Question

you can use this periodic table during the quiz. however, as stated in the course outline, and in the orientation session, this quiz is not open book. you cannot access course material while you write the quiz. nor can you google your answers, work as a group, use a cheat sheet, etc. question 15 (5 points) 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) al2o3 sio2 nh3 f2 icl (iodine chloride) you can use this periodic table during the quiz. however, as stated in the course outline, and in the orientation session, this quiz is not open book. you cannot access course material while you write the quiz. nor can you google your answers, work as a group, use a cheat sheet, etc.

Explanation:

Step1: Analyze $Al_2O_3$

$Al_2O_3$ is an ionic compound. Ions are held together by electrostatic (ionic) forces.

Step2: Analyze $SiO_2$

$SiO_2$ is a covalent - network solid. The main force is covalent bonding throughout the network.

Step3: Analyze $NH_3$

$NH_3$ has N - H bonds. Nitrogen is highly electronegative, so hydrogen - bonding is the predominant intermolecular force.

Step4: Analyze $F_2$

$F_2$ is a non - polar molecule. The predominant intermolecular force is dispersion (London) forces.

Step5: Analyze $ICl$

$ICl$ is a polar molecule. The predominant intermolecular force is dipole - dipole force.

Answer:

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