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Inorganic and Organic Chemistry Summary
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Detailed reviewer about Inorganic and Organic Chemistry. Includes various illustrations, formulas, and graphs making it easier to understand.
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INTRODUCTION TO General, Organic, and Biochemistry
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Inorganic and Organic Chemistry 1CHAPTER 1. ATOMIC STRUCTURE 𝑨𝒕𝒐𝒎𝒊𝒄 𝒘𝒆𝒊𝒈𝒉𝒕 = (% 𝒐𝒇 𝑰𝒔𝒐𝒕𝒐𝒑𝒆𝟏 × 𝒂𝒎𝒖𝟏)
+ (% 𝒐𝒇 𝑰𝒔𝒐𝒕𝒐𝒑𝒆𝟐 × 𝒂𝒎𝒖𝟐)
STRUCTURE OF ATOM = (0.9889 × 12) + (0.0111 × 13.0034)
= 11.8668 + 0.14433774
Atom: the basic unit of an element that can enter into chemical = 𝟏𝟐. 𝟎𝟏𝟏𝟏𝟑𝟕𝟕𝟒 𝒐𝒓 𝟏𝟐. 𝟎𝟏
combination.
Subatomic particles- a clusters of components inside the atom. Radioisotopes- heavier isotopes of an element that has unstable
*includes- electron, proton, and neutron. nucleus that tend to rearrange itself and releases energy to become
Electrons (e+) - negatively charged particles, it has a small mass more stable. This rearrangement is called radioactive decay. This
usually designated as 0 amu.
happens because in heavier isotopes the glue that holds the atomic
Protons (p+) – positively charged particles in the nucleus
nuclei is weaker and aims to have a stable state this process is called
Neutron (n0) - a dense central core within the atom
radioactivity.
*Protons and Neutrons are heavy particles and have
approximately same mass- 1 amu.
Ions- gained or lost electrons of an atom. 3 types of radiation (alpha (α), beta (β), gamma (γ), and neutron
(n))
Note: the electrical charge of a particle is a measure of its ability to
attract or repel other charged particles.
PLANETARY AND ORBITAL MODEL
Planetary model- portrays the atomic structure as a miniature solar
system in which the protons and neutrons are clustered at the
center of the atom in the atomic nucleus.
Orbital Model- depicts the general location of electron outside the
nucleus as a haze of negative charge referred to as the electron
cloud.
ATOMIC NUMBER, MASS NUMBER, AND ISOTOPES
Atomic Number- The number of protons in the nucleus of each
atom of an element. It also indirectly tells the electron that an atom
contains. Penetration of radiation
Atomic Mass Number- the total masses of all the constituents of an
atom (proton, and neutron).
𝑴𝒂𝒔𝒔 𝑵𝒖𝒎𝒃𝒆𝒓 = 𝑷𝒓𝒐𝒕𝒐𝒏𝒔 + 𝑵𝒆𝒖𝒕𝒓𝒐𝒏𝒔
= 𝑨𝒕𝒐𝒎𝒊𝒄 𝒏𝒖𝒎𝒃𝒆𝒓 + 𝒏𝒖𝒎𝒃𝒆𝒓 𝒐𝒇 𝒏𝒆𝒖𝒕𝒓𝒐𝒏𝒔
Isotopes- the structural variation of each elements, has the same
number of protons and electrons but vary in number of neutrons
they contain.
ELEMENTS, COMPOUNDS, MOLECULES, and MIXTURES
Element- a pure substance that cannot be broken down into simpler
substance by physical nor chemical methods. Consist of one type of
atom.
Molecules- when a two or more atom of the same element are
combined chemically.
Atomic Weight- most elements occur in nature as mixtures of 𝐻 (𝑎𝑡𝑜𝑚) + 𝐻 (𝑎𝑡𝑜𝑚) → 𝐻2 (𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒)
isotopes. We can calculate the average atomic mass of a specific
element called as the atomic weight of an element, through utilizing Compound- is a pure substance of two or more elements chemically
the masses of its isotopes and their relative abundances. combined.
Ex. Atomic weight of Carbon 4𝐻 + 𝐶 = 𝐶𝐻4 (𝑚𝑒𝑡𝑎𝑛𝑒)
Abundance of the Isotope Atomic Mass Unit 𝑁𝑎 + 𝐶𝑙 = 𝑁𝑎𝐶𝑙 (𝑠𝑜𝑑𝑖𝑢𝑚 𝑐𝑙𝑜𝑟𝑖𝑑𝑒)
12C= 98.89% 12.0000 amu Mixture- two or more substance that are not chemically combined
13C= 1.110% 13.0034 amu or bonded.
Heterogeneous Mixture- does not blend throughout; both
substances remains distinct.
“When life brings big winds of change that almost blow you over, close your eyes, hold on tight, and believe.”
Lisa Lieberman-Wang
, Inorganic and Organic Chemistry 2
*Suspensions- mixture that if left undisturbed the
containing particles settle out.
Homogeneous Mixture- substances are fully blended; individual
substances are not distinct.
*Solutions- contains atoms, ions, or molecules that are
fully dissolved.
*Colloids- a mixture containing mid-size particles that do
not settle out.
Tyndall Effect- dispersed colloid particles scatter light, allowing us to
differentiate between colloids & solutions.
Tyndall Effect
Chemical change- substance transformed into chemically different
substance.
PROPERTIES OF MATTER
Physical properties- can be observed without changing the identity
and composition of the substance.
*includes color, odor, density, melting point, boiling
point, and hardness.
Chemical properties- describe the way a substance may change, or
react, to form other substances.
*common chemical property, flammability, toxicity, UNITS OF MEASUREMENT
acidity, reactivity (many types), and heat of combustion. Metric system are the units used in scientific measurements.
Intensive properties- properties of substance that do not depend on SI Units- In 1960 an international agreement was reached specifying
the amount of sample being examined and are particularly useful in a particular choice of metric units for use in scientific
chemistry because many intensive properties can be used to identify measurements. (Système International d’Unités).
substances.
*boiling point, freezing point, flammable, density,
combustible, melting point, condensation point,
hardness, color, and corrosive.
Extensive properties- properties of substance that depend on the
amount of matter present.
*volume, mass, length, and weight.
PHYSICAL and CHEMICAL CHANGES
Physical change- substances changes their physical features or
appearances but not its chemical composition.
* all changes of state are example of physical changes.
“When life brings big winds of change that almost blow you over, close your eyes, hold on tight, and believe.”
Lisa Lieberman-Wang
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