GENERAL CHEMISTRY
Chapter 1: Matter & Its Properties
1.1
Particular Nature of Matter
MATTER
-
Anything that has mass & occupies space (has
volume)
Anything that takes up space and can be weighed
Often taken to mean anything that is composed
of atoms and molecules
IDENTIFICATION OF MATTER AS PER CHEMISTS
 Physical characteristics

- Color
-Size
-Mass
-Shape
Chemical Characteristics
-Interacts with another types of matter
Ex.Corrosion: Rust in Science/Chemistry
Matter is anything that is made of protons, neutron, &
electron
Subatomic particles is the basic foundation of atoms.
Subatomic Particles
-Basic foundation of atoms
PROTON (+)
NEUTRON ( )
ELECTRON (-)
STRUCTURE OF MATTER
ATOM
-
Building blocks of matter
In constant motion
Composed of PROTON, NEUTRON, ELECTRONS
NUCLEUS: Center of Atom
PROTONS AND NEUTRONS are always inside the nucleus.
ELECTRONS of an atom are found orbiting the nucleus
of the atom.
(-)
(+)
()
All substances are composed of invisible particles called
ATOM.
Combination of atoms leads to millions of materials with
different properties.
Atoms are made up of a positively recharged center, nucleus
(+)
ELEMENTARY PARTICLES (Quarks): smaller than
subatomic particles.
WHICH IS NOT A MATTER
-Time
-Radiation
-Rainbow
-Energy
-Thoughts
-Gravity
-Sound
-Sunlight
-Microwave
-Heat
-Magnetism
1.2 States of Matter
LOW TEMP – HIGH TEMP (Phases of Matter)
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Fermionic Condensate (Coldest)
Boss-Einstein Condensate
Solid
Liquid
Gas
Plasma
Quark-Gluon Plasma (Hottest)
1.FERMIONIC CONDENSATE
-a superfluid phase formed by fermionic particles at
very low temperature, formed by FERMIONS.
FERMIONS
-Zero Energy
-Anti-Social Elementary Particle
-Coldest
-Can be seen in laboratories
2.BOSE-EINSTEIN CONDENSATE (BEC)
-A state of matter created when particles called
BOSONS, are cooled to near absolute zero (-273
centigrade or -460 Farenheit)
BOSONS
-Social Elementary Particle
-Elementary Particle opposite to
fermion
3.SOLID
-A state of matter where there is a definite MASS,
VOLUME, & SHAPE.
4.LIQUID
-A nearly incompressible fluid that conforms to the
shape of its container but retains a nearly constant
volume independent of pressure. Liquids has definite
MASS and VOLUME but no definite shape.
5.GAS
-A substance that is gaseous, or vaporous state of
matter. This state of matter has NO definite mass,
volume, and shape.
6.PLASMA
-Appears when the atoms are in excited state
-In heat or extreme temperature (ex.sun,fire,star)
7.QUARK-GLUON PLASMA
-A new state of nuclear existing at extremebly high
temperatures and densities when composite states
called HADRON (proton.neutron,electron) lose their
identity & dissolve into a soup of their
constituent-quarks & gluons.
-Quite connected to bigbang theory.
PROCESS INVOLVED IN CHANGING PHASES OF MATTER
Through our naked eye, we can only observe solid, liquid ang gas.
Water exists in three stages:
Water : liquid
ice : solid
water vapor: gas
Need ENERGY to change the phases of matter.
The relationship between temperature spaces between the
molecules are directly proportional; the farther the spaces the
hotter the temperature and vice versa.
ENERGY: when energy is added to a substance that energy causes
the particles in the substance to move faster.
PHASE CHANGE
-Energy content is responsible for the different phases of matter.
-The higher the energy content the faster the phase change
- (DIRECTLY PROPORTIONAL)
2 TYPES OF PHASE CHANGE
1. Endothermic change (Adding Energy)
2. Exothermic change (Removing Energy)
ENDOTHERMIC CHANGE (Adding Energy)
-Phase change that requires the addition of
energy.
(endo: inside , therm: heat)
Phase change that are
endothermic:
1. Melting (solid – liquid)
2. Sublimation (Solid – gas)
3. Boiling (liquid – gas)
4. Vaporization (liquid – gas)
5. Evaporization (liquid to gas)
1. MELTING (Solid to Liquid)
- Melting is the changing of liquid to solid when the substance
absorbs energy.
MELTING POINTS
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TABLE SALT: 801 C
DIAMOND: 3700 C
WATER: 0 C / 32 F
MP = FP
2. SUBLIMATION (Solid to Gas)
-Solid to gas phase change occurs
-Ex. Dry ice goes directly from solid carbon dioxide to gas.
-Opposite of sublimation if deposition (gas to solid)
3. BOILING (Liquid to Gas)
-If enough heat energy is applied to a substance particles inside the
liquid can change to gas. These particles travel to the surface of the
liquid.
