?List these elements in order of decreasing electronegativity: Rb, Si, Cl, Ca, Ga

Why are bonding theories important? Cite some examples of what bonding theories can predict.

Write the electron configurations for Ne and Ar. How many valence electrons does each element have?

In the Lewis model, what is an octet? What is a duet? What is a chemical bond?

What is the difference between ionic bonding and covalent bonding?

How can the Lewis model be used to determine the formula of ionic compounds? You may explain this with an example.

What is the difference between lone pair and bonding pair electrons?

How are double and triple bonds physically different from single bonds?

What is the procedure for writing a covalent Lewis structure?

How do you determine the number of electrons that go into the Lewis structure of a molecule?

How do you determine the number of electrons that go into the Lewis structure of a polyatomic ion?

Why does the octet rule have exceptions? List some examples.

What are resonance structures? Why are they necessary?

Explain how VSEPR theory predicts the shapes of molecules.

If all of the electron groups around a central atom are bonding groups (that is, there are no lone pairs), what is the molecular geometry for: (a) two electron groups (b) three electron groups (c) four electron groups

Give the bond angles for each of the geometries in the preceding question.

What is the difference between electron geometry and molecular geometry in VSEPR theory?

What is electronegativity?

What is the most electronegative element on the periodic table?

What is a polar covalent bond?

What is a dipole moment?

What happens if you try to mix a polar liquid with a nonpolar one?

If a molecule has polar bonds, is the molecule itself polar? Why or why not?

Write an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure. (a) N (b) C (c) Cl (d) Ar

Write an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure. (a) Li (b) P (c) F (d) Ne

Write the Lewis structure for each element. (a) I (b) S (c) Ge (d) Ca

Write the Lewis structure for each element. (a) Kr (b) P (c) B (d) Na

Write a generic Lewis structure for the halogens. Do the halogens tend to gain or lose electrons in chemical reactions? How many?

Write a generic Lewis structure for the alkali metals. Do the alkali metals tend to gain or lose electrons in chemical reactions? How many?

Write a generic Lewis structure for the alkaline earth metals. Do the alkaline earth metals tend to gain or lose electrons in chemical reactions? How many?

Write a generic Lewis structure for the elements in the oxygen family (Group 6A). Do the elements in the oxygen family tend to gain or lose electrons in chemical reactions? How many?

Write the Lewis structure for each ion. (a) \(\mathrm{Al}^{3+}\) (b) \(\mathrm{Mg}^{2+}\) (c) \(\mathrm{Se}^{2-}\) (d) \(\mathrm{N}^{3-}\) Text Transcription: Al^3+ Mg^2+ Se^2- N^3-

Write the Lewis structure for each ion. (a) \(\mathrm{Sr}^{2+}\) (b) \(\mathrm{S}^{2-}\) (c) \(\mathrm{Li}^{+}\) (d) \(\mathrm{Cl}^{-}\) Text Transcription: Sr^2+ S^2- Li^+ Cl^-

Indicate the noble gas that has the same Lewis structure as each ion. (a) \(\mathrm{Br}^{-}\) (b) \(\mathrm{O}^{2-}\) (c) \(\mathrm{Rb}^{+}\) (d) \(\mathrm{Ba}^{2+}\) Text Transcription: Br^- O2^- Rb^+ Ba2^+

Indicate the noble gas that has the same Lewis structure as each ion. (a) \(\mathrm{Se}^{2-}\) (b) \(\mathrm{l}^{-}\) (c) \(\mathrm{Sr}^{2+}\) (d) \(\mathrm{F}^{-}\) Text Transcription: Se^2- I^- Sr^2+ F^-

Is each compound best represented by an ionic or a covalent Lewis structure? (a) \(\mathrm{SF}_{6}\) (b) \(\mathrm{MgCl}_{2}\) (c) BrCl (d) \(\mathrm{K}_{2}S\) Text Transcription: SF_6 MgCl_2 K_2S

Is each compound best represented by an ionic or a covalent Lewis structure? (a) NO (b) \(\mathrm{CO}_{2}\) (c) \(\mathrm{Rb}_{2}O\) (d) \(\mathrm{Al}_{2} \mathrm{S}_{3}) Text Transcription: CO_2 Rb_2O Al_2S_3

Write the Lewis structure for each ionic compound. (a) NaF (b) CaO (c) \(\mathrm{SrBr}_{2}\) (d) \(\mathrm{K}_{2} \mathrm{S}\) Text Transcription: SrBr_2 K_2O

