It is necessary to use prefixes in naming binary molecular compounds because they indicate the number of each element present.

They indicate the number of each element present

They follow tradition without purpose

Which exception to the octet rule is shown in the electron dot structure of this molecule?

Odd number of valence electrons

When xenon forms six bonds with fluorine, it does not follow the octet rule. Determine the number of lone pairs of electrons in the xenon atom and the total number of valence electrons in XeF6.

Xenon has 1 lone pair and XeF6 has 50 valence electrons.

Xenon has 0 lone pairs and XeF6 has 48 valence electrons.

Xenon has 1 lone pair and XeF6 has 48 valence electrons.

Xenon has 0 lone pairs and XeF6 has 50 valence electrons.

PBr5 is an exception to the octet rule, while PBr3 is not because phosphorus in PBr5 uses d orbitals to form five bonds and expand its octet, whereas in PBr3 phosphorus forms only three bonds and maintains an octet.

Phosphorus in PBr5 uses d orbitals to exceed the octet, whereas in PBr3 it does not.

PBr5 has more bromine atoms which do not affect the octet rule.

Both compounds obey the octet rule in the same way.

PBr3 has an expanded octet while PBr5 does not.

The boiling point difference between ethanol (78.3°C) and hexane (68.7°C) is because of the different intermolecular forces present. Which of the following best describes the intermolecular forces in these compounds?

Ethanol exhibits hydrogen bonding and hexane exhibits London dispersion forces.

Ethanol exhibits hydrogen bonding and hexane exhibits dipole-dipole interactions.

Both ethanol and hexane exhibit hydrogen bonding.

Ethanol exhibits London dispersion forces and hexane exhibits hydrogen bonding.

The structure of carbon tetrachloride, CCl4, is similar to that of methane. It is:

Nonpolar (due to tetrahedral symmetry that cancels out the dipole moments)

Polar (if the dipoles did not cancel due to an irregular geometry)

Molecules of carbon monoxide (CO) are polar because of the difference in electronegativity between carbon and oxygen.

They are polar due to the difference in electronegativity between carbon and oxygen.

They are nonpolar because they have a linear structure with symmetrical charge distribution.

They are polar because of the presence of hydrogen atoms.

They are nonpolar due to equal sharing of electrons.

Intermolecular forces differ between polar and nonpolar molecules based on the types of intermolecular interactions they exhibit.

Polar molecules exhibit dipole-dipole interactions and hydrogen bonding (when applicable), while nonpolar molecules primarily exhibit London dispersion forces.

Both polar and nonpolar molecules exhibit the same types of intermolecular forces.

Only nonpolar molecules exhibit intermolecular forces.

There is no difference in the intermolecular forces of polar and nonpolar molecules.

Dipole-dipole forces refer to general attractions between polar molecules, while a hydrogen bond is a specific, stronger type of dipole-dipole interaction that occurs when hydrogen is bound to F, O, or N.

Dipole-dipole forces refer to general attractions between polar molecules, while a hydrogen bond is a specific, stronger type of dipole-dipole interaction that occurs when hydrogen is bound to F, O, or N.

Dipole-dipole forces involve hydrogen atoms only, whereas hydrogen bonds involve any two polar molecules.

Dipole-dipole forces are covalent bonds, while hydrogen bonds are ionic bonds.

There is no difference; they are two terms for the same interaction.

Bond length and bond strength have an inverse relationship.

Shorter bonds are stronger than longer bonds.

Longer bonds are stronger than shorter bonds.

Bond length has no impact on bond strength.

Bond length determines bond polarity.

Describe the difference between an exothermic and an endothermic reaction in terms of bond breaking and bond forming. (Select the correct explanation)

In an exothermic reaction, the energy released during bond formation is greater than the energy required for bond breaking; in an endothermic reaction, the energy required for bond breaking is greater than the energy released during bond formation.

In an exothermic reaction, bonds break without energy requirements; in an endothermic reaction, bonds form without releasing energy.

Exothermic reactions involve only bond breaking while endothermic reactions involve only bond forming.

There is no difference between the bond energy dynamics in exothermic and endothermic reactions.

Hybridization is the concept explaining the mixing of atomic orbitals to form new hybrid orbitals, which then determine molecular shapes. Which of the following best describes hybridization?

It is the mixing of atomic orbitals to form hybrid orbitals that explain molecular geometry.

It is the process of electron transfer between atoms.

It describes the nuclear fusion within molecules.

It is a model that explains bonding solely based on electrostatic forces.

Predict the molecular geometry and bond angles of BF3.

Trigonal planar geometry with bond angles of 120°

Tetrahedral geometry with bond angles of 109.5°

Bent geometry with bond angles less than 120°

Linear geometry with bond angles of 180°

Resonance structures represent different possible distributions of electrons in a molecule that cannot be depicted by a single Lewis structure, and they are important in describing molecular bonding as they provide insight into the actual electron distribution and stability of the molecule.

