Foundational Chemistry Vocabulary Zumdahl Chemistry Wheaton Academy (Regular and Honor’s Chemistry) Elements and their symbols (must have memorized in the first week of school) Aluminum Al Lithium Li Antimony(Stibium) Sb Magnesium Mg Argon Ar Manganese Mn Arsenic As Mercury (Hydrargyrum) Hg Barium Ba Neon Ne Beryllium Be Nickel Ni Bismuth Bi Nitrogen N Boron B Oxygen O Bromine Br Phosphorus P Cadmium Cd Platinum Pt Calcium (Lime) Ca Potassium (Kalium) K Carbon C Radium Ra Cesium Cs Radon Rn Chlorine Cl Rubidium Rb Chromium Cr Silicon Si Cobalt Co Silver (Argentum) Ag Copper (Cuprum) Cu Sodium (Natrium) Na Fluorine F Strontium Sr Gold (Aurum) Au Sulfur (Brimstone) S Helium He Tin (Stannum) Sn Hydrogen H Titanium Ti Iodine I Tungsten(Wolfram) W Iron (Ferrum) Fe Uranium U Krypton Kr Xenon Xe Lead (Plumbum) Pb Zinc Zn June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Chapter 1: Chemistry—the science that deals with the materials of the universe and the changes that these materials undergo. Scientific Method—a process of studying natural phenomena that involves making observations, forming laws and theories, and testing theories by experimentation. Measurement—a quantitative observation, involves a number and a unit Theory—a set of tested hypotheses that gives an overall explanation of some part of nature Natural Law—a statement that expresses generally observed behavior Chapter 2: Matter- the material of the universe Atom – the fundamental unit of which elements are composed Compound- a substance with constant composition that can be broken down into elements by chemical processes Molecule- a bonded collection of two or more atoms of the same element of different elements Element- a substance that cannot be decomposed into simpler substances by chemical or physical means. It consists of atoms all having the same atomic number. Graphite- carbon based: material that makes up pencil “lead” Diamond- carbon based: hard gemstone Buckminsterfullerene- carbon based: a third form of elemental carbon Solid- one of the three states of matter; has a fixed shape and volume Liquid- one of the three states of matter; has a fixed volume but takes the shape of its container Gas- one of the three states of matter; has neither fixed shape nor fixed volume Physical Properties- a characteristic of a substance that can change without the substance becoming a different substance. Chemical Properties- the ability of a substance to change to a different substance Physical Change- a change in the form of a substance, but not in its chemical nature; chemical bonds are not broken in a physical change. Chemical Change- the change of substances into other substances through a reorganization of the atoms; a chemical reaction. Reaction- involves a change in the fundamental components of the substance; a given substance changes into a different substance or substances Mixture- a material of variable composition that contains two or more substances. Alloy- a substance that contains a mixture of elements and has metallic properties. Pure Substance- a substance with constant composition Homogeneous Mixture- a mixture that is the same throughout; a solution Solution- a homogeneous mixture Heterogeneous Mixture- a mixture that has different properties in different regions of the mixture. Distillation- a method for separating the components of a liquid mixture that depends on differences in the ease of vaporization of the components. Filtration- a method for separating the components of a mixture containing a solid and a liquid June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Chapter 3: Element Symbols—abbreviations for the chemical elements Law of Constant Composition—a given compound always contains elements in exactly the same proportion by mass Dalton’s Atomic Theory—1. Elements are made of tiny particles called atoms. 2. All atoms of a given element are identical. 3. All atoms of a given element are different from those of any other element. Atom—the fundamental unit of which elements are composed Compound—a substance with constant composition that can be broken down into elements by chemical processes Chemical Formula—a representation of a molecule in which the symbols for the elements are used to indicate the types of atoms present and subscripts are used to show the relative numbers of atoms Electron—a negatively charged particle that occupies the space around the nucleus of an atom Nuclear Atom—the modern concept of the atom as having a dense center of positive charge (the nucleus) and electrons moving around the outside Nucleus—the small, dense center of positive charge in an atom Proton—a positively charged particle in an atomic nucleus Neutron—neutral particle contained in the nucleus of the particle, slightly more massive than a proton but has no charge. Isotopes—atoms of the same element (the same number of protons) that have different numbers of neutrons. They have identical atomic numbers but different mass numbers. Atomic Number—the number of protons in the nucleus of an atom; each element has a unique atomic number Mass Number—the total number of protons and neutrons in the atomic nucleus of an atom Periodic Table—a chart showing all the elements arranged in columns in such a way that all the elements in a given column exhibit similar chemical properties Groups (of the periodic table)—a vertical column of elements having the same valence electron configuration and similar chemical properties. Alkaline Metals—a group 1 metal (first column on left hand side of periodic table) Alkaline Earth Metals—a group 2 metal (2nd column on left hand side of periodic table) Halogens—a group 7 element (2nd column from the right on the periodic table) Noble Gases—a group 8 element (last column on right on the periodic table) Transition Metals—several series of elements in which inner orbitals (d or f orbitals) are being filled. Metal—an element that gives up electrons relatively easily and is typically lustrous, malleable, and a good conductor of heat and electricity. Nonmetal—an element that does not exhibit metallic characteristics. Chemically, a typical nonmetal accepts electrons from a metal. Metalloids (Semi-metals)—elements that have both metallic and non-metallic properties. Diatomic Molecule—a molecule composed of two atoms Ion—an atom or a group of atoms that has a net positive or negative charge. Cation—a positive ion June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Anion—a negative ion Ionic Compound—a compound that results when a metal reacts with a nonmetal to form cations and anions. Chapter 4: Binary Compound- a two-element compound Binary Ionic Compound- contain a positive ion, and negative ion Polyatomic Ion- an ion containing two or more atoms Oxyanion- several series of polyatomic anions exist that contain an atom of a given element and different numbers of oxygen atoms Acid- a substance that produces hydrogen ions in aqueous solution; a proton donor. Chapter 5: Measurement—a quantitative observation Scientific Notation—expresses a number in the form n x 10^m; a convenient method for representing a very large or very small number and for easily indication the number of significant figures. Units—tells us what scale or standard is being used to represent the results of the measurement. English System—units system used in the United States Metric System—units system used in most of the industrialized world. It is preferred for scientific work. SI Units—International System of units based on the metric system and on units derived from the metric system. Volume—the amount of three-dimensional space occupied by a substance. Liter—1 dm3 Milliliter—1 cm3 Kilogram—fundamental SI unit of mass Gram—the prefixes for various mass units are based on the gram.1/1000 of a kilogram. Mass—the quantity of matter in an object Significant Figures—the certain digits and the first uncertain digit of a measurement Rounding Off—in a series of calculations, carry the extra digits through to the final result and then round off. Conversion Factor—a ratio of the two parts of the statement that relates the two units. Equivalence Statement—equivalents between the English and metric systems Dimensional Analysis—changing from one unit to another via conversion factors (based on the equivalence statements between the units) Fahrenheit Scale—temperature scale widely used in the United States and Great Britain, and it is the scale employed in most of the engineering sciences. Celsius Scale—temperature scale used in Canada and Europe and in the physical and life sciences in most countries Kelvin scale—another temperature scale used in the sciences Density—a property of matter representing the mass per unit volume Specific Gravity—the ratio of the density of a given liquid to the density of water at 4 degrees Celsius. June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Chapter 6: Atomic Mass Unit- smaller unit of mass; 1 amu = 1.66 X 10^-24 g Average Atomic Mass- average mass of an element Mole- the number equal to the number of carbon atoms in exactly 12 grams of pure 12C: Avogadro’s number. One mole represents 6.022 X 10^23 units. Avogadro’s number- the number of atoms in exactly 12 grams of pure 12C, equal to 6.002 X 10^23. Molar Mass- the mass in grams of one mole of a compound Mass Percent- the percent by mass of a component of a mixture or of a given element in a compound Empirical Formula- the simplest whole-number ratio of atoms in a compound Molecular Formula- the exact formula of a molecule, giving the types of atoms and the number of each type Chapter 7: Chemical Reaction—a chemical changed always involves a rearrangement of the ways in which the atoms are grouped.