chapter 13 chem
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| to move; Describes the behavior of gases in terms of energy, size, and motion of their particles | kinetic
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| all matter consists of tiny particles that are in constant motion | kinetic theory
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| what are Three assumptions are made regarding the kinetic theory and gases | 1- the particles in a gas are considered to be small, hard spheres with an insignificant volume.
2-the motion of the particles in a gas is rapid, constant and random
3-All collisions between particles in a gas are perfectly elastic.
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| what Two factors determine the kinetic energy(KE) of a particle | mass and velocity
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| reflects both the speed and direction of motion | velocity
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| In a sample of gas, what factors are the same and what is different? | All particles have the same mass
All particles do not have the same velocity
Do not have same KE
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| Measure of the average kinetic energy of the particles in a sample of matter | temperature
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| results from the force exerted by a gas per unit surface area of an object. | gas pressure
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| How does a balloon keep its shape? | The gas pressure is a result of billions of rapidly moving particles in a gas simultaneously colliding with an object
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| Force per unit area | pressure
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| The force exerted by air at any point on the earths surface | atmospheric pressure
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| how does atmospheric pressure vary at different points of the earth | Higher altitude lower atmospheric pressure
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| If there are no particles present then no collision can occur. So there is no pressure, the result is a ________ | vacuum
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| an empty space with no pressure | vacuum
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| why does Air exerts pressure on Earth | because gravity holds particles in air within Earth’s atmosphere
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| the collision of atoms and molecules in the air with objects | atmospheric pressure
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| As you climb a mountain atmospheric pressure decreases because the_______ of the atmosphere decreases. | density
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| device used to measure atmospheric pressure | barometer
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| SI unit for pressure | Pascal (Pa)
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| _______________ and ___________ are also used as measurements of pressure | Millimeters of mercury (Mm Hg) and atmospheres (atm)
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| ____ atm = _____ mmHg = _____ kPa | 1, 760, 101.3
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| What properties of gases make it possible for an air filled flotation device to work? | Low Density
Compression and expansion
Diffusion and effusion
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| compares mass of an object to its volume | density
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| reduce the volume; Large amount of empty space between air particles allows the air to be easily pushed into a smaller volume | compress
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| Air particles fills the available space | expansion
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| ________ ________ of gas particles causes the gases to mix until they are evenly distribute | Random motion
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| Movement of one material through another | diffusion
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| in diffusion, there is a Movement from an area of ________ concentration to an area of ______ concentration | higher; lower
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| in diffusion, Heavier particles are ______ Light particles are _____ | slower, faster
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| Gas escapes through a tiny opening | effusion
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| in effusion there is an Inverse relationship between ______ ______ and ______ ________ | effusion rate; molar mass
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| Can take the shape of its container; Fixed volume | liquid
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| Liquid molecules don’t have ______ positions | fixed
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| ____________ between liquid particles limit their range of motion | Forces of attraction
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| The density of a liquid is much ________ than that of its vapor at the same conditions | greater
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| why is the density of liquid water and steam different | because of the intermolecular force that holds them together
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| Change in volume is much ______ in a liquid than a gas | smaller
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| liquids can be ________ | compressed
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| A LARGE amount of _________ must be added to even slightly change the volume of a liquid | pressure
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| Ability to flow | fluidity
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| liquid_______ more slowly than a gas at the same temperature | Diffuses
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| liquid is less fluid than gas give an example | Water leak stays in the basement unless the amount of water released exceeds the volume of the basement
Gas leak can diffuse through out the house
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| Measure of resistance of a liquid to flow | viscosity
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| viscosity is Determined by the type of _______ ______ involved, the _______ __ ____ _______, and the _______ | intermolecular forces, shape of the particles, temperature
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| The stronger the attractive forces, the_______ the viscosity | higher
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| Viscosity _______ with an increase in temperature | decreases
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| give an example of viscosity and temperature | when you heat up syrup it becomes easier to pour
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| Intermolecular forces _______ have an equal effect on all particles in a liquid | DON’T
