Elements of Life Flashcards
Hydrochloric Acid
HCl
Nitric Acid
HNO3
Sulphuric Acid
H2SO4
Phosphoric Acid
H3PO4
Methanoic Acid
HCOOH
Ammonia
NH3
Isotopes
Different atomic number same mass number
Different number of neutrons same number of protons
Relative Atomic Mass
A measure of the average mass of an element compared to a standard unit of mass
Calculated by adding all masses of an element then averaging them based on their abundance
Atomic Mass
The actual mass of an individual isotopes - a fixed value
How to calculate RAM
Need abundance of each isotope
Need the mass number
(mass * abundance) + (mass * abundance)/(abundance + abundance)
Example of RAM with Chlorine
Cl-35 75%
Cl-37 25%
(75 * 35) + (37 * 25)/ 75 + 25 = 35.5
Atom
The smallest piece of an element, made up of protons, neutrons and electrons and has a neutral charge
Molecule
A group of atoms held together by covalent bonds
Ion
An atom or molecule which has lost or gained electrons so is positively or negatively charged
Element
A substance made from one type of atom only
Compound
A substance formed from two or more chemically bonded elements in a fixed ratio, shown by a chemical formula
Simple Structure
Made up of small molecules held together by weak intermolecular forces
Giant lattice structure
A 3-dimensional structure of particles held together by strong bonds (covalent or metallic)
Group
A vertical column in the periodic table. The element has the same number of outer electrons hence similar chemical properties
Intermolecular Forces
Attractive forces between neighbouring molecules
Neutralisation Reactions
Acid + Base –> Salt + Water
Combustion
Complete - +O2 —> CO2 + H2O
Incomplete - +O2 —> CO + H2O
Acid + Metal Carbonate
—> Salt + Water + Carbon Dioxide
Acid + Metal Oxide
—> Salt + Water
Acid + Metal Hydroxide
—> Salt + Hydrogen + Water
Common Acids
H+ Donors
Hydrochloric - HCl
Nitric - HNO3
Sulfuric - H2SO4
Phosphoric - H3PO4
Acid + Metal
—> Salt + Hydrogen
Common Alkalis/Bases
H+ Acceptors
Group 1 hydroxides + Oxides = Na2O
Group 2 hydroxides + Oxides = MgO
Polyatomic Ions
Hydrogen Sulfate - HSO4-
Carbonate - CO3 2-
Ethanoate - CH3COO-
Hydroxide - OH-
Sulphate - SO4 2-
Nitrate - NO3-
Hydrogen Carbonate - HCO3-
Ammonium - NH4+
Ar
Relative Atomic mass (average mass of an atom)
A
Atomic Mass (number of P+ and e-)
Z
Atomic Number (number of p+)
Nucleons
Protons and neutrons as they’re found in the nucleus
Avogadro’s constant
6.022 * 10^23
Molecular Formula (Mr)
Shows the actual number of atoms of each element present in a compound or molecule
Glucose’s Mr = C6H12O6
Empirical Formula
The simplest whole ratio of atoms of each element
Glucose = CH2O
Water of Crystallisation
Water that’s trapped between ions when an ionic solid forms
Ionic solids with woc = hydrated
Ionic solids without woc = anhydrous
woc shown in a formula
.xH2O where x = a number