Chemistry Ch. 12.3 and 12.4 Quiz

Crystalline solid (picture)

(an example would be ice cubes)

Amorphous solid (picture)

(ex. glass, rubber, and many plastics)

Concave meniscus (picture)

(the adhesive forces are greater, so the water rises along the container walls)

The force of attraction between molecules that are different.

adhesion

This is an element that exists in different forms at the same state - solid, liquid, or gas.

allotrope

This is a solid in which the particles are not arranged in a regular, repeating pattern. It does not contain crystals.

amorphous solid

Crystalline solids that have atomic unit particles:

atomic solids, covalent network solids, metallic solids

Crystalline solids that have low melting points:

atomic, molecular, metallic (low to very high)

Why does water have a high surface tension?

because its molecules can form multiple hydrogen bonds

Why are phase diagrams different for each substance?

because the normal boiling and freezing points of substances are different

The temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure is called the _____________ _____________.

boiling point

If the cylinder is extremely narrow, a thin film of water will be drawn upward. This is called ____________ ____________.

capillary action

The force of attraction between identical molecules.

cohesion

This is the process by which a gas or a vapor becomes a liquid.

condensation

_____________ is the reverse of vaporization.

condensation

The particles in a solid must be in ____________ ____________.

constant motion

Crystalline solids that have high melting points:

covalent network, metallic (low to very high), ionic

This is a solid whose atoms, ions or molecules are arranged in an orderly, geometric structure.

crystalline solid

Soaps and detergents ____________ the surface tension of water by disrupting the hydrogen bonds between water molecules.

decrease

Viscosity increases/decreases with temperature.

decreases

As temperature decreases, kinetic energy _____________ and velocity _____________.

decreases; decreases

This is the process by which a substance changes from a gas or vapor to a solid without first becoming a liquid.

deposition

_____________ is the reverse of sublimation.

deposition

When _____________ is added or removed from a system, one phase can change into another.

energy

These occur during phase changes.

energy changes

When vaporization occurs only at the surface of a liquid, the process is called _____________.

evaporation

Crystalline solids can be classified into ____________ categories: ____________, ____________, ____________, ____________, ____________.

five; atomic solids, molecular solids, covalent network solids, ionic solids, metallic solids

According to the kinetic molecular theory, individual particles do not have ____________ positions in the liquid.

fixed

Gases and liquids are classified as fluids because they can ____________ and ____________.

flow and diffuse

The _____________ _____________ is the temperature at which a liquid is converted into a crystalline solid.

freezing point

The density of a liquid is ____________ than that of it vapor at the same conditions.

greater

The stronger the attractions between particles, the ____________ the surface tension.

greater

When there are long chains of molecules, there is less distance between atoms on neigboring molecules and, thus, a lesser/greater chance for attractions between atoms.

greater

This is the transfer of energy from an object at a higher temperature to an object at a lower temperature.

heat

In typical liquids, the stronger the intermolecular attractive forces, the ____________ the viscosity.

higher

Molecules with larger particles will have a higher/lower viscosity.

higher

The added energy makes it easier for the molecules to overcome the intermolecular forces that keep the molecules from flowing when there is an increase/decrease in temperature.

increase

Crystalline solid that has ionic unit particles:

ionic solid

Liquids are more/less fluid than gases.

less

How ice melts: when molecules on the surface of the ice absorb enough energy to break the hydrogen bonds, they move apart and enter the _____________ phase.

liquid

The particles in a ____________ can flow to adjust to the shape of the container, but the liquid cannot expand to fill its container.

liquid

The _____________ _____________ of a crystalline solid is the temperature at which the forces holding its crystal lattice together are broken and it becomes a liquid.

melting point

The only crystalline solid that has good conductivity is:

metallic solid

Crystalline solid that has molecular unit particles:

molecular solid

In these solids, the molecules are held together by dispersion forces, dipole-dipole forces, or hydrogen bonds.

molecular solids

Solids are more/less dense than liquids.

more

At 25 degrees celsius and 1 atm of air pressure, liquids are ____________ ____________ than gases.

much denser

Covalent network solids have _____________ covalent bonds (ex. carbon and silicon).

multiple

Which force? For particles at the surface of the liquid, there are no attractions from above to balance the attractions from below.

net attractive force (pulling down on particles at the surface)

Do intermolecular forces have an equal effect on all particles in a liquid? Why?

no - because particles in the middle of the liquid can be attracted to particles above them, below them, and to either side.

Do all liquids have viscosity?

no - there are superfluids that lost their resistance to flow

Are liquids compressible? Why?

no. the change in volume for liquids is much smaller because liquid particles are already tightly packed. an enormous amount of pressure must be applied to reduce the volume of a liquid by a very small amount.

The only atomic solids are ____________ gases.

noble

Most molecular compounds are _____________ solids at room temperature.

not

How does the surface area increase?

particles from the interior must move to the surface

This is a graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure.

phase diagram

States of a substance are referred to as _____________ when they coexist as physically distinct parts of a mixture.

phases

Metallic solids consist of _____________ metal ions surrounded by a sea of mobile _____________.

positive; electrons

A mole of solid particles has as much kinetic energy as a mole of liquid or gas particles at the ____________ temperature.

same

The size and ____________ of the particles also affect viscosity.

shape

When viscosity occurs, the particles in a liquid are close enough for attractive forces to ____________ their movement as they flow past one another.

slow

The surface tends to have the ____________ possible area.

smallest

For something to be a solid rather than a liquid, there must be ____________ attractive forces acting between particles in the solid.

strong

This is the process by which a solid changes directly to a gas without first becoming a liquid.

sublimation (ex. dry ice)

This is the energy required to increase the surface area of a liquid by a given amount.

surface tension (a measure of the inward pull by particles in the interior)

These are compounds that lower the surface tension of water.

surfactants

These 2 things control the phase of a substance:

temperature and pressure

Why do liquids usually diffuse more slowly than gases at the same temperature?

the intermolecular attractions interfere with the flow.

What makes metals malleable?

the mobile electrons

What does the amount of energy required to melt 1 mol of a solid depend on?

the strength of the forces keeping the particles together in the solid

What is the viscosity of a liquid determined by?

the type of intermolecular forces in the liquid, the size and shape of the particles, and the temperature.

What things determine the structures of the lattice and the shape of a crystal?

the type of ions and the ratio of ions

When water vapor molecules lose energy they are more likely to form a hydrogen bond with another water molecule. The formation of a hydrogen bond releases _____________ energy and indicates a _____________ from the vapor phase to the liquid phase.

thermal; change

When a substance is ordinarily a liquid at room temperature, the gas phase is called a _____________.

vapor

The pressure exerted by a vapor over a liquid is called _____________ _____________.

vapor pressure

This is the process by which a liquid changes to a gas or vapor.

vaporization

This is the measure of the resistance of a liquid to flow.

viscosity

Are gases compressible?

yes