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Bio Unit 1 Exam
| Question | Answer |
|---|---|
| Characteristics of living things | Order, regulation, energy processing, evolutionary adaptation, growth/development, response to the environment, reproduction |
| how many species have been identified and named to date? | approx. 1.8 million |
| Taxonomy | branch of biology that names, identifies and classifies species |
| Three Domain System | Domain Bacteria and domain Archaea comprise the prokaryotes; Domain Eukarya includes all eukaryotic organisms |
| The domain Eukarya includes four multicellular kingdoms | Plantae, Fungi, Animalia, Protista |
| Unity in the diversity of life | DNA is the universal genetic language common to all organisms |
| Charles Darwin/Natural Selection | – Species showed evidence of “descent with modification” from common ancestors – Natural selection is the mechanism behind “descent with modification” |
| Darwin’s observation and Inference: | Darwin saw different types of finches in different areas, and inferred that this was because they evolved to help them survive in that specific area |
| SCIENTIFIC INQUIRY | -discovery science (Inductive Reasoning) - hypothesis-based science (Deductive reasoning) |
| Data | Qualitative –descriptions; Quantitative -measurements |
| Control Experiments | A control group provides a comparison for the experimental group; do not receive independent variable |
| Flow of energy | Sunlight Source Producers: Plants/ others capture solar energy/photosynthesis. Consumers: Herbivores/carnivores eat other organisms to get chemical energy. Decomposers: Fungi/bacteria break down dead matter and waste to use the remaining energy |
| Matter | anything that has mass and occupies space. |
| Compounds | A compound is a substance containing two or more different elements chemically combined. Ex: H₂O |
| Elements | a substance that cannot be broken down into simpler substances by ordinary chemical reactions. Ex: Carbon (C) Hydrogen (H) Oxygen (O) Nitrogen (N) |
| What elements make up 96% of living matter | C, H, N, O; 4% consists of calcium, phosphorus, potassium, and sulfur |
| Trace Elements | required in minute quantities ex: Iron, Iodine, Zinc |
| Atom | Smallest unit of an element that retains the properties of that element. (protons are positive, electrons are negative, neutrons are 0) |
| Subatomic Particles | charges |
| Atomic Number | number of protons |
| Mass number | number of protons plus the number of neutrons |
| Isotopes | two atoms of an element that differ in number of neutrons |
| Radioactive isotopes/their application | Some isotopes are unstable and spontaneously break down. Applications include: Medical diagnosis, Medical treatment, Dating fossils and geological materials, tracing substances through biological systems |
| Electron shell | Electrons occupy regions around the nucleus called electron shells or energy levels. The outermost electrons are especially important because they participate in chemical bonding. |
| Valance electron | electrons in the outermost electron shell. They determine how an atom interacts chemically with other atoms. |
| Orbital | a mathematical region of space around an atom's nucleus where an electron is most likely to be found |
| Octet Rule | N 2 8 8; describes the tendency of atoms to achieve a stable outer shell containing 8 electrons. |
| calculate # of electrons in valence shell given atomic # | use periodic table |
| Covalent bond | occurs when atoms share electrons |
| Single covalent bond | One pair of electrons is shared |
| Double covalent bond | Two pairs of electrons are shared |
| Nonpolar covalent bond | Electrons are shared approximately equally |
| Polar covalent bond | Electrons are shared unequally |
| Structural formula | Shows how atoms are connected. Example: H—O—H |
| Molecular formula | Shows the number and type of atoms. Example: H₂O |
| Electronegativity | an atom's ability to attract shared electrons toward itself. Higher electronegativity means a stronger attraction for electrons. |
| Ionic bonds | forms through attraction between oppositely charged ions. Ex: Sodium- Loses one electron, Becomes Na⁺ Chlorine: Gains one electron, Becomes Cl⁻ Then: Na⁺ + Cl⁻ → NaCl The attraction between the ions is the ionic bond. |
| Cation | positively charged ion |
| Anion | negatively charged ion |
| Hydrogen bonds | a relatively weak attraction involving a hydrogen atom that is covalently bonded to an electronegative atom and another electronegative atom |
| Reactants | Starting substances |
| Products | Substances formed by the reaction |
| Reversible reaction | Some chemical reactions can proceed in both directions. A + B ⇌ C + D The double arrow means the reaction is reversible. |
| Chemical equilibrium | At equilibrium: Forward reaction continues, Reverse reaction continues. Rates of the two reactions are equal. |
| Polar molecule | a structure that has a slightly positive charge at one end and a slightly negative charge at the other end |
| smallest to largest order of biological organization | Atom → Molecule → Organelle → Cell → Tissue → Organ → Organ System → Organism → Population → Community → Ecosystem → Biosphere |
| Cohesion | Cohesion = attraction between molecules of the same substance. Water molecules stick to other water molecules because of hydrogen bonding. |
| Adhesion | attraction between molecules of different substances. |
| Moderation of Temperature | Water can resist changes in temperature because hydrogen bonds must absorb or release energy when they break or form. Heat is absorbed when hydrogen bonds break, Heat is released when hydrogen bonds form. |
