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Chapter 2 Matter
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Section 1 Classifying Matter
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What is matter? Matter: anything that has mass and takes up space
Any materials you can hold or touch! Even air!!!
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How can matter be classified?
Classifying matter is based on what makes up the matter. 3 groups: Elements Compounds Mixtures
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Can elements be broken down into simpler substances?
Element: substance that can’t be broken down or separated by chemical means Made up of one kind of atom Atom: smallest unit of an element that keeps the element’s chemical properties
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Can elements be broken down into simpler substances?
Represented by symbols that are usually one or two letters O = Oxygen H = Hydrogen Ca = Calcium Pb = Lead
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Periodic Table lists all the elements and symbols
Molecule: combination of two or elements that are combined in a definite ratio
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How is a compound different from an element?
Compound: substance made up of atoms of different elements Contains 2 or more elements that are chemically combined Fe2O3 H2O NaCl
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When elements combine in a compound, they always combine in the same proportions!
H2O is always H2O H2O2 is NOT H2O
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Compounds Every compound differs from the elements that it contains (unique properties) Hydrogen gas Oxygen gas Water: H2O
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Chemical formulas are used to represent compounds
Shows how many atoms of each element are in a substance The number of atoms of each element is written as a subscript after the elements symbol
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4. How is a compound different from an element?
C12H22O11 How many carbon (C)? How many hydrogen (H)? How many oxygen (O)?
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Pure Substances and Mixtures
Pure Substance: matter that has a fixed composition and definite properties
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Mixture: combination of two or more pure substances that are not chemically combined
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Mixtures can be physically separated into parts.
Elements and Compounds are pure substances because they are chemically combined and can’t be physically separated Mixtures can be physically separated into parts. Parts of pure substances are chemically combined and can’t be physically separated.
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Classify mixtures on how well substances mix.
Homogeneous Mixture: components are evenly distributed
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Classify mixtures on how well substances mix.
Heterogeneous Mixture: substances that are not evenly distributed
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Miscible and Immiscible
Miscible: homogeneous mixture made up of many different liquids that can be mixed and stay mixed Example: Vinegar
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Miscible and Immiscible
Immiscible: Mixture that does not mix or will not stay mixed. Example: Oil and Water
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Review section 1 compound element homogeneous mixture heterogeneous
anything that has mass and takes up space substance that can’t be broken down or separated by chemical means smallest unit of an element that keeps the element’s chemical properties substance made up of atoms of different elements matter that has a fixed composition and definite properties substances that are not evenly distributed—can see parts components are evenly distributed—cannot see parts compound element homogeneous mixture heterogeneous mixture pure substance atom matter
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Label as element (E) or compound (C)
____ copper, Cu ____ iron oxide, Fe2O3 ____ water, H2O ____ cobalt, Co ____ carbon monoxide, CO ____ sulfur, S8 ____ salt, NaCl ____ mercury, Hg C C E C E C E
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Label as heterogeneous mixture (E) or homogeneous mixture (O)
____ a salad ____ salt water ____ Kool aide ____ vinegar ____ chocolate syrup ____ banana split ____ human blood ____ muddy water O O O O E O E
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Heterogeneous mixture, solution, element or compound?
Silver Gold Sugar water Paper Salt water alcohol E E S HM S C
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Heterogeneous mixture, solution, element or compound?
India ink Apple Carbon dioxide Copper Wood Aluminum air HM HM C E HM E S
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Heterogeneous mixture, solution, element or compound?
Salt Italian salad dressing Hydrogen Hot tea with sugar in it Cold tea with sugar in it Milk oxygen C HM E S HM HM E
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Heterogeneous Mixture
Matter Anything that has mass and occupies space Pure substances Fixed composition and properties Element Its atoms have the same number of protons Compound 2 or more elements chemically combined Mixture Variable composition and properties Homogeneous Mixture Uniform: cannot see the parts (solution) Heterogeneous Mixture Nonuniform: can see the parts
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Section 2 Properties of Matter
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7. Why are color, volume, and density classified as physical properties?
Because physical properties are defined as characteristics that can be observed without changing the identity of the substance For example: Shape Color Odor Texture
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8. What are 3 ways physical properties can help us classify substances?
Can help identify substances It is cold and wet—ice cream It is red, so STOP at the stop light!!! Can be observed and measured using our senses State of matter Melting point, boiling point Strength Hardness Magnetism
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8. What are 3 ways physical properties can help us classify substances?
