Module 2 - Chemistry Flashcards
Matter
Matter – composed of chemical elements
Chemical Elements + total body mass
Chemical elements – O2, C, H, N, = 96% of total body weight w/ Ca and P = 98.5%
Atoms
Units of matter of all elements
Element
Element – quantity of matter composed of atoms of same type
Radioactive isotope
Radioactive isotope – unstable and emits radiation
Free radical
Electrically charged atom or group of atoms with unpaired electron in outer shell
Become stable by giving up or taking from another atom or molecule
Nucleus
Protons ++
Neutrons
Electrons –
Ions
Ions - Either gives up or gains electrons – positive or negative charge b/c unequal # of protons and electrons
Cation charge
++
Anions charge
–
Isotopes
Different atoms with same element
Same # of protons
Diff # of neutrons
Antioxidants
Antioxidants – inactivate oxygen-derived free radicals
Molecules
Molecules – Two+ atoms share electrons
Compound
Compound – two+ different atoms – H2O
Chemical Bonds
Atoms of a molecule held together by force
Hydrogen Bonds
Hydrogen Bonds
Two atoms associate with hydrogen atom
Weakest
Cannot bind atoms into molecules
Serve as links b/w molecules to give strength and stability
Gives 3D shape to large molecules
Ionic Bonds
Ionic Bonds
Atom loses or gains a valance electron = ion
+ & - are attracted
2nd strongest
Exist as solids
Electrolyte – dissociate in solution to their + & - ions
Covalent Bonds
Covalent bonds
Strongest
Atoms of molecules share electrons
Most common
Polar or non-polar
Polar – bonding of hydrogen to oxygen or Nitrogen allow hydrogen bonds to form
Energy
Capacity to do work
Potential Energy
Potential energy
Energy stored by matter due its position
Kinetic Energy
Kinetic energy – matter in motion
Chemical Reactions
new bonds form or old bonds broken
Metabolism
Metabolism – all reactions
Reactants – starting substances
Products – ending substances
Total mass of reactants = total mass of products – law of conservation of mass
Synthesis reactions
Synthesis reactions – anabolic – bond is formed – atoms/molecules combine
A + B –> AB
Decomposition reaction
Decomposition reaction – catabolic – bond broken down
AB –> A + B
Oxidation and Reduction
Oxidation – atom will transfer electron to another atom or compound – charge is now more positive - loss of electron from molecule – decrease in potential energy
Na –> Na + e- (cant use – signs in chemisty)
Reduction – reduction of charge b/c more electrons = more negative charge - gain of electron by molecule – increase in potential energy
Cl + e- –> Cl-
Inorganic compounds vs organic compound
Inorganic compounds – lack carbon – simple molecules
Organic compounds – always have carbon and hydrogen – covalent bonds – usually have oxygen
Water
Water
Inorganic compound
Polarity
- Uneven sharing of valence electrons
- Partial negative near single oxygen
- Two partial positive new two hydrogen
Enables reactants to collide to form products
Dissolves wastes
Cohesion – high surface tension – difficult to break or stretch
Major part of mucus and lubricating fluids
Ionization/dissociation
Ionization/dissociation – separate into ions when dissolved in water
- Inorganic acids, bases, or salts
- Acids = into 1+ hydrogen (H+) and 1+ anions (- -ions)
- Bases = into 1+ hydroxide (OH-) and 1+ cations (++ ions)
- Salt = into cations and anions, neither H+ or OH-
Acids and Bases
Body needs specific quantities
Acidity vs alkalinity of solutions base on pH scale – 0-14
Neutral – 7.0
Below 7 = acid = more H+
Above 7 = alkaline = more OH-
pH urine and saliva = 6.3-6.6
pH blood = 7.4
pH 14 = Drain cleaner
pH 0 = battery acid
Buffer system
Buffer system – weak acid or base to even things out – carbonic acid-bicarbonate buffer
Carbohydrates Priorities
provide energy for life
sugars, starches, glycogen, and cellulose
some get converted to building structures and generate ATP
other are food reserves
Types of Carbs
3 groups
1) Monosaccharides – simple
2) Disaccharides – two monos formed by dehydration syn. Hydrolysis can spilt
3) Polysaccharides – complex – 100s+ monos - Glycogen – stored in liver or skeletal muscles
Lipids
Like carbs, have C, H, & O
No 2:1 ratio of H to O
Less polar covalent bonds
insoluble in polar substances – H2O
Soluble in non-polar - alcohol
Triglycerides
Triglycerides founds most
Protection
Insulation
Energy
Phospholipids
Phospholipids – membrane components
Steroids
Steroids – sex hormones estrogen and testosterone
Proteins
Proteins
Structure to body
Regulate processes
Protected
Muscle contractions
Transport substances
Denaturing of proteins – hostile environment makes protein lose its shape and function
serve as enzymes
Amino Acids
Amino acids – building blocks of proteins
C, H, O, and, N
Come together with covalent bonds to make a peptide bond
Enzymes
Proteins serve as enzymes
Catalysts for speeding up chemical reactions
Lower activation rate, saving ATP
1) Substrates approach active sites on enzyme
2) They bind and link with other substrates = enzyme-substrate complex
3) Conformational change
4) Product released and enzyme moves on
Nucleic Acids
Huge organic molecules
Basic units – nucleotides
C, H, O, N, and P
1) DNA – Deoxyribonucleic acid – genetic code and regulates cell activity
2) RNA – Ribonucleic acid – carries instructions from genes of cell to guide ribosomes assemble amino acids into proteins
ATP – Adenosine Triphosphate
ATP – Adenosine Triphosphate
Principle energy storing molecule
Energy is liberated and decomposed to ADP and P (Adenosine diphosphate and phosphorus)
Manufactured from ADP and P with energy from decomp reactions of glucose
