Post on 16-Oct-2020
• describe how the polarity of water molecules results in the hydrogen bonding.
• describe how the chemical properties of water are advantageous for life. Provide specific examples for water as a temperature regulator, solvent and lubricant.
• describe both acids, bases and indicate the importance of pH to biological systems.
• show / model how buffers work to regulate pH.
The rattlebox moth
Produces chemicals important for mating and defense
Defensive chemicals from plants that they eat
The compound produced during mating
Allows the moths to communicate using chemicals
Sperm, nutrients and alkaloid
Protection and life insurance!
Chemicals play many more roles in life than signaling
Making up our bodies, those of other organisms, and the physical environment
Are essential to life
Mostly made up of carbon, hydrogen, oxygen and nitrogen ; make up the bulk of living matter (96.3%)
Are essential to life, but occur in minute amounts
Dietary deficiencies in trace elements
Can cause various physiological conditions
Trace elements are essential to human health
And may be added to food or water
A quick review!
Chemical elements
Combine in fixed ratios to form compounds
Most of the compounds in living organisms contain at least three to four different elements, mainly C, H, O, N
Eg. Vit A – made up of C, H, O
Eg. Proteins – C, H, O, N, S
The smallest particle of matter that still retains the properties of an element is an atom
Subatomic Particles
An atom is made up of protons and neutrons
Located in a central nucleus
The nucleus is surrounded by electrons
Arranged in electron shells
Differences in Elements
Atoms of each element
Are distinguished by a specific number of protons
Isotopes
The number of neutrons in an atom may vary
Variant forms of an element are called isotopes
Some isotopes are radioactive
Living cells cannot distinguish between isotopes of the same element therefore they are taken up as per usual
Because radioactivity is easily detected, radioactive isotopes are useful as tracers
For monitoring the fate of atoms in living organisms (biological spies)
Biologists often use radioactive tracers
To follow molecules as they undergo chemical changes in an organism
Plant researchers have used them to study photosynthesis
Traced the isotope of C – 14C and found it ended up in a glucose molecule
Radioactive tracers are often used for diagnosis
In combination with sophisticated imaging instruments
PET – positron-emission topography detects intense chemical activity in the body
Patient is injected with an isotope that emits subatomic particles called positrons
Positrons collide with electrons and give off ‘hot spots’
Radioactive isotopes have many beneficial uses
But uncontrolled exposure to them can harm living organisms because any energy or radiation emitted can damage cells or more importantly DNA
Electrons in an atom
Are arranged in shells, which may contain different numbers of electrons
Atoms whose shells are not full
Tend to interact with other atoms and gain, lose, or share electrons
These interactions
Form chemical bonds
When atoms gain or lose electrons
Charged atoms called ions are created
An electrical attraction between ions with opposite charges
Results in an ionic bond
Sodium and chloride ions
Bond to form sodium chloride, common table salt
In covalent bonds
Two atoms share one or more pairs of outer shell electrons, forming molecules
Molecules can be represented in many ways
Double bonds in oxygen
A molecule is nonpolar
When its covalently bonded atoms share electrons equally because they have the same electronegativity
In a polar covalent bond
Electrons are shared unequally between atoms, creating a polar molecule
Gives water its universal solvent status!
This attraction forms weak bonds
Called hydrogen bonds
Because oxygen is pulling electronegativity from hydrogen, this cause the H to be slightly positive attracting another oxygen
Bozeman – Water and Life
Due to hydrogen bonding
Water molecules can move from a plant’s roots to its leaves
Insects can walk on water due to surface tension
Created by cohesive water molecules
Water’s ability to store heat
Moderates body temperature and climate
Heat is the amount of energy associated with the movement of atoms and molecules
It takes a lot of energy to disrupt hydrogen bonds
So water is able to absorb a great deal of heat energy without a large increase in temperature
Milder conditions near oceans because as oceans cool, they give off heat
66% of your body weight is water, this helps moderate your internal temperature
As water cools
A slight drop in temperature releases a large amount of heat
A water molecule takes energy with it when it evaporates
Leading to evaporative cooling
Humidity and sweat!
Hydrogen bonds hold molecules in ice
Farther apart than in liquid water
Ice is therefore less dense than liquid water
Which causes it to float
Floating ice
Protects lakes and oceans from freezing solid
Polar or charged solutes
Dissolve when water molecules surround them, forming aqueous solutions
Bozeman – Water: A polar Molecule
A compound that releases H+ ions in solution is an acid And one that accepts H+
ions in solution is a base
Acidity is measured on the pH scale From 0 (most acidic) to 14
(most basic)
The pH of most cells Is kept close to 7 (neutral)
by buffers
Buffers are substances that resist pH change
Bozeman – pH and Buffers (Complex Chemistry)
Crash Course – pH and pOH (complex chemistry)
Crash Course - Buffers
Some ecosystems are threatened by acid precipitation
Acid precipitation is formed when air pollutants from burning fossil fuels
Combine with water vapor in the air to form sulfuric and nitric acids
These acids
Can kill trees and damage buildings
In a chemical reaction
Reactants interact, atoms rearrange, and products result
2 H2O2 2 H2O
Living cells carry out thousands of chemical reactions
That rearrange matter in significant ways