Help determine uses Ability to conduct heat or electricity—then we can make pots and pans to use for cooking
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Summary: Physical properties
Shape Color Odor Texture State of matter Melting point Boiling point Strength Hardness Magnetism Ability to conduct heat Ability to conduct electricity
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9. Define density. A measurement of how much matter is contained in a certain volume of a substance The ratio of the mass of a substance to the volume of the substance D = M ÷ V or D = M/V Unit is g/cm3 or g/mL M D V
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10. How is density different from weight?
Density is mass/volume Weight is a measure of the pull of gravity on an object Weight can change e.g. on the moon an object will weigh less than on earth Density does not change on the moon—the same as here on earth
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Density problems M D V
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Density problems Diamond has a density of 3.26 g/mL. What is the mass of a diamond that has a volume of 0.35 mL? M = DV M = (3.26 g/mL)(0.35 mL) M = 1.14 grams M D V
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Density problems What is the volume of a sample of mercury that has a mass of 76.2 grams and a density of 13.6 g/mL? V = M / D V = 76.2 grams / 13.6 g/mL V = 5.60 mL M D V
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Density problems M D V Do the sheet of density problems.
Show work, just like my previous slides!!! Make sure each answer has a correct unit: Density is g/mL or g/cm3 Mass is grams Volume is mL or cm3 M D V
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answers M D V M = 2282.75 g M = 21.83 g M = 972.00 g V = 5.49 cm3
D = 3.16 x g/cm3 D = 0.70 g/cm Most likely gasoline M = g V = cm3 M D V
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Density problems The largest ruby in the world is 10.9 cm long, 9.10 cm wide, and 5.80 cm thick, giving it an overall volume of 575 cm3. If the density of ruby – a form of aluminum oxide – is 3.97 g/cm3, what is the mass of the largest ruby? M = DV M = (3.97)(575) M = g M D V
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Density problems Certain compounds called aerogels form rigid, lightweight foams that can support a mass many times greater than their own. If a sample of an aerogel has a volume of 87.3 cm3 and a density of g/cm3, what is its mass? M = DV M = (0.250)(87.3) M = g M D V
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Density problems Osmium, a hard, heavy metal used to make durable alloys, has a density of 22.5 g/cm3, the greatest density of any element. If a sample of osmium has a volume of 43.2 cm3, what is its mass? M = DV M = (22.5)(43.2) M = g M D V
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Density problems Magnesium is a fairly light metal that is combined with other elements to form lightweight alloys for use in airplanes. The big advantage of magnesium is that it has a relatively low density of 1.74 g/cm3. If a sample of magnesium has a mass of 9.56 g, what is its volume? V = M / D V = (9.56) / (1.74) V = 5.49 cm3 M D V
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Density problems Moon rocks are samples of the moon's crust that were collected and returned to Earth by crew members of the various Apollo missions. Many of the moon rocks are made of basalt, a light, volcanic rock with a density of about 2.7 g/cm3. If a moon rock has a mass of 432 g, what is its volume? V = M / D V = (432) / (2.7) V = cm3 M D V
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Density problems Although both diamond and graphite consist of pure carbon, they have very different densities. This is because of differences in the way the carbon atoms in each substance are arranged. If you had a diamond with a mass of 1.5 g and a density of 3.51 g/cm3, what would its volume be? V = M / D V = (1.5) / (3.51) V = 0.43 cm3 M D V
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Density problems Outer space is often described as a vacuum, but there is always some matter present. In the space 300 km above Earth's surface, there is as little as 1.58 x g of matter in a cm3 volume of space. Based on this data, what is the density of the matter in space? D = M / V D = 1.58 x 10-12 5.0 x 102 Subtract exponents! D = x g/cm3 D = 3.16 x g/cm3 M D V
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Density problems The volume of a liquid that fills a flask is 750 cm3. The mass of the liquid is 525 g. What is the liquids density? Is it most likely to be water (D = 1.0 g/cm3), gasoline (D = 0.70 g/cm3), or ethanol (D = 0.79 g/cm3) D = M / V D = (525) / (750) D = 0.70 g/cm3 Most likely gasoline M D V
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Density problems Because inland seas like the Caspian Sea or the Great Salt Lake evaporate faster than they can be refilled, they have higher concentrations of salts than oceans have. The highest concentration of salts in any body of water is found in the Dead Sea, in Israel. If you had 1230 cm3 of this water, which has a density of 1.22 g/cm3, what would be its mass? M = DV M = (1.22)(1230) M = g M D V
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Density problems Density 21.5 is the title of a composition written for a musician with a platinum flute. Platinum's density is closer to g/cm3. If the platinum flute's mass is 2000 g, what is its volume? V = M / D V = (2000) / (21.45) V = cm3 M D V
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More Density Problems M D V 0.85 g/cm3 1.98 g/cm3 1.11 g/cm3
8.85 g/cm3 copper cm3 g cm3 cm3 0.03 g/cm3 1.98 g/cm3 1.26 g/cm3 7.81 g/cm3 3.54 cm3 cm3 15.46 g g 41.42 g M D V R
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11. Why are flammability and reactivity classified as chemical properties?
