UNIT 2

MATTER – PROPERTIES AND CHANGES

MATTER (pp 21 – 24)

1. Matter is anything that has mass and volume.

2. The amount of matter in an object is known as ____________________.

3. The amount of space an object occupies is known as ____________________.

Basic Units of Matter

1. ____________________ are the basic units of matter.

2. There are over 110 different kinds in the known universe. These are catalogued on the periodic table.

3. Atoms combine to form ____________________. Molecules are a neutral group of atoms held together by chemical bonds.

4. A molecule may contain any number of atoms, but it behaves as one unit.

PROPERTIES OF MATTER (pp. 29 - 34)

1. Different types of matter are described by listing their characteristics, or properties.

2. Some properties of matter used to describe things are:

3. Properties fall into two basic categories: ________________ and _________________.

Physical Properties

1. These are properties that can be observed or measured without changing the composition of matter.

2. Examples are:

3. The ____________________ of matter is also a physical property.

4. The three common states of matter are:

5. Solids have a fixed volume and shape. The atoms and molecules are held tightly in a rigid structure, but do vibrate slightly about fixed positions.

6. Liquids have a fixed volume, but a variable shape. The atoms and molecules are not held together in a rigid manner. This allows them to move past one another and flow.

7. Gases have no fixed shape or volume and therefore expand to fill any container they occupy.

8. The word ____________________ refers to the gaseous state of a substance that is a solid or a liquid at room temperature.

9. A fourth state, ____________________, exists at very high temperatures.

10. In this high-energy state the atoms are torn apart into smaller pieces.

Intensive and Extensive Properties

1. A way to further describe physical properties.

2. An ____________________ property is a physical property that depends on the quantity of matter present.

3. ____________________ properties are physical properties that depend on how matter is structured.

Chemical Properties

1. These are properties that can be observed only when substances interact with one another.

2. Examples are:

***** Classify the following as a chemical property, intensive physical property, or extensive physical property:

blue color reacts with an aciddensity sour tasteflammability melting pointsolubility combustibilityhardness reacts with waterodor lusterboiling point liquid

CONSERVATION OF MASS

1. Although matter can undergo both physical and chemical changes, the total amount of matter does not change.

2. This is obvious for physical changes, but not always so for chemical changes.

3. Early scientists used analytical balances to determine the mass of the reactants and products. They discovered both were equal.

4. The _________________________ state that mass is neither created nor destroyed during a chemical reaction – it is conserved.

5. In the form of an equation, it looks like:

6. Lavoisier discovered that when mercury(II) oxide decomposes to form mercury and oxygen, the mass of the reactants will equal the mass of the products.

***** A 10.0g sample of magnesium reacts with oxygen to form 16.6g magnesium oxide. How many grams of oxygen reacted?

MATTER CHANGES (pp. 29 - 34)

1. A ____________________ is one that affects physical properties only. The basic identity and structure of the material does not change.

2. Changes of state are physical changes.

3. Some changes involve the rearrangement of atoms and the production of new materials.

4. These are called _________________________.

5. During a chemical change atoms are rearranged, but there is no loss or gain in the total number of atoms.

6. In the process of both physical and chemical changes, energy can be either released or absorbed. These changes, where energy is transferred from the system to, or from, the surroundings, have been given special names.

7. An _________________________ is a physical/chemical change during which the system absorbs energy from its surroundings.

8. An __________________________ is a physical/chemical change during which the system releases energy to its surroundings.

***** Classify each of the following as either a physical or chemical change. If applicable, also indicate whether the change is endothermic or exothermic:

grinding coffee beans slicing bread

digesting toast melting ice cream

toasting a marshmallow Jell-O solidifying

CLASSIFICATION OF MATTER (pp. 24 – 29; 34 - 39)

Mixtures and Pure Substances

1. A ____________________ is matter made up of only one kind of atom or molecule.

2. Pure substances have a fixed composition and a unique set of properties.

3. Both elements and compounds can be pure substances.

4. A ____________________ is a collection of two or more pure substances that are physically mixed together. Thus, a mixture cannot be represented by a chemical formula.

5. The properties of different substances in a mixture can vary.

6. The properties of mixtures can vary. Each substance in a mixture retains its chemical identity.

Classification of Mixtures

1. Mixtures can be further classified as either ____________________ or ____________________.

2. A homogeneous mixture is one in which the substances are uniformly distributed throughout.3. A heterogeneous mixture contains substances that are not evenly distributed.

4. Some parts of a heterogeneous mixture have different properties than other parts.

5. Homogeneous mixtures are also known as ____________________.

6. Solutions can be gaseous, liquid, or solid.

Elements

1. ____________________ are the simplest pure substances because they contain only one type of atom. An element cannot be separated into simpler substances by physical or chemical means.

