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Chemistry Final Exam Review: Key Concepts and Definitions, Exams of Physics

Harrisburg Area Community College (HACC) - LancasterPhysics

A comprehensive review of key concepts and definitions for a chemistry final exam. It covers a wide range of topics, including chemical bonding, states of matter, chemical reactions, and stoichiometry. Organized in a clear and concise manner, making it easy to understand and study. It is a valuable resource for students preparing for their final exam in chemistry.

Typology: Exams

2024/2025

Available from 10/31/2024

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Chemistry Final, Chemistry Final Exam
1.Independent variable: The variable that you manipulate in an
experiment
2.Dependent variable: The variable that you are measuring to see how it
changes in an experiment
3.Qualitative data: Data that has no number and just describes a
characteristic
4.Quantitative data: Data with numerical value
5.Mole: Unit of measurement that contains 6.02 E 23 atoms,
molecules, or other items
6.Density: Mass / volume
7.Solid: A form of matter with a constant volume and unchanging shape
8.Liquid: A form of matter with a constant volume which takes the
shape of its container
9.Gas: A form of matter that changes shape and volume to fill its
container
10.Polar covalent bond: A bond with an unequal distribution of shared
electrons
11.Law of Conservation of Mass: Mass is neither created nor
destroyed, only converted--the reason that we balance chemical
equations
12.Physical change: Changes the appearance of something. Ex: boiling,
smash- ing, freezing, chopping
13.Chemical change: Changes the chemical composition of something.
Ex: wood burning, milk spoiling
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Download Chemistry Final Exam Review: Key Concepts and Definitions and more Exams Physics in PDF only on Docsity!

Chemistry Final, Chemistry Final Exam

  1. Independent variable: The variable that you manipulate in an experiment
  2. Dependent variable: The variable that you are measuring to see how it changes in an experiment
  3. Qualitative data: Data that has no number and just describes a characteristic
  4. Quantitative data: Data with numerical value
  5. Mole: Unit of measurement that contains 6.02 E 23 atoms, molecules, or other items
  6. Density: Mass / volume
  7. Solid: A form of matter with a constant volume and unchanging shape
  8. Liquid: A form of matter with a constant volume which takes the shape of its container
  9. Gas: A form of matter that changes shape and volume to fill its container
  10. Polar covalent bond: A bond with an unequal distribution of shared electrons
  11. Law of Conservation of Mass: Mass is neither created nor destroyed, only converted--the reason that we balance chemical equations
  12. Physical change: Changes the appearance of something. Ex: boiling, smash- ing, freezing, chopping
  13. Chemical change: Changes the chemical composition of something. Ex: wood burning, milk spoiling
  1. Distillation: Separating a mixture by heating it to the boiling points of its com- ponents
  2. Chromatography: Separating a mixture by dissolving it in a mobile phase
  3. Atom: The smallest particle of an element that retains the properties of that element
  4. Heisenberg uncertainty principle: It is impossible to know both the velocity and the position of a particle at the same time
  5. Atomic orbital: A three-dimensional region around the nucleus of an atom that describes an electron's probable location in the electron cloud model
  6. Alkali metals: Group IA on the periodic table
  7. Alkaline earth metals: Group IIA on the periodic table
  8. Halogens: Group VIIA on the periodic table
  9. Noble gasses: Group VIIIA on the periodic table
  10. Ion: A particle with a positive or negative charge
  11. Ionic bond: Bond caused by the transfer of electrons
  12. Covalent bond: Bond caused by the sharing of electrons
  13. Precipitate: A solid produced in a chemical reaction in solution
  14. Physical property: A property that can be observed with the five senses without changing the substance. Ex: color, melting point, conductivity

into mul- tiple products

  1. Single Replacement reaction: The homewrecker reaction in which one ele- ment reacts with one compound
  2. Double replacement reaction: The switching reaction in which two compounds react with each other
  3. Combustion reaction: A reaction in which something with carbon and hydrogen reacts with oxygen to form carbon dioxide and water
  4. Empirical formula: The simplified formula, found with percent by mass
  5. Molecular formula: The true formula of a compound, found with empirical formula and molar mass
  6. Molarity: moles of solute / liters of solution
  7. mass number: number of neutrons and protons in nucleus
  8. atomic number: number of protons in nucleus
  9. average atomic mass: weighted average of all of the isotope's mass numbers found in nature
  1. valence electrons: electrons in the outermost shell (can be easily shared, gained or lost)
  2. core electrons: electrons in the inner shell 54. lewis Structures:
  3. Nobel Gas Notation: shortcut’ find the closest noble gas (column 18) with fewer electrons than the element then finish electron configuration
  4. transition elements: What are the elements in groups 3-12 called?
  5. electronegativity: A measure of the ability of an atom in a chemical compound to attract electrons
  6. dipole-dipole attraction: attractive force resulting when polar molecules line up so that the positive and negative ends are close to each other
  7. hydrogen bond: A strong attractive force formed between polar molecules when a hydrogen atom is covalently bound to a nitrogen, fluorine, or oxygen atom
  8. London dispersion forces: The intermolecular attractions resulting from the constant motion of electrons and the creation of temporary dipoles
  9. resonance structure: a structure that occurs when it is possible to
  1. reactants: a substance that takes part in and undergoes change during a reaction
  2. Boyle's Law: there is a inverse relationship between pressure and volume
  3. Charles's Law: there is a direct relationship between temperature and volume
  4. Ideal Gas law: PV = n R T
  5. Kinetic-Molecular Theory: a theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system
  6. standard pressure: 1 atm
  7. standard temperature: 273 K.
  8. concentration: A measurement of how much solute exists within a certain volume of solvent
  9. dilute: to lessen the concentration, force, or purity of by adding something
  10. endothermic: A chemical reaction that absorbs energy (heat)
  11. exothermic: A chemical reaction that releases energy (heat)
  12. molarity: A common measure of solute concentration, referring to the number of moles of solute per liter of solution.
  13. polarity: unequal sharing of electrons
  14. solute: A substance that is dissolved in a solution.
  15. solvent: A liquid substance capable of dissolving other substances
  16. sublimation: A change directly from the solid to the gaseous state without becoming liquid
  1. acid: a substance that produces hydrogen ions in a water solution
  2. base: a substance that produces hydroxide ions (OH-) when dissolved in water
  3. conjugate acid: the particle formed when a base gains a hydrogen ion
  4. conjugate base: particle that remains when an acid has donated a hydrogen ion
  5. indicator: A compound that changes color in the presence of an acid or a base
  6. neutralization: A reaction of an acid with a base, yielding a solution that is not as acidic or basic as the starting solutions were.
  7. pH: a numeric scale used to specify the acidity or basicity of an aqueous solution
  8. anions: Negatively charged ions
  9. cations: Positively charged ions
  10. combustion: A rapid reaction between oxygen and fuel that results in fire
  11. metaloid: Demonstrate properties of both metals and nonmetals. Examples are silicon and arsenic.
  12. Heisenberg uncertainty principle: it is impossible to know exactly both the velocity and the position of a particle at the same time
  13. precipitate: A solid that forms from a solution during a chemical reaction.