basic chem

Matter

fundamental building blocks of nature

Energy

capacity to do work (put matter into motion)

potential energy

energy stored in a structure, not being used but still can make matter move

gravitional/positional energy

energy stored in an object because of its height above the ground, energy due to the force gravity on object

example of gravitational potential energy

walking up a hill, need a harness if not we fall off

chemical potential energy

energy stored in between bonds of atoms, present in chemical bonds and how we get energy by food

electrical potential energy

stored energy that is built by seperation of charges , cells use this to create membranes

kinetic energy

energy of motion

electrical kinetic energy

energy of moving charges, or current measured in amps. important for electrical signaling

electrical kinetic energy example

charged particles are moving in body like ions (Na+ or K)

Mechanical kinetic energy

movement of anything that has mass, should not be charged. movement of arm is an example

electromagentic kinetic energy

light absorbed by electrons, its moving, no mass/charge. ex.energy traveling in waves (light, X-rays, UV rays)

First Law of Thermodynamics

Energy can change from one form to another, but it can never be created or destroyed"

(Total Energy In = Total Energy Out)

proton

positive and defines element

neutron

neutral charge and defines isotopes

electrons

negative charge and determines element bonding properties

electrons dictate

the charge of an atom

# protons =

atomic number (unique for each element)

# protons + # neutrons

atomic mass

isotope

same element; different # neutrons

ion

any atom with a positive or negative charge

anion

an ion with a NEGATIVE charge

cation

an ion with a POSITIVE charge

Electron Shells

electrons occupy "shells" as they orbit around the nucleus (2, 8, 8,..)

Ionic Bond

one atom donates electron(s) to another

Covalent Bond

two atoms share one/more electron

Polar Molecule -

electron sharing is unequal in the bonds, H2O

Non-polar Molecule

electron sharing is almost equal Example: Methane (CH4)

Calcium Ca

Bones, teeth, muscle and nerve action, blood clotting

Phosphorus P

Bones and Teeth, DNA, RNA, ATP. Important in energy transfer

Potassium K

Osmotic balance; cell voltage, muscle and nerve

action

Sulfur S

Component of proteins (cysteine) and other organic

molecules

Sodium Na

Osmotic balance; cell voltage, muscle and nerve

action

Chlorine Cl

Osmotic balance; cell voltage, muscle and nerve

action

Magnesium Mg

Co-factor for many enzymes

Iron Fe

Hemoglobin and many enzymes

Copper Cu

Co-factor of many enzymes

Zinc Zn

Co-factor of many enzymes

Manganese Mn

Co-factor of many enzymes

Cobalt Co

Co-factor of many enzymes and vitamin B12

Chromium Cr

Co-factor of many enzymes and potentiates Insulin

Selenium Se

Required for normal liver function

Molybdenum Mo

Co-factor of many enzymes

Flourine F

Teeth and bones

Tin Sn

Promotes growth (unknown mechanism)

Silicon Si

Growth, bone mineralization, connective tissue

synthesis

Vanadium V

Promotes growth and reproduction

Chemical Equation

# of atoms of each element same for reactants and products

Synthesis

A + B → AB (anabolic process), smaller to larger products

Decomposition

larger molecule broken down into smaller molecules

AB → A + B (catabolic process)

Displacement

one part is exchanged

AB + C → A + BC

Exergonic

energy is released during the reaction

A + B → C + D + ENERGY

glucose + oxygen ----> water + carbon dioxide +ENERGY (trapped by ATP)

Endergonic

energy required for reaction to proceed

A + B + ENERGY → C

pH=

-log10 [H+]

pH definiton

relative concentration of H+ in a solution of water

Acids

compounds which increase the concentration of H+ (pH = 1 to 6)

Bases

compounds which decrease the concentration of H+ (pH = 8 to 14)

Buffer

compound that prevents large changes in pH of a solution (pH "shock absorber")

temperature

speeds up the particles)