Phases+of+Matter+and+Solutions

= ﻿﻿﻿Indicators for Phrases of Matter and Solution =

__**Solute**__: the substance dissolved in a given solution (EX: sugar, salt, nail polish, glue, egg shells, iodine.) __**Solvent**__: a substance that dissolves another to form a solution.(EX: water, acetone, vinegar, hexane) __**Solution**__: the process by which a gas, liquid, or solid is dispersed homogeneously in a gas, liquid, or solid without chemical change. media type="youtube" key="hydUVGUbyvU" width="425" height="350"
 * __﻿ 1. Definitions__ -**

A song about solubility: media type="youtube" key="oF9sl77Jv7Y" width="425" height="350" __**Saturated**__: a solution containing the maximum amount of solute capable of being dissolved under given conditions __**Hydrogen Bonding**__: C hemical bonding formed between an electropositive atom (typically hydrogen) and a strongly electronegative atom, such as oxygen or nitrogen. Hydrogen bonds are responsible for the bonding of water molecules in liquid and solid states, and are weaker than covalent and ionic bonds. media type="youtube" key="LGwyBeuVjhU?fs=1" height="385" width="480" __**Molarity**__: the number of moles of solute per liter of solution. [|how to calculate molarity] __**Triple Point**__: The temperature and pressure at which a substance can exist in equilibrium in the liquid, solid, and gaseous states. The triple point of pure water is at 0.01°C (273.16K, 32.01°F) and 4.58 mm (611.2Pa) of mercury and is used to calibrate thermometers.

TRIPLE POINT :D media type="youtube" key="BLRqpJN9zeA" width="425" height="350"

**-Colligative Properties**media type="youtube" key="n0W7Y2Gwi2E" width="425" height="350" A music video explaining what colligative properties are: media type="youtube" key="-NeLlWq3-aQ?fs=1" height="385" width="480" __**Specific Heat Capacity**__- is the amount of //heat// per unit mass required to raise the temperature by one degree Celsius.
 * __Colligative Properties__** - are properties of solutions that depend on the number of molecules in a given volume of solvent and not on the properties (e.g. size or mass) of the molecules

[|more info. on specific heat capacity] **__Calorimetry__** is the science of measuring the heat of chemical reactions or physical changes media type="youtube" key="hrnYuI9Wbq0?fs=1" height="385" width="480" [] **__Molar Heat of Fusion__** - the amount of heat necessary to melt (or freeze) 1.00 mole of a substance at its melting point

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**__Molar Heat of Vaporation__** - the amount of heat necessary to boil (or condense) 1.00 mole of a substance at its boiling point



=**Specific Heat, Heat of Fusion and Vaporization: ** = media type="youtube" key="zz4KbvF_X-0" width="425" height="350"
 * __2. Describe the 3 states matter in terms of energy and distance between the particles__**

Solid-

particles are closer and moving around the least (stage with least energy)

Liquid- particles are a little further apart and move (slide) around more



and Gas-the particles are furthest apart and moving around the most (stage with most energy)

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//[|More information on the properties of matter]//
__**3.phase change that matter undergoes and state whether they are exothermic or endothermic**__ matter undergoes endothermic because it's using heat

media type="youtube" key="Yl4qNXebhys" width="425" height="350" __**4. Identify the solute and solvent in a solution**__ A homogenous mixture (solution) is made up of two components, a solute and a solvent. The solute is the substance that is added/ dissolved into the other substance (solvent) to make the solution and is the lesser quantity of the two. The solute may be a gas, liquid or solid. Solvents are the larger amount and tend to be a liquid or gas which dissolves the solute. For example: in the solution- Sugar water. Sugar is the solute where as water (larger amount) is the solvent. Another Example: http://wiki.answers.com/Q/Identify_the_solute_and_solvent_in_a_hot_chocolate_solution_that_is_made_of_chocolate_syrup_and_warm_milk

media type="youtube" key="R1Qgd3OXsO8" width="425" height="350" __**5. Hydrogen bonding and its boiling point**__

