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Chemistry final
| Question | Answer |
|---|---|
| Alchemy | A historical pursuit that combined chemistry, metallurgy, physics, medicine, astrology, mysticism, and art, which helped develop fundamental tools and techniques for working with chemicals. |
| Practical & mystical | Alchemy was a practice that had both practical applications (developing techniques) and mystical goals (like the search for the philosopher's stone or eternal life). |
| Practiced in China and India | Practiced as early as 400 BC/BCE in ancient China and India. |
| Arabs brought to Spain | The practice was later adopted by Arab scholars who preserved and expanded upon the knowledge, eventually bringing it to Spain and then throughout Europe during the Middle Ages. |
| Properties of Matter | Characteristics used to describe and distinguish between different substances. |
| Extensive Property | A property that depends on the amount of matter in a sample. |
| Examples of Extensive Properties | Volume, mass, length, shape. |
| Intensive Property | A property that depends only on the type of matter (the substance's composition) in a sample, not the amount. |
| Examples of Intensive Properties | Density, viscosity, luster, color, melting point, boiling point, conductivity, malleability, brittleness. |
| Physical Property | A quality or condition of a substance that can be observed or measured without changing the substance’s chemical composition. |
| Examples of Physical Properties | State of matter (solid, liquid, gas), color, melting point, boiling point, hardness, odor, density. |
| Chemical Property | The potential or ability of a substance to undergo a specific chemical change or reaction (change in composition). |
| Examples of Chemical Properties | Flammability, corrosive (reactivity with acids/bases), reactivity with water/air/oxygen, pH (potential to be an acid or base). |
| Solid | A form of matter that has a definite shape and a definite volume. Particles are packed tightly together in a fixed, often orderly, arrangement and vibrate in place with low kinetic energy. |
| Liquid | Has no definite shape but a definite volume. Particles are close in contact with each other but are in a mobile, random arrangement. They slide around each other, are not easily compressed, and typically expand when heated, higher energy than solids. |
| Plasma | referred to as the fourth state of matter, has no fixed shape or volume. It is an ionized gas consisting of a collection of charged particles. It is less dense than solids or liquids and is found in stars, lightning, and fluorescent lights. |
| Bose-Einstein Condensate (BEC) | A state of matter that exists only at temperatures just a little above absolute zero. A large fraction of the atoms occupies the same,lowest,energy quantum state,or wave of matter. It was predicted by Einstein and Bose and first observed in a lab in 1995. |
| Physical Change | A change during which some properties of a material might change (e.g., shape, state), but the chemical composition and identity of the substance remain the same. |
| Examples of Physical Changes | Melting, freezing, boiling, cutting, folding, crushing, dissolving salt in water. |
| Chemical Change | A change that produces matter with a different chemical composition and different properties than the original matter. New substances are formed. |
| Examples of Chemical Changes | Rotting, rusting, combusting (burning), cooking, oxidation, electrolysis, producing gas bubbles (effervescence), a permanent color change, a temperature change (not from heating/cooling). |
| Matter | Anything that has mass and takes up space (volume). |
| Mixture | A physical blend of two or more substances (elements or compounds) that are not chemically combined. |
| Homogeneous Mixture (Solution) | A mixture in which the composition IS uniform throughout the mixture. Components are evenly distributed and a single phase is visible. |
| Examples of Homogeneous Mixtures | Air, saline solution (saltwater), metal alloys (like brass or steel), vinegar. |
| Heterogeneous Mixture | A mixture in which the composition IS NOT uniform throughout the mixture. Components are not evenly distributed, and you can usually see separate parts or phases. |
| Examples of Heterogeneous Mixtures | Soup, salad, chocolate chip cookies, sand and gravel, ice and water (if viewed closely, the ice is a solid phase and water is a liquid phase). |
| Phase | Used to describe any part of a sample with uniform composition and properties. |
| Substance vs. Mixture Rule | If the composition of a material is FIXED and definite, the material is a pure substance (element or compound); if the composition of a material varies, it is a mixture. |
| Separation Methods | We use the difference in physical properties of the components to separate mixtures. |
| Filtration | The process that separates a solid from a liquid in a heterogeneous mixture by passing the liquid through a porous barrier (like filter paper). |
| Distillation | The process used to separate dissolved solids from a liquid (or separate liquids with different boiling points) by boiling the liquid to create a vapor (gas) and then condensing the vapor back into a pure liquid elsewhere, leaving the solids behind. |