Write the Lewis structure for each ionic compound. (a) SrO (b) \(\mathrm{Li}_{2} \mathrm{S}\) (c) \(\mathrm{CaI}_{2}\) (d) RbF Text Transcription: Li_2S CaI_2

Use the Lewis model to determine the formula for the compound that forms from each pair of atoms. (a) Ca and S (b) Mg and Br (c) Cs and I (d) Ca and N

Use the Lewis model to determine the formula for the compound that forms from each pair of atoms. (a) Al and S (b) Na and S (c) Sr and Se (d) Ba and F

Draw the Lewis structure for the ionic compound that forms from Mg and each atom. (a) F (b) O (c) N

Draw the Lewis structure for the ionic compound that forms from Al and each atom. (a) F (b) O (c) N

Determine what is wrong with each ionic Lewis structure and write the correct structure.

Determine what is wrong with each ionic Lewis structure and write the correct structure.

Use the Lewis model to explain why each element exists as a diatomic molecule. (a) hydrogen (b) iodine (c) nitrogen (d) oxygen

Use the Lewis model to explain why the compound that forms between hydrogen and sulfur has the formula H2S. Would you expect HS to be stable? \(\mathrm{H}_{3} \mathrm{S}\)? Text Transcription: H_3S?

Write the Lewis structure for each molecule. (a) \(\mathrm{PH}_{3}\) (b) \(\mathrm{SCI}_{2}\) (c) \(\mathrm{F}_{2}\) (d) HI Text Transcription: PH_3 SCl_2 F_2

Write the Lewis structure for each molecule. (a) \(\mathrm{CH}_{4}\) (b) \(\mathrm{NF}_{3}\) (c) \(\mathrm{OF}_{2}\) (d) \(\mathrm{H}_{2} \mathrm{O}\) Text Transcription: CH_4 NF_3 OF_2 H_2O

Write the Lewis structure for each molecule. (a) \(\mathrm{O}_{2}\) (b) CO (c) HONO (N is central; H bonded to one of the O atoms) (d) \(\mathrm{SO}_{2}\) Text Transcription: O_2 SO_2

Write the Lewis structure for each molecule. (a) \(\mathrm{N}_{2} \mathrm{O}\) (oxygen is terminal) (b) \(\mathrm{SiH}_{4}\) (c) \(\mathrm{CI}_{4}\) (d) \(\mathrm{Cl}_{2} \mathrm{CO}\) (carbon is central) Text Transcription: N_2O SiH_4 CI_4 Cl_2CO

Write the Lewis structure for each molecule. (a) \(\mathrm{C}_{2} \mathrm{H}_{2}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{4}\) (c) \(\mathrm{N}_{2} \mathrm{H}_{2}\) (d) \(\mathrm{N}_{2} \mathrm{H}_{4}\) Text Transcription: C_2H_2 C_2H_4 N_2H_2 N_2H_4

Write the Lewis structure for each molecule. (a) \(\mathrm{H}_{2} \mathrm{CO}\) (carbon is central) (b) \(\mathrm{H}_{3} \mathrm{COH}\) (carbon and oxygen are both central) (c) \(\mathrm{H}_{3} \mathrm{COCH}_{3}\) (oxygen is between the two carbon atoms) (d) \(\mathrm{H}_{2} \mathrm{O}_{2}\) Text Transcription: H_2CO H_3COH H_3COCH_3 H_2O_2

Determine what is wrong with each Lewis structure and write the correct structure.

Determine what is wrong with each Lewis structure and write the correct structure.

Write the Lewis structure for each molecule or ion. Include resonance structures if necessary. (a) \(\mathrm{SeO}_{2}\) (b) \(\mathrm{CO}_{3}^{2-}\) (c) ClO- (d) \(\mathrm{ClO}_{2}^{-}\) Text Transcription: SeO_2 CO_3^2- ClO_2

Write the Lewis structure for each molecule or ion. Include resonance structures if necessary. (a) \(\mathrm{ClO}_{3}^{-}\) (b) \(\mathrm{ClO}_{4}^{-}\) (c) \(\mathrm{NO}_{3}^{-}\) (d) \(\mathrm{SO}_{3}\) Text Transcription: ClO_3^- ClO_4^- NO3- SO3

