Post on 11-Jan-2016
Unit 1. Matter and ChangeChapter 1 and 3
Do Now:
What is matter as described in Chemistry?
Chapter 1 & 3
Objective Distinguish between:
intensive and extensive properties Physical & chemical changes/properties Classify matter
Matter and its Properties It’s Classified!
But first what is Scientific Method and what does it involve?
Properties & Changes in Matter
Extensive vs. Intensive
Physical vs. Chemical
A. Extensive vs. Intensive Extensive Property
depends on the amount of matter present
ex,.-
Intensive Property depends on the identity of substance, not
the amount
Ex.-
A. Extensive vs. Intensive Extensive Property
depends on the amount of matter present
ex,.- Volume, mass, Energy
Intensive Property depends on the identity of substance, not the
amount
Ex.- melting point, boiling point, conduct electricity or heat
WHAT ABOUT DENSITY??
A. Extensive vs. Intensive Examples:
boiling point
volume
mass
density
conductivity
A. Extensive vs. Intensive Examples:
boiling point…… intensive
Volume …. extensive
Mass ….. extensive
Density ….. intensive
Conductivity ….. intensive
PROPERTYB. Physical vs. Chemical Physical Property
can be observed without changing the identity of the substance
Chemical Property describes the ability of a substance to
undergo changes in identity
B. Physical vs. ChemicalExamples:
melting point
flammable
density
magnetic
tarnishes in
air
physical
chemical
physical
physical
chemical
CHANGEC. Physical vs. Chemical Physical Change
changes the form of a substance without changing its identity
properties remain the same
Chemical Change changes the identity of a substance products have different properties
B. Physical vs. Chemical Signs of a Chemical Change
change in color or odor
formation of a gas
formation of a precipitate (solid)
change in light or heat
B. Physical vs. Chemical Examples:
rusting iron
dissolving in water
burning a log
melting ice
grinding spices
B. Physical vs. Chemical Examples:
rusting iron
dissolving in water
burning a log or
charcoal
melting ice
grinding spices?
chemical
physical
chemical
physical
physical
In the example of burning of charcoal, carbon and oxygen are the reactants in the combustion reaction. Carbon dioxide is the product.
carbon + oxygen carbon dioxide
C + O2 CO2
(reactants) (product)
Properties and Changes in Matter
Homework Review Scientific Method:
Read page 12 – 16 Q 17
Complete - Work sheet
STATE OF MATTER
Chapter 3
Do Now Name the State of Matter
How do they differ?
States of Matter There are Four state of matter A. Solid B. Liquid C. Gas D. Plasma
State of matter depends on Kinetic Energy between the particles
A. Kinetic Molecular Theory
KMT
Particles of matter are always in motion.
The kinetic energy (speed) of these particles increases as temperature increases.
Four States of Matter
A. Solidsvery low KE - particles
vibrate but can’t move around
fixed shape fixed volume
Four States of Matter
B. Liquids low KE - particles can
move around but are still close together
variable shapefixed volume
Four States of MatterC. Gases
high KE - particles can separate and move throughout container
variable shapevariable volume
Four States of MatterD. Plasma
very high KE - particles collide with enough energy to break into charged particles (+/-)
gas-like, variableshape & volume
stars, fluorescentlight bulbs, CRTs
SOLUTIONS AND
MIXTURES
Objective: Classification of Matter
DO NOW: What is a solution? Describe the difference between a
heterogeneous and homogenous mixture
A. Pure Substances Element
composed of identical atoms EX: copper wire, aluminum foil
A. Pure Substances
Compound composed of 2 or more elements
in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)
A. Pure Substances Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions Elements can combine in different ratios to form
different compounds.
A. Pure Substances For example…
Two different compounds, each has a definite composition.
Pure Substances(constant composition)
Elements Listed on the Periodic
Table Cannot be broken down
into unique components Na, Cl, Al, O2, S8
Compounds Made of elements that
are chemically joined Can be broken down NaCl, H2O, AlCl3, H2SO4
B. Mixtures Variable combination of 2 or more pure substances.
Heterogeneous Homogeneous
B. Mixtures(variable composition)
Homogeneous – Solutions evenly distributed
Heterogeneous not evenly distributed
B. Mixtures
Solutionhomogeneousvery small particlesno Tyndall effect
Tyndall Effect
B. MixturesColloid
heterogeneousmedium-sized particlesTyndall effectparticles don’t settleEX: milk
B. MixturesSuspension
heterogeneous large particlesTyndall effectparticles settleEX: fresh-squeezed
lemonade
C. Mixtures Examples:
mayonnaise
muddy water
fog
saltwaterItalian salad dressing
C. Mixtures Examples:
mayonnaise
muddy water
fog
saltwaterItalian salad dressing
colloid
suspension
colloid
solution
suspension
A. Matter Flowchart
MATTER
Can it be physically separated?
