H Chem / Chem 2013. Notes – Chap 2 Properties of Matter.

H Chem / Chem 2013

Notes – Chap 2

Properties of Matter

Matter - Anything that takes up space, has mass, and applies

inertia.

1)Mass - Measures the amount of matter

Matter - Anything that takes up space, has mass, and applies inertia.

Weight - The gravitational force of attraction exerted by the earth on a body

(SI – Newton)

1) Mass - Measures the amount of matter

Matter - Anything that takes up space, has mass, and applies inertia.

2) Volume – The amount of

space an object occupies

Matter - Anything that takes up space, has mass, and applies inertia.

3) Inertia - It is the resistance to change in motion. Causes a body at rest to stay at rest, and when in motion to continue in motion.

Matter - Anything that takes up space, has mass, and applies inertia.

3)Inertia - It is the resistance to

change in motion. Causes a body at rest to stay at rest, and when in motion to continue in motion.

Energy - The ability to do work. This can be changed from one form to another, but

cannot be created or destroyed.

Examples - Light, heat, chemical, mechanical, nuclear

Types of Matter

• Atoms - The building blocks of matter. “Atomos” – its name means “uncut”. It is the smallest part of an element which has the properties of that element.

Types of Matter

• Example:H C

O

Fe Au

• Element - The simplest form of matter. It cannot be changed to another form by chemical change, and has only one kind of atom.

Types of Matter

• Example:H CHydrogen Carbon

O Oxygen

Fe AuIron Gold

• Element - The simplest form of matter. It cannot be changed to another form by chemical change, and has only one kind of atom.

Types of Matter

• Element - The simplest form of matter. It cannot be changed to another form by chemical change, and has only one kind of atom.

Types of Matter

• Substance - Name for matter like elements and compounds because of their uniform and definite composition as well as distinct properties

HydrogenOxygen

Silver Gold

NaCl – Table Salt

Hydrogen

Oxygen

SilverGold

• Chemical bond –Force of attraction between two atoms

• Molecule- The smallest particle of a material that can be identified as that material. It is made up of two or more atoms, but they may be the same type of atoms. Held together with a chemical bond

Types of Matter

H2 – Hydrogen molecule

NaCl – Table Salt molecules

• It includes:

H20 NaCl

O2 CO2

N2

• Molecule- The smallest particle of a material that can be identified as that material. It is made up of two or more atoms, but they may be the same type of atoms. Held together with a chemical bond

Types of Matter

• It includes:

H20 NaCl Water salt

O2 CO2

oxygen gas carbon dioxide

N2

nitrogen gas

• Molecule- The smallest particle of a material that can be identified as that material. It is made up of two or more atoms, but they may be the same type of atoms. Held together with a chemical bond

Types of Matter

H2 – Hydrogen gas

O2 – Oxygen gas

NaCl – Table Salt

• Chemical formulas –• Abbreviated form of

elements and compound showing the element symbols and numbers and ratios of atoms

• Examples-• He• CO2

• H2O

• NaCl• NaHCO3

Types of Matter

• Chemical formulas –• Abbreviated form of

compound showing the element symbols and ratio of atoms

• Examples-• He - Helium• CO2 –carbon dioxide

• H2O - water

• NaCl – sodium chloride (salt)

• NaHCO3 – sodium bicarbonate (baking soda)

Types of Matter

• Compound - A substance which cannot be broken into smaller substances by physical changes. It is composed of two or more different elements chemically combined in certain fixed proportions.

• Example:H20

NaClC6H12O6

C8H24O8

• Compound - A substance which cannot be broken into smaller substances by physical changes. It is composed of two or more different elements chemically combined.

• Example:H20 - water

NaCl – salt C6H12O6 – sugar

C8H24O8 - gasoline

Table Salt

NaCl- Sodium Chloride

• Mixtures - Any matter which contains more than one kind of molecule that is not chemically combined and can be separated physically. Not pure substances.

• The substances retain their individual properties

• Example: Sand, salad, salted water, air, mixed nuts

Types of Matter

• Solution - A special mixture formed when one kind of material (usually water) fills the space between the particles of another material.

Examples: Salt water, coffee, orange juice

Types of Matter

• Solution - A special mixture formed when one kind of material (usually water) fills the space between the particles of another material.

