BELL RINGER Explain, in terms of particles and energy, the different states of matter.

Name: BELL RINGER Explain, in terms of particles and energy, the different states of matter.
Uploaded: 2017-07-14T06:36:58+00:00
Duration: PTM28S19
Channel: Denis Eaton
Description: BELL RINGER Explain, in terms of particles and energy, the different states of matter.

Matter & Energy

MATTER & ENERGY MATTER - ENERGY - anything that has mass and volume
the ability to do work

Matter Mixture Pure Substance Homogeneous Mixture Heterogeneous
Can it be physically separated? YES NO Mixture Pure Substance Can it be chemically decomposed? Is the composition uniform? Yes No Yes No Homogeneous Mixture Heterogeneous Mixture Compound Element

BELL RINGER 1.What does C6H12O6 (aq) mean?
Time (sec) Temperature (ºC) 2. Looking at the graph on the right, characterize each variable as independent or dependent.

Examples Graphite - Pepper - Sugar(sucrose) - Paint - Milk - element
heterogeneous compound mixture Homogeneous mixture

Ne N2 SO3 Homogeneous Mixture

Practice

Physical Properties Are constants about the substance
Can use our senses to observe them Extensive depends on how much material you have Intensive A constant, does not matter how much Physical Changes  does not alter the substance Can be reversed

Chemical Properties Properties substances adhere to when they REACT with other substances Chemical Changes – ID by color change, bubbles, heat Δ Examples rust, burning a log, ice pack

ID the following as being intensive, extensive, or chemical properties
__________ The mass of copper wire is 325g. __________ The boiling point of ethanol is 77.0 °C __________ Baking soda reacts with vinegar to make CO2(g) __________ The density of mercury is 13.6 g/ml. __________ The solubility of sodium chloride in water is 40g/100 ml of water.

Physical vs. Chemical Chemical Changes - Mythbusters Mentos Rocket

Sugar and sulfuric acid –
Penny and Nitric Acid Flour with syringe Sugar and sulfuric acid – Half fill 2 100ml beakers with sugar. 40 ml of water and 40ml of H2SO4

Matter Pure Substance Mixture Compound Element Homogeneous Mixture
Can it be physically separated? NO YES Pure Substance Mixture Can it be chemically decomposed? Is the composition uniform? Yes No Yes No Compound Element Homogeneous Mixture Heterogeneous Mixture

BELL RINGER Classify each type of mixture.
NO, you don’t have to write down the chart Mixture 1 (100 ml) Mixture 2 (100 ml) Composition NaCl in H2O Fe fillings in H2O Observations Colorless liquid No visible solid on the beaker bottom Black solid on bottom of beaker Other Data Mass of NaCl(s) dissolved = 2.9 g Mass of Fe(s) = 15.9g Density of Fe(s) = 7.87g/cm3 Classify each type of mixture. Determine the volume of Fe fillings used to produce mixture 2.

Mixtures Made of two or more separate compounds
In chemistry, this is usually a solid and a liquid A. Types of mixtures 1. Suspension Heterogeneous Largest particles Over 1 µm If left alone, particles will settle Can also filter the mixture to remove particles 2. Colloid Heterogeneous Smaller particles, may be invisible Between µm Mixture is not transparent Particles do not settle. Cannot be filtered

[whipped cream, shaving cream]
Colloid Examples Medium/Phases Dispersed Phase Gas Liquid Solid Continuous Medium NONE Liquid Aerosols [fog, mist] Solid Aerosols [smog, clouds] Foam [whipped cream, shaving cream] Emulsion [milk, mayo] Solution [blood, ink] Solid Foam [Styrofoam, pumice] Gel [gelatin, agar, jelly] Solid Solution [colored glass]

Invisible - solution appears transparent
Homogeneous Smallest particles Under µm Invisible - solution appears transparent Particles cannot be filtered Must distill the solution to remove solids B. Solutions 1. Parts Solute - Smaller of the two materials – usually solid Solvent - Larger quantity of the two – usually water or liquid Solutions are labeled (aq) CaCl2(aq) Calcium chloride dissolved in water 2. Solubility How much solute can go into a solvent

Tyndall Effect Used to identify a colloidal solution or a suspension, light is reflected by the dissolved particles Solutions particles are too small

Tyndall Effect

Matter Pure Substance Mixture Compound Element Homogeneous Mixture
Can it be physically separated? NO YES Pure Substance Mixture Can it be chemically decomposed? Is the composition uniform? Yes No Yes No Compound Element Homogeneous Mixture Heterogeneous Mixture suspensions solutions colloids

