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    which of the following statements are correct with regard to lewis bonding theory and valence bonding theory?

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    Which of the following aspects of bonding are addressed by valence bond theory, but are NOT addressed by Lewis bond theory?

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    -The energetics of bond formation

    -The differences in length between various single bonds

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    Select all the statements that correctly describe the bonding in the molecule PF3 in terms of valence bond theory.

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    -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.

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    Terms in this set (52)

    Which of the following aspects of bonding are addressed by valence bond theory, but are NOT addressed by Lewis bond theory?

    -The energetics of bond formation

    -The differences in length between various single bonds

    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.

    -VB theory predicts that the bond angles in PF3 will be close to 900.

    Which of the following statements correctly defines hybrid orbitals?

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

    Select all the statements that correctly describe sp hybrid orbitals.

    -Each sp hybrid orbital has one large and one small lobe.

    -The angle between two sp hybrid orbitals is 180o.

    Which of the following statements correctly describe the formation of sp2 hybrid orbitals? Select all that apply.

    -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 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.

    Select all the statements that correctly describe the bonding in the molecule HCl in terms of valence bond theory.

    -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 hybridization model of bonding.

    -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.

    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 _____ o to the remaining unhybridized p orbital.

    -sp2 -trigonal -90

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    Verified questions

    PHYSICS

    A top fuel drag racer with a mass of 500.0 kg completes a quarter-mile (402 m) drag race in a time of 4.2 s starting from rest. The car's final speed is 125 m/s. What is the engine's average power output? Ignore friction and air resistance.

    Verified answer PHYSICS

    A student of mass 60.0 kg, starting at rest, slides down a slide 20.0 m long, tilted at an angle of

    30.0^{\circ} 30.0 ∘

    with respect to the horizontal. If the coefficient of kinetic friction between the student and the slide is 0.120, find the force of kinetic friction.

    Verified answer PHYSICS

    Four distinguishable harmonic oscillators a, b, c, and d may exchange energy. The energies allowed particle a are

    E_{a}=n_{a} \hbar \omega_{0}

    E a ​ =n a ​ ℏω 0 ​

    those allowed particle b are

    E_{b}=n_{b} \hbar \omega_{0}

    E b ​ =n b ​ ℏω 0 ​

    Source : quizlet.com

    Sample Questions

    1.

    The valence electrons of representative elements are

    (a) in s orbitals only.

    (b) located in the outermost occupied major energy level.

    (c) located closest to the nucleus.

    (d) located in d orbitals.

    (e) located in the innermost occupied shell.

    2.

    Which of the following pairs of elements and valence electrons is incorrect?

    (a) Al - 3 (b) Br - 7 (c) S - 4 (d) Sr - 2 (e) Tl - 3

    3.

    With regard to the species 16O2-, 19F- and 20Ne, which of the following statements is correct?

    (a) All three species contain 10 electrons.

    (b)The sum of the neutrons in all three species is 27.

    (c) The sum of the protons in all three species is 28.

    (d) Both 19F- and 20Ne contain 20 neutrons.

    (e) none of the above

    4.

    Which of the following does not have a noble gas electron configuration? (or Which of the following is not isoelectronic with a noble gas?)

    (a) S2- (b) Ba+ (c) Al3+ (d) Sb3- (e) Sc3+

    5.

    Which one of the formulas for ionic compounds below is incorrect?

    (a) SrCl2 (b) Cs2S (c) AlCl3 (d) Al3P2 (e) CaSe

    6.

    Which is classified as nonpolar covalent?

    (a) the H-I bond in HI

    (b) the H-S bond in H2S

    (c) the P-Cl bond in PCl3

    (d) the N-Cl bond in NCl3

    (e) the N-H bond in NH3

    7.

    Which one of the compounds below is most likely to be ionic?

    (a) GaAs (b) ScCl3 (c) NO2 (d) CCl4 (e) ClO2

    8.

    The correct electron-dot formulation for hydrogen cyanide shows:

    (a) 2 double bonds and two lone pairs of electrons on the N atom.

    (b) 1 C-H bond, 1 C=N bond, 1 lone pair of electrons on the C atom and 1 lone pair of electrons on the N atom.

    (c) 1 C-H bond, 1 C-N bond, 2 lone pairs of electrons on the C atom and 3 lone pairs of electrons on the N atom.

    (d) 1 triple bond between C and N, 1 N-H bond and 2 lone pairs of electrons on the C atom.

    (e) 1 triple bond between C and N, 1 C-H bond and 1 lone pair of electrons on the N atom.

    9.

    The correct dot formulation for nitrogen trichloride has:

    (a) 3 N-Cl bonds and 10 lone pairs of electrons.

    (b) 3 N=Cl bonds and 6 lone pairs of electrons.

    (c) 1 N-Cl bond, 2 N=Cl bonds and 7 lone pairs of electrons.

    (d) 2 N-Cl bonds, 1 N=Cl bond and 8 lone pairs of electrons.

    (e) 3 N-Cl bonds and 9 lone pairs of electrons.

    10.

    What is the total number of electrons in the correct Lewis dot formula of the sulfite ion?

    (a) 8 (b) 24 (c) 26 (d) 30 (e) 32

    11.

    In the Lewis structure for the OF2 molecule, the number of lone pairs of electrons around the central oxygen atom is

    (a) 0 (b) 1 (c) 2 (d) 3 (e) 4

    12.

    The electronic structure of the SO2 molecule is best represented as a resonance hybrid of ____ equivalent structures.

    (a) 2 (b) 3 (c) 4 (d) 5

    (e) This molecule does not exhibit resonance.

