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Scientific Method:-# # # # Observations :- facts natural law. model :- 1- Predictions. 2-hypothesis. theory:- experiments to test the theory. Chemistry:-The study of matter and the changes it can undergo MATTER:-Matter is any thing occupies space and has a mass. Matter------> has mass , mass to weight , occupies space. There are things you can see.. "e.x: water, tree, food". And there are things you can't see.. " air, gas in gas cylinders". Properties of Matter:-*Extensive Property-depends on specific sample under investigation . examples: mass and volume * Intensive Property identical in all samples of the substance. examples: color, density, melting point, etc. 1/ Physical Property The characteristics of a substance that can be observed without changing the substance. * Mass (EXTENSIVE property). * Volume (EXTENSIVE property). * Size. * Shape. * Density (INTENSIVE property). * Freezing and Boiling Points. * Odor. * Colour. Extensive property: depend on the quantity of Substance. Intensive property: does not depend on the quantity of substance . >> density = mass/ volume. Temperature Relationships:-C = 100/180 * (F - 32) F = (180/100)*C + 32 K = C + 273.15 - 40o F = - 40o C 2/ Chemical Properties The characteristics of a substance that can be observed with changing the substance. Burning>> CH4 + O2 Combination>> 2H2 + O2 Decomposition>> 2H2O CO2 + 2H2 2H2 O2 + 2H2 REPLACEMENT REACTION:-- Substance & Mixture:-SUBSTANCE: Is a form of matter which has a definite composition and distinct properties. Mixture: A combination of two or more substances in which the substances retain their distinct properties. TYPES OF MIXTURES:-HOMOGENEOUS: The composition is uniform (WATER + SALT) HETEROGENEOUS: The composition is not uniform (WATER + SAND) Separation of Mixtures:-* Filtration . * distillation. * chromatography. Filtration>>* separate solids by differences in melting points. * separate solids by differences in solubility (fractional crystallization). * mechanical separation. Distillation>> *separation by differences in boiling point(fractional distillation). * fractionating column - part of apparatus where separation occurs. Chromatography >> * liquid-column * paper * thin-layer (TLC) * gas * HPLC * electrophoresis (DNA mapping) Pure Substances:-- Elements & Compounds Elements:-- * Pure substances that cannot be separated into different substances by ordinary processes. * Are the building blocks of matter. Examples:>>> carbon , calcium , gold. Symbols from Latin Names Latin name Copper Gold Lead Mercury Potassium Silver Sodium Tin Symbol Cu Au Pb Hg K Ag Na Sn Element cuprum aurum plumbum hydrargyrum kalium argentums natrium stannum Compounds:-- * A substance that composed of atoms of two or more elements chemically united in fixed proportions. * Are separated only by chemical means Examples:>>> carbon tetrachloride CCl4 Sodium chloride NaCL calcium carbonate CaCO3 STATES OF MATTER:-- There are THREE states of matter>> solid , liquid , gas . Physical States :-Solid >> fixed volume & shap. Liquid >>- fixed volume. - shape of container, horizontal top surface. Gas>> takes shape and volume of container. liquid crystal>> some characteristics of solid and some of liquid states. Metals and Nonmetals:-Metals * Located to the left of the heavy line. * Shiny, ductile. * Good conductors of heat and electricity. Nonmetals *Located to the right of the heavy line. * Dull and brittle. * Poor conductors. ---------------------------------------------------------- Atomic Theory * Atoms are building blocks of elements. * Similar atoms in each element. * Different from atoms of other elements. * Two or more different atoms bond in simple ratios to form compounds. Subatomic Particles:-Particle Symbol Electron Proton Neutron ep+ n Charge -1 +1 0 Location of Subatomic Particles:-10 cm electrons protons neutrons nucleus 10 cm Atomic Number:-- Counts the number of Protons in an atom. Atomic Number on the Periodic Table Atomic Number Symbol 11 Na All atoms of an element have the same number of protons 11 protons Sodium 11 Na Learning Check State the number of protons for atoms of each of the following: A. Nitrogen ----> 1) 7 protons 2) 14 protons 3) 5 protons B. Sulfur ---- > 1) 16 protons 2) 6 protons 3) 32 protons C. Barium ---- > 1) 137 protons 2) 81 protons 3) 56 protons Mass