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Description
Flashcards by Malachy Moran-Tun, updated more than 1 year ago
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Created by Malachy Moran-Tun
about 3 years ago
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| Question | Answer |
| What are Group 1 Elements also known as? | Alkali Metals |
| How many Outer Electrons do Group 1 Metals have? | One outer electron |
| What Physical Properties do Group 1 Metals have? | > Low melting and boiling points (compared with other metals) > Very soft - can be cut with a knife |
| Why do Group 1 Metals NOT form Covalent Bonds? | > Form ionic compounds > Loose the outer electron very easily > Outer electron CANNOT be shared |
| Why are Group 1 Metals So Reactive? | > Easy to loose the outer electron > Loosing the outer electron forms a stable electronic structure (1⁺ ion) |
| How and Why does Reactivity Change as you do Down Group 1? | > Reactivity increases > Outer electron is more easily lost > Electron is further from the nucleus > Electrostatic shielding from shells > Less attraction to the nucleus > Less energy required to remove electron |
| What is the General Word Equation for Reactions with Water and Alkali Metals? | Alkali Metal + Water → Alkali Metal Hydroxide + Hydrogen |
| Why do Alkali Metals from Alkali in Water? | They produce hydroxides which contain OH⁻ ions |
| What happens when Lithium Reacts with Water? | > Bubbles Fiercely on Water Surface > 2Li(s) + 2H₂O(l) → 2LiOH(aq) + H₂(g) |
| What happens when Sodium Reacts with Water? | > Melts into a ball and fizzes as it moves around on the surface > 2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g) |
| What happens when Potassium Reacts with Water? | > Reacts very rapidly and bursts into a lilac flame as it flies about the surface > 2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g) |
| What are Group 7 Elements also known as? | Halogens |
| How many Outer Electrons do Group 7 Elements have? | Seven outer electrons |
| What type of Molecule do Halogens (Naturally) Exist as? | Diatomic Molecules (e.g. Cl₂, Br₂, I₂ etc.) |
| Why do Halogens Exist as Diatomic Molecules? | Share one pair of electrons in a covalent bond to give both atoms a full outer shell |
| How do the Melting and Boiling Points Change going Down Group 7? | Increase (Fluorine lowest → Iodine highest) |
| What Colour and State is Fluorine at Room Temperature? | Yellow Gas |
| What Colour and State is Chlorine at Room Temperature? | Green Gas |
| What Colour and State is Bromine at Room Temperature? | Orange Liquid |
| What Colour and State is Iodine at Room Temperature? | Grey Solid |
| What is the Chemical Test for Chlorine? | Damp blue litmus paper turns red then bleaches white |
| How and Why does Reactivity Change as you do Down Group 7? | > Reactivity decreases > Electron is harder to attract > Outer shell is further from the nucleus > Electrostatic shielding from shells > Less attraction to the nucleus > Less energy available to attract electron |
| What is the General Word Equation for Reactions with Metals and Halogens? | Halogen + Metal → Metal Halide (Salt) |
| What is the General Word Equation for Reactions with Hydrogen and Halogens? | Halogen + Hydrogen → Hydrogen Halide |
| What happens when Hydrogen Halides Dissolve in Water? | Form acidic solutions (e.g. HCl forms Hydrochloric Acid) |
| What happens if a More Reactive Halogen Reacts with a Halogen Compound? | More reactive halogen displaces the less reactive one |
| Why are Halogen Displacement Reactions Redox? | > Halogen Gains Electrons (Reduction) > Halide Ions Loose Electrons (Oxidation) |
| Halogen Displacement Practical in Guide of Revision | aaaaaaaaaaaaaaaaaaaaaaaaaaaaaahelloaaaaaaaaaaaaaaaaaaaaaaaaaaaaa |
| What are Group 0 Elements also known as? | Noble Gases |
| How many Outer Electrons do Group 0 Metals have? | Full Outer Shell (2, 8, 8 for first 3 periods) |
| What are the Physical and Chemical Properties of Group 0 Elements? | > Colourless Gases (at room temp.) > Monatomic (exist as single atoms) > Extremely unreactive (almost inert) > Non-Flammable > Low Melting / Boiling Points > Low Densities |
| Why are Group 0 Elements Inert? | They have a full outer shell of electrons so they don't gain / loose / share electrons easily |
| What are some Uses of Noble Gases? | > (All) Provide an Inert Atmosphere > Argon used in Filament Lamps (non-flammable) > Argon and Helium Protect Metals during Welding > Helium used in Airships and Party Balloons (Low-Density) |
| What happens to Melting / Boiling Points / Density as you go Down Group 0? | > Melting / Boiling Points Increase > Density Increases |
| you be done now | cool |
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