Of The Elements Flashcards
Period
Horizontal row
Group 1
Alkali metals
Group 7
Halogens
Group 8
Noble gases
From metal to non metal
From left to right
Group 1 elements physical properties
Good conductors of electricity and heat
Soft snd easily cut w knife
Low MPs and bps
Low densities (float on water)
Group 1 chemical properties
Shiny surfaces when cut
Becomes dull/tarnished when it reacts w oxygen
Burn in air or oxygen to form white solid oxides
2M + O2 -> M2O
Group 1 react w water
2M + 2H2O -> 2MOH + H2
Moves around water Hissing sound Bubbles of gas Gets smaller eventually disappearing (Melts into shiny ball) (Burns w lilac flame)
Potassium more reactive
Group 1 reactivity
More reactive further down group
Although they all have 1 electron on outer shell
Size of atom increase so outer ejection gets further away
Therefore outer electron less attracted to the nucleus
Chlorine colour at room temp
Gas
Pale green
Bromine at room temp
Liquid Red brown (readily evaporates into brown gas)
Iodine at room temp
Solid
Black
(Sublimes when heated to form purple gas)
Halogen reaction w iron
Chlorine- hit iron wool glows brightest
Brown smoke forms and brown solid left behind
Bromine- glows less brightly
Brown smoke and brown solid formed
Iodine- even less brightly
Brown gas and solid formed
Halogen w iron forms a…
Metal halide (halide= compound of halogen)
Iron + chlorine = iron(III) chloride
Halogen reactivity trend
Decreases down the group because of increasing size of atoms
Needs to attract extra electron
Further away outer shell from nucleus the less attraction
Halogen + hydrogen
Forms a hydrogen halide
Hydrogen+ chlorine-> hydrogen chloride
H2+ Cl2 -> 2HCl
Displacement reaction
More reactive will replace in metal halide
From an aqueous solution of a metal halide
Chlorine+ potassium bromide solution
-> potassium chloride solution + bromine
Aqueous chlorine
Pale green- usually appears colourless as it is so dilute
Aqueous bromine
Orange
Turn yellow when diluted
Aqueous iodine
Brown
Group
Vertical column
Hydrogen chloride + water
Hydrochloric acid
Hydrochloric acid properties
Turns litmus red
Turns universal I red
Reacts w metal to form a metal chloride and hydrogen
W a metal carbonate to form a metal chloride, water and co2
With a metal hydroxide or oxide to form a metal chloride in solution and water
Percentages of air
Nitrogen 78%
Oxygen 21%
Argon 0.9%
Carbon dioxide 0.04%
Using copper
Gas syringes Silica tube Copper Pass air backwards and forwards Need copper in excess Calculate volume lost
Using iron w oxygen
Iron filings
Burette end
Water will rise up from trough
Volume lost is equal to oxygen
Using phosphorus and oxygen
Phosphorus in water Same level inside and outside tube Heat with iron rod Reacting place bung on Water levels will change
How to prepare oxygen
W hydrogen peroxide Decomposes to form water and oxygen Manganese 4 oxide as catalyst Oxygen not soluble so not much is list Collected and measured using gas syringe
Oxygen and magnesium
Bright white flame
Forms white solid
Oxygen and carbon
Yellow flame
Forms colourless gas
Oxygen and sulfur
Blue flame
Forms colourless gas
Magnesium oxide and water
Magnesium hydroxide
Mg(OH)2
Carbon dioxide and water
Acidic oxide
Dissolves in water to form acidic solutions
H2CO3 carbonic acid
PH 5-6
Sulfur dioxide and water
Acidic oxide Dissolves in water to form an acidic solution H2SO3 Sulfurous acid pH 3-4
Oxides of metals are
Basics
Dissolve in water or don’t to form alkaline solutions
Oxides of non metals
Often acidic
Dissolve in water to form acidic solutions
Some oxides are neutral- eg carbon monoxide
Preparations of carbon dioxide
Metal carbonate+ acid
Eg calcium carbonate
By downward delivery as it is much denser than air
Thermal decomposition when heating metal carbonates
Copper carbonate
Green to black
Magnesium carbonate
No observable change
Stays white
Calcium carbonate
Stays white
No observable change
Zinc carbonate
White to yellow when hot
And white again when cold
Sodium carbonate
No observable change
Stays white
Doesn’t compose in a Bunsen flame
Uses of co2
Making carbonated drinks- pressure increased to increase solubility
In fizzy drinks
In fire extinguishers- co2 doesn’t support combustion
More dense than air so it sits on top of the burning fuel and prevent oxygen from getting to it
Carbon dioxide and climate change
Contributing?
Absorbs infrared radiation
Fossil fuels
Acid rain causes
Sulfur dioxide
Nitrogen
Causes a drop in ph lower than 6
Acid rain effects
Leaving vital minerals from the soil causing death of trees
Lowering ph of rivers killing fish
Weather of buildings and structures made out of limestone, marble and iron
