Chemistry Honors Chapter 10 States of Matter

Volatile

(Of a substance) easily evaporated at normal temperatures.

Normal Boiling Point

Boiling point at 1 atmosphere of pressure. Water is about 100⁰ C. Energy must continuously be added to keep a liquid boiling.

Definite Melting Point

When a solid gets to a certain point that it will melt.

KE=1/2mv² #kg.=1,500 g.(1 kg./1,000 g.)=1.5 kg. 17,500=1/2(1.5)v² 17,500=0.75v² v²=23,333.33 v=152.75 m/s.

A 1,500 gram moving ball has 17,500 Joules of kinetic energy. Determines its velocity in meters per second. Show your work!

250 g. water->gas 40.79 KJ/mol. # mol. water=250 g. H₂O(1 mol. H₂O/18.02 g. H₂O)=13.87 mol. H₂O 13.87(40.79) 565.9 KJ.

A beaker holds 250 grams of water. How much energy would be required to completely vaporize the water? Show your work!

Transformer

A device that drops the voltage.

Equilibrium

A dynamic condition in which two opposing changes occur at equal rates in a closed system.

Real Gas

A gas that does not behave completely according to the assumptions of the kinetic-molecular theory. Polar gases will have greater forces of attraction than nonpolar gases. These molecules are more likely to attract one another which doesn't obey the KMT.

Phase Diagram

A graph of pressure versus temperature that shows conditions under which the phases of a substance exist. Triple point happens when you have all three states of matter at once. Pressure can turn solid ice into water.

Supercooled Liquid

A liquid that instantly freezes when opening it from a freezer.

Effusion

A process by which gas particles pass through a tiny opening.

Surface Tension

A property common to all liquids which is a force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size.

Amorphous Solids

A solid in which particles are randomly arranged. The first word is Greek for "without shape". No regular pattern. Typically form from a cooling process such as glass, plastics, and igneous rocks. Some are used as structural materials, light bulbs, optical fibers, and transformer cores. These solids are also used in lights and windows. More recently made these solids are used in semiconductors such as solar cells, copiers, laser printers, and flat panel monitors.

Polar molecules would not behave ideally because polar molecules have a higher probability of sticking together.

Nonpolar molecules are most likely to be ideal. Why would polar molecules not behave ideally?

Crystal

A substance in which the particles are arranged in an orderly, geometric, repeating pattern.

Kinetic-Molecular Theory

A theory used to explain the behavior of atoms. States that particles of matter are always in motion. As temperature increases, particles will move faster. As temperature decreases, particles will move slower. At the same temperature, larger molecules will move slower than smaller particles. Explains the properties of solids, liquids, and gases.

Capillary Action

The attraction of the surface of a liquid to the surface of a solid, is a property closely related to surface tension.

Liquids

Although it may seem that this state of matter are the most common state of matter, they're actually the least common. It can only exist with a narrow range of temperatures and pressures. They have definite volume, but indefinite shape (it takes the shape of its container). Like gases, particles in this state of matter are constantly in motion, however they are much closer together. Attractive forces between these are more effective. Intermolecular forces exists! Some molecules can overcome these forces and become gases. Think about evaporation or the bubbles in a glass of water. They are more ordered than gases. Due to stronger attraction and lower mobility of particles. Most of them flow downhill. Due to gravity. Some can flow uphill. Helium is this state of matter is near absolute zero.

Phase

Any part of a system that has uniform composition and properties.

Temperature and Phase Change

As a substance changes state, the temperature of the substance remains the same until all of the substance has changed state. An example is when boiling water remains at 100⁰C until all liquid has become a gas, then the temperature can rise.

Formation of Solids

As liquids are cooled, the average energy of the particles decreases. When the energy is low enough, the attractions of the particles pulls them into a more orderly configuration.

It becomes less dense.

As water freezes, what happens to its density?

Condensation

The change of state from a gas to a liquid. It happens with the bubbles of a glass, taking a steamy show, rain clouds, and drawing pictures on the windows of a bus.