| Evaporative Cooling | When water evaporates: The highest-energy water molecules leave. This removes heat. The remaining surface becomes cooler. |
| Insulation of bodies of water by ice, more "ordered", making ice less dense | Hydrogen bonds organize water molecules into a more ordered structure. structure spaces molecules farther apart. Ice is less dense than liquid water. Ice floats. important for aquatic ecosystems because floating ice can insulate the water underneath. |
| Solution | a homogeneous mixture |
| Solvent | The substance that dissolves another substance |
| Solute | The substance being dissolved |
| Aqueous solution | A solution in which water is the solvent |
| Hydrophilic | Means “water-loving.” Substances that interact well with water. usually polar |
| Hydrophobic | Means “water-fearing.” Substances that do not interact well with water. |
| Colloid | a mixture containing particles that are larger than those in a solution but small enough to remain suspended. Examples: Milk, Gelatin |
| Acid | A substance that increases the concentration of H⁺ in a solution |
| Base | A substance that decreases H⁺ concentration or increases OH⁻ concentration |
| pH scale | 0 → 7 → 14 pH Description: < 7 Acidic 7 Neutral > 7 Basic/alkaline |
| Buffers | helps resist sudden changes in pH. Buffers are important because biological systems require relatively stable pH conditions HCl, NaOH |
| Acid precipitation | ccurs when precipitation becomes unusually acidic because atmospheric pollutants contribute to acid formation. |
| Acidification of the oceans | occurs when increasing amounts of atmospheric CO₂ dissolve into seawater and alter ocean chemistry. can make it more difficult for organisms such as corals and shell-forming organisms to build calcium carbonate structures. |
| Tetravalent | carbon can form four covalent bonds. |
| Frequent partners of Carbon- | H, N, O, C |
| Structural Isomers | Same molecular formula, different covalent arrangement. Geometric, Enantiomers |
| Hydroxyl group | –OH Common in: Alcohols Makes molecules more hydrophilic. |
| Carbonyl group | C=O Carbon double-bonded to oxygen. Aldehyde Carbonyl at the end of a carbon skeleton. Ketone Carbonyl within the carbon skeleton. |
| Amino group | NH₂ Contains nitrogen. Can act as a base by accepting H⁺. Found in amino acids. |
| Sulfhydryl group | Contains sulfur and hydrogen. Important in some proteins. |
| Phosphate group | PO₄ Contains phosphorus surrounded by oxygen. Important in: ATP, DNA, RNA, Phospholipids |
| Methyl group | CH₃ A carbon bonded to three hydrogens. Can influence the shape and function of biological molecules. |
| 3 of the four classes of life’s organic molecules are polymers | Carbohydrates, Proteins, Nucleic acids |
| Condensation | dehydration reaction. It joins molecules together while removing water. monomer to polymer |
| Hydrolysis | polymer to monomer. Water is added to break a larger molecule into smaller molecules. |
| Carbohydrate | Hydrophilic |
| Carb Monosaccharide | Simplest carbohydrates or single sugars Aldoses: Glucose, Ribose Ketoses: Ribulose, Fructose |
| Carb Dissacharides | Made with two monomers Maltose, Sucrose, Lactose |
| Carb Polysaccharide | polymers composed of many sugar building blocks Storage Polysaccharides – Starch. Glycogen Structural Polysaccharides – Cellulose, Chitin |
| Lipids | Do not form polymers, hydrophobic ; Important lipids - fats, phospholipids, and steroids |
| Fats | constructed from: Glycerol and Fatty acid • Triacylglycerol • Saturated and Unsaturated fatty acids • Fat molecules are formed by Ester linkages |
| Phospholipids | Compose of : Two hydrophobic tail and a hydrophilic head • Added to water selfassemble into a bilayer • Found in cell membranes |
| Steroids | • Have carbon skeleton consisting of 4 fused rings • Cholesterol, a steroid in animal cell membranes |
| Proteins | can function as: Enzymes, Structural proteins, Transport proteins, Defense proteins, Signaling proteins, Receptors, Motor proteins |
| Polypeptides | polymers built from the same set of 20 amino acids |
| Amino acids | organic molecules with - carboxyl and amino groups • 20 different Amino acids differ in their properties due to differing side chains, called R groups • Amino acids are linked by peptide bonds |
| Four Levels of Protein Structure | Primary, Secondary, Tertiary and Quaternary structure |
| DNA structure | double helix, Deoxyribose sugar, A, T, C, G, Contains thymine, Stores genetic information |
| RNA structure | single strand, Ribose sugar, A, U, C, G, Contains uracil, Important in gene expression/protein synthesis |
| Nucleic acids | DNA, Deoxyribonucleic acid/RNA, Ribonucleic acid; Their major role is handling/storing genetic information. |
| Geometric Isomers | Same covalent connections, but different arrangement around a double bond. Often described as: cis trans |
| Enantiomers Isomers | Molecules that are mirror images of one another. Left hand ↔ right hand |
| Carboxyl Group | COOH Contains: Carbonyl Hydroxyl Often acts as an acid because it can release H⁺. |
| Nucelotides | monomers of nucleic acid, Each nucleotide contains: A sugar, A phosphate group, A nitrogenous base |
| Primary | The amino acid sequence. |
| Secondary | Local folding patterns. Main examples: α-helix, β-pleated sheet; These are stabilized primarily by hydrogen bonding involving the peptide backbone |
| Tertiary | The overall three-dimensional shape of one polypeptide chain. Interactions among R groups help stabilize this structure. |
| Quaternary | Occurs when multiple polypeptide chains come together to form a functional protein |
Created by:
bethanygumpel