deck_8020633 Flashcards
<p>A branch of physical science that studies the composition, structure, properties and change of matter</p>
<p>Chemistry</p>
<p>Deals with chemical processes that occur in living organisms</p>
<p>Biochemistry</p>
<p>Works with fundamental principles of physics and chemistry</p>
<p>Physical Chemistry</p>
<p>Separation and identification of chemical substances</p>
<p>Analytical Chemistry</p>
<p>Focuses on substances that contain carbon and hydrogen in combination with a few other elements</p>
<p>Organic Chemistry</p>
<p>Focuses on most of the elements other than carbon</p>
<p>Inorganic Chemistry</p>
<p>Anything that occupies space (or has volume), displays a property known as mass, and possess inertia; can be a pure chemical substance or a mixture of substances</p>
<p>Matter</p>
<p>Refers to the parts or components of a sample of matter and their relative proportions</p>
<p>Composition</p>
<p>The qualities or attributes that can be used to distinguish one sample of matter from others</p>
<p>Properties</p>
<p>one that a sample of matter displays without changing its composition</p>
<p>Physical property</p>
<p>a physical property of a system that does not depend on the system size or the amount of material in the system</p>
<p>Intensive property (bulk property)/intrinsic property</p>
<p>one that is additive for <strong>independent, non-interacting subsystems</strong></p>
<p>Extensive property/extrinsic property</p>
<p>the ability (or inability) of a sample of matter to undergo a change in composition under stated conditions</p>
<p>Chemical property</p>
<p>a modern version of the metric system; a decimal system</p>
<p>SI = Système Internationale d’Unités (International System of Units)</p>
<p>Refers to how close a measured value is tothe accepted, or “real,” value</p>
<p>Accuracy</p>
<p>Refers to the degree of reproducibility of ameasured quantity</p>
<p>Precision</p>
<p>Not determined by chance but is introduced by an inaccuracy (as of observation ormeasurement) inherent in the system</p>
<p>Systematic Errors</p>
<p>Caused by inherently unpredictablefluctuations in the readings of a measurement apparatus or in the experimenter's interpretation of the instrumental reading</p>
<p>Random errors</p>
<p>describes the QUANTITY OF METTER in an object; SI unit, kilogram (kg)</p>
<p>Mass (𝒎)</p>
<p>the force of gravity on an object𝑊=𝑔×𝑚</p>
<p>Weight (𝑾)</p>
<p>those of length, mass, time, temperature, amount of substance, electric current, and luminous intensity (SI units)</p>
<p>Fundamental (base) quantities </p>
<p>combinations of certain of these fundamental quantities; e.g., velocity (m/s), volume (cm3 or cc or mL), density (g/mL)</p>
<p>Derived units</p>
<p>term applied to elements and compounds (whose composition and properties are uniform throughout a given sample and from one sample to another)</p>
<p>Substance</p>
<p>a substance made up of only a single type of atom distinguished by its atomic number, which is the number of protons in its atomic nucleus; divided into metals, metalloids, and nonmetals; 118 known chemical elements (as of 2010); 98 chemical elements occur naturally on earth</p>
<p>Element </p>
<p>the smallest constituent unit of ordinary matter that has the properties of a chemical element</p>
<p>Atom</p>
<p>substance in which atoms of different elements are combined with one another</p>
<p>Compound</p>
<p>the smallest entity having the same proportions of the constituent atoms as does the compound as a whole</p>
<p>Molecule</p>
<p>made of two or more types of substances</p>
<p>Mixtures</p>
<p>uniform in composition and properties throughout a given sample, but the composition and properties may vary from one sample to another</p>
<p>Solutions (homogeneous mixtures)</p>
<p>whose components separate into distinct regions; the composition and physical properties vary from one part of the mixture to another</p>
<p>Heterogeneous mixtures</p>
<p>occurs when a sample of matter changes its physical appearance; its composition remains unchanged; includes changes in texture, color, temperature, shape, state</p>
