PROPERTIES OF MATTER

Identify the characteristics of matter and substances

Differentiate among the three states of matter

Define physical properties of substances

Matter is anything that has mass and takes up space.

Mass of an object is the amount of matter the object contains.

Matter that has a uniform and definite composition is called a substance Pure substances contain

only one kind of matter Non example: lemonade

Discussion with shoulder buddy on why lemonade is not an example.

Diagrams of Matter

substanceELEMENTS COMPOUNDS

The simplest forms of matter that can exist under normal laboratory conditions

Represented by a unique chemical name and chemical symbols

Organized on the periodic table

Examples: oxygen, hydrogen, and carbon

Substances that can be separated into simpler substances only by chemical means.

Made up of 2 or more different elements that are combined chemically in a set ratio

Separating a compound requires energy such as heat or electricity.

Example: salt, baking soda, sugar

PRACTICE: Elements and their symbols

Sulfur , ________ _______________, N Silicon, _____ _________________, K Phosphorous, _______ ______________, He

MIXTURE

Mixture is a combination of two or more pure substances in which each pure substance retains its individual chemical properties Most everyday matter

occurs as a mixture Composition of mixtures

is variable Substances tend to mix

naturally (hard to keep pure)

Can be separated by physical means

TYPES OF MIXTURES

Heterogeneous mixture is a mixture that does not blend smoothly throughout and in which the individual substances remain distinct

Ex. Salad dressing Orange juice with pulp

Types of Mixtures

Homogeneous mixture is a mixture that has a constant composition throughout

It always has a single phase

If you cut two pieces, their composition will be the same.

Also referred to as a solution ex. Tea, metal alloy

Compare mixtures and substances

Create a Venn Diagram

Classify each of the following as homogeneous or heterogeneous mixture

Heterogeneous mixture , homogeneous mixture, or substance

Blood

Chocolate chip ice cream

Brass (a blend of copper and zinc)

Motor oil

Black coffee

Soda

Orange juice

Trail mix

Table salt

Tap water

Carbon dioxide

air

Raisin muffin

Separating Mixtures

When would you use distillation?

Distillation: a liquid is boiled to produce a vapor that is then condensed again to a liquid.

Separating mixtures Filtration is a technique

that uses porous barrier to separate a solid into a liquid

Crystallization is a separation technique that results in the formation of pure solid particles of a substance from a solution containing the dissolved substance. Example : rock candy Produces highly pure solids

Separating Mixture

Sublimation is the process during which a solid changes to vapor without melting. Ex. Dry ice

Chromatography is a technique that separates the components of a mixture dissolved in either a gas or a liquid based on the ability of each component to travel or to be drawn across the surface of a fixed substrate.

THINK and REFLECT

Describe the separation technique that could be used to separate each of the following mixtures Two colorless liquids A non-dissolving solid

mixed with a liquid Red and blue marbles of

the same size and mass Sulfur and iron Sand and salt Gasoline and water Aluminum and steel Copper and silver

PROPERTIES OF MATTER

Physical property is a quality or condition of a substance that can be observed or measured without changing the substance’s composition Examples: Color,

solubility, odor, hardness, density, melting point, boiling point

PROPERTIES OF MATTER

Extensive properties are dependent on the amount of substance present. Example: mass, length, and

volume, amount of energy

Intensive properties are independent of the amount of substance present. Example: density, scent,

color, ability to conduct electricity and to transfer energy as heat, boiling point, melting point

Classify if the property is intensive or extensive property

Intensive or extensive property

Color

Smells like vanilla

Length

Boiling point

Ability to attract a magnet

Density

mass

PROPERTIES OF MATTER

Chemical Property is the ability or inability of a substance to combine with or change into one or more other substances. Example: iron forming

rust when combined with oxygen.