| Element vs. Compound | Compounds can be broken down into simpler substances by chemical means, but elements cannot. |
| Element | The simplest form of matter that has a unique set of properties and cannot be broken down further by ordinary chemical or physical means. |
| Chemical Symbol | A one- or two-letter abbreviation used by chemists to represent elements. |
| Properties of Compounds | Compounds have completely different physical and chemical properties than the elements that make up the compound. |
| Etymology of Compound | Comes from the Latin word componere meaning “to put together” (chemically). |
| Breaking Down Compounds | In order to break down compounds into their constituent elements, they must undergo a chemical change. |
| Methods for Breaking Down Compounds | Applying energy through heating, electrolysis (using electricity), or reacting with other specific substances. |
| Symbols | Represent individual elements (e.g., H for Hydrogen, O for Oxygen). |
| Chemical Formulas | Represent compounds (e.g., H2Ocap H sub 2 cap O 𝐻2𝑂 for Water, NaCl for table salt). |
| Symbol Rules | Symbols are one or two letters. The first letter of a chemical symbol is always capitalized, and the second is always lowercase (e.g., Co for Cobalt vs. CO for Carbon Monoxide). |
| Berzelius's System | The modern system we use today was developed by Swedish chemist Jöns Jacob Berzelius in the early 19th century. |
| Measurements | A quantity that has both a number (magnitude) and a unit (e.g., 5 meters, 2.5 kg). |
| Importance of Measurement | Measurements are fundamental to the experimental sciences, crucial for accuracy and precision in chemistry. |
| Scientific Notation | A method for expressing very large or very small numbers efficiently. A given number is written as the product of two numbers |
| Accuracy | A measure of how close a measurement is to the true or accepted value of whatever is being measured. |
| Precision | A measure of how close a series of measurements are to one another (reproducibility). |
| Evaluating Accuracy | The measured value must be compared to the correct (accepted) value. |
| Evaluating Precision | You must compare the values of two or more repeated measurements. |
| Accepted Value | The correct value based on reliable references and measurements. |
| Experimental Value | The value measured in the laboratory by a researcher. |
| Error | The difference between the experimental value and the accepted value. (Error = Experimental Value - Accepted Value). |
| Percent Error | A calculation used to determine the relative accuracy of a measurement. (Percent Error = (Absolute Value of the Error / Accepted Value) ×cross × 100%). |
| Significant Figures (Sig Figs) | In any measurement, the significant figures include all the digits that are known for certain, plus a last digit that is estimated. |
| Rule 1 (Nonzero) | All nonzero digits are significant (e.g., 24.7 m has 3 sig figs, 714 cm has 3 sig figs). |
| Rule 2 (Interior Zeros) | Zeros between nonzero digits are significant (e.g., 40.79 m has 4 sig figs, 7003 cm has 4 sig figs). |
| Rule 3 (Trailing Zeros with Decimal) | Zeros at the end of a number and to the right of a decimal point are ALWAYS significant (e.g., 43.00 m has 4 sig figs, 1.010 mm has 4 sig figs). |
| Rule 4 (Leading Zeros) | Leftmost zeros in front of nonzero digits are NOT significant (placeholders only) (e.g., 0.0071 m has 2 sig figs, 0.42 cm has 2 sig figs). |
| Rule 5 (Trailing Zeros without Decimal) | Zeros at the rightmost measurement but left of an understood decimal point are ambiguous and usually NOT significant unless specified with a bar or decimal point (e.g., 7000 m has 1 sig fig; 28,190 cm has 4 sig figs). |
| Rule 6 (Unlimited Sig Figs) | Two situations have an unlimited number of sig figs |
| Calculation Rule | A calculated answer cannot be more precise than the least precise measurement from which it was calculated. |
| Rounding Rules (General) | 5 and greater you round up the preceding digit by 1. Less than 5 you keep the preceding digit the same (effectively rounding down). |
| SI Units | The International System of Units (metric system), a standardized system of measurement used globally in science. |
| Metric System Basis | The metric system is easy to use because it is based on multiples of 10 and conversion between units is straightforward. |
| Base Units | There are seven fundamental base units in the SI system. |
| Derived Units | Different quantities require different units, often derived from the base units. |
| Unit of length | meter (m). |
| Unit of volume | liter (L) or cubic meter ( m3m cubed 𝑚3). |
| Unit of mass | gram (g) or kilogram (kg). |
| Unit of temperature | Celsius (°C) and Kelvin (K). |
| Unit of energy | joule (J) and calorie (cal). |
| Temperature Conversion K | K = °C + 273.15 |
| Temperature Conversion °C | °C = K - 273.15 |
| Prefix Chart Hierarchy | The standard stair-step or ladder method for converting between metric units. |
| King Henry Died By Drinking Chocolate Milk | A common mnemonic for remembering the order of prefixes from largest to smallest. |
Created by:
ajbehnke