Chapter 3: Matter and Energy

Physical processes

________ can be used to separate mixtures because there are no chemical interactions between the components.

Bonds

________: Happens when atoms are held together by attractions.

Pure substances

________ that are compounds can be broken down by chemical processes into their elements.

Calorie

________ (cal): Defined as the amount of energy needed to raise the temperature of 1 g of water by 1 °C.

Sugar

________ dissolves in water to form a solution.

Strong attractive forces

________ hold the particles such as atoms or molecules close together.

piece of wood

A(n) ________ burns with a bright flame, and produces heat, ashes, carbon dioxide, and water vapor.

Celsius

Temperatures in science, are measured and reported in ________ (°C) units.

everyday temperatures

In the United States, ________ are commonly reported in Fahrenheit (°F) units.

Condensation

________: The water vapor is converted back to liquid as the water molecules lose kinetic energy and slow down.

Deposition

________: The reverse of sublimation; the gas particles change directly to a solid.

Pepper

________ is ground into flakes.

Filtration

________: It helps in separating solids from liquids, which involves pouring a mixture through a filter paper set in a funnel.

Evaporation

________: It is taking place as water molecules with sufficient energy escape from the liquid surface and enter the gas phase.

Compound

________: A pure substance that consists of atoms of two or more elements, always chemically combined in the same proportion.

nutrition laboratory

In the ________, foods are burned in a calorimeter to determine their energy value.

Freezer Burn

________: This occurs when a solid is left in the freezer for a long time, and so much water sublimes that solids become dry and shrunken.

Gas

________: It does not have a definite shape or volume.

Kinetic energy

________ is lost, the particles slow down, and attractive forces pull the particles close together; therefore, the substance is freezing.

Chromatography

________: Different components of a liquid mixture separate as they move at different rates up the surface of a piece of chromatography paper.

carbohydrate reserves

If the ________ are exhausted, fats and then proteins are used for energy.

Copper

________ is drawn into thin copper wires.

Sublimation

________: The particles on the surface of a solid change directly to a gas with no temperature change and without going through the liquid state.

Physical properties

________: These are those characteristics that can be observed or measured without affecting the identity of a substance.

Atoms

________: These are extremely tiny particles that make up each type of matter.

solid gain

Melting Point: The particles of a(n) ________ sufficient energy to overcome the attractive forces that hold them together.

Liquid

________: It has a definite volume, but not a definite shape.

Carbohydrates

________ are the primary fuel for the body.

tiny pieces of confetti

Paper is cut into ________.

Kelvins

________ (K): The unit of Kelvin Scale, no degree symbol is used.

metal

Shiny, silver ________ reacts in air to give a black, grainy coating.

Specific Heat

________: The amount of heat needed to raise the temperature of exactly 1 g of a substance by exactly 1 °C.

Curve

Cooling ________: A diagram of the cooling process in which the temperature decreases as heat is removed.

Heat Equation

________: Specific heat expression that is arranged to solve for heat.

Chemical properties

________: These are those that describe the ability of a substance to change into a new substance.

State of Matter

________: The physical forms of matter.

Heat Fusion

________: The energy that must be added to convert exactly 1 g of solid to liquid at the melting point.

Kelvin scale

On the ________, 273 °C temperature, is called absolute zero, has the value of 0 K.

solid separate

The particles in the ________ and move about in random patterns.

Homogenous Mixture

________: Also called a solution, the composition is uniform throughout the sample.

large mass of water

A(n) ________ near a coastal city can absorb or release five times the energy absorbed or released by the same mass of rock near an inland city.

Pure Substances

________: A matter that has a fixed or definite composition.

Matter

Anything that has mass and occupies space

Pure Substances

A matter that has a fixed or definite composition

Element

The simplest type of pure substance

Atoms

These are extremely tiny particles that make up each type of matter

Compound

A pure substance that consists of atoms of two or more elements, always chemically combined in the same proportion

Bonds

Happens when atoms are held together by attractions

Molecules

Small groups of atoms

Homogenous Mixture

Also called a solution, the composition is uniform throughout the sample

Heterogeneous Mixture

The components do not have a uniform composition throughout the sample

Filtration

It helps in separating solids from liquids, which involves pouring a mixture through a filter paper set in a funnel

Chromatography

Different components of a liquid mixture separate as they move at different rates up the surface of a piece of chromatography paper

State of Matter

The physical forms of matter

Solid

It has a definite shape and volume

Liquid

It has a definite volume, but not a definite shape

Gas

It does not have a definite shape or volume

Physical properties

These are those characteristics that can be observed or measured without affecting the identity of a substance

Chemical properties

These are those that describe the ability of a substance to change into a new substance

Degrees

Smaller units of temperature

Kelvins (K)

The unit of Kelvin Scale, no degree symbol is used

Energy

The ability to do work

Kinetic Energy

The energy of motion

Potential Energy

Determined by the position of an object or by the chemical composition of a substance

Heat

The energy associated with the motion of particles

Joule (J)

The SI unit of energy and work

Calorie (cal)

Defined as the amount of energy needed to raise the temperature of 1 g of water by 1 °C

Specific Heat

The amount of heat needed to raise the temperature of exactly 1 g of a substance by exactly 1 °C

Heat Equation

Specific heat expression that is arranged to solve for heat

Change of State

It occurs when the matter is converted from one state to another

Melting Point

The particles of a solid gain sufficient energy to overcome the attractive forces that hold them together

Freezing Point

Occurs when a liquid changes to a solid

Heat Fusion

The energy that must be added to convert exactly 1 g of solid to liquid at the melting point

Evaporation

It is taking place as water molecules with sufficient energy escape from the liquid surface and enter the gas phase

Boiling Point (bp)

The molecules within a liquid have enough energy to overcome their attractive forces and become a gas

Condensation

The water vapor is converted back to liquid as the water molecules lose kinetic energy and slow down

Sublimation

The particles on the surface of a solid change directly to a gas with no temperature change and without going through the liquid state

Deposition

The reverse of sublimation; the gas particles change directly to a solid

Freezer Burn

This occurs when a solid is left in the freezer for a long time, and so much water sublimes that solids become dry and shrunken

Heat of Vaporization

The energy that must be added to convert exactly 1 g of liquid to gas at its boiling point

Cooling Curve

A diagram of the cooling process in which the temperature decreases as heat is removed

calorimeter

In the nutrition laboratory, foods are burned in a _______ to determine their *energy value.*

energy values

The _____ for food are the kilocalories or kilojoules obtained from burning 1 g of carbohydrate, fat, or protein.

Specific Heat Formula