Bond Type and Intra and Intermolecular Forces

The forces that hold the atoms in a CCl₄ molecule together are _______, and the forces that hold the molecules together in sample are _________.

• intermolecular (covalent); intramolecular (dipole-dipole)

• intermolecular (dipole-dipole); intramolecular (dipole-dipole)

• intramolecular (covalent); intermolecular (London Dispersion)

• intramolecular (covalent); intermolecular (dipole-dipole)

This is an example of a __________ bond.

• non-polar covalent
• polar covalent
• ionic
• metallic

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

If students want to determine the strength of intermolecular forces among bond type, how should they go about doing this?

• Compare three different ionic compounds to determine the rate of dissolving.

• Use a magnifying glass to examine the intermolecuar forces in an ionic, polar and non polar covalent bond.

• Compare the conductivity of an ionic and non polar bond.

• Determine the melting point of an ionic, polar, and non polar bond.

Tags

NGSS.HS-PS1-3

Place the following compounds in order of increasing intermolecular forces.

Viscosity Compound

455 vegetable oil

10.5 water

5.0 isoproply alcohol

• vegetable oil, water, isoproply alcohol

• isoproply alcohol, water, vegetable oil

• water, isoproply alcohol, vegetable oil

• vegetable oil, isoproply alcohol , water

An unknown powder has been discovered in the kitchen. Before it can be used for cooking it must be identified. Is the unknown powder NaCl, C₁₂H₂₂O₁₁, or NaHCO₃?

The unknown powder is soluble in water but not soluble in oil. The unknown powder does not conduct electricity when dissolved in water and has a low melting point.

• The powder is NaCl or NaHCO₃ because they are both ionic.

• The powder is NaCl or NaHCO₃ because they are both covalent.

• The powder is C₁₂H₂₂O₁₁ because it is the only ionic formula.

• The powder is C₁₂H₂₂O₁₁ because it is the only covalent formula.

Why is this figure representative of a polar covalent molecule?

• Electrons are being shared equally due to the partial positive and negative charges.

• Electrons are being shared unequally due to the partial positive and negative charges.

• Electrons are being transferred due to partial positive and negative charge.

• Electrons are being transferred due to full positive and negative charge.

Tags

NGSS.HS-PS1-2

Why does this figure represent an ionic molecule?

• Electrons are shared equally due to positive and negative charge

• Electrons are shared unequally due to positive and negative charge

• Electrons are transferred due to positive and negative charge

Tags

NGSS.HS-PS1-3

If a substance conducts electricity in water, what type of bond is being described?

• ionic because ions are free to move and conduct electricity

• polar because ions are free to move and conduct electricity

• ionic because no ions are formed

• polar because no ions are formed

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-3

Which test would be used to determine the strength of intermolecular forces?

• color

• luster

• melting point

• solubility in water

Tags

NGSS.HS-PS1-3

Based on the data in the table, identify the bond type in each substance.

Substance Dissolves in water Electrolyte

1. CaCl₂ Yes Yes

2. Cl₂ No No

3. LiCl Yes Yes

• Substance 1, 2, and 3 are all covalent compounds because they all contain chlorine.

• Substance 1 and 3 are strong bonds and ionic. This is known because they form electrolytes in water which means that there are positive and negative ions forms. Substance 2 is non polar because it is not soluble in water.

• Substance 1 and 3 are weak bonds and covalent since they dissolve in water. Substance 2 is strong and ionic because it does not dissolve in water.

• Substance 1 and 3 are weak bonds and ionic since they dissolve in water. Substance 2 is strong and covalent because it does not dissolve in water.