Matter and its different phases.

1. VIADOR, MIKAELLA M. 1-B SEPT. 15, 2022
PHARMACEUTICAL INORGANIC CHEMISTRY (LEC)
ACTIVITY #1
1. Define MATTER.
o Matter is a substance composed of various particle types that occupies physical space
and has inertia. According to modern physics principles, each type of particle has a
distinct mass and size.
2. Enumerate the following and describe each.
a. States of matter
o Solid - all solids have a distinct shape, mass, and volume that prevents them from
conforming to the shape and volume of the container in which they are stored. This is one
of the characteristics that distinguishes solid matter from liquid matter. Particles in solid
materials are dense because they are tightly packed, and this limits their mobility.
o Liquid - unlike solids, liquid particles are more loosely packed. This allows them to flow
around each other, giving the liquid an arbitrary shape. Because liquids lack a specific
shape, they can conform to the shape of containers. Liquids have a lower density than
solids. Compressing solids and liquids is difficult.
o Gases - gases, unlike solids and liquids, can be compressed by shrinking the container,
which reduces the space between particles. This is responsible for the large vibrations of
atoms in gases and the high kinetic energy of particles. Gases can also be confined; in
which case they conform to the volume and shape of the container.
b. Properties of matter
 Physical properties, such as mass, color, and volume, are characteristics that
scientists can measure without changing the composition of the sample under study
(the amount of space occupied by a sample).
o Extensive - mass, weight, and volume are examples of extensive qualities that
change depending on the amount of the substance.
o Intensive - contrarily, intensive qualities, such as color, melting point, boiling
point, electrical conductivity, and physical state at a specific temperature, are
independent of the amount of the substance present.
 Chemical properties describe a substance's characteristic ability to react to form new
substances; they include flammability and corrosion susceptibility. A pure substance's
chemical and physical properties are the same in all samples.
c. Changes of matter
o Melting - when heat is applied to a solid, it melts. A solid transform into a liquid when
certain temperature and pressure conditions are met. At sea level, the melting point of ice
(solid water) is higher than zero degrees Celsius (32 degrees Fahrenheit). The melting
point of solid oxygen is -218.4 degrees Celsius.
o Freezing - when heat is removed from a liquid, its particles slow down and settle in one
location, resulting in freezing. When a liquid reaches a certain temperature, known as its
freezing point, it solidifies. For example, most fresh water freezes at zero degrees Celsius
(32 degrees Fahrenheit). Because of its salt content, sea water has a lower freezing point.
o Sublimation - is the process of converting a solid directly into a gas without passing
through the liquid phase. It can be achieved by raising the temperature of the substance
above its boiling point or by freeze-drying it under vacuum conditions. Carbon dioxide is
a common example of a solid that sublimates to a gas.
o Vaporization - the process of converting a liquid to a gas through evaporation or boiling
is known as vaporization. Because the liquid particles are constantly colliding, energy is
transferred to particles near the surface. When enough energy is transferred, some
particles in the substance are removed as free gas particles. The temperature and
pressure conditions under which a liquid turns into a gas are referred to as its boiling
point.
o Condensation - occurs when a gas is converted into a liquid. When water vapor, a gas,
reaches its dew point, it condenses into liquid water known as dew.

2. o Deposition - is a process that converts a gas directly into a solid without passing through
the liquid phase. Deposition is, in this sense, the inverse reaction to sublimation. When
the air touching the solid is cooler than the rest of the air, deposition occurs. This is what
happens when water vapor is directly converted into ice as frost.
d. Composition of matter
e. Phases of matter
 Matter exists in four natural states: solids, liquids, gases, and plasma. Man-made Bose-
Einstein condensates are the fifth state.
o Plasma - plasmas are gases that have been ionized at high temperatures. Helium,
neon, argon, krypton, xenon, and radon are examples of noble gases that can be
ionized into the plasma state. In the real world, stars are a good example of plasmas.
o Bose-Einstein Condensate - it was first predicted in the 1920s by Satyendra Bose
and Albert Einstein, but it wasn't created until 1995. BEC was created artificially by
combining lasers and magnets at extremely low temperatures just a few degrees
above absolute zero (zero Kelvin). At these temperatures, molecular motion nearly
ceases, resulting in almost no kinetic energy transfer from one atom to another. As a
result, the atoms begin to clump together, and thousands of individual atoms combine
to form one super atom and Cornell and Weiman did it with rubidium.
3. What is an atom? What are its subatomic particles? Define each.
 The atom is the smallest unit of matter that can be divided without releasing electrically
charged particles. Matter is fundamentally made up of elementary particles known as
quarks and leptons. Quarks are groups of subatomic particles that interact with a strong
force to form protons and neutrons. Leptons are type of elementary particle that also
includes electrons.
o Protons – are positively charged particles; the atomic number, also known as the
proton number, is the number of protons in an atom. An element's atomic number is
determined by its atomic number (e.g., the element of atomic number 6 is carbon).
o Electrons – are negatively charged particles; electrons are found in an electron cloud,
which is the area surrounding an atom's nucleus. Electrons have a negative charge
that is proportional to the positive charge of protons. Their mass is significantly less
than that of a proton or neutron (and as such is usually considered insignificant).
o Neutrons – neutrally charged particles; neutrons and protons coexist in the nucleus.
They, along with protons, account for nearly all of the atom's mass. The neutron
number is the number of neutrons found by subtracting the proton number from the
atomic mass number. The neutrons in an element determine an atom's isotope and,
in many cases, its stability. The number of neutrons does not always equal the number
of protons.

3. 4. Draw/illustrate an ATOM labeling its subatomic particles.
References:
https://www.techtarget.com/whatis/definition/matter
https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Chemistry_-
_The_Central_Science_(Brown_et_al.)/01%3A_Introduction_-
_Matter_and_Measurement/1.03%3A_Properties_of_Matter
https://chem.libretexts.org/Courses/Anoka-
Ramsey_Community_College/Introduction_to_Chemistry/03%3A_Matter_and_Energy/3.03%3A_Co
mposition_of_Matter
https://www.britannica.com/science/atom
https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Suppl
emental_Modules_(Physical_and_Theoretical_Chemistry)/Atomic_Theory/The_Atom/Sub-
Atomic_Particles