1. Matter – Properties and Changes
Properties of Matter
Changes of Matter
Mixtures of Matter
Elements and Compounds

2. PROPERTIES OF MATTER Types of Properties
Physical Properties - properties that can be observed and measured without changing the composition
examples – color, texture, hardness)
types of physical properties
1) intensive - do not depend upon amount of
the substance
2) extensive - depend upon amount of

3. Properties- Physical Examples: length color mass volume density phase
conductivity
texture

4. Properties of Matter
chemists use characteristic properties to tell substances apart and to separate them
some properties define a group of substances

5. Types of Properties
Physical- characteristics that can be observed or measured without changing the identity of a substance
Ex. melting point, boiling pt
Chemical- relates to a substances ability to undergo changes that transform it into a different substance
Easiest to see when a chemical is reacting

6. Physical Changes in Matter
change in a substance that doesn’t change the identity of the substance
Ex. grinding, cutting, melting, boiling
Includes all changes of state (physical changes of a substance from one state to another)

7. Solid definite volume definite shape
atoms are packed together in fixed positions
strong attractive forces between atoms
only vibrate in place

8. Liquid definite volume indefinite shape atoms are close together
atoms can overcome attractive forces to flow

9. Gases indefinite volume indefinite shape atoms move very quickly
atoms are far apart
pretty weak attractive forces

10. Changes of State

11. Plasma high temperature state in which atoms lose their electrons
Ex. the sun

12. CHANGES IN MATTER Types of Changes
1. physical - changes in which a substance is altered without changing composition
a. examples- phase changes, cut into pieces
2. chemical - changes in which one or more substances change into new substances with
new properties
a. reactants – substances that react
b. products - substances that are produced

13. PROPERTIES OF MATTER Types of Properties
Chemical Properties - properties relating to the ability of substances to combine with or change into other substance (has a uniform and unchanging composition)
examples
1) reaction with water
2) ability to combine with oxygen
3) reaction with acids

14. Changes Chemical Changes that result in a new substance
a.k.a chemical reaction
Word equation:
hydrogen + oxygen  water
reactants product
copper + silver nitrate  silver + copper nitrate

15. Changes Chemical Formula Equation Cu + 2AgNO3  Cu(NO3)2 + 2Ag
Pb(NO3) KI  PbI KNO3
(be able to identify reactants and products)

16. Chemical changes Examples of chemical changes 1) digestion of food
2) burning (combustion)
3) fermentation
4) rusting
5) tarnishing of silver

17. CHANGES IN MATTER Evidence of Chemical Changes
1. change in color and/or appearance
2. change in energy
3. change in odor
4) formation of a precipitate or a gas

18. Energy Changes in Matter
when any change occurs, energy is always involved
energy can be in different forms (light, heat, etc.)
energy is never destroyed or created (law of conservation of energy)

19. Energy changes related to chemical changes (reactions)
exothermic - energy is released (given off in the form of heat or light)
- burning, explosion
endothermic - energy must be continuously added to keep the reaction going
- electrolysis of water or salt

20. Energy Changes in Matter
Exothermic Reaction- reaction that gives off energy (feels warm on outside)
Endothermic Reaction- reaction that uses up energy (feels cold on outside)

21. MIXTURES
A. Definition of Mixture - combination of pure substances that retain their properties
B. Types of Mixtures
1. heterogeneous - individual substances are distinct (composition is not uniform throughout)
a. examples – sand, vegetable soup
2. homogeneous - individual substances are not distinct (uniform composition throughout)
a. examples - solutions

22. MIXTURES Types – homogeneous
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type of solution examples
solid – liquid sugar water, salt water
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gas – liquid carbonated beverages
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liquid – liquid alcohol, vinegar
gas – gas air
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solid - solid alloys (metal + metal)

23. MIXTURES Separating Mixtures
1. Filtration
2. Distillation
3. Crystallization
4. Chromatography

24. Separation Techniques
Filtration- solid part is trapped by filter paper and the liquid part runs through the paper
Vaporization- where the liquid portion is evaporated off to leave solid

25. Separation Techniques
Decanting- when liquid is poured off after solid has settled to bottom
Centrifuge- machine that spins a sample very quickly so that components with different densities will separate

26. Separation Techniques
Paper Chromatography- used to separate mixtures because different parts move quicker on paper than other

27. Elements

28. ELEMENTS AND COMPOUNDS Element-a pure substance that cannot be broken down by simple means
The periodic table organizes the 91 naturally occurring elements and scientifically created elements
A. Mendeleev created the original periodic table.

