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