FIRST SEMESTER Ways of classifying matter

GENERAL CHEMISTRY I a. Pure substances and Mixtures

Pure substances- form of matter that has a definite (constant)
composition and distinct properties. Pure substances are composed of
CHAPTER 1: MATTER AND ITS PROPERTIES only one component.
Mixtures- is a combination of two or more substances in which the
The Particulate Nature of Matter substances retain their distinct identities. Mixtures are composed of
Particles Composing Matter several components.
ATOMS - the smallest particles b. Elements and Compounds
MOLECULES - composed of atoms Elements- have a definite or fixed, composition and distinct properties.
IONS - particles with charges Pure substances that are made up of only one kind of atoms. Possible
examples: iron; gold; mercury.
States of Matter Compounds- have a definite or fixed, composition and distinct
Solid properties. Pure substances made up of two or more kinds of atoms.
 closely packed; restricted motion Possible examples: salt; sugar; water.
 fixed shape and volume c. Homogeneous and Heterogeneous Mixtures
 cannot be compressed Homogeneous Mixtures- a mixture whose composition is uniform all
 strong forces between the particles throughout. It has a uniform composition and exhibits the same
Liquid properties in different parts of the mixture.
 far apart; free movement Heterogeneous Mixtures- mixture in which the different components
 fixed volume but does not have fixed shape are easily recognized. Has a non-uniform composition and its
 cannot be compressed easily properties vary in different parts of the mixture.
 weaker than the forces in a solid
Gas Elements: The Building Blocks of Matter
 very far apart; very free (chaotic) movement Arrangement of Elements In The Periodic Table
 does not have fixed shape or volume Series/Periods- rows or horizontal arrangement are numbered with
 can be compressed easily Arabic numerals from 1 to 7.
 weak forces between the particles Families/Groups- columns or vertical arrangement, each group is also
Plasma assigned with numbers through several ways.
 made up of electrons and ions of gases A group elements- Representative or main group elements (1A-8A)
 require special conditions to maintain state B group elements- Transition elements. The elements in the two long
rows at the lower section of the table are known as the inner transition
 requires electricity
elements. (1B-8B)
 plasmas like gases have an indefinite shape and an
57 to 71 elements- Lanthanide elements or lanthanides
indefinite volume
89 to 103 elements- Actinide elements or actinides
Bose-Einstein Condensate
Group 1A- Alkali metals
 Is a gas-like state of matter that exists at extremely cold
Group 2A- Alkaline Earth metals
temperatures
Group 3A- Boron group
 It forms when the particles that make it up have a very low Group 4A- Carbon group
energy, when matter is in the BEC state it has zero viscosity Group 5A- Nitrogen group
 discovered by Albert Einstein and Satyendra Nath bose in Group 6A- Chalcogens or Oxygen group
1920’s Group 7A- Halogens
 the atoms are bosons; sociable Group 8A- Noble gases
Fermionic Condensate
 similar to BEC Classifications of Elements:
 superfluid phase formed by fermionic particles at low Metals
temperatures  hard
 the atoms are fermions; antisocial  ductile, they can be made into thin wires
 discovered in December 2003 by Deborah Jin  they are also malleable, they can be hammered without
breaking them
Physical and chemical properties  good conductors of heat and electricity
Non-Metals
Physical properties- no change in composition takes place during the  easily break
determination or measurement of these properties.  they cannot be hammered and molded without breaking.
Examples of Physical Property:
 they are insulators
Color, odor, taste, volume, hardness, density, boiling point, texture,
 like metals, non-metals have many uses also
electrical conductivity, solubility, malleability, tensile strength.
Metalloids
Chemical properties- a change in composition occurs during the
 behave like metals and non-metals
determination or measurement of these properties.
Examples of Chemical Property:  they have the same physical appearance as metals
1. Exposure of peeled potatoes to air causes it to oxidize and so, turn  they behave chemically like non-metals
brown.
2. Silver jewellery tarnish
3. Flammability
4. Corrosiveness
5. Reactivity with acids
Extensive properties- change their value when the amount of matter
or substance is changed. Examples: volume, mass, length, area.
Intensive properties- do not change their value when the amount of
matter is changed. Examples: color, odor, texture, hardness, density.
Characteristics Properties of Metals, metalloids, and on-metals:

Property Metals Non-Metals Metalloids

Appearance Shiny Can be shiny Dull

surface or dull
(metallic
luster )
Ductility/Mall Malleable & Shapes is Brittle, hard
eability ductile easily or soft, tend
(flexible) as changed to break
solids
Boiling/Meltin High melting Vary widely Low melting
g point point, and point and low
density density
Conductivity Conduct Tend to make Poor
heat and good conductors of
electricity semiconductor heat and
s electricity
Nature of Metallic Oxides can be Acidic in
solution/type oxides are acidic or basic, nature
of bonds basic in exhibit
nature, ionic amphoteric
bonded, property
form ionic
compounds

Compounds can also be classified into ACIDS, BASES, and SALTS.

ACIDS
 substances which ionize in water to produce hydrogen ion
(H+)
Properties of an Acid
 tastes sour
 conduct electricity
 corrosive, which means they break down certain substances
 some acids react strongly with metals
 turns blue litmus paper red
Uses of Acids
 Acetic Acid = Vinegar Methods of separating mixtures into their component substance
 Citric Acid = lemons, limes, & oranges. It is in many sour 1. Filtration- is a process used to separate an insoluble solid
candies such as lemonhead & sour patch. (precipitate) from a mixture.
 Ascorbic acid = Vitamin C which your body needs to 2. Distillation- is a process whereby a liquid is converted into vapour
function. by boiling and the vapour is condensed back to liquid by cooling.
 Sulfuric acid is used in the production of fertilizers, steel, 3. Crystallization-is a method to separate a soluble solid from its
paints, and plastics. solution based from the different solubility of solids in water at 25
 Car batteries degree Celsius.
BASES 4. Decantation- is a process of separating a solid from a liquid by
pouring of a liquid, after allowing the solid to settle in the liquid.
 substances which ionize to produce hydroxide ions in water.
5. Dissolution- is another method in which a mixture of a soluble and
Properties of a Base
insoluble solid substances can be separated by using an appropriate
 feel slippery
solvent.
 taste bitter 6. Chromatography-is a versatile technique for separating mixtures,
 corrosive the mixture flow over a material that retains some components more so
 can conduct electricity. (Think alkaline batteries.) different components flow over the material at different speeds.
 do not react with metals. 7. Sublimation-is the process of changing solid to the gaseous form
 turns red litmus paper blue. without passing through the liquid state.
Uses of Bases
 bases give soaps, ammonia, and many other cleaning Chemistry in the Society: Applications
products some of their useful properties. 1. Food
 the OH- ions interact strongly with certain substances, such 2. Water
as dirt and grease. 3. Shelter
 chalk and oven cleaner are examples of familiar products 4. Health and Sanitation
that contain bases. 5. Clothing
SALTS 6. Energy
 are crystalline compounds formed by the reaction of an acid 7. Education and communication
and a base. 8. Arts
9. Personal care products
pH Scale 10. Sports and Recreation
 pH is a measure of how acidic or basic a solution is. 11. Travel
 the pH scale ranges from 0 to 14. 12. Defense and Security
 acidic solutions have pH values below 7
 a solution with a pH of 0 is very acidic.
 A solution with a pH of 7 is neutral.