How can electronegativity be used to distinguish between an ionic bond and a covalent bond?

By determining the difference in electronegativity

Electron distribution in a polar-covalent bond results in:

Electron density is greater around the more electronegative atom, giving it a partial negative charge.

Electrons are equally shared, resulting in no partial charges.

Electrons are more around the less electronegative atom, giving it a partial positive charge.

Electrons are transferred completely, resulting in full charges.

Use the concept of potential energy to describe how a covalent bond forms between two atoms.

Electron-proton attraction is stronger than electron-electron and proton-proton repulsions.

Atoms repel each other and potential energy increases.

Electron-electron attraction is stronger than electron-proton attraction.

Potential energy is at maximum when atoms are far apart.

Identify the correct Lewis structure for water (H₂O).

H-O-H with two lone pairs on oxygen

H-O-H with one lone pair on oxygen

H-O-H with three lone pairs on oxygen

The lattice energy of compound A is greater in magnitude than that of compound B. What can be concluded from this fact?

It will be more difficult to break the bonds in compound A than those in compound B.

Compound A is not an ionic compound.

Compound B has larger crystals than compound A.

Compound A has larger crystals than compound B.

The forces of attraction between molecules in a molecular compound are generally

weaker than the attractive forces among formula units in ionic bonding.

stronger than the attractive forces among formula units in ionic bonding.

approximately equal to the attractive forces among formula units in ionic bonding.

What types of bonds are present in an ionic compound that contains a polyatomic ion?

Covalent bonds within the polyatomic ion and ionic bonds with other ions

Which of the following is the correct Lewis structure for the ammonium ion (NH₄⁺)?

N with four single bonds to H and a positive charge

N with three single bonds to H and a lone pair

N with two single bonds to H and two lone pairs

N with four single bonds to H and a negative charge

What is the correct Lewis structure for the sulfate ion (SO₄²⁻)?

S with two double bonds to O and two single bonds to O

S with four single bonds to O and a positive charge

S with three single bonds to O and one double bond to O

In metals, the valence electrons are considered to be

shared by all surrounding atoms.

attached to particular positive ions.

Which of the following is true about the melting point of metals compared to ionic compounds?

Metals have a low to high melting point, while ionic compounds have a high melting point.

Metals have a high melting point, while ionic compounds have a low melting point.

Both metals and ionic compounds have a low melting point.

Both metals and ionic compounds have a high melting point.

Identify the major assumption of the VSEPR theory, which is used to predict the shape of atoms.

Pairs of valence electrons repel one another.

Pairs of valence electrons attract one another.

Pairs of valence electrons do not interact.

Pairs of valence electrons form ionic bonds.

Chemical Bonding Test Review

Authored by Cassie Floyd

Chemistry

10th Grade

NGSS covered

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A chemical bond between atoms results from the attraction between the valence electrons and ____ of different atoms.

nuclei

inner electrons

isotopes

Lewis structures

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A covalent bond consists of

a shared electron.

a shared electron pair.

two different ions.

an octet of electrons.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

If two covalently bonded atoms are identical, the bond is identified as

nonpolar covalent.

polar covalent.

ionic.

dipolar.

A covalent bond in which there is an unequal attraction for the shared electrons is

nonpolar.

polar.

ionic.

dipolar.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Atoms with a strong attraction for electrons they share with another atom exhibit

zero electronegativity.

low electronegativity.

high electronegativity.

Lewis electronegativity.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Bonds that possess between 5% and 50% ionic character are considered to be

ionic.

pure covalent.

polar covalent.

nonpolar covalent.

The electrons involved in the formation of a chemical bond are called

core electrons.

valence electrons.

free electrons.

bound electrons.

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Chemical Bonding Test Review

A chemical bond between atoms results from the attraction between the valence electrons and ____ of different atoms.

A covalent bond consists of

If two covalently bonded atoms are identical, the bond is identified as

A covalent bond in which there is an unequal attraction for the shared electrons is

Atoms with a strong attraction for electrons they share with another atom exhibit

Bonds that possess between 5% and 50% ionic character are considered to be

The electrons involved in the formation of a chemical bond are called

A chemical bond that results from the electrostatic attraction between positive and negative ions is called a(n)

If electrons involved in bonding spend most of the time closer to one atom rather than the other, the bond is called a:

If a bond's character is more than 50% ionic, then the bond is called a(n):

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