Deposition (Desublimation)

The change of state from a gas to a solid.

Velocity

Based on the Kinetic Energy equation, what has a greater effect on kinetic energy?

I can conclude that "kinetic" means movement.

Based on these observations, what can you conclude about the meaning of "kinetic"?

There is space, fills container, and arrows and lines show movement. Drawing on right.

Based on what the KMT says about gases, draw what a container of gas molecules may look like? Explain your answer.

Drawing of a liquid on right.

Based on what the KMT says about liquids, draw what a container of liquid molecules may look like?

Drawing of a solid on right.

Based on what the KMT says about solids, draw what a container of solid molecules may look like?

Sublimation

The change of state from a solid to a gas.

Melting

Change from a solid to a liquid.

Elastic Collision

Collisions between gas particles and between particles and container walls. A collision in which there is no net loss of kinetic energy.

Covalent Molecular

Covalent molecules held together by intermolecular forces, low melting points.

Ideal

Determine if the the molecule, methane, CH₄ would likely behave as ideal (I) or real (R) gases.

Ideal; It's an ideal gas because it's symmetrical and the arrows cancel out as shown on the image to the right.

Determine if the the molecule, methane, CO₂ would likely behave as ideal (I) or real (R) gases. Why?

Real; It's a real gas because it's not symmetrical and has opposite charges as shown on the image to the right.

Determine if the the molecule, methane, H₂O would likely behave as ideal (I) or real (R) gases. Why?

Real

Determine if the the molecule, methane, NH₃ would likely behave as ideal (I) or real (R) gases.

KE=1/2mv² KE=1/2(5)(35²) KE=5/2(1,225) KE=3,062.5 J.

Determine the amount of kinetic energy in a 5 kg ball travelling horizontally at a speed at 35 m/s.

Kinetic Energy (KE)

Energy possessed by moving objects.

They're the same.

For crystalline solids, what are their melting and freezing points.

Yes, if you get the right temperature and pressure at the triple point, then a solid, liquid, and gas can happen at the same time.

Is it possible to have a container of water that contains the solid, liquid, and gas state at the same time? Why?

Enthalpy

Heat energy.

KE=1/2mv² m=mass (kg) v=velocity (m/s) Measured in joules (J) All gases at the same temperature have the same kinetic energy.

How can KE be calculated?

The larger the molecule is, the slower it will diffuse and effuse. When the dogs go outside, the little pups easily get through the dog door than the mom pup. Image on right.

How does effusion work?

At ground level, there's zero kinetic and potential energy. At the top, there's high potential and 0 kinetic energy. At point B, there is 0 potential energy and high kinetic energy. Once you reach the highest point, you can't go up the same or higher height than the same hill because you don't have as much energy. Energy gets lost due to friction.

How does kinetic energy work according to this diagram?

Viscosity

How fast a liquid flows and how thick it is.

1,000 g.

How many grams are in 1 kilogram?

47 g. ice->gas 40.79 KJ/mol. # mol. water=47 g. H₂O(1 mol. H₂O/18.02 g. H₂O)=2.61 mol. H₂O 40.79 KJ/mol. H₂O(2.61 mol. H₂O) 106.39 KJ.

How much energy is absorbed when 47.0 g. of ice boils at STP? Show your work!

47 g. ice->water 6.009 KJ/mol. # mol. water=47 g. H₂O(1 mol. H₂O/18.02 g. H₂O)=2.61 mol. H₂O 6.009 KJ/mol. H₂O(2.61 mol. H₂O) 15.67 KJ.

How much energy is absorbed when 47.0 g. of ice melts at STP? Show your work!

A single atom or molecule would possess a small kinetic energy because they're so small.

How much kinetic energy do you think a single atom or molecule would possess?

If it follows the rule, then it's an ideal gas. If not, then it's a real gas. It mostly breaks the fourth rule such as ammonia.

How to distinguish between ideal and real gases?