STATES OF MATTER Solids Liquids Gases Plasma

STATES OF MATTER

Atom Movement What happens to an atom when the kinetic energy changes?
Click Here Vibrational Rotational Translational - particles are constantly vibrating - about an axis, they flip over end to end - particles move from place to place

STATES OF MATTER SOLIDS - Vibrate only
very low KE - particles can vibrate but not move fixed shape & volume Do Not conform to the container shape Vibrate only

STATES OF MATTER Crystalline solid – arranged in a specific pattern such as diamonds, salt, or ice Amorphous solid – no molecular order as found in charcoal, plastics and glass

STATES OF MATTER LIQUIDS -
low KE - particles can move around but are still close together variable shape but packed closely together fixed volume (incompressible) Vibrate & Rotate

STATES OF MATTER GASES -
high KE - particles can separate and move throughout the container Variable shape & volume Fluid and Compressible Vibrate, Rotate, Translate

STATES OF MATTER PLASMA -
Very high KE - particles collide with enough energy to break into charged particles (+/-) variable shape & volume Stars, fluorescent light bulbs

Summary Shape Volume Kinetic Energy Solid fixed fixed V.low
Liquid varies fixed low Gas varies varies high

Very good display of the differences in states of matter
Animation Very good display of the differences in states of matter

HEAT vs. Temperature Temperature Heat
- the measure of an object’s average kinetic energy - the more an object moves, the higher the temperature Heat - flow of energy from a higher temperature object to a lower temperature object

Heat Transfer Endothermic - Exothermic -
Heat absorbed during a reaction Endothermic - Exothermic - Heat given off during a reaction

Think Temperature (KE) Time
Using the following graph, draw a line, representing the temperature of a substance as it is heated constantly starting as a solid all the way through to a gas. Temperature (KE) Time

BELL RINGER Which of the following phase changes are exothermic?
Just right down the correct choice! CO2(s) + heat  CO2(g) NH3(g)  NH3(l) + heat Cu(s) + heat  Cu(l) Hg(l) + heat  Hg(g)

Heating Curve Temperature (KE)  KE PHASE   KE PHASE   KE Time

Heating Curve Temperature (KE) Time q=mc T q=mHv q=mc T q=mHf
m = mass c = specific heat [4.18] q = heat loss/gain q=mc T Time

Get the formula from Reference Tables
Heat Energy Problems How much heat energy, in joules, is absorbed by 24.8 grams of water when it is heated from 21.2ºC to 28.3 ºC? Get the formula from Reference Tables q = mcΔT q = 24.8g (4.18J/g•ºC) 7.1ºC q = 736 J q = 740J

Heat Energy Problems How much heat energy is absorbed when 11.3g of ice melts to form liquid water at the same temperature? Get the formula from Reference Tables q = mHf q = (11.3 g) (334J/g) q = J q = 3770 J

Heat Energy Problems If it takes J of energy to condense 19.2 g of a substance, what is the heat of vaporization of a substance Get the formula from Reference Tables q = mHv 273.3J = (19.2 g) (x) Hv = 14.2 J/g

BELL RINGER q = mcΔT 849J = (95.4 g) (c) (23.0 K ) c = 0.387 J/g•K
The temperature of a piece of copper with a mass of 95.4 g increases from 25.0°C to 48.0°C when the metal absorbs 849 J of heat. What is the specific heat of copper? q = mcΔT 849J = (95.4 g) (c) (23.0 K ) c = J/g•K

Cooling Curve Lab

Heat Energy Problems How much heat is absorbed when g of water is completely vaporized at its boiling point? Get the formula from Reference Tables q = mHv q = (70.0 g) (2260J/g) q = J

Lauric Acid is starting as a liquid
BELL RINGER A What Just sketch the graph! B C Lauric Acid is starting as a liquid D Which line segment represents a phase change only? What is the melting point of lauric acid? At which point do the particles of lauric acid have the highest kinetic energy? What phase change occurs during this 10-minute graph?

Quiz Heat Problems

Heat of Fusion Lab Remember: The energy to melt the ice only comes from the warm water!!!!!!!!!

