Bonding and structure

• metals form positive ions
• non metals form negative ions
• metals are malleable, conductive(heat and electricity) and shiny
• non metals are dull, brittle, have LMaBPs, lower densities and are poor conductors
• transition metals can form coloured compounds
• transition metals can form different ions
• TM are often used as catalysts
• what is the reactivity series: Pottasium, Sodium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Tin, Lead, Hydrogen, Copper, Silver, Gold, platinum
• the nunomic for the reactivity series

  please stop calling me a careless zebra instead learn how copper saved gold proplery
• Group 1 metals are low density, weak and have LMP
• The group 1 metals are very reactive especially with group 7 metals
• group 1 metals are especially reactive with water, oxygen
• the MP and BP dcreases in Group 1
• group 1 metals have increasing reactivity because they have an increased distance that weakens the attractive force from the positive nucleus
• G1 always form ionic compounds. Which use Electrostatic forces between a positive metal ion and a negative non metal
• metal + oxygen -> metal oxide
• metal + water -> metal hydroxide + hydrogen
• metal + acid -> salt + hydogen
• metal oxide + acid -> salt + water
• metal carbonate + acid -> salt + water + carbondioxide
• lithium + oxygen -> Lithium oxide
• sodium + oxygen -> sodium oxide or sodium peroxide
• potassium + oxygen -> potassium super oxide or potassium peroxide
• the reactivity of the halogens decreases as you go down the period

  because they have a weaker force of attraction to an electron to complete its outer shell because it has a larger radius
• chlorine is a green gas
• bromine is a reddy brown volatile liquid
• iodine is a dark grey solid which produces purple poisonous gas
• iodine is an antiseptic, used to prepare people for surgery
• all the halogen gasses are poisonous
• halogens are diatomic

  because they share their outer shell electron with each other, called a covalent bond
• a strong covalent bond by the diatomic halogen gase

  
• the melting and boiling points increase, going down the period
• when a halogen reacts with a metal, it becomes a halide ion

  fluorine -> fluoride

  chlorine -> chloride

  bromine -> bromide

  iodine -> iodide
• so sodium + chlorine -> sodium chlorIDE

  magnesium + bromine -> magnesium chlorIDE
• the boiling point of Noble gasses increases as you go down the period
• the halogens arent flammable
• Ionic bonding is where the metal shares its outer shell electron with a non metal. This forms a positive metal ion and a negative non metal ion.

  this is then the same electronic structure as a Nobel gas in group 0
• in ionic bonding the metals are formed with electrostatic forces which are strong and cause the ionic bond between two elements of opposite charges
• you always need a square bracket around a dot and cross diagram with the charge on the outside
• an ionic compound forms regular lattices structures, ions are held together by strong electrostatic forces, and represented by a ball and stick diagram