Moles
Subject:
1 mole = 6.022x10^23 amy
Chemistry
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Book page:
http://course-notes.org/Chemistry
Definition of an Element
Subject:
Tags:
Elements
Any substance that contains only one kind of an atom is known as an element. Because atoms cannot be created or destroyed in a chemical reaction, elements such as phosphorus (P4) or sulfur (S8) cannot be broken down into simpler substances by these reactions.
Example: Water decomposes into a mixture of hydrogen and oxygen when an electric current is passed through the liquid. Hydrogen and oxygen, on the other hand, cannot be decomposed into simpler substances. They are therefore the elementary, or simplest, chemical substances - elements.
Each element is represented by a unique symbol. The notation for each element can be found on the periodic table of elements.
Definition of an Element
Subject:
Tags:
Elements
Any substance that contains only one kind of an atom is known as an element. Because atoms cannot be created or destroyed in a chemical reaction, elements such as phosphorus (P4) or sulfur (S8) cannot be broken down into simpler substances by these reactions.
Example: Water decomposes into a mixture of hydrogen and oxygen when an electric current is passed through the liquid. Hydrogen and oxygen, on the other hand, cannot be decomposed into simpler substances. They are therefore the elementary, or simplest, chemical substances - elements.
Each element is represented by a unique symbol. The notation for each element can be found on the periodic table of elements.
Definition of an Element
Subject:
Tags:
Elements
Any substance that contains only one kind of an atom is known as an element. Because atoms cannot be created or destroyed in a chemical reaction, elements such as phosphorus (P4) or sulfur (S8) cannot be broken down into simpler substances by these reactions.
Example: Water decomposes into a mixture of hydrogen and oxygen when an electric current is passed through the liquid. Hydrogen and oxygen, on the other hand, cannot be decomposed into simpler substances. They are therefore the elementary, or simplest, chemical substances - elements.
Each element is represented by a unique symbol. The notation for each element can be found on the periodic table of elements.
Rate Law
Subject:
Tags:
Rate Law, Reaction Order ?? factors affecting reaction rates?- chemical kinetics?- study of reaction speed physical state of reactants - more collisions >> faster reaction solid surface area increase >> reaction rate increase reactant concentration - higher concentration >> faster reaction temperature - higher temperature >> higher kinetic molecular energy >> more collisions >> faster reaction catalyst - substances that increase reaction rate w/o being used up collisions must include enough energy and correct positioning to lead to reaction average rate = change in concentration / change in time instantaneous rate?- rate at a specific moment in reaction rates tend to decrease as reaction continues initial rate - reaction rate when reaction first begins
Chapter 1 notes 1.4-1.9
Subject:
Chem AP Chapter 1 Notes 1.4 ? UNCERTAINTY IN MEASUREMENT Certain digits: numbers that remain regardless of who makes the measurements. Uncertain digits: digits that must be estimated. *Measurements always have a value of uncertainty. *Measurements depend on the precision of the equipment being used. *Always record numbers using sig figs. 25 = between 24 and 16 25.00 = between 24.99 and 25.01 Accuracy: refers to the agreement of a particular value with the true value. Precision: refers to the degree of agreement among several measurements of the same quantity. It reflects the reproducibility of a given type of measurement.
gen chem practice exam 2
Subject:
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gen chem practice exam 3
Subject:
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Chemistry 2
Subject:
The intermolecular forces can affect phase changes to a great degree. The stronger the intermolecular
forces present in a liquid, the more kinetic energy must be added to convert it into a gas.
Conversely, the stronger the intermolecular forces between the gas particles, the easier it will be
to condense the gas into a liquid. In general, the weaker the intermolecular forces, the higher the
vapor pressure. The same type of reasoning can be used about the other phase equilibria, in general,
the stronger the intermolecular forces, the higher the heats of transition.
Chemistry
Subject:
Note that the diagram has three general areas corresponding to the three states of
matter––solid, liquid, and gas. The line from A to C represents the solid’s change in vapor
pressure with changing temperature, for the sublimation equilibrium. The A-to-D line represents
the variation in the melting point with varying pressure. The A-to-B line represents
the variation of a liquid’s vapor pressure with varying pressure. The B point shown on this
phase diagram is called the critical point of the substance, the point beyond which the gas
and liquid phases are indistinguishable from each other. At or beyond this critical point, no
matter how much pressure is applied, the gas cannot be condensed into a liquid. Point A is
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