Classify the following as physical or chemical properties

Physical or Chemical Property

Iron and oxygen form rust

Iron is more dense than aluminum

Magnesium burns brightly when ignited

Oil and water do not mix

Mercury melts at -39C

Water has a density of 1.00g/cm3

Blue gray color

brittle

Reacts vigorously with fluorine

STATES OF MATTER

All matter that exists naturally on Earth can be classified as solid, liquid, or gas. The other state of matter

is plasma formed in lightening bolts and in stars.

Practice

In which state of matter do the following exist at room temperature?

Solid, liquid, or gas

Nitrogen

Diamond

Oxygen

Mercury

Cooking oil

Clay

Neon

Bromine

Silver

Hydrogen

THINK

Fingernail polish remover (mostly acetone) is a liquid at room temperature. Would you describe acetone in the gaseous state as a vapor or a gas?

Justify your answer

THINK PAIR SHARE

ILLUSTRATION AND DIAGRAMMING TIME!!!

Compare the properties of solids, liquids, and gases. Make a table that describes shape, volume, compressibility, and structure to share with the class.

Physical Change

What is a physical change?

A change which alters a substance without changing its composition is a physical change.

Example: cutting paper, chopping wood, and freezing water.

Chemical Change

What is a chemical change?

A process that involves one or more substances changing into new substances New substances formed in the

reaction have a different composition and different properties from the substances before the reaction

Ability of a substance to undergo a chemical reaction

Evidence of a Chemical Reaction

How do we know a chemical change has taken place?

A chemical reaction always produces a change in properties. Change in temperature Gas produced Precipitate formed Change in color Change in odor

Chemical Change/chemical Reactions

What are the reactants and products?

In chemical reactions, the starting substances are called reactants, and the substances formed are called products.

Iron + Sulfur Iron Sulfide

CREATION TIME

CREATE A T-CHART of Chemical and Physical changes

THINK PAIR SHARE

State the difference between a physical change and a chemical change, and list three likely indications that a chemical reaction has occurred. Which indication is most suggestive of a chemical reaction?

Classify the following changes as physical or chemical?

Physical or chemical change

Cookies are baked

Water boils

Salt dissolves in water

A firefly emits light

Milk spoils

A metal chair rusts

Bending a piece of wire

Burning coal

Cutting glass

Conservation of Mass

How does mass behave in a chemical reaction?

The law of conservation of mass states that mass is neither created or destroyed during a chemical reaction. Mass of the reactants

equals the mass of the products.

Conservation of Mass

Mass of reactants = mass of products

When ammonium nitrate (NH4NO3) breaks down explosively, it forms nitrogen gas (N2), oxygen gas (O2), and water (H2O). When 40 grams of ammonium nitrate explode, 14 grams of nitrogen, and 8 grams of oxygen are formed. How many grams of water are formed?

Practice: conservation of mass

In the complete reaction of 22.99 g of Sodium with 35.45 g of Chlorine. What mass of sodium chloride is formed?

PRACTICE: Conservation of mass

Hydrogen and oxygen react chemically to form water. How much water would be formed if 4.8g of hydrogen reacted with 38.4 grams of oxygen?

PRACTICE: conservation of mass

A 12.2 g sample of X reacts with a sample of Y to form 78.9 g of XY. What is the mass of Y that reacted?

THINK: Conservation of mass

When powered iron is left exposed to air, it rusts. Explain why the rust weighs more than the original powered iron?

Law of Definite Proportions

The law of definite proportions states that a compound is always composed of the same elements in the same proportion by mass, no matter how large or small the sample. The mass of the

compound is equal to the sum of the masses that make up the compound.

Percent by mass

The percent by mass is the ratio of the mass of each element to the total mass of the compound expressed as a percentage

Percent by mass =

Percent by mass is obtained by dividing the mass of the element by the mass of the compound and then by multiplying this ratio by 100 to express it as a percentage.

EXAMPLE:

A 78.0 g sample of an unknown compound contains12.4g of hydrogen. What is the percent by mass of hydrogen in the compound?