2. Every element has its own unique set of physical and chemical properties.

3. There are 91 naturally occurring elements 113 known elements.

4. About one dozen elements compose the things we notice every day.

5. Elements can consist of single atoms or be diatomic.

6. Some elements have ____________________.

7. Allotropes are different molecular forms of an elements that exist in the same physical state.

Compounds

1. ____________________ are pure substances that are composed of two or more different elements that are chemically combined.

2. They are created when atoms of different elements join together in a chemical reaction.

3. Every compound has a unique set of properties. These properties are often very different from the properties of the elements that make up the compound.

***** Classify each of the following as an element, a compound, a homogeneous mixture, or a heterogeneous mixture:

air bronze

wine glucose (C6H12O6)

table salt (NaCl) mayonnaise

mercury (Hg) oil & vinegar dressing

iron ore copper (II) sulfate (CuSO4)

Family Tree

1. In summary the family tree for matter looks like:

SEPARATION TECHNIQUES (pp. 39 - 41)

1. In order to study the composition of mixtures, they must be separated. This can be accomplished using a variety of physical means.

2. These separation techniques make use of differences in the physical properties of the materials in the mixture.

3. Thus, the materials obtained are not chemically changed by the process.

Techniques

1. ____________________ is used to separate heterogeneous mixtures of solids and liquids by using a porous barrier. The liquid passes through leaving the solid behind.

2. ____________________ is used to separate solids and liquids by allowing the liquid to evaporate, leaving the solid behind.

3. ____________________ uses spinning forces to pull all suspended solids to the bottom of the tube leaving a liquid layer on top.

4. ____________________ is pouring the liquid layer off the top of a solid-liquid mixture once the solid has settled or been centrifuged to the bottom. This can be done with liquid layers, but it is more difficult.5. ____________________ separates the components of a solution. The components (mobile phase) travel across the surface of another material (stationary phase)at different rates based on each other’s attraction to the stationary phase.

6. ____________________ separates the components of a solution based on differences in the boiling points of the substances involved.

***** Ocean water can be made suitable for drinking by boiling the water and then condensing the vapor back to the liquid state. What is the name of this process?

***** A forgetful student leaves an uncapped watercolor marker on an open notebook. Upon returning she discovers the leaking marker has produced a rainbow of colors on the top page.

a. Is the ink a pure substance or a mixture?

b. How do you know?

c. What separation technique is involved.

STANDARD UNITS

1. In 1960, scientists adopted a part of the metric system to use as the standard scientific system of measurement units. This is called the “Systeme Internationale” or SI.

2. There are seven basic units. These base units can be combined in various ways to describe nearly all physical measurements. They are:

Quantity Unit Symbol

Length

Mass

Time

Electric current

Thermodynamictemperature

Amount ofsubstance

Luminous intensity

PREFIXES

1. Any SI unit can be modified with prefixes to match the scale of the object being measured. Meters might be suitable for measuring a person’s height, but not the diameter of a living cell.

Prefix Symbol Meaning Power of Ten

2. The prefixes can be combined with various units to describe the size of a measurement.

***** Suggest appropriate SI units and prefixes to measuring the following objects:

- the length of your chemistry book

- the volume of a bathtub

- the mass of an eyelash

- the volume of an aluminum soda can

DERIVED UNITS - VOLUME

1. The seven base SI units cannot measure every observable property; therefore derived units are created by multiplying or dividing the seven base units in various ways.

2. The derived unit for volume is obtained by using length, width and height measured in meters:

3. We are more familiar with using the liter, L, as a volume unit.

4. More commonly we use the following units to measure volume:

***** Speed is calculated from length and time according to the following equation. What is the derived SI unit?

Speed = distance / time

DENSITY (pp 142 - 146)

1. Density is an intensive property. It does not depend on the quantity of matter present.

2. Density represents a ratio of mass to volume.

3. One interpretation of density is that it is a measure of how tightly matter is packed together.

4. Because the density of a substance is the same for all size samples of that substance, density can be used as a means of identifying materials.

5. To calculate density, one uses the following equation

6. The units for density are usually:

***** Determine the density of a piece of iron whose mass is 31.2 g and volume is 4.00 mL.

***** Clover honey has a density of 0.498 g/mL. Determine the mass of a sample having a volume of 225 mL.

***** Determine the volume of a piece of copper whose mass is 10.5g. The density of copper is 8.94 g/mL.

***** To determine the density of ethyl alcohol, a student pipets a 5.00 mL sample into an empty flask whose mass is 15.246g. She finds that the mass of the flask and the ethyl alcohol is now 19.171g. Calculate the density of the ethyl alcohol.

