Atomic Structure Flashcards
Isotopes definition
Atomskf the same element with the same number of protons but different numbers of neutrons
Relative isotopic mass definition
The mass of one isotope compared to one twelfth of the mass of one atom of carbon-12
Relative atomic mass definition
The weighted mean mass of one atom compared to one twelfth of the mass of one atom of carbon-12
Relative molecular mass definition
The average mass of a molecule compared to one twelfth of the mass of one atom of carbon-12
Calculate relative atomic mass of an element
(Sum of (isotopic mass x abundance) ) / sum of abundances
Group 1 ion charge
+1
Group 2 ion charge
+2
Group 3 ion charge
+3
Group 5 ion charge
-3
Group 6 ion charge
-2
Group 7 ion charge
-1
Hydrogen ion charge
+1
Silver ion charge
+1
Gold ion charge
+1
Ammonium ion charge
+1
Ammonium ion formula
NH4
Zinc ion charge
+2
Copper(II) ion charge
+2
Iron(II) ion charge
+2
Tin ion charge
+2
Lead ion charge
+2
Iron(III) ion charge
+3
Phosphate ion charge
-3
Phosphate ion formula
PO4
Carbonate ion charge
-2
Carbonate ion formula
CO3
Sulfate ion charge
-2
Sulfate ion formula
SO4
Nitrate ion charge
-1
Nitrate ion formula
NO3
Hydroxide ion charge
-1
Hydroxide ion formula
OH
Spectator ions do not change…
- Oxidation number
- State
Proton relative mass
1
Proton relative charge
+1
Neutron relative mass
1
Neutron relative charge
0
Electron relative mass
1/800
Electron relative charge
-1
Atomic number is the number of what
Protons
Mass number is the number of what
Total of protons and neutrons
Calcium chloride formula
CaCl2
Sodium carbonate formula
Na2CO3
