matter and energy - chemistry...
TRANSCRIPT
2
Universe ClassifiedUniverse Classified
Matter is the part of the universe that has mass and Matter is the part of the universe that has mass and volumevolume
Energy is the part of the universe that has the Energy is the part of the universe that has the ability to do workability to do work
Chemistry studiesChemistry studiesThe properties of different types of matterThe properties of different types of matterThe way matter behaves when influenced by other The way matter behaves when influenced by other
matter and/or energymatter and/or energy
3
Changes in Matter
Physical Changes do not change the Physical Changes do not change the fundamental components that make the fundamental components that make the substancesubstanceState Changes State Changes –– boiling, melting, condensingboiling, melting, condensing
Chemical Changes involve a change in the Chemical Changes involve a change in the fundamental components of the substancefundamental components of the substanceProduce a new substanceProduce a new substanceChemical reactionChemical reactionReactants Reactants →→ ProductsProducts
4
Classify Each of the following as Classify Each of the following as Physical or Chemical Properties Physical or Chemical Properties
The boiling point of ethyl alcohol is The boiling point of ethyl alcohol is 7878°°C.C.
Diamond is very hard.Diamond is very hard.
Sugar ferments to form ethyl alcohol.Sugar ferments to form ethyl alcohol.
5
Classify Each of the following as Physical or Chemical Properties
The boiling point of ethyl alcohol is 78The boiling point of ethyl alcohol is 78°°C.C.Physical property Physical property –– describes inherent characteristic of describes inherent characteristic of
alcohol alcohol –– boiling pointboiling pointDiamond is very hard.Diamond is very hard.Physical property Physical property –– describes inherent characteristic of describes inherent characteristic of
diamond diamond –– hardnesshardnessSugar ferments to form ethyl alcohol.Sugar ferments to form ethyl alcohol.Chemical property Chemical property –– describes behavior of sugar describes behavior of sugar ––
forming a new substance (ethyl alcohol)forming a new substance (ethyl alcohol)
6
solid, liquid, gassolid, liquid, gas
States of MatterStates of Matter
State Shape Volume Compress Flow
Solid KeepsShape
KeepsVolume
No No
Liquid TakesShape ofContainer
KeepsVolume
No Yes
Gas TakesShape ofContainer
TakesVolume ofContainer
Yes Yes
7
Classify Each of the following as Classify Each of the following as Physical or Chemical Changes Physical or Chemical Changes
Iron metal is melted.
Iron combines with oxygen to form rust.
Sugar ferments to form ethyl alcohol.
8
Classify Each of the following as Classify Each of the following as Physical or Chemical Changes Physical or Chemical Changes
Iron is melted.Physical change – describes a state change, but the
material is still iron
Iron combines with oxygen to form rust..Chemical change – describes how iron and oxygen
react to make a new substance, rust
Sugar ferments to form ethyl alcohol.Chemical change – describes how sugar forms a new
substance (ethyl alcohol)
9
Elements and CompoundsElements and CompoundsElements: Substances which can not be broken down into simpler substances by chemical reactions
Compounds: Substances that are chemical combinations of elements.
Compounds can be broken down into elements:Properties of the compound not related to the properties of the elements that compose it
Same chemical composition at all times
10
Classification of MatterClassification of Matter
Homogeneous = uniform throughout, appears to be one thing
pure substancessolutions (homogeneous mixtures)
Heterogeneous = non-uniform, contains regions with different properties than other regions
Pure SubstanceConstant Composition
Homogeneous
MixtureVariable Composition
Matter
11
Pure Substances vs. MixturesPure Substances vs. MixturesPure SubstancesHave the same physical and chemical properties
Have the same compositionHomogeneousSeparate into components based on chemical properties
MixturesDifferent samples may show different propertiesVariable compositionHomogeneous or HeterogeneousSeparate into components based on physical properties
All mixtures are made of pure substances
12
Identify the following as a Identify the following as a pure substance, pure substance, homogeneous mixture or homogeneous mixture or heterogeneous mixtureheterogeneous mixture
GasolineGasoline
A stream with gravel on the bottomA stream with gravel on the bottom
Copper metalCopper metal
13
Gasolinea homogenous mixture
A stream with gravel on the bottoma heterogeneous mixture
Copper metalA pure substance (all elements are pure substances)
Identify the following as a pure substance, homogeneous mixture or heterogeneous mixture
14
Separation of MixturesOne can separate mixtures based on different
physical properties of the components
EvaporationVolatility
ChromatographyAdherence to a Surface
FiltrationState of Matter (solid/liquid/gas)
DistillationBoiling Point
TechniqueDifferent Physical Property
15
Energy and Energy ChangesEnergy and Energy Changes
Capacity to do workchemical, mechanical, thermal, electrical, radiant,
sound, nuclear
Energy may affect mattere.g. raise its temperature, eventually causing a
state change
All physical changes and chemical changes involve energy changes
16
HeatHeatHeat: a flow of energy due to a temperature difference
1. Exothermic = Process results in the evolution of heat.Example: when a match is struck, it is an
exothermic process because energy is produced as heat.
2. Endothermic = A process that absorbs energy.Example: melting ice to form liquid water is an
endothermic process.
17
Units of EnergyUnits of Energy
One calorie is the amount of energy needed to raise the temperature of one gram of water by 1°Ckcal = energy needed to raise the temperature of
1000 g of water 1°C
joule 4.184 J = 1 cal
18
Example - Converting Calories to Joules
251Jcal1
J 4.184 60.1cal
joules4.184cal 1
=×
=
Convert 60.1 cal to joules
19
Energy and the Temperature of Matter
The increase in the temperature of an object depends on:the amount of heat added (Q)
the object’s mass
20
Specific Heat
Specific heat is the amount of energy required to raise the temperature of 1 gram of a substance by 1 Celsius degree
C gJ 4.184 is water ofheat specific the,definitionBy °
Amount of Heat = Specific Heat x Mass x Temperature ChangeQ = s x m x ΔT
21
Example – Calculate the amount of heat energy (in joules) needed to raise temperature of 7.40 g of water from 29.0°C to 46.0°C
Mass = 7.40 g
Temperature Change = 46.0°C – 29.0°C = 17.0°C
J 526 C17.07.40gC g
J 4.184 Heat =°××°
=
Specific Heat of Water = 4.184 C-g
J°C g
J°
Q = s x m x ΔT
22
Example – A 1.6 g sample of metal appears to be gold and requires 5.8 J to raise the temperature from 23°C to 41°C. Is the metal pure gold?
C gJ0.20
C18x g 1.6J 5.8 s
C18 C23 - C41 TT m
Q s
TmsQ
°=
°=
°=°°=ΔΔ×
=
Δ××=
Table 3.2 lists the specific heat of gold as 0.13Therefore the metal cannot be pure gold.
C gJ°