<p>Physical change </p>
<p>when one or more samples of matter are converted to new samples with different compositions; indications include change in temperature, change in color, noticeable odor, formation of a precipitate, formation of bubbles</p>
<p>Chemical change</p>
<p>State of matter that maintains a<strong>fixed </strong>volume and shape,with component particles (atoms, molecules or ions) <strong>[IFA] close together </strong>and <strong>fixed into place</strong></p>
<p><strong>Molecular Motion:</strong>Vibration</p>
<p>Solid</p>
<p>States of Matter that maintains a <strong>fixed volume,</strong> but has a <strong>variable shape</strong> that adapts to fit its container. Its particles <strong>[IFA] are still close together but move freely</strong></p>
<p><strong>Molecular Motion: </strong>Gliding</p>
<p>Liquid</p>
<p>States of Matter: has <strong>both variable volume and shape,</strong> adapting both to fit its container. Its particles <strong>[IFA] are neither close together nor fixed in place</strong></p>
<p><strong>Molecular Motion:</strong>Constant random motion</p>
<p>Gas</p>
<p>States of Matter: has <strong>variable volume and shape,</strong> but as well as <u>neutral atoms,</u> it contains a s<strong>ignificant number of ions and electrons,</strong> both of which <strong>can move around freely</strong></p>
<p>Plasma</p>
<p>The state or phase of a given set of matter can change depending on pressure and temperature conditions.</p>
<p>State of Matter</p>
<p>Phase Transitions:Solid to Liquid</p>
<p>Melting (Fusion)</p>
<p>Phase Transitions:Liquid to Gas</p>
<p>Vaporization</p>
<p>Phase Transitions:Gas to Plasma</p>
<p>Ionization</p>
<p>Phase Transitions:Plasma to Gas</p>
<p>Deionization</p>
<p>Phase Transitions:Gas to Liquid</p>
<p>Condensation</p>
<p>Phase Transitions:Liquid to Solid</p>
<p>Freezing</p>
<p>Phase Transitions:Solid to Gas</p>
<p>Sublimation</p>
<p>Phase Transitions:Gas to Solid</p>
<p>Deposition</p>
<p>Chemical Reaction:two or more simple substances combineto form a more complex substance</p>
<p>Synthesis </p>
<p>Chemical Reaction:when a more complex substance breaks down into its more simple parts</p>
<p>Decomposition</p>
<p>Chemical Reaction:a single uncombined elementreplaces another in a compound, one element trades places with another element in a compound</p>
<p>Single Replacement</p>
<p>Chemical Reaction:the anions and cations oftwo compounds switch places and form two entirely different compounds</p>
<p>Double Replacement</p>
<p>Chemical Reaction:involves a transfer of protons (H+) from one species (the acid) to another (the base)</p>
<p>Neutralization (acid-base reaction)</p>
<p>Chemical Reaction:the formation of a solid in a solution or inside another solid during a chemical reaction</p>
<p>Precipitation</p>
<p>Chemical Reaction:when ligands (with lone pairs) react with a metal atom (with empty orbitals) to form acoordination complex</p>
<p>Complexation </p>
<p>Chemical Reaction:transfer of electrons from one involved species (reducing agents) to another (oxidizing agent); the former species is oxidized and the latter is reduced</p>
<p>Reduction and oxidation (redox reaction)</p>
<p>Chemical Reaction:when atoms and molecules absorb energy (photons) of the illumination light and convert into an excited state; energy is released by breaking chemical bonds</p>
<p>Photochemical reaction</p>
<p>Chemical Reaction:very slow reaction between solids</p>
<p>Solid-state reaction</p>
<p>Chemical Reaction:surfaces at very low pressure such as ultra-high vacuum</p>
<p>Reaction at the solid-gas interphase</p>
<p>The total mass of substances present after a chemical reaction is the same as the total mass of substances before the reaction.</p>
<p>Law of Conservation of Mass</p>
<p>All samples of a compound have the same composition—the same proportions by mass of the constituent elements.</p>
<p>Law of Constant Composition (Law of DefiniteProportions)</p>