Write the Lewis structure for each ion. Include resonance structures if necessary. (a) \(\mathrm{PO}_{4}^{3-}\) (b) \(\mathrm{CN}^{-}\) (c) \(\mathrm{NO}_{2}^{-}\) (d) \(\mathrm{SO}_{3}{ }^{2-}\) Text Transcription: PO_4^3- CN^- NO-2^- SO_3^2-

Write the Lewis structure for each ion. Include resonance structures if necessary. (a) \(\mathrm{SO}_{4}{ }^{2-}\) (b) \(\mathrm{HSO}_{4}^{-}) (S is central; H is attached to one of the O atoms) (c) \(\mathrm{NH}_{4}^{+}\) (d) \(\mathrm{BrO}_{2}^{-}\) (Br is central) Text Transcription: SO_4^2- SO_4^- NH_4^+ BrO_2^-

Write the Lewis structure for each molecule. These molecules do not follow the octet rule. (a) \(\mathrm{BCl}_{3}\) (b) \(\mathrm{NO}_{2}\) (c) \(\mathrm{BH}_{3}\) Text Transcription: BCl_3 NO_2 BH_3

Write the Lewis structure for each molecule. These molecules do not follow the octet rule. (a) \(\mathrm{BBr}_{3}\) (b) NO Text Transcription: BBr_3

Determine the number of electron groups around the central atom for each molecule. (a) \(\mathrm{OF}_{2}\) (b) \(\mathrm{NF}_{3}\) (c) \(\mathrm{CS}_{2}\) (d) \(\mathrm{CH}_{4}\) Text Transcription: OF_2 NF_3 CS_2 CH_4

Determine the number of electron groups around the central atom for each molecule. (a) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (b) \(\mathrm{CH}_{2} \mathrm{SBr}_{2}\) (c) \(\mathrm{H}_{2} \mathrm{S}\) (d) \(\mathrm{PCI}_{3}\) Text Transcription: CH-2Cl_2 SBr_2 H_2S PCl_3

Determine the number of bonding groups and the number of lone pairs for each of the molecules in Problem 61. The sum of these should equal your answers to Problem 61.

Determine the number of bonding groups and the number of lone pairs for each of the molecules in Problem 62. The sum of these should equal your answers to Problem 62.

Determine the molecular geometry of each molecule. (a) \(\mathrm{CBr}_{4}\) (b) \(\mathrm{H}_{2} \mathrm{CO}\) (c) \(\mathrm{CS}_{2}\) (d) \(\mathrm{BH}_{3}\) Text Transcription: CBr_4 H_2CO CS_2 BH_3

Determine the molecular geometry of each molecule. (a) \(\mathrm{SiO}_{2}\) (b) \(\mathrm{BF}_{3}\) (c) \(\mathrm{CFCl}_{3}\)x (carbon is central) (d) \(\mathrm{H}_{2} \mathrm{CS}\) (carbon is central) Text Transcription: SiO_2 BF_3 BF_3 H_2CS

Determine the bond angles for each molecule in Problem 65.

Determine the bond angles for each molecule in Problem 66.

Determine the electron and molecular geometries of each molecule. (a) \(\mathrm{N}_{2} \mathrm{O}\) (oxygen is terminal) (b) \(\mathrm{SO}_{2}\) (c) \(\mathrm{H}_{2} \mathrm{S}\) (d) \(\mathrm{PF}_{3}\) Text Transcription: N_2O SO_2 H_2S PF_3

Determine the electron and molecular geometries of each molecule. (Hint: Determine the geometry around each of the two central atoms.) (a) \(\mathrm{C}_{2} \mathrm{H}_{2}\) (skeletal structure HCCH) (b) \(\mathrm{C}_{2} \mathrm{H}_{4}\) (skeletal structure \(\mathrm{H}_{2} \mathrm{CCH}_{2}\)) (c) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (skeletal structure \(\(\mathrm{H}_{3} \mathrm{CCH}_{3}\) Text Transcription: C_2H_2 C_2H_4 H_2CCH_2 C_2H_6 H_3CCH_3

Determine the bond angles for each molecule in Problem 69.

Determine the bond angles for each molecule in Problem 70.

