k up the melting points of the substances in each pair. Circle the formula of th

Question

k up the melting points of the substances in each pair. Circle the formula of the intermolecular substance in each pair which has the lower melting point. Write the forces of the substance on the left in the space to the left of the pair. Write the intermolecular forces of the substance on the right in the space to the right of the pair Write a sentence below each pair explaining why the one with the lower melting point has the weaker intermolecular force. (For example, substance A has a lower molar mass, therefore it has weaker London dispersion forces than substance B. For another example, substance A has a higher molar mass, therefore it has weaker dipole-dipole forces than substance B. For another example, substance A has ionic bonds which are stronger than hydrogen bonds in substance B, therefore substance B has the lower melting point.) All Intermolecular Forces All Intermolecular Forces Pairs HCI or C (diamond) NHs or AsHs Explain: HBr or HF Explain: CH2Cl2 or CHCl3 Explain NaCl or HF Explain C3Hs or C4H10 Explain: PCl3 or SO2 Explain 145

Explanation / Answer

Hydrogen bonding

dipole-dipole interactions

London dispersion forces

dipole-dipole interactions

London dispersion forces

dipole-dipole interactions

London dispersion forces

Hydrogen bonding

dipole-dipole interactions

London dispersion forces

dipole-dipole interactions

London dispersion forces

dipole-dipole interactions

London dispersion forces

Ion-dipole interactions

London dispersion forces

Hydrogen bonding

dipole-dipole interactions

London dispersion forces

All intermolecular forces Pairs All intermolecular forces

Hydrogen bonding

dipole-dipole interactions

London dispersion forces

NH3 or AsH3

dipole-dipole interactions

London dispersion forces

NH3 has stronger ionic hydrogen bonds than AsH3 therefore AsH3 has lower melting point

dipole-dipole interactions

London dispersion forces

HBr or HF

Hydrogen bonding

dipole-dipole interactions

London dispersion forces

HF has stronger ionic hydrogen bonds than HBr therefore HBr has lower melting point

dipole-dipole interactions

London dispersion forces

CH2Cl2 or CHCl3

dipole-dipole interactions

London dispersion forces

CH2Cl2 has lower molar mass and therefore weaker london dispersion forces and hence it has lower melting point

Ion-dipole interactions

London dispersion forces

NaCl or HF

Hydrogen bonding

dipole-dipole interactions

London dispersion forces

HF has lower melting point because NaCl has stronger ionic bonds which are stronger than hydrogen bond in HF

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