Example: % by mass

1.0 g of hydrogen reacts completely with 19.0g of fluorine. What is the percent by mass of hydrogen in the compound that is formed?

Practice: % by mass

If 3.5 g of element X reacts with 10.5 g of element Y to form the compound XY, what is the percent by mass of element x in the compound? The percent by mass of element Y?

Practice: % by mass

Two unknown compounds are tested. Compound 1 contains 15.0g of hydrogen and 120.0g of oxygen. Compound 2 contains 2.0g of hydrogen and 32.0g of oxygen. Are the compounds the same? Explain.

Law of multiple Proportions

The law of multiple proportion states that when different compounds are formed by a combination of the same elements, different masses of one element combine with same fixed mass of the other element in a ratio of small whole numbers.

Example: water and hydrogen peroxide

H2O = 2:1

H2O2 = 2:2

REVIEW QUESTIONS

Describe a method that could be used to separate each mixture Iron fillings and sand

Sand and salt

The components of ink

Helium and oxygen gases

Review Questions

Which of the following are the same and which are different? Justify your decision. A substance and a pure substance A heterogeneous mixture and a solution A substance and a mixture A homogeneous mixture and a solution

Correct the following statements

An element is a combination of two or more compounds

When a small amount of sugar is completely dissolved in water, a heterogeneous solution is formed.

Review Questions

Name the elements contained in the following compounds.

Sodium Chloride (NaCl) Ammonia (NH3 Ethanol (C2H6O) Bromine (Br2

Review Questions

What is the percent by mass of carbon in 44 g of carbon dioxide?

Review Questions

What is the percent by mass of oxygen in 44g of carbon dioxide?

Review Questions

A 25.3 g sample of an unknown compound contains 0.8g of oxygen. What is the percent by mass of oxygen in the compound?

Review Questions

Magnesium combines with oxygen to form magnesium oxide. If 10.57 g of magnesium reacts completely with 6.96 g of oxygen, what is the percent by mass of oxygen in magnesium oxide?

Review Questions

Express the following numbers in scientific notation. 34,500 2665 0.9640 789 75,600 0.002189

Review Questions

Perform the following mathematic problems using the rules for significant figures.

2.015 + 3.1 +332.41 = 33 * 1.3021 = 1.34 /0.01 = 3444.12-3.222-122.2 =

Review Question

Analyze Is gas escaping from an opened soft drink

an example of a chemical or physical change? Explain

Review Questions

List physical properties of eggs before and after they are cooked. Based on your observations, does a physical change or chemical change occur when eggs are cooked? Justify your answer.

Review Questions

You might have noticed that while eating ice cream on a hot day, some of the ice cream begins to melt. Is the observed change in the state of ice cream a physical or chemical change? Justify your answer.

Review Question

Which states of matter are compressible?

Which states of matter are not compressible?

Explain.

Review Question

Phosphorous combines with hydrogen to form phosphine. In this reaction, 108.3 g of phosphorous combines with excess hydrogen to produce 129.9 g of phosphine. After the reaction, 11.0g of hydrogen remains unreacted. What was the initial mass of hydrogen before reaction? What mass of hydrogen is used in the reaction?

Review Questions

If you have 100 particles of hydrogen and 100 particles of oxygen, how many units of water can you form? Will you use all of the particles of both elements? If not, what will remain?

Hint: Chemical formula H2O

Review Questions

Which of the following is not a chemical change? Paper being shredded Steel rusting Charcoal burning A newspaper yellowing in the sun

Review Questions

Which of these properties could not be used to distinguish between table salt and table salt? Boiling point Melting point Density color

Review Questions

The state of matter characterized by a definite volume and an indefinite shape is Solid Mixture Liquid Gas

Review Question

Initial: finalReactant:_________1. Product2. Mixture3. Matter4. compound

Review Questions

Words: sentenceElements :_________

1. Reactant2. Theory3. Compound4. Substance