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Chapter 10 Chemistry

TermDefinition
Kinetic Molar Theory the idea that particles of matter are always in motion
Ideal Gas a hypothetical gas that fits all the assumptions of the KMT (does not exist)
Assumption 1 gases consist of large numbers of tiny particles that are far apart relative to their size
Assumption 2 collisions between gas particles and with the container are completely elastic
Since The Volume Of An Ideal Gas Is 0... they have low densities and high compressibility
Elastic Collision a collision where there is no loss of total kinetic energy
In An Elastic Collision, The Energy Must... remain constant as long as the temperature is constant
Assumption 3 gas particles are in continuous, rapid, random motion
Kinetic Energy & IMFA Are Related Because... kinetic energy must overcome IMFA
Assumption 4 there are no attractive forces between gas particles
The 4 IMFAs In Order From Strongest To Weakest ion-ion > h-bonding > dipole > dispersion
There Are IMFA Forces In Gases Because… all gases have IMFA
Assumption 5 temperature depends on the average amount of kinetic energy
Gas Will Behave Nearly Ideal When... it has a high temperature and low pressure
Gas Will Deviate From Ideal Behavior When... the polarity and IMFA get higher/stronger
Expansion when gas spreads out and fills a container (3&4)
Fluidity the ability of particles to slide past each other when KE overcomes IMFA (4)
Low Density small mass in large volume (1)
High Compressibility lots of empty space between particles can be pushed close together (1)
Diffusion random scattering of gas particles (3)
Effusion gas particles escape through a hole (3)
There Are Less Liquids Then Solids & Gases Because... they have a small temperature range
Properties Of A Liquid Are... definite volume, take shape of container, particles vibrate and slide, space between particles, high density
Fluid substances flow and make the shape of the container
S.L.G. IMFA Forces Strongest To Weakest solid (closest together) > liquids > gases (farthest apart)
Liquids Are Incompressible Because... there is little to no empty space between particles
Liquids Can Diffuse Because... there is a constant and random motion of particles
To Make A Substance Diffuse Faster... increase temperature to increase the average KE speed
Surface Tension the tension of the surface film of a liquid due to the attraction of surface particles
Surface Particles Are Pulled... by net inward force (to the sides and down)
Inner Particles Are Pulled... in all directions equally
The Cause Of Surface Tension Is... unbalanced forces on the surface particles
Tension Has A Direct Relationship With... IMFA
Capillary Action attraction of a liquid to the surface of a solid
Adhesive Forces (smile) attraction between liquid and container
Cohesive Forces (frown) attraction of liquid to itself
Evaporation process by which particles escape from a non-boiling liquid to a gaseous state
Evaporation Qualities occurs @ all temps, must overcome IMFA, energy from collsions, occurs on surface
Boiling rapid conversion from liquid to gas
Boiling Qualities occurs @ BP, must overcome atmospheric pressure, energy comes from an outside source, occurs all over
Amorphous vs Crystalline Solid amorphous has a solid arrangement and melts over a range while crystalline solids are geometric and have a distinct melting point
Definite Volume the container won't make a difference in the volume
Low Diffusion Rate particles do not move from their fixed positions
Metallic Crystal Solid held together by delocalized electrons / good conductor, insoluble, MP varies / example: gold (Au)
Ionic Crystal Solid held together by electrostatic force of attraction / forms crystal lattice, soluble, high MP / example: NaCl (table salt)
Covalent Network Crystal Solid held together by covalently bonds with neighbors / one giant molecule, insoluble, high MP / example: SiO2 (sand)
Covalent Molecular Crystal Solid held together by weak IMFA forces (dispersion,dipole-dipole,h-bonding) / polar & non-polar, soluble in similar substances, low MP / example: SiO2 (sand)
Supercooled Liquid a substance that looks solid but also has some liquid properties
Molecules With Less Mass... will move faster than those with greater mass
Gases Will Effuse Faster When... their molar weight is lower
If Two Gases Are Injected Into Opposite Sides Of A Tube... they will mix closer to the gas with greater volume/mass
Relationship Between Temperature And Average Particle Speed In A Gas higher temperature, faster speed
