'or'bromine' (c)&Oxygen'or'sulfur' ' & & & & 1.25'Which'compounds'have'nonpolar'covalent'bonds,'which'have'polar'covalent'bonds,'and' which'are'ionic?' ' ' (a)&LiF' ' (b)'CH3F' (c)&MgCl2' (d)'HCl' ' ' ' 1.26'Using&the&symbols&d-'and'd+,'indicate'the'direction'of'polarity,'if'any'in'each'covalent' bond.' ' ' (a)&C–Cl' (b)'S–H'' (c)&C–S'' (d)'P–H' ' ' ' 1.28'Write'Lewis'structures'for'these'ions.'Show'all'valence'electrons'and'all'formal'charges.' ' (b)'Bicarbonate'ion,'HCO3–' ' (c)'Carbonate'ion,'CO32–' (a)&Amide'ion,'NH2–' ' ' ' ' ' ' ' ' ' (e)'Formation'ion,'HCOO–' ' (f)'acetate'ion,'CH3COO–' ' (d)&Nitrate'ion,'NO3–' ' ' ' ' ' ' ' '

1.32'Following'are'several'Lewis'structures'showing'all'valence'electrons.'Assign'all'formal' charges'in'each'structure'as'appropriate.' '

H

H

O

C

C

H

(a)' ' '

H

O

C

H

H

H

O

C

C

C

H '

H

'

(b)'

H

N

C

O

C

H

H

H

H

C

C

C

H

H '

'

C

C

H

H

(c)'

'

H

H

H

C

O

H

H H H H H H H (d)' ' ' (e)' ' ' (f)' ' ' 1.49'Draw'a'three-dimensional'representation'for'each'molecule.'Indicate'which'ones'have'a' dipole'moment'and'in'what'direction'the'dipole'moment'points.' ' (a)&CH3F' ' (b)''CH2Cl2' ' (c)''CH2ClBr' ' (d)'CFCl3' ''''''''''''(e)''CCl4' ' ' ' ' ' ' ' (f)&CH2=CCl2' ' (g)'CH2=CHCl' ' (h)'HCºC-CºCH' (i)'CH3CºN' ' ' ' ' ' ' ' (j)&(CH3)2C=O' ' (k)&BrCH=CHBr'(two'answers' ' ' ' ' ' ' ' '

1.51'Which'statements'are'true'about'resonance'contributing'structures?' ' (a)''All'contributing'structures'must'have'the'same'number'of'valence'electrons.'T&/&F& & (b)&&All'contributing'structures'must'have'the'same'arrangement'of'atoms.''T&/&F& & (c)'''All'atoms'in'a'contributing'structure'must'have'complete'valence'shells.'T&/&F& & (d)&'All'bond'angles'in'sets'of'contributing'structures'must'be'the'same.'T&/&F& & 1.56'State'the'orbital'hybridization'(on'the'space'provided)'of'each'highlighted'atom.' H

H

H C

C

H

H

(a)&

H

H

H C

_____&

C

(b)& H

H &_____&

H C

&

C

H

(c)'

_____& H

H O

C

H C

O

(d)& H

_____&

&

(e)&

H

C

H

O

N

O

H

C

C

H

O

H

&_____&

(f)&

O

H

H

_____&

H H C

N

H

H C

C

CH

H2 C

C

CH2

2 H H (g)& &_____& (h)&& _____& (i)& 2 &_____& ' 1.57&Describe'each'highlighted'bond'in'terms'of'the'overlap'of'atomic'orbitals' '

H

H C

(a)' H ' ' ' ' ' ' ' '

C H

& &

&

(b)'

&

&

(c)'

&

1.75''' (a)&&Draw'a'Lewis'structure'for'the'ozone'molecule,'O3.'(The'order'of'atom'attachment'is'' O–O–O,'and'they'do'not'form'a'ring.)'Chemists'use'ozone'to'cleave'carbon-carbon''''' double'bonds'(Section'6.5C)' ' ' ' ' ' ' ' ' ' (b)&'Draw'four'contributing'resonance'structures;'including'formal'charges' & & & & & & & (c)'''How'does'the'resonance'model'account'for'the'fact'that'the'length'of'each'O–O'bond' in'ozone'(128'pm)'is'shorter'than'the'O–O'single'bond'in'hydrogen'peroxide'(HOOH,'147' pm)'but'longer'than'the'O–O'double'bond'in'the'dioxygen'(123'pm)?'...