Chem 6.6-7.6

Which of the following elements may form an expanded valence shell? Select all that apply. N Cl S O Xe

Cl S Xe

A bond in which the shared electron density is concentrated along the axis between the bonding nuclei is called a(n) ___________ bond.

sigma

Select the partial orbital diagram that correctly shows the hybrid orbitals and electron distribution of the O atom in the molecule OF2. A B C D

B

A group of sp3 hybrid orbitals is formed by the hybridization of _____ s and _____ p orbital(s) from the valence shell of an atom. one, one three, one one, three one, two

one, three

A bond formed by sideways overlap of two p orbitals (one from each bonding atom) is called a(n) _________ bond. This type of bond has _________ region(s) of electron density.

pi, 2

An atom or molecule that contains an odd number of valence electrons is known as a free________

radical

90o octahedral 120o trigonal planar 109.5o tetrahedral 180o linear 90o and 120o trigonal bipyramidal

90- octahedral 120- trigonal planar 109.5- tetrahedral 180- linear 90o and 120- trigonal bipyramidal

Which of the following elements, when covalently bonded, commonly have fewer than an octet of electrons with a formal charge of zero? Select all that apply. Phosphorus Beryllium Boron Silicon Chlorine

Beryllium Boron

The attraction between an ion and a nearby polar molecule is called an ion - ___________ interaction. This attractive force is important when a(n) ____________ compound dissolves in a polar solvent such as H2O. Listen to the complete question

dipole, ionic

The strength of dispersion forces between two species depends on the mobility of their _________. The larger an atom or molecule, the more easily it becomes _______, and the _________ the dispersion forces it exhibits.

electrons, polarized, greater

Refer to the boiling point graph shown. H2O, NH3, and HF have much _________ boiling points than other group hydrides because these compounds can form _________ bonds between their molecules. Since this type of intermolecular force is very _________, it takes more _________ to separate the molecules so they can move from the liquid to the gas phase.

higher, hydrogen, strong, energy

Molecular shape is determined by the number of electron domains around a central atom, where an electron domain may be a(n) ___________ electron pair or any _______________ between two atoms.

lone, bond

Certain molecules are electron deficient, having fewer than _________ electrons around the central atom. Elements that commonly form electron deficient compounds are beryllium and __________. (One word answer.)

8, boron

Which of the following statements correctly describe the formation of sp2 hybrid orbitals? Select all that apply. Three sp2 hybrid orbitals are formed by the hybridization of one s and one p orbital. A group of sp2 hybrid orbitals assumes a trigonal planar geometry. An sp2 hybrid orbital is identical to an sp hybrid orbital in shape and energy. The formation of sp2 hybrid orbitals leaves one unhybridized valence p orbital.

A group of sp2 hybrid orbitals assumes a trigonal planar geometry. The formation of sp2 hybrid orbitals leaves one unhybridized valence p orbital.

Which of the following statements correctly describe a π bond? Select all that apply. A π bond concentrates electron density along the axis between two nuclei. A π bond is formed by the side-to-side overlap of two p orbitals. A π bond holds two electrons, one in each region of the bond. A multiple bond always contains at least one π bond.

A π bond is formed by the side-to-side overlap of two p orbitals. A multiple bond always contains at least one π bond.

Select all the statements that correctly describe sp hybrid orbitals. The combination of one s and one p orbital results in the formation of one sp hybrid orbital. Each sp hybrid orbital has one large and one small lobe. An sp-hybridized atom has one unhybridized p orbital in its valence shell. The angle between two sp hybrid orbitals is 180o.

Each sp hybrid orbital has one large and one small lobe. The angle between two sp hybrid orbitals is 180o.

Which species has a net dipole moment (i.e., are polar overall)? Select all that apply. NBr3 BCl3 Cl2 CH2Cl2 CO2

NBr3 CH2Cl2

Which of the following aspects of bonding are addressed by valence bond theory, but are NOT addressed by Lewis bond theory? The arrangement of atoms in a molecule The number of valence electrons in a molecule The differences in length between various single bonds The energetics of bond formation

The differences in length between various single bonds The energetics of bond formation

Select all the statements that correctly describe hybridization involving d orbitals. When sp3d orbitals are formed there will be four unhybridized d orbitals remaining. Any atom can form sp3d2 orbitals. The hybridization of one s, three p, and one d orbital gives five sp3d orbitals. A group of six sp3d2 orbitals will have an octahedral arrangement. An atom that needs to form six bonds will hybridize five d orbitals and one p orbital.

