Chemistry

Avogadro’s number

Avogadro’s number

Number of atoms in 1 mol

Approximately 6.02 x 10^23

Hydrocarbons

Substances that contain hydrogen and carbon

Combustion

Exothermic reaction that occurs when oxygen reacts quickly with a substance to form a new substance

Endothermic reaction

Chemical reaction that absorbs energy

Exothermic reaction

Chemical reaction that releases energy

Neutralization

Process in which acids and bases react with each other so that the H+ ion and OH- ion combine to make a single water molecule

Diatomic molecule

Molecule composed of two atoms of the same element

Covalent bond

Bond formed when non-metallic atoms share electrons

Molecule

Group of non-metallic atoms bound together by covalent bonds

Multivalent elements

Element with more than one stable ion

Polyatomic ions

Charged particle made up of several non-metallic atoms joined together

Law of conservation of mass

Total mass of the reactants in a chemical reaction equals the total mass of the products

Salting

Method of drying food to preserve it, salt draws water out of food

Fermentation

Biochemical preservation technique involving bacteria

MSDS

Material safety data sheet

WHMIS

Workplace hazardous materials information system

Hydrated compounds

Compounds that contain water as a part of their structure

Molar mass

Mass of 1 mole of a substance, sum of the atomic masses of all the pieces of the compound

Mole

Specific group of objects

Atom, molecule, eggs

Double replacement reaction

Compound + Compound > Compound + Compound

Single replacement reaction

Compound + Element > Compound + Element

Combustion reaction

Fuel + Oxygen > Carbon Dioxide + Water

Decomposition reaction

Compound > Element + Element

Formation reaction

Element + Element > Compound

Non-Metal ion

Gains electrons, negative charge

Metal ion

Lose electrons, positive charge

Cation

Positive ion

Anion

Negative ion

Ionic compound

Metal + non-metal

Formation of ionic compound

Some elements pick up an extra electron or two or three

Valence shell

The outer shell

Occurrence of chemical bonding

When two particles can exchange or combine their outer electrons in a way that is attractive

Chemical bonding

The interaction of electrons from one atom with the electrons of another atom

Mass number

Mass of the nucleus

# of neutrons = atomic mass - atomic #

Atomic number

Number of protons

Isotope

Different format of the same element, have a different number of neutrons

Noble gases

Group 18

Non-reactive

Halogens

Reactive non-metals in group 17

Transition metals

Group 3-12

Hardness, high density, high melting and boiling points

Alkaline earth metals

Group 2

General white colour, malleable, extrudable, and machineable

Less reactive

Alkali metals

Group 1

Soft and silvery

React vigorously with water and must be stored in oil

Properties of metalloids

State may vary

Colour could vary

May conduct electricity but not well

Could be malleable or ductile

Properties of non-metals

Gas, liquid, solid

Colour differs

Cannot conduct

Not malleable or ductile

Properties of metals

Most solid at room temperature, except mercury

Silver or grey in colour, shiny

Good conductors of heat and electricity

Malleable and ductile

Arrangement of groups

Elements in the same group all share similar physical and chemical characteristics

Arrangement of periods

All elements in the same row have the same energy level

Group

Vertical column

Period

Horizontal row

Demetri Mendeleev

Father of the modern periodic table

Neutron

No charge

Electron

Negative charge

Lightest subatomic particle

Proton

Positive charge

Most of the mass of an atom

The nucleus

Makes up the nucleus

Protons and neutrons

Neils Bohr

Proposed that electrons exist in energy levels

Move in electron shells

Nucleus

Tiny dense center of the atom

Ernest Rutherford

Discovered the nucleus and proposed that electrons move around the nucleus

Hantaro Nagaoka

Suggested that the atom represents the solar system

Raisin bun model

J.J. Thompson’s model

Atom is a positively charged sphere with small negative charges embedded

J.J. Thompson

Atoms seemed to have either a positive or negative charge

Discovered the electron

John Dalton

All matter is made up of small particles called atoms

Aristotle

First ever talked about matter being made up of elements

Atomists

They disagreed with the early Greek views

Early Greeks

Believed that all matter was made of only four things, fire, water, earth and air

Examples of chemical properties

Reaction with acid, ability to burn, behavior in air, reactions to heat, poisonous, toxic, explosive

Examples of physical properties

Melting point, boiling point, hardness, state at room temperature, ductility, malleability

Chemical property

Describes how a substance interacts with other substances such as acids

Physical property

Describes the physical appearance and composition of a substance

Properties

Characteristics that can be used to describe a substance

Sublimation

Solid > Gas

Deposition

Gas > Solid

Gas

Particles are separated by large spaces and move quickly, take shape of the container

Liquid

The particles are touching but can flow past each other, takes shape of the container

Solid

Particles are packed so closely together that they can only vibrate in place

Plasma

Results when a large amount of energy is added to a gas

Determines the state

Temperature

States of matter

Solid, liquid, gas, plasma

Matter

Anything that has mass and takes up space

Colloids

Cloudy mixture where the particles are so small that they cannot be easily separated, milk

Suspensions

Cloudy mixture with tiny particles of one substance held within another, can be separated, tomato juice

Aqueous solution

If dissolved in water

Homogeneous mixture

One substance (solute) is dissolved into another (solvent) creating a substance that looks like one substance, sugar in hot coffee

Heterogeneous mixture

All different parts of the substance are visible

4 types of mixtures

Heterogeneous, homogeneous, suspension, colloid

Mixture

A combination of pure substances that have not chemically combined to form a compound

Compound

Created when 2 or more elements combine chemically in fixed proportions

Elements

Cannot be broken down into any simpler substance, organized into the periodic table

Pure substance

Mad up of only one kind of matter, has a unique set of properties