29. Periodic Table

30. Periodic Table
two rows below the periodic table are the lanthanide and actinide series
these rows fit after #57 and #89
they are only at the bottom to keep the width of the chart smaller

31. Types of Elements Metals
an element that is a good conductor of electricity
at room temperature, most are solids
malleable- can be rolled or hammered into sheets
ductile- can be made into wire
high tensile strength- can resist breakage when pulled
most have silvery or grayish white luster

32. Types of Elements Nonmetals
an element that is a poor conductor of heat and electricity
many are gases at room temperature
some are solids: usually brittle, not malleable

33. Types of Elements Metalloids
an element that has some characteristics of metals and nonmetals
appear along staricase line
B, Si, Ge, As, Sb, Te
all are solids at room temperature
less malleable that metals but less brittle than nonmetals
are semiconductors

34. Types of Elements Noble Gases generally unreactive gases
in far right column of periodic table

35. ELEMENTS AND COMPOUNDS Compounds
definition - a compound is a pure substance that is the combination of two or more different elements
ie: NaCl – table salt
Na- combustible solid and Cl – poisonous gas
examples of compounds
a. sodium bicarbonate NaHCO3
b. hydrochloric acid HCl
c. sulfur dioxide SO2

36. ELEMENTS AND COMPOUNDS Compounds
examples of formation of compounds from elements (synthesis reactions)
a. 2 Na + Cl > 2 NaCl
b. 2 H2 + O > 2 H2O
c. N H > 2NH3

37. ELEMENTS AND COMPOUNDS Compounds
examples of decomposition of compounds to form elements
a. 2NaCl  2Na + Cl2
b. 2 H2O  2H2 + O2

38. The organization of Matter

39. Can it be separated by physical means?
Matter Flowchart
MATTER
yes no
Can it be separated by physical means?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be decomposed by chemical means? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element

40. The Law Conservation of Mass
States that mass can neither be created nor destroyed.
Mass of reactants = mass of products
28 g of Na + 28 g of Cl = 56 g of NaCl

41. Law of Conservation of Mass and chemical changes-
Mass reactants = Mass products
(mass is neither created nor destroyed in chemical reactions)
Lavoisier ( ) experiment
[ 216 g of HgO --> 200 g Hg + 16g O2 ]
216 grams of mercury oxide when heated will produce 200 grams of mercury and 16 grams of oxygen

42. Law of Definite Proportions
1.Definition - a compound is always composed of the same elements in the same proportions by mass
2. examples
a. water- H2O (always has a ratio of 1 gram of
hydrogen to 8 grams of oxygen)
b. ammonia - NH3 (always combine in a ratio of 14 grams of nitrogen to 3 grams of hydrogen)

43. Law of Multiple Proportions
1. definition - when different compounds are formed by a combination of the same elements, different masses of one element will combine with the same relative mass of the other element in a ratio of small whole numbers

44. Law of Multiple Proportions
WATER (H2O)
2 grams of hydrogen combine with 16 grams of oxygen
PEROXIDE (H2O2)
2 grams of hydrogen combine with 32 grams of oxygen
The ratio that compares the amount of oxygen in water and peroxide is 1:2

45. Law of Multiple Proportions
SULFUR DIOXIDE (SO2)
32 grams of sulfur combine with 32 grams of oxygen
SULFUR TRIOXIDE (SO3)
32 grams of sulfur combine with 48 grams of oxygen
The ratio that compares the amount of oxygen in sulfur
dioxide and sulfur trioxide is 2:3

46. Periodic Table Groups Periods also called families vertical columns
numbered 118
have similar chemical properties
Periods
horizontal rows
properties changes consistently across a period