When sp3d orbitals are formed there will be four unhybridized d orbitals remaining. The hybridization of one s, three p, and one d orbital gives five sp3d orbitals. A group of six sp3d2 orbitals will have an octahedral arrangement.

In an ABx molecule, the angle between two adjacent A-B bonds is called the __________ angle. This angle is determined by the number of _____________ domains or groups surrounding the central atom.

bond, electron

In general, a lone pair repels bonding electron pairs _____ than bonding pairs repel each other. A lone pair will therefore _____ the bond angle between bonding pairs. A double bond has a similar effect. more, increase less, decrease more, decrease less, increase

more, decrease

Hybrid orbitals are designated by using a superscript to indicate the ________ of each type of orbital used to form them. For example, the designation sp2 indicates that _________ s and ___________ p orbitals were combined to form this orbital type.

number, 1, 2

Consider the molecule CCl4. Each C-Cl bond in this molecule is ________ because the electronegativity difference between C and Cl is equal to 0.5. Since CCl4 is tetrahedral in shape and symmetrical, the individual bond dipoles ________ and the molecule is __________ overall.

polar, cancel, nonpolar

A group of hybrid orbitals formed by the hybridization of s and p orbitals from the valence shell of an atom all have the same ______ and _______. size, orientation shape, orientation size, shape

size, shape

The triple bond in the structure shown consists of a σ bond formed by the overlap of a(n) _____ orbital on the C with a(n) _____ orbital on the N to form the σ bond. The π bonds are formed by the overlap of two pairs of _____ orbitals. sp, p, sp2 sp2, sp2, p sp, sp, p sp2, p, p

sp, sp, p

The hybridization of one s and one p orbital will result in the formation of two __________ hybrid orbitals. This will leave ___________ unhybridized valence p orbital(s), which is/are at right angles to the hybrid orbitals.

sp, two

The combination of one s and two p orbitals will form a group of three ________ hybrid orbitals. These hybrid orbitals adopt a(n) _________- planar geometry and are at an angle of _______ to the remaining unhybridized p orbital.

sp2, trigonal, 90

True or false: When using VSEPR theory to determine molecular shape, a triple bond counts as a single electron domain even though it consists of 3 shared electron pairs.

true

For an atom surrounded by 5 or 6 electron groups, hybrid orbitals are formed by combining ___________ s orbital(s), __________ p orbital(s) and 1 or 2 __________- orbitals.

1, 3, d

The molecular shape of a species, which is the arrangement of the bonded atoms around the central atom, is determined not only by the number of ___________ electron domains that join the atoms, but by the number of ____________ electron domains as well, since these electrons also occupy space.

bonding, nonbonding

What approximate value will be observed for the bond angle marked in the structure shown? (Note that Lewis structures commonly do not reflect the actual shape of the species.) between 109.5o and 180o greater than 180o less than 109.5o greater than 109.5o

less than 109.5o

A double bond is always made up of _____ σ and _____ π bond(s). A double bond is _____ than a single bond. 1; 1; weaker 1; 1; stronger 2; 0; weaker 0; 2; stronger

1; 1; stronger

The Lewis structure for the molecule BBr3 is given. The B atom in this structure is surrounded by a total of ____________ electron domains and is therefore ___________ -hybridized. There is _____________ unhybridized p orbital on the B atom, which contains no electrons. (Do NOT enter any special formatting for the hybridization.)

3, sp2, 1

In the molecule KrBr2 there are __________ electron domains surrounding the central Kr atom; _________ bonding pair(s) and ______ lone pair(s). The molecular geometry around the central atom is therefore __________.

5, 2, 3, linear

The structure shown contains _____ σ bond(s) and _____ π bond(s). 1, 6 5, 1 5, 2 6, 2 6, 1

6, 1

The Lewis structure for the AsF5 is shown. The approximate value of the bond angle marked "a" is equal to _____ while the approximate value of the bond angle marked "b" is equal to _____. (Remember that this species has a three-dimensional shape, as indicated by the wedged and dashed bonds.) 90o, 60o 90o, 90o 90o, 120o 120o, 120o

90o, 120o

Which of the following compounds exhibit hydrogen bonding between their molecules? Select all that apply. A B C D E

A B E

Why is BeF2 a nonpolar molecule? BeF2 is linear and therefore the individual bond dipoles cancel to give no net dipole. The individual bonds in BeF2 are nonpolar so the molecule is nonpolar. BeF2 contains polar bonds but is unsymmetrical in shape, which makes it nonpolar.

