Question

question 15 (5 points) saved for each of the following substances, identify the intermolecular force that predominates: 1. dispersion (london) 2. dipole - induced dipole 3. ion - induced dipole 4. dipole - dipole 5. hydrogen - bond 6. ion - dipole 7. metallic 8. covalent network 9. electrostatic (ionic) 1. f2 2. sio2 3. al2o3 4. nh3 5. icl (iodine chloride)

Explanation:

Step1: Analyze $F_2$

$F_2$ is a non - polar molecule. Non - polar molecules have dispersion (London) forces as the predominant intermolecular force. So for $F_2$, the answer is 1. dispersion (London).

Step2: Analyze $SiO_2$

$SiO_2$ is a covalent network solid. The strong covalent bonds hold the structure together and there are no significant intermolecular forces in the traditional sense among discrete molecules. But considering the options, it doesn't match with the other intermolecular force types, and it is a covalent network structure. So for $SiO_2$, the answer is 8. covalent network.

Step3: Analyze $Al_2O_3$

$Al_2O_3$ is an ionic compound. The predominant force holding it together is the electrostatic (ionic) force. So for $Al_2O_3$, the answer is 9. electrostatic (ionic).

Step4: Analyze $NH_3$

$NH_3$ has a nitrogen atom bonded to hydrogen atoms. Nitrogen is highly electronegative, and $NH_3$ can form hydrogen - bonds. So for $NH_3$, the answer is 5. hydrogen - bond.

Step5: Analyze $ICl$

$ICl$ is a polar molecule. Polar molecules have dipole - dipole forces as the predominant intermolecular force. So for $ICl$, the answer is 4. dipole - dipole.

Answer:

1. $F_2$: 1. dispersion (London)
2. $SiO_2$: 8. covalent network
3. $Al_2O_3$: 9. electrostatic (ionic)
4. $NH_3$: 5. hydrogen - bond
5. $ICl$: 4. dipole - dipole