A **hydrogen bond** is the attractive interaction of a hydrogen atom with an electronegative atom, such as nitrogen, oxygen or fluorine, that comes from another molecule or chemical group. The hydrogen must be covalently bonded to another electronegative atom to create the bond. These bonds can occur between molecules (//intermolecularly//), or within different parts of a single molecule (//intramolecularly//).[2[|]] The hydrogen bond (5 to 30 kJ/mole) is stronger than a van der Waals interaction but weaker than covalent or ionic bonds. This type of bond occurs in both inorganic molecules such as water and organic molecules such as DNA. Intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C) compared to the other group 16 hydrides that have no hydrogen bonds. Intramolecular hydrogen bonding is partly responsible for the secondary, tertiary, and quaternary structures of proteins and nucleic acids. It also plays an important role in the structure of polymers, both synthetic and natural. For more information click

More information about ** Hydrogen bonding and its boiling point **
[|http://www.elmhurst.edu/~chm/vchembook/163boilingpt.html]


 * __6. Calculate The Molarity of a Solution__**
 * __click this page for the information__**


 * __Activation Energy Video . . . . Endo & Exo thermic Reactions broken down into depth__**

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In this lab a group of students got together to show the audience the difference between exothermic & endothermic reactions. Hope you like it :DD [] Here is a funny video explaining the differences between endo and exothermic.

Chemical reaction in which, a greater amount of energy is required to break the existing bonds in the reacants, the is relased when the bonds form in the product molcules.
 * ENDOTHERMIC REACTION:** that absorbs heat from its surroundings as the reaction proceeds;

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a chemical reaction, in which more energy is released then is required, to break bonds in the intial reaction. media type="youtube" key="80Q3GgeeIVM" height="390" width="480"
 * EXOTHERMIC: Reaction** that gives off heat to the environment.

__**7. Interpret a phase diagram with respect to phase of matter, triple point, melting point, and boiling point.**__

[|Info. about phase diagrams with diagram]

Phase diagrams illustrate the variations between the states of matter of elements or compounds as they relate to pressure and temperatures.
 * Triple point – the point on a phase diagram at which the three states of matter: gas, liquid, and solid coexist
 * Critical point – the point on a phase diagram at which the substance is indistinguishable between liquid and gaseous states
 * Fusion (melting) (or freezing) curve – the curve on a phase diagram which represents the transition between liquid and solid states
 * Vaporization (or condensation) curve – the curve on a phase diagram which represents the transition between gaseous and liquid states
 * Sublimation (or deposition) curve – the curve on a phase diagram which represents the transition between gaseous and solid states

media type="youtube" key="gbUTffUsXOM?fs=1" height="385" width="480" **__8.__**__**Define hydrogen bonding and describe its effect on physical properties including boiling point, vapor pressure and heat of vaporization.**__ A hydrogen bond is the attractive interaction of a hydrogen atom with an electronegative atom, like nitrogen, oxygen or fluorine (thus the name "hydrogen bond", which must not be confused with a covalent bond to hydrogen). ... A great affect. H bonding links the molecules together rather strongly so that water acts sort of like a super molecule. HOH which was not H bonded would be a very volatile gas like H2S because its molecular weight is low. But water's high polarity and oxygen's high electronegativity are ready made for H bonding, and we have liquid water on the planet and in our bodies, etc. Hydrogen bonding is the strongest intermolecular attractive force. It causes the boiling point to be elevated since the molecules are more attracted to each other and thus require more energy to break from the liquid phase.
 * Hydr vs. phy**
 * Hydr vs boli**

__**9.Calculate energy changes, using specific heat capacity.**__ media type="youtube" key="haannJ_7w-k?fs=1" height="385" width="480" URL: []

**Calculating Energy changes** //Energy in the lab is most easily measured as heat.// As you can see from the demonstration relating to heat and temperature, the amount of heat transferred can be readily determined by changes in temperature of the surroundings. When a substance undergoes a temperature change without a phase, chemical or nuclear change occurring, three factors determine the amount of heat (Q) a substance will absorb or release.The three factors are: 1) **mass** of the substance (m). 2) **specific heat capacity ** of the substance (a measure of how much energy the substance absorbs to change the temperature 1oC). 3) **temperature change** the substance undergoes ( T).**10. Calculate specific heat capacity using calorimetry data:**

__**10. Calculate Specific Heat Capacity Using Calorimetry Data **__ media type="youtube" key="XwCLvJdVrIs?fs=1" height="385" width="480" Calorimetry is a device used to measure heat of reaction. When calculating heat capacity styrofoam cups are used as a calorimeter, because it is a container with good insulated walls to prevent heat exchange with the environment. This is the equation for calculating heat capacity: q = cp x m x ΔT\