BeF2 is linear and therefore the individual bond dipoles cancel to give no net dipole.

Select the partial orbital diagram that correctly shows the hybrid orbitals and electron distribution of the N atom in the molecule NBr3. A B C D

C

Which of the following options correctly describe the structure shown? Select all that apply. C2 will have a linear geometry. The overall geometry of this molecule is octahedral. The bond angles around C2 are approximately equal to 180°. C1 will have a tetrahedral geometry. The bond angles around C1 will be equal to 90°.

C2 will have a linear geometry. The bond angles around C2 are approximately equal to 180°. C1 will have a tetrahedral geometry.

Which of the following compounds would experience the strongest overall intermolecular forces? CCl4 CBr4 Br2 CH4

CBr4

CH3OH Hydrogen bonding CH3F Dipole-dipole forces C3H8 Dispersion forces CaCl2 Ionic bonding

CH3OH Hydrogen bonding CH3F Dipole-dipole forces C3H8 Dispersion forces CaCl2 Ionic bonding

A momentary change in the electron density surrounding an atom or a molecule causes it to have a(n) __________ dipole even if it is not normally polar. This induces a similar effect in a nearby molecule or atom and there will be a weak attraction between the two particles as a result. These weak interactions are called __________ forces or London forces.

instantaneous, dispersion

The boiling point of a molecular substance reflects the strength of its ________ forces, the forces between the individual molecules. The stronger these forces, the ________ the amount of energy needed to separate the molecules, and the __________ the boiling point will be.

intermolecular, greater, higher

linear 5 electron domains; 3 lone pairs seesaw 5 electron domains; 1 lone pair square planar 6 electron domains; 2 lone pairs bent 4 electron domains; 2 lone pairs trigonal pyramidal 4 electron domains; 1 lone pair

linear 5 electron domains; 3 lone pairs seesaw 5 electron domains; 1 lone pair square planar 6 electron domains; 2 lone pairs bent 4 electron domains; 2 lone pairs trigonal pyramidal 4 electron domains; 1 lone pair

When two polar molecules are close together, the partial positive charge on one molecule will attract the partial ________ charge on the other. This type of intermolecular force is called a __________-_______ attraction.

negative, dipole-dipole

Elements that do not obey the octet rule because they have more than eight valence electrons are said to have an _____________ valence shell. This is only possible for elements that have available _________ orbitals, which are the elements found from period ____________ of the periodic table onward.

expanded, d, 3

True or false: A molecular covalent substance (such as CO2) has a low melting point because the covalent bonds that hold the molecules together are weak and do not require much energy to break.

false

True or false: Any molecule in which all of the bonds are identical will be nonpolar.

false

The larger a molecule or atom, the _____ the number of electrons and the _____ polarizable it will generally be. The strength of the dispersion forces for a particular substance therefore generally _____ as molar mass increases, providing molecules of similar shape are compared. greater; less; decreases greater; more; increases fewer; less; decreases greater; more; decreases

greater; more; increases

When a hydrogen atom is covalently bonded to either oxygen, __________ , or fluorine there will be an attraction between that hydrogen and a lone pair of _________ on a nitrogen, oxygen, or fluorine atom on an adjacent molecule. This attraction is called a __________ bond.

nitrogen, electrons, hydrogen

Dispersion forces are the only type of intermolecular force exhibited by atoms and by __________ molecules. Without the existence of dispersion forces, such substances would only exist as _____________

nonpolar, gases

Hydrogen bonding requires H to be covalently bonded to N, O, or F. Because these elements are very ________ and _________ they effectively pull electron density from the bonded H, leaving a H nucleus (a proton). This large positive charge on tiny H allows a close and very strong attraction (H-bond) to N, O, or F on a neighboring molecule.

small, electronegative

Which statement correctly explains how polarizability affects intermolecular forces? A more polarizable molecule experiences stronger dispersion forces and therefore stronger intermolecular forces overall. A more polarizable molecule has greater fluctuations in its dispersion forces and therefore experiences weaker intermolecular forces overall. A more polarizable molecule is more likely to experience hydrogen bonding, causing stronger intermolecular forces overall. A more polarizable molecule has a larger permanent dipole moment and experiences stronger dipole-dipole forces.

