Chapter 2 Flashcards
Ionic Bond
- One atom loses an electron and another gains one
- Atom that gains an electron is called an anion (- Charge)
- Atom that loses an electron is called a cation (+ Charge)
- The charge between the ions holds bond together.
Decomposition Reaction
-Compounds are broken down into molecules/atoms
-Breaking of bonds
-Synthesis Reaction
(AB>A+B)
Hydrolysis
- Addition of water to break a bond
- Catabolic Reaction
Structure of An atom (Particles)
Proton) Positive particle found in the nucleus
Electron) Negative particle found in electron cloud orbiting the nucleus.
Neutron) Neutral particle found in the nucleus
Radiant/ Electromagnetic energy
- Travels in waves. (Visible light, x rays, etc..)
Hydrogen Bond
-Slight attraction attracting a electropositive hydrogen to an electronegative atom.
Chemical Energy
-Found in bonds of chemical substances
Biochemistry
Study of the chemical composition of living things
Molecules
Two or more atoms bonded together
Compounds
Two or more different atoms bonded together. (Different)
Inorganic compounds
Do not contain carbon
Ex) Water, salts, acids and bases
Mass number
Total Number of protons and neutrons in the nucleus
Synthesis Reaction
-Atoms/ molecules combine to form a larger compound
-Bond Forms
-Anabolic Reaction
(A+B>AB)
Energy Principals
- Energy can change forms
- Some will be lost during this process as heat.
Electrons (Properties)
- Determines whether or not a chemical reaction will take place.
- Located in electron shells outside the nucleus.
Nonpolar Covalent Bond
Atoms are shared equally and there is no net charge
Isotopes
Different Variations of atoms. The number of neutrons is different than the standard atom
Two Electron Models
Planetary Model) shows electrons following set path around the nucleus
Orbital Model) shows electrons as a negatively charged cloud surrounding the nucleus
Organic compounds
Contain carbon
Ex) Carbs, Fats, Proteins and Nucleic acids
Polar Covalent Bond
- Unequal sharing of electrons
- Atoms with 6 or 7 electrons are electronegative (strong electron attraction)
- Atoms with 1 or 2 electrons are electropositive
Matter
- Has mass and occupies space
- Either a liquid, solid or gas.
Covalent Bond
Atoms in the bond share two or more electrons.
Electrical Energy
-The movement of charged particles
Dehydration Reaction
- Removal of water to from a bond
- Anabolic reaction
Exchange/Displacement reaction
-Both a Synthesis and Decomposition reaction
AB+CD>AC+BD
Mechanical Energy
- The direct movement of matter
Chemical Bonds
-Energy interactions between electrons
Properties of Water
- High Heat Capacity) Absorbs heat without temp change
- High Heat of Vaporization) Requires a lot of energy to evaporate
3) Polar Solvent Properties) excellent solvent because it is a polar molecule - Reactivity) Excellent at breaking down/building molecules
- Cousioning) the internal organs
Atomic Weight
Average mass number of all the different isotopes for a certain element.
Mixtures
Two or more components physically mixed
-Can be solutions, colloids, or suspensions
Solutions
- Homogenous Mixture) particles are mixed evenly. Consist of a solvent and a solute
- Solvent) Substance present in the greatest amount
- Solute) dissolved in solvent
Energy (Define and different types)
-The ability to do work or put matter into motion
Kinetic energy) energy in motion
Potential energy) stored energy.
Atomic Number
Number of Protons in the Nucleus
Four elements that make up 96.1% of our bodies
Carbon, Hydrogen, Oxygen and Nitrogen.
Salts
- Held together by ionic bonds
- Formed by an anion and a Cation.
- Called an electrolyte (can conduct electricity in a solution)
Properties of Acids and Bases
- Electrolyte
- Ionize and dissolve in water
Acids
- Proton Donors (Release H+ ions into a solution)
- High H+, Low OH-, pH 0-6.99
Bases
- Proton Acceptors (Pick up H+ ions in a solution)
- Low H+, High OH-, pH 7.01-14.
pH Scale
- Measurement of H+ ions in a solution.
- Goes 1 to 14
- Logarithmic scale (ph of 5 is ten times more acidic than a pH of 6)
Neutralization
- When a Acid and Base come together they neutralize (pH of 7)
- H+ and OH- come together to form water and the cation and anion form a salt.
Buffers
- Keeps pH within normal limits
- Removes H+ from acidic solutions
- Adds H+ to basic solutions
Carbonic Acid System
- Important buffer system of the blood
- If pH drops H2CO3 will be formed
- I pH rises HCO3 will be formed and H+ ions will be released.
Properties of Carbon
-Electroneutral (shares electrons instead of donating them. Will form 4 covalent bonds)
Monomers and Polymers
- Monomers are building blocks
- Long chains of monomers are called polymers.
Carbohydrates (properties)
- contain C, H, and O ([CH2O]n)
- maks sugars and starches
- Major source of Fuel
Monosaccharides
- Three to seven Carbon atoms
- Monomers of Carbs
- Important carbs include pentose sugars (ribose and deoxyribose) and hexose sugars (glucose).`
Disaccharides
- Two linked sugars
- Too large to fit through the cell membrane
- Important ones include glucose, lactose, and maltose
Polysaccharides
- Made of lots of sugars
- Not very soluble
- Starch and Glycogen are examples
Lipids
- Contain C, H, O (oxygen is present in the least amount)
- Not soluble in water (Hydrophobic)
Neutral Fats/ Triglycerides
- Fat when solid and oil when liquid
- Made of three fatty acids bound to a glycerol (trigliceride)
- Store energy and insulate and protect the body.
Saturated Fats
- Fatty acid chain has maximum amount of H+ ions attached
- Max amount of covalent bonds.
- Solid at room temp
Unsaturated Fat
-Fatty acid chain has double bonded carbon atoms which creates kinks in the chain.
Phospholipid
- Triglyceride but one Fatty acid tail is replaced with a phosphorus head
- Has a polar hydrophilic head and a nonpolar hydrophobic
Eicosanoids
- Diverse lipids derived from a fatty acid
- Prostaglandins are important eicosanoids which plays a role in blood clotting, pressure, inflammation, and labor contractions.
Fat Soluble vitamins
vitamins A,D,E, and K
Lipoproteins
Transports fats in the blood.
Proteins
-Polymers made of amino acids.
4 levels of structure of protein
1) Primary) Straight chain of linked amino acid
2) Secondary
Alpa) Twisting Structure
Beta) Folded Structure.
3) Tertiary Structure) Mixture of Primary and Secondary Structures. Most proteins are this structure
4) Quaternary) More than one polypeptide chain.
Shapes of Protiens
Structural) long, fibrous protein that is resistant and used for structure.
Globular) Compact and spherical. has an active site for a specific function.
Protein Denaturation
- Proteins unfold and the active site is destroyed.
- Caused by decreased pH or increased temperature.
Enzymes
- Biological catalysts.
- Speed up chemical reaction by lowering the activation energy required to start a reaction
Nucleic Acids
- Deoxyribonucleic acid and ribonucleic acid
- Largest molecules in the body
- Monomers are called nucleotides
DNA
- Purines (two ring bases): Adenine (A), Guanine (G)
- Pyrimidines (one ring bases): Cytosine (C), and Thymine (T)
- Base-pair rule – each base pairs with its complementary base (A always pairs with T; G always pairs with C)
- Double helix in the cell nucleus
- Provides instructions for protein synthesis
RNA
Four bases: (Adenine (A), Guanine (G), Cytosine (C), and Uracil (U))
Pentose sugar is Ribose
