Chapter 2: The Nature of Matter
C6H12O6 + 6O2à CO2 + H2O
What elements are represented?
What compounds are represented?
How many atoms of each element are represented?
Is it balanced?
Which scientific law do balanced chemical equations enforce?
Atoms – The basic unit of matter.
Composed of:
______– positively charged particles in the nucleus of the atom
Neutrons – particles with mass that have _____ charge; found in the nucleus of the atom
Electrons – ______charged particles moving around the nucleus in orbits.
Atoms with equal numbers of protons and electrons are “______”
Atoms with ______numbers of electrons and protons = “ions”
Atoms with more protons than electrons = cation (______charge)
Atoms with more electrons than protons = ______(negative charge)
Elements – What is an Element?
One or more ______
Can_____ be broken down or split
Represented by a one or two letter symbol; ex. Na (sodium) and C (carbon)
Atomic number = number of ______of an element.
Atomic ______= number of protons plus number of neutrons. Ex: Carbon has 6 protons and 6 neutrons; atomic weight is 12
Let’s Practice: Look at Carbon – C
What is its atomic mass?
Can we tell how many electrons it has?
How? (hint – look at its atomic number)
Isotope – Atoms of the same element that have different numbers of______.
Ex: Carbon can have 6, 7, or 8 neutrons
Radioactive isotope – isotopes with ______nuclei. Give off radiation
electrons= those electrons that orbit the ______energy level of an atom.
1st energy à ______electrons; 2nd energy level à _____ electrons
When filled, it makes the element more stable
Unfilled energy levels make the element more ______with other elements.
Compound – substance formed by the chemical combination of 2 or more elements. Ex: H2O, NaCl, & HCl.
Compound usually has ______properties than the elements it is composed of
Ex: H2O is a liquid composed of gaseous hydrogen and gaseous oxygen.
Chemical bonds – forces that ______elements of a compound together.
Forces are created by the interaction of each of the element’s ______electrons
*______Bond – formed when one or more electrons are transferred from one atom to another. Ex: Sodium (Na) donates one electron to Chlorine (Cl) to form an ionic bond and make sodium chloride (NaCl – table salt)
*Covalent Bond – formed when one or more electrons are ______between elements. This
type of bond between elements creates a molecule. Ex: H2O
Properties of Water
A common molecule with unique characteristics:
*______– due to the way the hydrogen atoms are arranged around the oxygen atom,
water molecules have a (+) end and a (-) end = polar. What does it look like?
This electrical orientation causes water to be attracted to other charged elements and form hydration spheres around them. This keeps the elements from combining with other charged elements.
Ex: salt placed in water dissolves. In other words, the sodium separates from chlorine & water molecules keep them apart. Water helps keep things dissolved = universal ______
*Has a high heat capacity and heat of vaporization – water absorbs, transports, and releases a great deal of ______without changing its state (ice to water to vapor).
That’s why, on a hot day, you just perspire and not evaporate. The water in your body stays liquid (and not turn into a vapor) while it is carrying the heat to the surface of your skin.
*______- sticks to itself; ex: beading water
*______- sticks to other things
*Highly reactive – virtually no chemical reactions occur in living systems without the presence of water
*Major component of body lubricants (mucus), protective cushions (amniotic fluid and cerebrospinal fluid), and transport mediums (______)
Salts
In living systems, salts are compounds that dissolve in water and become______.
Electrolytes conduct electricity in body.
Ex: Na, Ca, K, Cl = major electrolytes
______has a concentration of these in it.
ACIDS
Compounds that give off ______ions (H+) in solution. Acids read ______7 on pH scale.
The more H+ given off, the lower the number on the pH scale.
Bases
Compounds that give off ______ions (OH-) in solution. Bases read ______7 on pH scale. The more OH- given off, the higher the pH.
Biochemistry
Chapter 2.3: The Macromolecules of Life
Organic Chemistry- Study of all compounds that have bonds between ______atoms.
Importance of Carbon:
Carbon has 4 ______electrons
Tends to form ______bonds with other carbon atoms
…chains……rings……branches……or combinations of chains, rings, and branches.
Carbon is able to form large and complex molecules called “______”
Macromolecules made by “______”- where small compounds (“______”) are put
together to make larger compounds (“______”).
4 types of organic macro-molecules (organic polymers):
*Carbohydrates *Lipids *Proteins *Nucleic Acids
Carbohydrates “______”
Made of C, H, O in a 1:2:1 ratio;
Ex: C6H12O6
Monomer = ______
Examples: Glucose-______energy
Starch-plant storage
Glycogen- animal storage
______-structure in plants
Chitin-exoskeleton crayfish
Used as the main source of fuel and/or for structural purposes
Lipids: “______”
Made mostly of C and H
Monomer: glycerol attached to fatty acids
Used to store______, make cell membranes, waterproof coverings, chemical messengers
Examples: saturated fats, unsaturated fats, polyunsaturated fats, oils, waxes, ______, steroids
Nucleic Acids
Made of C, H, O, N, and P
Monomers: ______
Used to store and transmit ______information
Examples include ______and RNA
Found in anything that contains cells
Proteins
Contains C, H, O, N, S, and P
Monomers: ______
Used to regulate chemical reactions and cell processes, form body structures, transport materials, or
fight disease
Examples include enzymes, antibodies, muscle tissue
Contained in______, legumes, dairy products
Enzymes = special types of ______
Enzymes are proteins capable of increasing ______of a reaction without being consumed in the
process
Some reactions enzymes are involved in include: ______, Synthesis of molecules, and
______& release of energy
Enzymes have the ability to carry out reactions at ______temperatures that would normally
require extremely high temperatures
Activation Energy – energy required to ______enzymes to substrates and cause a change
Substrate – molecule undergoing a change; also called the ______.
Activation site – place ____ the ______where a specific substrate attaches
Reactant –______side of chemical equation; what is added together to form products
Product – end ______of the enzyme-substrate reaction; right side of a chemical equation
Optimum – best conditions for reaction to occur. In your body: pH of 7 and temperature of 37oC
Denature – permanently change shape of enzyme due to pH or temperature extremes; can prevent the enzyme from functioning properly.
Coenzyme – needs to be present in some enzymes to aid in the reaction. If it is missing the enzyme may not work; vitamins act as coenzymes.
Inhibitors – things that prevent enzymes from working properly
Competitive inhibitors – compete with substrate for binding sites on enzyme; slows down reaction; ex: ethanol and isopropanol
Noncompetitive inhibitors – irreversible binding to enzymes; stop reaction permanently
Ex: some heavy metals.