Term
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Definition
| Something that has mass and takes up space |
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Term
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Definition
| A substance that cannot be broken down by a chemical reaction |
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Term
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Definition
| Made of 2+ elements in a fixed ratio |
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Term
| How many elements and what percentage is essential? |
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Definition
| 92 elements, 25% essential |
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Term
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Definition
| Carbon, Hydrogen, Oxygen, Nitrogen, Phosporous, Sulfur - these elements are the building blocks of life. |
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Term
| What is an atom, and what is its composition? |
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Definition
| The smallest unit of matter, made up of neutrons and protons in the atomic nuclues, and electrons orbiting the nucleus. |
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Term
| What do all the numbers on the periodic table represent? |
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Definition
| Atoms of one element have the same number of protons, which is the atomic number. The mass number above it is the number of protons + the number of neutrons. |
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Term
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Definition
| Atoms of an element that have different number of neutrons, and different mass. |
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Term
| What are the positions around the nucleus of the atom called? |
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Definition
| Electron shells or energy levels. |
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Term
| What happens when an electron is closer to the nucleus? Further away? |
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Definition
| When it moves away, it absorbs energy, when it moves closer, it gives off energy. The further from the nucleus you get, the more energy levels increase. |
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Term
| What is bonding? List all types of bonds, as well as their relative strength. |
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Definition
| Bonding is when atoms share or transfer electrons. Covalent bonding is when atoms share electrons. When atoms bond, they form a molecule. This is a strong bond. An example of a weak bond is a hydrogen bond. Ionic bonds are also strong, and occur when one atom donates electrons to another. |
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Term
| What is polarity? Explain how it relates to bonding. |
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Definition
| In a covalent bond, when electrons move closer to one atom, the molecule becomes polar. Likewise, in hydrogen bonds, which occur between water usually, the hydrogens are slightly positive, and the oxygen is slightly negative. This slight polarity causes these two parts to be attracted to opposite parts in a different molecule. This creates a hydrogen bond. |
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Term
| When the polar water molecule sticks to another water molecule, what is this called? How about when it sticks to a non water molecule? |
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Definition
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Term
| Surface tension - what is it? |
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Definition
| A measure of how difficult it is to stretch or break the surface of the water. |
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Term
| Kinetic Energy causes motion. What is it called when it causes the motion of atom/molecules? |
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Definition
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Term
| What is temperature and heat? What is specific heat? |
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Definition
| Temperature is the average kinetic energy of molecules in matter. Heat is the transfer of energy from one object to another (in Kilocalories usually just called calories). Specific heat is the amount of heat absorbed or lost for 1g of a substance to change temperature by 1 degree Celsius. |
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Term
| How does this relate to water? |
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Definition
| Water has a high specific heat, and a high heat of vaporization, due to the structure of hydrogen bonds. However, water also keeps the earth's climate stable due to evaporative cooling. |
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Term
| What does water break down into? How does this relate to PH? |
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Definition
| Hydroxide ions (OH-) and Hydronium ions (H3O+, usually expressed as H+). PH measures the concentration of these two ions. |
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Term
| Which ion causes acidity, and which ion causes basicness? Which way does the PH scale go? |
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Definition
| H+ causes acidity, and OH- causes alkalinity. From most acdidic (0) to most basic (14). |
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Term
| Why is PH important to water? |
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Definition
| Rain usually has PH around 5.6. Because of atmospheric waste, acid rain can result with PH less than 5.6. This damages the environment. |
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Term
| What is the element all organic molecules contain? |
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Definition
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Term
| Carbon has ... electrons, and therefore is likely to form what bond? |
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Definition
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Term
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Definition
| Hydrogen and Carbon exclusively. They form the skeleton of many organic molecules. |
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Term
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Definition
| compounds with the same molecular formula but different structures and properties. |
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Term
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Definition
| Structural, molecular formula but different structure. Cis-trans isomers have same covalent bonds but differen in how electrons are placed (double bond). Enantiomers are mirror images of each other. |
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Term
| Functional groups are what? List the most common ones in AP Bio. |
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Definition
| Molecules used most often in chemical reactions. Hydroxyl, Methyl, Carbonyl, Amine, Phosphate, Sulfhydryl. |
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Term
| What is a macromolecule? What are the major macromolecules and the exception? |
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Definition
| Macromolecules are larger molecules made from smaller molecules. Carbohydrates, Proteins, and Nucleic acids are macromolecules, but Lipids aren't. |
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Term
