CEE 3- GENERAL CHEMISTRY (MODULE 1)

Chemistry

branch of science that deals with the study of matter

Physical science

studies the non-living components

central science

Act as the bridge between different science

ABC of pharmacy

basis of pharmacy practice

Antoine Laurent De Lavoisier

Who is the father of modern chemistry?

matter

anything that has VOLUME and MASS

volume

amount of space occupied by matter

cubic meter

What is the SI unit for volume

mass

amount of matter making up the material

kilogram (kg)

What is the SI unit of mass

Weight

Define as the mass x gravitational pull

Newton (kg x m/s2)

What is the SI unit of weight

Atom

basic unit of matter

Law of DEFINITE proportion/ Law of constant composition

What law defines that, the composition of a pure compound is ALWAYS the same regardless of its source

Proust's Law

other name of law of definite proportion/law of constant composition

Law of Multiple Proportion

What law defines that atoms or two or more elements may combine in DIFFERENT ratios to produce more than 1 compound

Dalton's Law

Other name for Law of Multiple proportion

Law of reciprocal proportion

What law defines that if two elements A and B separately combine with the same fixed mass of a third element C, the the masses of A and B that combine with each other are in the same ratio

Richter's Law

Other name for Law of Reciprocal Proportion

Law of Mass Conservation

What law was created by Antoine Laurent De Lavoisier

Law of Mass Conservation

What law defines that, there is no change observed in the total mass of the substances involved in a chemical reaction.

Element

A pure substance that only contains 1 kind of atom; cannot be chemically decomposed

Compounds

A pure substance that has 2 or more DIFFERENT elements; can be chemically decompose

Homogenous Mixture

A type of mixture that has a uniform parts; has 1 phase

Heterogenous Mixture

A type of mixture that has a physical distinct part; has multiple phases

Molecules

It is composed of 2 or more elements with neither the same nor different elements.

True solution

It has a particle size of LT 1 nm; has a uniform mixture; atom, molecules, ion of the substance become dispersed

Colloids

It has a particle size between 1nm-0.05 mcm; the dividing line between true solution and suspension

Colloid

Not a true solution

Tyndall's effect

light-scattering effect

Brownian's movement

Zigzag movement

Adsorption

Capacity to adhere in the surface

Charged ellectrically

Nernst/Zeta Potential

Suspensions

More than 0.05 mcm

Coarse Mixture

Type of mixture present in suspension; large particles can be seen via the naked eyes.

Gold Number (expressed by: Zsigmondy)

Protective power of colloid

Plasma

4th state of matter; the most abundant state of matter in the universe; ionized gas; greatly affected by the magnetic field

Bose Einstein Condensate

5th state of matter: DILUTED GAS cooled to a temperature close to absolute 0K (-273.15K)

Enthalpy

total heat content inside the system (represented by H)

Entropy

degree of disorderness/randomness of a system (represented by S)

Centrifugation

separates finely-suspended particles in a liquid through HIGH SPEED WHIRLING

Chromatography

via solubility-adsorption difference in solvent affinity

Decantation

difference in density/specific gravity

Distillation

via evaporation then condensation, different in boiling point

Filtration

separates an insoluble solid from a liquid using filter paper; different in particle size

Magnetic separation

differentiates paramagnetic and diamagnetic substances

Vibration

Molecular motion of solids

Gliding

Molecular motion of liquid

Random motion

Molecular motion of gases

Physical change

Changes the phase/physical form; does not form a new product

Chemical Change

Changes the chemical STRUCTURE and COMPOSITION of matter; forms new product

Soot (C)

What do you call the product that emits black color in incomplete combustion?

Endothermic Reaction

Heat is absorbed and represented by ▲H(+); cold surroundings; also known as BOND BREAKING

Exothermic Reaction

Heat is released and represented by ▲H(-); hot surroundings; also known as BOND-FORMING

Intrinsic/Intensive property

Independent on the amount of matter present; INHERENT to matter

Extrinsic/Extensive property

Dependent on the amount of matter present

Atom

composed of three subatomic particle

Proton

Determines the IDENTITY of an element

Neutron

no charge

Electron

1836x lighter than proton

Democritus

coined the term atom from greek word atomos

Atomos

means indivisible

John Dalton

created the billiard ball model

Billiard Ball Model

This model defines that the atom is a hard, indestructible sphere, hallow sphere

J.J Thompson

created the Plum pudding/ Raisin-bread model

J.J Thompson

performed the CATHODE RAY experiment

J.J Thompson

Discovered ELECTRON

ELECTRON

The first subatomic particle discovered

R.A Millikan

performed the drop-oil experiment; discovered the elementary charge (electron).

Ernest Rutherford

created the NUCLEAR Model

Ernest Rutherford

Who performed the GOLD FOIL experiment and discovered Protons

James Chadwick

discovered neutrons; bombarded the Beryllium with polonium

Neils Bohr

created the PLANETARY MODEL; redefined Rutherford's idea by adding that the electrons were in ORBITS

Erwin Schrodinger

created the quantum mechanical/ electron clouds; improved Boh's idea

Eugene Goldstein

Anode Ray (Canal Ray)

Nuclides

atom with a specific number of protons and neutrons in the nucleus

Atomic Number

represents the number of proton

Atomic mass/ mass Number

# of proton + # of neutron

# of neutrons

mass # - atomic number

Electron orbital/ electron cloud

region or space where the probability of finding an electron is GREATEST

Node

locus of points in an atom in which the electron density is ZERO

Electron Shell

One or more orbitals of VARYING SHAPE

Valence electron

electron occupying the outermost shell

Electron Configuration

arrangement of the elctron in an atom

Isotopes

same number of protons; same element

Protium

most abundant hydrogen

deuterium

Heavy hydrogen

Tritium

Only radioisotope of Hydrogen

Isobar

same mass number; different elements

Isotone

same number of neutrons; different elements

Isoelectronic

same number of electrons; different elements

Heisenberg's uncertainty

An electronic principle that defines, it is impossible to determine the momentum and position of an electron simultaneously.

Pauli's exclusion

An electronic principle that defines there is NO 2 electrons that can have the exact set of quantum numbers

Afbau's building up

An electronic principle that defines electrons are first placed on the subshell with a lower energy level

Hund's rule (maximum multiplicity rule)

An electronic principle that defines electrons are fill-up orbitals singly first

Paramagnetic

With unpaired electron; attracted to manet

Diamagnetic

with paired elctron; not attracted to magnet

Principal Quantum number (n)

main energy level of the electron shell/orbital; determins the size of the orbital

1-7

what is the range value of the principal quantum number

Azimuthal quantum number/angular quantum number

represent the subshell/sublevel; it also determins the angular momentum and SHAPE of the orbitals