    13.

    Consider the bicarbonate ion (also called the hydrogen carbonate ion). After drawing the correct Lewis dot structure(s), you would see:

    (a) two double bonds around the central carbon atom.

    (b) three single bonds around the central carbon atom.

    (c) four single bonds around the central carbon atom.

    (d) two equivalent resonance forms.

    (e) three equivalent resonance forms.

    14.

    Draw one of the resonance structures of SO3. The formal charge of S is

    (a) +2 (b) +1 (c) 0 (d) -1 (e) -2

    15.

    Which one of the following violates the octet rule?

    (a) PCl3 (b) CBr4 (c) NF3 (d) OF2 (e) AsF5

    Source : www.chem.tamu.edu

    9.2: Valence Bond Theory

    9.2: Valence Bond Theory

    Last updated May 24, 2020

    9.1: Orbitals and Theories of Chemical Bonding

    9.3: Molecular Orbital Theory

    picture_as_pdf Readability Cite this page Donate

    Sigma (σ) and Pi (π) bonds in Valence Bond Theory (VBT)

    Exercise 9.2.1 9.2.1

    Which of the following statements concerning hybrid orbitals is/are CORRECT?

    The number of hybrid orbitals equals the number of atomic orbitals that are used to create the hybrids.

    When atomic orbitals are hybridized, the s orbital and at least one p orbital are always hybridized.

    To create tetrahedral structures, the s orbital and all three p orbitals must be hybridized.

    a. 1 only        b. 2 only        c. 3 only        d. 2 and 3        e. 1, 2, and 3

    Answer

    Exercise 9.2.2 9.2.2

    Which of the following statements concerning σ and π bonds is/are correct?

    Sigma bonds can only be formed from unhybridized orbitals.

    Pi bonds are formed from unhybridized p orbitals.

    A pi bond has an electron distribution above and below the bond axis.

    a. 1 only        b. 2 only        c. 3 only        d. 1 and 2        e. 2 and 3

    Answer

    Exercise 9.2.3 9.2.3

    Which of the following concerning σ and π bonds is/are correct?

    A sigma bond may be formed from the sideways overlap of two parallel p orbitals.

    No more than two pi bonds are possible between adjacent carbon atoms.

    The considerable energy required to rotate pi bonded atoms is the primary reason for geometrical isomerism in some pi bonded molecules.

    a. 1 only        b. 2 only        c. 3 only        d. 1 and 2        e. 2 and 3

    Answer

    Number of Sigma (σ) and Pi (π) bonds 

    Exercise 9.2.4 9.2.4

    How many sigma and pi bonds are in the molecule pictured below?

    Answer

    Exercise 9.2.5 9.2.5

    How many sigma (σ) bonds and pi (π) bonds are in dioxygen?

    Answer

    Exercise 9.2.6 9.2.6

    How many sigma (σ) bonds and pi (π) bonds are present in the given molecule?

    Answer

      Hybridization 

    Exercise 9.2.7 9.2.7

    What is the hybridization of the central nitrogen atom in N2O?

    Answer

    Exercise 9.2.8 9.2.8

    What is the hybridization of the sulfur atom in SCl2?

    Answer

    Exercise 9.2.9 9.2.9

    The hybridization of the nitrogen atom in NH3 is _____.

    Answer

    Exercise 9.2.10 9.2.10

    In valence bond theory, each sigma bond in CH4 is formed from the overlap of a hydrogen atom's 1 orbital with a(n) ________ hybridized orbital on the carbon atom.

    Answer

    Exercise 9.2.11 9.2.11

    SF3+, has a tetrahedral electron-pair geometry and a trigonal-pyramidal molecular geometry. The hybridization of the central sulfur atom is ________.

    Answer

    Exercise 9.2.12 9.2.12

    The hybridization of the carbon atom in CF3+ is ________.

    Answer

      Hybridization and Molecular Geometry 

    Exercise 9.2.13 9.2.13

    In the context of valence shell electron pair repulsion (VSEPR) theory, what is the molecular geometry around a central atom that is sp3 hybridized and has one lone pair of electrons?

    Answer

    Exercise 9.2.14 9.2.14

    What is the molecular geometry around a central atom that is sp2 hybridized, has three sigma bonds, and one pi bond?

    Answer

    Exercise 9.2.15 9.2.15

    When an atom in a molecule or ion is described as sp3 hybridized, its electron pair geometry is

    Answer

    Reactions and Hybridization 

    Exercise 9.2.16 9.2.16

    Upon combustion, ethene (C2H4) is converted to carbon dioxide and water.What change occurs in the hybridization of carbon atoms in this reaction?

    Answer

    Exercise 9.2.17 9.2.17

    Ammonia reacts with oxygen and water to produce nitric acid. What change in hybridization of the nitrogen atom occurs in this reaction?

    Answer

    Exercise 9.2.18 9.2.18

    Nitric acid, HNO3, dissociates in water to form nitrate ions and hydronium ions. What change in hybridization of the nitrogen atom occurs in this dissociation?

    Answer

    Label Hybridization from Lewis Dot Structures 

    Exercise 9.2.19 9.2.19

    Which of the underlined atoms (C1, C2, N, and O) are sp2 hybridized?

    Answer

    Exercise 9.2.20 9.2.20

    Which of the labeled carbon atoms (C1-C4) is/are sp hybridized?

    Answer

    Exercise 9.2.21 9.2.21

    What is the hybridization of oxygen atom O?

    Source : chem.libretexts.org

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    James 8 month ago
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