[] [] __**11. Calculate energy changes using molar heat of fusion and heat of vaporization**__

MOLAR HEAT OF FUSION SONG :D media type="youtube" key="jaaGqui9NVY" width="425" height="350"

Here is the definition of the molar heat of fusion: the amount of heat necessary to melt (or freeze) 1.00 mole of a substance at its melting point Note the two important factors: 1) It's 1.00 mole of a substance 2) there is no temperature change Keep in mind the fact that this is a very specific value. It is only for one mole of substance melting. The molar heat of fusion is an important part of energy calculations since it tells you how much energy is needed to melt each mole of substance on hand. (Or, if you are cooling off a substance, how much energy per mole to remove from a substance as it solidifies. Every substance has its own molar heat of fusion. The units are usually kilojoules per mole (kJ/mol). Sometimes the unit J/g is used. The first unit is technically the more correct unit to use. The molar heat of fusion for water is 6.02 kJ/mol. Remember the value!!! Molar heat values can be looked up in reference books. They are determined by experiment. The molar heat of fusion equation looks like this: q = ΔHfus (mass/molar mass) for more info click this media type="youtube" key="P7Ui3TH_MHk?fs=1" height="385" width="480"
 * Molar Heat of Fusion**

[] Here is the definition of the molar heat of vaporization: the amount of heat necessary to boil (or condense) 1.00 mole of a substance at its boiling point Note the two important factors: 1) It's 1.00 mole of a substance 2) there is no temperature change Keep in mind the fact that this is a very specific value. It is only for one mole of substance boiling. The molar heat of vaporization is an important part of energy calculations since it tells you how much energy is needed to boil each mole of substance on hand. (Or, if we were cooling off a substance, how much energy per mole to remove from a substance as it condenses.) Every substance has its own molar heat of vaporization. The units are usually kilojoules per mole (kJ/mol). Sometimes the unit J/g is used. The first unit is technically the more correct unit to use. The molar heat of vaporization for water is 40.7 kJ/mol. Remember the value!!! Molar heat values can be looked up in reference books. They are determined by experiment. The molar heat of vaporization equation looks like this: q = ΔHvap (mass/molar mass) for more info click this media type="youtube" key="zz4KbvF_X-0?fs=1" height="385" width="640"
 * Heat of Vaporization**

__** 12. Compare the freezing point of pure water with a water solution (with a nonvolatile solute). **__ The freezing point of pure water is 0 degrees Celcius (32 degrees Fahrenheit). When a nonvolatile solute is added to a water solution it changes the freezing point of the solution. Depending on the nonvolatile solute, the water solution can remain in a liquid state even if it is below the usual freezing point of water. If a solution only has pure water, it will still freeze at 0 degrees Celcius. This is also known as freezing point depression, which is [|“] [|the decrease in the freezing point of a solvent caused by the presence of a solute.”] An example of a water solution with a nonvolatile solute is salt water.

A video example of the freezing point of pure water changing when a nonvolatile solute is added: media type="youtube" key="JzPG-PO9iRQ" width="425" height="350"

The van 't Hoff factor (named after J. H. van 't Hoff ) is a measure of the effect of a solute upon colligative properties, such as vapor pressure , osmotic pressure and freezing point depression. The van 't Hoff factor is the ratio between the actual concentration of particles produced when the substance is dissolved, and the concentration of a substance as calculated from its mass. For most non- electrolytes dissolved in water, the van' t Hoff factor is essentially 1. For most ionic compounds dissolved in water, the van 't Hoff factor is equal to the number of discrete ions in a formula unit of the substance.
 * __13. Describe the relationship of number of dissolved particles in a solution on boiling and freezing point.__**

__**14. Identify and describe the type of intermolecular force in a molecular compound. (Hydrogen bonds, dipole-dipole attractions, Van der Waals). **__ Main article: [|London dispersion force] Otherwise known as quantum-induced instantaneous polarization, the London dispersion force is caused by correlated movements of the electrons in interacting molecules. The electrons, which belong to different molecules, start "feeling" and avoiding each other at the short intermolecular distances, which is frequently described as formation of "instantaneous dipoles" that attract each other.media type="youtube" key="8qfzpJvsp04?fs=1" height="385" width="640"
 * London dispersion forces **