<p>If two elements can be combined to form a number of possible compounds, then the ratios of the masses of the second element which combine with a fixed mass of the first element will be ratios of small whole numbers.</p>
<p>Law of Multiple Proportions</p>
<p>Atomic Models:all matter was composed of smallindivisible particles called atoms (atomos, Gr. “uncuttable”)</p>
<p>Democritus</p>
<p>Atomic Models:“billiard ball model” (1808); proposedthat each chemical element is composed of atoms of a single, unique type, and though they cannot be altered or destroyed by chemical means, they can combine to form more complex structures</p>
<p>John Dalton</p>
<p>Atomic Models:“plum pudding model” (1903); discovered the electron through his work on cathode rays</p>
<p>J.J. Thomson</p>
<p>Atomic Models:“nuclear/planetary model” (1911); discovered that most of the mass and positive charge of an atom is concentrated in a very small fraction of its volume, which he assumed to be at the very center</p>
<p>Ernest Rutherford</p>
<p>A type of particle that carry two fundamental units of charge; same mass as He</p>
<p>Alpha (α) particles</p>
<p>A type of negatively charged particles produced by changes occurring within the nuclei of radioactive atoms; same properties as electrons</p>
<p>Beta (β) particles</p>
<p>Atomic Models:“shell model” (1923); electrons are arranged around the nucleus in discrete energy levels or shells</p>
<p>Neils Bohr</p>
<p>Atomic Models:“electron cloud model”; assumes that the electron is a wave and tries to describe the regions in space, or orbitals, where electrons are most likely to be found</p>
<p>Erwin Schrödinger</p>
<p>made the first cathode ray tube(CRT)</p>
<p>Michael Faraday</p>
<p>determined the electronic charge ethrough a series of “oil drop” experiments;e = –1.6022x10^-19 Cme = 9.1094x10^-28 g</p>
<p>Robert Millikan</p>
<p>discovered X-rays</p>
<p>Wilhelm Roentgen</p>
<p>discovered radioactivity</p>
<p>Antoine Henri Becquerel</p>
<p>discovered gamma (γ) radiation, which is not made of particles</p>
<p>Paul Villard</p>
<p>discovered transmutation (fundamental changes at the subatomic level in which one element is changed into another in radioactive decay</p>
<p>Frederick Soddy (and Rutherford)</p>
<p>(1932) discovered neutral particles called neutrons that originate from the nuclei of atoms</p>
<p>James Chadwick</p>
<p>The more precisely the position is determined, the less precisely the momentum is known in this instant, and vice versa.</p>
<p>Heisenberg’s Uncertainty Principle</p>
<p>the sets of numerical values which give acceptable solutions to the Schrödinger wave equation for the hydrogen atom</p>
<p>Quantum Numbers</p>
<p>Quantum Numbers:the electron shell, or energy level, of an atom</p>
<p>Principal quantum number (n)</p>
<p>Quantum Numbers:describes the subshell: l = 0 (s orbital); 1 (p orbital), 2 (d orbital), 3 (f orbital)</p>
<p>Azimuthal quantum number (l)/ angular quantum number or orbital quantum number;</p>
<p>Quantum Numbers:describes the specific orbital (or “cloud”) within that subshell; orientation of the subshell's shape; range from −l to l</p>
<p>Magnetic quantum number (ml)</p>
<p>Quantum Numbers:describes the spin (intrinsic angular momentum) of the electron within that orbital</p>
<p>Spin projection quantum number (ms)</p>
<p>States that it is impossible for two electrons of an atom to have the same values of the four quantum numbers (n, l, ml and ms).</p>
<p>Pauli’s Exclusion Principle(Wolfgang Pauli (1925))</p>
<p>-coined by Robert Mulliken in 1932 as an abbreviationfor one-electron orbital wave function- mathematical function that describes the wave-likebehavior of either one electron or a pair of electrons in an atom- the region in space where an electron is most likely tobe found</p>
<p>Atomic Orbitals:sharp (s orbital, l = 0)principal (p orbital, l = 1)diffuse (d orbital, l = 2)fundamental/fine (f orbital, l = 3)</p>
<p>The distribution of electrons of an atom or molecule in atomic or molecular orbitals</p>
<p>Electron Configuration</p>