A more polarizable molecule experiences stronger dispersion forces and therefore stronger intermolecular forces overall.

Which of the following statements correctly defines a free radical? Any covalent species found in the upper atmosphere A species in which the central atom has fewer than 8 electrons A species with an odd number of valence electrons Any reactive ionic species

A species with an odd number of valence electrons

ABx A central atom in structure B terminal atom x number of terminal atoms

A- central atom in structure B- terminal atom x- number of terminal atoms

Which of the following statements correctly defines intermolecular forces? Intermolecular forces are the forces that hold atoms together in any molecular substance. Intermolecular forces are the weak forces of attraction found between the individual molecules of a molecular covalent substance. Intermolecular forces are the forces that hold the internal structure of the atom together. Intermolecular forces are the forces of attraction between any two bonded particles.

Intermolecular forces are the weak forces of attraction found between the individual molecules of a molecular covalent substance.

NO2 Fewer than eight valence electrons due to an odd number of valence electrons SCl6 More than eight valence electrons due to an expanded octet BeF2 Fewer than eight valence electrons due to a shortage of valence electrons

NO2- Fewer than eight valence electrons due to an odd number of valence electrons SCl6- More than eight valence electrons due to an expanded octet BeF2- Fewer than eight valence electrons due to a shortage of valence electrons

Which of the following statements correctly defines hybrid orbitals? Orbitals that are used to form different types of bonds Orbitals formed by the overlap of two orbitals from two different atoms Orbitals used for bonding that are formed by mixing atomic orbitals from the same atom Orbitals formed by mixing atomic orbitals from two different atoms in certain combinations

Orbitals used for bonding that are formed by mixing atomic orbitals from the same atom

Which of the following correctly describes the bond angle in a molecule of the general type ABx? The angle between the central atom A and any surrounding atom B The angle between the central atom A and any A-B bond The angle between two adjacent A-B bonds

The angle between two adjacent A-B bonds

Because lone pairs exert greater repulsions than bonded pairs, lone-pair domains always occupy the _____ positions in a trigonal bipyramid. axial equatorial

equatorial

Select all the options that correctly describe the bond angles associated with each electron-domain geometry. An octahedral system will have an ideal bond angle of 45o. A bond angle of 180o is observed for a linear system. Four electron domains will result in a bond angle of 90o. The trigonal bipyramidal system has two different bond angles. A species with 3 electron domains will exhibit an ideal bond angle of 120o

A bond angle of 180o is observed for a linear system. The trigonal bipyramidal system has two different bond angles. A species with 3 electron domains will exhibit an ideal bond angle of 120o.

Select all the statements that correctly explain why lone pairs prefer to occupy equatorial positions in a system with five electron domains. A lone pair in an axial position will be too far away from the other electron pairs. A larger bond angle leads to more electron repulsion. A lone pair in an equatorial position has more space. There is less repulsion between electron domains in equatorial positions.

A lone pair in an equatorial position has more space. There is less repulsion between electron domains in equatorial positions.

Select all the statements that correctly describe a σ bond. A σ bond results from end-to-end (direct) overlap of two orbitals. A σ bond can only result from the overlap of p orbitals. A σ bond concentrates electron density above and below the plane of the two bonded atoms. All single bonds are σ bonds.

A σ bond results from end-to-end (direct) overlap of two orbitals. All single bonds are σ bonds.

Select all the statements that correctly describe the five basic electron-domain geometries. An octahedral geometry indicates that there are six electron domains. If there are four electron domains, the system will adopt a square planar arrangement. A linear geometry is typical of a three-electron-domain system. A system with three electron domains will have a trigonal planar electron-domain arrangement.

An octahedral geometry indicates that there are six electron domains. A system with three electron domains will have a trigonal planar electron-domain arrangement.

Which of the following statements correctly describe sp3 hybrid orbitals? Select all that apply. The four sp3 hybrid orbitals are lower in energy than the original atomic orbitals from which they were formed. An sp3 hybrid orbital is unsymmetrical in shape, having one small and one large lobe. The sp3 hybrid orbitals are perpendicular to each other. The four sp3 hybrid orbitals of a group are equivalent in shape and energy.