Determine the electron and molecular geometries of each molecule. For molecules with two central atoms, indicate the geometry about each central atom. (a) \(\mathrm{N}_{2}\) (b) \(\mathrm{N}_{2} \mathrm{H}_{2}\) (skeletal structure HNNH) (c) \(\mathrm{N}_{2} \mathrm{H}_{4}\ (skeletal structure \(\mathrm{H}_{2} \mathrm{NNH}_{2}\) Text Transcription: N_2 N_2H_2 N_2H_4 H_2NNH_2

Determine the electron and molecular geometries of each molecule. For molecules with more than one central atom, indicate the geometry about each central atom. (a) \(\mathrm{CH}_{3} \mathrm{OH}\) (skeletal structure \(\mathrm{H}_{3} \mathrm{COH}\) (b) \(\mathrm{H}_{3} \mathrm{COCH}_{3}\) (skeletal structure \(\mathrm{H}_{3} \mathrm{COCH}_{3}\) (c) \(\mathrm{H}_{2} \mathrm{O}_{2}\) (skeletal structure HOOH) Text Transcription: CH_3OH H_3COH H_3COCH_3 H_2O_2

Determine the molecular geometry of each polyatomic ion. (a) \(\mathrm{CO}_{3}{ }^{2-}\) (b) \(\mathrm{ClO}_{2}^{-}\) (c) \(\mathrm{NO}_{3}{ }^{-}\) (d) \(\mathrm{NH}_{4}^{+}\) Text Transcription: CO3^2- ClO_2^- NO_3^- NH_4^+

Determine the molecular geometry of each polyatomic ion. (a) \(\mathrm{ClO}_{4}^{-}\) (b) \(\mathrm{BrO}_{2}^{-}\) (c) \(\mathrm{NO}_{2}^{-}\) (d) \(\mathrm{SO}_{4}{ }^{2-}\) Text Transcription: ClO_4^- BrO_2^- NO_2^- SO_4^2-

Refer to Figure 10.2 to determine the electronegativity of each element. (a) Mg (b) Si (c) Br

Refer to Figure 10.2 to determine the electronegativity of each element. (a) F (b) C (c) S

List these elements in order of decreasing electronegativity: Rb, Si, Cl, Ca, Ga.

List these elements in order of increasing electronegativity: Ba, N, F, Si, Cs.

Refer to Figure 10.2 to find the electronegativity difference between each pair of elements; then refer to Table 10.2 to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (a) Mg and Br (b) Cr and F (c) Br and Br (d) Si and O

Refer to Figure 10.2 to find the electronegativity difference between each pair of elements; then refer to Table 10.2 to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (a) K and Cl (b) N and N (c) C and S (d) C and Cl

Arrange these diatomic molecules in order of increasing bond polarity: ICl, HBr, \(\mathrm{H}_{2}\), CO. Text Transcription: H_2

Arrange these diatomic molecules in order of decreasing bond polarity: HCl, NO, \(\mathrm{F}_{2}\), HI. Text Transcription: F2

Classify each diatomic molecule as polar or nonpolar. (a) CO (b) \(\mathrm{O}_{2}\) (c) \(\mathrm{F_{2}\) (d) HBr Text Transcription: O_2 F_2

Classify each diatomic molecule as polar or nonpolar. (a) \(\mathrm{I}_{2}\) (b) NO (c) HCl (d) \(\mathrm{N}_{2}\) Text Transcription: I_2 N_2

For each polar molecule in Problem 85 draw the molecule and indicate the positive and negative ends of the dipole moment.

For each polar molecule in Problem 86 draw the molecule and indicate the positive and negative ends of the dipole moment.

Classify each molecule as polar or nonpolar. (a) \(\mathrm{CS}_{2}\) (b) \(\mathrm{SO}_{2}\) (c) \(\mathrm{CH}_{4}\) (d) \(\mathrm{CH}_{3} \mathrm{Cl}\) Text Transcription: CS_2 SO_2 CH_4 CH_3Cl

Classify each molecule as polar or nonpolar. (a) \(\mathrm{H}_{2} \mathrm{CO}\) (b) \(\mathrm{CH}_{3} \mathrm{OH}\) (c) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (d) \(\mathrm{CO}_{2}\) Text Transcription: H_2CO CH_3OH CH_2Cl_2 CO_2

Classify each molecule as polar or nonpolar. (a) \(\mathrm{BH}_{3}\) (b) \(\mathrm{CHCl}_{3}\) (c) \(\mathrm{C}_{2} \mathrm{H}_{2}\) (d) \(\mathrm{NH}_{3}\) Text Transcription: BH_3 CHCl_3 C_2H_2 NH_3