These conditions are ideal because under high temperature, molecules move faster which means it's harder to stick together. With low pressure, that means that the molecules are more spread out and less condensed.

Ideal gases tend to exist at high temperature and low pressure. Why are these conditions ideal?

Movement and Kinetic Sand

In what ways have you heard/seen the word "kinetic" used?

Critical Point

Indicates the critical temperature and pressure.

Triple Point

Indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance coexist at equilibrium.

Molar Enthalpy of Fusion

It's another word for melting. The amount of heat required to melt one mole of solid at the solid's melting point. It's represented in this equation, ∆Hf. Stronger attractions result a higher result.

Fluids

Liquids and gases are considered this because they flow. The ability for a gas to be flowed.

Evaporation (Vaporization)

Liquids will eventually turn into a gas.

Covalent Network

Multiple atoms covalently bonded together, very hard, high melting points.

Unlike ideal gases, these conditions are best for real gases because under low temperature, molecules move slower which means it's easier to stick together. With high pressure, that means that the molecules are less spread out and more condensed.

Real gases exist in high pressures and low temperatures. Why are these conditions best for real gases?

Metallic

Sea of electrons, good conductors.

Ionic

Structured, brittle and good insulators.

Diffusion

Such spontaneous mixing of the particles of two substances caused by their random motion.

Molar Enthalpy of Vaporization

The amount of energy that is needed to vaporize one mole of liquid at the liquid's boiling point at constant pressure. It's represented in the equation, ∆Hv. The stronger the attraction between molecules, the higher it will be. Water has this relatively high due to its hydrogen bonding.

Potential Energy

The counterpart of KE. Stored energy.

Elastic Energy

The energy stored in an object when the shape of the object is changed. The ability to resist a distorting influence and to return to its original size and shape when that influence or force is removed.

Critical Pressure

The lowest pressure at which the substance can exist as a liquid at the critical temperature (water=217.75 atm).

Temperature

The measure of kinetic energy.

Compressibility

The opposite of fluidity.

Freezing

The physical change of a liquid to a solid by removal of energy. All liquids have that ability (just at different temperatures).

Unit Cell

The smallest portion of a crystal lattice that shows the 3-D structure.

Critical Temperature

The temperature above which the substance cannot exist in the liquid state (water=373.99⁰C).

Boiling Point

The temperature at which the equilibrium vapor pressure of a liquid equals the atmospheric pressure.

Freezing Point

The temperature at which the solid and liquid are in equilibrium at 1 atm pressure. The loss of energy results in a solid being formed.

Crystal Structure

The total three-dimensional arrangement of particles of a crystal.

Lower atmospheric pressure=lower boiling point; Increasing pressure will increase the temperature of a liquid. An example is a pressure cooker. It's when you put your roast or chicken and put your lid. Boiling point affects pressure.

What does lower atmospheric pressure mean? Explain and provide an example.

Optical Fibers

These are used for high speed internet.

Solids

These particles are more closely packed together. Intermolecular forces are much more effective. Attractive forces hold particles in a relatively fixed position, with only vibrational movements. They have vibration motion, but they cannot move freely. Most organized and most attractive forces. They have low energy, high organization, and high attraction.

Crystalline Solids

These solids consists of crystals. Contain organized, geometric patterns. Most compounds are crystalline. The total 3-D arrangement of particles. Represented by a coordinate system called a lattice.

It takes longer to boil than to melt because it takes much more energy to separate them than to have motion.

Using the heating curve graph, which takes longer between boiling and melting water why?

Equilibrium Vapor Pressure of a Liquid

Vapor molecules exert a pressure proportional to the concentration of molecules in the vapor phase. The more volatile a substance is, the higher its vapor pressure will be. These substances evaporate quicker than gasoline. This is due to relatively weak forces of attraction between their particles. Nonvolatile liquids tend to evaporate very slowly. It's intermolecular forces can affect it. Strong IMF=Less Volatile=Lower VP. The arrow represents pressure. A gas has a weak IMF which is more volatile and a higher VP.