| What makes a macromolecule? What structures are its building blocks and how are they formed? |
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Definition
| Monomers make up a macromolecules, linked together through dehydration reactions, in which a water molecule is produced alongside the finished macromolecule. Monomers bond covalently. |
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Term
| What reaction breaks the bonds of macromolecules (polymers)? |
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Definition
| A dehydration reaction, which adds water and breaks bonds. |
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Term
| What are carbohydrates? Name their structures, as well as the function of each of them. |
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Definition
| Carbohydrates are sugars (monomers) and polymers. Monosaccharides are simple sugars, needed for cellular work. Dissacharides are double sugars linked through a glycosidic bond, used for quick energy. Polysaccharides are used for energy storage. |
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Term
| 4 Common examples of polysaccharides are: |
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Definition
| Starch, energy storage in plants; Glycogen, animal energy storage in liver and muscles; cellulose, used in plant cell walls for support; and chitin, which makes up the exoskeleton of arthropods and functions as cellulose in fungi. |
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Term
| Lipids are not macromolecules, but they have another special property. What is it? |
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Definition
| They are hydrophobic, repelling water, because of their nonpolarity. |
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Term
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Definition
| Glycerol (3 carbon, with hydroxyl group, as well as hydrocarbons). Fatty acids attach to this (fatty acids are a carboxyl group with a hydrocarbon skeleton). |
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Term
| Saturated fats are formed. They are... |
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Definition
| Solid at room temperature, and BAD. |
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Term
| Unsaturated fats are formed with an additional ... bond. How does this bond occur? Also describe their properties. |
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Definition
| Carbon Carbon double bond. This bond occurs by the removal of hydrogen atoms. They are liquid at room temperature, and much better for you than saturated fats. |
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Term
| What are cis and trans fats? |
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Definition
| Types of unsaturated fats; Cis fats have the hydrogen of the hydrocarbon after the carbon carbon bond on the same side as before, and they are more healthy. Trans are opposite, and are less healthy. |
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Term
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Definition
| Energy storage (twice as efficient as polysaccharides). Also cushion vital organs. |
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Term
| But there is another type of fat (and there will be more). Name it and describe its structure, as well as its function (think cell membrane). |
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Definition
| Phospholipids are 2 fatty acids attached to glycerol, which is then attached to a phosphate group. The phosphate forms a hydrophilic head, and the fatty acids a hydrophobic tail. These fats form the membrane of your cells. |
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Term
| The last type of fats are... Name them, their structure, as well as the most versatile type. |
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Definition
| Steroids! Consist of 4 fused carbon rings. A famous steroid is cholesterol, a component in animal cell membranes and forms hormones (estrogen, testosterone). |
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Term
| What are the functions of proteins? Where are they made? What are they made of? |
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Definition
| Functions include: support in the cell, storage, cell transport, defenses, and various enzymes. Made in ribosomes. Made of amino acids linked together, so they are polymers (polypeptides). |
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Term
| What are amino acids made of? How many are there? What determines amino acid uniqueness? |
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Definition
| Amino Acids are made of a hydrogen atom, carboxyl group, amino group, and a variable R group (that makes them unique). There are 20 amino acids. |
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Term
| How are amino acids joined? |
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Definition
| They are joined by peptide bonds when dehydration removes a hydroxyl group from the carboxyl end of 1 amino acid and hydrogen from the amino group of another. |
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Term
| When there is high or low PH, high temperature, and salinity, what happens to proteins? Is this permanent? |
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Definition
| They denature (fall apart), which can be permanent. |
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Term
| Amino acid polypeptides are programmed by... Which is a region of something, and a polymer of something else. |
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Definition
| A gene, which is a region of DNA, and a polymer of nucleic acids. |
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Term
| There are how many types of nucleic acids? List them, and their main differences in structure. |
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Definition
| There are two types of nucleic acids, Ribonucleic acid and Deoxyribonucleic acid. Their structures are similar, except DNA is missing one oxygen in its sugar, and RNA is only single stranded, while DNA is double stranded. |
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Term
| What are the function of these two acids? |
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Definition
| DNA carries genetic information, which RNA then transcribes and carries to a ribosome to form proteins. |
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Term
| What are monomers of nucleic acids? What are they made of? |
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Definition
| Nucleotides are the monomers. They are made of a nitrogen base, five-carbon sugar, and a phosphate group. In DNA, the sugar has one less oxygen. |
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Term
| Nitrogen bases are rings of what? What are their types? List examples. |
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Definition
| Rings of carbon and nitrogen. Purines are six membered (Adenine and Guanine). And pyrimidines are five membered (Cytosine, Thymine and Uracil [U replaces T in RNA]). |
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Term
| What are the pairings of the nitrogen bases? |
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Definition
| Adenine with Thymine, Guanine with Cytosine. |
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Term
| How do strands of DNA relate to each other? That is, which way do they run? What shape do they form? |
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Definition
| They run antiparallel from 5' to a 3' end. DNA forms a double helix. |
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