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