Unit%201B%20%20Matter%20Properties%20

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Unit 1B Matter Properties Changes
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Section IClassification of Matter
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(No Transcript)
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• Mixture
• DEF a combination of two or more substances in
  which the basic identity of each substance is not
  changed

NaCl H2O Salt water
Pure substance Pure substance Mixture

1. can be separated by physical means
2. retains its own properties
3. can be classified as heterogeneous or homogeneous

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Heterogeneous Mixture

• DEF a mixture that does not have a uniform
  composition and in which the individual
  substances remain distinct
• can see individual substances (phases)

granite
salad
banana split
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Homogeneous Mixture

1. DEF a mixture that has a uniform composition
   throughout and always has a single phase
2. also called a solution

Saline solution
steel
pure air
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• Consists of two (2) parts
• solute DEF the substance that is being
  dissolved
• solvent DEF the substance that dissolves the
  solute
• salt water - salt (solute), water (solvent)
• Aqueous solution (aq)
• DEF solvent is water
• universal solvent

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1. can be solid, liquid, or gas

G-G Air
G-L Carbonated beverage
S-S Steel (iron carbon), alloy
S-L Salt water
L-L Vinegar
L-G Water vapor
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Separating Mixtures

• Filtration
• DEF a technique that uses a porous barrier
  (filter paper) to separate a solid from a liquid
• sand and water

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• Based on unique physical properties
• Magnetism can separate a sand-iron mixture

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• Sieve
• DEF a technique that uses a screen with
  different pore sizes that separate solids of
  different sizes
• sand and rocks

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• Evaporation
• DEF a technique that removes the liquid from a
  solution, usually to leave a solid
• salt and water

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• Distillation
• DEF a technique that is based on differences in
  the boiling points of the substances involved

alcohol (bp 80oC) and water (bp 100oC)
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• Chromatography
• DEF technique that separates the components of a
  mixture on the basis of the tendency of each to
  travel or be drawn across the surface of another
  material
• colors in ink

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• Pure Substances
• DEF matter with the same fixed composition and
  properties
• two (2) types of Pure Substances
• Elements
• Compounds

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Elements

1. DEF a substance that cannot be broken down into
   simpler substances
2. Building block of all matter
3. composed of one type of atom (EX copper)
4. only 92 elements occur naturally on earth

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Organizing the Elements

• Periodic Table
• DEF a chart that organizes all known elements
  into horizontal rows (periods) and vertical
  columns (groups or families)
• Each element has a unique chemical name and
  symbol
• Chemical name (named after)
• people (Einsteinium)
• countries (Germanium)
• states (Californium)
• mythological figures (Plutonium)
• Latin name (Iron-ferrum Fe)

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• Symbol
• contains 1,2 or 3 letters
• 1st letter is capitalized others are lower case
• K (Potassium)
• Na (Sodium)
• Uun (Ununnilium)

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Compounds

• DEF a chemical combination of two or more
  elements joined together in a fixed proportion
• can be broken down into simpler substances by
  chemical means
• EXAMPLE water (H2O), salt (NaCl), sugar
  (C6H12O6)
• Has properties that are different from those of
  its elements

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• Formula
• DEF combination of the chemical symbols that
  show what elements make up a compound and the
  number of atoms of each element
• EXAMPLE C12H22O11
• 12 atoms carbon
• 22 atoms hydrogen
• 11 atoms oxygen

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Law of Definite Proportions

1. DEF states that, regardless of the amount, a
   compound is always composed of the same elements
   in the same proportions by mass

H2O 2 H 1 O
NaCl 1 Na 1 Cl

1. Percent by mass ()

by mass Mass of element x 100
Mass of compound
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Percent by Mass
A 78.0 g sample of an unknown compound contains
12.4 g of hydrogen. What is the percent by mass
of hydrogen in the compound?
by mass Mass of element x 100
Mass of compound
Hydrogen 12.4 g x 100
78.0 g
15.9
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Percent by Mass
What is the percent by mass of carbon in glucose
(C6H12O6)?
C 6 x 12 g 72 g
H 12 x 1 g 12 g
O 6 x 16 g 96 g
180 g
(mass of compound)
Carbon 72 g x 100
180 g
40.0
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Law of Multiple Proportions