***** A solid with an irregular shape and a mass of 12.65g is added to a graduated cylinder filled with water to the 29.7 mL mark. After the solid sinks to the bottom, the water level of the graduated cylinder is read to be 36.6 mL. Calculate the density of the solid.

NAME:

PERIOD:

HOMEWORK 2.1 (2013-2014)

a. Read pp. 21 – 24; 29 - 34b. Review your notesc. Answer the following:

1. Classify each of the following as an intensive physical property, an extensive physical property or a chemical property:

Iron and oxygen combine to form rust

Iron is denser than aluminum

Oil and water do not mix

Mercury melts at -390C

Neon is a gas

Hydrogen sulfide smells like rotten eggs

Styrofoam chips take up more space than marbles

2. A student checks the volume, melting point, and shape of two unlabeled samples of matter and finds the measurements are identical. From this she concludes that the samples have the same composition. Explain the error in her thinking and discuss properties that should be checked to help determine the identity of the objects.

3. Describe what happens during a physical change and list three examples of physical change.

4. Describe what happens during a chemical change and list three examples of a chemical change.

5. Classify each of the following examples as a physical change or a chemical change:

a. crushing aluminum can

b. aluminum combining with oxygen to form aluminum oxide

c. a balloon popping

6. In the complete reaction of 22.99 g of sodium with 35.45 g of chlorine, what mass of sodium chloride is formed?

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

NAME:

PERIOD:

HOMEWORK 2.2 (2013-2014)

a. Read pp. 21-29; 34-39 b. Review your notesc. Answer the following:

1. Classify each of the following as either an intensive or an extensive physical property or a chemical property by placing an (X) in the appropriate box:

INTENSIVEPHYSICAL

EXTENSIVEPHYSICAL

CHEMICAL

Color redDensity

FlammabilitySolubility

Reacts with acidCombustibleTastes bitter

Reacts with waterVolumeHardness

Boiling pointLusterOdor

2. Classify each of the following as either a physical change (P) or a chemical change (C)

_____ Hydrochloric acid reacts with sodium hydroxide to produce a salt, water and heat

_____ Aluminum foil is cut in half

_____ Water changes to steam

_____ Potassium chlorate decomposes to potassium chloride and oxygen gas

_____ Iron rusts

_____ A candle melts in the sunlight

_____ Milk sours

_____ Wood rots

_____ A balloon inflating

_____ A leaf changes color

_____ Dew forms on the grass

3. Classify each of the following as either an exothermic process or an endothermic process:

__________Sodium reacts with water to produce a flame _________ Ice melts

__________Butter melts on toast __________Burning magnesium produces a bright light

4. Choose the words from the list to fill in the blanks in the following paragraph (each word may be used only once):

chemical property intensive property compoundmixture element physical propertyextensive property property heterogeneous matterhomogeneous matter substance

Matter that has uniform characteristics throughout is called _________________________. Matter that has

parts with different characteristics is called _________________________. A characteristic by which a

variety of matter is recognized is called a(n) _________________________. A characteristic that depends

upon the amount of matter in the sample is called a(n) _________________________. A characteristic that

does not depend upon the amount of matter is called a(n) _________________________. A characteristic

that can be observed without producing new kinds of matter is called a(n) _________________________.

A characteristic that depends on how a kind of matter changes during interactions with other kinds of

matter is called a(n) ________________________. Matter can also be classified according t the basic

types of matter it contains. A simple substance that cannot be broken down into other substances by

chemical means is called a(n) _________________________. A chemical combination of simple

substances is called a(n) _________________________. A physical combination of different substances

that retain their individual properties is called a(n) _________________________. Either an element or a

compound may be referred to as a(n) _________________________.

5. Classify each of the following as an element, compound, heterogeneous mixture, or homogeneous mixture.

1. water ____________________

2. carbon ____________________

3. air ____________________

4. granite ____________________

5. table salt ____________________

6. homogenized milk ____________________

7. sand in water ____________________

8. oxygen ____________________

9. steel ____________________

NAME:

PERIOD:

HOMEWORK 2.3 (2013-2014)

a. Read pp. 39 - 41 b. Review your notesc. Answer the following:

1. Ocean water can be made suitable for drinking by boiling the water and then condensing the vapor back to the liquid state. What is the name of this process?

2. A forgetful student leaves an uncapped marker on an open notebook. Upon returning, she discovers the leaking marker has produced a rainbow of colors on the top page.

a. Is the ink in the marker a pure substance or a mixture? Explain your answer.

b. What separation technique is involved?

3. Name the separation technique that would be used to separate each of the following:

a. two colorless liquids

b. a nondissolving solid mixed with a liquid

c. a white powdery substance floating in a liquid

4. Crude oil (petroleum) is a mixture of several materials, including gasoline, kerosene, diesel fuel, and heating oil. Explain why distillation is a better method then filtration to separate the various components of crude oil.

