Download Chapter 1 - Manual Science Chemistry/Physics

 Chapter 1: Matter and Change
o Prior Knowledge:
 Energy, atom, element, compound, proton, neutron, and electron.
o Reading Toolkit:
 K/W/L:
 What do you know about chemistry?
 What do you want to know about chemistry?
 What have you learned about chemistry?
o Section 1: Chemistry is a Physical Science
 Overview: Defines the field of chemistry and distinguishes between different branches of
chemistry.
 Objectives:
 Define chemistry
 List examples of the branches of chemistry
 Compare and contrast basic research applied research, and technological development.
 Main Ideas:
 Chemistry is the study of matter and its processes.
o A chemical is any substance that has a definite composition.
o What questions does chemistry seek to answer?
o Why do we use instruments in science?
o What is the benefit of having standard measurements?
o What are some things that are not made up of at least one chemical?
o Micro-structure vs Macro-structure
 There are several branches of chemistry.
o Science and technology are different. Science is the acquisition of knowledge
and technology is the application of that knowledge.
o Organic – the study of most carbon-containing compounds
o Inorganic – the study of non-organic substances
o Physical – the study of the properties and changes of matter and their
relationship to energy
o Analytical – the identification of the components and composition of materials
o Biochemistry – the study of substances and processes occurring in living things
o Theoretical – the modeling and prediction of chemical behavior
o Basic Research – done for the sake of increasing knowledge
o Applied Research – done to solve a problem
o Technological Development – done to develop and produce products
 Questions:
 Explain what chemistry is.
 Name six branches of study in chemistry.
 Compare and contrast basic research, applied research, and technological development.
 Scientific and technological advances are constantly changing how people live and work.
Discuss a change you have observed in your lifetime that has made life easier or more
enjoyable for you.
o Section 2: Matter and Its Properties
 Overview: Defines matter and contrasts major physical and chemical changes that matter can
undergo. This section also outlines the basic form of a chemical equation and describes how
matter is classified.
 Objectives:
 Distinguish between the physical properties and chemical properties of matter.
 Classify changes of matter as physical or chemical.
 Explain the gas, liquid, and solid states in terms of particles.
 Explain how the law of conservation of energy applies to changes in matter.
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 Distinguish between a mixture and a pure substance.
Main Ideas:
 Atoms are the building blocks of matter.
o The fundamental building blocks of matter are atoms and molecules.
 Volume – amount of space an object occupies.
 Mass – a measure of the amount of matter.
 Matter – anything that has mass and takes up space.
 Atom – smallest unit of an element that maintains the chemical identity
of that element.
 Molecule – smallest stable unit of a substance; can be composed of one
or more kinds of atoms.
 Element – a pure substance that cannot be broken down into simpler,
stable substances, and is only made up of one type of atom.
 Compound – a substance that can be broken down into simpler stable
substances. Made up of two or more elements that are chemically
bonded.
 All substances have characteristic properties.
o Properties distinguish substances
o A property may define a group of substances
o Properties can be used to identify unknown substances
 Extensive Properties – depends on the amount of matter present
 Intensive Properties – does not depend on the amount of matter
present
 Physical Properties – can be observed/measures without changing the
chemical identity of the substance.
 Physical Change – a change that doesn’t change the chemical identity of
a substance.
o States of Matter
 Change of State – a physical change of substance from one state to
another, i.e. melting or boiling
 Solid – definite volume and definite shape; lowest amount of
energy
 Liquid – definite volume but indefinite shape
 Gas – neither definite volume or shape
 Plasma – high temperature physical state in which atoms lose
most of their electrons; highest amount of energy
 Chemical Properties – a substance’s ability to undergo changes that
would transform it into a different substance
 Chemical Change/Reaction – a change where one or more substances is
changed into one or more substances
 Reactants – substances that react in a chemical change
 Products – substances that are formed in a chemical
change/reaction
o Most chemical/physical reactions involve a transfer in energy
 A transfer in energy can take many forms, such as heat or light
o Law of conservation of mass/energy is always followed in chemical reactions
 Reactants  Products + Products
 Matter can be a pure substance or a mixture.
o All matter can be classified in terms of uniformity of composition and the
properties of a given sample
o Mixtures – a blend of two or more kinds of matter, each of which retains its own
identity and properties
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Homogenous – same proportion/composition of components
throughout. Also called solutions.
 Heterogeneous – not uniform
Separating Mixtures
 Filtration
 Decantation
 Centrifugation
 Chromatography
 Electrolysis
 Decomposition
Pure Substances – either compounds or elements
 Every sample of a pure substance has the same exact characteristic
properties
 Every sample of a pure substance has the exact same composition
Laboratory Chemicals and Purity – laboratory grade chemicals are generally
treated as though they are pure, but all chemicals have some impurities.
Questions:
 What is the main difference between physical properties and chemical properties?
o Give an example of each.
 Classify each of the following as either a physical change or a chemical change:
o Tearing a sheet of paper
o Melting a piece of wax
o Burning a log
 How do you decide whether a sample of matter is a solid, a liquid, or a gas?
 Contrast mixtures with pure substances.
 Compare the composition of sucrose purified from sugar cane with the composition of
sucrose purified from sugar beets. Explain your answer.
Section 3: Elements
 Overview: Introduces the periodic table as a classification scheme for the elements with
descriptions of metals, nonmetals, and metalloids.
 Objectives:
 Use the periodic table to name elements, give their symbols.
 Use the periodic table to write the symbols of elements, given their names.
 Describe the arrangement of the periodic table.
 List the characteristic that distinguish metals, nonmetals, and metalloids.
 Main Ideas:
 The periodic table organizes elements by their chemical properties
o Elements serve as the building blocks of matter.
o Elements cannot be decomposed by chemical changes
o Each element has characteristic properties
o The vertical columns of the periodic table are called groups, or families.
 Each group’s elements have similar properties.
o The horizontal rows of elements in the periodic table are called periods.
 Physical and chemical properties change somewhat regularly across a
period.
 Elements that are closer together in the same period tend to be more
similar than those farther apart.
 Some elements are metals
o An element that is a good conductor of heat and electricity
o Tend to have a metallic luster, or “shininess”
o Tend to be malleable
o Tend to be ductile, due to high tensile strength
o Other characteristics can vary tremendously
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Some elements are nonmetals or metalloids
o Nonmetals
 Many are gases at room temperature
 Tend to be brittle
 Tend to have low conductivity of heat and electricity
o Noble Gases
 Generally nonreactive
 All gases
o Metalloids
 All solids at room temperature
 Tend to be semiconductors
 Tend to be intermediate in conductivity, malleability, and luster
Questions
 Use the periodic table to write the names for the following elements: O, S, Cu, Ag.
 Use the periodic table to write the symbols for the following elements: iron, nitrogen,
calcium, mercury.
 Which elements are most likely to undergo the same kinds of reactions, those in a
group, or those in a period?
 Describe the main differences between metals, nonmetals, and metalloids.
 If you find an element in nature in its pure elemental state, what can you infer about the
element’s chemical reactivity? How can you tell whether that element is a metal or a
nonmetal?