An sp3 hybrid orbital is unsymmetrical in shape, having one small and one large lobe. The four sp3 hybrid orbitals of a group are equivalent in shape and energy.

Select all the statements that correctly describe the hybridization model of bonding. Before a covalent bond forms, atomic orbitals from a specific atom mix or hybridize to form hybrid orbitals. Hybridization refers to the combination of one atomic orbital from each of the atoms bonding. A hybrid orbital can hold more than 2 electrons. A covalent bond can be formed when a hybrid orbital from one atom overlaps with an orbital from another atom.

Before a covalent bond forms, atomic orbitals from a specific atom mix or hybridize to form hybrid orbitals. A covalent bond can be formed when a hybrid orbital from one atom overlaps with an orbital from another atom.

Which intermolecular forces are exhibited between molecules of the compound shown? Select all that apply. Dipole-dipole forces Covalent bonds Hydrogen bonding Dispersion forces

Dipole-dipole forces Dispersion forces

Which of the following statements correctly describe dispersion or London forces? Select all that apply. Dispersion forces are a weak attraction between temporary dipoles. Dispersion forces are stronger for smaller molecules. Dispersion forces are the primary intermolecular force exhibited by polar molecules. All covalent compounds exhibit dispersion forces.

Dispersion forces are a weak attraction between temporary dipoles. All covalent compounds exhibit dispersion forces.

Select all the statements that correctly describe the bonding in the molecule PF3 in terms of valence bond theory. Each P-F bond is formed by the overlap of a 3p orbital from P with a 2p orbital from F. The P atom in this molecule will have an empty valence orbital. VB theory predicts that the bond angles in PF3 will be close to 900. The P atom uses its 3s orbital for bonding.

Each P-F bond is formed by the overlap of a 3p orbital from P with a 2p orbital from F. VB theory predicts that the bond angles in PF3 will be close to 900.

Which statement correctly describes the basic principle of VSEPR theory? Each bonding group of electrons around a central atom is located as far from the others as possible. Each bonding pair of electrons around a central atom is located as far from the others as possible. Each atom attached to the central atom of a structure is located as far from the others as possible. Each group of valence electrons around a central atom is located as far from the others as possible.

Each group of valence electrons around a central atom is located as far from the others as possible.

Which of the following options correctly reflect the relationship between dispersion forces and particle size? Select all that apply. For molecules of similar shape, dispersion forces tend to increase with increasing molar mass. Dispersion forces are strongest for small particles since they can get closer together in space. Dispersion forces tend to decrease with size as larger particles are farther apart and therefore attract each other less. Larger particles are more polarizable and experience stronger dispersion forces.

For molecules of similar shape, dispersion forces tend to increase with increasing molar mass. Larger particles are more polarizable and experience stronger dispersion forces.

How does hybridization of atomic orbitals allow us to reconcile valence bond theory with VSEPR theory? Hybridization enables us to account for the number of singly-occupied orbitals required for bonding. Hybridization enables us to predict the shapes of molecules. Hybridized atomic orbitals produce new mixed orbitals that extend over the entire molecule. Hybridization of atomic orbitals produces orbital shapes and spatial orientations that correlate to those predicted in VSEPR theory.

Hybridization enables us to account for the number of singly-occupied orbitals required for bonding. Hybridization of atomic orbitals produces orbital shapes and spatial orientations that correlate to those predicted in VSEPR theory.

Which of the following statements correctly describe how to determine whether a given molecule is polar or nonpolar? Select all that apply. If the individual bond dipoles cancel, the molecule is nonpolar. A molecule that has a symmetrical geometry is always nonpolar. For a molecule that has polar bonds, the molecular geometry must be known in order to predict the overall polarity. If a molecule contains no dipole moments across any bonds it will be nonpolar.

If the individual bond dipoles cancel, the molecule is nonpolar. For a molecule that has polar bonds, the molecular geometry must be known in order to predict the overall polarity. If a molecule contains no dipole moments across any bonds it will be nonpolar.

Select all the statements that correctly describe how to determine the molecular shape of a species using VSEPR. If unshared electron pairs are present, the molecular geometry will differ from the electron-domain geometry. The total number of shared and unshared electron pairs around the central atom gives the electron-domain geometry. A double bond is counted as two separate electron domains around a central atom. Use the molecular formula to draw the Lewis structure. Count only the bonding electrons around the central atom.