Homogeneous Mixture(solution)
Heterogeneous Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be chemically decomposed?
noyesIs the composition
uniform?
noyes
Colloids Suspensions
A. Matter Flowchart Examples:
graphite
pepper
sugar
(sucrose)
paint
soda
A. Matter Flowchart Examples:
graphite
pepper
sugar
(sucrose)
paint
soda
element
hetero. mixture
compound
hetero. mixture
solution
Air – Homogeneous Mixture
Alloys – Homogeneous Mixtures
Cereal – Heterogeneous Mixture
Sand – Heterogeneous Mixture
Separating MixturesOnly a physical change- no new matter Filtration - separate solids from liquids
with a barrier (filter paper)
Distillation - separate liquids because of different boiling points Heat mixture Catch vapor in cooled area
Chromatography - different substances are attracted to paper or gel, so move at different speeds
Separating Mixtures cont…. Crystallization - results in formation of
solid particles of a substance from a solution containing the dissolved substance
Sublimation – separation when a solid changes to a vapor without melting or going through a liquid phase
Filtration Distillation Chromatography
d. Crystallization e. SublimationEx: rock candy Ex: Dry Ice
Homework Pg 83 – Q 15, 17
Pg 94 & 95 – Q 42, 43, 48, 58, 63
The Periodic Table
A. Mendeleev
Dmitri Mendeleev (1869, Russian) Organized elements
by increasing atomic mass.
Elements with similar properties were grouped together.
There were some discrepancies.
C. Johannesson
A. Mendeleev Dmitri Mendeleev (1869, Russian)
Predicted properties of undiscovered elements.
C. Johannesson
B. Moseley Henry Moseley (1913, British)
Organized elements by increasing atomic number.
Resolved discrepancies in Mendeleev’s arrangement.
C. Johannesson
II. Organization of theElements
A. Metallic CharacterMetalsNonmetalsMetalloids
C. Johannesson
B. BlocksMain Group
ElementsTransition MetalsInner Transition
Metals
C. Johannesson
Do Now: Classify the following as either a METAL, NON-METAL or METALLOID:
a. Aub. Sic. Br
Periods and Families Periods: horizontal rows on the periodic
table physical and chemical properties change
somewhat regularly across a row. Elements closer to each other in the same
period tend to be similar properties than those that are farther apart.
Families: vertical rows of elements, aka groups Each group contains similar chemical
properties
Types of ElementsMETALS:
Shiny
Conductors of heat and electricity
Most metals are malleable (can be pounded into thin sheets; a sugar cube sized chunk of gold can be pounded into a thin sheet which will cover a football field),
Most metals are ductile (can be drawn out into a thin wire).
Metals cont…..
All are solids at room temp (except Mercury, which is a liquid)
Metals tend to have low ionization energies, and typically lose electrons (i.e. are oxidized) when they undergo chemical reactions
Alkali metals are always 1+ (lose the electron in s subshell)
Alkaline earth metals are always 2+ (lose both electrons in s subshell)
Compounds of metals with non-metals tend to be ionic in nature.
Types of ElementsNON- METALS:
Vary greatly in appearance Non-lustrous Poor conductors of heat and electricity The melting points of non-metals are
generally lower than metals Seven non-metals exist under standard
conditions as diatomic molecules: H2(g) N2(g) O2(g) F2(g) Cl2(g) Br2(l) I2(l) (volatile liquid - evaporates readily)
Non-Metals cont…….. Nonmetals, when reacting with metals,
tend to gain electrons (typically attaining noble gas electron configuration) and become anions: Nonmetal + Metal -> Salt
Compounds composed entirely of nonmetals are molecular substances (not ionic)
Types of Elements
Metalloids:
Elements may share properties of metals and non-metals.
A stair-step line separates the metals from the nonmetals on the periodic table.
Metalloids Properties: All metalloids are solids at room temperature.
Less malleable than metals but not as brittle as nonmetals.
Metalloids tend to be semiconductors of electricity. (intermediate between metals and nonmetals).
Metalloids
Properties:
Metalloids are used in semiconducting materials found in computers, calculators, televisions and radios.
Elements include: boron, silicon, germanium, antimony
Noble Gases Noble Gases - the elements in Group
18 of the periodic table. They are considered nonmetals. These elements are generally
unreactive. All are gases at room temperature. Examples: neon, argon, krypton,
xenon (all used in lighting) and helium.
DO NOW:Name an element that is:
a. An element that is brittle and conducts electricity
b. An element that is malleablec. An element that has tendency to
become an anion
Group Practice Look at Page 95 – Insert Questions
Law of Conservation of Matter:
Matter is neither created nor destroyed.
Since chemical reactions cannot create or destroy atoms, chemical equations representing the reactions must always be BALANCED.
Mass reactants = Mass products
% by Mass of Substance
Mass of Element Percent by mass = X
100
Mass of Compound