Solids, Liquids, and Gases

1
Solids, Liquids, and Gases

• By
• Cindy, Jenalee, Katie

2
Basic Types of Solids

• Ionic Solids-
• Molecular Solids-
• Covalent Network-
• Metallic solids-
• Crystalline-

3
Ionic Solids

• consists of ions which are packed within to make
  the best use of the space.
• maximize the number of ions of opposite charge
  that surround a particular ion.
• regardless of structure and coordination number
  are held together by electrostatic forces.

4
Molecular Solids

• contains efficiently packed molecules and
  intermolecular forces between the molecules

5
Covalent Network

• consists of solely of carbon atoms, where each
  atom is covalently bonded to four other atoms and
  therefore consists of strong bonds.

6
Metallic Solids

• Most elements are in this form.
• almost all of the s-fillers, d-fillers, and
  f-fillers have this form.
• Characteristics- shiny luster, malleability,
  ductility, ability to conduct electricity, and
  tendency to form cations.

7
Crystalline

• based upon a simple pattern of arrangement of
  molecules, which is repeated many times and
  creates boundaries in the material where the
  pattern cannot continue.

8
Basic Crystalline Structures

• These are just some of the basic crystalline
  structures. All of which have a basic geometric
  shape.

9
Cont

• Amorphous
• has no regular arrangement of their molecules and
  appears like a instant photo of a picture.
• Polymerics
• long chain molecules wrapped around each other.
  The chains are made up of repeated monomers.

10
Solid Basics

• Composure
• Elements or compounds inside mixtures
  combinations of different elements and compounds.
• Main Characteristics
• Hold their own shape If put inside a container
  it will not change shape or if a solid is ground
  up the powder will still consist of tiny solids
  that will not change.
• Atoms in Solids
• Not allowed to move around much, no matter how
  small the pieces may be.

11
Temperature Basics of a Solid

• As a liquid state of matter decreases in
  temperature it generally forms a solid state.

12
Liquids

• Liquid State
• Similar to Solids Ability to be compressed and
  associated with somewhat low kinetic energy
• Similar to gases Tends to flow or have fluidity
  and takes on the container its in
• Common Phases
• Melting and freezing Particles travel slowly and
  cant get past one another they settle. Pure
  liquids have a definite freezing point.
• Boiling Point Temperature of liquid at which its
  vapor pressure is equal to the atmospheric
  pressure. The normal boiling point 101.32kPa.

13
Basic Characteristics of a Liquid

• A liquid is formed as the temperature of a solid
  increases and as the temperature of a gas
  decreases.

14
Liquids

• General liquid information
• Molecular Structure
• Flicking cluster theory liquid is a combination
  of solid and gas. For a diagram of the Flicking
  Cluster Theory go to next slide.
• Le Charteliers Principle
• If stress is applied to a system at equilibrium
  the system will tend to readjust so that the
  stress is reduced. Applies to any system in
  equilibrium changes in stress temperature in
  liquids increasing corresponding with vapor
  increase.
• Vapor Pressure
• Pressure exerted by gas phase units that are
  leaving the surface of a liquid, when a substance
  is heated the vapor pressure will increase.

15
Transition Graph

• This graph shows the Flicking Cluster Theory. As
  you can see a liquid is indeed a combination of a
  solid and a gas.

16
Liquids

• Boiling Point Temperature of a liquid at which
  its vapor pressure is equal to the atmospheric
  pressure. The normal boiling point is the
  temperature at which vapor pressure is equal to
  standard atmospheric pressure or 101.32 k. For
  more information on vapor pressure
• Liquid Concepts
• Evaporation
• - Boiling evaporates throughout the
  liquid
• - Freezing Temperature drops so
  equilibrium produces large blocks of solid state,
  totally at the expense of the gas phase

17
Liquids

• Surface Tension
• Energy required to increase the surface area of a
  liquid by a unit amount.
• As shown in this picture the insect floats on
  water due to the immense amount of surface
  tension acting on it.

18
Gases

• Gas Laws
• For a list of different gas laws
• Boyles Law
• Absolute temperature and amount (moles) remain
  the same, this also shows how pressure
  increases/decreases as the volume of gas
  increases and decreases. In other words expresses
  relationship between volume and pressure.

19
Gases

• Charles Law
• Pressure and the amount (Moles) remain the same.
  This expresses volume of gas and its absolute
  temperature.
• Pressure Law
• Expresses the relationship between the pressure
  of a gas and its absolute temperature. The amount
  (Moles) and the volume remain unchanged.

20
Gases

• General gas equation
• It shows the interdependence or relationship
  between
• - The pressure
• - Volume
• - Absolute Temperature of a gas
  when the amount of the gas ( in Moles) is fixed.
• Ideal gas equation
• Mathematical equation is pVnRT
• - Pressure times volume is equal to
  the product pf number of moles, the gas constant
  R and temperature, or pee vee equals en ar tee.

21
Gases

• Avagodros Principle
• This states that Equal volumes of all gases
  under identical conditions of temperature and
  pressure, contain equal number of molecules.
  
• - For an example of this principle
  click -gt

22
Gases

• Daltons Law of Partial Pressures
• This states that if there is a mixture of gases
  which do not react chemically together, than the
  total pressure exerted by the mixture is a sum of
  the partial pressures exerted by the individual
  gases making up the mixture.
• - According to this law, the total
  pressure exerted by a mixture of gases is the sum
  of pressures that each individual gas would exert
  if it were continued alone within a volume
  occupied by the mixture.

23
Example

• This implies that, if there are 2 million
  molecules of oxygen in a 10 liter container at a
  pressure of 5 atm, when the temperature is 300 K,
  there must also be exactly 2 million molecules of
  Carbon Dioxide (another gas) in another 10 liter
  container that has exactly 5 atm of pressure and
  at a temperature of 300 K (the same conditions of
  temperature and pressure). This temperature holds
  true for all gases.

24
Gases

• Mathematically, Daltons Law of Partial Pressure
  is represented as follows the total pressure
  from all the gases making up the mixturethe
  partial pressures exerted separately by the
  individual gases which are represented by four
  letters added together.
• Grahams Law of Diffusion
• This is the law that shows the relationship
  between the rate of diffusion of a gas and its
  density when its temperature and its pressure
  remains constant.

25
Gases

• Basically, it shows the rate of diffusion of
  gases decrease as their densities increase.
• The Concept of Molar Volume
• The molar volume of a gas is the volume occupied
  by the one mole of that gas at standard
  temperature and pressure, and this volume is
  numerically equal to 22.41 liters (dm3). This is
  true of all gases. For a great example?

26
Example of Molar Volume

• This implies that at Standard Temperature and
  Pressures (STP), 71.0 g of Chlorine gas (1 mole
  of Chlorine molecules) will occupy a volume of
  22.41 L.
• In addition, 44.0 g of Carbon Dioxide (1 mole of
  carbon dioxide molecules) will also occupy a
  volume of 22.41 L at STP.

27
Gases

• At standard temperature and pressure the value of
  the temperature is (273 K). The pressure is at
  one atmosphere.
• Characteristics of a gas
• A gas when poured into a container, fills the
  container and takes the shape of the container.
• Gas is compressible
• The force that the gas exerts per unit area of
  the container is known as the gas pressure. This
  force is constant for every unit area of the
  walls of the container within the gas is enclosed.

28
Gas Movement

• The Molecules of a gas move freely, therefore
  taking the shape of a sealed container.

29
Basic Characteristics of a Gas

• As the temperature of the liquid state increases
  a gas is formed. Also, the molecules within the
  container move faster as the temperature
  increases.