Matter Unit Vocabulary

• • • • • • • • • Matter Kinetic Theory Solid Liquid Gas Plasma Phase change – Freezing – Melting – Deposition – Sublimation – Condenstation – Vaporization Physical properties – Ducility – Malleability – Melting point – – Boiling point Freezing point – Solubility – Reaction to light – Electrical conductivity Chemical properties – Flammability – Oxidation – decomposition • • • • • • • • • • • • • Physical change Chemical change Demoritus John Dalton JJ Thomson Ernest Rutherford Niels Bohr Atomos Bohr Model Cloud Model Valence Electrons Energy Levels – Shells Properties of Water – Universal solvent – – Adhesion Cohesion – High specific heat – Capillary action – Surface tension – – Polarity States of matter – Heat of vaporization – pH

Matter

• Anything that has mass and occupies space • The materials or “stuff” that all objects and substances in the universe are made of • 4 States of Matter = Solid, liquid, gas, and plasma

Matter

• Because all matter takes up space (has volume) and contains a certain amount of material (has mass), all matter can be detected and measured

Examples of Matter

• • • Rocks, water, trees, bicycles, lighting, animals, stars, smoke, are all easily seen and observed Dust mites that live in your furniture and rugs you may need a microscope to view Air maybe invisible but we can feel it when the wind blows and see it bend the branches of trees (oxygen, nitrogen, hydrogen, CO 2 )

What is not matter?

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Light

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Sound

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Gravity

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Friction

Matter

• Atoms are the building blocks of matter • The elements in our periodic table make up all matter

Kinetic Theory

All matter consists of tiny particles that are in constant motion.

Kinetic Theory

1. All matter is composed of small particles (atoms, molecules, or ions). There is an attractive force between them.

2. They are in constant, random motion. The particles may collide with one another or the sides of their container.

3. As the temperature increases the speed of the particles increases. As the temperature decreases the speed of the particles decreases.

SOLIDS

•State of matter that has a definite shape and a definite volume. •Particles of solids are tightly packed, vibrating about a fixed position.

•

Particles are strongly attracted to each other

LIQUID



A state of matter that has a definite volume but takes the shape of its container



Liquids do not have a definite shape



Particles of liquids are tightly packed, but are far enough apart to slide over one another, allowing it to flow

 GAS

A state of matter that has no definite shape and no definite volume; expands to fill the shape of its container



Particles of gases are very far apart and move freely.



Attractive forces are very weak • Contain mostly empty space – because the particles are so far apart • Particles spread throughout a given volume until distributed equally – diffusion

Gas vs. Vapor

• Gas – a substance that

is naturally in the gaseous state at room temperature

• EXAMPLE: Helium • Vapor – the gaseous

state of a substance that is a solid or liquid at room temperature

• EXAMPLE: Steam

 PLASMA

A state of matter that does not have a definite shape or volume and whose particles have broken apart



Consists of + and – charged particles (electrons are knocked off due to collisions)



A plasma is a very good conductor of electricity and is affected by magnetic fields.

• Plasma is the most common state of matter in the universe

STATES OF MATTER

SOLID LIQUID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place, definite shape and volume Close together with no regular arrangement.

Move about, flow and slide past each other. Definite volume, no definite shape takes shape of its container.

Well separated with no regular arrangement.

Move freely at high speeds. No definite shape or volume. Easily compressible.

PLASMA Has no definite volume or shape and is composed of electrical charged particles PLC-Unit 1B

STATES OF MATTER

SOLID Tightly packed, in a regular pattern Vibrate, but do not move from place to place LIQUID Close together with no regular arrangement.

Vibrate, move about, and slide past each other GAS Well separated with no regular arrangement.

Vibrate and move freely at high speeds PLASMA Has no definite volume or shape and is composed of electrical charged particles

Phase Change

A transition of matter from one state to another.

Some phase changes are more common and easier for us to visualize. For example, you have probably witnessed

freezing, melting

, and

vaporization

just by making ice, melting ice, and boiling water.

Condensation

often occurs on the outside of cold beverage containers. This is when the humid air changes directly to a liquid on the surface of the container.

Sublimation

Dry ice is actually solid carbon dioxide. When it sits in the open or is placed in water it rapidly changes directly from solid to gas creating a foggy cloud.

Deposition

Frozen patterns of ice on your car windshield is an example. Deposition involves a gas changing to a solid. This occurs during winter months when the humid air directly freezes into solid ice.

