Particle Theory of Matter:

1. All matter is made up of tiny particles called atoms 

2. All particles in substances are identical

3.  All particles are in motion and change with temperature 

4. All particles have space in between them

5. All particles have attractive forces 

Colloids: Tiny particles

Solids have a definite shape and volume because the particles in a solid can only move a little bit. All they can do is vibrate.

Liquids take the shape of their container because the particles can move more freely then they can in solids. A liquids particles are held together by strong attractions to each other, so it has a definite volume. These particles move from one area to another.

Gases always fill whatever container they are put in. Since gases have very little attraction, the particles are quite far apart. These particles are constantly moving everywhere.

• Chemical properties: How something interacts with another substance Observed through chemical reaction.

Physical properties

• A physical property is a property of a system that is measurable

• There are 10 different ways to measure physical properties. They are

  1. State ( type of motion it has, solid, liquid, or gas)

  2. Color, size and shape

  3. Malleability (how much it can bend without breaking)

  4. Ductility (how well it stretches)

  5. Hardness

  6. Toughness

  7. Melting point

  8. Boiling point

  9. Solubility (how well it breaks apart in water)

  10. Conductivity (how well it conducts electricity)

• Exothermic= releases energy Endothermic= Takes in energy

• Qualitive properties: Physical properties that can be described with words

• Quantitative properties: Physical properties that can be described with numbers

• WHMIS: Workplace Hazardous Materials Information System. This is involved in this like flammability, exploding substances, corrosion, biohazards, chronic toxicity, even death

Density

• Density is how much mass a substance has per volume.

• Formula: density= mass/volume

• Formula: mass= density x volume

• Formula: volume= mass/density

Buoyancy: Archimedes Principle

Chemical Properties

• a chemical property is how a substance reacts. a chemical change means that the identity of a substance has changed

• chemical properties include toxicity, reactivity, combustibility, and stability

• A reaction rate is how fast or slow a reaction occurs, based on how much product or reactant is used in a specific amount of time

• LD50 is a standard measure to determine if a substance is toxic or not

• Combustibility: a measure of how readily a substance reacts with oxygen to produce fire

• Stability is not the opposite of reactivity. It does not change form quickly when left alone

• Catalyst: a substance that speeds up the rate of a reaction without being used up or changed itself.

• Indicators that a chemical change has occurred: Bubbles, temperature change, color change, odor change, precipitate forms ( solid that forms when 2 liquids are mixed)

• Chemical reaction- when atoms of 2 or more substances are rearranged to form new substances

• Reactants go in, Reaction is the outcome

• Photosynthesis= reactant 1 + reactant 2= product 1 + product 2

  Photosynthesis= Sunlight+ Co2+ H20+water= O2 and Glucose (C6H206)

• There are 2 kinds of equations, chemical and word equations

Word equations= Chemical reactions are written using the names of the substances

Ex: Silver+ Nitrogen= Silver Nitride

Chemical equations= Chemical reactions that use chemical formulas to represent the substances

Ex: Silver Nitride AGs + N2g= AG3N

Prefixes: Mono 1, Di 2, Tri 3, Tetra 4, Penta 5, Hexa 6, Hepta 7, Octa 8, Nena 9, Decca 10

Roman numerals: use when an element has more than 1 change ex: 1= II

• There are 7 elements that are naturally diatomic. This means that when they are all by themselves, there are actually 2 of them stuck together rather than 1. These elements are nitrogen, (n2) oxygen( o2), fluorine (f2), hydrogen, (h2) bromine (br2), iodine, (i2) and chlorine (cL2)

• Combustion- when oxygen reacts with a carbon fuel such as gasoline

• Corrosion- when oxygen reacts with metal over time

• Photosynthesis- How plants convert Co2 and o2 into glucose and energy

• Cellular respiration= oxygen, glucose, water, energy, carbon dioxide

Types of Matter

• Conservation of mass= Matter can’t be created or destroyed. It is also a closed system

• Matter can be classified as either a pure substance or a mixture.

