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51 Cards in this Set
- Front
- Back
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Matter
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- defined as anything that occupies space
-composed of atoms |
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3 States of Matter
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-Solid
-Liquid -Gas |
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Atoms
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-particles too small to see that compose matter
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Molecules
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-two or more atoms joined together in specific geometric arrangements
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Solid
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- Shape: Definite
- Volume: Definite -Particles: Rigidly clinging; tightly packed -Compressibility: Very Slight |
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Liquid
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- Shape: Indefinite
- Volume: Definite -Particles: Mobile; adhering -Compressibility: Slight |
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Gas
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- Shape: Indefinite
- Volume: Indefinite -Particles: Independent of each other and relatively far apart -Compressibility: High |
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Branching Matter
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1. Matter
-A. Pure Substance --a. Elements --b. Compounds -B. Mixtures --a. Homogeneous --b. Heterogeneous |
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Pure Substance
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-composed of only one type of atom or molecule
-ex. He, water, |
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Mixture
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-composed of two or more different types of atoms or molecules combined in variable proportions
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Element
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-A substance that cannot be broken down into simpler substances
-ex graphite (carbon) |
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Algae contains rougly?
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50% protein, 6-7% fibre, 4-6% fat, 6% ash (minerals)
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Mixtures
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-ex. soil, flame, apple juice, air, sea water, brass
-varying proportions of its constituent components |
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Heterogeneous Mixture
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ex. oil + water
-composition varies from one region to another |
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Homogeneous Mixture
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ex. salt water or sweetened
-uniform composition; atoms and molecules that compose them mix uniformly |
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Properties
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--used to distinguish on substance from another
-- physical and chemical |
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Physical Property
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- substance displays without changing its composition
-change in state -change in shape, size,etc. ex: Melting point, boiling point, color, odor, taste, ductility, malleability, luster, density, viscosity, shape, mass, volume, temperature |
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Chemical Properties
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- those that a substance displays only through changing its compositions
ex. chemical changes, flammability, corrosivity, reactivity, explosivity |
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Physical Change
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- matter changes its appearance but not its composition
ex, Water => gas |
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Chemical Changes
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- matter does change its composition
- ex. copper turns to green exposure to air reacts and forms new compounds |
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Chemical Reaction
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- matters undergoes chemical change
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Reactants vs Products
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-Before vs After substances in chemical change
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Indicating whether physical or chemical change occurred...
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- phase changes = physical property
- chemical changes = often heat exchange or color change -physical changes = no atomic level associations; difference form of the substance -chemical changes = completely new substance Vaporization vs Burning |
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Separating Mixtures through Physical Changes
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Decanting- pouring off
Distillation- boiling off more volatile substance; re condensed Filtration- mixture poured through filter paper |
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Law of Conservation of Mass
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-Matter us neither created nor destroyed in chemical reaction
-matter remains constant burning butane Butane + Oxygen // 58g + 208g = 266g =======> Carbon Dioxide + Water// 176g + 90g = 266g |
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Energy
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-the capacity to do work
-behavior of matter is driven in large part by energy, so understanding energy is critical to understanding chemistry |
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Law of Conversation of Energy
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-Energy can be neither created nor destroyed
-total amount of energy is constant; energy can be changed from one form to another or transferred from one object to another, but not created; but not created |
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Kinetic Energy
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-Energy associated with its motion
ex water flowing a dam |
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Potential Energy
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-energy associated with its position
ex water held behind a dam |
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Electrical Energy vs Chemical Energy
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Energy associated with the flow of electrical charge vs energy associated with potential chemical changes that can move or heat other objects ex chemical energy stored in gasoline to move a car
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Joule (J)
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-SI unit of energy
-4.184J required to raise temperature of 1g of Water by 1*C -4.184J = 1 calorie (cal) |
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calorie (cal)
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- 1 cal raises temp of 1g of water by 1 *C
- larger unit that J -1cal = 1 4.184J |
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Calorie (Cal)
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- equivalent to 1,000 little (cal)ories
- food Calories - = 4184J or 4.184 kJ |
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Exothermic
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- chemical reactions that release energy
-reactants have more energy than the products, and energy is released as the reaction occurs |
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Endothermic
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- chemical reactions that absorb energy from their surroundings as they occur
-ex cold pack = chemicals mix and absorb heat from surroundings - products have more energy than the reactants, and energy is absorbed as the reaction occurs |
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Temperature
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-related to the random motion of the atoms and molecules that compose it
-hotter the object the greater the motion and higher the temperature -measure of thermal heat of matter -measured in three ways Fahrenheit (*F), Celsius (*C), Kelvin (K) |
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Heat
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-exchange of thermal energy caused by temperature difference
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Fahrenheit
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- water freezes at 32*F
-water boils at 212*F -Room temp 72*F -assumes 0*F freezing point of salt water solution -96*F body temp |
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Celsius
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- water freezes at 0*C
-boils at 100 *C - Room temp 22*C *C= (*F-32) / 1.8 |
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Kelvin
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- 0K the coldest temp possible
- 0K = Absolute zero -at this temperature even molecular motion virtually stops 273K water Freezes 373K water boils -273*C -459*F K= *C + 273 |
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Heat Capacity
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-quantity of thermal energy (usually in joules) required to change the temperature of a given amount of the substance by 1*C
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Specific Heat Capacity
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- units of joules per gram per degree Celsius
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Using the specific heat capacity (C)
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The C of a substance can be used to quantify the relationship between the amount of heat added to a given amount of the substance and the corresponding temperature increase
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Heat Equation
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Heat (J) = Mass (G)x Specific Heat Capacity (J/g*C) x Temperature Change (*C)
q = m x C x DeltaT |
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Greek Atoms
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-matter 4 elements (earth, air, water, earth)
-matter is continuous |
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Alchemists
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-Philospher's Stone (base metals to gold)
- fountain of youth -Panacea cure of all ills - solvent of dissolving anything ACTUAL CONTRIBUTIONS -new techniques (sublimination, coagulation, crystallization, etc) -lab tools -new substances |
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Chemistry as a Quantitative
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-conservation of mass
-definite porportions -multiple proportions |
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Conservation of Mass
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-Lavoisier 1700s
-matter neither created nor destroyed |
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The Law of Definite Proportions
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-1799 Proust
- compound same elements in definite proportions |
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Dalton
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- Billard ball model
-atom small solid sphere -definite proportions -matter indivisible atoms -chem reactions reaarangements of atoms to form new compounds |
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Cathode Ray
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-deflection of cathode rays (electrons) by applied electric field
-movement of ray caused new Thompson model |
