Good Morning! 05/03/23• Today we will…

–Be working through the notes for Chapter 10.–The Chapter 10 Packet is going to be due on

Monday, not Friday as the schedule suggests.

–We have Advisory today, the 25 minute variety

–We will be working on the notes in groups on the Laptops. Explanation will be on the next slide

To Access the Powerpoint…

• Log on first (the laptops must be connected to the internet)

• Then open the Folder names “Shortcut to Science Shares”

• In this folder open up “Durand”• Then Chem then States of Mater.• Finally click on the ppt named Ch 10

notes.

Chapter 10 Notes

Necessary Assumptions of Kinetic Theory

Gases are composed of

particles that are very small, hard

spheres that are relatively

far apart.

There is lots of empty space between the gas particles.

There is no significant attractive or repulsive force between the gas particles.

The gas particles move rapidly in constant random motion in a straight line.

This is called a random walk.

Gas particles only change direction if they collide

with another gas particle or the wall of the

container.

All collisions are perfectly elastic. In other words,

kinetic energy is transferred without any

loss in the collision.

Uncontained gases can diffuse into space without

limit. • Link to Video

Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing.

DiffusionDiffusion

PressurePressureis equal to force/unit areaSI units = Newton/meter2 = 1 Pascal (Pa)

AreaForce Pressure

meter square 1Newton 1 Pascal1

AF P

1 standard atmosphere = 101.3 kPa1 standard atmosphere =

1 atm =760 mm Hg = 760 torr

Measuring PressureMeasuring PressureThe first device for measuring atmosphericpressure was developed by Evangelista Torricelli during the 17th century.The device was called a “barometer”

Baro = weight Meter = measure

An Early An Early BarometerBarometer

The Aneroid BarometerThe Aneroid Barometer

Standard Temperature and Standard Temperature and PressurePressure “STP”“STP”

P = 1 atmosphere, 760 torr T = C, 273 Kelvins The molar volume of an ideal gas is 22.42 liters at STP

Converting Pressure Units.

1 atmosphere (Atm) = 760 mm Hg (Torr) =

101.3 kiloPascals(kPa)Convert 2.5 atm to kPa

2.5 atm

x101.3 kPa

1 atm= 253.25kPa

Vaporization:

Changing state from a liquid to a gas phase by heating.

Evaporation:When vaporization occurs at any temperature.

Only occurs at the surface of a liquid.

Triple Point: The conditions necessary for a substance to be in equilibrium with all its

phases. (Solid, Liquid, Gas)

All phases exist at the same time!

Liquid gas = gas liquidSolidliquid = liquidsolid Solidgas = gassolid

Phase changes by Name

Sublimation: Occurs when a solid changes directly to a gas phase

without passing through the liquid state.

Example: (Dry Ice)

Sublimation happens to solids that have high vapor

pressure.

Phase changes by Name

Carbon dioxide CCaarrbboonn

ddiiooxxiiddee

Water

WWaatteerr

CarbonCCaarrbboonn

Kinetic Theory and SolidsMotion is vibration or

rotation of atoms around a fixed point.

Solid: Have a fixed mass and volume.

True Solid: A substance that has a fixed melting

point.

Amorphous Solid: Disordered arrangement of the particles resulting in a solid that has no definite

melting point. 

Glass is an amorphous solid.(Has a very high viscosity)

Types of Solids

Amorphous solids: considerable disorder in their structures (glass).

Resistance to flow (molecules with large intermolecular forces).

Viscosity

Representation of Components in a Crystalline Solid

The spheres represent atoms, ions, or molecules that make up the substance.

Lattice: A 3-dimensional system of points designating the centers of components

Unit Cell: Smallest group of atoms that can make a geometric arrangement.

Simple-cubic

Body-centered

Face-centered

Allotropes: Different molecular forms of the same element in the

same physical state.Graphite Diamond