Intra vs Inter Molecular Forces intra: within a particle // inter: between particles
Polar vs Non-Polar Evaporation Speed polar liquids have higher IMFA to overcome, so they are slower to evaporate
Conductors Of Electricity metallic solids only
Soluble In Water ionic solids only
Amorphous Solids not very compressible, undefined shape, can be a supercooled liquid, clear melting point
Crystalline Solids compressible, defined shape, can not be a supercooled liquid, unclear melting point
The More Free Electrons... the higher the electric conductivity
Physical Change chemical compound is not effected
Liquids Form A Meniscus Because... when one molecule sticks to the container, the others cling to it
Vapor Pressure the pressure exerted by its vapor at equilibrium
# Particles Entering The Vapor Phase Equals... # particles leaving vapor phase
Rate Of Evaporation Equals... rate of condensation
If More Particles Enter The Vapor Phase... it reaches a high equilibrium (more particles can overcome IMFA to escape to vapor)
Volatile evaporates easily
Non-Volatile does not evaporate easily
Boiling Defined Using Vapor Pressure Is... when the vapor pressure of a liquid equals the atmospheric pressure
As P-atm Increases, Boiling Point... increases (takes more energy to boil)
As P-atm Increases, Altitude... decreases
As Altitude Increases, Boiling Point decreases
The Property Boiling Depends On Is... IMFA
As Boiling Point Increases, IMFA... gets stronger
Normal Boiling Point Is Found At Standard... pressure (1atm = 101.3kPa = 760 torr - 760 mmHg)
With Pressure, Boiling Points... vary greatly
With Pressure, Melting Points... do not vary greatly
The State On The Bottom Line Of A Heating Curve Is... solid (q=mtΔt)
The State On The First Plateau Of A Heating Curve Is... melting/freezing (q=mHf)
Melting/Freezing Is Also Referred To As... fusion
The State On The Middle Line Of A Heating Curve Is... liquid (q=mcΔt)
The State Of The Second Plateau Of A Heating Curve Is... boiling/condensing (q=mHv)
Boiling/Condensing Is Also Referred To As... vaporization
The State On The Top Line Of The Heating Curve Is... gas (q=mcΔt)
On The Heating Curve, Temperature Changes... on the lines (solid,liquid,gas)
On The Heating Curve, Temperature Does Not Change... on the plateaus (fusion,vaporization)
The Standard Melting/Freezing Point Is... 0 degrees
The Standard Boiling/Condensing Point Is... 100 degrees
Potential Energy the energy of matter based on its position
Heat Of Fusion energy needed to melt 1 gram of a substance at its MP
Heat Of Vaporization energy needed to boil 1 gram f a substance at its boiling point
The Unique Characteristics Of Water Are Caused By Its... structure with large empty spaces with low density
Water Molecules Are Polar Because... the two hydrogen atoms are linked to the oxygen atom by polar covalent bonds / unequal distribution of electrons
Ice Floats In Water Because... it is less dense / lower polarity
It Takes More Energy To Boil Because... it has to overcome IMFA
Exposure To Steam Is Dangerous Because... it has lots of energy
Water's Unique Properties Are... high heat fusion / high heat vaporization / radiator (steam releases heat) / high specific heat
Weather If Affected By... specific heat
Dipole-Dipole Forces Are Between... two non-metal atoms
Ion-Ion Forces Are Between a metal & a non-metal
Primary Dispersion Forces Are In... non-polar covalent compounds & single atom molecules
Hydrogen Bonding Is Between... hydrogen and oxygen, nitrogen, or flourine
High Density close arrangement of liquid particles
Delocalized Electrons free moving electrons
The States That Exist At The Triple Point Are... solid, liquid, & gas
The Critical Point Is... the temperature at which a substance will always be a gas regardless of the pressure
Sublimation the phase change from a solid straight to a gas
Deposition the phase change from a gas straight to a solid
S.L.G. Speed Of Diffusion Fastest To Slowest gas (weak IMFA) > liquid > solid (strong imfa)
Amorphous Solid Can Act As A Liquid Because... their particles flow around
Properties Of A Solid definite volume, tightly packed particles, strong IMFA, low rate of diffusion, vibrating particles
Standard Atmospheric Pressure (kPa) 101.3
During Boiling, The Kinetic Energy Must... completely break IMFA
Super Critical Fluid has both properties of liquids & gases
Critical Point gas, liquid, & super critical fluid meet
Created by: abievans
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