Ch 2 Flashcards
Describe the 3 states of matter
- solid: a definite shape and volume
- liquid: a changeable shape but definite volume
- gas: changeable shape and volume
Compare Kinetic and Potential energy and identify examples of each
- kinetic: energy in action (a ball rolling)
- potential: stored energy (a ball at rest)
Know the 4 forms of energy used by humans and give examples
- Chemical energy: adenosine triphosphate or ATP(energy in chemicals)
- electrical energy: nerve impulses
- mechanical energy: sound waves
- radiant or electromagnetic energy: light rays
What are the major consequences of energy conversions?
you will always lose some energy that will create heat during the conversion
List the 4 major elements of the body and their symbols and state their common function
- Carbon C: a component of all organic molecules, which include carbohydrate, lipids, proteins, and nucleic acids
- Hydrogen H: a component of all organic molecules, as an ion, it influence the pH of body fluids
- Oxygen O: a component of both inorganic and organic molecules. as a gas, it is needed for the production of cellular energy
- Nitrogen N: a component of proteins and nucleic acids
Identify the remaining 9 minor elements by symbol and know their significance to the body
- Calcium Ca: found as a salt in bones and teeth. its ionic form is required for muscle contraction, conduction of nerve impulses, and blood clotting
- Phosphorus P: part of calcium phosphate salts in bones and teeth. also present in nucleic acids, and as part of ATP and phospholipids
- Potassium K: its ion is the major positive ion in cells. necessary for conduction of nerve impulses and muscle contraction
- Sulfur S: component of proteins, particularly muscle proteins
- Sodium NA: as an ion, sodium is the major positive ion found in extracellular fluids. important for water balance, conduction of nerve impulses, and muscle contraction
- Chlorine CL: its ion is the most abundant negative ion in extracellular fluids
- Magnesium MG: present in bone. also an important cofactor in a number of metabolic reactions
- Iodine: needed to make functional thyroid hormones
- Iron Fe: component of hemoglobin and some enzymes
Describe the structural components of an atom. What makes it stable?
Neutrons, protons, and electrons
equal number of protons and electrons
Identify the characteristics of a suspension and be able to recognize examples.
Solute particles are very large, settle out, and may scatter light
ex: blood settles into plasma and red blood cells
Identify the characteristics of a colloid and be able to recognize examples
solute particles are larger than in a solution and scatter light; they do not settle out
ex: jello, milk, or paint
Identify the characteristics of a solution and be able to recognize examples
solute particles are very tiny, do not settle out or scatter light
ex: water
Be able to calculate molar concentrations of solutions
To find the molar concentration of a solution, simply divide the total moles of solute(its atomic weight in grams) by the total volume of the solution in liters
What is the chief difference between mixtures and compounds?
- Mixtures do NOT allow chemical bonding between components
- Compounds do allow chemical bonding between components
What is the Octet Rule? How is it used to determine the type of chemical bond any element will form?
except for the first shell of electrons, atoms will interact to have 8 electrons in their valence shell
the atom will always try to stabilize the outer shell: A 4 will seek a 4, a 7 will seek a 1, and an 8 will try to stay separate
How does the Octet Rule apply to an element with 1 or 2 valence electrons?
the atom will give up their electron to another atom that wants it fill out it’s valence shell. this will give the atom a positive charge or a Cation
How does the Octet Rule apply to an element with 6 or 7 valence electrons?
the atom will take some electrons from another atom that wants to give them up. this will give the atom a negative charge or a Anion
Use the Periodic Table of Elements to predict if an element will gain or lose electrons and what type of chemical bond will be formed. (create examples)
Describe how an ionic bond is formed
An ionic bond can be formed after two or more atoms permanently lose or gain electrons to form an ion.
describe how a covalent bond is formed
formed by sharing of two or more valence shell electrons. allows each atom to fill its valence shell at least part of the time
Know the difference between the following types of covalent bonds and recognize examples. single - double - triple - Nonpolar Covalent - Polar covalent -
- single: when a covalent bond forms to share 1 electron
- double: when a covalent bond forms to share 2 electrons
- triple: when a covalent bond forms to share 3 electrons
- nonpolar covalent: electrons are shared equally. produces electrically balance (such as CO2)
- polar covalent: unequal sharing of electrons produces polar molecules (such as H20)
Describe how a hydrogen bond is formed
attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule.
