States of matter PART-I Matter and Types

1. STATES OF MATTER
Matter and Types
PART-I
Nabeela Moosakutty
Lecturer
Dept. of Pharmaceutics
KTN College of Pharmacy

2. States of Matter
• Different forms of matter:
• Solid
• Liquid
• Gas
•
State depends on 2 things:
• Particle (atoms/molecules) arrangement
• Particle motion

3. Solid Matter
•
•
•
Fixed volume
Fixed shape
Particles packed
together tightly –
usually in a repeating
pattern
Examples: wood,
glass, salt, plastic

4. Solid Matter
•
•
Particles vibrate in place
• remember – matter is always in motion!
Want to separate the particles in a solid?
BREAK it!

5. Liquid Matter
•
•
•
•
•
Fixed volume, changing
shape
Particles can move
from place to place
Particles attracted to
each other, but more
easily separate
Take the shape of the
container its put in
Examples: milk, oil,
honey, water

6. Gas Matter
•
•
•
Volume changes, shape
changes
Examples: air, oxygen,
water vapor
Particles always push
outward on container
• Spread to fill
container if there is
more space
• Or pack closer
together when there
is less space =
PRESSURE from the
pushing!

8. • THREE STATES OF MATTER
Some Characteristics of Gases, L iquids and Sol ids and the
M icroscopic E xplanation for the B ehavior
Gas Liquids Solids
assumes the shape and
volume of its container
particles can move past one
another
assumes the shape of the
part of the containerwhich
it occupies
particles can move/slide
past one another
retains a fixed volume and
shape
rigid - particles locked into
place
compressible
lots of free space between
particles
not easily compressible
little free space between
particles
not easily compressible
little free space between
particles
flows easily
particles can move past one
another
flows easily
particles can move/slide
past one another
does not flow easily
rigid - particles cannot
move/slide past one
another

9. • TYPES OF I NTERMOLECULAR FORCES
Dispersion forces
or London forces
Itis theweakestintermolecularforce
It is a temporary at ractiveforcethat
results whentheelectronsin two
adjacent atoms occupy positions that
make theatoms form temporarydipoles
This forceis sometimescal edan
induceddipole- induceddipole at
raction
Theseatractiveforces that cause
nonpolar substances to condenseto
liquids and tofreezeinto solids when
thetemperatureis loweredsuf iciently

10. DIPOLE- DIPOLEFORCES
Dipole-dipole forces are at ractiveforces betweenthepositive end
of onepolar
molecule and the negative end of another polar molecule. Dipole-
dipole forces havestrengthsthatrange from5 kJ to20 kJ per
mole.They aremuchweaker
than ionic or covalent bonds and have a significant ef ect
only whenthe moleculesinvolvedareclose
together(touching oralmost touching).

11. INDUCED-DIPOLEFORCES
Ion–induceddipoleforces
An ion-induceddipole at ractionis
a weak at ractionthatresults
whentheapproach of an ion
induces a dipole in an atom or in
a nonpolar molecule by
disturbing the arrangement of
electrons in thenonpolar species.
• Dipole–InducedDipoleForces
A dipole-induced dipole at raction
is a weak at raction that results
when a polar moleculeinducesa
dipole inan atomorina nonpolar
molecule by disturbing the
arrangement of electrons in
thenonpolar species.

12. • HYDROGENBOND
The hydrogen bond is a special dipole-dipole interaction
betweenthe hydrogenatomina polar N-H, O-H orF- H
bondand an electronegative O, N or F atom.
A – H ----B
A and B
or
are O, N
A – H ----A
and F

13. Pressure: Gases andTemperature
 Particles speed up (more
energy)
 = Volume increases!
• Decreased temperature
• (remove heat)
 Particles slow down (less
energy)
 = Volume decreases!
Increased temperature
(add heat)