Isotope-same element (same atomic #), different # of neutrons so mass is different

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Jesse Barrett
5 years ago
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1 Proton-subatomic particle located in nucleus. Charge of +1, mass of 1 amu Neutron-subatomic particle located in nucleus. No charge, mass of 1 amu Electron-subatomic particle located outside nucleus. Charge of -1, no mass rbital-area of most probable location for electrons Valence electrons-outermost electrons. Determines chemical properties which is why elements in same group are chemically similar. Last number in electron configuration. In the ground state, Sulfur (S): Excited state- electron pushed to a higher energy level. Sulfur: Atomic mass- protons plus neutrons Atomic number- number of protons (also number of electrons if it is neutral) Isotope-same element (same atomic #), different # of neutrons so mass is different Ion-atom or molecule with positive or negative charge Ionization energy (and trend)-energy needed to remove most loosely held electron. Increases across a period, decreases down a group Table S Electronegativity (and trend)-atom s ability to attract an electron. Increases across a period, decreases down a group Table S Atomic radius (and trend)-size of an atom. Decreases across a period, increases down a group. Table S Metal-elements on the left side of periodic table. Conductivity, malleable, ductile, luster Nonmetal-elements on right side of periodic table. Not conductive, brittle, dull Metalloid-elements located on staircase. Properties are a mix of metals and nonmetals Covalent bond-electrons are shared between two nonmetals Ionic bond-electrons are transferred between a metal and nonmetal Metallic bond-sea of mobile electrons, exists between just one type of metal

2 Intermolecular forces-attractive forces that keep molecules attracted to one another Hydrogen bonding-strongest intermolecular force. Needs H bonded to either fluorine, oxygen, or nitrogen Polar (bond)- covalent bond with electronegativity difference of Non-polar (bond)-covalent bond with electronegativity difference of 0.5 or higher Polar (molecule)-asymmetric distribution of charge Non-polar (molecule)-symmetric distribution of charge Mole-fundamental unit of chemistry Gram-formula mass- mass of one mole of a substance Molecular formula-shows the actual amount of elements in a compound Empirical formula-simplified version of molecular formula Single replacement reaction- A + BC AC + B Double replacement reaction- AB + CD AD + CB Combustion reaction- reaction with oxygen to produce C 2 and H 2 Synthesis reaction- when multiple reactants combine to form one product Decomposition reaction- one reactant is broken down into multiple products Average kinetic energy-temperature Melting- solid liquid Freezing- liquid solid Boiling- liquid gas Condensation- gas liquid Sublimation- solid gas Deposition- gas solid

3 Entropy- disorder or randomness. Solids have low entropy, gases have high entropy Heat of vaporization-energy needed to boil something (H v for water on Table B) Heat of fusion-energy needed to melt something (H f for water on Table B) Specific heat capacity- energy needed to heat one gram of something by one degree (C for water on Table B) Ideal gas-high temperature, low pressure. Move in constant, random straight-lines STP-standard temperature and pressure. Table A Temp is 273 K and press. is 1 atm Soluble- will dissolve Insoluble- won t dissolve Table F Table F Molarity- moles of solute divided by liters of solution. Unit of concentration Saturated solution-as much stuff is dissolved as possible. n Table G it is right on the line Unsaturated solution-more stuff could be dissolved. n Table G it is below the line Supersaturated solution-extra stuff was dissolved. n Table G it is above the line Boiling point elevation-the increase in boiling point that comes from dissolving stuff in solution Freezing point depression-the decrease in freezing point that comes from dissolving stuff in solution Equilibrium-when concentration of products and reactants are constant. Forward and reverse reaction rates are equal Potential energy (PE) diagram-shows the heat lost/gained during a reaction Heat of reaction- energy lost or absorbed during a reaction. PE products -PE reactants Activation energy- energy barrier that must be overcome for a reaction to take place. A catalyst lowers it by giving new reaction pathway. Activation EnergyPeak-PE reactants Endothermic-reaction that absorbs energy Exothermic-reaction that releases energy

4 xidation-reduction reaction- a reaction that involves the transfer of electrons xidation-loss of electrons Reduction-gain of electrons Voltaic cell-electrochemical cell that spontaneously converts chemical energy to electrical Electrolytic cell- non spontaneous electrochemical cell converts electrical energy to chemical Anode-where oxidation takes place Cathode-where reduction takes place Salt bridge-allows for the exchange of ions between half cells xidation state/number- charge on an atom/ion Hydrocarbon-compound that only contains carbon and hydrogen Homologous series- Alkane-all single bonds. General formula=c n H 2n+2 Alkene- one double bond. General formula=c n H 2n Alkyne- one triple bond. General formula=c n H 2n-2 Isomer- same molecular formula, different structure Saponifaction reaction- organic reaction used to produce soap Esterification reaction- organic acid + alcohol ester + H 2 Fermentation reaction- breaking down sugar with an enzyme to produce an alcohol Substitution reaction- replacing hydrogens in an alkane with new atoms Addition reaction- adding new atoms across a double/triple bond in an alkene/alkyne Polymerization reaction- used to make long chains. Produces rubbers/plastics/fabrics/etc. Fusion- light nuclei combine to form larger atom

5 Fission- splitting a heavy element into smaller atoms Nuclear Decay- breakdown of a radioactive isotope Alpha particle- mass of 4, charge of +2 (2 neutrons, 2 protons) Beta particle- no mass, -1 charge Positron- no mass, +1 charge Half-life- amount of time it takes for half of a radioactive substance to decay into something else Transmutation- reaction that changes an atom from one element to another Acid (arrhenius acid)- substance that produces H + when dissolved in water. ph below 7. H + donor Table K Base (arrhenius base)- substance that produces H - when dissolved in water. ph above 7. H + acceptor, H - donor Table L Neutralization reaction- acid + base salt + water HCl + NaH NaCl + H 2 Electrolyte-a substance that produces ions when dissolved in water. This makes it capable of conducting electricity in solution. Acids, bases, and ionic compounds (salts) are electrolytes Titration-using a solution of known concentration to determine the concentration of an unknown solution equation: M a V a (# of H + in acid)=m b V b (# of H - in base)

1. Atomic Concepts. The student should be able to: relate experimental evidence to models of the atom

1. Atomic Concepts. The student should be able to: relate experimental evidence to models of the atom 1. Atomic Concepts The modern model of the atom has evolved over a long period of time through the work of many scientists. Each atom has a nucleus, with an overall positive charge, surrounded by negatively