| A | B |
|---|
| Na is the symbol for | sodium |
| Li is the symbol for | Lithium |
| K is the symbol for | potassium |
| in the Periodic Table the alkali metals are found in | group number 1 |
| For elements in group 1 the number of e in outer shell is | 1 |
| the electronic pattern of Na (proton no = 11) is | 2,8,1 |
| K (proton no = 19) electronic pattern is | 2,8,1 |
| The bonding in alakali metal compounds is | ionic |
| when Na (2,8,1) forms ions it | loses 1e from its outer shell |
| when Na (2,8,1) loses 1e from its outer shell | it forms ions with 1+ charge |
| Because all group 1 elements have 1e in outer shell | they all form ions with 1+ charge |
| When Na(2,8,1) reacts with Cl (2,8,7)the outer e | is transferred to the outer shell of the Cl |
| When Cl (2,8,7) gains 1e from na | the Cl becomes Cl(-) ions |
| Na(+) & Cl(-) form | NaCl |
| NaCl has a high melting point because | there are strong attractive forces between the Na(+) and Cl(-) ions |
| The structure of NaCl is | a giant structure of ions |
| With water alkali metals react | very vigorously |
| Of Li, Na, and K - K (2,8,8,1) is the biggest atom because | it has most e shells |
| K has the biggest atom so | it is the most reactive |
| When added to water they all release a gas - it is | hydrogen |
| The solution formed when Na is added to water is | alkaline |
| Na+ H2O - The solution formed has a pH of greater than 7 because | it is alkaline |
| Na + H2O - alkaline solution formed is | sodium hydroxide |
| Na added to water - products are are | sodium hydroxide + hydrogen |
| We can tell H2 is liberated because | it pops with a lighted splint |
| K + H2O ---> | KOH + 1/2 H2 |
| Na + H2O ---> | NaOH + 1/2 H2 |
| Na(+) & O(2-) ions form | Na2O (subscript 2) |
| Li(+) & O(2-) ions form | Li2O (subscript 2) |
| Na2O & Li2O have similar formulae because | Li(+) and Na(+) have same charge |
| in the reactions heat is released -reactions are | exothermic |
| Na(+) & OH(-) form | NaOH |
| Na(+) & O(2-) form | Na2O (subscript 2) |
| K(+) & O(2-) form | K2O (subscript 2) |
| K(+) & Cl(-) form | KCl |
| Reactivity increases | down the group |
| Cs is lower down - its reactivity | is greater than K |
| Cs will form ions of formula | Cs(+) |
| Formula of caesium chloride should be | CsCl |
| formula of caesium oxide should be | Cs2O (subscript 2) |