If unshared electron pairs are present, the molecular geometry will differ from the electron-domain geometry. The total number of shared and unshared electron pairs around the central atom gives the electron-domain geometry. Use the molecular formula to draw the Lewis structure.

Select all the statements that correctly describe the arrangement of lone pairs in systems with 5 and 6 electron domains. In a trigonal bipyramidal system lone pairs prefer to occupy equatorial positions. In the octahedral system a lone pair will prefer to occupy an axial position. If there are two lone pairs in an octahedral system they will be located opposite each other. In a system with 5 electron domains a lone pair will occupy an axial position.

In a trigonal bipyramidal system lone pairs prefer to occupy equatorial positions. If there are two lone pairs in an octahedral system they will be located opposite each other.

Individual bond dipoles will cancel for a species that has identical bonds and a symmetrical geometry. Individual bond dipoles will not cancel for a species with an unsymmetrical geometry. A species will be nonpolar if individual bond dipoles cancel. A species will be polar overall if individual bond dipoles do not cancel.

Individual bond dipoles will cancel for a species that has identical bonds and a symmetrical geometry. Individual bond dipoles will not cancel for a species with an unsymmetrical geometry. A species will be nonpolar if individual bond dipoles cancel. A species will be polar overall if individual bond dipoles do not cancel.

Select all the statements that correctly explain why bond angles in molecules containing lone pairs or multiple bonds may be different than the VSEPR ideal. Multiple bonds contain higher electron densities that repel more than single bonds. Lone pairs exert greater repulsion that causes compression in adjacent bond angles. Multiple bonds repel more strongly than single bonds that results in compression in adjacent bond angles. Lone pairs take up less space than bonded pairs of electrons between two nuclei that allows the expansion of adjacent bond angles. Multiple bonds are longer than single bonds that results in the expansion of adjacent bond angles.

Multiple bonds contain higher electron densities that repel more than single bonds. Lone pairs exert greater repulsion that causes compression in adjacent bond angles. Multiple bonds repel more strongly than single bonds that results in compression in adjacent bond angles.

Draw the Lewis structures for NH2-, NH3, and NH4+. How would you expect the H-N-H bond angle in each species to compare? NH3 < NH2- < NH4+ NH4+ < NH3 < NH2- NH2- = NH3 < NH4+ NH2- < NH3 < NH4+

NH2- < NH3 < NH4+

Which of the following options correctly describe the NH2-CH=O structure? Select all that apply. Nitrogen will have a tetrahedral molecular geometry. Nitrogen will have a trigonal pyramidal molecular geometry. Nitrogen will have a trigonal planar molecular geometry. Carbon will have a bent molecular geometry. Carbon will have a trigonal planar molecular geometry.

Nitrogen will have a trigonal pyramidal molecular geometry. Carbon will have a trigonal planar molecular geometry.

Select all the statements that correctly describe the bonding in the molecule HCl in terms of valence bond theory. Valence bond theory predicts the H atom uses an excited electron in a 2s orbital for bonding. The H-Cl bond is formed by the overlap of a 3p orbital from Cl with a 1s orbital from H. Valence bond theory predicts the potential energy is a minimum for an optimal orbital overlap for H and Cl. The Cl atom in this molecule will have an empty valence orbital.

The H-Cl bond is formed by the overlap of a 3p orbital from Cl with a 1s orbital from H. Valence bond theory predicts the potential energy is a minimum for an optimal orbital overlap for H and Cl.

Select all the statements that correctly describe the C=N double bond in the structure shown. The σ bond is formed by the overlap of an sp2 orbital from N with a p orbital from C. The N lone pair is located in an sp2 orbital. The double bond consists of two π bonds. The σ bond is formed by direct head-to-head overlap of two sp2 hybrid orbitals, one from each atom. The π bond is formed by sideways overlap of a p orbital from each atom.

The N lone pair is located in an sp2 orbital. The σ bond is formed by direct head-to-head overlap of two sp2 hybrid orbitals, one from each atom. The π bond is formed by sideways overlap of a p orbital from each atom.

Which of the following statements correctly describe the VSEPR model? Select all that apply. The VSEPR model states that the electron domains surrounding a central atom attract each other. The VSEPR model is used to predict the geometry of a covalently bonded species. The VSEPR model is used to predict the number of bonds a given element will form. According to this model, the valence electrons around a central atom are located as far from each other as possible. A Lewis structure is necessary in order to apply the VSEPR model.

