CHEMISTRY REVIEW

MATTER

What is Chemistry

• Chemistry - the study of the structure, composition and properties of matter & how matter interacts with other matter

• Matter – anything that has mass and occupies space (has volume)

PROPERTIES OF MATTER:

Physical Properties Can be determined without altering chemical composition of the

substance.• Qualitative properties are observed with the senses (not measured).

• Ex. colour, odour, taste, lustre, malleability, ductility, viscosity, form, texture.• Quantitative properties are numerical measurements.

• Ex. density, boiling/melting point, solubility, volume, weight.

Chemical Properties Describe how matter behaves in the presence of other substances,

or when subjected to fire, heat, light, pressure or electricity.

Ex. - magnesium reacts with hydrochloric acid to produce hydrogen gas - glass does NOT react to this acid

Classifying MatterClassifying Matter

MATTER

HomogeneousCompoundElements Heterogeneous

Pure Substances

Made of 1 component…

Mixtures

Made of more than 1 component…

Has one kind of atom.

Eg. Copper, gold, oxygen

Has more than one kind of atom bonded in a fixed ratio called a molecule

Eg. Water, CO2

Contains one evenly mixed ‘phase’ – looks like 1 thing.

Eg. Solution

Contains more than one unevenly mixed ‘phase’ – you can see the individual parts.

The Periodic Table

The Periodic Table

• There are 118 elements on the Periodic Table. 92 of them are naturally occurring.

• All matter in the universe is made up of at least 1 element.

How is it Organized?

Periods: (horizontal rows) • Numbered 1-7• Each period represents an energy level where

electrons can be found• Counting across a row to an element’s location

tells how many electrons are in its outer shellGroups or families: (vertical columns) • Groups are numbered from 1-18• Group members have similar chemical

properties which get stronger as you go down a column. Eg. Alkali Metals

How is it Organized?

Metals & Non-metals

• Metals are on the left side

• Non-metals are on the right side

• Exception: Hydrogen (H) is a non-metal

• Metalloids are the elements that are between the metals and non-metals – they have some properties of both.

Properties of Metals & Non-metals

Properties of metals

• High lustre (shiny)• Most are grey or silver in

colour• Malleable (hammer into

sheets)• Ductile (stretch into wire)• Good conductors of

heat and electricity• Most are solids at room

temp…except Hg…it’s a liquid!

Properties of non-metals

• Low lustre (dull)• Various colours (including

colourless)• Brittle (shatter when

hammered)• Not ductile (shatter when

stretched)• Poor conductors (are

insulators)• Mostly solids and

gasses at room temp.

NON-METALS

METALS

Main group elements: Groups 1,2,17 and 18

Alkali metals: Group 1 – very soft, very reactive, one valence electronAlkaline earth metals: Group 2– somewhat soft, somewhat reactive, two valence

electrons Halogens: Group 17 – very reactive non-metals, one short of a full set

of valence electrons, diatomic molecules Noble gases: Group 18 – almost completely un-reactive or inert, full

valence shell. Exist as monatomic gases

ATOMIC STRUCTURE REVIEW

• A chemical Symbol represents 1 atom of an element. eg: Al

• Atoms are not solid spheres as first thought, the majority of an atom is empty space! What gives matter “solidness” is the tiny subatomic particles that make up atoms.

• There are three types of subatomic particles:

Sub-atomic Particles

Particle Symbol Location Charge Size

Proton P In the nucleus

Positive 1

Electron E In the orbitals (shells) around

nucleus

Negative 0

Neutron N In the nucleus

Neutral 1

Back to the Periodic Table

C6

12

This is the Atomic Number or A

This is the Symbol

This is the Atomic Mass or Z

CARBON This is the Element’s Name

And now the short form…

A

Z

6

12

CARBON (C)

OR…

(Atomic Number)

(Atomic Mass)

Bohr-Rutherford Diagrams

The Nucleus contains protons & neutrons

Outer shell (orbital / energy level) called the Valence shell

Maximum # of electrons ateach energy level(inner to outer) 2, 8, 8…

How to Draw a Bohr-Rutherford Diagram

• First you need to determine how many protons, electrons and neutrons you have: (PEN)

• Look at the Periodic Table:• The atomic number = the number of protons (+) &

the number of electrons(-) (# of + = # of -)• The atomic mass can help you determine the

number of neutrons: (Neutrons = atomic mass – atomic #)

• All that’s left is to draw the diagram!

How to Draw a Bohr-Rutherford Diagram for ANY Element.

1. Figure out how many protons, electrons and neutrons there are in one atom of the element.

2. Draw the nucleus (a small circle).• Inside the nucleus write the number of protons

and neutrons.3. Calculate the number of orbitals you will need

by following the limits on the number of electrons each orbital can have.

4. Draw the orbitals as rings around the nucleus.5. Draw the electrons (as coloured-in circles) on

the orbitals.