Glasses, Plastics, and Magma

What are examples of amorphous solids?

O₂, HH₃, and H₂O

What are examples of covalent molecular crystals?

SiO₂ and Diamond

What are examples of covalent network crystals?

The smell has the ability to spread through such as cooked brownies and poop in your shoes.

What are examples of diffusion?

Melting Point: 0⁰C Boiling Point: 100⁰C Enthalpy of Fusion: 6.009 kJ/mol Enthalpy of Vaporization: 40.79 kJ/mol.

What are key information of water?

1. Gases consist of large numbers of tiny particles that are far apart relative to their size. 2. Collisions between gas particles and between particles and container walls are elastic collision. 3. Gas particles are in continuous, rapid, random motion. They therefore possess kinetic energy which is energy of motion. 4. There are no forces of attraction between gas particles. 5. The temperature of a gas depends on the average kinetic energy of the particles of the gas.

What are the 5 assumptions of the Kinetic-Molecular Theory of gas?

Ionic, Covalent Network, Metallic and Covalent Molecular

What are the four types of crystalline solids?

Expansion, Fluidity, Low Density, Compressibility, Diffusion, and Effusion

What are the physical properties of a gas?

Relatively High Density, Relative Incompressibility, Ability to Diffuse, Surface Tension, Evaporation, Boiling, Capillary Action (Chromatography and Meniscus), and Viscosity

What are the properties of liquids?

Definite Shape and Volume, Definite Melting Point (Supercooled Liquids), High Density and Incompressibility, and Low Rate of Diffusion

What are the properties of solids?

Melting, Sublimation, Freezing, Vaporization, Condensation, and Deposition

What are the six changes of state?

Syrup and Honey

What are things that are viscous?

Velocity determines the direction.

What's the key difference between speed and velocity?

They fill their space.

What happens when a gas expands?

Compressing a solid is gonna break. It is not gonna compress unless it has air.

What happens when you try to compress a solid? When will it compress?

Water is an example of a crystalline solid.

What is an example of a crystalline solid?

Metals

What is an example of a metallic crystal?

NaCl

What is an example of an ionic crystal?

Evaporation is a process by which liquid changes to its vapors at a temperature below its boiling point, while vaporization is a process by which liquid changes to its vapors at its boiling point. Evaporation takes place at all temperatures, while vaporization takes place at only fixed temperature i.e. (that is) its boiling point temperature. During evaporation temperature may change while temperature during vaporization does not change. Evaporation is a slow and silent process while vaporization is a fast and violent process. Evaporation takes place only at surface of liquids while vaporization takes place over the entire mass of the liquid. Evaporation doesn't have to open at the boiling point.

What is the difference between evaporation and vaporization?

Pressure

When a gas hits a container wall.

Ideal Gas

When looking at gases, the KMT (aka Kinetic Molecular Theory) provides a model of this type of gas. A hypothetical gas that perfectly fits all the assumptions of the KMT. These gases follow the assumptions of the KMT.

It's going up.

Where is the atmospheric pressure going according to the diagram?

Melting, Sublimation, and Evaporation

Which changes of state absorb (gaining) energy?

Freezing, Condensation, and Deposition

Which changes of state give off (losing) energy?

KE=1/2(0.6)(90²) KE=0.3(8,100) KE=2,430 J. KE=1/2(3)(60²) KE=1.5(3,600) KE=5,400 J. KE=1/2(10)(27.78²) KE=5(771.6049) KE=3,858 J. Number 2 would have the greatest kinetic energy.

Which of the following has the greatest kinetic energy? A 600 gram ball traveling 90 m/s. A 3 kg. ball traveling 60 m/s. A 10 kg. ball traveling 100 km/hr. Show your work!

A gas has a low density because of the equation m/v. If I have a high volume, then the density is lower.

Why does a gas have a low density?

Water will form at the bottom because that's where the heat sources are at.

Why will water form at the bottom?