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CP Chemistry – January 23, 2007
• 1) Welcome! Please choose any seat with a green sheet.
• 2) Complete the student information sheet on your desk.
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CP Chemistry – January 23, 2007
• 1) Complete Student Information Sheet
• 2) Review Course Syllabus
• 3) Notes: Introduction to chemistry
• 4) Activity: Expectations for course
• 5) Complete Textbook Questionnaire
• 6) Homework: Syllabus Quiz & Interviews
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CP ChemistrySpring 2007
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Chemistry January 25, 2007
• 1) Notes on Chemistry & Branches
• 2)
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Introduction to Chemistry• Chemistry is the study of the
composition of matter and the changes they undergo
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Opportunities for Chemists• Chemists are involved in a variety of different
jobs that include the following:
• a. Textiles
• b. Cosmetics
• c. Development of new medicines such as AZT
• d. Research
• e. Analysis of Substances’ Compositions
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Branches of Chemistry• Chemistry has 5 main branches:
• a. Organic Chemistry: study of substances that contain carbon
• b. Inorganic Chemistry: study of substances that do NOT contain carbon
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Branches of Chemistry Cont• c. Physical Chemistry: deals with the
applications of theories and experiments to describe the behavior of substances
• d. Analytical Chemistry: deals with the composition of substances
• e. Biochemistry: study of the chemistry of living things
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Practicality of Chemistry• Chemistry is practical in that it can be
applied to improving the lives of humans
• Technology is the application of scientific knowledge to improve the quality of life for humans
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Homework Assignment• You are to interview three (3) individuals who had
taken high school Chemistry previously. Record their responses to the following questions:
• 1. Describe your high school Chemistry experience. (What did you learn? How do you remember it?)
• 2. Describe the relevance of Chemistry to your daily life. In other words, describe situations where Chemistry improves your life
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Review Questions• Determine which field of chemistry would most likely
do the following:• a. Predict how a liquid will react as it is cooled to
absolute zero• b. Study the nutritional value of vitamin E in the body• c. Determine the percentage of Calcium ions in ocean
water• d. Study the compounds of nitrogen
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Early History of Chemistry• Science is a continuously changing process
• Early pioneers in chemistry were called alchemists
• Alchemists first appeared with the Taoists in China and Pythagoreans in Greece after the 6th century BCE
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Alchemists• Alchemists sought to transmute (or change) one
substance into another– usually they tried to turn lead into gold
• Early alchemists developed many techniques still used today such as distillation as well as specially shaped bottles such as flasks
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History of Chemistry Continued• Chemistry is derived from an Arabic word
meaning “gold cooking”
• Alchemy declined in the late 1400s as the field of medicine began to grow
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Growth of Chemistry From Alchemy• In 1606, King Charles II formed the “Royal
Society of London.”
• This group used the scientific method to study matter in addition to what alchemists had learned
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Matter and Properties
• Matter is anything that has mass and takes up space
• Matter makes up everything
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Matter and Properties
• There are four states of matter:
• Solid
• Liquid
• Gas
• Plasma
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Solids• Solids have definite shape and volume
• The particles are tightly packed together
• Examples of Solids:
• Coal, Sugar, Gold
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Liquids• Liquids have a fixed volume but change shape
• The particles are NOT as tightly packed together as a solid
• Examples:
• Water, Milk
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Gases• Gases do NOT have a definite shape or
volume
• The particles are very loosely packed together
• Examples:
• Oxygen, Carbon Dioxide
• Liquids and Gases both take the shape of their containers
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Plasma• Plasma is the most common state of matter
in the universe
• It is not commonly found on Earth
• Plasma is a gaseous mixture of electrons and positive ions
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Plasma• Examples:
• Fluorescent and Neon Lights
• The Sun
• Plasma is produced by heating a gas to an extremely high temperature
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Classwork Activity• Arrange the four states of matter in order of
• a. The closeness of the molecules to each other
• b. Provide examples of each type of matter
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Physical Properties• Physical Properties are properties that can
be measured without changing the substance’s composition
• Examples:
• Color, Mass, Melting Point
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Physical Change• Physical Changes are any changes to a
substance that still causes the substance to retain its original properties that it had before
• Examples:
• Melting, Boiling, Cutting, Sublimation
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Activity• Determine which of the following represents
a physical change:
• a. The freezing of water to form ice cubes
• b. The generation of carbon dioxide from Alka Seltzer tablets
• c. The cutting of wood
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Chemical Properties• Chemical Properties are the ability of
different substances to undergo chemical reactions and form new substances
• Examples:
• The burning of wood
• Milk turning sour
• Leaves changing color in the fall
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Chemical Changes• A chemical change occurs when a substance
undergoes a change in composition
• New substances are always formed during a chemical change
• Example: the combustion of methane (CH4) to form H2O and CO2
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Chemical Changes Continued• Chemical Changes usually require or
release energy
• Evidences of a chemical reaction:
• a. Evolution of Light and Heat
• b. Production of a gas
• c. Formation of a solid
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Classifying Substances• Substances can be classified into the
following three groups:
• a. Mixtures
• b. Elements
• c. Compounds
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MatterCan the substance be separated by ordinary physical means?