Debye (induced dipole) force
The induced dipole forces appear from the induction (also known as polarization), which is the attractive interaction between a permanent multipole on one molecule with an induced multipole on another. This interaction is called Debye force after Peter J.W. Debye.  Keesom interactions (named after Willem Hendrik Keesom) are attractive interactions of dipoles that are Boltzmann-averaged over different rotational orientations of the dipoles. Energy of Keesome interaction depends on the inverse sixth power of the distance, unlike the interaction energy of two spatially fixed dipoles, which depends on the inverse third power of the distance. <span style="font-family: Arial,Helvetica,sans-serif;">Often, molecules have dipolar groups within them, but have no overall dipole moment. This occurs if there is symmetry within the molecule, causing the dipoles to cancel each other out. This occurs in molecules such as tetrachloromethane. Note that the dipole-dipole interaction between two atoms is usually zero, because atoms rarely carry a permanent dipole, see atomic dipoles. media type="youtube" key="LSeEmdY3SK0?fs=1" height="385" width="480"

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<span style="font-family: Arial,Helvetica,sans-serif;">Hydrogen bonding
<span style="font-family: Arial,Helvetica,sans-serif;">Main article: [|Hydrogen bond]

**__//Hydrogen bonding video//__**
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<span style="font-family: Arial,Helvetica,sans-serif;">A hydrogen bond is the attractive interaction between a hydrogen atom and an electronegative atom, such as nitrogen, oxygen or [|fluorine][1] <span style="font-family: Arial,Helvetica,sans-serif;">. The hydrogen bond is often described as a strong electrostatic dipole-dipole <span style="font-family: Arial,Helvetica,sans-serif;">interaction. However, it also has some features of covalent bonding: it is directional, stronger than a [|van der Waals interaction], produces interatomic distances shorter than sum of van der Waals radii, and usually involves a limited number of interaction partners, which can be interpreted as a kind of valence.

Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter on energy. __ **The Particle Theory of Matter:** __
 * 1. Matter is made up of tiny particles (Atoms & Molecules)
 * 2. Particles of Matter are in constant motion.
 * 3. Particles of Matter are held together by very strong electric forces
 * 4. There are empty spaces between the particles of matter that are very large compared to the particles themselves.
 * 5. Each substance has unique particles that are different from the particles of other substances
 * 6. Temperature affects the speed of the particles. The higher the temperature, the faster the speed of the particles.

Kids acting out The Particle Theory of Matter

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15. Fun chemistry games to play! Try out the Chemistry Hangman one :) [|Various chemistry games]

16. how to calculate the molarity of a solution [|calculating molarity]

CALCULATING MOLARITY :D ! media type="youtube" key="MH0pNcvfsm8" width="425" height="350"


 * __17. Graph a heating curve (temperature vs. time) and interpret with respect to phase changes and phase to matter.__**

In the absence of of reactions that change the molecular structure of a compound, two types of behavior are possible when a compound is heated: the compound can simply get hotter (that is, its temperature increases) or a phase change occur. The transition from the solid phase to the liquid phase is an example of a phase change, which is often called melting. Boiling or vaporization is an example of a phase change from the liquid to the gas phase. [|for more info and graph click this]


 * __18. Identify the Solute and Solvent in a Solution.__**

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 * __19. Calculate the Molarity of a Solution__**

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 * __20. Calculate Specific Heat Capacity Using Calorimetry Data__**

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media type="youtube" key="XwCLvJdVrIs?fs=1" height="385" width="480" Calorimetry is the measurement of the amount of heat evolved or absorbed in a chemical reaction.
 * __21.__ __Calculate Specific Heat Capacity using Calorimetry Data__**

[] [] [|http://www.sciencejoywagon.com/chemzone/review/][|__http://www.youtube.com/watch?v=zz4KbvF_X-0&playnext=1&list=PL93755190845379D7&index=53__] [] http://www.youtube.com/watch?v=HAPc6JH85pM&feature=related [|http://www.youtube.com/watch?v=V9WYweBA6vA][|__http://www.youtube.com/watch?v=V9WYweBA6vA__]