NAME:

PERIOD:

HOMEWORK 2.4 (2013-2014)Metric Prefixes - Density

a. Review pp 116 – 121; pp 142 - 146.b. Review your class notesc. Answer/solve the following:

1. For each of the following commonly used measurements, indicate its symbol.

a. _______ milliliter e. _______ milligram i. _______ liter

b. _______ centimeter f. _______ kilogram j. _______ millimeter

c. _______ kilometer g. _______ gram k. _______ meter

d. _______ millisecond h. _______ microgram l. _______ nanometer

2. A piece of tin has a mass of 14.46g. It occupies a volume of 2.00 mL. Calculate the density of the tin.

3. A piece of lead has a mass of 22.7g. It occupies a volume of 2.00 mL. Calculate the density of the lead.

4. The density of chromium is 7.20 g/mL. Calculate the volume of a piece of chromium whose mass is 31.5g.

5. The density of silver is 10.5 g/mL. Calculate the volume of a piece of silver whose mass is 31.5g.

6. A sample of platinum occupies a volume of 10.0 mL. The density of the platinum is 21.41 g/mL. Determine the mass of the platinum.

7. A sample of iron occupies a volume of 10.0 mL. The density of iron is 7.90 g/mL. Determine the mass of the iron.

8. Name the laboratory method used to determine the volume of an irregularly shaped solid.

9. In addition to the above method, describe the other method for determining the volume of a solid having regular, measurable dimensions.

10. Describe the laboratory method used to determine the density of a liquid.

11. Which would have the greater density, a large sheet of aluminum metal or small pellets of aluminum metal? Why?

12. A student is trying to determine whether her necklace is pure silver. The mass of the necklace is 199.0 g. She places the necklace is a graduated cylinder of water and notes that the water level rises from 31.4 mL to 51.9 mL. Calculate the density of the necklace and determine whether it is pure silver. The density of silver is 10.5 g/mL.

NAME:

PERIOD:

UNIT 2 REVIEW (2013-2014)

Classify each of the following as an element, a compound, a homogeneous mixture or a heterogeneous mixture:

Element Compound Homogeneous Heterogeneous1. Flat soda2. Sugar3. Soil4. Iron5. Nail polish6. Carbon dioxide7. Beach sand8. City air9. Nitrogen10. Graphite11. Brass12. Milk13. Titanium14. Blood15. Aluminum

Classify each of the following as an extensive physical property, an intensive physical property or a chemical property:

Extensive Intensive Chemical16. Red color17. Density18. Flammability19. Solubility20. Reacts with acid21. Bitter taste22. Supports combustion23. Melting point24. Reacts with water25. Hard26. Boiling point27. Luster28. Reacts with silver nitrate29. Ductility30. Odor

Classify each of the following as either a physical change or a chemical change

Physical Change Chemical Change31. Sodium hydroxide dissolves in water32. Hydrochloric acid reacts with sodium hydroxide33. Aluminum foil is crumpled34. Water changes to steam35. Iron rusts36. Candle melts in sunlight37. Potassium chlorate decomposes38. A balloon inflates39. Cookies bake in the oven40. A stone is crushed41. A standard light bulb emits light42. Solid air freshener seems to disappear over time43. Breaking a wooden pencil44. Burning gasoline45. Wire is bent

Choose the BEST separation technique for each of the following scenarios by placing an X in the box of the technique. Each techniques may be used only ONCE.

Filtration Evaporation Decanting Centrifuge Chromatography Distillation46. A mixture of alcohol and water47. Separating very fine precipitate particles from a solvent for further study.48. Removing tiny pieces of metal from the oil used to lubricate a car engine.49. Recovering ammonium nitrate that is completely dissolved in water. 50. Comparing the dye pattern of different brands of red markers51. Removing the water layer from a mixture of river water and sediment.

Classify each of the following as either an exothermic process or an endothermic process:

52. ____________________ Sodium reacts with water to produce a flame

53. ____________________ Ice melts

54. ____________________ Dew forms on a windshield in the morning

55. ____________________ Butter melts on toast

56. ____________________ Burning magnesium produces a bright light

57. Calculate the density of a piece of metal that has a mass of 25.0 g and a volume of 6.0 cm3.

58. Calculate the volume occupied by a sample of benzene having a mass of 880.0g and a density of 0.88 g/cm3.

59. Calculate the mass of bromine present when it has a volume of 50.0 cm3 and a density of 3.12 g/cm3.

60. Calculate the mass in grams of 0.675 L of acetic acid; density = 1.05 g/cm3.