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Karteikarten von Anushka John, aktualisiert more than 1 year ago
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Erstellt von Anushka John
vor etwa 8 Jahre
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| Frage | Antworten |
| Elements are classed as s, p or d according to what? | The orbital the highest energy electron is in |
| What happens to atomic radius as you go across (left to right) the period? | *atomic radius decreases *increased number of protons in the nucleus, so greater nuclear charge *without much difference in shielding *causes stronger attraction to outer electrons, so they are pulled closer (same in period 2) |
| What is the general trend for 1st ionisation energy across both period 2 and 3? | GENERALLY increases This is due to the increased number of protons, so there is a greater positive nuclear charge attracting the outer electrons, making them harder to remove |
| What is the first anomaly in the trend of 1st ionisation energy across period 2 and 3? | PERIOD 2: small drop between Be and B * the outermost electron in Be is in 2s and in B is in 2p, which is a higher energy level so easier to remove PERIOD 3: small drop between Mg and Al ( same as above, expect replace 2s -> 3s and 2p -> 3p) |
| What is the second anomaly in 1st ionisation energy across period 2 and 3? | PERIOD 2: small drop between nitrogen and oxygen O's outer electron paired with another electron in the same 2p orbital. Mutual repulsion makes it slightly easier to remove PERIOD 3: small drop between phosphorus and sulphur S's outer electron paired with another electron in the same 3p orbital. Mutual repulsion makes it slightly easier to remove |
| Explain the trend for Na. Mg and Al | METALLIC BONDING *Strong intermolecular bond * Gets stronger the more electron there are in the outer shell - as more electrons are released into the sea of delocalised electrons. *lots of energy needed to overcome electrostatic forces of attraction between electrons and ions |
| Explain why Si has the highest boiling point? | MACROMOLECULAR * many strong covalent bonds between the atoms * high energy needed to break covalent bonds |
| Explain the trend in boiling points for P4(s), S8(s) and Cl2 (g) | SIMPLE MOLECULAR *weak van Der Waals ofrces of attraction between the molecules *little energy is needed to overcome them *boiling point for S8 >P4> Cl2 as it has more electrons and so greater van Der Waals between the molecules. |
| Explain why Ar has the lowest boiling point | MONOATOMIC GAS *very weak van Der Waals between the atoms and so very easily overcome |
| Period 2 has a similar trend in boiling points to Period 3. Describe the bonding in the different Period 2 elements and their relative boiling points. | Li and Be - METALLIC (high bp) B and C - MACROMOLECULAR (very high bp) N2 and O2 - SIMPLE MOLECULAR gases (low bp) Ne - MONOATOMIC gas (very low bp) |
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