YES
NO
Mixture
Element or Compound
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Elements• Elements are composed solely of one type
of substance
• Examples:– Fe, Iron; O2, Oxygen; Ca, Calcium
• Elements cannot be broken down further
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Compounds• Compounds are composed of two or
more elements
• Compounds can only be chemical broken down into component elements
• Examples:
• CO2 and H2O
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Mixtures• Mixtures are a combination of two or more
different types of matter
• The different types of matter are not chemical mixed together
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Mixtures
• Mixtures can be separated through physical means
• There are two types of mixtures:
• a. Homogeneous Mixtures
• b. Heterogeneous Mixtures
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Homogeneous Mixtures• Homogeneous Mixtures appear to
be composed of only one form
• They are uniform in composition
• Examples:
• Coffee & Salt Water
• A solution is another name for a homogeneous mixture
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Heterogeneous Mixtures• Heterogeneous Mixtures are composed of
two or more different forms
• They are NOT uniform in composition
• Examples: Sand and Spaghetti Sauce with Meatballs
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E lement sO n e Typ e o f A tom
CompoundsTw o or M ore D iffe ren t
Typ es o f A tom s
S ubst ance(C an W rite C h em ica l F orm u las ;
C on ta in O n ly O n e Typ e o f M atte r)
H omogeneousU n ifo rm C om p os it ion
H et er ogeneousN on -u n ifo rmC om p os it ion
M ix t ur es(C om p osed o f Tw o D iffe ren t
Typ es o f M atte r)
M at t er
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Homework• Find 5 substances at home and classify
them as to element, compound, heterogeneous, and homogeneous mixture. You must find one substance the represents each category of classification
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Practice• Classify each of the
following as element, compound, heterogeneous mixture or homogeneous mixture
• a. Chlorine• b. Water• c. Soil• d. Sugar Water• e. Oxygen• f. Carbon Dioxide• g. Rocky Road Ice Cream• h. Alcohol• i. Pure Air• j. iron
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Chemical Symbols• A chemical symbol is a short hand
abbreviation for each element
• Examples:
• HydrogenH
• Iron Fe
• The symbols come from the English or Latin name for the element
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Chemical Reactions• In a chemical reaction, one or more
substances change into a new substance
• Reactants are the original substances present in a chemical reaction
• Products are the new substances produced
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Chemical Reactions Continued• Chemical reactions are always written in the
following manner:
Reactants Products
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Practice: Identify the reactants and products in the following:
• 1. H2 + O2 H2O
• 2. Mg + O2 MgO
• 3. HgCl2 Hg + Cl2
• 4. Fe(OH)3 + HCl H2O + FeCl3
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Law of Conservation of Mass• Law of Conservation of Mass states that
mass is neither created or destroyed in a chemical reaction
• If 5 g of Na reacts with 10 g of Oxygen completely, what mass of NaO is produced?
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Law of Conservation of Mass Cont• 1) 45 g of hydrogen reacts with 60 g of
oxygen. How much H2O is formed?
• 2) If 500 g of KClO3 decomposes and produces 303 g of KCl, how many grams of O2 are produced?
• 2 KClO3 2 KCl + 3 O2
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Law of Conservation of Mass Continued
• 3. How much CO2 is produced from 200 g of CaCO3 decomposing if 112 g of CaO are produced?
• CaCO3 CaO + CO2