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# Energy & Matter - PowerPoint PPT Presentation

Energy & Matter. 2.1, 1.1, 1.2, 1.3. 1. Energy (2.1). Energy : The capacity to do work or produce heat . 7 types of energy: • mechanical • thermal (heat) • radiant (light) • sound • electrical • chemical • nuclear. 2. Kinetic Energy : Energy of motion.

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### Energy & Matter

2.1, 1.1, 1.2, 1.3

• Energy: The capacity to do work or produce

heat.

• 7 types of energy:

• mechanical

• thermal (heat)

• sound

• electrical

• chemical

• nuclear

2. Kinetic Energy: Energy of motion.

Ex. thermal,

mechanical

3. Potential Energy: stored energy; determined by position.

4. Energy can be transferred from a system to its surroundings.

Ex. Photosynthesis is light → chemical

5. Energy absorbing changes are called endothermic. If energy is released the change is called exothermic.

1. Common Unit: calorie The amount of heatneeded to raise 1g of water 1oC. (One calorie = 1g°C)

2. SI Unit for energy: Joule (J)

C. Law of Conservation of Energy:

Energy is neither created nor destroyed, it just changes form.

1. Energy can be transferred in the form of

heat.

2. Temperature is a measurement of heat or

kinetic energy. (how fast the average

particle is moving!)

Heat vs. Temperature Animation

Kinetic Energy (Temperature) and Melting

Room Temp 20°C→

Room Temp 70°F→

← Room Temp 293 K

K = °C + 273

°C = K - 273

4. Kelvin: °C = K

5. The zero point on the Kelvin scale is called absolute zero (-273°C)

6. All motion of particles stops! Therefore the kinetic energy is zero.

2. Matter is anything that has mass and takes up space.

1. Volume: Amount of space an object takes up.

2. Mass: Quantity of matter in a substance. Constant everywhere. Ex) the moon

3. Weight: Force produced by gravity acting on a mass. This is different in different locations.

Mass does not depend on gravity. The mass of an object remains the same in all locations.

Weight depends on gravity. Weight equals Mass x gravity. The weight of an object changes with location.

Weight and Mass Demo

1. Physical: density, color, melting point, viscosity, surface tension, specific heat

2. Chemical: flammability, reactivity with other

chemicals or air (O2)

C. States of Matter (1.1):

Plasma is the 4th state of matter “ionized gas” like the sun/fluorscent lights

1. Gasespossess the greatest amount of kinetic energy.

2. Two factors that determine the state of matter of a substance: speed of the particlesand the distance between them.

3. These two factors contribute to the attractionbetween the particles.

4. Substances changephasewhen they overcome these attractions.

5. The overallkineticenergy(temperature) will remain constant until the entire substance has completely changed phase.

Vapor (gas)

condensation

Cooling Curve

100

Vaporization

(boiling/evaporation)

Liquid

freezing

0

Heating Curve

Solid

(◦C)

melting

1. Physical Changes:

• a. Do NOT change the identityof the substance.

• b. Often change what the substancelooks like.

• c. Examples:cutting

dyeing

changes of state

Solid

deposition

melting

sublimation

freezing

condensation

vaporization

evaporation –at the surface

boiling - throughout

Gas

(Vapor)

Liquid

Gases are in the gaseous state at room temp.

Vapors are in the solid or liquid state at room temp.

Comparison of the three states of matter

@ 4◦C

Density = .998 g/mL

@ 20ºC

Ice Density = .92g/mL

2. Chemical Changes:

a. Alter the identityof the substance.

b. The new substance has different properties

than the original substance.

c. Examples of Chemical Changes: burning, rusting

d. Signs that a chemical change has occurred:

1. gas released (bubbles/odor/fizz/smoke)

2. color change (can be physical too)

3. formation of a precipitate (insoluble solid that

falls out of solution.)

4. temperature change (can be physical also)

Law of Conservation of Matter (2.2): Matter is neither created or destroyed it just changes form.

G. Classification of Matter (1.3)

1. Pure substances: Substances that have a uniqueset of

physical and chemicalproperties.

a. Elements: The smallest part of an element is

an atom.

1. Cannot be separated into simpler substances.

2. Represented by symbolsthat have 1or2letters.

Ex) K, Na, Au, Ag, Hg, Fe

(three lettered symbols are temporary)

Element Symbol: 1 or 2 letters (1st is a capital)

1

H

Hydrogen

1.008

b. Compounds:

1. Made up of 2or more kinds of atoms

chemicallycombined in a fixed proportion.

2. Represented by formulas.

3. Examples: CO, CO2, H2O, NH3

Atomic Number: # of protons

Element Name

Atomic Mass: (weighted average of all an elements’s isotopes)

a. Heterogeneous Mixture: Visibly different

throughout. Will separate upon standing.

chip cookies, sand & water (suspension)

b. Homogeneous Mixture: The same

throughout. May be clear, will not separate.

Ex) Kool-aid (solution)

milk (colloid)

gold jewelry (alloy)

Brass is an alloy of copper and zinc.

Bronze is an alloy of copper and tin.

Steel is an alloy of carbon and iron.

Colloids

Solutions

Alloys

ex) gold jewelry

ex) Kool-Aid

ex) milk

ex) sand & water

1. Heterogeneous Mixtures can be separated by:

a. Filtration- Material remaining on the filter paper is called the residue. The filtrate goes through the filter paper. Ex) sand & water

a. Distillation- separates liquids (and 1 solid) by differences in boiling point. The remaining material is called theresidue. The material that goes through is called the distillate.

Ex) alcohol & H2O

• A Closer Look at Distillation

b. Crystallization- Evaporate liquid and the solid will crystallize. Ex) salt and water

c. Chromatography – used to separate pigments and ink by differences in solubility(density) on a strip of paper.Ex) black ink - rainbow

a. Electrolysis – decomposes a compound into its elements. Ex) water into H2 and O2