This course has been designed for students of The …Phytochemistry+pt_1+PPT.pdf · Deeper Connection with Our Surroundings. Dangers Uses ... Study of matter, it’s properties, and

This course has been designed for students of The School for Aromatic Studies (SAS).

Use or reproduction beyond the students and faculty of SAS is strictly prohibited

without written consent. This webinar and its content have been created by Grey

Mountain Herbs and Nicholas Zemp. All rights reserved.

Chinese & Western Herbalist

Aromatherapist

BS in Biochemistry from Utah

Valley University

©2016 Grey Mountain Herbs. All Rights Reserved

Better Understanding of Essential Oils

Reduced Chemical Phobia

Deeper Connection with Our

Surroundings

Dangers Uses

Powerful industrial solvent

Used in chemical and biological weapons

Fire suppressant & retardant

Used as an industrial coolant in nuclear powerplants


Inhalation of even a small amount can cause death

Prolonged exposure causes extensive tissue damage

Major component of acid rain

Oxidizes many metals, including the steel in buildings & bridges

Research conducted by Nathan Zohner (1997), 86% of respondants supported a ban on DHMO.

Ingredients: water, fructose, glucose, sucrose, fibre E460, glutamic acid, aspartic acid, leucine, arginine, alanine, valine, glycine, proline, isoleucine, serine, threonine, phenylalanine, lysine, methionine, tyrosine, histidine, cysteine, tryptophan, linoleic acid, linolenic acid, oleic acid, palmitic acid, steric acid, palmitoleic acid, ash, phytosterols, oxalic acid, E300, tocopherol, thiamine, Colorings (E63a, E163b, E163e, E163f, E160a), Flavorings (ethyl ethanoate, 3-methyl butyraldehyde, 2-methyl butyraldehyde, pentanal, methylbutyrate, octene, hexanal, decanal, 3-carene, limonene, styrene, nonane, ethyl 3-methylbutanoate, non-1-ene, hexan-2-one, hydroxylinalool, linalool, terpinyl acetate, carophyllene, alpha-terpineol, alpha-terpinene, 1,8 cineole, citral, benzaldehyde), methylparaben.










Don’t stress about it

Remember that learning is a process

Practice, Practice, Practice!

Apply it to your everyday life


Limonene

Fundamentals of All Matter

Study of matter, it’s properties, and reactions.

Happening everywhere

We do chemistry everyday


You already

ARE a

chemist!!

Chemical Properties

Reactivity

Flammability

Radioactivity

Toxicity

Heats of Combustion

Physical Properties

Boiling & melting points

Color

State of matter (solid, liquid, gas)

Hardness

Density



Name - IUPAC accepted name

Atomic # - number of protons

Symbol – 1 or 2 letters that represent an element when writing chemical formulas

Atomic mass – the amount of mass contained within a single atom of the element


Composed of subatomic particles

Neutral atoms have no charge (equal numbers of protons and electrons)

Charged atoms called ions

Can have differing numbers neutrons (isotopes)


Fundamental building block of all matter

Dalton’s Atomic Theory formed between 1803-1808

Made of minute indivisible particles

All atoms of a given element have the same properties (chemical, physical)

Combine in simple whole # ratios

Nearly another 100 years before subatomic particles discovered


“It is the nature of the self to manifest itself, in

every atom slumbers the might of the self.”

~Muhammad Iqbal

Protons

Positive charge

Determines the element

1 amu (atomic mass unit)

Discovered in 1919 by Ernest Rutherford

Neutrons

Neutral charge

Stabilizes nucleus

Can have different numbers in nucleus

Isotopes e.g. 14C carbon-14

Atomic mass determined by relative abundance of isotopes

Discovered by James Chadwick in 1932


• Discovered in 1897 by J.J. Thompson using cathode ray tubes and magnetic fields

• Have a negative charge

• Has a negligible mass (9.1094 x 10-28 grams)

• Organized into shells, subshells and orbitals

• Shells: 1, 2, 3…

• Subshells: s, p, d, f


Valence Shell: The outer most shell of an atom. Contains electrons with highest

energy.

Chemical reactions occur here

Octet Rule: Atoms will gain or lose electrons (sometimes through bonding) to achieve a stable valence shell configuration of 8 electrons.


1st shell:

1 subshell (s)

2 electrons

2nd shell:

2 subshells (s,p)

8 electrons

3rd shell:

3 subshells (s,p,d)

18 electrons

4th shell:

4 subshells (s,p,d,f)

32 electrons

5th shell:

4 subshells (s,p,d,f)

32 electrons

6th shell:

3 subshells (s,p,d)

18 electrons

7th shell:

2 subshells (s,p)

8 electrons


Na

Na=1s2 2s2 2p6 3s1

or

Na = [Ne]3s1


Cl = 1s2 2s2 2p6 3s2 3p5

or

Cl = [Ne] 3s2 3p5

Cl

Ionic Bonding

Between a nonmetal and a metal

Electrons are taken from one atom

Non polar

Covalent Bonding

Between two nonmetals

Electrons are shared between valence shells

Can be polar or non polar



Na Cl

Cl


Na

+-


Na+ + Cl- → NaCl

Sodium Chloride

Table Salt!

Ionic Bonding

Between a nonmetal and a metal

Electrons are taken from one atom

Non polar

Covalent Bonding

Between two nonmetals

Electrons are shared between valence shells

Can be polar or non polar


Electrons shared between valence shells


e-

e-

Electrons shared between valence shells


e-

e-

Hydrogen Bond

Between partially charged hydrogen and another electronegative element

Dipole-dipole interactions

Interactions between permanent dipoles in molecules

Van der Waals Forces

Weak interactions between areas of high and low electron density



Unequal sharing of electrons

Electronegativity Differential

1.7< is an ionic bond

.4 to 1.7 is a polar covalent bond

.4> is a covalent bond

Molecular Geometry is vitally important!!


δ-

δ+ δ+


Linear

BentTrigonal Planer

Carbon Oxygen Hydrogen

δ-

δ+ δ+

δ+

δ+

δ-

Represent chemical compounds in 2 dimensional space

Shows Bonding

Lines or dashes

Shows Valence Electrons

Dots

Shows Formal Charge

Shows resonance

Helps us determine molecular geometry


Single anions end in –ide

Ex. – Chloride

Binary compounds

Start with cation – remains unchanged

Add anion ending in –ide

Add appropriate prefix if there are multiple atoms

Ex. – xenon hexa fluoride XeF6


Arrhenius acids

Acid – (H+) hydrogen ion or a single proton

Base – (OH-) hydroxide ion

Brønstead-Lowery

Acid – proton donor

Base – proton accepter

Lewis acids

Acid – accepts an electron pair

Base – donates an electron pair


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Documents

This course has been designed for students of The …Phytochemistry+pt_1+PPT.pdf · Deeper Connection with Our Surroundings. Dangers Uses ... Study of matter, it’s properties, and