Solution are said to be: Homogeneous mixtures –

they look the “same” throughout

Mixtures that look “different” are called:

Heterogeneous mixtures

Examples: Salt water, coffee, orange juice

Types of Matter

• Solution - A special mixture formed when one kind of material (usually water) fills the space between the particles of another material.

Examples: Salt water, coffee, orange juice

Solution are said to be: Homogeneous mixtures

– they look the “same” throughout

Mixtures that look

“different” are called:Heterogeneous mixtures

Types of Matter

Solution are said to be: Homogeneous

mixtures – they look the “same” throughout

Mixtures that

look “different” are called:

Heterogeneous mixtures

Types of Matter

Solutions

• Solutions consist of one or more solutes and a solvent.

• Solute – the dissolved substance in a solution. Salt in salt water is a solute

• Solvent – The dissolving agent in a solution. Water dissolving salt in salt water is an example

• Aqueous – Solutions which are actually water based

• Colloid – The type of mixture which contains small particles suspended in a solution

Solutions

• Aqueous – Solutions which are actually water based

• Colloid – The type of mixture which contains small particles suspended in a solution– Tyndall effect : The

scattering of light indicating small solid particles

Solutions

Solutions

• Suspension - A type of heterogeneous mixture where the solid particles are large enough to settle out or can be separated by filtration. The process that separates solids from a liquid

Solutions

• Separation of solutes from homogeneous mixtures can be accomplished by distillation.

• The process where a liquid is boiled to produce a vapor that is condensed to a liquid.

Solutions

• Separation of solutes from homogeneous mixtures can be accomplished by distillation.

• The process where a liquid is boiled to produce a vapor that is condensed to a liquid.

States of Matter (4)Determined by the amount of energy

in their moving particles.

States of Matter (4)

1) Solids -State of matter which maintains a constant volume and shape. Normally has a crystalline structure.

Example: Ice, Rocks and Minerals

Solids

States of Matter (4)

2) Liquids – State of matter which takes the shape of its container and has a relatively constant volume.

Example: Water,

Mercury

States of Matter (4)

3) Gases -State of matter with no constant shape and whose volume varies with temperature and pressure.

Vapor – Gaseous state of a substance that is generally a liquid or solid at room temperature.

Ex: Water vapor

Example: Air, Oxygen,

Water vapor

Water vapor (steam)

States of Matter (4)

4) Plasma - State of matter similar to gas, made up of electrical particles at extremely high temperatures. It is found in the sun and stars.

Changes of State

• Melting -solid to liquid (ice to water)

• Fusion (freezing) -liquid to solid(water to ice)

• Evaporation - liquid to gas (water to steam/water vapor)

• Condensation - gas to liquid (water vapor to water)

• Sublimation - solid to gas (ice to water vapor)

Changes of Matter

• Physical Change -When a substance is changed to a new form, but its molecules are the same as before, and it can be changed back physically.

• Includes density, melting, boiling, texture, color, flexibility

• Examples: When substances are bent, smashed, ripped, melted, frozen, etc. Ripping a piece of paper, melting ice.

Special Properties of Matter

• Density – The amount of matter (mass) in a given volume. It is how much something weighs versus how much space it takes up

• Measured in grams per milliliter (g/mL) or grams per cubic centimeter (g/cm3).

• Examples: Water has a density of 1 g/mL wood is .7 g/mLiron is 7.8 g/mL.

Special Properties of Matter

• Measured in grams per milliliter (g/mL) or grams per cubic centimeter (g/cm3).

• Examples: Water has a density of 1 g/mL wood is .7 g/mLiron is 7.8 g/mL.

Changes of Matter

• Chemical Change - When a substance is changed to a new form, but its molecules are different from before, and can’t be changed back.

• Describes its ability to change. Flammability, ability to react

• Examples: When substances are burned or chemically react. Burning paper, iron rusting, fireworks exploding.

Chemical Changes

• Chemical properties – The ability of a substance to undergo chemical change

• Chemical reaction – When one or more substances change into two or more substances– Reactant : Substance present

at the beginning of a reaction– Product: Substance produced

in the reaction

Reactants Products

Chemical changes

• Evidence of chemical change:

1) Transfer of energy (warm or cold)

2) Change in color3) Production of a gas4) Formation of a

precipitate (solid from a liquid mixture)

Law of Conservation of Mass

• During a chemical reaction, the mass of the products is always equal to the mass of the reactants.

• Mass is neither created nor destroyed, only changed to a different form .