Physical Pharmacy - Lecture 1
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Questions and Answers

Which state of matter has a definite shape and volume?

  • Solid (correct)
  • Plasma
  • Liquid
  • Gas

What is the primary property of gases regarding their shape and volume?

  • Indefinite shape and indefinite volume (correct)
  • Definite shape and indefinite volume
  • Indefinite shape and definite volume
  • Definite shape and volume

How do the particles in a liquid behave compared to those in a solid?

  • Particles in liquids have moderate proximity and are disordered (correct)
  • Particles in liquids are very close and have a definite shape
  • Particles in liquids are closer and more ordered
  • Particles in liquids are far apart and completely disordered

What type of forces holds matter together?

<p>Chemical or intramolecular forces (B)</p> Signup and view all the answers

Which of the following best describes the characteristics of solids?

<p>Definite shape, definite volume, and low compressibility (B)</p> Signup and view all the answers

Which state of matter is characterized by taking the shape of its container but maintaining a fixed volume?

<p>Liquid (C)</p> Signup and view all the answers

What happens to the proximity of particles as matter transitions from solid to gas?

<p>Particles move farther apart. (B)</p> Signup and view all the answers

Which property differentiates gas from both solid and liquid states significantly?

<p>Gas is easily compressible. (C)</p> Signup and view all the answers

What type of forces exist between molecules in different states of matter?

<p>Intermolecular forces (A)</p> Signup and view all the answers

Which statement accurately describes the intermolecular forces in solids?

<p>They are strong enough to lock molecules in place. (D)</p> Signup and view all the answers

What is the typical strength range of van der Waals' forces?

<p>1-10 Kcal/mole (A)</p> Signup and view all the answers

What happens to the average kinetic energy of gas molecules compared to other states of matter?

<p>It is much larger than in solids and liquids. (D)</p> Signup and view all the answers

How much energy is typically required to separate molecules compared to breaking covalent bonds?

<p>16 kJ/mol (B)</p> Signup and view all the answers

What leads to the formation of dipoles in asymmetrical molecules?

<p>Unbalanced distribution of electrons (A)</p> Signup and view all the answers

What is the relationship between intermolecular forces and temperature?

<p>Higher temperature decreases the strength of intermolecular forces. (C)</p> Signup and view all the answers

Which of the following best describes van der Waals' forces?

<p>They are weak forces caused by fluctuations in electron density. (C)</p> Signup and view all the answers

What is cohesion?

<p>The physical force between molecules of the same substance. (B)</p> Signup and view all the answers

How is a molecule defined in the context of atomic interactions?

<p>A unit formed by strong attractive forces creating observable properties. (B)</p> Signup and view all the answers

What characterizes ionic bonding?

<p>The transfer of electrons resulting in charged ions. (B)</p> Signup and view all the answers

At equilibrium, what occurs between attractive and repulsive forces?

<p>Attractive and repulsive forces are equal. (D)</p> Signup and view all the answers

Which of the following correctly describes covalent bonding?

<p>Is characterized by the sharing of electrons between non-metal atoms. (A)</p> Signup and view all the answers

What is a common property of ionic compounds at room temperature?

<p>They exist as crystalline solids. (A)</p> Signup and view all the answers

What occurs when attractive forces are strong enough to bind atoms into a molecule?

<p>A chemical bond is formed. (A)</p> Signup and view all the answers

Which describes the nature of repulsive forces at the molecular level?

<p>They raise potential energy and create a barrier. (A)</p> Signup and view all the answers

What type of Van der Waals force occurs between two permanent dipoles?

<p>Dipole-dipole (A)</p> Signup and view all the answers

Which of the following is an example of a scenario where dipole-induced dipole forces occur?

<p>A polar molecule interacting with a non-polar molecule (C)</p> Signup and view all the answers

What is the primary characteristic of London dispersion forces?

<p>They can occur between non-polar molecules. (C)</p> Signup and view all the answers

Which of the following correctly describes dispersion forces?

<p>They are the weakest and very short-lived. (B)</p> Signup and view all the answers

In which scenario do dipole-dipole interactions typically manifest?

<p>Between two polar molecules. (B)</p> Signup and view all the answers

Which interaction causes a temporary dipole to form in a non-polar molecule?

<p>Dipole-induced dipole force (D)</p> Signup and view all the answers

What distinguishes London dispersion forces from the other types of intermolecular forces?

<p>They occur due to instantaneous dipoles. (C)</p> Signup and view all the answers

Which of the following statements is true regarding the types of intermolecular forces?

<p>Dipole-induced dipole forces involve a temporary dipole in a non-polar molecule. (D)</p> Signup and view all the answers

Flashcards

Solid

A form of matter that is relatively incompressible and has a fixed shape and volume, like ice.

Liquid

A form of matter that is relatively incompressible, has a fixed volume but no fixed shape, like water in a bottle.

Gas

A form of matter that is easily compressible, has no fixed shape or volume and takes up all the space in a container, like air.

Intramolecular force

The force between atoms within a molecule, holding them together.

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Adhesion

The force of attraction between unlike molecules.

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Cohesion

The force of attraction between like molecules.