Physical properties

• Characteristics that can be observed without changing the makeup or identity of the matter • Examples: color, size, state of matter, density, ductility, malleability, boiling point, melting point, freezing point, electrical conductivity, solubility, reaction to light

Density

• The ratio of the mass of an object to its volume • Formula: d = m/V • Units: g/mL or g/cm 3

Ductility

• The ability to be pulled into a thin strand • EX: wire

Malleability

• The ability to be pressed or pounded into a thin sheet • EX: aluminum foil, sheet metal

Boiling Point

• The temp at which a substance changes from a liquid to a gas • EX: the boiling point of water = 100 0 C

Melting Point

• The temp at which a substance changes from a solid to a liquid • EX: the melting point of chocolate is 34 0 C

Freezing Point

• The temp at which a substance changes from a liquid to a solid • EX: the freezing point of water = 0 0 C

Electrical Conductivity

• How well a substance allows electricity to flow through it • EX: copper wires, electrical lines

Solubility

• The ability to dissolve in another substance • EX: sugar in water

Reaction to Light

• Reflection – to bounce off ( mirror) • Refraction – to bend (water) • Absorption – to take in (leaf)

Reaction to Light

• Transmission – allow to pass through – Opaque – little to no light passes through (blanket) – Translucent – some light passes through (sunglasses) – Transparent- most light passes through ( glass window)

Chemical properties

• The ability of matter to undergo a specific chemical change, creating a different type of matter with new properties • Examples: flammability, decomposition, oxidation

Flammibility

• To burn • Must occur in the presence of oxygen • EX: Flame tests help to identify metals by their characteristic flame color

Decomposition

• To rot or breakdown • Complex compounds breakdown to simpler substances • EX: CO 2 breaks down to Carbon and Oxygen

Oxidation

• The process of losing electrons • EX: iron rusts when exposed to oxygen

Physical Changes

• A process where a substance’s chemical properties have not changed • Can be a change in size, color, shape, state of matter • EX: ice melting, salt dissolving in water, glass breaking

Chemical Change

• Occurs when new substances or materials are produced to have different chemical properties from the reactants • EX: rust is the product of iron and oxygen, wood burning

Democritus

• Greek philosopher in 440 bc • Was the first to proposed the existence of atoms • “Atomos” meaning “not to be cut”

John Dalton

• • • British chemist 1803 Atomic Theory – He came up with the theory that all substances were made of atoms Atoms were small, hard, dense spheres that could not be created, destroyed, or altered

Dmitri Mendeleev

• Known as the father of the present day periodic table • Organized the elements (each type of atom) by similar properties in 1869

J. J. Thomson

• British scientist 1898 • Proposed that atoms themselves were made of smaller particles .

• He discovered that atoms contained negatively charged particles, but did not know their location

J. J. Thomson

• Theorized the negatively charged particles were spread evenly throughout the positively charged material • Thomson’s model of the atom was called the “plum-pudding” model

Ernest Rutherford

• 1911 a former student of Thomson's • Proposed that atoms had a dense, positively charged nucleus surrounded by electrons

Niels Bohr

• 1913 Danish scientist • Said that electrons revolve around the nucleus in circular paths, called orbits • And that electrons could only exist in certain orbits and at certain energy levels http://youtu.be/wCCz20JOXXk

• Today’s model electron cloud model Bohr’s model was an important stepping stone to today’s, which was developed in the 1920’s • Electrons surround the nucleus, traveling not in prescribed paths but in regions of various thicknesses called clouds http://youtu.be/kYkD-dcupAU

Bohr Model •

Electrons orbit the nucleus of an atom in set energy levels

P = 20 N = 20

Energy Level

• The specific energies an electron in an atom can have • In the Bohr model used to describe the different orbits or shells that the electrons travel in around the nucleus

Valence Electrons

• The electrons in the highest or outermost energy level

•

Polarity

When electrons are not shared equally in a covalent bond, causing one end of the water molecule to have a positive charge while the other has a negative charge

Each end of a water molecule is attracted to the opposite charged end of another water molecule. Water's polarity is responsible for the "stickiness" or cohesion between the molecules.

States of Matter

• The only known substance to naturally exist on Earth in all three states of matter is water Solid - Ice Gas - Clouds Liquid - Lakes

pH • The measure of how acidic or basic water is

Universal Solvent

• More substances dissolve in water than in any other liquid

Cohesion

• Water molecules are attracted to more water molecules so they stick to each other Water ↔ Water

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Adhesion

Water molecules are attracted to and stick to other substance

Water ↔ Other

Surface Tension

• Water molecules have a stronger attraction to each other than to the air above, so the water molecules cling tightly to each other forming what’s like a skin at the surface

•

Capillary Action

Movement of water within the spaces of a porous material due to the forces of adhesion, cohesion and surface tension

High Specific Heat

• The amount of energy required to raise the temperature of water by one degree Celsius is quite large, causing the temperature of water to change slowly

Heat of Vaporization

• Water absorbs heat as it changes from a liquid to a gas