Number:-- Counts the number of protons and neutrons in an atom. (A) mass number (Z) 23 Na atomic number 11 Number of Electrons:>>> * An atom is neutral. * The net charge is zero. * Number of protons = Number of electrons. * Atomic number = Number of electrons. * Mass number = Number of protons + Number of neutrons. Examples>> 65 Zn 30 31 16 P O 8 15 30 p+ 35 n 30 e- 15 p+ 16 n 15 e- 8 p+ 8n 8 e- Isotopes:-* Atoms with the same number of protons, but different numbers of neutrons. * Atoms of the same element (same atomic number) with different mass numbers. Example>>> Isotopes of chlorine 35 37 Cl 17 Cl 17 Learning Check 1/Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of these carbon atoms. 12 13 C C 6 #p ___6____ #n __6_____ #e __6_____ 14 C 6 6 ____6___ ___7____ ____6___ _____6__ ____8___ ____6___ ---------------------------------- 2/ An atom of zinc has a mass number of 65. (A): Number of protons in the zinc atom >> 1) 65 2) 35 3) 30 (B): Number of neutrons in the zinc atom >> 1) 65 2) 35 3) 30 (C): What is the mass number of a zinc isotope with 37 neutrons? 1) 67 2) 65 3) 37 ------------------------------------ 3/ Write the atomic symbols for atoms with the following: A. 8 p+, 8 n, 8 eB. 17p+, 20n, 17e- _________________ _________________ C. 47p+, 60 n, 47 e- _________________ -------------------------------------- Elements, Compounds, and Formulas:-- * Elements>>> can exist as single atoms or molecules. * Compounds>>> combination of two or more elements. * molecular formulas for molecular compound. *empirical formulas for ionic compounds. Bulk Substances * mainly ionic compounds - empirical formulas -structural formulas Charge on Ions *compounds have electrical neutrality. *metals form positive monatomic ions. *non-metals form negative monatomic ions. Naming Binary Compounds Common Compound:--s H2O>>water NH3>>ammonia N2O>>nitrous oxide CO>>carbon monoxide CS2>>carbon disulfide SO3>>sulfur trioxide CCl4>>carbon tetrachloride PCl5>>phosphor pentachloride SF6>>sulfur hexafluoride Polyatomic Ions:-Ammonium>NH4+ Perchlorate>ClO4Cyanide>CNhydroxid OHNitrate>NO3Nitrite>NO2Nitride>N3- Binary Ionic Compounds:-*Contain 2 different elements *Name the metal first, then the nonmetal as -ide. *Use name of a metal with a fixed charge Groups 1A, 2A, 3A and Ag, Zn,cl Examples: sodium chlorid NaCl zinc iodide ZnI2 aluminumoxide Al2O3 Learning Check N1 Complete the names of the following binary compounds: 1/ Na3N sodium ______________. 2/ KBr potassium ____________. 3/ Al2O3 aluminum _____________. 4/ MgS ______________________. Sulfate>SO42Carbonate>CO32Phosphate>PO43Floride>FChloride>ClBromide>BrIodide>I- Names of Variable Ions:-Use a roman number after the name of a metal that forms two or more ions Transition metals and the metals in groups 4A and 5A.. Examples>> FeCl3 (Fe3+) iron (III) chloride CuCl (Cu+ ) copper (I) chloride PbCl2 (Pb2+) lead (II) chloride SnF4 (Sn4+) tin (IV) fluoride Learning Check N2 Name the following compounds: A. CaO>> B. SnCl4>> 1) calcium oxide . 3) calcium (II) oxide. 2) calcium(I) oxide. 1) tin tetrachloride. 3) tin(IV) chloride. 2) tin(II) chloride. C. Co2O3 >> 1) cobalt oxide. 3) cobalt trioxide. 2) cobalt (III) oxide. Learning Check N3 Complete the names of the following binary compounds with variable metal ions: FeBr2 Cu2O SnCl4 Fe2O3 CuS iron (_____) bromide. copper (_____) oxide. ___(_____ ) ______________ ________________________ ________________________ Naming Binary Covalent Compounds:-Two nonmetals *Name each element *End the last element in -ide *Add prefixes to show more than 1 atom Prefixes Mon >>> 1 Tetra >>> 4 Di >>> 2 penta >>> 5 Tri >>> 3 hexa >>> 6 Learning Check N4 CO carbon ______oxide. CO2 carbon _______________ PCl3 phosphorus _______chloride CCl4 carbon ________chloride. N2O _____nitrogen _____oxide. Learning Check N5 A/ P2O5 1) phosphorus oxide 2) phosphorus pentoxide 3) diphosphorus pentoxide B/ Cl2O7 1) dichlorine heptoxide 2) dichlorine oxide 3) chlorine heptoxide C/ Cl2 1) chlorine 2) dichlorine 3) dichloride --------------------------------------------------------. تمنياتي لكم بالتوفيق والنجاح 10 -13 c m el ec tr on s Valence of Metal Ions Monatomic Ions => +1 Group IA => +2 Group IIA Maximum positive valence equals Group A # Valence of Non-Metal Ions Monatomic Ions => -2 Group VIA => -1 Group VIIA Maximum negative valence equals (8 - Group A #)