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Mass

The amount of matter in an object.

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Volume

The amount of space an object occupies.

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Chemical Bond

Attractive forces that are strong enough to form a new molecular unit.

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Non-bonding attraction

Attractive forces that are not strong enough to form a new molecular unit.

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Ionic Bonding

The electrostatic force of attraction between positively and negatively charged ions. It occurs between non-metals and metals.

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Covalent Bonding

Occurs between atoms with a small difference in electronegativity, which are close to each other in the periodic table. It happens between non-metals and non-metals.

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Electron Transfer

The transfer of electrons between two atoms with a large difference in electronegativity.

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Electron Sharing

The sharing of electrons between atoms.

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Dipole-Dipole Forces

The attractive force between two permanent dipoles, where the positive end of one dipole aligns with the negative end of the other.

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Dipole-Induced Dipole Forces

The attractive force between a permanent dipole and a temporarily induced dipole. The permanent dipole induces a temporary dipole in the other molecule by distorting its electron cloud.

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London Dispersion Forces

The weakest type of Van der Waals force, occurring due to temporary fluctuations in electron distribution within non-polar molecules. This creates short-lived, temporary dipoles that can attract each other.

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Van der Waals-Keesom Force

The force existing between two molecules with permanent dipoles.

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Van der Waals-Debye Force

The force existing between a permanent dipole and an induced dipole.

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Van der Waals-London Force

The force existing between two instantaneously induced dipoles.

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London Dispersion Forces

Attractive forces that occur between neutral molecules due to temporary fluctuations in electron distribution.

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London Dispersion Forces

The weakest type of intermolecular force that arises from temporary fluctuations in electron distribution.

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Kinetic energy

The energy of motion of molecules. The higher this energy, the faster and more randomly molecules move, and the less likely they are to be held together by intermolecular forces.

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Dipole-dipole interactions

Attractions between polar molecules, where the positive end of one molecule is attracted to the negative end of another.

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Hydrogen bonding

Attractions between polar molecules and molecules that can form temporary dipoles. This is a stronger force than London Dispersion forces.

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Study Notes

Physical Pharmacy - Lecture 1

  • The lecture is an introduction to physical pharmacy.
  • The syllabus topics will cover:
    • State of matter
    • Thermodynamics
    • Solutions of non-electrolytes
    • Solution of electrolytes
    • Ionic equilibria
    • Buffer & Isotonic solution

Matter

  • All matter is composed of small particles (atoms, molecules, or ions).
  • Matter exists in three states: solid, liquid, and gas.

States of Matter

  • Solid: Particles are tightly packed in a regular pattern, vibrate but cannot move past each other. Solids maintain their shape.
  • Liquid: Particles are close together with no regular pattern, flow and can easily move or slide past each other. Liquids take the shape of their containers.
  • Gas: Particles are well separated with no regular pattern, vibrate freely at high speeds. Gases take the shape of their containers.

Particle Properties

  • Solid: Proximity - close; Energy - little; Order - ordered; Volume - definite; Shape - definite
  • Liquid: Proximity - close; Energy - moderate; Order - disordered; Volume - definite; Shape - indefinite
  • Gas: Proximity - far apart; Energy - a lot; Order - very disordered; Volume - indefinite; Shape - indefinite

Measuring Matter

  • Volume: Measured using a measuring cup.
  • Mass: Measured using a balance or scale.

Binding Forces

  • All matter is held together by a force.
  • The force between atoms within a molecule is a chemical, or intramolecular force.
  • The force between molecules is a physical, or intermolecular force.

Repulsive and Attractive Forces

  • All particles exert both attractive and repulsive forces on each other.
  • If attractive forces are strong, the result is a chemical bond (molecule).
  • If forces are not strong enough to bind into a new unit, it is a non-bonding attraction.
  • Repulsion and attraction forces lead to an equilibrium state.

Intramolecular Forces

  • Ionic Bonding: Electrostatic force of attraction between positively and negatively charged ions (between non-metals and metals). These are generally crystalline solids. (e.g. NaCl).
  • Covalent Bonding: Sharing of electrons (s and p electrons) between atoms (between non-metals).

Intermolecular Forces

  • Forces between molecules.
  • The average kinetic energy of gas molecules is larger than the attraction's energy between them.
  • Liquids have stronger intermolecular forces than gases, holding molecules close together.
  • Solids have the strongest intermolecular forces, locking molecules in place.

Heating Curve

  • Represents the change in temperature of a substance as it is heated.
  • Different phases are seen as it changes from solid to liquid and then to vapor.

Types of Intermolecular Forces

  • Van der Waals forces:
    • Dipole-Dipole forces (e.g., HCI, CH3F)
    • Dipole-Induced Dipole forces (e.g., polar and non-polar molecules)
    • Dispersion/London forces (e.g., non-polar molecules).

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Physical Pharmacy Lecture 1 PDF

Description

This quiz covers the introduction to physical pharmacy, focusing on the states of matter and fundamental properties of different phases. Explore topics including thermodynamics, solutions of non-electrolytes and electrolytes, ionic equilibria, and buffers. Ideal for students beginning their journey in pharmacy studies.

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