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| what are particles in the middle of a liquid attracted to | attracted to particles all around them
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| what are particles on the surface of a liquid attracted to | no attraction from above to balance the attractions from below, Net attractive force pulling down on particles at the surface
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| The stronger the attractions between particles, the _______ the surface tension | greater
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| force of attraction between like molecules | cohesion
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| force of attraction between different molecules | adhesion
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| The movement of a liquid upward | capillary action
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| give an example of capillary action | Example: Paper towels and diapers
Water is drawn into the narrow spaces between the cellulose fibers by capillary action
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| conversion of liquid to gas | vaporization
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| when vaporization occurs at the surface of a liquid that is not boiling. | evaporation
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| During evaporation only the molecules with a certain ______ ________ ______ can escape the surface of the liquid | minimal kinetic energy
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| measure of the force exerted by a gas above a liquid | vapor pressure
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| conversion of gas to liquid | condensation
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| the temperature at which the vapor pressure of a liquid is equal to the external pressure on the liquid | boiling point
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| Normal boiling point | 101.3 kPa
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| Change in altitude affects the boiling point because atmospheric pressure is_______ at higher temperatures | lower
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| sea level water boils at 100 C but in denver it boils at ____ | 95 C
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| A mole of a solid particle has as much ______ _______ as a mole of liquid particles | kinetic energy
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| why do solids have a definite shape a volume? | In a solid there are strong attractive forces between particles These forces limit the movement to vibrations in a fixed location Particles are packed closer together
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| temperature at which a solid turns into a liquid | melting point
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| temperature at which a liquid turns into a solid | freezing point
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| Crystal-particles are arranged in an orderly repeating 3-D pattern called a ______ _______ | crystal lattice
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| smallest arrangement of connected points that can be repeated in three directions to form the lattice | unit cell
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| two or more different molecular forms of an element | allotropes
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| Solid in which the particles are not arranged in a regular repeating pattern ; lacks an ordered structure | amorphous solids
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| when do amorphous solids form usually? | when a molten material cools to quickly example: Glass, rubber and many plastics, Glasses can be considered super-cooled liquids
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| Phase changes that require energy | melting, vaporization, sublimation
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| What does happen to ice cubes in a glass of ice water? | Heat flows from the water to the ice
Heat- transfer of energy from an object at a higher temp to an object at a lower temp
Energy breaks the hydrogen bonds and causes the ice to enter its liquid phase
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| Temperature at which the forces holding a crystal lattice together are broken and becomes a liquid | melting point
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| The process by which a liquid changes to a gas or vapor | vaporization
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| When vaporization occurs only at the surface of a liquid Method by which your body controls its temp | evaporation
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| As temperature________ more molecules are able to escape from the liquid | increases
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| Pressure exerted by a vapor over a liquid (closed container) | vapor pressure
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| Temperature when the vapor pressure of liquid equal s the atmospheric pressure Molecules have enough energy to vaporize | boiling point
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| Process by which a solid changes directly to a gas | sublimation
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| give some examples of sublimation | Solid iodine
Solid carbon dioxide(dry ice)
Solid air fresheners
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| Phase changes that Release Energy | Condensation
Deposition
Freezing
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| The process by which a gas or a vapor becomes liquid Reverse of vaporization Loses energy, velocity is reduced | condensation
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| Process by which a substance changes from a gas or vapor to a solid without becoming a liquid first Reverse of sublimation Example: snowflakes | deposition
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| Heat is removed, molecules lose KE and their velocity decreases When enough energy has been removed, the molecules will stay in fixed position | freezing
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| Temperature at which a liquid is converted into a crystalline solid | freezing point
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| A graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure | phase diagrams
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| The point on a phase diagram that represents the temperature and pressure at which three phases of a substance can coexist | triple point
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| what happens to boiling point when you reach higher altitudes? | High altitudes have lower atmospheric pressure. higher up into the atmosphere= lower air pressure.since the boiling point occurs only when the vapor pressure of the liquid=atmospheric pressure, the boiling point of water will be lower
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