Studied by 2 people
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
