Chemistry - Chapter 13.1 - 13.2 Study Guide
101.3 kPa
1 atm = _____ kilopascal (kPa)
760 mmHg; 7.501 mmHg
1 atm = _____ millimeters of mercury (mmHg); 1 kPa = _____ millimeters of mercury (mmHg)
14.7 psi; 0.145 psi
1 atm = _____ pounds per square inch (psi or lb/in²); 1 kPa = _____ pounds per square inch (psi or lb/in²)
760 torr; 7.501 torr
1 atm = _____ torr; 1 kPa = _____ torr
0.009869 atm
1 kPa = _____ atmosphere (atm)
Barometer, Manometer
A _____ is used to measure atmospheric pressure and a _____ is used to measure gas pressure in a closed container
Physical Property
A characteristic of matter that can be observed or measured without changing the sample's composition
Elastic Collision
A collision in which no kinetic energy is lost
Atmosphere (atm)
A common measurement for air pressure
Hydrogen Bond
A dipole-dipole attraction that occurs between molecules containing a hydrogen atom to a small, highly electronegative atom with at least one lone electron pair
Gas
A form of matter that flows to conform to the shape of its container, fills the container's volume, and is easily compressed
Temperature
A measure of the average kinetic energy of the particles in a sample of matter
Barometer
An instrument used to measure atmospheric pressure
Dipole-Dipole Force
Attractions between oppositely charged regions of polar molecules
Chemical property has to do with the identity of a gas and Physical property has to do with how the gas behaves
Compare and contrast the chemical and physical properties of gases:
The large amount of empty space between gas particles allows them to be squeezed, or pushed, into a smaller volume. Once the pressure is stopped, the particles expand to the original volume.
Describe Compression and Expansion for gases:
Because there are no significant forces of attraction between gas particles, gases flow easily past one another. This random motion allows gases to mix until they are evenly distributed. The movement of gas particles past one another is called diffusion. The process of allowing a gas to escape from a more concentrated container is called effusion.
Describe Diffusion and Effusion for gases:
Gases have low density (mass per unit volume) in comparison to solids. The difference in density is partly due to the mass of the particles and also because there is a great deal of space between gas particles.
Describe Low Density for gases:
Due to individual gas particles having little mass, they exert little pressure. With many gas particles colliding in a container, the pressure can be high.
Describe pressure as it relates to the behavior of gases:
Kinetic-Molecular Theory; 1860; Ludwig Boltzmann & James Maxwell
Describes the behavior of matter in terms of particles in motion; When was it devised?; By who?
Dipole Moment (μ) [μ = Qd]
Describes the strength of the dipole
1. Size is very small. It is assumed that there are no significant attractive or repulsive forces among gas particles. 2. Motion is constantly moving in a random pattern. It is assumed that gas particles move in a straight path until they hit an object. 3. Energy is conserved. It is assumed that mass and velocity impact the energy level of a gas particle.
Distinguish between the three main physical properties of gas particles:
Kelvin
Doesn't have a degree symbol and is the SI unit for temperature
Pressure
Force per unit area
Intermolecular Forces
Forces that are weaker than intramolecular forces when bonding between molecular structures
Intramolecular Forces
Forces that hold particles in ionic, covalent, and metallic bonds together
Khaos
Gas comes from what greek word?
Polar Molecules
Have high boiling points and are usually solids at room temperature
Nonpolar Molecules
Have low boiling points and are usually gases or liquids at room temperature
Charge; Distance between Atoms
In "μ = Qd", what does "Q" stand for?; What does "d" stand for?
Polar Molecules
In most cases, polar bonds produce _____
Plasma
Is composed of electrons and positions ions at a very high temperature
Diffusion
Is used to describe the movement of one material through another
Kinetic Energy
KE, Energy of motion
Solid, Liquid, Gas, & Plasma
List the 4 Phases of Matter:
Dispersion; Dipole-Dipole; Hydrogen Bond
List the Intermolecular Forces
Ionic, Covalent, Metallic
List the Intramolecular Forces:
Low Density, Compression and Expansion, Diffusion and Effusion
List the Properties of Gases:
Kinetic
Means "to move"
Intra-; Inter-
Means "within"; Means "between"
Temperature, kinetic energy
Motion or kinetic energy is proportional to _____. The greater the temperature the greater the _____.
Water
Name a Polar Molecule:
Polar Covalent Bond
Occurs when a pair of different elements covalently bonded has one atom, which attracts the shared pairs more strongly than does the other
Heavier
Smaller mass molecules move faster than _____ mass molecules
Vapor
Something that was a solid or liquid at room temperature
Graham's Law of Effusion
States that the rate of effusion for a gas is inversely proportional to the square root of its molar mass
Dalton's Law of Partial Pressures
States that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture
Pascal (Pa); Newtons
The SI unit of pressure that is equal to 1 N/m²; What does the "N" stand for?
Mean Free Path
The average distance a molecule travels between collisions
Composition
The essential characteristic for determining the chemical and physical properties of matter that means "the types of atoms present"
Structure
The essential characteristic for determining the chemical and physical properties of matter that means "their arrangement"
Dipole Amount
The higher the _____, the higher the melting point and boiling point
Temperature, Mass
The mean free path for molecules varies with _____ and _____
Magneto Hydrodynamics
The study of Plasma
Van der Waals forces
Weak attractive forces between the nucleus of one atom and the electron of another atom. Are intermolecular forces and are between non-bonded atoms.
Dispersion Forces
Weak forces that result from temporary shifts in electron clouds
1 kg (m²/s²)
What is 1 Joule equivalent to?
Positive nuclei and shared electrons
What is the Basis of Attraction for Covalent forces?
Oppositely charged regions of polar molecules (Permanent)
What is the Basis of Attraction for Dipole-Dipole forces?
Cations and Anions (Transfer of Electrons)
What is the Basis of Attraction for Ionic forces?
Metal cations and mobile electrons (Delocalized electrons)
What is the Basis of Attraction for Metallic forces?
4.5 x 10⁹ times a second
What is the Mean Free Path of Oxygen?
K = °C + 273.15
What is the equation for converting Kelvin into Celsius?
Joule (J)
What is the unit for Kinetic Energy?
Kilogram (kg)
What is the unit for Mass?
Meters per sec (m/s)
What is the unit for Velocity?
-273 °C, 0 K
What is the value for absolve zero in °C and K?
Robert Hooke
Who proposed the Kinetic Theory?
Polarity
_____ is directly related to difference between electronegativities
Mass
m, Amount of matter
Absolute Zero
the temperature at which all molecular motion ceases
Velocity
v, Reflects both the speed and the direction of motion