Classify each molecule as polar or nonpolar. (a) \(\mathrm{N}_{2} \mathrm{H}_{2}\) (b) \(\mathrm{H}_{2} \mathrm{O}_{2}\) (c) \(\mathrm{CF}_{4}\) (d) \(\mathrm{NO}_{2}\) Text Transcription: N_2H_2 H_2O_2 CF_4 NO_2

Write electron configurations and Lewis structures for each element. Indicate which of the electrons in the electron configuration are shown in the Lewis structure. (a) Ca (b) Ga (c) As (d) I

Write electron configurations and Lewis structures for each element. Indicate which of the electrons in the electron configuration are shown in the Lewis structure. (a) Rb (b) Ge (c) Kr (d) Se

Determine whether each compound is ionic or covalent and write the appropriate Lewis structure. (a) \(\mathrm{K}_{2} \mathrm{S}\) (b) CHFO (carbon is central) (c) MgSe (d) \(\mathrm{PBr}_{3}\) Text Transcription: K_2S PBr_3

Determine whether each compound is ionic or covalent and write the appropriate Lewis structure. (a) HCN (b) ClF (c) \(\mathrm{MgI}_{2}\) (d) CaS Text Transcription: MgI_2

Write the Lewis structure for \(\mathrm{OCCl}_{2}\) (carbon is central) and determine whether the molecule is polar. Draw the three-dimensional structure of the molecule. Text Transcription: OCCl_2

Write the Lewis structure for \(\mathrm{CH}_{3} \mathrm{COH}\) and determine whether the molecule is polar. Draw the three-dimensional structure of the molecule. The skeletal structure is: Text Transcription: CH_3COH

Write the Lewis structure for acetic acid (a component of vinegar) \(\mathrm{CH}_{3} \mathrm{COOH}_{2}\), and draw the three-dimensional sketch of the molecule. Its skeletal structure is: Text Transcription: CH_3COOH

Write the Lewis structure for benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}\), and draw a three-dimensional sketch of the molecule. The skeletal structure is the ring shown here. (Hint: The Lewis structure consists of two resonance structures.) Text Transcription: C_6H_6

Consider the neutralization reaction. \(\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaCl}(a q)\) Write the reaction showing the Lewis structures of each of the reactants and products. Text Transcription: HCl(aq) + NaOH(aq) ¡ H2O(l) + NaCl(aq)

Consider the precipitation reaction. \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{LiCl}(a q) \longrightarrow \mathrm{PbCl}_{2}(s)+2 \mathrm{LiNO}_{3}(a q)\) Write the reaction showing the Lewis structures of each of the reactants and products. Text Transcription: Pb(NO3)2(aq) + 2 LiCl(aq) ¡ PbCl2(s) + 2 LiNO3(aq)

Consider the redox reaction. \(2 \mathrm{K}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{KCl}(s)\) Draw the Lewis structure for each reactant and product and determine which reactant was oxidized and which one was reduced. Text Transcription: 2 K(s) + Cl2( g) ¡ 2 KCl(s)

Consider the redox reaction. \(\mathrm{Ca}(s)+\mathrm{Br}_{2}(g) \longrightarrow \mathrm{CaBr}_{2}(s)\) Draw the Lewis structure for each reactant and product and determine which reactant was oxidized and which one was reduced. Text Transcription: Ca(s) + Br2( g) ¡ CaBr2(s)

Each compound listed contains both ionic and covalent bonds. Write the ionic Lewis structure for each one including the covalent structure for the polyatomic ion. Write resonance structures if necessary. (a) KOH (b) \(\mathrm{KNO}_{3}\) (c) LiIO (d) \(\mathrm{BaCO}_{3}\) Text Transcription: KNO_3 BaCO_3

Each of the compounds listed contains both ionic and covalent bonds. Write an ionic Lewis structure for each one, including the covalent structure for the polyatomic ion. Write resonance structures if necessary. (a) \(\mathrm{RbIO}_{2}\) (b) \(\mathrm{Ca}(\mathrm{OH})_{2}\) (c) \(\mathrm{NH}_{4} \mathrm{Cl}\) (d) \(\mathrm{Sr}(\mathrm{CN})_{2}\) Text Transcription: RbIO_2 Ca(OH)_ NH_4Cl Sr(CN)_2