They represent various electron distributions that explain the true electron layout and bonding in a molecule.

They are identical pictures of a molecule that do not affect bonding.

They show positions of atoms only without electron involvement.

They only indicate the presence of isotopes in a molecule.

Some molecules have multiple bonds while others do not due to differences in their electron configurations and bonding requirements.

Because of differences in electron configurations and bond formation requirements.

Because some atoms are heavier.

Because some molecules are larger.

Electronegativity affects bond polarity by increasing polarity as the difference between the electronegativities of the bonded atoms increases.

It has no effect on bond polarity.

It only affects bond polarity in ionic bonds.

Explain how formal charge is used to determine the most stable Lewis structure. Choose the answer that states the minimal formal charge distribution.

It is used to minimize formal charges and ensure negative charges reside on more electronegative atoms.

It is not used at all in determining stability.

It maximizes the formal charges to create more reactive structures.

It solely depends on atom size without considering electronegativity.

Factors such as the difference in electronegativity between atoms and the molecular geometry determine whether a molecule is polar or nonpolar.

Both electronegativity differences and molecular geometry are crucial.

Only electronegativity differences are important.

Only molecular geometry matters.

Relationship between molecular shape and molecular polarity: Molecular shape determines the overall polarity of a molecule. Symmetric molecules tend to be nonpolar, while asymmetric molecules tend to be polar.

Molecular shape determines molecular polarity: symmetric molecules are nonpolar, while asymmetric molecules are polar.

Molecular polarity solely depends on electronegativity differences between atoms.

Molecular shape does not affect polarity, which is randomly distributed.

There is no relationship between molecular shape and molecular polarity.

Some molecules deviate from ideal bond angles predicted by VSEPR theory due to the increased repulsion from nonbonding electron pairs compared to bonding pairs.

The presence of lone pairs increases repulsion, causing bond angles to decrease.

Multiple bonds always lead to expansion of bond angles.

Resonance structures eliminate variations in bond angles.

Hybridization has no effect on bond angles.

Molecular orbital theory differs from valence bond theory because:

It considers electrons to be delocalized over the entire molecule, while valence bond theory treats electrons as localized between pairs of atoms.

It only describes the electronic structure of homonuclear diatomic molecules.

It is used exclusively for ionic bonds, while valence bond theory applies to covalent bonds.

There is no significant difference between the two theories.

Bond dissociation energy is significant in chemical reactions as it provides information about the energy required to break a chemical bond.

It provides information about the energy required to break a bond in a chemical reaction.

It helps to identify the structure of molecules.

It solely determines the reaction speed.

It indicates the physical state of the substance.

Lone pairs affect molecular geometry as compared to bonding pairs by:

They exert greater repulsive force, resulting in smaller bond angles.

They exert the same repulsive force as bonding pairs, resulting in similar bond angles.

They exert less repulsive force, resulting in larger bond angles.

They do not affect molecular geometry at all.

Chapter Review: Chapter 7

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Chapter Review: Chapter 7

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10th Grade

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Practice Problem

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Hard

Gairy Desgouttes

Used 1+ times

FREE Resource

40 questions

Show all answers

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The valence atomic orbitals of two atoms interact through side-by-side overlap when forming a pi bond.

They overlap end-to-end

They overlap side-to-side

They do not overlap at all

They interact via random orientation

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which covalent molecule has the weakest bond?

They are all equally strong

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many single covalent bonds can noble gases typically form?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many sigma bonds are there in a double covalent bond?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A methane molecule consists of one carbon atom and four hydrogen atoms. How many lone pairs of electrons are present in a methane molecule?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Determine whether the nitrogen atom has a complete octet of electrons and determine the number of lone pairs of electrons. Choose the correct answer.

Has a complete octet and one lone pair

Has a complete octet and two lone pairs

Does not have a complete octet and one lone pair

Does not have a complete octet and two lone pairs

OPEN ENDED QUESTION

3 mins • 1 pt

Name the following molecular compounds:

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Chapter Review: Chapter 7

40 questions

The valence atomic orbitals of two atoms interact through side-by-side overlap when forming a pi bond.

Which covalent molecule has the weakest bond?

How many single covalent bonds can noble gases typically form?

How many sigma bonds are there in a double covalent bond?

A methane molecule consists of one carbon atom and four hydrogen atoms. How many lone pairs of electrons are present in a methane molecule?

Determine whether the nitrogen atom has a complete octet of electrons and determine the number of lone pairs of electrons. Choose the correct answer.

Name the following molecular compounds:

Which is the correct formula for the compound nitrogen dioxide?

Which is the correct name for the solution H2SO3(aq)?

It is necessary to use prefixes in naming binary molecular compounds because they indicate the number of each element present.

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