Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
42 Cards in this Set
- Front
- Back
|
Atom
|
the smallest component of an element having the chemical properties of the element
|
|
|
Electron
|
Particle with a negative (-1) charge, surrounding the nucleus in orbitals which take up most of the volume of the atom.
The mass of an electron can be assumed to be 1/2000th the mass of a proton. |
|
|
Nucleus
|
The centre of the atom
Where you find protons and neutrons Where the mass of the atom is concentrated. |
|
|
Protons
|
Positively charged particles
Relative mass 1 Relative charge +1 |
|
|
Neutrons
|
Neutral Particle
Relative mass 1 Relative charge 0 |
|
|
Mass Number
|
Total number of protons and neutrons in the neucleus
|
|
|
Atomic Number
|
Number of protons in the nucleus
|
|
|
Ion
|
An ion is an atom or molecule which has lost or gained one or more valence electrons, making it positively or negatively charged
|
|
|
Isotope
|
atoms of an element with different numbers of neutrons and different masses
|
|
|
Relative Mass
|
Carbon-12 is used as the standard
measurement of relative masses |
|
|
Relative Atomic Mass
|
the average mass of an atom of an element compared with Carbon-12 on a scale where Carbon-12 is 12
|
|
|
Relative Isotopic Mass
|
the average mass of an isotope of an element compared with Carbon-12 on a scale where Carbon-12 is 12
|
|
|
Relative Molecular Mass
Relative Formula Mass |
the average mass of a molecule or formula unit compared with Carbon-12 on a scale where Carbon-12 is 12
|
|
|
Amount of Substance
|
the number of particles
|
|
|
Mole
|
The unit used to measure amount of substance
|
|
|
The Avogadro Constant
|
6.02x10 to the 23 mol-1
|
|
|
Molar Mass
|
the mass per mole of a substance
(same as Relative Molecular Mass) |
|
|
Empirical Formula
|
the simplest whole number ratio of atoms of each element present in a compound
|
|
|
Molecular Formula
|
the actual number of atoms of each element in a molecule
|
|
|
Acids
|
releases H+ ions in aqueous solution
Proton Donors |
|
|
Alkali
|
soluble base that releases OH– ions in aqueous solution
|
|
|
Hydrochloric Acid
|
HCl
|
|
|
Sulfuric Acid
|
H2SO4
|
|
|
Nitric Acid
|
HNO3
|
|
|
Common Bases
|
Metal Oxides
Metal Hydroxides Ammonia |
|
|
Sodium Hydroxide
|
NaOH
(Base) |
|
|
Potassium Hydroxide
|
KOH
(Base) |
|
|
Aqueous Ammonia
|
NH3
(Base) |
|
|
Salt
|
produced when the H+ ion of an acid is replaced by a metal ion or NH4+
|
|
|
Acid reaction with Base
|
When acids react with bases, they neutralise each other. Alkalis release OH- ions in water. These OH- ions accept H+ ions from an acid to form water.
Metal Oxide + Acid > Salt + Water Metal Hydroxide + Acid > Salt + Water |
|
|
Acid reaction with Metals
|
Metal + Acid > Metal Salt + Hydrogen
|
|
|
Acid reaction with Carbonate
|
Metal Carbonate + Acid > Metal Salt + Carbon Dioxide + Water
|
|
|
Anhydrous
|
When a salt lattice does not contain water molecules it is said to be anhydrous
|
|
|
Hydrated
|
When a salt lattice contains water molecules
|
|
|
Water of crystallisation
|
The water contained in a salt lattice
|
|
|
Oxidation
|
Loss of electrons
|
|
|
Reduction
|
Gain of electrons
|
|
|
Oxidising agent
|
Accepts electrons and gets reduced
|
|
|
Reducing agent
|
Donates electrons and gets reduced
|
|
|
Metals
(relating to Redox reactions) |
generally form ions by losing
electrons with an increase in oxidation number to form positive ions |
|
|
Non-metals
(relating to Redox reactions) |
generally react by gaining
electrons with a decrease in oxidation number to form negative ions |
|
|
Metals reducing Acids
|
Metal atoms are oxidised
Hydrogen ions in solution are reduced, forming hydrogen molecules |
