Giant review of grade 10

The things inside the nucleus of an atom

• Proton

• Neurtron

Valence electrons

Electrons on the outermost shells. The further they are from the nucleus the easier they are to remove.

The octet rule

When elements lose, gair, or share an electron to get either a full or empty shell

Metals 

They give away electrons because the have only a couple of them, becoming positive ions.  

They also share valence electrons in a localized manner 

Ion

A charged atom (ie. an atome with an unbalanced number of protons and electrons)

Cations

Positively charged ions

Non-metals

Because they have more electrons, they gain them. Becoming anions. They also share electrons in a localized manner. 

Anions

Negatively charged ions

What do cations and anions do with eachother?

Attract eachother in ionic crystal lattices

Molecular compounds

Two non metals bonded together.

Properties of ionic compounds 

• They are made of billions of ions that are all strongly attracted to eachother

• They have high melting points

• Ions form a 3D structure (crystal lattices)

use of chemical formulas

To show the most simple ratio of cation and anions in the crystal lattice

Zero sum

The ratio that exist to make the charges of the anion and cation cancel out.

Solid hydrates

Water in ion compounds crystal lattices as solids. This is shown with a dot.

Acids

• compounds that are dissolved in water, or aqueous. They act like acids and have a low pH

• If there no polyatomic ion put ‘hydro’ infront 

Molecules

two or more atoms that are covalently bonded

Bonding capacity

Number of unpaired electrons in the valence shell.

Reactants 

Starting materials of a reaction

Products 

Material that gets made in the chemical reaction

Rule with reactans and products

When reactants are changed into products, number of each atoms cannot change. Ie. Daltons atomic law: ‘matter cannot be destroyed or created. Just reaarnaged.’

Physical changes

When the subtances is not changed, but it’s form

Things that both chemical and physical changes do

• Absorb energy= endothermic

• released=exothermic 

signs of a chemical change 

• Drastic colour change

• precipitate forming 

• bubbles of gas

• new smell

• light and heat 

collision theory 

• For a chemical reaction to happen, the reactants must physically collide with eachother

kinemtic molecular theory 

Particles are always in motion, the hotter they are the faster they go. 

There for:

• Hotter= faster, more collisons, more reactions

• increase concentration of reactants= more collisons

• Increase of surface area= more collisons

Accuracy 

the agreement with the accepted or true value 

precision

• Agreement within a group of observations of same quantity 

•  Its ability to measure mass with a high degree of precision

Random error

An equal chance of affecting the quantity either making it to high or to low.

Systematic errors

Affect data in the same way each time

Absolute uncertainty 

Expressed as an amount 

Relative 

Expressed a percentage

Acids

When non metals react with water

Bases

When metals react with water

Difference between complete and incomplete combustion

• Incomplete happens when there isn’t enough supply of oxygen

• Complete produces carbon dioxide, incomplete produces carbon monoxide

• Incomplete is less efficient and makes more pollutants.