1. Classification of Matter Chapter 3
Larry Emme
Chemeketa Community College

2. Matter Defined

3. Matter is anything that has mass and occupies space.
Matter can be invisible.
Matter appears to be continuous and unbroken.

4. Physical States of Matter

5. Physical Properties of Solids, Liquids, and Gases
State
Shape
Volume
Particles
Compressibility
Solid
Definite
Tightly packed
Very Slight
Liquid
Indefinite
Mobile; Cohering
Slight
Gas
Independent
High

6. Substances and Mixtures

7. Matter refers to all of the materials that make up the universe.

8. Substance
A particular kind of matter that has a fixed composition and distinct properties.
Examples
ammonia, water, and oxygen.
NH3
H2O O2

9. Homogeneous Matter Examples
Matter that is uniform in appearance and with uniform properties throughout.
Examples
ice, soda, solid gold

10. Heterogeneous Matter Examples
Matter with two or more physically distinct phases present.
Examples
wood, blood

11. Phase
A homogenous part of a system separated from other parts by physical boundaries.
Examples
In an ice water mixture ice is the solid phase and water is the liquid phase

12. Mixture
Matter containing 2 or more substances that are present in variable amounts. Mixtures are variable in composition. They can be homogeneous or heterogeneous.

13. Homogeneous Mixture (Solution)
A homogeneous mixture of 2 or more substances. It has one phase.
Example
Sugar and water. Before the sugar and water are mixed each is a separate phase. After mixing the sugar is evenly dispersed throughout the volume of the water.

14. Heterogeneous Mixture
A heterogeneous mixture consists of 2 or more phases.
Example
Sugar and fine white sand. The amount of sugar relative to sand can be varied. The sugar and sand each retain their own properties.

15. Classification of matter: A pure substance is always homogeneous in composition, whereas a mixture always contains two or more substances and may be either homogeneous or heterogeneous.

16. Learning Check Freshly opened Coke is an example of a An element
A compound
A homogeneous mixture
A heterogeneous mixture

17. Learning Check Freshly opened Coke is an example of a An element
A compound
A homogeneous mixture
A heterogeneous mixture

18. Comparison of Mixtures and Compounds
Composition
May be composed of elements, compounds, or both in variable composition
Composed of two or more elements in a definite, fixed proportion by mass
Separation
By physical or mechanical means
Only by chemical changes
Identification
Components do not lose their identity
A compound does not resemble the elements from which it is formed

19. Learning Check
A clear, colorless liquid is heated in a beaker until all of the liquid is gone. The walls of the beaker are coated with a white crystalline solid. The liquid was:
An element
A compound
A homogeneous mixture
A heterogeneous mixture

20. Learning Check
A clear, colorless liquid is heated in a beaker until all of the liquid is gone. The walls of the beaker are coated with a white crystalline solid. The liquid was:
An element
A compound
A homogeneous mixture
A heterogeneous mixture

21. Elements

22. An element is a fundamental or elementary substance that cannot be broken down into simpler substances by chemical means

23. Each element has a number.
All known substances on Earth and probably the universe are formed by combinations of more than 100 elements.
Each element has a number.
Beginning with hydrogen as 1 the elements are numbered in order of increasing complexity.

24. Most substances can be decomposed into two or more simpler substances.
Water can be decomposed into hydrogen and oxygen.
Table salt can be decomposed into sodium and chlorine.
An element cannot be decomposed into a simpler substance.

25. ATOM The smallest particle of an element that can exist.
The smallest unit of an element that can enter into a chemical reaction.

26. Distribution of Elements

27. Elements are not distributed equally by nature.
Oxygen is the most abundant element in the human body (65%).
Oxygen is the most abundant element in the crust of the earth (49.2%).
In the universe the most abundant element is hydrogen (91%) and the second most abundant element is helium (8.75%).

28. Distribution of the common elements in nature.

29. Names of the Elements

30. Sources of Element Names
Greek-Color
Iodine: from the Greek iodes meaning violet.
Latin-
Property
Fluorine: from the Latin fluere meaning to flow.
German-
Color
Bismuth: from the German weisse mass meaning white mass.
Location
Germanium: discovered in 1866 by a German chemist.
Famous-
Scientist
Einsteinium: named for Albert Einstein.

31. Sources of Element Names
Famous-
Warrior
Xenon: named for Xena the warrior princess.
Famous-
Scientist
Rutherfordium: named for Ernest Rutherford.
Location
Californium: discovered in 1950 at the Univ. of California at Berkeley.