Chemical properties describe how a substance changes into a new substance, either by combining with other elements or by breaking apart into new substances Reactivity is the capacity of a substance to combine chemically with another substance
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11.Why are flammability and reactivity classified as chemical properties?
Chemical properties describe how a substance changes into a new substance, either by combining with other elements or by breaking apart into new substances Flammability is the ability to burn—or the ability to combine with oxygen in the air s.3
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Review of section 2 Characteristics that can be observed without changing the identity of the substance The ratio of the mass to the volume of a substance Describes how a substance changes into a new substance Measure of the pull of gravity on an object Capacity of a substance to combine chemically with another substance Ability to burn flammability reactivity weight density physical property chemical property
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review of section 2 A gold nugget having a mass of 153 grams was found to have a volume of 7.92 mL. What is its density? What is the mass of 4000 mL of mercury if the density of mercury is 13.6 g/mL? Calculate the volume of a sample of carbon tetrachloride having a mass of 82 grams and a density of 1.60 g/mL
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review of section 2 M D V A gold nugget having a mass of 153 grams was found to have a volume of 7.92 mL. What is its density? D = M / V D = (153 g) / (7.92 mL) D = g/mL
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review of section 2 M D V What is the mass of 4000 mL of mercury if the density of mercury is 13.6 g/mL? M = DV M = (13.6 g/mL)(4000 mL) M = g
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review of section 2 Calculate the volume of a sample of carbon tetrachloride having a mass of 82 grams and a density of 1.60 g/mL V = M / D V = (82 g) / (1.60 g/mL) V = mL M D V R
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Section 3 Changes of Matter
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12. Define and give an example of a physical change of matter.
A change of matter from one form to another without a change in chemical properties e.g. breaking chalk melting ice cutting hair crushing a can energy can be absorbed or released without the formation of a new material
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13. Why is dissolving a physical change of matter?
sugar in water: the sugar is still there sugar molecules are spread out between water molecules molecules of sugar do not change
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14. Define and give an example of a chemical change of matter.
a change that occurs when one or more substances change into entirely new substances with different properties examples leaves changing color in the fall effervescent tablets—release gas batteries die oxygen breathed in, carbon dioxide breathed out
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chemical change examples
chemical changes fruits & vegetables ripen food is digested baking burning food fading paint iron rusting chemical changes can only be reversed by other chemical changes
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15. Why must mixtures and compounds be separated in different ways?
mixtures can be separated by physical changes, they are NOT chemically combined compounds can only be broken down by chemical changes, they are chemically combined D
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Section 3 Review Change of matter from one form to another without a change in chemical properties Change of matter that occurs when one or more substances change into entirely new substance with different properties physical change chemical change
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Physical property or Chemical property?
Color Magnetism Reactivity Stability Melting point Flammability Ability to conduct heat physical physical chemical chemical physical chemical physical
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Physical property or Chemical property?
Shape Strength texture Odor State of matter physical physical physical physical physical
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Physical change or Chemical change?
Fading of dye in cloth Digestion of food Baking a cake Frying an egg Burning coal Kicking a football Crushing a can Cutting hair chemical chemical chemical chemical chemical physical physical physical
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Physical change or Chemical change?
Growth of a plant Melting butter Formation of clouds Tearing paper Exploding TNT Melting of ice Dissolving sugar in water chemical physical physical physical chemical physical physical
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Physical change or Chemical change?
Burning butter Healing of a wound Perming your hair Pounding a piece of copper Digging a hole in the ground Leaves turning color in the fall chemical chemical chemical physical physical chemical
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Chapter 2 Review pp. 70 - 73 Using Key Terms # 4 , 7
Understanding Ideas # 8 – 14 Critical Thinking # 20 , 21 Graphing Skills # 23 Math Skills # 24 – 26 Understanding Concepts # 1 – 3 Reading Skills # 7, 8 Interpreting Graphics # 9, 10
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