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Chem 105 Exam 1
| Term | Definition |
|---|---|
| Chemistry | is the study of matter and the changes it undergoes |
| Matter | is anything that has mass and occupies space |
| Scientific Method Process | 1. Observation and description of a phenomenon 2. Hypothesis 3. Use of the hypothesis to predict the existence of other phenomena, or explain the results of new observations 4. Experimental tests of the predictions |
| Scientific Method | fail-safe method for analyzing observations Observation - Hypothesis - Experiments (prove or disprove) - Publication (further experiments) - Conformation - Application |
| hypothesis | educated guess |
| theory | A hypothesis that has been tested with a significant amount of data |
| law of nature | a generalization that describes recurring facts or events in nature |
| Physical Sciences | chemistry, physics, geology, and astronomy |
| biological sciences | botany and zoology |
| Physics | sciences of matter and energy and of interactions between them |
| Geology | study of origin, history, and structure of the earth |
| Astronomy | is the scientific study of matter in outer space. |
| Botany | science or study of plants |
| zoology | deals with animals and animal life including the study of structure, physiology, development, and classification of animals |
| Physical Chemistry | chemistry is applied to physics |
| geochemistry | chemistry of the earth is studied |
| biochemistry | chemistry of biological entities |
| Basic science | is research without the goal of a practical application |
| Applied Science | science of applying the knowledge gained from one or more natural scientific fields to practical problems |
| Macroscopic | matter large enough to be seen by the naked eye |
| Microscopic | requires the aid of a microscope or similar instruments to be viewed |
| submicroscopic | matter is too small to be seen even with the most powerful microscopes |
| Mass | quantity of matter in an object |
| weight | force that results from the attraction between matter and the earth |
| property | anything that can be observed or measured about a sample of matter |
| intensive | independent of the sample size such as concentration, density, and boiling and freezing points. |
| extensive | depends on the size or amount of the sample like mass, volume and energy |
| elements | substances containing only one kind of atom |
| atom | smallest unit found in elements |
| pure substances | matter with fixed composition at the submicroscopic level |
| compounds | decomposed into simpler substances by normal chemical means |
| mixtures | a combination of substances |
| heterogeneous | which different substances can easily be seen within the mixture |
| homogeneous | COMPOSED OF IDENTICAL PARTS; UNIFORM IN COMPOSITION |
| solution | a mixture of different solutions |
| chemical properties | describe the tendency of a material to react and change into a different compound |
| physical properties | can be measured without changing the identity of the material |
| physical change | since it resulted in a change in only physical not chemical identity |
| chemical change | change in which a part of the substance is being converted into a different kind of matter |
| chemical reaction | the process in which one or more substances are converted to one or more different substances |
| reactants | substances that undergo a change in chemical reaction |
| products | substances that are formed in a chemical reaction |
| molecule | smallest unit of a chemical compound that can exist independently |
| diatomic | molecules formed from two atoms |
| energy | is defined as the ability to do work ī |
| potential energy | energy in storage by virtue of position or arrangement |
| kinetic energy | is the energy of objects in motion |
| chemical formula | written combination of element symbols that represents the different atoms combined in a chemical compound |
| subscripts | are used in chemical formulas as numbers written below the line to show the numbers or ratios of atoms in a compound |
| molecular formulas | are chemical formulas that represent molecules with atomic symbols an subscripts |
| structural formulas | chemical formulas that show the connections between atoms in molecules with straight lines |
| chemical equations | describe the identities and relative amounts of both reactants and products in a chemical reaction |
| qualitative | not numerical but are used to identify the chemical species involved |
| quantitative | determine the amount of product formed or the amount of reactants used in a chemical reaction |
| accuracy | agreement of the measured value with the true value of the same quantity. |
| John Dalton | Creator of Dalton's atomic theory (1766-1844) |
