Atoms and reactions

Jen
Mind Map by Jen, updated more than 1 year ago
Jen
Created by Jen about 6 years ago
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GCSE Chemistry - UNIT 1 Mind Map on Atoms and reactions, created by Jen on 03/18/2014.
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Atoms and reactions
1 Isotopes
1.1 Isotopes of the same element have:
1.1.1 Same no. of protons and neutrons
1.1.2 Different no. of neutrons in nucleus
1.1.3 Different masses
1.2 Different isotopes of the same element react in the same way because:
1.2.1 Chemical reactions involve electrons
1.2.2 Neutrons make no difference to chemical reactivity
2 ATOMIC (PROTON) NUMBER - the number of protons in the nucleus of an atom
3 ISOTOPES - atoms of the same element with different numbers of neutrons
4 MASS (NUCLEON) NUMBER - the number of particles in the nucleus
5 ION - a +ve or -ve charged atom or (covalently bonded) group of atoms (molecular ion)
6 Atomic masses
6.1 Relative Isotopic Mass
6.1.1 Same as a mass number for an isotope
6.2 Relative Atomic Mass
6.2.1 'Weighted mean mass' to account for the contribution of each isotope to overall mass of an element
6.2.2 Contribution made by isotope depends on:
6.2.2.1 % abundance of isotope
6.2.2.2 Relative mass of isotope
6.3 Relative molecular mass
6.3.1 Mass of a molecule measured as the realtive molecular mass by comparison with carbon-12
6.3.2 Add together relative atomic masses of each atom in the molecule
6.4 Relative formula mass
6.4.1 Compounds with giant structures don't exist as simple molecules
6.4.2 Add together relative atomic masses of each atom making up formula unit
7 RELATIVE ISOTOPIC MASS - the mass of an atom of an isotope compared with one-twelfth of the mass of an atom of carbon-12
8 RELATIVE ATOMIC MASS - the weighted mean mass of an atom of an element compared with one-twelfth on the mass of an atom of carbon-12
9 RELATIVE MOLECULAR MASS - the weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12
10 RELATIVE FORMULA MASS - the weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12
11 Amount of substance and the mole
11.1 Amount of substance
11.1.1 Symbol, n
11.1.2 Measured using unit called the 'mole'
11.1.3 Based on standard count of atoms
11.1.3.1 Avagadro's constant
11.1.3.1.1 No. of atoms per mole of the carbon-12 isotope
11.2 Mass of 1 mole of atoms of any element = the relative atomic mass in grams
11.3 A 'mole' is the amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope
11.4 Molar mass - add together all relative atomic masses for each atom that makes up a formula unit
11.5 n = m/M
12 Types of formula
12.1 Empirical formula
12.1.1 Always used for compunds with giant structures
12.2 Molecular formula
12.2.1 Used for compounds that exist as simple molecules
12.2.1.1 Tells you no. of each type of atom that makes up a molecule
13 AMOUNT OF SUBSTANCE - the quantity whose unit is the mole. Chemists use it as a means of counting atoms
14 AVAGADRO CONSTANT - the no of atoms per mole of the carbon-12 isotope
15 MOLE - the amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope
16 MOLAR MASS - the mass per mole of a substance. Units = g mol-1
17 EMPIRICAL FORMULA - the simplest whole-number ratio of atoms of each element present in a compound
18 MOLECULE - small group of atoms held together by covalent bonds
19 MOLECULAR FORMULA - the actual no of atoms of each element in a molecule
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