BELL RINGER If it takes 22.0 kj of energy to change 43.2 g of a substance to a liquid, what is its heat of fusion? 509 Joules/gram

Separation Techniques
Since the components of a mixture are different substances, with at least some physical properties that are unique to each substance, mixtures can be separated by physical means into their components by techniques such as … Filtration Distillation Decanting Chromatography And many others

Filtration Mixture of solid and liquid Stirring rod Filtrate (liquid component of the mixture) Filter paper traps solid Funnel Is the process of removing ‘straining’ a solid, precipitate, from a liquid using a porous paper

Filtration For separation of substances in different phases
Ex – Air filters, coffee filters, fuel filters Decanting Immiscible liquids – separation by differing densities  use a separatory funnel

Filtration

decanting Pouring a liquid off of a solid

decanting carefully pouring a solution from a container, leaving the precipitate in the bottom of the container. Precipitate – solid formed in a solution during a chemical reaction

chromatography Separation of a mixture based upon bonding preferences or size of molecules Tie-dye Pen ink Chlorophyll Paternity testing

Separation of Mixtures
Chromatography separation of substances based on their attraction for substances not in the mixture Gas Paper

Paper Chromatography

Distillation The separation of a mixture based upon boiling point differences. The substance with the lower boiling point will vaporize and re-condense as a purified substance Used to purify liquids Distilled water Cooling water out in Run hose into sink Connect hose to cold water tap

Distillation Cooling water out Run hose into sink in Connect hose
to cold water tap

Fractional Distillation
separation of substances by their boiling point Miscible liquids Solutions Volatility – measure of the speed at which a substance evaporates

Distillation SHAKE TEST

White Board Review What would be the temperature change if 3.00g of water absorbed 29.2 J of energy?

White Board Review At 1.00 atm of pressure, 25.0 g of a compound at its normal boiling point are converted to a gas by the addition of J What is the heat of vaporization of this substance?

White Board Review If J are added to 32.8 g of water at 30.0°C, what will be the final temperature of water?

White Board Review 23422 J of energy was used to change the temperature of 162.8g substance from 13.2°C to 19.4°. What is the specific heat of the substance?

White Board Review A 14.3g sample of liquid water at 100.0°C is cooled to solid water at 0.0°C. How much energy was released?

Describe how to separate ammonia from hydrogen and nitrogen.
BELL RINGER Gas Boiling Point Melting Point Solubility in Water Nitrogen -196ºC -210ºC Insoluble Hydrogen -252ºC -259ºC Ammonia -33ºC -78ºC Soluble Describe how to separate ammonia from hydrogen and nitrogen.

Law of Conservation of Energy
=energy is not created nor destroyed REMEMBER: Heat energy always travels from the higher temperature to the lower temperature until both temperatures are the same.

Temperature Scales Temperature
measures how fast an object’s molecules are moving = KE Different scales have been developed Only need two fixed points to develop your own scale

Temperature Conversions
On Reference Tables K = °C + 273 A 1.0 °C change = 1.0K change

Some Test Topics: Matter Classification
PE vs. KE (how measured, when changing) Separation Techniques Temperature Conversions Heat Formulas Phase Changes (aqueous) Heating/Cooling Curves - interpret

How can you tell if a physical change has occurred?
BELL RINGER How can you tell if a physical change has occurred?

Separation by Chromatography
sample mixture a chromatographic column stationary phase selectively absorbs components mobile phase sweeps sample down column detector

_________ Curve Temperature (KE) Label Everything! Time

Pure Substances Element contain only ONE kind of atom Ex - copper gold

The compound has completely different properties than the element
Pure Substances COMPOUND composed of 2 or more elements in a fixed ratio new properties different from individual elements Na Cl2 NaCl The compound has completely different properties than the element

WE ARE DONE!

BELL RINGER Heat (Joules)
C D E Heat (Joules) The graph shows the heating curve of 2.0 gram of a solid as it is heated at a constant rate, starting below its melting point. What is the heat of vaporization and along which line on the graph is it measured?

Heat Problems

Problem #3 back of sheet from last class 100 ° C 0 ° C

Analysis By Separation Lab
X 100%

Analysis By Separation Lab
Write-Up Procedure – replaces the purpose Safety Data: ALL Data and calculations Questions – answered in complete sentences Summary

BELL RINGER A student has a flask containing two immiscible liquids. One of the liquids is a solution of a solid in water. Describe how you would separate the mixture into its three separate components?

BELL RINGER If it S

Specific Heat Lab

How many phases of matter exist? What are they?
BELL RINGER How many phases of matter exist? What are they?

How can you tell if a physical change has occurred?
BELL RINGER How can you tell if a physical change has occurred?

BELL RINGER Just sketch the graph! What is the freezing point of the substance in the above graph? In a box on your paper, draw at least 9 particles (•) of the substance during the first 3 minutes of heating.

Precision and Accuracy

BELL RINGER Explain, in terms of particles and energy, the different states of matter.

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