Chemistry: Period 3 Part 1
This flashcard set categorizes elements based on their atomic structures. It identifies metals like Na, Mg, and Al as forming giant lattices, silicon as macromolecular, nonmetals like P₄, S₈, and Cl₂ as simple covalent molecules, and noble gas argon as monoatomic.
type of structure Na Mg Al
giant lattice
Key Terms
type of structure Na Mg Al
giant lattice
type of structure Si
macromolecular
type of structure P4 S8 Cl2
simple covalent molecules
type of structure Ar
mono atomic
type of bonding Na Mg Al
metallic
type of bonding Si P4 S8 Cl2
covalent
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| Term | Definition |
|---|---|
type of structure Na Mg Al | giant lattice |
type of structure Si | macromolecular |
type of structure P4 S8 Cl2 | simple covalent molecules |
type of structure Ar | mono atomic |
type of bonding Na Mg Al | metallic |
type of bonding Si P4 S8 Cl2 | covalent |
type of forces Na Mg Al | metallic bonds- attraction between positively charged metal ions and delocalised electrons in a lattice |
type of forces Si | covalent- shared pair of electrons |
type of forces P4 S8 Cl2 | VDWs- temporary induced intermolecular forces |
type of forces Ar | VDWs |
bp and mp Na Mg Al Si | increasingly high |
bp and mp P4 S8 Cl2 Ar |
|
trend across period in atomic radius | decreases |
why does atomic radius decrease across period |
|
trend cross period first IE | increases |
why does first IE increase across period |
|
trend in electronegativity across period | increases |
observations of sodium with water | fizzes and floats on surface Na dissolves |
sodium and water equation | Na+H2O > NaOH + 1/2H2 |
observations of magnesium with cold water |
- occasional bubble |
equation magnesium and cold water | Mg + H2O> Mg(OH)2 + H2 |
observation magnesium with steam |
- white solid |
| Mg + H2O > MgO + H2 |
why is aluminium unreactive with water | -resistant to further oxidation because of Al2O3 coating |
do silicon, phosphorus and sulphur react with water | no |
observations chlorine and water | (with universal indicator paper) | red then bleaches white |
equation chlorine and water | Cl2 + H2O >< HClO + HCl |
what is the reaction of water and chlorine an example of | disproportionation- chlorine simultaneously oxidised and reduced |
does argon react with water | no |
what do the period 3 elements react with oxygen to form | they react exothermically to form oxides, with the exception of chlorine and argon |
observation sodium and oxygen |
| - white solid |
equation sodium and oxygen | 4Na + O2 > 2Na2O |
observation magnesium and oxygen |
| - white solid |
equation magnesium and oxygen | Mg + 1/2O2 > MgO |
observation aluminium and oxygen |
| - fine powder- white sparkles/white solid |
equation aluminium and oxygen | 4Al + 3O2 > 2Al2O3 |
what kind of compounds are the metal oxides | basic |
observations silicon with oxygen | v slow |
equation silicon with oxygen | Si+ O2 > SiO2 |
observations phosphorus and oxygen | white flames and fumes |
equation phosphorus and oxygen | 4P + 5O2 > P4O10 |
observations sulphur and oxygen | blue flame | choking gas |
equation sulphur and oxygen | S + O2 > SO2 |
what kind of compounds are non metal oxides | acidic compounds |
what can sulphur (IV) oxide (SO2) react with oxygen to form | sulphur (VI) oxide (SO3) |
sulphur 4 oxide and oxygen | SO2 + 1/2O2> SO3 |
contact process | SO3 + H2O > H2SO4 |
why do NA20, MGO AND AL203 have high melting points | ionic- strong electrostatic attractions between oppositely charged ions require a lot of energy to break |