Understanding our world and being able to use that knowledge to help us means describing things and understanding how they behave.

Properties of Matter

What are the ways and words we can use to describe “stuff?”

How does “stuff” behave? What does it do when we make changes to it?

Once we make changes to stuff what are its new characteristics? Can we change new stuff back into the old stuff?”

Is the “stuff” one thing (pure) or more than one thing (mixture)?

Properties are the characteristics and behaviors we use to describe matter!

Matter: anything that has mass (weighs something) & takes up space (has volume). Matter has 3 forms or physical states

Properties of Matter - physical state 1

Physical: properties of a pure substance, we can see without changing it into a new substance. Examples include:

Chemical: properties of a pure substance that describe its ability to combine with or change into a new substance. Examples:

1.physical state: solid, liquid, gas

2.color3.shape4.mass5. texture6.melting & boiling point7.density8.solubility in water

1. Flammability2. Reactivity

Physical & Chemical Properties2

Properties can be broken down into two types - physical and chemical properties. What’s the difference?

a defined density (1 g/mL)

• Pure substance - a substance that contains a single type of matter. When the substance is pure, it has a unique set of properties

Matter can either be found in nature as a pure substance or a mixture. What does it mean to be pure?

…imagine you had a colorless liquid that boiled at 100° C, melted at 0° C, and had a density of 1 g/mL, you could say it is most likely water!!

Properties - Pure Substances 3

• Pure substances have characteristic properties which we can use to identify the substance…

Example: pure water contains ONLY molecules of water (H2O) and

NOTHING else!! When water is pure it has the following properites:

a defined melting point (0 °C)

a defined boiling point (100 °C)

no color

no taste

does not burn

Properties of Matter - Mixtures4

• Mixture - two or more substances mixed together, but not chemically combined. Each component in a mixture keeps its individual properties.

The mixture will behave differently than the two materials separate. Salt water will have a different boiling point than pure water!

• Because the parts of a mixture are not chemically combined, the parts can often be separated (purified) into their pure forms by taking advantage of their properties.

Salt can be separated from water by distilling the water (heating it to boiling), leaving behind salt, collecting water pure as it condenses.

Example: salt water contains water molecules (H2O) and sodium

chloride (NaCl) molecules.

If you separate salt from water, the two substances will have the same properties as they would before you mixed the two.

Some substances are able to dissolve other materials. If you put sugar into water, the water will dissolve the sugar. The sugar will soon disappear (sugar molecules are dissolved in the water)…

Solubility and Solutions 5

• Solution - a special type of mixture where one of the components mixes evenly throughout (dissolves) so that you can’t visibly see one of the parts.

• Solubility - the property describing how much of a material can be dissolved.

Pepper is not soluble in water. We can say pepper is insoluble in water.

Salt has a high solubility in water. We can dissolve a lot of salt in water.

• Dissolving a substance is an example of a phyiscal change. The substance is STILL THERE, and hasn’t been changed into anything new!

Mixtures4

• Mixture -- If you separate salt from salt water, the water will have the same

properties as it would before you mixed the two- BUT… The mixture as a whole can behave differently (salt water will

have a different boiling point than pure water)

• Components in mixtures can often be separated (purified) into their pure forms by taking advantage of their properties

- Salt can be separated from water by distilling the water (heating it to boiling), leaving behind salt, collecting water pure as it condenses

• Solution -

- In mixtures you see more than one Thing (phase)

- In a solution you see only one thing (phase)

- A mixture containing stuff not soluble in water could be filtered, leaving behind the stuff that doesn’t dissolve (sand & water)

Pure substance!

Sprite?

SolutionDissolved Ingredients

including gas (CO2)

mixture of salts, fish, seaweed…

only water - pure

Pure substance!Sodium Chloride -

pure

Mixture!

Let’s play Solution or Not Solution!!Distilled

water water?

The ocean?

Salt?

Density6

Density is the ratio of the mass of an object to its volume.

• Density is determined by measuring the mass of an object, and measuring the volume, then dividing the two. Mass is measured in grams (g), volume in milliliters (mL).

• Density is a characteristic property of pure substances; it will always be the same under a given set of conditions. Example: density of water at 25 °C is 1 g/mL.

Density (D) = Mass g (M)Volume mL (V)

• Objects with lower densities tend to float (cork floats in water). Objects with higher densities tend to sink (oil floats because it is less dense).

Cork in waterOil floating on top of water

Density 7

• Lots of things affect density…

• Water with salts dissolved in them tend to be more dense than pure water. So, salt water (for example, in the ocean) will sink to the bottom while fresh water will float on top.

Temperature: cool air sinks, warm air rises

Cold water sinks, warm water rises, creating layers of water

Density8

• The Dead Sea in Israel has such a high concentration of salt (amount dissolved in water) that people can float in the water.

• Ocean water is ~3.5% salt. The Dead Sea has a salinity of ~34%!!!!

Let’s try to describe matter in some more detail…

Matter

Pure substances:

(water, salt, sugar)

Mixtures: (soil, air)

Compounds, Molecules & Elements

can be broken down further into

Molecules and Compounds 9

• Molecule - a single unit of a pure substance, chemically combined (bonded) in a defined ratio.

