CHEM 101 Cumulative Exam Review PDF

**CHEM 101 Cumulative Exam Review** [This guide is not comprehensive. You should review all the information on the reading logs and worksheets.] Know important terms listed in reading logs. Chemistry- study of the composition, structure, properties and reactions of matter Chemical- substance tha...

**CHEM 101 Cumulative Exam Review** [This guide is not comprehensive. You should review all the information on the reading logs and worksheets.] Know important terms listed in reading logs. Chemistry- study of the composition, structure, properties and reactions of matter Chemical- substance that always has the same composition and properties whenever it is found Element- a pure substance made up of only one type of atom Compound- derived from the utilization of physical or chemical resources Pure substance- consists only of one element or one compound Mixture- consists of two or more different substance not chemically joined together Metal- have shiny metallic luster and reflective surface Nonmetals- generally dull or nonreflective and don't have metallic luster Metalloids- have metallic or nonmetallic appearance depending on the elements Atomic number- the number of protons in the nucleus of an atom which determines the chemical properties of an element and its place in the periodic table Mass number- total number of protons and neutrons in an atom Isotope- each of two or more forms of the same element that contains equal numbers of protons but different numbers of neutrons in their nuclei Average atomic mass- an element is the weight average mass of the atom in a naturally occurring sample of the element Valence electrons- are electrons that are located in the outermost electron shell of an atom Half-life- the time taken for the radioactivity of a specified isotope to fall to half its original value Fission- action of dividing or splitting something into two or more parts Chain reaction- chemical reaction or other process in which the products themselves promote or spread the reaction Fusion- result of 2 nuclei joining to form 1 larger nuclei Octet rule- the tendency of atoms to prefer to have eight electrons in a valence shell Ionic bond- type of linkage formed from the electrostatic attraction between oppositely charged ion in a chemical compound Covalent bond- chemical bond that involves the sharing of electrons to form electron pairs between atoms Valence electrons- electrons located in the outermost electron shell of an atom Molar mass- sum of the mass of all atoms found in one mole worth of a substance Combustion reaction- evolving heat and light Decomposition- involves a substance breakdown into two or more substances Synthesis- is the opposite, two or more substances combining to produce one Single replacement- an element in a compound is replaced by a large element in the reaction Double replacement- element of like charges trade places Endothermic- a reaction accompanied by or requiring the absorption of heat Exothermic -- reaction accompanied by the release of heat Charles' Law- the pressure on a sample of a dry gas is held constant, the kelvin temperature and therefore the volume is going to be in direct proportion Avogadro's Law- a law stating that equal volumes of gases at the same temperature and pressure contain equal number of molecules Gay-Lussac's Law- the pressure of a given amount of gas held at constant volume is directly proportional to kelvin temperature Dalton's Law- the total pressure by a mixture of gases of each of the sum of the partial pressures of each of the constituent gases Solution- homogenous type of a mixture of two or more substances Solute- a substance that can be dissolved into a solution by a solvent Solvent- substance with the ability to dissolve other substances to form a solution Electrolyte- substance that conducts electricity when dissolved in a solvent like water Saturated- contained the greatest possible number of hydrogen atoms and so having no carbon Unsaturated- having carbon-carbon double or triple bonds and therefore not containing the hydrogen atoms for the numbers of carbons Supersaturated- increase the concentration of a solution beyond saturation point Arrhenius Acid- compound that increased the H^+^ ion concentration in aqueous solution Arrhenius Base- compound that increased OH^-^ ion concentration in aqueous solution Bronsted- Lowry Acid- proton donor Bronsted- Lowry Base- proton acceptor Amphoteric substance- a substance that has the ability to act either as an acid or base LeChatelier's Principle- a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change pH- measure of how acidic/base water is Buffer- a solution that resists changes pH when acid or alkali is added Organic chemistry- study of carbon compounds Hydrocarbon- compound of hydrogen and carbon Alkane- any of the series of saturated hydrocarbon including methane, ethane, propane and higher members Cycloalkane- saturated hydrocarbon molecule where the carbon atoms are arranged in close ring structure Isomer- each of two or more compounds with the same formula but different arrangement of atoms in the molecule and different properties