Pure substances: Elements (Sodium, Oxygen, Nitrogen) Compounds (Water, Table Salt, Sugar) Made of 1 element.

Mixtures: Solutions (Coffee, Milk, Air. Contains more than 1 type of substance throughout) Made up of 2 elements

Mechanical mixtures (Orange juice with pulp, Contains more that 1 type of substance, not the same throughout)

• Homogenous Mixture: Looks like one substance but is made of many

• Heterogeneous Mixture: Looks like there are 2 or more parts to a mixture.

• Subatomic Particles: Particles that are within an atom; such as electrons, neutrons, and protons

• The periodic table of elements

• This system was invented by Russian chemist Dmitri Mendeleev.

• The periodic table is organizes atoms into groups (columns) and periods (rows). The last digit of the group number tells you how many valence (outer) electrons the atom has. The period number tells you how many energy levels (shells) the atom has. The elements are listed in increasing order of proton number (atomic number)

• Metalloids are elements that share a mixture of metals and non metal mixture.

• Metals are located on the left hand side of the staircase. They are shiny.

• Non metals are located on the right hand side of the staircase. They are brittle and they tend to be gases

• The red column is the alkali metals. They are very reactive with air and water. They are the most reactive metals

• The orange column is the alkaline earth metals. They are less reactive than alkali metals. They easily react with oxygen

• The purple column is the halogens. They are the most reactive non metal, They react very easily with the 1st and 2nd column (group)

• The dark purple column is called the noble gases. They are very unreactive, but are also very stable.

Each group is made up of elements that are in the same family that share similar properties.

• The mass increases from left to right along a period.

  

  On an element, there is also a charge symbol.

Symbol is always 1 capital letter or 1 capital and 1 lowercase letter

We can find and calculate the number of subatomic particles an element has.

#protons= p+ = atomic #

#electrons= e- = atomic #

#newtons= n°= atomic mass- atomic number. Round to whole #

Ionic compounds

• Ionic compounds always contain a metal and a non-metal , so they are always on opposite sides of the staircase.

• Metals always want to lose electrons

• Non metals want to gain electrons

• You can discover their charges on the periodic table!

• Charges are always written as number first, then their sign.

  Balancing the charges

  1. Look up each element and write each symbol with its charge, writing the positive ion first and the negative ion second

  2. Check to see if the total positive charge is equal to the total negative charge

  3. Add more of own or both ions until the total charges are unequal

  4. Write your chemical formula, making sure the positive ion is first and the negative ion is second, using subscripts to show how many of each ion you needed

  Ex: Na 1+ Cl 1-

  Na, Cl 1s are invisible

NaCl

To cross your changes (always put in lowest terms)

1. Look up each element and write each symbol with its charge writing the positive ion first and the negative ion second

2. Draw arrows showing that the charge on one ion becomes the subscript on the other ion

3. Write your chemical formula making sure that your charges have become subscripts and that you don’t write the + or - signs anymore

4. CHECK that your subscripts are in the lowest terms possible

Ex: : Na 1+ Cl 1-

Na, Cl ones are invisible

NaCl

The Lewis dot diagram

Steps

1. Count all the valence electrons

2. Determine the central atom (the odd atom out)

3. Draw single bonds to the central atom

4. Put all the remaining Valence electrons on atoms as 1 part

5. Turn ion pairs into double or triple bonds to give every atom an octlet

Valence electrons

• In an atom, electrons move in orbitals around a nucleus

• Valence electrons are special electrons that are the ones in the outermost shell and are available for bonding

• Not all electrons are valence electrons

• You can find out the number of valence electrons of a atom by looking at what column the atom falls under in the periodic table. Ex: Oxygen is in the 3rd column, so it has 6 valence electrons

• Helium is an exception of this! It only has 2 valence electrons

• To break you bonds: needs energy, When bonds form, energy is released.