Properties of Matter Chapter 2. 2-1: Classifying Matter.
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Transcript of Properties of Matter Chapter 2. 2-1: Classifying Matter.
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Properties of Matter
Chapter 2
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2-1: Classifying Matter
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Pure Substances
Pure substance – matter that always has exactly the same composition Table salt and table sugar are two
examples of pure substances. Substances can be classified into two categories
—elements and compounds.
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Elements
Element – a substance that cannot be broken down into simpler substances
An element has a fixed composition because it contains only one type of atom Examples: The elements oxygen and nitrogen are
the main gases in the air you breathe.
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Elements
Chemists use symbols of one or two letters to represent elements. The first letter is always capitalized. If there is a second letter, it is not capitalized. C represents carbon. Al represents aluminum. Au represents gold.
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Compounds
Compound – a substance that is made from two or more simpler substances and can be broken down into those simpler substances Ex. – Water is composed of the elements
hydrogen and oxygen. Oxygen and hydrogen are gases at room temperature, but water is a liquid.
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Mixtures
Heterogeneous mixture – the parts of the mixture are noticeably different from one another The sand is a
heterogeneous mixture of different kinds of grains.
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Mixtures
Homogeneous mixture – the substances are so evenly distributed that it is difficult to distinguish one substance in the mixture from another The spoon is stainless steel, a homogeneous
mixture of iron, chromium, and nickel.
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Solutions
Solution – The mixture that forms when substances dissolve and form a homogeneous mixture
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2-2: General Properties of Matter
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Matter – anything that has mass and volume Properties – characteristics of matter
Ex. – Color, odor, shape, texture, and hardness
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Mass – The amount of matter in an object The mass of an object does not change unless
some matter is either added to or removed from an object
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Weight – response of mass to the pull of gravity
Gravity – force of attraction between all objects in the universe
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Volume – the amount of space an object takes up Measured in liters (L), milliliters (mL), and cubic
centimeters (cm3) 1 L = 1000 mL or 1000 cm3
______ mL = 3.5 L 3500 mL = 3.5 L
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Density – the mass per unit volume of an object
Densities of Some Common Substances
Substances Density (g/cm3)
Air 0.0013
Gasoline 0.7
Wood (oak) 0.85
Water (ice) 0.92
Water (liquid) 1.0
Aluminum 2.7
Steel 7.8
Silver 10.5
Lead 11.3
Mercury 13.5
Gold 19.3
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2-3: Phases of Matter
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Phase – state in which matter can exist: solid, liquid, gas or plasma
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Solid – matter with a definite shape and a definite volume
Crystal – solid in which the particles are arranged in a regular, repeating pattern
Quartz Sodium Chloride (Table Salt)
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Amorphous solid – solid that loses its shape under certain conditions
Sealing Wax
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Liquid – matter with no definite shape but with a definite volume
Viscosity – the resistance of a liquid to flow Honey has a higher viscosity than water
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Gas – matter with no definite shape or volume
Plasma – high-energy phase of matter Plasma is one of the most common phases of
matter in the universe
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2-4: Phase Changes
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Solid-Liquid Phase Changes
Melting – the change of a solid to a liquid Melting point – the temperature at which a
solid changes to a liquid
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Solid-Liquid Phase Changes
Freezing – the change of a liquid to a solid Freezing point – the temperature at which a
liquid changes to a solid The freezing point of a substance is equal to
its melting point
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Liquid-Gas Phase Changes
Vaporization – the change of a substance from a liquid to a gas
Evaporation – vaporization at the surface of a liquid
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Liquid-Gas Phase Changes
Boiling – the process in which particles inside a liquid as well as those on the surface change to a gas
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Liquid-Gas Phase Changes
Boiling point – temperature at which a substance changes from the liquid phase to the gas phase Boiling point of water –
100 degrees Celsius Boling point of a diamond
– 4200 degrees Celsius
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Liquid-Gas Phase Changes
At high altitudes, air pressure is lower, so the boiling point is reduced. Water will boil at a
temperature lower than 100 degrees Celsius at high altitudes
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Liquid-Gas Phase Changes
Condensation – the change of a gas to a liquid Water vapor in the surrounding air loses heat
energy when it comes in contact with the cold glass
Water vapor condenses and becomes liquid
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Solid-Gas Phase Changes
Sublimation – the surface particles of a solid escape directly into the gas phase Ex. – snow turns to water vapor Ex. – dry ice
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Heat, Temperature, and Phase Changes Heat is energy that causes the particles of
matter to move faster and farther apart. As the particles move faster, they leave one phase and pass into another.
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2-5: Chemical Changes
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Observing Chemical Properties Chemical property – any ability to produce a
change in the composition of matter
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Observing Chemical Properties Two chemical properties:
Flammability – a material’s ability to burn in the presence of oxygen
Reactivity – The property that describes how readily a substance combines chemically with other substances Iron + Oxygen = Rust
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Chemical Changes
Chemical changes – the changes that substances undergo when they change into new and different substances
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Chemical Changes
A change in color is a clue that a chemical change has produced at least one new substance (most of the time) As a match burns, it shrivels up and turns black.
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Physical Property
Physical property can be observed with senses and can be determined without destroying matter
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Physical Changes
Physical change – a change in size, shape, or state of a substance but no new substance is formed