32. Symbols of the Elements

33. A symbol stands for the element itself one atom of the element
a particular quantity of the element

34. Rules governing symbols of the elements are:
Symbols have either one or two letters.
If one letter is used it is capitalized.
C carbon
H hydrogen
If two letters are used, only the first is capitalized.
Ba barium
Ne neon

35. 50 Common Elements and Their SymbolsAl
aluminum Cr
chromium Li
lithium Rn
radon Sb
antimony Co
cobalt Mg
magnesium Rb
rubidium Ar
argon Cu
copper Mn
manganese Se
selenium As
arsenic F
fluorine Hg
mercury Si
silicon Ba
barium Ga
gallium Ne
neon Ag
silver Be
beryllium Ge
germanium Ni
nickel Na
sodium B
boron Au
gold N
nitrogen Sr
strontium Br
bromine He
helium O
oxygen S
sulfur Ca
calcium H
hydrogen P
phosphorus Sn
tin C
carbon I
iodine Pt
platinum W
tungsten Cs
cesium Fe
iron K
potassium U
uranium Cl
chlorine Kr
krypton Ra
radium Xe
xenon Pb
lead Zn
zinc

37. Metals, Nonmetals and Metalloids

38. Metals

39. Most elements are metals Metals are solid at room temperature.
Mercury is an exception. At room temperature it is a liquid.
Metals are good conductors of heat and electricity.
Most elements
are metals
physical
properties of metals
Metals are malleable (they can be rolled or hammered into sheets).
Metals have high luster (they are shiny).

41. Metals have high densities
Metals are ductile (they can be drawn into wires).
Most metals have a high melting point.
Metals have high densities

42. Nonmetals

43. Physical Properties of Nonmetals
Lack luster (they are dull)
Have relatively low melting points
Have low densities.
Poor conductors of heat and electricity
At room temperature carbon, phosphorous, sulfur, selenium, and iodine are solids.

44. Metalloids

45. Metalloids have properties that are intermediate between metals and nonmetals

46. The Metalloids
boron
silicon
germanium
arsenic
antimony
tellurium
polonium

47. Metals are found to the left of the metalloids
Nonmetals are found to the right of the metalloids
Metals 1 H 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac
104 Rf
105 Db
106 Sg
107 Bh
108 Hs
109 Mt
110 Ds
111 Rg
112 Cn
113 Nh
114 Fl
115 Mc
116 Lv
117 Ts
118 Og
Metalloids
Nonmetals 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96 Cm 97 Bk 98 Cf 99 Es
100 Fm
101 Md
102 No
103 Lr

48. Compounds

49. A compound is a distinct substance that contains two or more elements combined in a definite proportion by weight.

50. There are two types of compounds: molecular and ionic.

51. Molecules

52. A molecule is the smallest uncharged individual unit of a compound formed by the union of two or more atoms.

53. A water molecule consists of two hydrogen atoms and one oxygen atom.
If it is subdivided the water molecule will be destroyed and hydrogen and oxygen will be formed.

54. Ionic Compounds

55. An ion is a positively or negatively charged atom or group of atoms.

56. A cation is a positively charged ion.

57. Thanks to
Claire de Noyo
Fall 2015

58. An anion is a negatively charged ion.

59. Ionic compounds are held together by attractive forces between positively and negatively charged ions.

60. Thanks to Elizabeth Gimzewski (Fall 2011)

61. Ionic Compound Formulas

62. Sodium chloride and other ionic compounds consist of large aggregates of cations and anions.

63. The actual chemical formulas of ionic compounds express the smallest whole number ratio that exists between these cations and the anions.

64. The formula NaCl does not mean that a molecule of NaCl exists.
The formula NaCl means that the ratio of sodium to chlorine in a sodium chloride crystal is one to one.

65. The ratio of Na+ to Cl- is 1:1

66. Compounds can be classified as molecular or ionic
Compounds can be classified as molecular or ionic. Ionic compounds are held together by attractive forces between their positive and negative charges. Molecular compounds are held together by covalent bonds.

67. Elements That Exist as Diatomic Molecules

68. A diatomic molecule contains exactly two atoms of the same or different elements.

69. Elements That Exist as Diatomic Molecules
Symbol
Molecular Formula
Hydrogen H H2
Nitrogen N N2
Oxygen O O2
Fluorine F F2
Chlorine Cl
Cl2
Bromine Br
Br2
Iodine I I2

71. Chemical Formulas

72. Ca calcium CaCl2 Cl chlorine chemical formulas
Show the symbols of the atoms of the elements present in a compound.
CaCl2
Ca calcium
Cl chlorine

73. CaCl2 chemical formulas
Show the ratio of the atoms of the elements present in a compound.
CaCl2

74. Rules for Writing Chemical Formulas

75. When a formula contains one atom of an element the symbol of that element represents the one atom. The number one (1) is not used as a subscript.

76. NaCl indicates the element sodium (one atom) indicates
the element chlorine
(one atom)

77. When the formula contains more than one atoms of an element the number of atoms is indicated by a subscript written to the right of the symbol of that atom.

78. H3PO4 indicates the element oxygen (O) indicates indicates the element
hydrogen (H)
indicates
the element
phosphorous (P)
indicates
4 O atoms
indicates
3 H atoms

79. When the formula contains more than one of a group of atoms that occurs as a unit, parentheses are placed around the group, and the number of units of the group is indicated by a subscript placed to the right of the parentheses.

80. Ba3(PO4)2 indicates the element barium indicates three Ba atoms
indicates the phosphate group
composed of one phosphorous
atom and four oxygen atoms
indicates three Ba atoms

81. Formulas written as H2O, H2SO4, Ca(NO3)2 and C12H22O11 show only the number and kind of each atom contained in the compound; they do not show the arrangements of the atoms in the compound or how they are chemically bonded to each other.

82. The End