Saturated Fats- lacks double bonds between the individual carbon atoms Unsaturated Fats- at least one double bond in the fatty acid chain Aromatic Compound- a hydrocarbon that contains one or more benzene-like ring Carbohydrate- sugar molecule and a macronutrient found in food and drinks that gives our body energy Enantiomers- pair of molecules that have the same chemical formula but mirror one another Steroid- any of a group of lipids that have a certain chemical structure Protein- complex molecule made up of amino acids Nucleic Acid- complex organic substance present in living cells Diatomic elements. - Composed of only two atoms of the same element - Acronym: BrINCIHOF - Bromine -liquid at room temperature - Iodine- solid at room temperature - Nitrogen- gases at room temperature - Chlorine- gases at room temperature - Hydrogen- gases at room temperature - Oxygen- gases at room temperature - Fluorine- gases at room temperature - Bonds holding these diatomic molecules together are covalent bonds Convert metric units, like grams to kilograms and vice versa, etc. - 0.0687km = \_\_\_\_cm - 1.2miles = \_\_\_km - 17.0ft/s = \_\_\_\_m/min Modern Atomic theory, isotopes, parts of an atom 1. Aluminum 2. Oxygen 3. Iron Ion formation, Ionic nomenclature, covalent nomenclature - **Ion formation**: atoms form ions by gaining or losing electrons to achieve a stable electron configuration often resembling the nearest noble gas - Cations (positive) lose electrons - Example: - Na loses 1 election \-\-- Na^+^ - Mg loses 2 electrons\-\-- Mg^2+^ - **Ionic nomenclature:** consist of metal and nonmetals - Naming them the cation goes first then the anion - Single element anions changes to the suffix "-ide" - Example: - Chlorine = chloride - Polyatomic ions use the standard names - Example: - Sulfate - Examples: - NaCl ; sodium chloride - FeCl~3~ ; Iron(III) chloride - NH~4~NO~3~ ; Ammonium nitrate - **Covalent nomenclature**- covalent compounds consist of two nonmetals - Naming you would use "-ide" , using the prefixes to indicate the number of atoms of each element - Mono -1 , Di-2, Tri-3 - Examples: - CO~2~; carbon dioxide - N~2~O~4~; Dinitrogen tetroxide - SF~6~; sulfur hexafluoride - PCl~3~; phosphorous trichloride Structural descriptions of biochemical molecules. (proteins, carbohydrates, lipids, nucleic acids) - Proteins: monomers and are polymers of amino acids linked by peptide bonds - four major structures of proteins: - **primary structure**- linear chain of amino acids. Number and sequence of amino acids varies. - **secondary structure**-shortening of amino acid chain by coiling or pleating - **tertiary structure**- further folding of chain to create a more compact structure - **quaternary structure**- only some proteins have this structure which is two or more chains bonded together - carbohydrates: monosaccharides and consist of carbon, hydrogen and oxygen - **starch**- storage form in plants, make of alpha glucose - **glycogen**- storage form in animals and highly branches - **cellulose**- structural component in plant cell walls made of beta glucose - lipids- fatty acids and glycerol and are hydrophobic composed of mainly C and H - types of lipids: - **Fats (Triglycerides):** - Glycerol backbone + three fatty acid chains. - Fatty acids can be **saturated** (no double bonds, straight chains) or **unsaturated** (one or more double bonds, kinked chains). - **Phospholipids:** - Glycerol backbone, two fatty acid tails, and a phosphate group. - Amphipathic (hydrophilic head and hydrophobic tails), forming cell membranes. - **Steroids:** - Four fused hydrocarbon rings (e.g., cholesterol, hormones like testosterone and estrogen). - Nucleic acids: consists of RNA and DNA, phosphate groups Periodic trends (atomic size, electronegativity, ionization energy, etc.) **Summary Table of Trends** **Property** **Across Period (Left → Right)** **Down Group (Top → Bottom)** ------------------------ ---------------------------------- -- ------------------------------- **Atomic Size** Decreases Increases **Electronegativity** Increases Decreases **Ionization Energy** Increases Decreases **Electron Affinity** Becomes more negative Becomes less negative **Metallic Character** Decreases Increases Types of chemical reactions. 1. \_\_\_K + \_\_\_\_B~2~O~3~ \_\_\_ K~2~O + \_\_B 2. \_\_\_ HCL + \_\_\_ NaOH \_\_\_ NaCl + \_\_H~2~O 3. \_\_\_C~10~H~22~ + \_\_\_ O~2~ \_\_\_CO~2~ + \_\_\_H~2~O 4. \_\_\_C + \_\_\_S~8~ \_\_\_CS~2~ Moles & Stoichiometry problems Using volumes of gas for stoichiometry. Properties of gases, liquids, solids. Kinetic molecular theory of gases. Gas law problems, P~1~V~1~ = P~2~V~2~ type problems (etc.) Shapes of molecules using VSEPR theory. Solution calculations, %mass, molarity, & dilution (C~1~V~1~) = (C~2~V~2~) Acid-base definitions. Chemical behavior of weak acids and bases. Neutralization reactions. Types of radiation. Balancing nuclear equations. Organic nomenclature and structures, functional groups Using density to convert mass to volume or vice versa. Calculating drug dosage. Calculating pH from hydrogen ion concentration and vice versa. Half-life calculation. Nomenclature. Significant digits.