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(a)
Interpretation:
Interpret major type of intermolecular forces between HCl.
Concept Introduction:
Intermolecular forces are the forces responsible for the interaction between the neighbouring particles or these are the forces present between the molecules. The name intermolecular indicates the forces present between the atoms or ions. The main intermolecular forces are:
Dipole-dipole forces
These forces are the interaction present between the polar molecules.
London dispersion forces
These forces are the forces known for short term attraction due to unequal distribution of electron.
Hydrogen bond
These forces exist between hydrogen and the atom which is highly electronegative in nature not directly associated or bonded with it.
(b)
Interpretation:
Interpret major type of intermolecular forces between MgF2.
Concept Introduction:
Intermolecular forces are the forces responsible for the interaction between the neighbouring particles or these are the forces present between the molecules. The name intermolecular indicates the forces present between the atoms or ions. The main intermolecular forces are:
Dipole-dipole forces
These forces are the interaction present between the polar molecules.
London dispersion forces
These forces are the forces known for short term attraction due to unequal distribution of electron.
Hydrogen bond
These forces exist between hydrogen and the atom which is highly electronegative in nature not directly associated or bonded with it.
(c)
Interpretation:
Interpret major type of intermolecular forces between PBr3.
Concept Introduction:
Intermolecular forces are the forces responsible for the interaction between the neighbouring particles or these are the forces present between the molecules. The name intermolecular indicates the forces present between the atoms or ions. The main intermolecular forces are:
Dipole-dipole forces
These forces are the interaction present between the polar molecules.
London dispersion forces
These forces are the forces known for short term attraction due to unequal distribution of electron.
Hydrogen bond
These forces exist between hydrogen and the atom which is highly electronegative in nature not directly associated or bonded with it.
(d)
Interpretation:
Interpret major type of intermolecular forces between NH3.
Concept Introduction:
Intermolecular forces are the forces responsible for the interaction between the neighbouring particles or these are the forces present between the molecules. The name intermolecular indicates the forces present between the atoms or ions. The main intermolecular forces are:
Dipole-dipole forces
These forces are the interaction present between the polar molecules.
London dispersion forces
These forces are the forces known for short term attraction due to unequal distribution of electron.
Hydrogen bond
These forces exist between hydrogen and the atom which is highly electronegative in nature not directly associated or bonded with it.
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Chapter 10 Solutions
Pearson eText Basic Chemistry -- Instant Access (Pearson+)
- Identify the kinds of intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding) that are important in each of the following substances. (a) propane (C3H8) (b) ethylene glycol [HO(CH2)2OH] (c) cyclohexane (C6H12) (d) phosphine oxide (PH3O) (e) nitrogen monoxide (NO) (f) hydroxylamine (NH2OH)arrow_forwardIdentify the kinds of forces that are most important in holding the particles together in a crystalline solid sample of each of the following substances. (a) Kr (b) HF (c) K2O (d) CO2 (e) Zn (f) NH3arrow_forwardWhat would be the predominant force of attraction between molecules of CS2? Dipole-dipole forces Covalent bonding Hydrogen bonding London dispersion forcesarrow_forward
- Which of the following molecules will exhibit intermolecular hydrogen bonding? NH i ii i iv O I and III O Il and IV O Il and III O II, III, and IVarrow_forwardWhich of the substances has polar interactions (dipole–dipole forces) between molecules? CHF3 CCl4 SO2 H2 HBrarrow_forwardDetermine the electronegativity difference and the molecular polarity (P for polar and NP for nonpolar) of the following compounds then further classify the dominant intermolecular forces of attraction exhibited. Place HB for hydrogen bonding, LDF for London dispersion force, DD for dipole-dipole and ID for the ion-dipole bond. The first one is already done for you. 1.78 | P | hydrogen fluoride | HB 02 C2H6 NH4 H2O I2 HFarrow_forward
- Complete the table Solid Liquid Gas Plasma Rigid Free-flowing Diffuses Freely Strong bonds Weak bonds No bonds Ionization Has definite volume and shape Has definite volume and no definite shape Has no definite shape and volume Has no definite shape and volume High density Moderate density Low density Less than the density of gas Has the least intermolecular space Moderate intermolecular space Free-flowing intermolecular space High intermolecular force of attraction Moderate intermolecular force of attraction Weak intermolecular force of attraction Incompressible Difficult to compress Highly compressible Atoms to have a small vibration, but they remain fixed in their positions. Atoms to vibrate, move about, and slide pass each other Atoms vibrate and move freely at high speeds Low kinetic energy Moderate kinetic energy kinetic energy High kinetic Energy Extremely high kinetic…arrow_forwardintermolecular forces between Cl2 Cl2, H2O H2O, HBr HBr, HF HFarrow_forwardIndicate the type of intermolecular forces each would have to form their structural arrangement. H2O CO2 SiO2 H2S X6arrow_forward
- List down the intermolecular forces present in each species. HBr CS₂ C₂H6 CH3COOH Br2arrow_forwardWhich of the following molecules has the least polarity? NH3 HI Br₂ HBr ⒸHCIarrow_forwardHydrogen bonding occurs between O oxygen atoms of different water molecules hydrogen and oxygen of the same water molecule a hydrogen on one water molecule and an oxygen on another water molecule O hydrogen atoms of different water moleculesarrow_forward
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