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17 Cards in this Set
- Front
- Back
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Define Ionization Energy.
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The energy required to remove one mole of electrons from one mole of neutral gaseous atoms.
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What is the general trend for Ionization Energy across a period.
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Ionization Energy increases across the period.
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Why does boron have a lower Ionization Energy than beryllium, breaking the trend across the period? (The same explanation is applicable to the exception of Al having a lower IE than Mg)
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Boron starts a new p-orbital, and it's higher energy level means it is removed more easily.
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Why does oxygen have a lower Ionization Energy than nitrogen, breaking the trend across the period? (The same explanation is applicable to the exception of S having a lower IE than P)
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Oxygen has a 4th p-orbital elecron, which is repelled by the eletrons already occupying each of the three p-orbitals, making it easier to remove.
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Define Electronegativity.
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The ability of an atom to attract a shared (bonding) pair of electrons.
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Explain the concept of charge density.
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As the metal ion gets larger, the charge is diluted over the increased surface area of the ionic sphere (lower charge density). As the charge desnity decreases, the force of attraction between the ion and the delocalised electrons is lowered. This results in a lower melting point.
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Explain the melting point trend down Group 7 (halogens)?
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The melting point increases down the group, as van der Waal's forces increase due to increased molecular mass.
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What type of bonding do the first three elements of period three have? (Na, Mg and Al)
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Metallic bonding.
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What type of structure does Si have?
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Giant Covalent.
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What is the trend in melting point across the first three elements of period 3 (Na, Mg, Cl)?
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Increasing melting point, due to greater ionic charge and increased number of delocalized electrons.
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Are Na2O and MgO alkaline, amphoteric, insoluble or acidic in solution?
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Alkaline. Respective pHs 13 and 11.
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Is SiO2 alkaline, amphoteric, insoluble or acidic in solution?
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Insoluble. pH 6.
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Is Al2O3 alkaline, amphoteric, insoluble, or acidic in solution?
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Amphoteric. pH 7.
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What bond type do the P2O5, SO3, and Cl2O7 have?
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Molecular Covalent.
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Do ionic oxides dissolve to produce alkaline or acid solutions?
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Alkaline.
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Do molecular covalent oxides dissolve to produce alkaline or acid solutions?
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Acid.
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What are ligands?
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Molecules (or ions) which donate an electron pair to form a dative covalent bond with the central transition metal atom (forming a complex molecule or ion).
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