"Chemistry 11Sci Notes" Essays and Research Papers

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Chemistry 11Sci Notes

Chemistry 200 Exam 1 Review Problems 1. Calculate the number of atoms in 10.0 grams of Fe. 2. Give the mass number, #protons, #neutrons and #electrons for the isotope strontium-88. 3. Calculate the number of moles of carbon in 50.0 g of benzene C6H6 4. A substance is found to be 38.7 % C, 9.7 % H and 51.6 % O by mass. Its molar mass is 62.1 g/mole. What is its molecular formula? 5. Name the following: a) Ca(OH)2 b) KCN c) HClO4(aq) d) FeSO4 e) Na2O f) SF6 g)...

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Chemistry Notes

Chemistry Unit 2 Area of Study: 1: Water Chapter 11: Measuring solubility Measuring Solubility Solubility: the maximum amount of that substance that can be dissolved in a that temperature Saturated solution: a solution which no more solute can be dissolved at that temperature Measuring solubility Determine the maximum mass of solute that can be dissolved in 100 grams of solvent at a particular temperature Worked Example A maximum of a 6g of solute can be dissolved in 20g of water at 20ºC...

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As Chemistry Notes

Topic 5 – Bonding and Structure Revision Notes 1) Introduction • Atoms form bonds to get a full outer shell of electrons • There are three types of bonding: ionic, covalent and metallic • The structures produced by forming bonds are either giant or simple • The possible combinations of structure and bonding are giant ionic, simple covalent, giant covalent and giant metallic • Simple covalent is sometimes called simple molecular • Giant covalent is sometimes called giant...

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4.02 Chemistry Notes

4.02 chemistry notes Law of Conservation of Mass One of the most important principles of chemistry is the law of conservation of mass. This law states that matter is neither created nor destroyed during an ordinary chemical reaction. In other words, all of the atoms that were present at the beginning of a reaction are present at the end of the reaction—they have just been rearranged to bond differently and form new substances. It is important that chemical equations represent this law by always...

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Electro Chemistry Study Notes

Chemistry Exam Revision - Redox & Electrochemical Series - Define oxidation and reduction in term of loss and gain of oxygen; loss and gain of electrons and change in oxidation state (number). • Oxidation is the loss of electrons; an increase in oxidation state or a gain in oxygen by a molecule, atom, or ion. • Reduction is the gain of electrons; a decrease in oxidation state or a loss of oxygen by a molecule, atom, or ion. • OIL RIG (Oxidation is Loss, Reduction is Gain) - Rules for assigning...

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Inorganic Chemistry Notes Ch2

Aufbau principle Cr: [Ar] 4s1 3d5 Many times, half-filled and completely filled orbitals are unusually stable, so sigma electrons can rarely end up promoted to pi electrons Types of electrons Valence: outer electrons responsible for chemistry Transition metals: Any unfilled (n-1)d electrons are counted as valence Inner/core: Effective Nuclear charge Zeff: nuclear charge that affects an electron Attraction to nucleus an electron feels Increased by large nuclear...

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chemistry 2ab notes

Chemistry Notes: Metals: • A metal consists of a lattice of positive ions surrounded by a ‘sea’ of mobile delocalised valence electrons. • Metallic bonding is the electrostatic attraction between the delocalised electrons and the positive ions in the metallic lattice. Properties of metals: Property Explanation Relatively high density The particles are very close together. This is because of high electrostatic forces between the sea of valence electrons and the positively charged nucleus. ...

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Science Chemistry Notes

filtering the sand and salt solution. The salt solution passed through the filter and the insoluble sand stays behind in the filter paper. Pure salt can then be recovered by evaporating the water from the salt solution. Web Link: Doc Brown’s Chemistry Clinic; http://www.wpbschoolhouse.btinternet.co.uk/page01/ElCpdMix/EleCmdMix.htm [pic] Examples of some compounds: |Cartoon picture |Chemical compound |Elements present |Number of...

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Chemistry Gen: Course Description Year 2 PART - II CGT 21a Unit I. Basic physical chemistry I * Gaseous state: Gas laws, kinetic theory of gas, collision and gas pressure derivation of gas laws from kinetic theory, average kinetic energy of translation. Boltzmann constant and absolute scale of temperature, Maxwell's distribution law of molecular speeds (without derivation), most probable, average and root mean square speed of gas molecules, principle of equipartition of energy (without...

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AP Chemistry Notes

Unit 8 Textbook Notes 12.1 The N2O4-NO2 Equilibrium System When you put a sample of N2O4, a colorless gas, in a closed container at 100C a reddish-brown color starts to show. This is due to NO2 formed by the decomp. of part of the original substance. The forward and reverse reactions are taking place at the same rate. The concentrations of species present remain constant with time. These concentrations are independent of the direction from which equilibrium is approached. The equilibrium constant...

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