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