The VSEPR model is used to predict the geometry of a covalently bonded species. According to this model, the valence electrons around a central atom are located as far from each other as possible. A Lewis structure is necessary in order to apply the VSEPR model.

The Lewis structure for the molecule NF3 is shown. Select all the statements that correctly describe the bonding in this molecule. The N lone pair is located in an unhybridized p orbital. The N atom has three bonds and is therefore sp2-hybridized. The bond angles for this molecule are slightly less than 109.5o The N uses one sp3 hybrid orbital to form each N-F bond.

The bond angles for this molecule are slightly less than 109.5o The N uses one sp3 hybrid orbital to form each N-F bond.

Which position will a lone pair preferentially occupy in a trigonal bipyramidal geometry and why? All positions are equivalent in the electron-domain geometries, but a second lone pair will occupy a domain 180o from the first. The axial position because it affords less separation from other domains for greater attractive stability. The equatorial position because it affords more separation from other domains for the greater repulsion of a lone pair. The axial position because it affords more separation from other domains for the greater repulsion of a lone pair.

The equatorial position because it affords more separation from other domains for the greater repulsion of a lone pair.

Select all the statements that correctly describe the bonding in a covalently bonded species using hybridization. The ground-state electron configuration of the atom shows the orbitals available for hybridization. The number of electron domains around the atom determines the number of hybrid orbitals required. Two electrons are placed in each hybrid orbital to show the orbitals available for bonding. The appropriate number of atomic orbitals are combined, starting with a p orbital.

The ground-state electron configuration of the atom shows the orbitals available for hybridization. The number of electron domains around the atom determines the number of hybrid orbitals required.

As the boiling point graph shows, H2O, NH3, and HF deviate from the boiling point trend shown for the hydrides of the carbon group. Select the statement that correctly explains this deviation. These compounds are ionic, and are therefore held together by much stronger attractive forces than those found between CH4 molecules. The hydrogen bonding between molecules of H2O, NH3, and HF is much stronger than the intermolecular forces between CH4 molecules.

The hydrogen bonding between molecules of H2O, NH3, and HF is much stronger than the intermolecular forces between CH4 molecules.

Select all the correct statements regarding ion-dipole interactions. The magnitude of ion-dipole interactions is inversely proportional to the size of the polar molecule. Ion-dipole interactions only occur in mixtures. Ion-dipole interactions are responsible for the solubility of ionic compounds in aqueous solutions. The typical magnitude of ion-dipole interactions is smaller than that of the van der Waals interactions in a pure substance. The magnitude of ion-dipole interactions is inversely proportional to the charge on the ion. An ion-dipole interaction exists between an ion and a polar molecule.

The magnitude of ion-dipole interactions is inversely proportional to the size of the polar molecule. Ion-dipole interactions only occur in mixtures. Ion-dipole interactions are responsible for the solubility of ionic compounds in aqueous solutions. An ion-dipole interaction exists between an ion and a polar molecule.

Select all the statements that correctly describe the bonding and geometry in the polyatomic ion SeCl5-. The molecular geometry is square pyramidal. The molecular geometry is trigonal bipyramidal. There are 6 electron domains around the central atom. The lone pair occupies an equatorial position. There is one lone pair on the central atom.

The molecular geometry is square pyramidal. There are 6 electron domains around the central atom. There is one lone pair on the central atom.

Select all the statements that correctly describe the bonding and geometry in the polyatomic ion SeCl5-. The molecular geometry is square pyramidal. The molecular geometry is trigonal bipyramidal. There are 6 electron domains around the central atom. There is one lone pair on the central atom. The lone pair occupies an equatorial position.

The molecular geometry is square pyramidal. There are 6 electron domains around the central atom. There is one lone pair on the central atom.

A particular hybrid orbital is designated sp3d2. What information is provided by the superscripts in this designation? The number of electrons located in each type of orbital The number of each type of atomic orbital combined to produce this type of hybrid orbital The energy level of each different type of atomic orbital combined to produce the hybrid orbital The number of bonds formed by the relevant atom

The number of each type of atomic orbital combined to produce this type of hybrid orbital

Why is the hybridization model necessary to explain the bonding in a molecule such as CH4? Select all that apply. Carbon should only form ionic bonds based on its atomic electron configuration. The observed bond angles cannot be explained using unhybridized orbitals. The atomic electron configuration of carbon cannot account for four equivalent bonds. Carbon has no available orbitals to form bonds based on its atomic electron configuration.

