![Chemistry](http://s1.studyres.com/store/data/004508888_1-6f1c472d28342b20db537a3259363a50-300x300.png)
Chemistry
... ketones, reduction of carboxylic acids and using Grignard reagent- general reactions and examples (R as H, CH3 and C2H5 wherever applicable. Preparation of phenol: From i) benzene via sulphonation ii) diazonium salt iii) cumene. Physical properties of primary alcohols and phenol: Boiling point and s ...
... ketones, reduction of carboxylic acids and using Grignard reagent- general reactions and examples (R as H, CH3 and C2H5 wherever applicable. Preparation of phenol: From i) benzene via sulphonation ii) diazonium salt iii) cumene. Physical properties of primary alcohols and phenol: Boiling point and s ...
Chapter 3 - Significant Figures - Scientific Measurement
... Our test is also different than the other tests. There are basically two parts: Multiple Choice (60 questions – 90 minutes) and Free Response (4 short questions and 3 long questions – 90 minutes). There is no penalty for guessing on the multiple choice questions. Something different though exists fo ...
... Our test is also different than the other tests. There are basically two parts: Multiple Choice (60 questions – 90 minutes) and Free Response (4 short questions and 3 long questions – 90 minutes). There is no penalty for guessing on the multiple choice questions. Something different though exists fo ...
Chapter 6
... • Note that temperature is different from heat, though the two concepts are linked. Temperature is a measure of the internal energy of the system, while heat is a measure of how energy is transferred from one system (or body) to another. The greater the heat absorbed by a material, the more rapidly ...
... • Note that temperature is different from heat, though the two concepts are linked. Temperature is a measure of the internal energy of the system, while heat is a measure of how energy is transferred from one system (or body) to another. The greater the heat absorbed by a material, the more rapidly ...
chapter 4 lecture slides
... 4. The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds (e.g. LiH, CaH2). In these cases, its oxidation number is –1. 5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1. 6. The sum of the oxidation numbers of all the atoms in a molecule o ...
... 4. The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds (e.g. LiH, CaH2). In these cases, its oxidation number is –1. 5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1. 6. The sum of the oxidation numbers of all the atoms in a molecule o ...
Column A
... J) Draw the electron dot diagram (Lewis Dot Structure) and then tell if it would give up or take on electrons to get a full shell. Also tell what charge it would have (positive or negative and how much ex: +2) ...
... J) Draw the electron dot diagram (Lewis Dot Structure) and then tell if it would give up or take on electrons to get a full shell. Also tell what charge it would have (positive or negative and how much ex: +2) ...
CH 2 development of atomic theory
... When we work with a small group of atoms, we use the unit amu–atomic mass unit. This is a very small amount and not very practical when working n the lab. We want a value that is tangible, and based on the gram. For larger amounts of matter, we use the molar mass, which is related to a larger counti ...
... When we work with a small group of atoms, we use the unit amu–atomic mass unit. This is a very small amount and not very practical when working n the lab. We want a value that is tangible, and based on the gram. For larger amounts of matter, we use the molar mass, which is related to a larger counti ...
C1 – Topic 2 notes - ARK Elvin Academy
... Note that state symbols are added to each substance: o s – solid o g – gas o l – pure liquid (e.g water) o aq – aqueous solution…formed when substances dissolve in water (e.g sodium hydroxide) Mass is conserved in chemical reactions: Atoms are NOT made or destroyed in a chemical reaction. They are o ...
... Note that state symbols are added to each substance: o s – solid o g – gas o l – pure liquid (e.g water) o aq – aqueous solution…formed when substances dissolve in water (e.g sodium hydroxide) Mass is conserved in chemical reactions: Atoms are NOT made or destroyed in a chemical reaction. They are o ...
Topic 2 notes - WordPress.com
... Note that state symbols are added to each substance: o s – solid o g – gas o l – pure liquid (e.g water) o aq – aqueous solution…formed when substances dissolve in water (e.g sodium hydroxide) Mass is conserved in chemical reactions: Atoms are NOT made or destroyed in a chemical reaction. They are o ...
... Note that state symbols are added to each substance: o s – solid o g – gas o l – pure liquid (e.g water) o aq – aqueous solution…formed when substances dissolve in water (e.g sodium hydroxide) Mass is conserved in chemical reactions: Atoms are NOT made or destroyed in a chemical reaction. They are o ...
CHEE 221: Chemical Processes and Systems
... 1. Material balances – for a nonreactive process, usually but not always, the maximum number of independent equations that can be written equals the number of chemical species in the process 2. Process constraints– given in the problem statement 3. Physical constraints – e.g., mass or mole fractio ...
... 1. Material balances – for a nonreactive process, usually but not always, the maximum number of independent equations that can be written equals the number of chemical species in the process 2. Process constraints– given in the problem statement 3. Physical constraints – e.g., mass or mole fractio ...
UNIT 2 ATOMS, MATTER, AND THE MOLE
... 1. EX: water has the formula H2O, which means for one atom of oxygen there are two atoms of hydrogen. 2. H2O2 is not water. It is called hydrogen peroxide, has two atoms of hydrogen for every two atoms of oxygen and behaves much differently that water. This brings us to the next law. F. LAW OF MULTI ...
... 1. EX: water has the formula H2O, which means for one atom of oxygen there are two atoms of hydrogen. 2. H2O2 is not water. It is called hydrogen peroxide, has two atoms of hydrogen for every two atoms of oxygen and behaves much differently that water. This brings us to the next law. F. LAW OF MULTI ...