| law of constant composition | all samples of a pure substance contain the same elements in the same proportions by mass |
| law of multiple proportions | states that the masses of one element will always combine with a fixed mass of the second element |
| law of conservation of mass or matter | there is no detectable loss or gain in mass when a chemical reaction occurs |
| Nucleus | contains 99% of the mass and is found in the center of the atom |
| nuclear model of the atom | protons and neutrons are found in the nucleus of the atom and the electrons are located in a three dimensional area around at a relatively large distance away from the nucleus |
| atomic number | number of protons in an atom rep. by letter Z. |
| mass number | number of protons plus the number of neutrons in the nucleus of an atom and is represented by the letter |
| Isotopes | different atoms of the same element that contain different numbers of neutrons (same z, different A) |
| ions | new charged species |
| anions | gain electrons, becoming negatively charged |
| cations | lose electrons, become positively charged |
| Atomic mass number (u with line coming down at beginning | established to compare the mass of any atom to that of the carbon 12 isotope |
| atomic weight | weighted average mass in atomic mass units the isotopes of an element |
| waves | repeat at regular intervals of time and distance |
| amplitude | maximum height of the wave |
| wavelength | is the distance between one peak and the next |
| frequency | is the number of waves that pass a particular point in a given time period (Hz 1/s) |
| electromagnetic radiation | consist of oscillating electric and magnetic fields perpendicular to one another |
| constructive interference | positive effect light rings |
| destructive interference | negative effect, dark rings |
| excited state | higher energy state |
| ground state | lower original state |
| principle shells | discrete energy levels |
| niels bohr | 1911, he showed that electrons in atoms were limited to these energy levels or shells 1st shell=2 electrons, 2nd shell=8 electrons, 3rd shell=18 electrons, 4th shell=32 electron |
| atomic orbital | is a region of 3-deminesional space where electrons exist around the nucleus |
| sub shells | each energy shell consists of a certain number and type of orbitals grouped into Ex: S,P,D,F |
| aufbau principle | electrons are added to atoms one at a time to available orbital with the lowest energy first |
| electron configuration | distribution of these added electrons |
| Valence orbitals | orbitals of the outermost or highest energy level and partially filled subtle of lower energy |
| valence electrons | electrons found in these valence orbitals- most involved in chemical reactions |
| period | each row of the table 1-7 |
| groups | tio of the table |
| metal | substance that is malleable, has luster, and is a good conductor of electricity |
| metalloids | fall along the actual line separating the metals from the nonmetals and share certain properties of both |
| semi-conductors | weak conductors of electricty |
| transition metals | showing a regular decrease in metallic behavior IIIB |
| inner transition metals | are found at the bottom of the table |
| name for inner transition metals | lanthanides (Ce-Lu( and actinides (Th-Lr) |
| alkaline earth metals | Group 1A slightly less reactive than the alkali metals |
| alkali metals | Group 2A very reactive, especially with water and must be handled carefully |
| halogens | Group 7A among the most reactive nonmetals with reactivity's decreasing down the group |
| Noble gases | VIIIa Inert gases because of their seemingly nonreactive behavior |
| 1s^1 | referring to electorn configuration, hydrogen |
| 2s^1 | lithium |
| ionization energy | amount of energy needed to remove an electron and increases from left to right and decreased from top to bottom on the periodic table |
| Ernest Rutherford Gold Foil Experiment | atom is mostly empty space. Over 99% of mass is found in a very small region in the nucleus. lead to modern view of the atom |
| Representative Elements | S and P blocks |
| Transition Elements | D and F blocks |
| Atomic Radii | Gets smaller from left to right Gets larger from top to bottom |
| Ionic Radii | Cations are smaller than neutral atoms, anions are larger |
| Extra Credit: Where did the W on the periodic table for tungsten come from? | Wolfram, Tungsten's original name. |
| John Dalton | 1. all matter is made up of small indivisible particles called atoms 2. atoms of the same element are identical; atoms of different element have different properties 3. compounds are formed when atoms of different elements combine in small whole numb |
Created by:
dmstewart416
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