The observed bond angles cannot be explained using unhybridized orbitals. The atomic electron configuration of carbon cannot account for four equivalent bonds.

The electron-domain geometry of a species is the arrangement of electron ____________ around the central atom, whereas the molecular geometry is the arrangement of bonded ________________. Two species with the same electron-domain geometry may have different molecular geometries.

domain, atoms

Which of the following statements correctly describe valence bond theory? Select all that apply. The space formed by overlapping orbitals can accommodate a maximum of two electrons. A covalent bond results from the attraction between the nuclei of the two bonded atoms and the shared electron pair. The overlap of orbitals to form a bond results in a lower potential energy for the system. Covalent bonding results from the combination of the wave functions of the orbitals.

The space formed by overlapping orbitals can accommodate a maximum of two electrons. A covalent bond results from the attraction between the nuclei of the two bonded atoms and the shared electron pair. The overlap of orbitals to form a bond results in a lower potential energy for the system.

Which of the following would cause the central atom in a Lewis structure to have less than a full octet of electrons? Select all that apply. The total number of valence electrons is odd. The species has a shortage of valence electrons. One or more atoms in the structure have nonzero formal charges. The structure has a partial separation of charge.

The total number of valence electrons is odd. The species has a shortage of valence electrons.

Select all the statements that correctly describe dipole-dipole attractions. These are the forces of attraction between two polar molecules. For two compounds of similar molar mass, the greater the molecular dipole moment, the stronger the dipole-dipole attraction. Any molecule that contains polar covalent bonds will experience dipole-dipole attractions. Dipole-dipole forces arise from the attraction between the like partial charges on two adjacent molecules.

These are the forces of attraction between two polar molecules. For two compounds of similar molar mass, the greater the molecular dipole moment, the stronger the dipole-dipole attraction.

Which of the following statements correctly explain why hydrogen bonding requires that H should be covalently bonded to N, O, or F? Select all that apply. These elements are small, allowing their lone pairs to approach the H of an adjacent molecule closely. N, O, and F make only weak bonds to H, allowing the H to bond freely to other atoms. All these elements are in the second period and 2p orbitals interact strongly with H. N, O, and F are so electronegative that a H covalently bonded to any one of these elements has very high positive character.

These elements are small, allowing their lone pairs to approach the H of an adjacent molecule closely. N, O, and F are so electronegative that a H covalently bonded to any one of these elements has very high positive character.

Which of the following statements are correct with regard to Lewis bonding theory and valence bonding theory? Valence bond theory can make predictions about bond angles that Lewis theory cannot. Lewis theory does not explain differences in bond strength, while valence bond theory does. Lewis bond theory explains why bonds form, while valence bond theory does not. Valence bond theory predicts a different number of valence electrons around a central atom than Lewis theory does.

Valence bond theory can make predictions about bond angles that Lewis theory cannot. Lewis theory does not explain differences in bond strength, while valence bond theory does.

Molecular geometry is specified for a central atom in a structure. A "central" atom is _____. an atom that is surrounded by four other atoms any atom that is bonded to two or more other atoms an atom located in the very center of the structure

any atom that is bonded to two or more other atoms

bent 3 electron domains; 1 lone pair T-shaped 5 electron domains; 2 lone pairs square pyramidal 6 electron domains; 1 lone pair tetrahedral 4 electron domains; 0 lone pairs linear 2 electron domains; 0 lone pairs

bent 3 electron domains; 1 lone pair T-shaped 5 electron domains; 2 lone pairs square pyramidal 6 electron domains; 1 lone pair tetrahedral 4 electron domains; 0 lone pairs linear 2 electron domains; 0 lone pairs

Most covalently bonded substances consist of individual separate molecules. Each individual molecule is held together by means of strong ___________ bonds between the atoms. In addition, there are weak forces of attraction between the individual molecules, called _________ forces.

covalent, intermolecular

According to valence bond theory, a(n) _____ bond is formed by the overlap of orbitals from two atoms. Energy is released during this process so that the system is at a _____ potential energy after bonding. covalent, lower ionic, lower ionic, higher covalent, higher

covalent, lower