BOILING POINT
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WATER: 100 C
TABLE SALT: 1413 C
DIAMOND: 4300 C
4. VAPORIZATION (Liquid to Gas)
-Vaporization is the changing of a liquid to a gas when the substance
absorbs heat energy.
-It occurs in the surface
Vaporization VS. Boiling (Difference)
 Vaporization – on the surface
 Boiling – Transfers the temperature from the bottom to the
surface.
5. EVAPORIZATION (Liquid to Gas)
-It is the cooling process
-As water in the perpiration evaporates from your skin it absorbs and
carries away heat energy from your body.
Perspiration: Helpful thing to maintain your homeostasis
Homeostasis: Yourself – surroundings
EXOTHERMIC CHANGE (Removing Energy)
-Phase change that requires the removal of
energy.
(exo: outside , therm: heat)
Phase change that are exothermic:
1. Freezing ( liquid - solid )
2.Condensation ( gas – liquid )
3.Deposition (gas –solid)
1. FREEZING (Liquid to Solid)
- Opposite of melting; liquid changing to solid is freezing.
-Freezing occurs when a substance loses heat energy
-The freezing point of a substance is equal to the melting point.
2. CONDENSATION (Gas to liquid)
-Gases can change phase also in a gas to liquid phase change
-A substance in the gas phase that loses heat will change into liquid.
This is called CONDENSATION.
-“They tend to equalize their temperature with the surrounding”
-Water vapor in surrounding air loses heat energy when it comes in
contact with the cold gas; water vapor condenses.
3. DEPOSITION (Gas to solid)
1.3 Physical and Chemical Properties of Matter
COMPOSITION
-the components of a sample of matter
-their relative proportion
Ex.
Co2
- C + 2O = Co2
H2O
- 2H + O = H2o
PROPERTIES
-Qualities or attributes that we can use to
distinguish one sample of matter from others.
2 CATEGORIES
1. PHYSICAL PROPERTIES
2. CHEMICAL PROPERTIES
1.Physical Properties
-A trait of matter than can be observed or
measured without changing the chemical
composition of the matter.
Physical Change
– No chemical reaction allowed.
- Retain its identity
1. Color:
- How the object absorbs & reflects light.
2. Texture:
- How the substance looks & feels.
3. Temperature:
- A measure of the average kinetic energy
(energy of motion) of particles in a
substance.
4. Mass:
- Amount of matter in an object (in g or kg)
DIFFERENCE OF MASS & WEIGHT
MASS
WEIGHT
Not affected by
gravity
Affected by
gravity
5. Volume:
- The amount of space an object occupies. (in
ml, L, cm, m, etc.)
6. Density:
- Ration of mass to volume; reflects the
degree of packing of particles in matter.
DENSITY OF MATTER
Highest Density
Lowest Density
Hydrogen
Osmium (23 g/cm^2)
7. Luster:
- the wat that a substance reflects light
(metallic, non-metallic, glassy, pearly,
dull)
8. Ductility:
- Ability of a substance to be stretched into
a wire (wire-like).
9. Malleability:
- Ability of a substance to be hammered flat
and to retain the old shape.
10. State (Phase) of matter (S,L,G…)
- Solid, Liquid, Gas
11. Melting point/Freezing point:
- The exact temperature at which solid
becomes a liquid or a liquid becomes solid.
INTENSIVE VS. EXTENSIVE PROPERTIES OF MATTER
INTENSIVE PROPERTY:
- Does not depend on amount of substance
present.
- Ex. 1kg nail: nail 2kg nail: is still a nail
- Are determined by the chemical composition of the particles
and their structure (arrangement)
EXTENSIVE PROPERTY:
- One that does depend on the amount of
substance present.
- Depend only on the numbers of particles not
on their composition or internal
arrangement.
2. CHEMICAL PROPERTIES (Attributes)
-A trait of matter that can only be observed if
a substance has the property. In the process of
testing the chemical property.
Chemical Change
-Chemical Reaction
-Identity Changes
1. Reactivity with Oxygen
- Rusting
- Tarnishing
2. Reactivity with water
- Reactivity with water means how easily and
quickly an element or a compound reacts
with water
- Some substances are water-reactive, meaning
they spontaneously undergo a chemical
reaction with water, as they are highly
reducing in nature
- Examples of water-reactive substances are
alkali metals and alkaline earth materials.
3. Reacting with acids & Basics
4. Combustibility / Flammability
- Combustibility is the ability of solid to
be fired.
- Flammability: a liquid that is put to fire.
5. Chemical Formula (Chemical Composition)
- What something is made of is always…
“All chemical properties are intensive. None are
extensive”
-Because chemical properties never depend on how
much/ the amount.
-Intensive properties make the best characteristic
properties because intensive properties are
determined by the composition & structure.
