Module 2 - Chemistry

Question 1

Matter

Answer 1

Matter – composed of chemical elements

Question 2

Chemical Elements + total body mass

Answer 2

Chemical elements – O2, C, H, N, = 96% of total body weight w/ Ca and P = 98.5%

Question 3

Atoms

Answer 3

Units of matter of all elements

Question 4

Element

Answer 4

Element – quantity of matter composed of atoms of same type

Question 5

Radioactive isotope

Answer 5

Radioactive isotope – unstable and emits radiation

Question 6

Free radical

Answer 6

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

Question 7

Nucleus

Answer 7

Protons ++
Neutrons
Electrons –

Question 8

Ions

Answer 8

Ions - Either gives up or gains electrons – positive or negative charge b/c unequal # of protons and electrons

Question 9

Cation charge

Answer 9

++

Question 10

Anions charge

Answer 10

–

Question 11

Isotopes

Answer 11

Different atoms with same element
Same # of protons
Diff # of neutrons

Question 12

Antioxidants

Answer 12

Antioxidants – inactivate oxygen-derived free radicals

Question 13

Molecules

Answer 13

Molecules – Two+ atoms share electrons

Question 14

Compound

Answer 14

Compound – two+ different atoms – H2O

Question 15

Chemical Bonds

Answer 15

Atoms of a molecule held together by force

Question 16

Hydrogen Bonds

Answer 16

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

Question 16

Ionic Bonds

Answer 16

Ionic Bonds
Atom loses or gains a valance electron = ion
+ & - are attracted
2nd strongest
Exist as solids
Electrolyte – dissociate in solution to their + & - ions

Question 17

Covalent Bonds

Answer 17

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

Question 18

Energy

Answer 18

Capacity to do work

Question 19

Potential Energy

Answer 19

Potential energy
Energy stored by matter due its position

Question 20

Kinetic Energy

Answer 20

Kinetic energy – matter in motion

Question 21

Chemical Reactions

Answer 21

new bonds form or old bonds broken

Question 22

Metabolism

Answer 22

Metabolism – all reactions
Reactants – starting substances
Products – ending substances
Total mass of reactants = total mass of products – law of conservation of mass

Question 23

Synthesis reactions

Answer 23

Synthesis reactions – anabolic – bond is formed – atoms/molecules combine
A + B –> AB

Question 24

Decomposition reaction

Answer 24

Decomposition reaction – catabolic – bond broken down AB --> A + B

Question 25

Oxidation and Reduction

Answer 25

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-

Question 26

Inorganic compounds vs organic compound

Answer 26

Inorganic compounds – lack carbon – simple molecules Organic compounds – always have carbon and hydrogen – covalent bonds – usually have oxygen

Question 27

Water

Answer 27

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

Question 28

Ionization/dissociation

Answer 28

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-

Question 29

Acids and Bases

Answer 29

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

Question 30

Buffer system

Answer 30

Buffer system – weak acid or base to even things out – carbonic acid-bicarbonate buffer

Question 31

Carbohydrates Priorities

Answer 31

provide energy for life sugars, starches, glycogen, and cellulose some get converted to building structures and generate ATP other are food reserves

Question 32

Types of Carbs

Answer 32

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

Question 33

Lipids

Answer 33

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

Question 34

Triglycerides

Answer 34

Triglycerides founds most Protection Insulation Energy

Question 35

Phospholipids

Answer 35

Phospholipids – membrane components

Question 36

Steroids

Answer 36

Steroids – sex hormones estrogen and testosterone

Question 37

Proteins

Answer 37

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

Question 38

Amino Acids

Answer 38

Amino acids – building blocks of proteins C, H, O, and, N Come together with covalent bonds to make a peptide bond

Question 39

Enzymes

Answer 39

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

Question 40

Nucleic Acids

Answer 40

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

Question 41

ATP – Adenosine Triphosphate

Answer 41

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