MatterChapter 1: Matter and Energy

What is matter?

• Basic stuff on Earth and in the rest of the universe

MatterMass – a measure of the

quantity of matter

Volume – a measure of the space that matter takes up

Mass and Weight

Mass• The quantity of matter contained in a body

Weight• A measure if the force with which gravity pulls a body

toward the center of Earth

Weight-less

States, or Phases, of Matter

Solid

•Rigid body•Definite volume•Shape can be changed by applying a force

Liquid

•Has a specific volume •Takes the shape of its container

Gas

•Does not have a specific volume•Expands of contracts to fill its container

Identifying Matter

• By their characteristics, called Properties.

States, color, odor, temperature, density, solubilityPhysical Properties

• The qualities of a substance that can be demonstrated without changing the composition of the substance

A gas with a choking odor forms when sulfur burnsChemical Properties

• Describe how matter behaves when it changes into another kind of matter.

Mass per unit of volume of a given sample of matter

Properties which can be measured are physical constants

Physical Properties of Salt

Name Formula Color Density Melting Point

Boiling Point

Solubility in g/liter of water

Sodium Chloride

NaCl Colorless 2.2g/mL 801°C 1413°C 360 at 20°C

Structure of Matter

O

H H

Water(liquid)

2 H H2

Hydrogen

(gas)

O O

Oxygen(gas)

Electrolysis

Rearrangement of atoms

Attractive Forces in Matter

O

H H Lines = BondsBonds between the atoms – the attractive forces between them

Angle between the bonds – determines the shape, or the geometry, of the molecule

Conservative of Matter

• The matter exhibits a uniform, or regular behavior. Such behavior is called a law of nature.

• When burned, all matter behaves in the same general way.The total mass of the products formed by burning is equal to the mass of the matter burned plus the mass of the oxygen consumed.

- Antoine Lavoisier

Law of conservation of matter(mass): Matter (or mass) may be neither

created nor destroyed in a

chemical changed

The composition of matter

Ele

me

nt

•One kind of atom•114 elements•88 exist in nature•All samples of elements are homogeneous

Compoun

d

•Two or more elements combine•Can be separated by chemical means•Homogeneous matter, substance

Mixture

•Two or more kinds of matter in varying proportions•Can be separated by physical means, solubility•Heterogeneous mixtures

Compounds vs. mixtures

• A compound has a single set of properties.

• The properties of a mixture are the properties of each of its components and depend on the proportions in which the components are present.

Changes in Matter and Energy

• Matters may undergo physical changes and chemical changes.

• Energy – The ability, or capacity, to do work.

Related to stabilityPotential Energy

• The energy a body possesses because of its position with respect to another body.

Related to temperatureKinetic Energy

• The Energy of motionLaw of

Conservation of energy

Heat and Temperature

Expressed in units: calories(cal),joules(J) and kilojoules(kJ)Heat

• A measure of the total energy in a system.

Expressed in degrees on Fahrenheit, Celsius, or KelvinTemperature

• A measure of the average kinetic energy of the particles in a system

Energy associated with changes in matter

Change Kind of change Energy Change

Converting 1 gram of ice at 0°C to water at 0°C

Physical (Phase) Absorbs 334 joules

Heating 1 gram of water from 0°C to water at 100°C

Physical (Temperature) Absorbs 418 joules

Converting 1 gram of water at 100°C to steam at 100°C

Physical (Phase) Absorbs 2260 joules

Burning 1 gram of coal Chemical Liberates 32,800 joules of 32.8 kilojoules

Burning 1 gram of hydrogen to form liquid water

Chemical Liberates 143,000 joules or 143 kilojoules

Relationship between Matter and Energy

Matter and Energy can be converted from one to the other.

Matter Energy

𝐸=𝑚𝑐2E = energym= massC = Speed of

light

Law of conservation of mass-energy: The total quantity

of mass and energy in the universe is

constant.

Energy and Changes of State

Heated upTemperature up?

t1 t2 t3 t4 t5 t60

10

20

30

40

50

60

70

80

90

Time

Tem

pera

ture

/°C

Liqui

d

Heating Curves

Heat used to break

the attractive

forces

Heat used to break the forces of attraction between

molecules

Heat required to melt a quantity of solid is

called the heat of fusionHeat required to boil a

quantity of liquid is called the heat of

vaporization

1)Heat of vaporization > Heat of Fusion2) Temperature remain constant during a phase change

Solid

Melting

Gas

Boiling

Heating Curves of Water

The curve levelled off at 25s mark, and started

to rise again at 105s mark, it took 80s to melt all the

ice

In 80 seconds, the melting ice

must have absorbed 80 x

16 = 1280 joules.

It took 1280 joules to melt 4 grams of ice. How many joules would it take to melt 1 gram of ice?

4 grams of ice, initially at -50°C, are heated at a steady rate of 16 joules per second

The heat of fusion of

ice is 320J/g

Measurement of Heat

1°C or 1K

10 grams

42 joules

1°C or 1K

10 grams

1.3 joules

Water Lead

Measurement of Heat

• The quantity of heat required to change the temperature of one gram of a substance by one kelvin, or one degree Celsius, is called the specific heat capacity, and can be expressed in the unit joules per gram degree:

Heat = mass x change in temperature x specific heat capacity

q = heatm = massC = Specific capacity = Change in

(Example: Specific heat of water= 4.184)

Calculation

• A chemical reaction causes the temperature of 100 grams of water to increase by 4.0 K. How much joules of heat are released by the reaction?

𝑞 ( 𝑗𝑜𝑢𝑙𝑒𝑠 )=𝑔𝑟𝑎𝑚𝑠𝐻2𝑂×∆𝑇 ×4.18 𝐽 /𝑔 ∙𝐾

𝑞 ( 𝑗𝑜𝑢𝑙𝑒𝑠 )=100𝑔×4𝐾×4.18 𝐽 /𝑔 ∙𝐾¿1672 𝐽

Solution

Calculation

• If 418 joules are applied to 20g of water, initially at a temperature of 293 K , what is the final temperature of the water?

𝑞 ( 𝑗𝑜𝑢𝑙𝑒𝑠 )=𝑔𝑟𝑎𝑚𝑠𝐻2𝑂×∆𝑇 ×4.18 𝐽 /𝑔 ∙𝐾

418 𝐽=20𝑔𝐻 2𝑂×∆𝑇 ×4.18 𝐽 /𝑔 ∙𝐾

5.0°

Solution

298 K

Calorimeter

Insulated container

•Known amount of water at a know temperature

Thermometer •Detect changes in temperature

Stirrer •Maintain a consistent temperature

Styrofoam •An excellent insulator

Heat transfer

•Reactions that release heat to their surroundings•Freezing, Condensation (Bond formation)

Exothermic reactions

•Reactions that absorb heat from their surroundings•Melting, Evaporation, Boiling(Bond breaking)

Endothermic reactions

Exit

Enter

Other units of Energy

Calories• Food Calories, C• 1 calorie = 4.18 joules

British Thermal Units• Power of an air

conditioner, BTU(per hour)

• 1 BTU = 1050 joules