Topic 6 Flashcards
Done
6.1
Why are alkali metals in group 1?
1 electron on outermost shell
6.2
Give 3 physical properties of alkali metals
-Soft
-Low mp
-Very reactive
6.3
Describe the reaction of lithium with water
-Fizzing
-Moves on water surface
-Dissolves/disappears
6.3
Describe the reaction of sodium with water
-Melts into molten ball
-More fizzing + moves + dissolves faster than Li
6.3
Describe the reaction of potassium in water
-Lilac flame
-Explodes
-More fizzing + moves + dissolves faster than Na
6.4
What happens to the reactivity of alkali metals as you go down the group
Increases
6.4 6.5
Explain the pattern of reactivity of the alkali metals in terms of electronic configurations
-As descend, reactivity increases
-Ions larger
-Greater d between e^- on outermost shell & positive nucleus
-e^- shielding (more e^- = reduce F)
-Electrostatic F of attraction decreases
-e^- lost more easily
6.6
State the colour and physical state of fluorine
Pale yellow gas
6.6
State the colour and physical state of chlorine
Green/yellow gas
6.6
State the colour and physical state of bromine
Yellow/orange solid
6.6
State the colour and physical state of iodine
Grey/black solid
6.6
What colour is iodine vapour?
Purple
6.7
What happens to the appearance of the halogens as you go down group 7?
Darker
6.7
What happens to the boiling point of the halogens as you go down the group? Explain this trend
-Increases
-Molecule size increases
-Stronger intermolecular F between molecules
-More energy needed to separate bonds
6.7
What is a use of fluorine?
Toothpaste
6.7
What is a use of chlorine?
Kill micro-organisms in swimming pools
6.8
What are bromine and iodine used for?
Antiseptics
6.8
Describe the chemical test for chlorine gas
Damp blue litmus paper turns red then bleached
6.9
What is the product when a halogen reacts with a metal?
Metal halide
6.9
State one feature of the halogens in terms of their safety
Toxic
6.9
a) What is formed when potassium reacts with chlorine ?
b) What is formed when sodium reacts with fluorine?
a) Potassium chloride
b) Sodium fluoride
(If not sure why see card 15)
6.10
What is the product when a halogen reacts with hydrogen?
Hydrogen halide
6.10
A test tube was filled with hydrogen chloride gas. The test tube was inverted in water and left. The liquid level rose up to the top of the test tube. Explain what was formed in the test tube after the water had entered [2 marks]
-Hydrogen chloride dissolves
-Hydrochloric acid
6.10
a) What is formed when fluorine is reacted with hydrogen?
b) What is formed when chlorine is reacted with hydrogen?
c) What is formed when these products are added to water?
a) Hydrogen fluoride
b) Hydrogen chloride
c) Acidic solutions
6.10
What acid is formed when hydrogen chloride is dissolved in water?
Hydrochloric acid
6.11
Place iodine, chlorine and bromine in order from most to least reactive starting with most
-Chlorine
-Bromine
-Iodine
6.11
Does chlorine react with potassium chloride? If so describe the colour change
No bc Cl can’t displace Cl
6.11
Does chlorine react with potassium bromide? If so describe the colour change
-Yes
-Colourless to yellow
6.11
Does chlorine react with potassium iodide? If so describe the colour change
-Yes
-Colourless to dark brown
6.11
Does bromine react with potassium chloride? If so describe the colour change
No
6.11
Does bromine react with potassium bromide? If so describe the colour change
No
6.11
Does bromine react with potassium iodide? If so describe the colour change
-Yes
-Colourless to dark brown
6.11
Does iodine react with potassium chloride? If so describe the colour change
No
6.11
Does iodine react with potassium bromide? If so describe the colour change
No
6.11
Does iodine react with potassium iodide? If so describe the colour change
No
6.11
Describe how halogen displacement reactions work. Use potassium bromide when it reacts with chlorine as an example
-Most reactive halogen displaces all other halogens
-Potassium bromide + Chlorine -> Potassium chloride + Bromine
6.11
a) What is formed when potassium iodide reacts with bromine?
b) What is formed when sodium iodide reacts with bromine?
a) Potassium bromide + Iodine
b) Sodium bromide + Iodine
6.12
Explain why halogen displacement reactions are redox. Use the reaction between chlorine and potassium iodide as an example
-Cl₂ + 2KI -> 2KCl + I₂
-Make into ionic equation
-Cl₂ + 2I^- -> 2Cl^- + I₂
-Chlorine atoms reduced (gain e^-) = chloride ions
-Iodide ions oxidised (lose e^-) = iodine atoms
-Reduction & oxidation occurs at same t so is redox
6.13
Explain what happens to the reactivity of the halogens as you go down group 7
-Less reactive
-Ions bigger -> d between nuc & outermost shell increases
-Weaker electrostatic F of attraction between + nuc & incoming - e^-
-Harder to gain e^-
6.14
State 4 properties of noble gases
-Inert
-Non-flammable
-Colourless
-↓ mp & bp
6.14
Explain why the noble gases are chemically inert
-Full outer shell of e^-
-So unreactive -> stable
6.15
What is a use of helium? State 2 properties that allow this and why
Weather balloons
Low density
-Less dense than air
Non-flammable
-Won’t burn
6.15
What is neon used for?
Advertising signs
6.15
What is xenon used for?
-Advertising signs
-Filament lamps
6.15
What is argon used for? What properties allow this?
Advertising signs
Filament lamps
-Inert
Welding
-Inert
-Non-flammable
6.15
What is krypton used for?
Lasers
6.16
Explain what happens to the boiling points of the halogens as you move down the group
-Increase
-Get larger
-Increase in intermolecular F
-More energy needed to overcome
6.16
What happens to the density as you go down group 0 (noble gases)?
Increases
Describe and explain the observations when a small piece of lithium is placed on the surface of a big container of water. A few drops of universal indicator have been added to the water
-Li reacts w/ water -> Hydrogen (fizzing)
-Universal indicator: green to purple (alkaline solution of lithium hydroxide produced)
Name a product that is always produced when a metal reacts with water or dilute acid
Hydrogen
