11/10/2019 Introductory Chemistry Labs Highschool
Chemistry Lab WorksheetsChemistry is the study of matter. We look at the phases of matter and theinteracts between matter. This set of printable chemistry labs has the perfectbalance between fun and learning.
Student will really love it. Every labhas been kid and teacher tested and approved. Students observe the cooling rate of water.
A neat pH lab! We look at acids and bases in a funexperiment. Students perform chemical tests to learnwhat foods contain carbohydrates, lipids, and/or proteins.
Students will learn how soap, alcohol, andtemperature differences affect the dissolution speed of water. Students are assigned an element andmust promote it in a contest like environment. Have your classes make an atom. Put them all overthe classroom ceiling and make your own periodic table. Students make a warm air balloons to investigate gaslaws.
This station lab, examines chemical and physicalchanges. Examines endothermic versus exothermic reactions.
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Free High School Chemistry Labs & Lessons!.Free Chemistry Labs - Download pdf and/or MS Word docs with instructions on lab activities that include experiments with gum, balloons, snow globes, paper planes, onion DNA, pennies, and more. Teach Yourself Chemistry Visually in 24 Hours - by Dr. Wayne Huang and his team. The series includes High School Chemistry, AP Chemistry, General Chemistry, Organic Chemistry and Biochemistry. Master Chemistry The Easy and Rapid Way with Core Concept Tutorials, Problem-Solving Drills and Super Review Cheat Sheets.
Chemical Bonding BasicsIn bonding, atoms lose, gain, or share electrons in order to have the same number of electrons as the noble gas that’s nearest on the periodic table. Ionic, covalent, and metallic bonds are formed by combinations of metals and nonmetals.Metal + nonmetal = ionic bond.Nonmetal + nonmetal = covalent bond.Metal + metal = metallic bondWhen two elements engage in ionic bonding, one or more electrons are transferred from the metal to the nonmetal, forming ions (charged atoms). The metal, having lost one or more electrons, forms a cation, an ion with a positive charge; the nonmetal, having gained one or more electrons, becomes an anion, an ion with a negative charge. Chemistry Concepts: Energy Levels and OrbitalsA lot of chemistry is explained by the sharing and trading of electrons between atoms. Understanding how electrons are arranged in an atom is a building block of Chem I.Electrons in an atom are contained in specific energy levels (1, 2, 3, and so on) that are different distances from the nucleus. The larger the number of the energy level, the farther it is from the nucleus.
Electrons that are in the highest energy level are called valence electrons. Within each energy level is a volume of space where specific electrons are likely to be located. These spaces, called orbitals, are of different shapes, denoted by a letter (s, p, d, f, g).
(In most cases, only the electrons contained in the s and p orbitals are considered valence electrons.) Electrons seek the lowest energy level possible.The following electron-filling pattern indicates how the electrons fill into the energy levels. Knowing this pattern is useful in many aspects of chemistry, including predicting the bonding situation of a particular atom and in the prediction of the geometry of a covalent compound.Electron filling pattern: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f. Digging the Mole Concept in ChemistryThe mole (abbreviate mol and sometimes called Avogadro ‘ s number) is a conversion number that allows a chemist or chemistry student to move from the microscopic world of atoms, ions, and molecules to the macroscopic world of grams, kilograms, and tons.
The mole is used in reaction stoichiometry to predict how much product can be made from a certain amount of reactant or how much reactant is required to produce a certain amount of product.If you know the particles, moles, or grams of a substance, you can calculate the other two measurements by using the following equation:1 mole = 6.022 × 10 23 particles/mol = formula weight expressed in grams. The Basic Chemistry of Acids and BasesA lot of chemistry requires you to understand the difference between acids and bases. An acid is a substance that donates an H + ion to another chemical species called a base. A base is a substance that accepts (combines with) an H + ion.If you need to know the concentration of the H + ion in solution, you can do so by representing the H + molarity, H +. Another way to represent the H + concentration is the pH, which is the negative logarithm of the H + molarity. The following equation shows this mathematical relationship as well as the way to calculate the H + molarity given the pH:pH = –logH +; H + = 10 –pH.pH = 7 is neutral.pH less than 7 is acidic.pH greater than 7 is basic.
The Combined Gas Law and Ideal Gas LawWhen studying the properties of gases, you need to know the relationships between the variables of volume (V), pressure (P), Kelvin temperature (T), and the amount in moles (n) so that you can calculate missing information ( P, V, T, or n) and solve reaction stoichiometry problems. Although the pairs of variables have individual relationships, the two most important and useful gas laws are the combined gas law and the ideal gas law: Combined gas law( P 1 V 1)/ T 1=( P 2 V 2)/ T 2( T must be in Kelvin)Ideal gas lawPV = nR T(R = 0.0821 L atm/K.mol).
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