Describe the following types of chemical reactions and be able to give examples of each: Synthesis (combination) -Anabolism - Decomposition - Catabolism - Exchange (displacement) - Oxidation-reduction (redox) - Reversible -
Synthesis (combination): smaller particles are bonded together to form larger, more complex molecules(amino acids bonding to form protein)
Anabolism: synthesis of larger molecules
Decomposition: bonds are broken in larger molecules, resulting in smaller less complex molecules(glycogen breaks down to glucose molecules)
Catabolism: breakdown of larger molecules
Exchange (displacement): bonds are both broken and made (a molecule from a major bond breaks off and joins a new molecule in bond)
Oxidation-reduction (redox): a reaction in which food fuels are broken down for energy
Reversible: all chemical reactions are theoretically reversible. chemical equilibrium occurs if neither a forward or revers reaction is dominant
Understand the importance of chemical equilibrium to metabolism.
it allows for a constant state of energy flow
Know the 4 factors that influence the rate of chemical reactions. Determine the impact when a factor is changed.
- temperature(get from book) up: rate up
- concentration of reactant up: rate up
- particle size down: rate up
- catalysts: rate up without chemically changed or part of product(ex. enzymes)
Know the differences between organic and inorganic compounds. Identify examples of each.
- inorganic- does not contain both hydrogen and carbon at the same time(ex. water or salt)
- organic compounds- always contain carbon and can also have hydrogen at the same time
Know the 5 unique properties of water and the implications for the human body.
- High heat capacity: absorbs and releases heat with little temperature change
- High heat of vaporization: evaporation requires large amounts of heat
- Polar solvent properties: dissolves and dissociates iconic substances
- Reactivity: critical part of hydrolysis and dehydration synthesis reactions
- Cushioning: protects certain organs from physical trauma
Know the concept of the pH scale & identify if a solution is acidic, basic, or neutral
0-14
0-6 are acids
7 neutral compound
8-14 are bases
Know why a weak acid is a buffer
because it allows for a quick and easy neutralization of a base
Know why a weak base is a buffer
because it allows for a quick and easy neutralization of an acid
Understand how the carbonic acid-bicarbonate system maintains blood pH.
H2CO3 = HCO3- + H+
this equation is the back and forth of blood pH
Know the bonding properties of carbon in organic compounds
- is electroneutral, share electrons; never gains or loses them
- forms four covalent bonds with other elements
Name the 4 major organic molecules that are unique to living systems. Know their monomers.
- carbohydrates: carbon, hydrogen, and oxygen
- lipids: carbon, hydrogen, and a little oxygen
- proteins:
- nucleic acids:
Identify the 6 most common functional groups inorganic compounds and state their significance
-Carbonyl: makes ketones and aldehydes
-Hydroxyl: makes alchols
-Sulfhydryl
-Amino
-Carboxyl: make organic acids(latic and acetic)
-Phosphate
(find other acids significance)
Identify the chemical reaction used to build polymers.
Dehydration synthesis
Identify the chemical reaction used to break down polymers.
Polymers are broken down into monomers via hydrolysis reactions, in which a bond is broken, or lysed, by addition of a water molecule
Name the 3 classes of carbohydrates.
- Monosaccharides
- Disaccharides
- Polysaccharides
Know the general functions of carbohydrates.
major source of fuel and is a structural molecule
State the importance of the following carbohydrates to cellular metabolism. Recognize examples. Monosaccharide – Isomer – Disaccharide – Polysaccharide –
- single chain structures, the building block, monomers, of the other carbohydrates. ex. Glucose and deoxyribose
- have the same molecular formula, but their atoms are arranged differently, giving them different chemicals properties. ex. galactose and fructose
- formed when 2 monosaccharides are joined by dehydration synthesis, a water molecule will be lost in the making. ex. sucrose, lactose, and maltose
- are polymers of simple sugars linked together by dehydration synthesis. ex. starch and glycogen
Describe the general chemical structure of lipids. Name the 4 main types.
contains carbon, hydrogen, oxygen and sometimes phosphorus Triglycerides or neutral fats– Phospholipids– Steroids– Eicosanoids -
Know the chemical properties of the following lipids and how they are important to cells and tissues. Recognize examples: Triglycerides including saturated, monounsaturated and polyunsaturated fats -
Phospholipids -
Steroids -
Eicosanoids -
- major form of stored energy in the body / fat deposits protect and insulate organs / has 3 fatty acid chains / fatty acids and glycerol / ex. fats
- chief component of cell membranes / help transport lipids in blood / ha 2 fatty acid chains and 1 phosphate group with an attached nitrogen containing group
- flat molecules made of 4 interlocking hydrocarbon rings / fat soluble and contain little oxygen / ex. cholesterol
- derived from a 20-carbon fatty acids found in cell membranes / ex. prostaglandins
Describe the monomers of proteins. Include the following: Peptide bond – Amine group – Carboxyl group – Central carbon – R-group -
Carbon, oxygen, hydrogen, and nitrogen(2 also contain sulfur)
- when the acid end of one amino acid links to the amine end of the next amino acid
- NH2
- COOH
- the carbon atom that is always in the middle of an amino acid
- the molecules in the middle of an amino acid that connect the amine and acid groups together.
Know how each amino acid contributes to the physical and chemical properties of the protein.
a single change in the amino acid ladder can change the entire use of the protein strand.