1. DEF states that when different compounds are
   formed by the combination of the same elements,
   they combine in small-whole number ratios

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Section IIProperties and Changes of Matter
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• Physical Properties
• DEF characteristics of a sample of matter that
  can be observed or measured without any change in
  its identity
• EXAMPLE color, electrical conductivity, boiling
  point, melting point, density, state of matter
  (solid, liquid, or gas)

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States of Matter

• DEF physical forms of matter
• Four (4) states of matter
• Solid
• Liquid
• Gas
• Plasma
• state of matter is based upon
• particle arrangement
• energy of particles
• distance between particles

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SOLID

1. DEF a form of matter that has a definite shape
   and definite volume
2. particles vibrate in place

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LIQUID

1. DEF a form of matter that has a definite volume
   but takes the shape of its container
2. particles vibrate in place are able to slip past
   each other which allows liquid to flow

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GAS

• DEF a form of matter that has no definite shape
  and no definite volume takes the shape of its
  container
• Particles are far apart and constantly moving
• Gas vs. Vapor
• Gas a substance that is naturally in the
  gaseous state at room temperature
• EXAMPLE Helium

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• Vapor the gaseous state of a substance that is
  a solid or liquid at room temperature
• EXAMPLE Steam

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PLASMA

1. DEF a form of matter that does not have a
   definite shape or volume and whose particles have
   broken apart
2. composed of electrons and positively charged ions
3. conducts an electric current (gases do not)
4. affected by electric and magnetic fields which is
   used to contain plasma (gases are not)

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• Artificial plasma created by passing electric
  current through gases
• EXAMPLE fluorescent lights, plasma TV

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STATES OF MATTER
SOLID
LIQUID
GAS
PLASMA
Tightly packed, in a regular pattern Vibrate, but
do not move from place to place
Close together with no regular arrangement. Vibrat
e, move about, and slide past each other
Well separated with no regular arrangement. Vibrat
e and move freely at high speeds
Has no definite volume or shape and is composed
of electrical charged particles
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• Chemical Properties
• DEF a property that can be observed only when
  there is a change in the composition of a
  substance
• Describes the ability or inability of a substance
  to react with other substances or to decompose
• EXAMPLE ability to rust, unreactive, flammable

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• Physical Change
• DEF a change in matter that does not involve a
  change in the identity of the substance
• same substance remains after change
• EXAMPLE change of state, dissolving

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• Melting is an example of a reversible change. For
  example, when chocolate is warmed until it melts,
  the melted chocolate can be changed back into
  solid chocolate by cooling.

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• Chemical Change
• DEF the change of one or more substances into
  other substances
• also called a chemical reaction
• evidence of a chemical change
• precipitate
• gas formation
• color change
• energy change
• Odor

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• Law of Conservation of Mass (LOCOM)
• DEF matter is neither created nor destroyed
  during a chemical reaction
• Massreactant Massproduct

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Law of Conservation of Mass
From a laboratory process a student collected
10.0 g hydrogen and 79.4 of oxygen. How much
water was originally involved?
Massreactant Massproduct
Masswater Masshydrogen Massoxygen
Masswater 10.0 g 79.4 g
89.4 g
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Law of Conservation of Mass
A 10.0-g sample of magnesium reacts with oxygen
to form 16.6 g of magnesium oxide. How many
grams of oxygen reacted?
Massreactant Massproduct
Massmagnesium Massoxygen MassMgO
10.0 g Massoxygen 16.6 g
6.6 g
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Energy

• DEF capacity to do work
• all physical and chemical changes require energy
• can be exothermic or endothermic

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Exothermic

• DEF chemical reaction that gives off heat energy
• EXAMPLE burning wood in a fireplace

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Endothermic

• DEF chemical reaction that absorbs heat energy
• EXAMPLE photosynthesis
• absorbs light energy from sun and produces sugars
  from carbon dioxide and water