• Compound - many molecules of the same pure substance. Example: a glass of water contains many millions of molecules of water.

• Examples: water (H2O), hydrogen peroxide (H2O2), sodium chloride (NaCl)

- elements can’t be broken down further and still keep their properties

- each element has distinctive properties. Some are stable, and can be found by themselves in nature. Others are so reactive, they will only be found combined with other elements.

- about 100 different elements

- elements identified by 1 or 2 letter symbols. Letters often are the first letters of the name of the element (Chlorine -> Cl)

- organized in a specific way into the Periodic Table of the Elements.

Elements10

• Element - a pure substance consisting of a single type of atom

Metals: properties include malleability, ductility, good conductors of heat/electricity, magnetic

Nonmetals: properties include poor conductors of heat & electricity, solids are brittle & dull

Metalloids: have both characteristics of metals and metalloids

Periodic Table of the Elements 11

The Periodic Table organizes elements into a set of patterns, arranged by increasing atomic number, invented by Russian chemist Dimitri Medeleev (1869)

You are probably familiar with certain elements…

Elements: Hydrogen & Oxygen12

Elements: Chlorine & Nitrogen 13

Elements: Carbon & Sodium14

Adding other metals (Nickle, Tungsten) to steel gives different properties.

Elements: Iron & Aluminum 15

• Metals: Sodium (Na), Iron (Fe), and Aluminum (Al)

- Shininess, magnetic

- malleability: ability of a substance to be molded/formed

- conductivity: ability of a substance to transfer heat/electricity

• Reactivity: willingness and ability to combine with other elements

- Many of the elements are so reactive that they are not found

alone in nature. Wanna see how reactive?

- brittle, dull, not magnetic, not malleable

- have poor conductivity - good insulators

- many are gases, tend to be reactive

• Nonmetals: Hydrogen (H2), Oxygen (O2), Carbon (C ), Chlorine (Cl2)

Properties of Elements16

are composed of

Atoms: smallest building block of which matter is composed

Matter

Elements: pure substance with distinctive properties can’t be broken down further by physical or chemical means and retain their properties

Pure substances:

(water, salt, sugar)

Mixtures: (soil, air)

Compounds, Molecules & Elements

can be broken down further into

Describing Matter 17

• Theory of atomic structure says that all atoms consist of:

-

-

-

-

-

-

++ +

+++

Nucleus -

contains protons with a positive charge (+)

and neutrons (neutral, no charge)

Electrons -particles with negative charge (-) orbiting nucleus in a “cloud”

• An element is identified by the number of protons in its nucleus, called the atomic number. An atom having 6 protons

in its nucleus is a called a carbon atom

• Atoms: smallest building block of which matter is composed, when combined in specific ratios, they make the elements

Structure of Atoms 18

• Atoms can combine to form a single molecule of a new substance. Remember, a molecule is a single unit of a substance, combined in defined ratios

Na

Sodium atom

+

Chlorine atom

Cl

• Atoms in molecules are held together by attractive forces called bonds.

1 Sodium chloride molecule

Na Clreaction

Combining Atoms 19

Sodium - very reactive metal

+Chlorine - toxic & reactive green gas

Sodium chloride - inert (not reactive) colorless solid you can eat!

Compounds often have different properties than the elements that make them up!

• Atoms combining in defined ratios

Combining Atoms20

Hydrogen - very light, flammable

gas

2 Hydrogen atoms

H H +

Oxygen atom

O

1 Water molecule

reaction HH

O

Oxygen - colorless gas, explosive

+ Water - needed by all life, can drink it

Again, compounds often have different properties than the elements that make them

up!

• Physical properties: characteristic of a pure substance that can be observed without changing it into another substance.

• Physical changes: changes to a substance that can be observed without changing its identity. Examples…

- water always has a density of 1 g/mL at 25° C

• Physical changes are sometimes hard to notice…

Changes to Matter 21

Now that we have described matter and put it into different catagories, we can describe how matter changes…

- at atmospheric pressure, water always melts at 0°C, and boils at 100°C

- Change of state, which is easily reversed. For example, water freezes into ice, boils into water vapor, but it’s still water!

- Dissolving a substance into another substance. Salt dissolves in water, but they are not chemically combined. They can be separated (distillation)

• Chemical properties: a characteristic ability of a substance to change into another substance.

• Chemical changes are often much more obvious than physical changes

- Sodium metal is very reactive, never found alone in nature

1. Color change

2. Light, heat, or energy released (burning)

3. Gases or solids form where there were none before

Chemical Changes22

• Chemical changes: changes to a substance that results in a new substance forming.

- Examples of chemical properties: flammablility, reactivity (the desire of a substance to combine with and form new susbtances

Chemical Changes 23

Atoms - smallest building blocks of matter (e.g. an atom of Oxygen contains 16 protons)

Molecules - several atoms bonded together in a defined ratio to form a pure substance (e.g Oxygen atoms react with Hydrogen atoms to form a single molecule of water)

HO

H

Compounds - many molecules of the same pure substance

Elements - many atoms of the same kind (e.g. Oxygen)

O

From Smallest to Largest24