1.4
Classification of Matter
-Mixture
-Pure Substance
= PURE SUBSTANCE =
-SOMETHING THAT CAN NOT BE BROKEN DOWN INTO SIMPLER
MATTERS USING PHYSICAL METHODS.
2 TYPES OF PURE SUBSTANCE
1. ELEMENTS – Simplest kind of pure substance.
2. COMPOUNDS - A compound is a substance made up
of two or more different chemical elements
combined in a fixed ratio.
“NOT ALL ELEMENTS ARE EQUALLY COMMON”
MOST ELEMENTS CAN EXIST AS A SINGLE ATOM
DIATOMIC GASES
HYDROGEN
H2
NITROGEN
N2
OXYGEN
O2
FLOURINE
F2
CHLORINE
Cl2
BROMINE
Br2
IODINE
L2
ALLOTROPES
-different structural forms of the same element.
e x a m p l e: OXYGEN HAS 3 ALLOTROPES
O2:
O3:
O4:
Monotomic
Oxygen
Diatomic
Oxygen
Molecule
Ozone
Molecule
Allotropes of Carbon
 Diamond
 Fullereness
 Graphite
 Carbon Nanotubes
All are pure substance. Each
has different structure.
= COMPOUNDS =
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2 OR MORE ELEMENTS BOUNDED TOGETHER
COMPOSED OF MULTIPLE ELEMENTS
CANNOT BE BROKEN DOWN BY PHYSICAL METHODS
CAN BE BROKEN DOWN BY CHEMICAL REACTIONS
COMPOUNDS CAN DECOMPOSE
HAVE DEFINITE COMPOSITION
The properties of compounds are very different from
the properties of elements that make them up.
ex. Na + Cl = NaCl (Sodium Chloride)
Na (Sodium) : explosive
Cl (Chlorine) : poisonous
NaCl: No longer poisonous or explosive
= MIXTURE =
-SOMETHING THAT CAN BE BROKEN DOWN INTO SIMPLER
MATERIALS USING PHYSICAL METHODS.
3 POSSIBLE TYPES OF MIXTURE
1. Element + Another element
2. Compound + Another compound
3. Element + Compound
MAIN (2) TYPES OF MIXTURE:
1. HOMOGENOUS MIXTURE
2. HETEROGENOUS MIXTURE
MAIN TYPES OF MIXTURE
HOMOGENOUS MIXTURE
-parts are distributed
evenly. (uniform)
HETEROGENOUS MIXTURE
-parts are distributed
unevenly.
Ex. Salt water
Ex.Spaghetti, Meatballs,
water + oil mixture
Solutions
– homogenous liquid mixture
Alloys
– homogenous metallic mixture
-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.
COMPOUND VS. MIXTURE
COMPOUND
MIXTURE
-Properties of compound are
-The properties of mixture are
totally different from the
realted.
properties of elements that
make them up.
MATTER FLOWCHART
METHODS OF SEPARATING MIXTURES INTO THEIR OWN
COMPOUND
1. Mechanical Separation (Often done by hand)
-Takes advantage of physical properties such as colors &
shapes.
-In other words arranging
Ex. Recycling plastic, paper, metal
2. Magnetic Separation
-Takes advantage of the physical property of magnetism.
3. Filtration (Uses filtering material)
-Takes advantage of the physical property of the state of
matter.
2 TYPES OF FILTERING
1. Solid – Liquid : coffee maker
2. Solid – Solid : Sand sieve
4. Decanting
-Solid/Liquid on product
-To pour off a liquid, leaving another solid or liquid behind
-Decantation is a process for the separation of mixtures of
immiscible liquids or of a liquid and a solid mixture such as a
suspension
-Does not use filtering material
5. Distillation
-The separation of a mixture of liquid
-Distillation, the process involving the conversion of a liquid
into vapor that is subsequently condensed back to liquid
form.
-A simple distillation definition or distillation meaning is a
process of purifying a liquid compound by heating it into a
vapor that is then condensed back into a liquid. By heating a
liquid to the temperature at which it turns into a vapor, it is
separated from any possible impurities that are dissolved
within it.
6. Evaporation
-vaporizing a liquid
-liquid to gas
7. Density separation
-Always liquid product
-This process step is meant to separate materials based on
their weight to process them further in different lines. Smart
and compact solutions based on density principles allow
separation of materials with specific gravity characteristics.
8. Centrifuge
-Circular motion helps denses components sink to the
bottom faster.
-Centrifugation is a technique used for the separation of
particles from a solution according to their size, shape,
density, viscosity of the medium and rotor speed. The
particles are suspended in a liquid medium and placed in a
centrifuge tube. The tube is then placed in a rotor and spun
at a define speed.
9. Paper Chromatography
-Uses the property of molecules attraction to separate a
mixture.
10. Fractional Crystallization
-dissolved substance crystallize out of a solution once their
solubility limit is reached as the solution cools.