C3.1 Flashcards
Molecular formulae
Used for simple covalent compounds
Empirical formulae
Used for ionic and giant metallic lattices
Diatomic
When two atoms are joined together they are said to be diatomic
Examples of the diatomic elements
oxygen
nitrogen
hydrogen
fluorine
iodine
bromine
chlorine
Ex: magnesium + iron nitrate -> magnesium nitrate +iron
Magnesium nitrate +iron
Name the + ions
H+, Na+, Li+, Ag+, NH4+, K+
Name the 2+ ions
Ba2+, Ca2+, Cu2+, Fe2+, Mg2+, Zn2+, Pb2+
Name the 3+ ions
Fe3+, Al3+
Name the - ions
Cl-, Br-, F-, I-, OH-, NO3-
Name the 2- ions
O2-, S2-, SO4 2-, CO3 2-
Calcium nitrate
Ca(NO3)2
Lithium sulfate
Li2SO4
During a chemical reaction
The total masses stay the same before and after
Matter…
Cannot be created or destroyed
Oxidation is
Loss
Reduction is
Gain
What is an ionic compound?
Anything bonded to a nitrate
When ions are free to move
They can collide into different ions
What is an aqueous solution?
A solution containing a substance that is dissolved in water
When ions that are dissolved collide and react…
A precipitate forms
Fast or slow reaction?
Fast
Equation for moles
moles = mass/relative mass
What is a mole?
One mole of a substance is equal to 6.022 × 10²³ units of that substance
When you have the mass and need the amount of moles
Divide by the molar mass
When you have the amount of moles and need the mass
Multiply by the molar mass
When you have the moles and need the number of particles
Multiply by 6.02*10^23
When you have the number of particles and need moles
Divide by 6.02*10^23
What is Avogadro’s constant?
6.02*10^23
What does the Law of Conservation of Mass state?
- No atoms are made or lost during a reaction
- The mass of the reactants will be the same as the mass of the reactants after a reaction