Chem 101 Test #1 review questions. Please don`t look at the
... So X = mass of stribnite – mass of S = .37398 -0.14595 = 0.22803 g X To get molar mass of X first, get moles X: # moles of X = (1.52 x10-3 moles X2S3 )(2 mol/1 mol X2S3) = 0.00304 moles X Therefore: molar mass = mass of X/moles of X = 0. 22803 g X /0.00304 moles X = 75.0101g/mol Check the periodic t ...
... So X = mass of stribnite – mass of S = .37398 -0.14595 = 0.22803 g X To get molar mass of X first, get moles X: # moles of X = (1.52 x10-3 moles X2S3 )(2 mol/1 mol X2S3) = 0.00304 moles X Therefore: molar mass = mass of X/moles of X = 0. 22803 g X /0.00304 moles X = 75.0101g/mol Check the periodic t ...
vce chemistry trial exam 1
... C is correct. HPLC allows the separation of organic compounds such as esters. NMR spectroscopy allows the estimation of the structure of organic compounds based on their 13C and 1H spectra. A is incorrect because neither UV-visible spectroscopy nor NMR spectroscopy allow the separation of compounds. ...
... C is correct. HPLC allows the separation of organic compounds such as esters. NMR spectroscopy allows the estimation of the structure of organic compounds based on their 13C and 1H spectra. A is incorrect because neither UV-visible spectroscopy nor NMR spectroscopy allow the separation of compounds. ...
Topic 1: Quantitative chemistry (12
... Deduce which ions will be formed when elements in groups 1, 2 and 3 lose electrons. Deduce which ions will be formed when elements in groups 5, 6 and 7 gain electrons. State that transition elements can form more than one ion. Examples such as Fe 2+ and Fe 3+. Predict whether a compound of two eleme ...
... Deduce which ions will be formed when elements in groups 1, 2 and 3 lose electrons. Deduce which ions will be formed when elements in groups 5, 6 and 7 gain electrons. State that transition elements can form more than one ion. Examples such as Fe 2+ and Fe 3+. Predict whether a compound of two eleme ...
Atoms, Molecules, and Ions
... Syracuse University’s Academic Integrity Policy reflects the high value that we, as a university community, place on honesty in academic work. The policy defines our expectations for academic honesty and holds students accountable for the integrity of all work they submit. Students should understand ...
... Syracuse University’s Academic Integrity Policy reflects the high value that we, as a university community, place on honesty in academic work. The policy defines our expectations for academic honesty and holds students accountable for the integrity of all work they submit. Students should understand ...
Practice Test: Equilibrium
... 8. What will happen to Keq if the temperature is lowered? ____________ 9. In summary, what is the only thing that will change the equilibrium constant? _____________________________ Which way would the equilibrium shift (right or left) if the following changes are made to the equilibrium: ...
... 8. What will happen to Keq if the temperature is lowered? ____________ 9. In summary, what is the only thing that will change the equilibrium constant? _____________________________ Which way would the equilibrium shift (right or left) if the following changes are made to the equilibrium: ...
Fundamentals
... held in hand-and the atomistic view is a quantity called the mole. A mole, abbreviated mol, contains 6.022137 X 1023particles, a number referred to as Avogadro's number (NA) in recognition of the importance of Avogadro's hypothesis to the development of chemistry. Perhaps 6.022137 X 1023particles pe ...
... held in hand-and the atomistic view is a quantity called the mole. A mole, abbreviated mol, contains 6.022137 X 1023particles, a number referred to as Avogadro's number (NA) in recognition of the importance of Avogadro's hypothesis to the development of chemistry. Perhaps 6.022137 X 1023particles pe ...
Chapter 6: Moles, Molar Mass, Percent Composition and Formulas
... ii) It’s impossible to count atoms with your hands. iii) Numbers of moles are smaller and easier to do math with than big numbers of atoms and molecules. 6) Convert moles of an atom to grams a) I need 2.0 moles of copper (Cu) for an experiment. How many grams is that? b) Atomic mass of Cu = 63.55 g/ ...
... ii) It’s impossible to count atoms with your hands. iii) Numbers of moles are smaller and easier to do math with than big numbers of atoms and molecules. 6) Convert moles of an atom to grams a) I need 2.0 moles of copper (Cu) for an experiment. How many grams is that? b) Atomic mass of Cu = 63.55 g/ ...
PHYSICAL PROPERTIES - can observe w/o changing the
... atomic level. Can’t be reversed with a physical change. Examples: burning, dissolving something in an acid, letting iron rust, letting silver tarnish, mixing vinegar and baking soda, cooking an egg Also called a CHEMICAL REACTION (5 signs to watch for) formation of an odor, change in temp, formation ...
... atomic level. Can’t be reversed with a physical change. Examples: burning, dissolving something in an acid, letting iron rust, letting silver tarnish, mixing vinegar and baking soda, cooking an egg Also called a CHEMICAL REACTION (5 signs to watch for) formation of an odor, change in temp, formation ...
Intro to Chem
... ◦ Physical methods that are used to separate mixtures cannot be used to break a compound into simpler substances. ◦ Chemical change is a change that produces matter with a different composition than the orginal matter. Sugar broken down into C and H2O(g) when heated. Broken down into H2 and O2 b ...
... ◦ Physical methods that are used to separate mixtures cannot be used to break a compound into simpler substances. ◦ Chemical change is a change that produces matter with a different composition than the orginal matter. Sugar broken down into C and H2O(g) when heated. Broken down into H2 and O2 b ...
I. Properties of Matter
... what is the percent by mass of each of the elements in the compound? ...
... what is the percent by mass of each of the elements in the compound? ...
Stoichiometry
![](https://commons.wikimedia.org/wiki/Special:FilePath/Combustion_reaction_of_methane.jpg?width=300)
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.