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| the submicroscopic particles that constitute the fundamental building blocks of ordinary matter |
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| two or more atoms joined in a specific geometrical arrangement |
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| the siceince that seeks to understand the behavior of matter by studying the bahvior of atoms and molecules |
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| anything that occupies space and has mass. a specific instance of matter is a substance. matter can be classified by its state (physical form - solid, liquid, or gas) and its composition (the basic components that make it up) |
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| made up of only one component and its composition is invariant (it does not bary from one sample to another); can be broken down to elements or compounds, depending on whether or not they can be broken down into simpler substances. |
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| a substance composed of two or more components in proportions that can vary from one sample to another. can be divided into heterogenous and homogenous |
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| a substance that cannot be broken down into simler substances |
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| a substance composed of two or more elements in fixed, definite proportions |
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| one in which the composition varies from one region to another because the atoms or molecules that compose them seperate |
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| one with the same composition throughout because the atoms or molecules that compose them mix uniformly |
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| change that alters only state or appearance, but not composition |
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| change that alters the composition of matter. During this change, atoms rearrange, transforming the original substances into different substances |
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| one that a substance displays without changing its composition. includes odor, color, etc |
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| one that a substance displays only by changing its composition via chemical change. includes flamability, toxicity, etc |
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| the capacity (needed) to do work |
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| the action of a force through a distance |
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| the sum of its kinetic energy and its potential energy |
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| the energy associated with motion |
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| the energy associated with its position or composititon |
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| the energy associated with the temperature of the object |
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| a measure of the quantity of matter within an object |
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| a measure of the gravitational pull on an object's matter |
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| the ratio of a substance's mass to its volume |
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| one that is independent of the amount of the substance |
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| one that depends on the amount of the substance |
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| refers to how close the measured value is to the actual value |
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| refers to how close a series of measurements are to one another or how reproducible they are |
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| a tentative interpretation or explanation of the observations |
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| a highly controlled procedure designed to generate observations; used to test hypothesis' |
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| a brief statement that summarizes past observations and predicts future ones |
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| a model for the way nature is and tries to explain not merely what nature does but why |
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| law of conservation of mass |
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| formulated by Lavoisier. "in a chemical reaction, matter is neither created nor destroyed" |
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| law of definite proportions |
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| "all samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements." |
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| law of multiple proportions |
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| "when two elements (call them A and B) form two different compounds, the masses elemnt B that combine with 1 g of element A can be expressed as a ratio of small whole numbers." |
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| 4 parts of the Atomic Theory |
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Definition
1. Each element is composed of tiny, indestructible particles called atoms.
2. All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements.
3. Atoms combine in simple, whole-number ratios to form compounds.
4. Atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms only change the way that they are BOUND TOGETHER with other atoms. |
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| the emission of small energetic particles from the core of certain unstable atoms |
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| 3 parts of the Nuclear Theory |
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Definition
1. Most of the atom's mass and all of its positive charge are contained in a small core called the nucleus.
2. Most of the volume of the atom is empty space, throughout which tiny, negatively charged electrons are dispersed.
3. There are as many negatively charged electrons outside the nucleus as there are positively charged particles (protons) within the nucleus, so that the atom is electically neutral. |
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| atoms with the same number of protons but different numbers of neutrons |
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| the number of protons in the atom's nucleus |
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| the sum of the number of neutrons and protons in an atom |
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| charged (either positive or negative) particles that result from an atom losing or gaining electrons in a chemical reaction |
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| When the elements are arranged in order of increasing mass, certain sets of properties recur periodically. |
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| the average mass of an element based on calculations of the masses of its isotopes (and weighted according to the natural abundance of those isotopes) |
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| defined as "the amount of material containing 6.02214 x 10^23 particles". This number is also Avagadro's number. |
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| an element's molar mass in grams per mole is numerically equal to the element's atomic mass in atomic mass units. |
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| Key Conversions to Remember |
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1 kg = 2.205 lb
453.59 g = 1 lb
28.35 g = 1 oz
1 L = 1000 mL = 1000 cm^3
1 L = 1.057 qt
3.785 L = 1 gal
1 km = .6214 mi
1 m = 39.37 in = 1.094 yd
1 in = 2.54 cm |
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C = (F-32)/1.8
K = c + 273.15
F = 1.8(C) + 32 |
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| using units as a guide to solving problems |
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| a fractional quantity with the units we are converting from on the bottom and the units we are converting to on the top |
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| bonds which occur between metals and nonmetals; involve the TRANSFER of electrons from one atom to another. |
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| bonds which occur between two or more nonmetals; involves the SHARING of electrons between two atoms |
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| indicates the elements present in the compound and the relative number of atoms or ions of each |
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| Types of chemical formulas |
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Definition
empirical formula: gives the RELATIVE number of atoms of each element in the compound
molecular formula: gives the ACTUAL number of atoms of each element in a molecule of a compound
structural formula: uses lines to represent covalent bonds and shows how atoms n a molecule are connected or bonded to each other |
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| exist in nature with single atoms as their basic units |
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| elements that exist in nature as molecules(two or more atoms of the element bonded together). most molecular elements exist as DIATOMIC molecules - Oxygen(O2) |
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| usually composed of two or more covalently bonded nonmetals |
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| composed of cations and anions bound together by ionic bonds |
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| anions containing oxygen and another element. nitrite, chlorate, phosphate... |
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| ionic compounds that contain a specific number of water molecules associated with each formula unit |
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| MOLECULAR compounds that release hydrogen ions (H+) when dissolved in water. they are composed of hydrogen, usually written first in their formula, and one or more nonmetals, written second |
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| contain hydrogen and an oxyacid(anion containing nonmetal and oxygen) |
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| a process in which one or more substances are converted into one or more different ones; |
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| a particular type of chemical reaction in which a substance combines with oxygen to form one or more oxygen-containing compounds |
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| represents a chemical reaction. the substances on the left are called REACTANTS, substances on the right are called PRODUCTS |
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| compounds that originate from living things. (sugar from sugarcane). They are composed of carbon and hydrogen, and a few other elements including nitrogen, oxygen, and sulfur |
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| compounds that originate from the Earth. (salt mined from ground) |
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| organic compounds that contain only hydrogen and carbon. hydrocarbons containing only single bonds are called ALKANES, doubles bonds are called ALKENES, and triple bonded hydrocarbons are called ALKYNES. |
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| functionalized hydrocarbons |
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| hydrocarbons in which a FUNCTIONAL GROUP-a characteristic atom or group of atoms(generally an OH group such as in alcohol)- is incorporated into the hydrocarbon |
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