Each molecule listed contains an expanded octet (10 or 12 electrons) around the central atom. Write the Lewis structure for each molecule. (a) \(\mathrm{PF}_{5}\) (b) \(\mathrm{SF}_{4}\) (c) \(\mathrm{SeF}_{4}\) Text Transcription: PF_5 SF_4 SeF_4

Each molecule listed contains an expanded octet (10 or 12 electrons) around the central atom. Write the Lewis structure for each molecule. (a) \(\mathrm{ClF}_{5}\) (b) \(\mathrm{SF}_{6}\) (c) \(\mathrm{lF}_{5}\) Text Transcription: ClF_5 SF_6 IF_5

Formic acid is responsible for the sting you feel when stung by fire ants. By mass, formic acid is 26.10% C, 4.38% H, and 69.52% O. The molar mass of formic acid is 46.02 g/mol. Find the molecular formula of formic acid and draw its Lewis structure.

Diazomethane has the following composition by mass: 28.57% C, 4.80% H, and 66.64% N. The molar mass of diazomethane is 42.04 g/mol. Find the molecular formula of diazomethane and draw its Lewis structure.

Free radicals are molecules that contain an odd number of valence electrons and therefore contain an unpaired electron in their Lewis structure. Write the best possible Lewis structure for the free radical HOO. Does the Lewis model predict that HOO is stable? Predict its geometry.

Free radicals (as explained in the previous problem) are molecules that contain an odd number of valence electrons. Write the best possible Lewis structure for the free radical \(\mathrm{CH}_{3}\). Predict its geometry. Text Transcription: CH_3

Some theories on aging suggest that free radicals cause a variety of diseases and aging. Free radicals (as explained in Problems 111 and 112) are molecules or ions containing an unpaired electron. As you know from the Lewis model, such molecules are not chemically stable and quickly react with other molecules. Free radicals may attack molecules within the cell, such as DNA, changing them and causing cancer or other diseases. Free radicals may also attack molecules on the surfaces of cells, making them appear foreign to the body’s immune system. The immune system then attacks the cell and destroys it, weakening the body. Draw the Lewis structure for each of these free radicals, which have been implicated in theories of aging. (a) \(\mathrm{O}_{2}^{-}\) (b) \(\mathrm{O}^{-}\) (c) OH (d) \(\mathrm{CH}_{3} \mathrm{OO}\) (unpaired electron on terminal oxygen) Text Transcription: O_2^- O^- CH_3OO

Free radicals (see Problem 113) are important in many environmentally significant reactions. For example, photochemical smog, which forms as a result of the action of sunlight on air pollutants, is formed in part by these two steps: \(\begin{array}{l} \mathrm{NO}_{2} \stackrel{\text { UV light }}{\longrightarrow} \mathrm{NO}+\mathrm{O} \\ \mathrm{O}+\mathrm{O}_{2} \longrightarrow \mathrm{O}_{3} \end{array} \) The product of this reaction, ozone, is a pollutant in the lower atmosphere. Ozone is an eye and lung irritant and also accelerates the weathering of rubber products. Write Lewis structures for each of the reactants and products in the preceding reactions. Text Transcription: NO2 NO + O O + O2 O3 UV light

Examine the formulas and space-filling models of the molecules shown here. Determine whether the structure is correct. If the structure is incorrect, sketch the correct structure.

Draw the Lewis dot structure for the atoms Al and O. Use the Lewis model to determine the formula for the compound these atoms form.

Draft a list of step-by-step instructions for writing a correct Lewis dot structure for any molecule or polyatomic ion.

For each of the following molecules: \(\begin{array}{llll} \mathrm{CS}_{2} & \mathrm{NCl}_{3} & \mathrm{CF}_{2} & \mathrm{CH}_{2} \mathrm{F}_{2} \end{array} \) (a) Draw the Lewis dot structure. (b) Determine the molecular geometry and draw it as accurately as you can. (c) Indicate the polarity of any polar bonds with the \(\delta\) symbol. (d) Classify the molecule as polar or nonpolar. Text Transcription: CS_2 NCl_3 CF_2 CH_2F_2 delta

The VSEPR model is useful in predicting bond angles for many compounds. Consider the tabulated data for bond angles in related species and answer the questions. (a) Draw Lewis structures for all of the species in the table. (b) Use the Lewis structures from part a) to explain the observed bond angles in \(\mathrm{NO}_{2}\) and its associated ions. Text Transcription: NO_2