<p>Electron Configuration:(from the German aufbau, "building up, construction") – the lowest-energy orbitals are filled before electrons are placed in higher-energy orbitals</p>
<p>Aufbau’s principle</p>
<p>“bus seat rule”; the orbitals of the subshell are each occupied singly with electrons of parallel spin before double occupation occurs</p>
<p>Hund’s rule of maximum multiplicity</p>
<p>exactly 1/12 of the mass of an unbound neutral atom of carbon-12 in its nuclear and electronic ground state; equivalent to 1 Da (dalton)</p>
<p>Unified atomic mass unit (amu or u) </p>
<p>the number of protons in an atom</p>
<p>Atomic number (proton number, Z) </p>
<p>the total number of protons and neutrons (nucleons)</p>
<p>Mass number (A)</p>
<p>the number of neutrons; A – Z</p>
<p>Neutron number </p>
<p>the average of the isotopic masses weighted according to the naturallyoccurring abundances of the isotopes of the element</p>
<p>Atomic mass (atomic weight)</p>
<p>the general term used to describe an atom with a particular atomic number and mass number</p>
<p>Nuclides</p>
<p>two or more atoms having the same atomic number (Z) or number of protons, but different mass numbers (A) or number of neutrons</p>
<p>Isotopes</p>
<p>nuclides of equal number of neutrons, but different number of protons</p>
<p>Isotones</p>
<p>atoms of different chemical elements that have the same number of nucleons; differ in atomic number, but have the same mass number</p>
<p>Isobars</p>
<p>nuclides with equal protonnumber and equal mass number, but different statesof excitation</p>
<p>Nuclear isomers</p>
<p>neutron and proton number exchanged</p>
<p>Mirror nuclei</p>
<p>unstable and radioactive nuclides</p>
<p>Radionuclides</p>
<p>decay products</p>
<p>Radiogenic nuclides </p>
<p>an elementary particle and a fundamentalconstituent of matter</p>
<p>Quark</p>
<p>composite particles made of quarks, e.g.,protons (2 up quarks + 1 down quark) and neutrons (3quarks)</p>
<p>Hadron</p>
<p>composite subatomic particles made up of 3quarks; e.g., neutron</p>
<p> Baryon</p>
<p>any baryon containing on or more strangequarks, but no charm, bottom, or top quark</p>
<p>Hyperon</p>
<p>composed of one quark and one antiquark, bound together by a strong interaction; about 2/3 the size of a proton or neutron; charged mesons decay to form electrons and neutrinos; uncharged mesons may67 decay to photons</p>
<p>Meson</p>
<p>an elementary, half-integer spin particle thatdoes not undergo strong interactions; e.g., electron</p>
<p>Lepton</p>
<p>neutral leptons</p>
<p>Neutrino</p>
<p>a tabular arrangement of the chemical elements, organized on the basis of their atomic number, electron configurations, and recurring chemical properties</p>
<p>Periodic Table of Elements</p>
<p>Periodic Table of Elements:places similar elements</p>
<p>vertical groups (or families)</p>
<p>Periodic Table of Elements:horizontal rows </p>
<p>periods</p>
<p>published a list of 33 elements grouped into gases, metals, nonmetals, and earths</p>
<p>Antoine Lavoisier</p>
<p>Law of Triads (1829), e.g., Li, Na, K were grouped together as soft, reactive metals</p>
<p>Johann Wolfgang Döbereiner</p>
<p>(1858) observed valency</p>
<p>August Kekulé</p>
<p>(1862) first noticed the periodicity of elements; published an early form of periodic table called the telluric helix (orscrew)</p>
<p>Alexandre-Emile Béguyer de Chancourtois</p>
<p>Law of Octaves (1863 to 1866)</p>
<p>John Newlands</p>
<p>Categories of Elements:generally malleable and ductile; goodconductors of heat and electricity; lustrous and shiny</p>
<p>Metals</p>
<p>Categories of Elements: “opposite” properties of metals</p>
<p>Nonmetals</p>
<p>Categories of Elements:have some metallic and somenonmetallic properties; e.g., B, Si, Ge, As, Sb, Te, Po,At</p>
<p>Metalloids</p>
<p>Categories of Elements: have complete octet; e.g., He, Ne, Ar,Kr, Xe, Rn</p>
<p>Noble gas</p>
<p>Categories of Elements:the series of 14 elements that follow57La at Period 6</p>
<p>Lanthanides </p>
<p>Categories of Elements:the series of 14 elements that follow 89Acat Period 7</p>
<p>Actinides</p>
